U.S. DEPARTMENT OF COMMERCE /

National Bureau of Standards

Compilation of Rate Constants

for the Reactions of Metal Ions

in Unusual Valency States

fQC1 "

100

.U573

no. 62

1978

C.2
NATIONAL BUREAU OF STANDARDS

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LIBRARY

JUl 2 6 1979

Compilation of Rate Constants

for the Reactions of Metal Ions

in Unusual Valency States

George V. Buxton and Robin M. Sellers

Cookridge Radiation Research Centre,

Cookridge Hospital,

Leeds LSI 6 6QB,

Great Britain

N SRP S

U.S. DEPARTMENT OF COMMERCE, Juanita M. Kreps, Secretary

Dr. Sidney Harman, Under Secretary

Jordan J. Baruch, Assistant Secretary for Science and Technology

, NATIONAL BUREAU OF STANDARDS, Ernest Ambler, Director

Issued June 1978
Library of Congress Cataloging in Publication Data

Buxton, George V

Compilation of rate constants for the reactions of metal ions in unusual valency states.

(Nat. stand, ref. data ser., Nat. Bur. of Stand. ; NSRDS-NBS 62)

Supt. of Docs, no.: C 13.48:62

1. Chemical reaction, Rate of—Tables, etc. 2. Metal ions—Tables.

I. Sellers, Robin M., joint author. II. Title. III. Series: United States. National Bureau of Standards. National standard reference data series

; NSRDS-NBS 62. QC100.U 573 no. 62 [QD502] 602’. Is [546’. 3] 78-816

NSRDS-NBS 62

Nat. Stand. Ref. Data Ser., Nat. Bur. Stand. (U.S.), 62, 78 pages (June 1978)

CODEN. NSRDAP

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Foreword

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III
Preface

This report is one of a series of data publications on radiation chemistry; the aim of the series

is to compile, evaluate, and present the numerical results on processes occurring in systems which

have been subjected to ionizing radiation. Various kinds of data are important in radiation chemistry. The quantities which were measured first were the observed radiation yields or G values (molecules formed or destroyed per 100 eV). Various indirect methods based on G values have been used to determine yields of transient species and relative rates of reactions. The spectral properties (optical,

electron spin resonance) of transients have provided a direct method for their identification, and rates of the very fast reactions of transients which occur in irradiated systems have been measured directly

by spectroscopic methods. Conductivity and luminescence methods have also provided a means of

measuring properties of transients and their kinetics. Some reactions which occur in irradiated systems

have also been studied by other methods, such as photochemistry, electric discharge, ultrasonics, chemical initiation, electron impact, etc. The emphasis in these publications is on the data of radiation

chemistry, but where other pertinent data exist, they are included.

The data of radiation chemistry are voluminous; thousands of systems have been investigated.

As a result there are certain collections, e.g. rate constants of particular types of reactions or certain

properties of transients, for which tabulations of the data are considered essential, but for which

critical assessment of each value is impossible. On the other hand, certain systems and properties

have been studied so extensively that critical examination of these data is desirable and timely.

Authors of this series of data publications have been asked to evaluate the extent to which the data can be critically assessed, to describe their criteria for evaluation, and to designate preferred values

whenever possible.

IV
Contents

P«ge Introduction 1

Arrangement of the tables 2

List of abbreviations 4

Table 1. Silver(O) and (II) reactions 5

Table 2. Gold(O) and (II) reactions 6

Table 3. Cadmium(I) reactions 7

Table 4. Cobalt(I) reactions 13

Table 5. Chromium(I), (II) and (V) reactions 20

Table 6. Copper(I) and (III) reactions 24

Table 7. Europium(II) reactions 29

Table 8. Iron(II) reactions 30

Table 9. Mercury(O) and (I) reactions 31

Table 10. Indium(II) reactions 35

Table 11. Iridium(I I) reactions 35

Table 12. Manganese(I) reactions 35

Table 13. Molybdenum(II) reactions 36

Table 14. Nickel(I) reactions 37

Table 15. Lead(I) reactions 44

Table 16. Praesodymium(IV) reactions 45

Table 17. Platinum(I) and (III) reactions 46

Table 18. Rhodium(II) reactions 50

Table 19. Ruthenium(I), (II), (III) and (IV) reactions 51

Table 20. Samarium(II) reactions 53

Table 21. Thallium(O) and (II) reactions 55

Table 22. Thulium(II) reactions 59

Table 23. Ytterbium(II) reactions 60

Table 24. Zinc(I) reactions 62

Table 25. Intramolecular electron transfer reactions for

some metal complexes 65

References 66

V

Compilation of Rate Constants for the

Reactions of Metal Ions in Unusual

Valency States*

George V. Buxton and Robin M. Sellers**

Cookridge Radiation Research Centre, Cookridge Hospital, Leeds LS16 6QB, Great Britain.

Kinetic data have been compiled for reactions of uncommon oxidation states of metals which are produced by radiolysis of aqueous solutions of metal ions. Most of the reaction rates are for transient species, and the rates were determined by pulse radiolysis; some data were obtained by flash photolysis and gamma

radiolysis. Metal ions from Groups IB, IIB, IIIA, IVA, VIB, VIIB, VIIIB, and the lanthanides are included

in the compilation.

Key words: Aqueous solution; chemical kinetics; complex ions; electron transfer; metal ions; radiation chemistry; rates; transients..

Introduction

The discovery of the hydrated electron as a major product of the radiolysis of water and the development of

pulse radiolysis have together resulted in the accumulation, during the last ten years, of a considerable amount of

information on the chemistry of unusual valency states of metal ions in aqueous solution, which has been reviewed

recently (G. V. Buxton and R. M. Sellers, 77-0121). 1 For the most part attention has been focussed on hyperreduced states produced in reaction (1), which affords a simple, and often unique, method of their formation.

Reactions of hydroxyl radicals and hydrogen' atoms, and of simple radicals derived from them, with metal ions have

been less commonly studied.

e~Q + Mn+ -* M(n-l)+

(1) 2M(n_l)+ — Mn+ + M(n-2)+

(2)

M(n—1 )+ _|_ S — products (3)

This compilation lists the rate constants for reactions of these metal ions in unusual valency states. In the

majority of cases the species are unstable, generally decaying by dismutation (2), or reaction with the solvent or a

solute (3). This instability has been the principal criterion on which the decision to include data in this tabulation

has been based. However, because the bulk of information on these metal ions has been obtained by pulse radiolysis

methods, we have also included some rate constants for the reactions of stable metal ions such as Cu+

, Cr2+ and

Eu2+ measured by these methods. In these examples, indicated in the tables, much other data not recorded here has

been obtained by other techniques.

* This is a data review prepared for, and in cooperation with, pthe Radiation Chemistry Data Center of the Radiation Laboratory, University of Notre Dame, Indiana 46556. The

Laboratory is operated under contract with the Department of Energy. The work of the Center is supported in part by the National Bureau of Standards, Office of Standard Reference Data. ••Present address: Central Electricity Generating Board, Berkeley Nuclear Laboratories, Berkeley, Gloucestershire GL13 9PB, Great Britain.

1 Literature references are given at the end of this paper.

1
Arrangement of the Tables

The tables are listed in alphabetical order of the chemical symbols of the metals involved. Within each table

the arrangement is by oxidation state, starting with the lowest, and is further subdivided according to the

complexing ligands in the order aquo ions (and hydrolysed forms), inorganic ligands in alphabetical order of the first letter of the chemical symbol of the principal element of that ligand (e.g. N for ammonia), and organic ligands in alphabetical order of their written names. For each individual transient species the reactants are in the order:

inorganic species, organic radicals, both in alphabetical order of their chemical symbols, followed by organic

compounds in alphabetical order of their written names.

Table 25 is somewhat different, and lists the rate constants for some intramolecular electron transfer

reactions. The reactions are subdivided according to the method of production of the transient species. Note that all the rate constants in this table are first order, and have therefore units of s-1

. Reactions of metallo-proteins and

related compounds are not dealt with in this compilation.

The data given for each reaction are the measured rate constant, and a brief description of the experimental

conditions etc. as outlined below. Literature data published to approximately mid-1976 are covered.

Reaction: Three main methods have been used to measure the rate constants reported here:

(i) by monitoring the rate of removal of the absorption of the

metal species at some convenient wavelength

(ii) by monitoring the rate of formation of some product

(iii) by competition kinetics.

Methods (i) and (iii) have the disadvantage that they do not involve characterisation of the products of the reaction,

and in many instances in the literature no additional experiments have been performed to overcome this. Often the

reaction type has been assumed. Particular attention has been given to this problem in this compilation. Where there

is no experimental information on the products given in the original work or elsewhere, only the left hand side of

the equation is given, followed in brackets by the possible type of reaction as originally suggested, or as seems

appropriate. If experimental evidence is given, the products are quoted, and the nature of the evidence indicated in the column headed 'Comments'.

In some cases the reactive intermediates themselves have not been fully characterised, and in such instances

brief details of the method and conditions of formation are given.

Rate Constants: Most of the rate constants listed were measured under conditions where the reaction obeyed

first order kinetics and no knowledge of absolute concentrations of the transient species is required. Error limits on

the rate constants are those quoted in the original work. In the great majority of cases their magnitude is ± 10 - 15% of the rate constant value, which is typical of the precision of the mean of pseudo first order rate constants measured by pulse methods. If the data source gives no errors none are shown here, but they should be assumed to be at least ± 25% to allow for the possibility that the rate constant is derived from a single measurement.

Second order rate constants are prefaced by “2A; =” or “2k/e\ =” as appropriate. In cases where it is not

clear whether the value refers to 2k or k this is noted in the 'Comments' column. The measured quantity is 2k/ €\

and is subject to the same limitations given above for pseudo first order rate constants. Calculation of 2k requires a knowledge of €\, and where this quantity is quoted in the original work it is given under 'Comments'. In many

instances, however, the values of €\ used to calculate 2k have not been clearly stated. Evaluation of €x requires a knowledge of the concentration of transient species present which, in radiation

chemical systems, means that the dose per pulse and the G value2 of the species must be known. In our experience

these quantities are each likely to be uncertain by ± 10%, so that the error in 2k may be as much as three times as

large as the error in 2k/e\. Therefore, in the absence of any quoted errors, the error in 2k should be assumed to be

± 50%.

*G is the number of molecules of a species produced per 100 eV of absorbed energy.

2
Equilibrium constants are quoted under the 'Rate Constants' heading, and are prefixed by “A = ” followed by

the appropriate units. If the individual rate constants for the forward and reverse processes are known these are shown as “£

f” and “&r” respectively. Activation energies are prefaced by “Aa =” and are given in units of kj

mol-1

. Ionic Strength (1): Ionic strengths have either been taken directly from the original work, or calculated from

the conditions given. In the few instances where the formation of ion pairs has been taken into account the values

are followed by an asterisk. If insufficient information is given to enable the ionic strength to be calculated the

column has been left blank. The ionic strength of rate constants extrapolated to zero ionic strength is given as > 0”. Unfortunately in a number of studies little or no attempt has been made to maintain the ionic strength constant. The practice of many reaction kineticists of adding a high concentration of inert electrolyte, such as NaCIO*, has not been widely adopted by radiation chemists, no doubt because of possible complications due to direct radiolysis of the

electrolyte (cf. J. Konstantatos and D. Katakis, 67-0019). There is no reason however why an ionic strength of say

0.1 or 0.5 mol dm-3 should not become standard for pulse radiolytic measurements. It is to be hoped that more

consideration will be given to this problem in future studies.

Temperature: Where temperatures are quoted in the original work these have been given. In the absence of

any information temperatures are given as room temperature (RT). The temperature ranges over which activation

parameters have been measured are given as appropriate. Since many of the rate constants quoted in these tables are near the diffusion controlled limit and have therefore small activation energies, little uncertainty is engendered by

an imprecise knowledge of the temperature. For example a change in temperature of 5° from 25° changes k by 11%

for an activation energy of 16 kj mol-1. Comments: Information and comments relevant to the reactions and rate constants are given in this column as outlined above. No attempt has been made to give a complete description of the conditions employed in the

measurement of the rate constants quoted, but where the concentration of one or more of the solutes exceeds 0.1

mol dm-3this has been noted.

References: The references are listed following the tables in order of the serial number of the paper in the

files of the Radiation Chemistry Data Centre at the University of Notre Dame. The first two digits of this number

represent the year in which the work was published. The references in the tables also give the first four letters of

the first author's name and a dot for each additional author up to a maximum of four dots.

3
List of Abbreviations

Reaction: af

dis

et

int et 0 at pt

et - is ? Rate Constant: 2k

€XK

PK

kf

kr

9

Ionic Strength: -0

(D

*

var Temperature: RT

pH: nat Method: comp.

f.ph.

7

P

r Chemical Symbols: bpy

en

g!y

EDTA4- NAD+ NTA3- PNDA

L

adduct formation

dismutation (disproportionation)

electron transfer

intramolecular electron transfer

oxygen atom transfer

proton transfer

inner sphere electron transfer

uncertain

rate constant for second order reaction

extinction coefficient at wavelength X

activation energy (units kj mol-1

) equilibrium constant

acid dissociation constant (= -logioA)

rate constant for forward reaction of

equilibrium

rate constant for reverse reaction of

equilibrium

value uncertain

extrapolated to zero ionic strength

calculated taking into account the

formation of ion pairs

various room temperature

natural pH of the solution

competition kinetics

flash photolysis

y-radiolysis

pulse radiolysis

bipyridyl

ethylenediamine

glycine

ethylenediamine tetraacetate nicotinamide adenine dinucleotide

nitrilotriacetate /)-nitroso-7VyV-dimethylaniline

ligand (specified in table).

4
Table 1. SilverfO) and Silverfll) reactions

No.

1.1

1.2

1.3

1.4

1.5

1.6

1.7

1.8

1.9

1.10

1.11

1.12

Reaction k!dm* mol-1

s -1 • / trc pH Method Comments Ref.

Ag{0) - aquo ions and

complexes

Ag° + Ag+ — Aga+ 5.9 x 10» RT P

r Product characterised by absorption spec- trum and charge.

Puki..68-0431

(6.5 ± 0.3) x 10# - 29 1.0 P

r - Farh...73-1053

(5.2 ± 0.3) x 10* 29 1.0 P

r Measured at pressure of 6.72 kbar.Farh...73-1053

Ag*+ + Ag+ —>• Ag*+ + Aga°

3.8 x 10* -> 0 RT P

r Products characterised by absorption spectrum.Puki..68-0431

Aga° + Ag+ Ags+ ca.10* RT P

r Product characterised by absorption spectrum.Puki..68-0431

Aga0/ Ags

+ + MnO«“ (et) 1.2 x 1010 0.003 RT P

r Measured by the

rate of depletion of the MnOi- absorption.

Baxe..65-0385

Ag,+ + Oa (et or af) 3.8 x 10* RT P

r Product uncertain, but transfers an

electron to

1 ,4-benzoquinone

(see SeU.76-1134).

Baxe..65-0393

Agj+ + 1,4—benzoquinone —* Ags2+

(?) +

(1,4—benzoquinone)

-

(1.5 ± 0.3) x 10* 25±2 5.8 P

r Measured by the

rate of formation

of the semiquinone

in the presence of

1 mol dm-3

2-methyl-2-propanol.

Sell.76-1134

Ags+ + menaquinone —

Agj2+

(?) + (menaquinone)

- slow 7.0 P

r Only 24% electron

transfer, which may

be due to side

reactions. Solutions contained

1 mol dm-3

2-methyl-2-propanol.

Rao.73-1047

Ag(0) - ammine complexes

Ag« + Ag(NH,)a+ —

Aga(NHs)n

+ 5.2 x 10* RT Pr Ag° generated from

eaQ + Ag(NHs)a+ -

might be same as product of egq +

Ag+

. Product contains unknown number of ammine

ligands.

Puki.68-0435

Aga(NH,)n

+ + Aga(NHs)n

+ —

Ag«(NHs)n

2+ ?

2k = 2.6 x 1010 RT P

r Product uncertain;

gives ultimately

Aga°.

Puki.68-0435

Aga(NH,)n+ + Ag(NH,)a+ Ags(NHs)n

2+

?

108 RT Pr Measured from rate of formation of

product, nature of which is uncertain.

Puki.68-0435

Agill) - aquo complex

Ag2+ + Ag2+ -

Ag+ + Ag3+ 1.5 x 10* - RT - Pr - Puki..68-0431

Ag2+ + anisole —* Ag+ + anisole+ (3.8 ± 0.4) x 107 20±2 nat(?) Pr Product characterised by absorption spectrum and esr.

0'Ne..75-1171

5
Table 1. Silver(0) and Silver(II) reactions — Continued

No. Reaction A/dm3 mol'•1 s -i a I t/°c PH Method Comments Ref.

1.13 Ag*+ + 1,2-dimethoxybenzene —* Ag+ +

(l,2-dimethoxybenzene)+

(6.0 ± 0.6) x 107 - 20±2 nat(?) P

r Product characterised by absorption spectrum and0'Ne..75-1171

1.14 Ag*+ + 1,3—dimethoxybenzene —* Ag+ +

(l,3-dimethoxybenzene)+

(6.3 ± 0.6) x 107 - 20±2 nat(?) P

r Product characterised by absorption

spectrum and esr.

0'Ne..75-1171

1.15 Aga+ + 1,4—dimethoxybenzene —> Ag+ +

(1,4—dimethoxybenzene)+

(4.6 ± 0.5) x 107 20±2 nat(?) P

r Product characterised by absorption

spectrum and esr.

0'Ne..75-1171

1.16 Ag2+ + 1,2,3-trimethoxybenzene —* Ag+ +

( 1 ,2,3-trimethoxybenzene)+

(2.5 ± 0.3) x 107 20±2 nat(?) Pr Product characterised by absorption

spectrum and e9r.

0'Ne..75-1171

1.17 Aga+ + 1,2,4—tri- methoxybenzene —*• Ag+ + (1,2,4-trimethoxybenzene)+

(7.0 ± 0.7) x 107 20±2 nat(?) Pr Product characterised by absorption

spectrum and esr.

0'Ne..75-1171

1.18 Aga+ + 1,3,5-tri- methoxybenzene —

Ag+ + (1,3,5-trimethoxybenzene)+

(5.6 ± 0.6) x 107 20±2 nat(?) Pr Product characterised by absorption

spectrum and esr.

0'Ne..75-1171

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

Table 2. Gold(0) and Gold(ll) reactions

No. Reaction A/dm3 mol-1

s_1 8 / t/°c pH Method Comments Ref.

Au(0) from. Au(CN)tT +

2.1 Au° + Au° -> Auj° (3.2 ± 0.9) x 10» 0.001 RT 11 P

r Product assumed. Ghos.68-0302

(2.9 ± 0.7) x 10® 0.1 RT 13 P«- Solutions contain- ed 9.8 x 10_a mol

dm-3 Ha .

Ghos.68-0302

2.2 Au° + Fe(CN)*3-

(et?) 5.5 x 10“ - RT -

P

r - Ghos.68-0302

2.3 Au° + NjO (et or O at) 5.5 x 10* - RT - Pr - Ghos.68-0302

2.4 Au° + 02 (et or af) Au(0) from Au(CN)t~ + H

3.6 x 10» RT Pr “ Ghos.68-0302

2.5 Au° + Au° —> Aua° Au(II) from Au(CN)*~ + OH

(5.0 ± 1.0) x 10* 0.015 RT 2 Pr “ Ghos.68-0302

2.6 Aun + Au11 (2.4 ± 0.6) x 10* 0.01 RT 2 Pr Solutions contain- Ghos.68-0302

(dis or af) (4.8 ± 1.2) x 10“ 0.01 RT 4,7 Pr

ed 0.1 mol dm-3 HQ.

Solutions contain- ed 0.01 mol dm-3 KQ.

Ghos.68-0302

Au(II) from AuCU~ + H

2.7 Aun + Au11 —* (1.4 ± 0.3) x 10" 0.01 20 2 Pr Nature of products Baxe.70-0580

Au1 + Aura

(8.6 ± 0.7) x 10“ 0.011 20 2 Pr

-see ref. 70-0580.

Solutions contain- ed 10-3 mol dm-3 Q“.

Baxe.70-0580

(1.2 ± 0.1) x 10» 0.131 20 2 Pr Solutions contain- ed 10-3 mol dm-3

Cl~ + 0.12 mol dm-3 NaQO«

Baxe. 70-0580

(2.7 ± 0.6) x 10“ 0.02 20 2 Pr Solutions contain- ed 10-3 mol dm-3 Q

-

.

Baxe.70-0580

(2.5 ± 0.2) x 107 0.11 20 2 Pr Solutions contain- ed 10-1 mol dm-3 Q

-

.

Baxe.70-0580

*If the data 9ource gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

6
Table 3. Cd(I) reactions

No. Reaction A/dm® mol-1

s-1 * / t/°C PH Method Comments Ref.

3.1 Cd+ + BrOs

-

(et) (1.25 ± 0.2) x 10® 0.08 RT nat P

r - Meye.68-0855

Em = 13.4 ± 1.7 kj 0.08 3-90 nat P

r - Meye. 70-1228

mol-1

3.2 Cd+ + Cd+ —* Cd2a+ 2k = ca. 1.2 x 10* 0.4 25±2 nat pr Measured at 300 nm Buxt.75-1027

taking €soo = 8080

dm® mol-1 cm

-1

. Rate constant estimated from studies of Cd+ decay in presence of several

different OH scavengers. 2A = 3.0 x 10® 0.002 RT nat P

r Measured at 300 nm

taking €300 = 16500

dm® mol-1 cm

-1

. Rate

constant estimated from computer analysis of Cd+ decay.

Competing reactions taken to be Cd+ +

H202 and Cd+ +

R- (R = CH3COHCH3, CHsCHOH, CH2OH). Product identified from effect of ionic strength on its decay.

Kelm..75-1064

2k = 5.0 x 10® 0.004 RT nat Pr Measured at 313 nm

taking £301 = 14000

dm® mol-1 cm

-1

. Rate constant in- dependent of OH

scavenger used.

Bark.75-1153

3.3 Cd+ + Co(en)ss+ (et) (1.6 ± 0.2) x 10® 0.08 RT 5-6 P

r - Meye.69-0428

3.4 Cd+ + cis-Co(en)2Cl2+

(2.3 ± 0.3) x 10® 0.08 RT 5-6 P

r - Meye.69-0428

(et) 3.5 Cd+ + tra/w-Co(en)2Cl2+

(2.6 ± 0.4) x 10® 0.08 RT 5-6 Pr - Meye.69-0428

(et) 3.6 Cd+ + Co(en)aCOs+

(et) (6.7 ± 1.0) x 10® 0.08 RT 5-6 P

r - Meye.69-0428

3.7 Cd+ + cw-Co(en)2F2+

(6.0 ± 0.9) x 10® 0.08 RT 5-6 Pr - Meye.69-0428

(et) 3.8 Cd+ +Co(en)2FH20a+ (et) (4.1 ± 0.6) x 10® 0.08 RT 5-6 pr - Meye.69-0428

3.9 Cd+ + cw-Co(en)2NH3Qa+ (1.75 ± 0.26) 0.08 RT 5-6 P

r - Meye.69-0428

(et) x 10® 3.10 Cd+ +cis-Co(en)2NH3N02a+ (2.8 ± 0.7) x 10® 0.08 RT 5-6 Pr - Meye.69-0428

(et) 3.11 Cd+ + Co(NHs)«s+ (et) (1.72 ±. 0.3) 0.08 RT 5-6 P

r - Meye.69-0428

x 10® 3.12 Cd+ + Co(NHs)5Bra+ (et) (25 ± 0.4) x 10® 0.08 RT 4.0 P

r - Meye.69-0428

3.13 Cd+ + Co(NH2)5aa+ (et) (2.2 ± 0.3) x 10® 0.08 RT 5-6 P

r - Meye.69-0428

3.14 Cd+ + Co(NH3)5CNa+ (et) (9.1 ± 1.4) x 10® 0.08 RT 5-6 Pr - Meye.69-0428

3.15 Cd+ + Co(NH,)5P+

(et) (5.4 ± 0.8) x 10® 0.08 RT 5-6 Pr - Meye.69-0428

3.16 Cd+ + Co(NHs)5fumarate+

(8.3 ± 2.1) x 10® 0.08 RT 5-6 Pr Products of the Meye.69-0428

(et or af?) reaction have relatively large absorption. 3.17 Cd+ + Co(NH,)5H20a+ (6.2 ± 0.9) x 10® 0.08 RT 4.0 Pr - Meye.69-0428

(et) 7
TABLE 3. 01(1) reactions — Continued

No. Reaction k/ dm* mol 1 s

1 * / t/°C pH Method Comments Ref.

3.18 Cd+ + Co(NH3)80Hj+ (9.0 ± 1.3) x 10* 0.08 RT 7.1 Pr _ Meye.69-0428

(et) 3.19 Cd+ + OKNHs)6Ns

*+

(1.41 ± 0.2) 0.08 RT 5-6 Pr - Meye.69-0428

(et) x 10» 3.20 Cd+ + Co(NH,),NCSa+ (1.32 ± 0.2) 0.08 RT 5-6 P

r - Meye.69-0428

(et) x 10* 3.21 Cd+ + Co(NHs)5OOCCHsa+ (9.0 ± 1.3) x 107 0.08 RT 5-6 P

r - Meye.69-0428

(et) 3.22 Cd+ + Cr*+ < 107 - RT nat P

r - Baxe. .66-0848

3.23 Cd+ + CHV (et) (9.8 ± 1.0) x 10* 0. 02* 25±2 nat P

r - Buxt..76-1072

3.24 Cd+ + CtjOt*

-

(et) ( 1.6 ± 0. 2) x 1010 0. 02* 25±2 nat Pr - Buxt.76-1072

3.25 Cd+ + Cua+ (et) ( 1.2 ± 0. 2) x 10* 0.08 RT nat Pr - Meye.68-0855

( 1.1 ± 0. 2) x 10* 0.04 RT 5-8 y Measured by competition kinetics using NO3- as competitor and taking

*(Cd+ + NO*') =

3.5 x 10* dm*

mol-1 s"1

.

Fiti70-0117

3.26 Cd+ + H202 - (1.55 ± 0.2) x 10a - RT nat Pr - Meye.68-0855

Cda+ + OH + OH-

(2.2 ± 0. 2) x 10* - 25 nat P

r - Buxt..76-1072

2.8 x 10* - RT nat pr Buxt..67-0062 Em = 9.2 ± 0.8 - 1-30 nat pr - Buxt.76-1072

kj mol-1

Products identified

in y-radiolysis

studies (see Buxt.. 73-0039).

3.27 Cd+ + Hs0

+ < 10* 0.08 RT -

P

r - Meye.68-0855

3.28 Cd+ + I0S- (et) (2.3 ± 0.3) x 10* 0.08 RT nat Pr - Meye.68-0855

(2.1 ± 0. 2) x 10* 0.04 RT 5-8 y Measured by competition kinetics using NO*

-

as competitor and taking

*(Cd+ + NO*”) =

3.5 x 10* dm*

Fiti70-0117

mol-1s-1. 3.29 Cd+ + MnOr (et) (7.8 ± 0.8) x 10* ca.22 7.0 Pr Measured by the

rate of depletion

of the MnO«- absorption in the presence of ca. 1 mol dm-

* 2-methyl2-propanol.

Rao.73-1104

1.3 x 1010 ca. 20 nat Pr Measured by the Baxe..65-0385

0.004 rate of depletion

of the MnO«

-

absorption. 3.30 Cd+ + Nia+ < 107 - RT nat Pr - Baxe. .66-0848

3.31 Cd+ + NO2 (et) (2.0 ± 0.3) x 10* 0.08 RT nat Pr - Meye.68-0855

£, = 12.5 ± 1.7 0.08 3-90 nat Pr - Meye.70-1228

kj mol-1 3.32 Cd+ + N0S - (et) (3.5 ± 0.5) x 10* 0.08 RT nat Pr - Meye.68-0855

8
Table 3. Cd(I) reactions — Continued

No. Reaction A/dm3 mol 1 s

1 * / t/°C pH Method Comments Ref.

3.33 Cd+ + NaO - CdO+ + Na < 2 x 10* _ RT nat P

r Meye.68-0855

1 x 10* - RT nat P

r - Buxt..67-0062

(3.5 ± 0.4) x 10* - 25 nat P

r Solutions contain- Buxt..76-1072 = 45.6 ± 1.3 - 1-30 nat P

r ed 0.1 mol dm-3

kj mol-1 methanol.

Products inferred from y-ray induc- ed chain reaction

in the system

Cd3+ + HCOr + NjO.

C(Na) measured in the system Cda+ +

NaO. (see ref. 73-0039).

3.34 Cd+ + Oa (et or af) (2.4 ± 0.4) x 10® RT nat Pr - Meye.68-0855

3.3 x 10® RT nat Pr - Baxe..66-0848

(3.6 ± 0.4) x 10® 25±2 nat P

r Absorption spec- Buxt..76-1072 trum of products

similar to that of 0a-

; but decay

slower (see ref. 76-1072). Pro3.35 Cd+ + OH —>• Cda+ + OH" ca. 8 x 10*

1.8 x 1010

2 x 1010

25 nat

RT nat

RT nat

duct transfers an

electron to /)-benzoquinone

(see ref. 76-1134).

Evidence possibly

indicates product

to be CdOa+. pr Estimated from decay of Cd+

in absence of OH sca- vengers taking into account the major competing

reaction Cd+ + Cd+

. pr Experimentally determined rate constant for the decay

of Cd+in the absence of OH scavengers. Not correct- ed for Cd+ + Cd+

or other competing

reactions. pr Estimated from computer analysis of the decay of

the optical absorption and conductivity of Cd+

in the absence of OH

scavengers, taking

Cd+ + Cd+ and Cd+ + HaOa as the competing reactions. Products

identified from

conductivity

changes.

Buxt.75-1027

Baxe. .66-0848

Kelm..75-1064

9
Table 3. Cd(I) reactions — Continued

No. Reaction A/dm® mol 1 s

1 “ / t/°C PH Method Comments Ref.

3.36 Cd+ + Pba+ (et) 7.5 x 107 _ RT nat Pr _ Baxe..66-0848

3.37 Cd+ + Ru(NHs)«s+ (et) (2.2 ± 0.3) x 10“ 0.08 RT nat Pr - Nav..70-1229

3.38 Cd+ + SaO»a- -> (2.4 ± 0.2) x 10® Cda+ + SO«" + S04a- 0.02® 25±2 nat P

r Product identification: S04- observed to form at same rate as Cd+

decayed.

Buxt..76-1072

3.39 Cd+ + Zna+ < 107 - RT nat Pr - Baxe. .66-0848

3.40 Cd+ + -CHaOH - CdCHaOH+ 2 x 10® RT nat P

r Product inferred from conductivity measurements.Kelm..75-1064

3.41 Cd+ + CHaCHOH — < 2 x 10® - RT nat Pr - Bark.75-1153

CdCHsCHOH+

(1.3 ± 0.7) x 10® RT nat P

r Product inferred from conductivity measurements.

Kelm..75-1064

3.42 Cd+ + -CHOHCHaOH < 2 x 10® - RT nat Pr - Bark.75-1153

3.43 Cd+ + CHaCOHCH, < 2 x 10® CdCH,COHCH,+ RT nat Pr Bark.75-1153

(2.4 ± 1.2) x 10» RT nat Pr Product inferred from conductivity measurements.Kelm..75-1064

3.44 Cd+ + •CHOHCHOHCHaOH < 2 x 10® - RT nat Pr - Bark.75-1153

3.45 Cd+ + -CHa(CHs)aCOH -> ca. 1 x 10® Cda+ + (CHs)aC =CHa + OH"

RT nat Pr Isobutene detected

as product.

Kelm. .75-1064

< 2 x 10® - RT nat Pr - Bark.75-1153

3.46 Cd+ + -(CHaCHaOUCHCHaO)- < 2 x 10® RT nat Pr Radical from

polyethylene glycol

(mw 104

) + OH.

Bark.75-1153

3.47 Cd+ + allyl alcohol < 5 x 107 - 25±2 nat Pr - Buxt..76-1072

3.48 Cd+ + 9,10-anthra- (1.03 ± 0.1) x 10® quinone —* Cda+ +

(9, 10-anthraquinone)

-

ca. 22 7.0 Pr Measured by the

rate of formation

of the semiquinone

in the presence of

ca. 1 mol dm-® 2-methyl-2-propanol.

Rao.73-1104

3.49 Cd+ + benzophenone —* 1.0 x 10® Cda+ + (benzophenone)

- RT 7.0 Pr Measured by the

rate of formation

of the ketyl radical in the presence

of ca. 1 mol dm-® 2-methyl-2-propanol.

Rao.75-1032

3.50 Cd+ + 1,4-benzoquinone —* (4.1 ± 0.8) x 10® Cda+ + (1,4—benzoquinone)

- 25±2 5.4 Pr Measured by the

rate of formation

of the semiquinone

in the presence of

1 mol dm-® 2-methyl-2-propanol.

SeU.76-1134

4.4 x 10® RT 7.0 Pr Measured in the presence of ca. 1 mol dm-

® 2-methyl2-propanol.

Rao.75-1032

(7.7 ± 0.8) x 10® - ca.22 7.0 Pr Measured in the Rao.73-1104

presence of ca. 1 mol dm-

* 2-methyl2-propanol.

10
TABLE 3. Cd(I) reactions — Continued

No. Reaction A/dm* mol-1

s-1 • / t/°C pH Method Comments Ref.

3.51 Cd+ + 2-hydroxy- (3.57 ± 0.4) x 10* _ co.22 7.0 P

r Measured by the Rao.73-1104

1,4-naphthoquinone — rate of formation Cd*+ + (2-hydroxy- 1,4— of the semiquinone

naphthoquinone)

-

in the presence of

ca. 1 mol dm-* 2-methyl-2-propanol.

3.52 Cd+ + menaquinone — (4.6 ± 0.5) x 10* - RT 7.0 P

r Measured by the Rao.73-1047,

Cd2+ + (menaquinone)

-

rate of formation

of the semiquinone

in the presence of

ca. 1 mol dm-* 2-methyl-2-propanol.

Rao.75-1032

(4.68 ± 0.5) x 10» ca. 22 7.0 P

r Measured in the presence of ca. 1 mol dm-

* 2-methyl2-propanol.

Rao.73-1104

3.53 Cd+ + NAD+ -* (2.9 ± 0.3) x 10» - ca. 22 7.0 P

r Measured by the Rao.73-1104

Cd**+ NAD- rate of formation

of NAD- in the presence of ca. 1 mol dm-

* 2-methyl2-propanol. 3.54 Cd+ + 1,4- (7.35 ± 0.7) x 10» - ca. 22 7.0 P

r Measured by the Rao.73-1104

naphthoquinone-2- rate of formation sulphonate — of the semiquinone

Cd2+ + (1,4- in the presence of naphthoquinone-2- ca. 1 mol dm-*

sulphonate)- 2-methyl-2-propanol.

3.55 Cd+ + PNDA (et) 1.4 x 1010 - RT nat Pr - Dain.68-0066

3.56 Cd+ + riboflavin —* (5.10 ± 0.5) x 10* - ca. 22 7.0 Pr Measured by the Rao.73-1104

Cda+ + (riboflavin)-rate of formation

of the reduced

riboflavin in the presence of ca. 1 mol dm-

* 2-methyl2-propanol.

Cd(I) complexes

CdEDTA*-

3.57 CdEDTA*- + BrO,

-

(et) (8.9 ± 1.8) x 108 0.16 RT 11.3 Pr - Meye.70-1228

Ea = 4.6 ± 1.2 0.16 3-90 11.3 Pr - Meye.70-1228

kj mol-1

3.58 CdEDTA*- + CdEDTA*-

'A'/Csw = (5.8 0.16 RT 11.3 Pr Unclear whether A Meye.70-1228

(et or af) ± 1.5) x 10* cm s-1 or 2A.

'A' = (4 ± 2) 0.16 RT 11.3 Pr Unclear whether A Meye.70-1228

x 107 or 2A. 3.59 CdEDTA*- + IOs -

(et) (2.7 ± 0.6) x 108 0.16 RT 11.3 Pr - Meye.70-1228

3.60 CdEDTA*- + NO,

-

(et) (3.2 ± 0.6) x 108 0.16 RT 11.3 Pr - Meye.70-1228

Eh = 8.4 ± 1.2 0.16 3-90 11.3 Pr - Meye.70-1228

kj mol-1

3.61 CdEDTA*- + NO,

-

(et) Cd(en)

„

+

(n unknown)

(1.66 ± 0.3) x 107 0.16 RT 11.3 Pr Meye.70-1228

3.62 Cd(en)„+ + BrO,

-

(et) (1.28 ± 0.3) x 10* 0.64 RT 11.4 Pr - Meye.70-1228

3.63 Cd(en)„+ + IO,

-

(et) (2.5 ± 0.5) x 10* 0.64 RT 11.4 Pr - Meye.70-1228

3.64 Cd(en)n

+ -|- NO,-

(et) (1.12 ± 0.2) x 10* 0.64 RT 11.4 Pr - Meye.70-1228

3.65 Cd(en)„+ + NO,

-

(et) (4.5 ± 0.9) x 10" 0.64 RT 11.4 Pr - Meye.70-1228

11
TABLE 3. Cd(I) reactions — Continued

No. Reaction A/dm* mol 1 s" 1 * / t/°C pH Method Comments Ref.

Cdigly) 3.66 Cd(gly) + BrOs ~ (et) (6.1 ± 1.2) x 107 0.21 RT 10.5 P

r - Meye.70-1228

3.67 Cd(gly) + 10,- (et) (1.8 ± 0.4) x 10* 0.21 RT 10.5 P

r - Meye.70-1228

3.68 Cd(gly) + NO," (et) (8.5 ± 1.7) x 10“ 0.21 RT 10.5 P

r - Meye.70-1228

3.69 Cd(gly) + NO," (et) (2.4 ± 0.5) x 10“ 0.21 RT 10.5 Pr - Meye.70-1228

CdNTA2"

3.70 CdNTA2" + BrO," (et) (1.02 ± 0.2) x 107 0.10 RT 10.7 P

r - Meye.70-1228

3.71 CdNTA2" + CdNTA2"<N Jse II rH 0.10 RT 10.7 Pr Unclear whether k Meye.70-1228

(et or af) ± 0.4) x 10s or 2k. cm s"1

'k' = (8 ± 4) x 0.10 RT 10.7 Pr Unclear whether k Meye.70-1228

10* or 2k. 3.72 CdNTA2" + 10," (et) (6.1 ± 1.2) x 10* 0.10 RT 10.7 Pr - Meye.70-1228

3.73 CdNTA2" + NO," (et) (4.2 ± 0.8) x 107 0.10 RT 10.7 Pr - Meye.70-1228

3.74 CdNTA2" + NO," (et) (4.5 ± 0.9) x 107 0.10 RT 10.7 Pr - Meye.70-1228

Cd(I)-radical complexes 3.75 CdCH,CHOH+ + H,0 - 257 s"1 - RT nat Pr Products inferred Kelm..75-1064

Cd2+ + CHsCHaOH + OH" from conductivity measurements.

3.76 CdCH3C0HCH3+ + H2 0 — 161 s"1 - RT nat Pr Products inferred Kelm..75-1064

Cd2+ + CHsCHOHCH, + OH" from conductivity measurements.

3.77 Cd,2+ + -CH^CH^COH - ca. lx 10* - RT nat Pr Isobutene detected Kelm..75-1064

Cd+ + Cd2+ + (CH,),C: =CHa + OH" as product.

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

12
Table 4. Cobalt(I) reactions

No. Reaction A/dm8 mol-1s

1 a / t/°C pH Method Comments Ref.

Co\„

4.1 Co+ + Br2“ (et) (1.0 ± 0.3) x 1010 RT nat f.ph. Competing reactions Br2” + Br2_

and Co+ + Co+ not

considered.

Thor.70-7726

4.2 Co+ + BrOs~ (et) (4.8 ± 0.5) x 10* 0.019* 25±2 nat P

r - Buxt..76-1072

(7.1 ± 1.1) x 10* -0 25±2 nat P

r - Buxt..76-1072

4.3 Co+ + Cd8+ < 107 - RT nat P

r - Baxe..66-0848

4.4 Co+ + Co+(et c af) 2A < 4 x 10* 0.019* 25±2 nat P

r Estimated at 370 Buxt.75-1027 nm taking €370 =

2080 dm8 mol-1 cm

-1

. 4.5 Co+ + Cus+ (et) (4.1 ± 0.4) x 10s 0.019* 25±2 nat P

r - Buxt..76-1072

(1.06 ± 0.36) x 1010 0.04 RT 5-8 y Measured by competition kinetics using NOs~ as competitor and taking

A(Co+ + NOD = 1.8 x 10* dm8 mol-1

s-1.

Fiti70-0117

4.6 Co+ + H202 -> (1.6 ± 0.2) x 10* - 25 nat Pr - Buxt..76-1072 Co8+ + OH + OH 1.9 x 10* - RT nat P

r - Buxt..67-0062 Ea = 13.0 ± 1.0 - 1-30 nat P

r - Buxt..76-1072

kj mol-1 Products identified

in y-radiolysis

studies (see ref. 73-0039).

4.7 Co+ + IOs

-

(et) (4.3 ± 0.4) x 10* 0.019* 25±2 nat Pr - Buxt..76-1072

(4.9 ± 0.8) x 10* 0.04 RT 5-8 y Measured by competition kinetics using NOjas competitor and taking

A(Co+ + NOD =

1.8 x 10* dm8 mol-1

s_l.

Fiti70-0117

4.8 Co+ + MnO«-

(et) 1.06 x 10l° ca. 20 nat Pr Measured by the Baxe. .65-0385

0.004 rate of depletion

of the MnO«~ absorption. 4.9 Co+ + N20 -* CoO+ + N2 7 x 10* RT nat y Estimated from N2 yields in the yradiolysis of Co2+ + N20 solutions.

Buxt..67-0062

(1.0 ± 0.1) x 10* - 25±2 nat Pr - Buxt..76-1072

Products inferred from y-ray induced

chain reaction in the system Co*+ +

HC02 - + N20. (see

ref. 73-0039).

4.10 Co+ + NOs “ (et) (1.8 ± 0.2) x 10* 0.019 25±2 nat Pr - Buxt..76-1072

4.11 Co+ + Nia+ < 107 - RT nat Pr - Baxe..66-0848

13
Table 4. Cobalt(I) reactions — Continued

No.

4.12

4.13

4.14

4.15

4.16

4.17

4.18

4.19

4.20

Reaction A/dm* mol-1

s -1 * / t/°C pH Method Comments

Co+ + Oa (et or af) (6.0 ± 0.6) x 10* - 25±2 nat

Co+

4- OH (et) ca.8 x 10* - 25±2 nat

Co+ + Pba+ < 107 - RT nat Co+ + S208a- - (2.8 ± 0.5) x 10* 0.019 25±2 nat Coa+ + S04 " + SO«aCo+ + Zna+ < 107 - RT nat Co+ + allyl alcohol — ca. 108 - 25 ±2 nat

(Co-allyl alcohol)+

Co+ + 9,10-anthra- (1.05 ± 0.1) x 10* - ca. 22 nat quinone —* Coa+ + (9,10-

anthraquinone)

-

Co+ + benzophenone —* 2.5 x 10* - RT 7.0 Coa+ + (benzophenone)

-

Co+ + 1,4-benzoquinone —*• 4.8 x 10* - RT 7.0 Coa+ + (1,4—benzoquinone)

-

(5.1 ± 0.5) x 10* - 25±2 4.7

(7.35 ± 0.7) x 10* - ca. 22 7.0

pr Absorption of products similar to that of Oa

- but decay slower (see

ref. 76-1072).

Product transfers an electron to

1,4-benzoquinone

(see ref. 76-1134).

Evidence possibly

indicates product

to be CoOa+. pr Estimated from decay of Co+

in absence of OH scavengers, taking into account the major competing

reaction Co+ + Co+. pr

pr Formation of SO«

-

inferred from the absorption produced on pulse radiolysis of solutions of Coa+ + SaO*a_. pr

pr Product characterised by its absorption spectrum. pr Measured by the

rate of formation

of the semiquinone

in the presence of

ca. 1 mol dm-

* 2-

methyl-2-propanol.

pr Measured by the

rate of formation

of the ketyl radical in the presence

of ca. 1 mol dm-* 2-methyl-2-propanol.

pr Measured by the

rate of formation

of the semiquinone

in the presence of

ca. 1 mol dm-* 2-methyl-2-propanol.

pr Measured in the presence of 1 mol

dm-

* 2-methyl-2-

propanol. pr Measured in the presence of ca. 1 mol dm-

* 2-methyl2-propanol.

Ref.

Buxt..76-1072

Buxt.75-1027

Baxe..66-0848

Buxt..76-1072

Baxe. .66-0848

Buxt.76-1072

Rao.73-1104

Rao.75-1032

Rao.75-1032

Sell.76-1134

Rao.73-1104

14
TABLE 4. Cobalt(I) reactions — G.utinued

No.

4.21

4.22

4.23

4.24

4.25

4.26

4.27

Reaction A/dm* mol-1s_1 * / t/°C pH Method (Comments Ref.

Co+ + menaquinone —

G>,+ + (menaquinone)

-

(4.0 ± 0.4) x 10* RT 7.3 P

r Measured by the

rate of formation

of the semiquinone

in the presence of

ca. 1 mol dm-* 2-methyl-2-propanol.

Rao.73-1047

Rao.75-1032

(4.1 ± 0.1) x 10a ca. 22 7.0 Pr Measured in the presence of ca. 1 mol dm-

* 2-methyl2-propanol.

Rao.73-1104

Co+ + 1,4-

naphthoquinone-2-

sulphonate — Coa+ +

( 1 ,4—naphthoquinone-2-

sulphonate)

-

(6.83 ± 0.7) x 10a ca. 22 7.3 P

r Measured by the

rate of formation

of the semiquinone

in the presence of

ca. 1 mol dm-* 2-methyl-2-propanol.

Rao.73-1104

G)+ + riboflavin —

Co2+ + (riboflavin)-

Co(I) complexes

Co(CN)s*~ {from Co(CN)sa~ + eaq_

)

(2.55 ± 0.3) x 10» ca. 22 7.0 P

r Measured by the

rate of formation

of the reduced

riboflavin in the presence of ca. 1 mol dm-

* 2-methyl2-propanol.

Rao.73-1104

Co(CN)b4- + H20 ->

Co(CN)5H»- + 0H“

(1.1 ± 0.1) x 10* s" 1 20 ca. 13 Pr Measured in the presence of ca. 0.1 mol dm-

* H2. Proton transfer mechanism implied from isotope effect (compare

entry 4.25).

Vene.71-0097

Co(CN)54_ + D20 (1.9 ± 0.2) x 20 ca. 13 Co(CN)bD3 - + OD" 104 s_l

CoL+(L = 5,7,7, 12, 12, 14-hexamethyl-l ,4,8,1 l-tetraazacyclotetradeca-4, 14-diene)

pr Measured in D20 in the presence of

ca. 0.1 mol dm-* h2. tY

^NH N'

Vene.71-0097

CoL+ + H20 -> CoLHa+ + 0H“

20 0.001 RT 9-10 Pr Measured in tne presence of 1 mol

dm-

* 2-methyl-2-

propanol. See ref. for evidence for proton transfer mechanism.

Tait.. 76-1001

CoL+ + HsO

+ CoLHa+ + H20

1.2 x 10* 0.015 RT 3.5-4.2 pr Measured in the presence of 1 mol dm-

* 2-methyl-2-

propanol. See ref. for evidence for proton transfer

Tait.. 76-1001

mechanism.

15
Table 4. Cobalt(I) reactions — Continued

No. Reaction A/dm3 mol 1 s

1 * I t/°C pH Method Comments Ref.

4.28 CoL+ + HaP04 “ —

CoLH+ + HP(V

3.0 x 107 0.005

-0.01 RT 5.5 P

r Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol. See ref. for evidence for proton transfer mechanism.

4.29 CoL+ + NaO (et) 9.0 x 108 0.01 RT 9.2 P

r Reaction possibly involves two electron oxidation to Co(III) complex. 4.30 CoL+ + Oa — CoLOa+ 9.0 x 10* 0.02 RT 9.2 P

r Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol. Reaction does not involve

the formation of CoL*+

, assumed

therefore to involve the coordination of the Oa.

CoL+(L = 5,7,7,12,14,14—hexamethyl-1,4,8,1 1-tetraazacyclotetradeca—4, 11-diene).

4.31 CoL+ + Co(bpy)s3+

(et) 1.2 x 10* ca. 0.02 RT 9.2 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol. 4.32 CoL+ + Co(en)j3+

(et) 7.9 x 108 ca. 0.02 RT 9.2 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol. 4.33 CoL+ + Co(NHs)«3+

(et) 7.5 x 108 ca. 0.02 RT 9.2 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol. 4.34 CoL+ + CoL2+

(et) 4.0 x 108 ca. 0.02 RT 9.2 P

r Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol. 4.35 CoL+ + CoL 2+

(et)

(L' = 2,3,9,10-tetramethyl6.7 x 108 ca. RT

0.02

- 1 ,4,8, 1 l-tetraazacyclotetradeca- 1 ,2,8, 1 0-tetraene)

9.2 Pr Measured in the presence of 1 mol dm-3 2-methyl-2-

propanol.

4.36 CoL+ + Cr(bpy)s3+

(et) 1.2 x 10* ca. 0.02 RT 9.2 P

r Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1001

Tait..76-1001

Tait.. 76-1001

Tait.. 76-1001

Tait..76-1001

Tait..76-1001

Tait..76-1001

Tait.. 76-1001

Tait.. 76-1001

16
Table 4. Cobalt(I) reactions — Continued

No.

4.37

4.38

4.39

4.40

4.41

4.42

4.43

4.44

4.45

Reaction A/dm3 mol-1 9-l a / t/° C pH Method Comments Ref.

CoL+ + Fe(bpy)ss+ (et) 2.3 x 107 ca. 0.02 RT 9.2 P

r Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1001

CoL+ + HaO -> CoLH2+ + OH"

48 0.001 RT 9-10 P

r Measured in the presence of 1 mol dm-3 2-methyl-2-

propanol. See ref. for evidence for proton transfer mechanism.

Tait.. 76-1001

CoL+ + H30

+ —

CoLH+ + HaO

3.1 x 10® 0.015 RT 3. 5-4.2 pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol. See ref. for evidence for proton transfer mechanism.

Tait.. 76-1001

CoL+ + HP042_ —

CoLH2+ + PO*3"

1.0 x 10B 0.06-

0.3 RT 10.0 P

r Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol. See ref. for evidence for proton transfer mechanism.

Tait..76-1001

CoL+ + HaP04- —

CoLH+ + HP042" 9.8 x 107 0.005-0.01 RT 5.5 pr Measured in the presence of 1 mol dm-3 2-methyl-2-

propanol. See ref. for evidence for proton transfer mechanism.

Tait.. 76-1001

CoL+ + NH4+ CoLH+ + NHs6.8 x 10® 0.015-

0.1 RT 7.0 P

r Measured in the presence of 1 mol dm-3 2-methyl-2-

propanol. See ref. for evidence for proton transfer mechanism.

Tait..76-1001

CoL+ + NaO (et) 3.9 x 107 0.01 RT 9.2 P

r Reaction possibly

involves two electron oxidation to Co(III) complex.

Tait.. 76-1001

CoL+ -|- Oa — CoLOa+

1.7 x 10® 0.02 RT 9.2 P

r Measured in the Tait..76-1001

presence of 1 mol

dm-3 2-methyl-2-

propanol. Reaction does not involve formation of CoL2+

, assumed therefore

to involve the

coordination of

the Oa. CoL+ + Ru(NH3)«2+

(et) 4.0 x 10® 0.016- RT 9.2 P

r Measured in the Tait.. 76-1001

0.028 presence of 1 mol

dm-3 2-methyl-2-

propanol.

17
Table 4. Cobalt(I) reactions — Continued

No.

4.46

4.47

4.48

4.49

4.50

4.51

4.52

4.53

Reaction A/dm8 mol-1

s -1 “ / t/°C pH Method Comments Ref.

CoL+ + Ru(NHs),NO»+(et) 3.9 x 107 0.016-

0.028 RT 9.2 P

r Measured in the presence of 1 mol

dm-2 2-methyl-2-

propanol.

Tait.. 76-1001

CoL+ + acetic acid —* CoLH+ + CHsCOO- 7.5 x 107 0.01-

0.05 RT 4.8 P

r Measured in the presence of 1 mol

dm-8 2-methyl-2-

propanol. See ref. for evidence for proton transfer mechanism.

Tait.. 76-1001

CoL+ + 9,10-anthraquinone

-2-sulphonate —* CoL2+ +

(9,10-anthraquinone-2-

sulphonate)

-

4.4 x 10* 0.004 RT 9.2 P

r Measured in the presence of 1 mol

dm-8 2-methyl-2-

propanol. Semiquinone product

characterised by

its absorption.

Tait.76-1001

CoL+ + 3-benzoylpyridine

(et + ?)

4.6 x 108 0.004 RT 9.2 Pr Measured in the presence of 1 mol

dm-8 2-methyl-2-

propanol. Only

50% electron transfer to the 3-

benzoylpyridine

.

Other reaction pathway(s) not

characterised.

TaiL. 76-1001

CoL+ + fluorenone —

CoL2+ + (fluorenone)- 4.3 x 10® 0.004 RT 9.2 P

r Measured in the presence of 1 mol

dm-8 2-methyl-2-

propanol. Ketyl

radical product

characterised by

its absorption.

Tait.76-1001

CoL+ + menaquinone —

CoL2+ + (menaquinone)

- 4.6 x 10* 0.004 RT 9.2 Pr Measured in the presence of 1 mol

dm-8 2-methyl-2-

propanol. Semiquinone product

characterised by

its absorption.

Tait.76-1001

CoL+ + methyl iodide (et) 4.7 x 108 0.015 RT 9.2 P

r No evidence for Tait.76-1001

substitution (Su2)

reaction pathway.

CoL+

(L = 2,3,9,10-tetramethyl-l,4,8,ll-tetraazacyclotetradeca-l,3,8,10-tetraene)

CoL+ + Co(bpy)s8+(et) 8.5 x 107 0.016- RT 6.5 P

r Measured in the Tait.76-1001

0.028 presence of 1 mol dm-8 2-methyl-2-

propanol.

18
TABLE 4. Cobalt(I) reactions — Continued

No. Reaction k/ dm3 mol 1 s

1 a / f/°C pH Method Comments Ref.

4.54 CoL+ + Cifbpy)3s+ (et) 1.6 x 10* 0.016-

0.028

4.55 CoL+ + HsO

+ -> 1.6 x 10* 0.06- CoLH2+ + HaO 0.6

4.56 CoL+ + 02 CoL02+

1.1 x 10* 0.02

4.57 CoL+ + acetic acid —* 6.2 x 104 0.01- CoLHa+ + CHsCOO- 0.05

4.58 CoL+ + 9,10-anthraquinone- 3.8 x 10* 0.004

2.6-

sulphonate — CoLa+ + (9,10-anthraquinone2.6-

sulphonate)

-

4.59 CoL+ + indigosulphonate —> 4.9 x 10* 0.004 CoLa+ + (indigosulphonate)-

4.60 CoL+ + riboflavin —

1.0 x 10* 0.004 CoLa+ + (riboflavin)-

RT 6.5 pr

RT 0.25- pr 1.25

RT 6.5 P

r

RT 4.8 P

r

RT 6.5 Pr

RT 6.5 pr

RT 6.5 P

r

Measured in the presence of 1 mol

dm-

* 2-methyl-2-

propanol.

Measured in the presence of 2 mol

dm-

* 2-propanol. See ref. for evi- dence for proton

transfer mechanism.

Measured in the presence of 1 mol

dm-

* 2-methyl-2-

propanol. Reaction does not involve formation of CoLa+

, assumed therefore

to involve the coordination of On. Measured in the presence of 2 mol

dm-3 2-propanol. See ref. for evi- dence for proton

transfer mechanism.

Measured in the presence of 1 mol

dm-

* 2-methyl-2-

propanol. Semiquinone product

characterised by

its absorption.

Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol. Radical anion product characterised by its absorption.

Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol. Radical anion product characterised by its absorption.

a

If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

Tait.. 76-1001

Tait.. 76-1001

Tait.. 76-1001

Tait..76-1001

Tait.. 76-1001

Tait.. 76-1001

Tait.. 76-1001

19
TABLE 5. Chromium(I), chromium(II) and chromium(V) reactions

No. Reaction A/dms mol 1 s-1 * I t/°C pH Method Comments

Cr{I) Reactions CrU

5.1 Cr+ + H*0 < 5 x 10ss-1 - 22±2 3.0-4.3

CrIP+

{from H + Cr"

+

) 5.2 CrHa+ + H„0 <1 s-1 - 22 ±2 0-2

5.3 CrHa+ + HsO+ — (1.8 ± 0.2) x 104 var 22±2 0-2

Cr3+ + Ha + H20

Cr[II) reactions (includes only those measured by radiolytic methods). Crit 5.4 Cr*+ + Bra

- - (1.9 ± 0.2) x 10* 0.2 22±3 1 CrBra+ + Br

-

5.5 Cr2* + Cla-

(2.4 ± 0.3) x 10» 0.2 22±3 1 CrCla+ + Cl-

(a) or Crs+ + 2Cl

-

(b)

5.6 Cr2+ + la- -

Crla+ + I -

(1.5 ± 0.2) x 10» 0.2 22±3 1

5.7 Cr*+ + MnO«

-

(et) 3.7 x 10s ca.0.01 20 nat

5.8 Cr2+ + NaO < 10® - 25 nat

pr Estimated from first order, dose dependent

decay of Cr+. Major

competing reactions thought to be Cr+ +

HaOa. Ha detected as product (G = 2.9 at pH 3.4).

pr

pr G(Ha) = 3.8 at pH

0-2 .

pr Reaction occurs by

inner sphere dif- fusion controlled mechanism.

GfCrBr2*) = 2.4 in y-radiolysis experi- ments.

pr Reaction occurs by

parallel mechanisms

involving inner- sphere (path a) and

outer sphere (b) dif- fusion control with approximately equal

probability. G(CrCl2+

) = 1.4 in y-radiolysis

experiments. pr Reaction occurs by

inner sphere dif- fusion controlled mechanism. Crla+

characterised by

flash photolysis and y-radiolysis

experiments. C(CrIa+

) = 0.85 at 0°C.

pr Measured by the

rate of depletion

of the MnO«- absorption.

y Estimated from

the values of G(Na) measured in the y-radiolysis of Cr3+ -+ NaO solutions.

Ref.

Cohe.74-1 142

Cohe.74—1 142 Cohe.74-1142

Laur.74— 1104

Laur. 74—1104

Laur.74— 1104

Baxe. .65-0385

Sell72-0844

20
TABLE 5. Chromium(I), chromium(II) and chromium(V) reactions — Continued

No. Reaction k!dm* mol 1 s 5.9 1 * / t /°C pH Method Comments Ref.

Cra+ + (),-

Cr02a+

5.10

Cr*+ + C0NH2 -

CrC0NH2a+ 5.11

Cr3* + -CH20H -> CrCHa0H3+

5.12

Cra+ + C02" -+ CrC02+

5.13

Cra+ + CHaCH0 -> CrCH2CH0a+ or CrCH2CH(0H)2a+

5.14

Cr2+ + CH2C00H

CrCH2C00Ha+

5.15 0*+ + -CHOH.COOH —

CrCHOH.COOHa+

(1.6 ± 0.2) x 10* 25±2 2.6-4.3 P

r Measured from the

rate of formation

of Cr02a+ in the presence of 0.5 mol dm-

* 2-methyl2-propanol. Product

characterised by its absorption spectrum and by conductivity

Sell. 76-1134

measurements.

(1.6 ± 0.2) x 10* RT 1-3 P

r Measured from the

rate of formation

of Cr02a+ .

Ilan.. 75-1215

(1.9 ± 0.3) x 10* - 25±2 3.4 P

r Measured by com- Sell.76-1134

(comp) petition with 1,4—

benzoquinone taking

k(Cr3+ + C*H402) =

3.2 x 10* dm* mol-1

0—

1

(6.5 ± 0.7) x 10* 22 ±2 0-4.5 Pr

8 . Measured by the

rate of formation

of the product in the presence of 1 mol dm-

* formamide.

Product characterised by its absorption

spectrum and decay

kinetics.

Cohe. 74-1 146

1.6 x 10* 22±2 0-1 Pr Measured by the rate of formation of the

product. Product

characterised by its absorption spectrum and decay kinetics.

Cohe.74—1146

(1.1 ± 0.1) x 10* ca. 25±2 1.4 Pr Measured by rate Elli....73-1057 0.04 of formation of the product in the presence of 1 mol dm-*

formic acid. Product

characterised by its spectrum and decay

kinetics. 3.5 x 10* 22±2 0-1 Pr Measured by the rate of formation of the

product, which may

be in the form of an acetal.

Cohe.74—1146

2.5 x 10* 22±2 0-1 Pr Measured by the rate of formation of the

product. Product

characterised by its absorption spectrum and decay kinetics.

Cohe.74—1146

1.4 x 10* 22±2 0-1 Pr Measured by the rate of formation of the

product. Product

characterised by its absorption spectrum and decay kinetics.

Cohe.74—1146

21
Table 5. Chromium(I), chromium(II) and chromium(V) reactions — Continued

No.

5.16

5.17

5.18

5.19

5.20

5.21

5.22

5.23

5.24

Reaction k! dms mol-1s-1 a I t/°C pH Method Comments Ref.

Cr24 + CHjCHOH

CrCH(CH3)OH3+ 7.9 x 107 22 ±2 0-1 P

r Measured by the rate of formation of the product. Product

characterised by its absorption spectrum and decay kinetics.

Cohe.74-1 146

Cr3+ + -CHOHCHjOH —

CrCHaCHO*4or CrCHaCH(OH)a*+

1.5 x 10s 22 ±2 3.0-4.5 Pr Measured by the rate of formation of the

product. Product is identical to that formed in the reaction Cr24 + CHaCHO (see entry 5.13).

Cohe.74—1146

Cr24 + -CH(COOH)a -* CrCH(C00H)a2+ 6.0 x 107 22±2 0-1 Pr Measured by the rate of formation of the product. Product

characterised by its absorption spectrum and decay kinetics.

Cohe.74—1146

Cr24 + CHjCHCOOH -

CrCH(CH3)C00H2+

1.1 x 10® 22±2 0-1 Pr Measured by the rate of formation of the

product. Product

characterised by its absorption spectrum and decay kinetics.

Cohe.74— 1146

Cra+ + CHsC(OH)COOH —

CrCOH(CH3)COOHa+ 9.2 x 107 22±2 0-1 P

r Measured by the rate of formation of the product. Product

characterised by its absorption spectrum and decay kinetics.

Cohe.74-1146

Cr24 + -CHaN(CH3)CHO — (1.1 ± 0.1) x 10s - 22±2 0-4.5 P

r Measured by the rate Cohe.74—1146

CrCHaN(CH3)CH02+ of formation of the product in the presence of 1 mol dm-3 CHsN(CHs)CHO. Product

characterised by its absorption spectrum and decay kinetics. Cr24 + (CH3)3COH —

CrCOH(CH3)32+ 5.1 x 107 22±2 0-1 P

r Measured by the rate of formation of the

product. Product

characterised by its absorption spectrum and decay kinetics.

Cohe.74—1146

Cr24 + -R — CrR2+

•R = radical from dioxane (H abstraction)

1.0 x 108 22 ±2 0-1 P

r Measured by the rate of formation of the product. Product

characterised by its absorption spectrum and decay kinetics.

Cohe.74-1146

Cr24 + •CH3C(CH3)3OH

CrCHaC(CH3)2OH2+ 1.0 x 108 22±2 0-1 P

r Measured by the rate of formation of the

product. Product

characterised by its absorption spectrum and decay kinetics.

Cohe.74—1 146

22
TABLE 5. Chromium(I), chromium(II) and chromium(V) reactions — Continued

No. Reaction A/dm3 mol-1

s -1 * / t/° C pH Method Comments Ref.

5.25 Cra+ + CHjCHOCHjCHj -» 3.4 x 107 _ 22±2 0-1 P

r Measured by the rate Cohe.74—1146

CrCH(CH3)OCH2CH3a+ of formation of the

product. Product

characterised by its absorption spectrum and decay kinetics. 5.26 Cra+ + CH2C(CH3)2COOH - 1.1 x 10* - 22±2 0-1 P

r Measured by the rate Cohe.74—1146

CrCH2C(CH3)2C00Ha+ of formation of the

product. Product

characterised by its absorption spectrum and decay kinetics. 5.27 Cra+ + anthraquinone- (2.8 ± 0.3) x 10* - co.22 7.0 P

r Measured by the rate Rao.75-1032

2,6-disulphonate —

of formation of the Crs+ + (anthraquinone- semiquinone in the 2,6-disulphonate)

- presence of ca. 1 mol dm-3 2-methyl-2-

propanol. 5.28 Cra+ + 1,4-benzo- (3.2 ± 0.3) x 10* - 25±2 3.4 P

r Measured by the rate Sell.76-1134

quinone —* Crs+ + of formation of the

(1,4—benzoquinone)

-

(3.5 ± 0.4) x 10* - ca.22 7.0 P

r

semiquinone in the presence of 0.5 mol

dm-3 2-methyl-2-

propanol.

Measured by the rate of formation of the semiquinone in the presence of ca. 1 mol

dm-3 2-methyl-2-

propanol.

Rao.75-1032

5.29 Cra+ + tetra- (1.2 ± 0.2) x 10* - 25±2 3.4 Pr Measured by the rate Sell.76-1134

nitromethane —* of formation of the Cr3+ + N02 + C(N02)3-

nitroform anion in the presence of 1 mol dm-3 2-methyl-2-

propanol.

Cr{V) {from CrOt

a~ + e^)

5.30 Crv + Crv

(dis or af) 2A/€«>o = (7 ± 3) 0.003 25 nat P

r - SeU72-0844

x 10* cm s-1

*If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

23
TABLE 6. Copper(I) and coppeiflll) reactions

No. Reaction k/ dm* mol-1s-1 * / t/°C pH Method Comments Ref.

CuU

6.1 Cu+ + Cu(OH)a+

(et) (1.8 ± 0.6) x 10® 0.003 25 4.8 P

r See comments under

entry 6.37.

Sell72-0844

(1.6 ± 0.5) x 10® 0.003 25 6 Pr See comments under

entry 6.37.

Sell72-0844

(3.6 ± 1.2) x 10* 0.002 RT nat P

r - Meye71-0174

6.2 Cu+

4- MnO«

-

(et) 5 x 10® ca. 20 2 Pr Measured by the Baxe. .65-0385

0.08 rate of depletion

of the MnO«

_ absorption. Dependence of k on [Cu*+

] detected.

(6.4 ± 0.6) x 10® 0.004 25 nat P

r Measured by the

rate of depletion

of the MnO«“ absorption.

SeU72-0844

6.3 Cu+ + NaO < 10* 25 nat y Estimated from Na yields in the yradiolysis of Cu*+ + NaO solutions.

Sell72-0844

6.4 Cu+ + -CHaOH ^ kf ca. 1010 - RT 4.5 Pr Identity of product Buxt.77-1500

CuCHaOH+

kT ca. 10* s_1 - RT 4.5 Pr

inferred from its absorption spectrum. Rate constants esti- mated from rate of

Buxt.77-1500

growth and decay of CuCHaOH+

. 6.5 Cu+ + (CHslaCOH ca. 6 x 10® - RT 4.5 Pr Identity of product Buxt.77-1500

CuCOH(CHs)a+

inferred from its absorption spectrum. 6.6 CuCOH(CH,)a+ + H

+ — 3.2 x 107 - RT 3-4.5 Pr Estimated from de- Buxt.77-1500

Cu+ + products pendence of decay of

absorption attri- buted to CuOH(CHs)a+ on [H+

] (see entry 6.5). 6.7 Cu+ + •CHaCHjOH -* 1.9 x 1010 - RT 4.5 7 Estimated from yields Buxt.77-1500

CHa =CHa + OH" + Cua+ of Cu1 in y-radiolysis

of Cu*+ + CaH« solutions. Products inferred from

data for entry 6.8. 6.8 Cu+ + -CHafCHalaCOH — 2.6 x 10® - RT 4.5 y Product inferred Buxt.77-1500

CuCHa(CH3)aCOH+ from its absorption spectrum. Esti- mated from yields of Cu1 in the y-radiolysis of Cu*+

4- 2-

methyl-2-propanol 4- CaH« solutions. Final product is CHa=C(CHs)3.

6.9 Cu+ + acrylamide K = (2.1 ± 0.1) x - 25±2 4 Pr Measured from the Buxt..76-1 186

Cu-acrylamide+ 10* dm* mol-1

effect of [acrylkf = 2 x 10® 2.5 amide] on the yield kT = 1.1 x 10* s _1 2.5 and rate of formation

of Cu-acrylamide+

. 6.10 Cu+ + benzoquinone < 10* - 25±2 4.9 Pr Estimated from the SeU.76-1134

non-formation of benzosemiquinone in the pulse radiolysis of Cu*+ + benzoquinone

solutions. 24
Table 6. Copper(I) and copper(III) reactions — Continued

No. Reaction A/dm3 mol 1 s

1 * / t/° C pH Method Comments

6.11 Cu+ + ethylene K = (2.22 ± 0.1) _ 25±2 4 y Measured from he

Cu-ethylene+ x 10* dm3 mol-1 effect of admitting

ethylene to solutions of Cu-acrylamide+

(see entry 6.9). 6.12 Cu+ + fumaric acid kt = (1.7 ± 0.4) - 22±2 3.65 P

r Measured from the Cu-fumaric acid+ x 10® rate of formation kT = (2.4 ± 0.4) - 22±2 3.65 P

r of the product in x 105

s -1 the presence of 1 K = (7.1 ± 2.0) mol dm-3 methanol. x 10s dm3 mol-1 K = (9.0 ± 2.0) - 22±2 3.65 P

r Measured from the x 103 dm3 mol-1

effect of [fumaric

acid] on the yield of Cu-fumaric acid+ - in the presence

of 1 mol dm-3 methanol. 6.13 Cu+ + iso-butene K = (2.7 ± 0.1) - 25±2 4 y Measured from the Cu-iso-butene+ x 104 dm3 mol-1

effect of admitting iso-butene to solutions of Cu-acrylamide+

. 6.14 Cu+ + maleic acid kt = (2.0 ± 0.4) - 22±2 3.65 P

r Measured from the Cu-maleic acid+ x 10® rate of formation

kT = (1.8 ± 0.4) - 22±2 3.65 Pr of the product in x 10s

s-1 the presence of 1 K = (1.1 ± 0.3) mol dm-3 methanol. x 10* dm3 mol-1

. K = (1.3 ± 0.2) - 22 ±2 3.65 P

r Measured from the x 10* dm3 mol-1

effect of [maleic

acid] on the yield of Cu-maleic acid+

in the presence of

1 M methanol. 6.15 Cu+ + tetranitro- (4.2 ± 0.4) x 10® - RT -

P

r Measured from the methane —* Cu2+ + rate of formation N02 + C(N05)3-

of the nitroform

anion.

(4.7 ± 0.5) x 10® 25±2 4.9 Pr Measured from the

rate of formation

of the nitroform

anion.

Cu(F) Complexes

Y"f M HN.

CuL+(L = 5,7,7,12,14,14--hexamethyl-1,4,8,11 -tetraazacyclotetradeca-4, 1 1 -diene) Id' -/Jk

6.16 CuL+ + Co(bpy)a3+ (1.2 ± 0.1) x 107 0.016- RT 7.0 P

r Measured in the

(et) 0.028 presence of 1 mol dm-3 2-methyl2-propanol. 6.17 CuL+ + CoL'(OHa)(OH)2+ < 10® 0.016- RT 7.0 P

r Measured in the 0.028 presence of 1 mol dm 3 2-methyl2-propanol.

(L' = 5,7,7,12,14,14-hexamethyl-l,4,8,ll-tetraazacyclotetradeca-4,ll-diene).

Ref.

Buxt..76-1 186

Meye75-1092

Meye75-1092

Buxt..76-1186

Meye75-1092

Meye75-1092

Asmu...64—0133

SeU.76-1134

Tait.. 76-1039

Tait.. 76-1039

25
Table 6. Copper(I) and copper(III) reactions — Continued

No. Reaction A/dm3 mol 1 s

1 8 / f/°C PH Method Comments Ref.

6.18 CuL+ + Co(en)ss+ < 103 0.016-

0.028 RT 7.0 P

r Measured in the presence of 1 mol dm-3 2-methyl2-propanol.

Tait.. 76-1039

6.19 CuL+ + Co(NH3)«3+ < 10s 0.016-

0.028 RT 7.0 P

r Measured in the presence of 1 mol dm-3 2-methyl2-propanol.Tait..76-1039

6.20 CuL+ + CoL'(OH)2+ < 10s 0.016- RT 7.0 0.028

(L' = 2,3,9,10-tetramethyl-l,4,8>H-tetraazacyclotetradeca-l,3,7,10-tetraene).

P

r Measured in the presence of 1 mol dm-3 2-methyl2-propanol.Tait..76-1039

6.21 CuL+ + Cr(bpy)s3+(et) (3.7 ± 0.4) x 10« 0.016-

0.028 RT 7.0 P

r Measured in the presence of 1 mol dm-3 2-methyl2-propanol.Tait..76-1039

6.22 CuL+ + Fe(bpy)s3+ < 10s 0.016-

0.028 RT 7.0 P

r Estimated in the presence of 1 mol dm-3 2-methyl2-propanol.Tait..76-1039

6.23 CuL+ + H30

+

(pt) (5.0 ± 0.5) x 108 0.06-

0.3 RT <1.25 P

r Reaction may

involve proton

transfer to the metal centre to give a hydrido

complex.

Tait. 76-1039

6.24 CuL+ + H2P0r < 104 0.01-

0.1 RT 5.50 P

r “ Tait..76-1039

6.25 CuL+ + NjO (et or 0 at) (1.7 ± 0.2) x 108 RT 7.0 P

r Measured in the presence of 1 mol dm-3 2-methyl2-propanol.

Reaction possibly

involves two electron oxidation to Cu(III) complex.

Tait.76-1039

6.26 CuL+

-f O2 —

CuL02+

(2.6 ± 0.3) x 107 RT 7.0 Pr Product does not

transfer an electron to 1,4-benzoquinone, and identified therefore as 03 adduct.

Tait..76-1039

6.27 CuL+ + Ru(NH3)«s+

(et)

(7.2 ± 0.7) x 104 0.016-

0.028 RT 7.0 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait.76-1039

6.28 CuL+ + Ru(NH3)3N03+ < 10s 0.016-

0.028 RT 7.0 Pr Estimated in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait.76-1039

6.29 CuL+ + acetic acid < 104 0.015-

0.06 RT 4.85 Pr Estimated in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait.76-1039

6.30 CuL+ + 9,10-anthraquinone-2,6-disulphonate (et)

(4.3 ± 0.4) x 10* 0.004 RT 7.0 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait.76-1039

26
Table 6. Copper(I) and copper(III) reactions — Continued

No. Reaction A/dm* mol-1

s -1 “ / t/° c pH Method Comments Ref.

6.31 CuL+ + 9,10-anthraquinone-2-sulphonate (et)(1.1 ± 0.1) x 10® 0.004 RT 7.0 P

r Measured in the presence of 1 mol

dm-

* 2-methyl-2-

propanol.

Tait..76-1039

6.32 CuL+ + 1,4—benzoquinone (et)

(2.6 ± 0.3) x 10® 0.004 RT 7.0 P

r Measured in the presence of 1 mol

dm-

* 2-methyl-2-

propanol.

Tait..76-1039

6.33 CuL+ + 3-benzoylpyridineno reaction observed

0.004 RT 7.0 Pr Tait..76-1039

6.34 CuL+ + eosin Y no reaction observed0.004 RT 7.0 P

r “ Tait..76-1039

6.35 CuL+ + fluorescein no reaction observed

0.004 RT 7.0 Pr Tait..76-1039

6.36 CuL+ + methyl iodide (3.1 ± 0.3) x 10®

(et or Sn2)

Cu(II1) Reactions

Cu(IIl) aquo ion ( Cu(OH)s, Cu(OH)i+ and CuOIP+

)b

0.01 RT 9.2 Pr Measured in the presence of 1 mol dm-

* 2-methyl-2-

propanol.

Tait.. 76-1039

6.37 CuOH2+ — Cu(OH)j+ +

H

+ pAT = 2.4 ± 0.2 var 25 0.6 P

r Degree of hydrolysis deduced fromSell72-0844

conductivity experi- ments (see ref. 70-0512).

Note: pK of this value

is also in keeping

with the data of Baxendale et al (ref. 65-0394) and of Meyerstein (ref. 71-

0174) taking into account equilibrium

6.39.

pAT = 3.05 ± 0.05 var RT 2-7 pr - Baxe..65-0394

6.38 Cu(OH)a+ ^ kt = (4.2 ± 1.4) var RT 3.50 P

r Estimated from decay Baxe..65-0394

CuOH+ + OH x 104 s-1 of Cura in the pre- and K = 1.3 x sence of Br

-

, CHjOH,

10-4 dm* mol-1 HaOa etc. Values of

kt = (2.8 ± 1.0) var RT 3.65 pr kT taken to be same

x 104 s -1 as A(Cu2+ + OH). and K — 9.0 x 10

-

® dm* mol-1 6.39 Cu(OH)a+ — p*> 6 var 25 0-6 P

r - SeU72-0844

Cu(OH)s + H

+ 6.40 Cu(OH)a+ + Cu+

(et) (1.8 ± 0.6) x 10® 0.003 25 4.8 P

r Estimated from decay

of Cum in deaerated

Sell72-0844

solutions. (1.6 ± 0.5) x 10® 0.003 25 6 P

r Possibly some contri- bution from Cu(OH)s +

Cu+.

SeU72-0844

(3.6 ± 1.2) x 10® 0.002 RT nat Pr Possibly some contribution from Cu(OH)s + Cu+

.

Meye7 1-0174

6.41 Cu(OH)a+ + Cu(gly)+

(8.1 ± 0.5) x 107 0.004 RT 5.5 P

r - Meye7 1-0775

(et?)

27
Table 6. Copper(I) and copper(III) reactions — Continued

No. Reaction k/ dm* mol 1 s

1 * / t/° c PH Method Comments Ref.

6.42 Cu(OH),+ + Cu(OH)a+ 2k = (4.6 ± 0.6) 0.002 RT 6 P

r Estimated from the Meye71-0174

(af) x 107 decay of Cum in NjO saturated solutions. 2k < 5 x 107 0.004 25 6 P

r Possibly some contri- bution from Cu(OH)a+ + Cu(OH)s and Cu(OH)s + Cu(OH)s.SeU72-0844

6.43 Cu(OH)a+ + ca. 3 x 10* ca. RT 5.2 P

r Estimated from decay Meye71-0174

CuNOa+(et) 0.002 of Cum in presence

of Nor.

6.44 Cu(OH)a+ + mena- (2.0 ± 0.2) x 10* - RT 9.0, P

r 40% of Cum claimed Rao.73-1047

quinone (?) 10.6 to react by electron transfer. Cum

formed by OH +

Cu(C10«)a. RT 8.0 P

r 20.3% electron transfer. Cum formed by

OH + CuSO«.

Rao.73-1047

- 10.6 P

r 39% electron transfer. Rao.73-1047 Cum formed by OH +

CuSO«.

Cu(III) Complexes. (The precise nature of these complexes is uncertain: all were formed by OH oxidation of the corresponding Cun

complex). 6.45 Cu^HaL + 2k = (3.0 ± 0.5) <0.008 RT 11.1 P

r - Meye71-0775

Cum(NHs)n (af?) x 107 6.46 Cura(a-alanine)a (8.0 ± 2.4) x 10* <0.002 RT 6.3 P

r - Meye7 1-0775

(int et?) s” 1

6.47 Cum(/3-alanine)a (7.0 ± 2.1) x 10* <0.002 RT 5.8 Pr - Meye7 1-0775

(int et?) 9 _1

6.48 Cura(a-amino-n- (5.0 ± 1.5) x 10* <0.002 RT 6.1 P

r - Meye7 1-0775

butyric acid)a (int et?) s” 1 6.49 Cum(/3-amino-n- (4.5 ± 1.3) x 10* <0.002 RT 6.0 P

r - Meye7 1-0775

butyric acid)a (int et?) s' 1 6.50 Cum(y-amino-n- (1.2 ± 0.4) x 10* <0.002 RT 4.8 P

r - Meye7 1-0775

butyric acid)2 (int et?) s” 1

6.51 Cum(a-amino- (1.5 ± 0.5) x 10* <0.002 RT 6.2 Pr - Meye71-0775

iso-butyric acid)a s-1

(int et?) (2.5 ± 0.8) x 10*

<a“l <0.002 RT 7.3 P

r - Meye7 1-0775

6.52 Cum(en)n (int et?) < 3 s_1 0.002 RT 5.8 Pr _ Meye71-0775

120 s_1 0.002 RT 11.6 Pr - Meye7 1-0775

6.53 Cum(en)n + 2k = 5.5 x 10s 0.002 RT 5.8 Pr - Meye71-0775

Cum(en)n (af?) 2k = 3.9 x 107 0.002 RT 11.6 Pr - Meye7 1-0775

6.54 Cum(gly)2 (int (6.0 ± 2.0) x 10* <0.002 RT 6.1 Pr - Meye71-0775

et?) 9_i

(2.2 ± 0.7) x 104

s”1 <0.002 RT 7.5 Pr - Meye71-0775

•If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k). “The form of Cum reacting reinterpreted from original references according to equilibria 6.37 and 6.39.

28
TABLE 7. Europium(II) reactions

No. Reaction Ar/dm3 mol-1

s

1 * I t /°C pH Method Comments Ref.

Eu\, (Includes only those rate constants measured by pulse radiolysis). 7.1 Eu2+ + BrOr < 104 ca. RT nat P

r - Fara.72-0065

0.01

7.2 Eu2+ + Co(NHs)sCl2+ 90 ± 9 0.06 25 6 P

r - Fara.73-0107

(et-is) (4.7 ± 0.5) x 102 1.0 (NaC10«)

25 6 P

r - Fara.73-0107

(5.3 ± 0.5) x 102 1.0 (NaCl)

25 6 P

r — Fara.73-0107

7.3 Eu2+ + Co(NH,)5 CN2+ < 30 0.06 25 6 Pr - Fara.73-0107

7.4 Eu2+ + Co(NHs)bP+

(2.8 ± 0.3) x 10s 0.06 25 6 Pr - Fara.73-0107

(et-is) (1.5 ± 0.2) x 104 1.0 (NaCIO*)

25 6 Pr — Fara.73-0107

(2.4 ± 0.2) x 104 1.0 (NaCl)

25 6 Pr — Fara.73-0107

7.5 Eu2+ + Co(NHs)sOH2+ca. 100 0.3 25 - Pr - Fara.73-0107

(et-is) 7.6 Eua+ + Co(NH3)5N32+ < 30 0.06 25 6 Pr - Fara.73-0107

7.7 Eu2+ + Co(NH3)B NCS2+ < 10 0.06 25 6 Pr - Fara.73-0107

7.8 Eu2+ + Cua+ < 104 ca. RT nat Pr - Fara.72-0065

0.01

7.9 Eu2+ ± HjOa < 104 ca. RT nat Pr - Fara.72-0065

0.01 7.10 Eu2+ + IOs" < 104 ca. RT nat Pr - Fara.72-0065

0.01

7.11 Eu2+ + MnO«“ (et) 6.5 x 10» ca. RT nat Pr - Fara.72-0065

0.01 7.12 Eu2+ + NOa" (et) 6.2 x 10s ca. RT nat Pr - Fara.72-0065

0.01 7.13 Eu2+ + NOs“ < 104 ca. RT nat Pr - Fara.72-0065

0.01 7.14 Eu2+ + NaO < 104 ca. RT nat Pr - Fara.72-0065

0.01 7.15 Eu2+ + 0, < 104 ca. RT nat Pr - Fara.72-0065

0.01 7.16 Eu2+ + OH (et) 9 x 108 - RT nat Pr Measured from Fara.72-0065

the rate of decay

of Eu2+ in the absence of OH scavengers. Major competing reaction is OH

+ OH.

(1.3 ± 0.2) x 10* - RT 2 Pr - Pika..73-1084

3.8 x 10* - RT nat Pr - Gord65-0799

7.17 Eu2+ + Ru(NH3)3Br2+

ca. 3 x 10s 0.06 25 6 Pr - Fara.73-0107

(et-is) 7.18 Eu2+ + Ru(NH3)5C12+ (1.5 ± 0.2) x 104 0.06 25 6 Pr - Fara.73-0107

(et-is) 7.19 Eu2+ + Ru(NH3)bH30

3+ < 2 x 103 0.3 25 2 Pr - Fara.73-0107

7.20 Eu2+ + Ru(NH3)*s+ ca. 1 x 10s 0.06 25 6 Pr - Fara.73-0107

(et-is) (2.3 ± 0.2) x 103 1.0 25 6 Pr - Fara.73-0107

(NaC10«)

(1.5 ± 0.2) x 104 1.0 25 6 Pr - Fara.73-0107

(NaCl) 7.21 Eu3+ + Ru(NH3)s0H2+ (6.0 ± 0.6) x 104 0.06 25 6 Pr - Fara.73-0107

(et-is) (1.0 ± 0.1) x 10s 0.3 25 6 Pr - Fara.73-0107

•If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

29
TABLE 8. Iron(II) and iron(III) radical complex reactions

No. Reaction A/dm3 mol-1

s

1 • I t/° C pH Method Comments Ref.

8.1 FeH2+ + H

+ - Fes+ + Ha (1.06 ± 0.1) x 104 0.1- 19-24 0.1- P

r Ha product charac- Jays.. .69-0434

1.0 1.0 terised by vpc; Fe3+ by its absorption spectrum.

8.2 FeHOaa+ — Fes+ + HOa~

(1.8 ± 0.1) x 10s 1.0 20,25 0.1- P

r Fem detected as Jays.. 73-0038

s" 1 (HC1CV

NaQ04)

0.3 product. = 8.8 ± 0.8 kj

mol-1

8.3 FeHOaa+ + Fea+ K = 22 ± 2 dm3 1.0 20 0.1- P

r Measured from the Jays.. 73-0038

FeHOaFe4+ mol-1 (HCKV 0.3 effect of [Fe11

] on NaQ04) the absorption of K = 27 ± 2 dm3 1.0 25 0.1- P

r FeHOaFe4+. mol-1 (HQ04 / NaQ04)

0.3

AT = 33 ± 1 dm3 1.0 30 0.1- P

r mol-1 (HQ04 / NaC104)

0.3 K = 37.5 dm3 1.0 40 0.1- P

r mol-1 (HC104 / NaQ04)

0.3

8.4 FeHOa2+ + SO«a- ^ K = 90 ± 20 dm3 1.0 22 ±1 0.1- Pr Measured from the Jays..73-1022

FeHOaSO« mol-1 (HC104 / 0.3 effect of [S042-

] NaQ04) on the absorption

of FeHOaFe4+. 8.5 FeHOaFe4+ - (1.8 ± 0.1) x 104 1.0 20 0.1- P

r Fera detected as Jays.. 73-0038

Fes+ + HOa" + Fea+ S _1 (HCKV

NaQ04)

0.3 product.

(2.5 ± 0.1) x 104 1.0 25 0.1- P

r

s-1 (HCKV

NaQI4)

0.3

Ea = 47.7 ± 4.6 kj

mol-1

8.6 FeHOaFe4+ + SO«a” K = 100 ± 20 dm3 1.0 22 ±1 0.1- P

r Measured from the Jays. .73-1022

FeHOaFeSO«a+ mol-1 (HC104 / 0.3 effect of [S042-

] NaQ04) on the absorption

of FeHOaFe4+. 8.7 FeHOaS04 - FeS04+ + ca. 104

s -1 22 ±1 0.1- P

r FeS04+ character- Jays.. 73-1022

H(V 0.3 ised by its absorption spectrum. 8.8 FeH02FeS042+ - ca. 104 s-1 22 ± 1 0.1- P

r FeS04Fe3+Jays.. 73-1022

FeS04Fes+ + HOa" 0.3 characterised by

its absorption

spectrum.

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

30
TABLE 9. Mercury(O) and mercury(I) reactions

No. Reaction A/dm3 mol 1 s

1 a / t/° c pH Method Comments Ref.

Hg°

9.1 Hg° + Hg*+ Hga2+ (5.9 ± 0.6) x 10* RT 3-4 P

r Measured from the pH dependence of

the formation of Hgaa+ .

Fuji..73-1080

9.2 Hg° + HgOH+

(5.0 ± 0.5) x 103 - RT 3-4 P

r Measured from the Fuji..73-1080

Hgaa+ + OH" pH dependence of

the formation of Hgaa+

. 9.3 Hg° + Hg(OH)a — < 5 x 107 - RT 3-4 P

r Measured from the Fuji..73-1080

Hgaa+ + 20H" pH dependence of

the formation of Hgaa+ . See also comments for entry

9.6. HgS

9.4 Hga+ + Hga+

(et?) 2k = (1.4 ± 0.2) <0.017 RT 1.9 P»- Rate constant cal- Fara.72-0290

x 1010 culated taking

Cass = 9000 dm3 mol-1 cm

-1

. Hg(D

Hgn„ (and hydrolysedforms) *

9.5 Hg+ HgOH + H

+ pAT = 5.1 var RT 4-7 P

r Measured from the

effect of pH on

the absorption

spectrum of Hg+.

Fuji.. .75-1044

9.6 Hg+ + Hg+

-*j Hg» + Hga+ 2k = (4.9 ± 0.5) — 0 RT 2.0 pr Transient product Fuji..73-1080

x 10* formed, whose decay 2k = (5.2 ± 0.5) -*0 RT 4.3 P

r is dependent on

x 10® [Hg11

], and which

gives Hgaa+

. These

results taken to indicate that Hg+ + Hg+

results in dismutation. Rate

constants calculated taking €355 = 1.4 x 104 dm3 mol-1 cm

-1

. Hg+ + Hg+ (— Hgaa+

) 2k = (8.0 ± 1.0) <0.017 RT 1.9 P

r Products not char- Fara.72-0290

x 10® acterised, but reaction considered to involve

dimerisation. Rate

constant calculated taking €373 = 7800 dm3 mol-1 cm

-1

. 9.7 HgOH + HgOH — 2k = (4.4 ± 0.4) < 0.1 RT - Pr Products identified Fuji.. .75-1044

HgaO + H20 x 10® from pH dependence

or Hga(OH)a of their absorption

spectra. Rate constant calculated taking

Csso = 5300 dm3 mol-1 cm

-1

. 9.8 Hg1 + Hg1 2k = (4.9 ± 1.0) - RT 1.2 Pr - Pika. .75-1218

x 10® 2k = (5.1 ± 1.0) - RT 3.15 Pr - Pika. .75-1218

x 10® 2k = (3.5 ± 0.7) - RT 4.8 Pr - Pika. .75-1218

x 10® 2A = ca. 1.1 x - RT 10.2 Pr - Pika. .75-1218

10»° 31
TABLE 9. Mercury(O) and mercury(I) reactions — Continued

No. Reaction A/dm* mol 1 s -1 “ / t/°C PH Method Comments Ref.

9.8 Hg1 + Hg1 2k = ca. 1.5 x - RT 11.0 P

r - Pika..75-1218 1010 2k = (7.0 ± 1.4) l(KOH) RT 14 P

r - Pika..75-1218

x 10® + data at intermediate pH's Pika..75-1218

9.9 Hg1 + Oa (et or af) (4.0 ± 0.6) x 10* - RT 2.7 Pr - Pika..75-1218

(1.2 ± 0.2) x 10* - RT 11.2 P

r - Pika..75-1218

(1.6 ± 0.2) x 10® l(KOH) RT 14 Pr - Pika. .75-1218

Note: A change in mechanism of the decay of Hg1 aquo ions is observed on increasing the pH. There appears to be no good

understanding of why this should be, and we suggest, therefore, that the reaction mechanisms written above should be viewed

with caution. Note also that the spectral data for Hg+ obtained by Faraggi and Amozig (ref. 72-0290) and by Fujita et al. (ref. 73-1080) do not correspond.

Hg{l) Complexes

HgBr and related species 9.10 HgBr + HgBr —> HgaBra 2k = 8 x 10® RT Pr Product characterised by its absorption specJung. .76-1042

trum. 2k = (1.0 ± 0.1) - RT - Pr - Fuji...76-1087

x 1010 9.11 HgBr + 02 —

>

HgBrOa > 10* RT Pr Product characterised by conductivity experi- ments and nonformation of Oa-

/ HOa absorption.

Jung..76-1042

9.12 HgBr + 1,4-benzo- > 10® - RT 5-5.5 Pr Benzosemiquinone Jung. .76-1042

quinone —HgBr+ + product characterised

( 1 ,4—benzoquinone)

- by its absorption

spectrum. 9.13 HgBr + tetranitro- 2.2 x 10® - RT - Pr Nitroform anion pro- Jung..76-1042

methane — HgBr+ + duct characterised C(NOa)3 ~ + NOa by its absorption

spectrum. 9.14 HgBrOa + 1,4-benzo- 7 x 10® - RT - Pr Benzosemiquinone Jung..76-1042

quinone — HgBr+ + product charac- Oa + (1,4-benzo- terised by its quinone)

-

absorption spectrum. HgCl

9.15 HgCl + HgCl — 2k = (8.0 ± 0.5) - RT - Pr Product charac- Nazh. 73-0043

HgaCk x 10® terised by its absorption spectrum, and gravimetrically giving

C(Hg3Qa) = 3.0 in solutions containing

2-propanol. 9.16 HgCl + O2 — HgClOa (1.0 ± 0.3) x 10® RT Pr Product characterised by conductivity experiments and non-formation

of Oa- /HOa absorption.

Nazh.73-0043

9.17 HgCl + OH — ca. 1010 - RT - Pr Products charac- Nazh. 73-0043

HgCl + OHterised by conductivity

experiments. 9.18 HgCl + 1,4-benzo- 3.0 x 10® - RT - Pr Benzosemiquinone Jung. .76-1042

quinone —* HgCl+

(3.9 ± 0.4) x 10® - 25±2 5.1 Pr product charac- Sell. 76-1 134

+ (1,4—benzosemi- terised by its quinone)

- absorption spectrum. 9.19 HgCl + tetranitro- (4.5 ± 0.3) x 10® - RT 5-5.5 Pr Nitroform anion Nazh.73-0043

methane — HgCl+ product charac- + C(NOa)s - + NOa

32

terised by its absorption spectrum.
TABLE 9. Mercury(O) and mercury(I) reactions — Continued

No. Reaction &/dm* mol 1 s

1 * / t/° C pH Method Comments Ref.

9.20 HgClOa + 1,4-benzo- 7 x 10* _ RT P

r Benzosemiquinone Jung. .76-1042

quinone —> HgCl+ product charac- + Oa + (l,4~benzo- terised by its semiquinone)

- HgCN

absorption spectrum.

9.21 HgCN + HgCN -> 2k = (3.4 ± 0.5) < 0.2 RT Pr Product charac- Fuji.. .75-1203

Hga(CN)a x 10® terised by its absorption spec- trum and decay to give Hg° and Hg(CN)a. Rate constant cal- culated taking 6ass = 3800 dm* mol-1 cm

-1

. 2k = 1.2 x 1010 - RT P

r - Jung..76-1042

9.22 HgCN + Oa -> 4 x 10® - RT P

r Oa" product charac- Jung..76-1042

HgCN+ + Oa" terised by its absorption spectrum,

lifetime in neutral

solution, and conductivity measurements. 9.23 HgCN + OH (et) 3.1 x 10® RT P

r Estimated from

initial decay

of HgCN in the absence of OH

Fuji...75-1203

scavengers. 9.24 HgCN + CHaOH 4.0 x 10® RT P

r Estimated from

initial decay

of HgCN in the presence of methanol.

Fuji...75-1203

9.25 HgCN + CHsCHOH (et to 3.9 x 10® - RT P

r Estimated from Fuji.. .75-1203 HgCN?) initial decay

of HgCN in the presence of

ethanol. 9.26 HgCN + (CHs)aCHOH — 2.4 x 10® - RT P

r Estimated from Fuji.. .75-1203 Hg° + CN~ + CH3COCH3 + H

+

initial decay

of HgCN in the presence of 2-

propanol. G(acetone) = 3.0 measured.

9.27 HgCN + .CHaC(CH,)aOH 1.6 x 10® - RT P

r Estimated from Fuji...75-1203

(af?) initial decay

of HgCN in the presence of 2-

methyl-2-propanol.

Isobutene not detected as product. 9.28 HgCN + 1,4-benzo- 3.5 x 10® - RT P

r Benzosemiquinone Jung. .76-1042

quinone —* HgCN+ + product charac-

( 1 ,4—benzoquinone)

-

terised by its absorption spectrum. 9.29 HgCN + tetranitro- 3.1 x 10® - RT Pr Nitroform anion Jung.. 76-1042

methane —*• HgCN+ + product charac- C(NOa)s + NOa terised by its absorption spectrum. Hgl

9.30 Hgl + Hgl — Hgala 2k = 5.0 x 10® - RT P

r Product charac- Jung. .76-1042

tensed by its absorption spectrum.

33
Table 9. Mercury(O) and mercury(I) reactions — Continued

No. Reaction A/dm3 mol 1 s

1 “ / t/° C PH Method Comments Ref.

9.31 Hgl + 0, - HglOa > 10» RT Pr Product characterised by conductivity experi- ments and nonformation of Oa

-

/ HOa absorption.

Jung. .76-1042

9.32 Hgl + 1,4-benzoquinone —* Hgl+ +

( 1 ,4—benzoquinone)

-

> 109 RT P

r Benzosemiquinone

product characterised by its absorption spectrum.

Jung..76-1042

9.33 Hgl + tetranitro- methane —> Hgl+ +

C(NOa)s

- + NOa

HgSCN

1.4 x 10» RT P

r Nitroform anion

product characterised by its absorption spectrum.

Jung.. 76-1042

9.34 HgSCN + HgSCN —

Hga(SCN)a

2k = 6.0 x 10» RT P

r Product characterised by its absorption spectrum.

Jung. .76-1042

9.35 HgSCN + Oa HgSCNOa > 109 RT Pr Product characterised by conductivity experi- ments and nonformation of Oa

-

/ HOa absorption.

Jung..76-1042

9.36 HgSCN + 1,4—benzoquinone —*• HgSCN+ +

( 1 ,4—benzoquinone)

-

> 109 RT P

r Benzosemiquinone

product characterised by its absorption spectrum.

Jung..76-1042

9.37 HgSCN + tetranitro- methane — HgSCN+ +

C(NOa)s ± NOa

2.8 x 109 RT Pr Nitroform anion product characterised by its absorption spectrum.

Jung..76-1042

9.38 HgSCNOa + 1,4—benzoquinone —

HgSCN+ + Oa

( 1 ,4—benzoquinone)

-

1.0 x 109 +RT Pr Benzosemiquinone

product characterised by its absorption spectrum.

Jung.. 76-1042

*If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

34
Table 10. Indium(II) reactions

No. Reaction A/dm3 mol 1 s_1 8 / t/° C pH Method Comments Ref.

In$

10.1 Ina+ + In2+ (et or af) 2k = ca. 1.2 x 0.7 RT 3 Pr Reinterpreted from Tayl.69-0971

10* (LiC104) data in ref. 76-1087.

2k = (1.6 ± 0.2) 0.0075 25 3.6 Pr Measured in the pre- R.M. Sellers, x 10* sence of 1 mol/dm3 2-methyl-2-propanol

taking €mo = 7000

dm3 mol-1 cm

-1

.

unpub. data

10.2 Ina+ + OH (et) 2k = (4.9 ± 0.7) - 25 3.6 Pr Measured from the R.M. Sellers, x 10* initial decay of

Ina+ in the absence

unpub. data

of OH scavengers. 10.3 Ina+ + N20 < 108 25 nat y Estimated from the values of G(Na) measured in the

Sell72-0844

•y-radiolysis of

In3+ + Na0 solutions.

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2A).

Table 11. Iridium(II) reactions

No. Reaction A/dm3 mol-1

s -1 8 / t/° C PH Method Comments Ref.

Ir° {from eaq + IrClss_

) 11.1 Ir

11 + Ir11 (dis) 2k = (3.3 ± 0.4) 0.0018 RT - pr - Bros73-1066

x 10*

*If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2A).

Table 12. Manganese(I) reactions

No. Reaction A/dm3 mol-1s -1 8 / t/°C pH Method Comments Ref.

Mn+A<l 12.1 Mn+ + Cua+ (et?) AreJ = 1.6 ± 0.2 2.0 RT 5-8 y Measured by competi- Fiti70-0117

(MnSO«) tion kinetics using

N03 “ as competitor

in the presence of 0.5 mol dm-3 MnSO«.

Rate constant relative

to A(Mn+ + NOs

-

). 12.2 Mn+ + I03- (et?) Are, = 1.4 ± 0.1 2.0 RT 5-8 y Measured by competi- Fiti70-0117

(MnSO«) tion kinetics using

NOs” as competitor

in the presence of 0.5 mol dm-3 MnSO«.

Rate constant relative

to A(Mn+ + NO,").

12.3 Mn+ + N03_

(et?) see entries 12.1 and 12.2.

*If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

35
Table 13. Molybdenum reactions

No. Reaction A/dm3 mol-1

s

1 “ / t/°C pH Method Comments Ref.

[Mo^OuCCFs)*] (from Mo^OiCCFi)* + e, in methanol)

13.1 [Mo^OjCCFsh] +

[Mo2(OaCCFs)4]-

'A' = (4.5 ±

x 10*

1.0) — RT

(dis?) 'A' = (2.5 ±

x 10®

1.0) - RT

13.2 [Mo^OjCCFsW (5.9 ± 0.3) x 10B - RT

+ Oa (af?)

pr Measured from decay Baxe...76-1003

of Mo(l 1/2) species pr in methanol. Two decay

processes observed, one of which believed

to be a dismutation

reaction. Rate constant (unclear whether

A or 2A) calculated taking C780 = 2600

dm3 mol-1 cm

-1

. Note that if the slower process does

not involve the Mo(l 1/2) species, the value of €, and

hence A, is incorrect. pr Measured in Baxe...76-1003

Methanol.

Starting material [Mo^OjCCFsh]

not regenerated,

so reaction does

not involve

electron transfer.

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2A).

36
Table 14. Nickel(I) and nickel(III) reactions

No. Reaction A/dm3 mol-1

s

1 * / t/°c pH Method Comments Ref.

14.1 Ni+ + BrOr < 8.4 x 10* 0.08 RT nat P

r _ Meye.68-0855

14.2 Ni+ + Cda+ < 107 - RT nat P

r - Baxe..66-0848

14.3 Ni+ + Co(en)s,+ < 5 x 10* 0.08 RT 5-6 P

r - Meye.69-0428

14.4 Ni+ + cis— (5.9 ± 0.9) x 10s 0.08 RT 5-6 P

r - Meye.69-0428

Co(en)aCla+

(et) 14.5 Ni+ + trans- (8.3 ± 2.1) x 108 0.08 RT 5-6 P

r - Meye.69-0428

Co(en)aCl3+

(et) 14.6 Ni+ + Co(en)aCOs + < 5 x 10s 0.08 RT 5-6 P

r - Meye.69-0428

14.7 Ni+ + cis-Co(en)aFa+ < 5 x 10* 0.08 RT 5-6 Pr - Meye.69-0428

14.8 Ni+ + Co(en)aFHaOa+ < 5 x 10* 0.08 RT 5-6 P

r - Meye.69-0428

14.9 Ni+

4- cis- (4.7 ± 0.7) x 10* 0.08 RT 5-6 Pr - Meye.69-0428

Co(en)aNHsCla+ (et) 14.10 Ni+ + cis- (3.3 ± 0.8) x 10* 0.08 RT 5-6 Pr - Meye.69-0428

Co(en)aNHsNOaa+ (et) 14.11 Ni+ + Co(NHa)«3+ < 5 x 10* 0.08 RT 5-6 Pr - Meye.69-0428

14.12 Ni+ + Co(NHs)5 Bra+ (et) (1.05 ± 0.2) x 10" 0.08 RT 4.0 Pr - Meye.69-0428

14.13 Ni+ + Co(NHs)BCla+ (et) (6.5 ± 1.0) x 10* 0.08 RT 5-6 Pr - Meye.69-0428

14.14 Ni+ + Co(NHs)BCNa+ (et) (3.3 ± 0.8) x 10* 0.08 RT 5-6 Pr - Meye.69-0428

14.15 Ni+ + Co(NHs)5P+ < 5 x 10* 0.08 RT 5-6 Pr - Meye.69-0428

14.16 Ni+ + Co(NHs)BHa0

3+ < 5 x 10* 0.08 RT 4.0 Pr - Meye.69-0428

14.17 Ni+ + Co(NHs)BOHa+(et) (1.3 ± 0.3) x 10* 0.08 RT 7.6 Pr - Meye.69-0428

14.18 Ni+ + Co(NHs)sNsa+(et) (5.8 ± 1.5) x 108 0.08 RT 7.6 Pr - Meye.69-0428

14.19 Ni+ + (4.1 ± 1.0) x 108 0.08 RT 7.6 Pr - Meye.69-0428

Co(NH*)BNCSa+ (et) 14.20 Ni+ + < 5 x 10* 0.08 RT 5.6 Pr - Meye.69-0428

Co(NHj)sOOCCHsa+ 14.21 Ni+

-|- Crs+ < 107 - RT nat Pr - Baxe..66-0848

14.22 Ni+ + Cua+ < 2.4 x 107 0.08 RT nat Pr - Meye.68-0855

14.23 Ni+ + HaOa -> (3.2 ± 0.3) x 107 - 25 nat Pr - Buxt..76-1072

Nia+ + OH + OH” (4.3 ± 0.6) x 107 - RT nat Pr - Meye.68—0855

2.1 x 108 - RT nat Pr - Buxt..67-0062

Products identified in y-radiolysis studies (see

ref. 73-0039).

14.24 Ni+ + HaO

+ < 10* 0.08 RT nat Pr - Meye.68-0855

14.25 Ni+ + IOs - (et) (2.2 ± 0.3) x 108 0.08 RT nat Pr - Meye.68-0855

14.26 Ni+ + MnO«- (et) 7.5 x 10s 0.005 RT nat Pr Measured by the

rate of depletion of the MnO«~ absorption.

Baxe..65-0385

14.27 Ni+ + Ni+ slow (< 108

) var RT nat Pr Estimated from

decay of Ni+

in presence and

absence of OH

Kelm..74—1037

scavengers. 14.28 Ni+ + NOa- (et) (1.5 ± 0.2) x 108 0.08 RT nat Pr - Meye.68-0855

14.29 Ni+ + NOs" < 1.4 x 10* 0.08 RT nat Pr - Meye.68-0855

14.30 Ni+ + NaO 6.3 x 10* - RT nat Pr Measured in the Meye.68-0855

NiO+ + Na

(9.1 ± 0.9) x 10* - 25 ± 2 nat Pr

presence of 1 mol dm-3 NiSO<

Measured in the presence of 0.5 mol dm-3 NiSO«.

Buxt..76-1072

5.1 x 107 - RT nat Pr - Buxt..67-0062 E, = 40.6 ± 3.8 kj - 1-30 nat Pr - Buxt..67-0062 mol-1

37

Products inferred from y-ray induced

chain reaction in the system Nia+ +

HCOa + NaO. G(Na) also measured in Nia+ + NaO solutions,

(see ref. 73-0039).
TABLE 14. Nickel(I) and nickel(III) reactions — Continued

No. Reaction k/ dm3 mol-1

s _1 * I t/°C pH Method Comments

14.31 Ni+ + OH ^

Nia+ + OH2 x 1010 - RT nat pr Measured from a computer fit of

the decay of Ni+

in the absence

of OH scavengers assuming competing

reactions to be OH

-I- OH and Ni+ +

HaOj. Product

identified by conductivity measurements (but see ref. 75-1027).

14.32 Ni+ + 02 — NiOa+ (1.4 ± 0.2) x 10* - RT nat pr

2.2 x 10® - RT nat pr -

Product characterised by its absorption spectrum

(ref. 76-1072), reactivity with tetra- nitromethane and

lack of reactivity with 1,4—benzoqui- none (ref. 76-1134).

14.33 Ni+ + Pba+ < 107 - RT nat P

r -

14.34 Ni+ + Ru(NH3)ss+ (et) (4.0 ± 0.6) x 108 0.08 RT nat P

r -

14.35 Ni+ + Sa08s“ (1.5 Nia+ + SO«" + SO«a” ± 0.2) x 108 0.049 25 ± 2 nat Pr S04- product characterised by its absorption spectrum and decay kinetics. 14.36 Ni+ + Zna+ < 107 - RT nat Pr -

14.37 Ni+ + CHaOH —

NiCHaOH+

4.2 x 10® RT nat Pr Product characterised by its absorption spectrum and conductivity measurements.

14.38 Ni+ + CO," -*• NiCOa 6.6 x 10® 4 x 10-4 RT nat Pr Product characterised by its absorption spectrum and conductivity measurements. 14.39 Ni+ + CaH4OH -

NiCaH4OH+ 2.3 x 10® 4 x 10-4 RT nat Pr Product characterised by its absorption spectrum and conductivity measurements. 14.40 Ni+ + CHjCOHCHs -* NiCOH(CHs)a

1.4 x 10® 4 x 10-4 RT nat Pr Product characterised by its absorption spectrum and conductivity measurements.

14.41 Ni+ + HaC(CHs)aOH —

Nia+ + OH“ + CHa =C(CHs)a

3 x 10® 4 x 10-4 RT nat Pr Isobutene detected

as product; OH~

detected by conductivity measurements. 14.42 Ni+ + -C5 H9 -* NiCs H»+

(•CsH» = cyclopentyl radical)

2.8 x 10® 4 x 10-4 RT nat Pr Product characterised by its absorption spectrum and conductivity measurements.

Ref.

Kelm...74-1037

Meye.68-0855

Baxe..66-0848

Baxe..66-0848 Navo.70-1229

Tait.. 76-1001

Baxe..66-0848

Kelm...74-1037

Kelm...74—1037

Kelm...74— 1037

Kelm...74— 1037

Kelm...74— 1037

Kelm...74—1037

38
Table 14. Nickel(I) and nickel(III) reactions — Continued

No. Reaction A/dm3 mol-1 s~ l • I t/°C pH Method Comments

14.43 Ni+ + allyl alcohol —* ca. 103 - 25 ± 2 nat P

r -

Ni-allyl alcohol*

14.44 Ni+ + 1,4—benzo- (2.3 ± 0.5) x 103 _ 25 6.0 pr Measured by the quinone — Nia+ + rate of formation (1,4-benzoquinone)

- of the semiquinone

in the presence of

1 mol dm-3 2-methyl2-propanol. 14.45 Ni+ + menaquinone —

»

2.4 x 10» - ca. 25 7.0 Pr Measured by the Nia+ + (menaquinone)

-

(2.5 ± 0.3) x 10* RT 7.0 P

r rate of formation

of the semiquinone

in the presence

of ca. 1 mol dm-3

2-methyl-2-propanol.

14.46 Ni+ + tetranitro- (1.4 ± 0.2) x 10* - 25 ± 2 5.9 Pr Measured by the methane —* Nia+ + rate of formation C(NOa)s - + NOa of the nitroform anion in the presence of 1 mol dm-3 2-methyl2-propanol.

Ni(I) Complexes

NP-cyano complexes

14.47 Ni(CN)aa_ + Ni(CN)sa_ 2A = (1.5 ± 0.2) 0.1 20 ± 2 -

P

r Product charac- — Nia(CN)*4- x 103 (HCOaNa) terised by its absorption spectrum. 14.48 Ni(CN)43- - (8.1 ± 1.0) x 103 0.1 20 ± 2 -

P

r Ni(CN)aa_ characNi(CN)s*

- + CN“ 9-1 (HCOaNa)

MH HN.

terised by its absorption spectrum.

NiL+

(L = 5,5,7,12,12,14-hexamethyl-l,4,8,1 1-tetraazacyclotetradecane). c x

1

14.49 NiL+ + Co(bpy)s3+ (1.3 ± 0.1) x 10» 0.016- RT 7.0 P

r Measured in the 0.028 presence of 1 mol dm-3 2-methyl2-propanol. 14.50 NiL+ + (1.1 ± 0.1) x 10e 0.016- RT 7.0 P

r Measured in the CoL'(OHa)(OH)a+ (et) 0.028 presence of 1 mol dm-3 2-methyl2-propanol.

(L' = 5,7,7, 12, 14,14-hexamethyl-l,4,8,ll-tetraazacyclotetradeca-4, 11-diene). 14.51 NiL+ + Co(en)s3+

(et) (1.1 ± 0.1) x 10s 0.016- RT 7.0 Pr Measured in the 0.028 presence of 1 mol dm-3 2-methyl2-propanol. 14.52 NiL+ + Co(NH3)e3+

(et) (1.9 ± 0.2)x 10s 0.016- RT 7.0 P<- Measured in the 0.028 presence of 1 mol dm-3 2-methyl2-propanol. 14.53 NiL+ + CoL'(OH)a+

(et) (1.7 ± 0.2)x 107 0.016- RT 7.0 P

r Measured in the 0.028 presence of 1 mol dm-3 2-methyl2-propanol.

(L' = 2,3,9,10-tetramethyl-l,4,8,ll-tetraazacyclotetradeca-l,3,8,10-tetraene).

Ref.

Buxt..76-1072

Sell.76-1134

Rao.75-1032

Rao.73-1047

Sell.76-1134

Mula.... 74-1072

Mula....74-1072

Tait..76-1039

Tait..76-1039

Tait..76-1039

Tait.. 76-1039

Tait.. 76-1039

39
TABLE 14. Nickel(I) and nickel(III) reactions — Continued

No. Reaction A/dm3 mol-1 s“l a / t/° c PH Method Comments Ref.

14.54 NiL+ + Cr(bpy)s3+(et) (7.7 ± 0.8) x 103 0.016-

0.028 RT 7.0 P

r Measured in the presence of 1 mol dm-3 2-methyl2-propanol.

Tait..76-1039

14.55 NiL+ + Fe(bpy)ss+ (et) (6.4 ± 0.6) x 107 0.016-

0.028 RT 7.0 P

r Measured in the presence of 1 mol dm-3 2-methyl2-propanol.Tait..76-1039

14.56 NiL+ + HsO

+

(pt) (1.1 ± 0.1) x 10® 0.06-

0.3 RT <1.25 Pr Reaction mayinvolve proton

transfer to the metal centre to give a hydrido

complex.

Tait..76-1039

14.57 NiL+ + HaPOr (pt) < 104 0.01-

0.1 RT 5.50 P

r Tait..76-1039

14.58 NiL+ + NaO (et or 0 at) (3.9± 0.4) x 107 RT 7.0 Pr Reaction possibly involves two

electron oxidation

to Ni(III) complex.

Tait..76-1039

14.59 NiL+ + Oa NiL2+ + Oa"

(1.6 ± 0.2) x 10* RT 7.0 P

r Product transfers an electron to

1 ,4-benzoquinone

but not menaquinone,

and identified therefore as Oa", although Oa adduct, NiLOa+ could conceivably react in same way.

Tait..76-1039

14.60 NiL+ + Ru(NHs)«3+

(et)

(3.8 ± 0.4) x 108 0.016-

0.028 RT 7.0 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1039

14.61 NiL+ + Ru(NH3)5N03+

(et)

(7.4 ± 0.7) x 107 0.016-

0.028 RT 7.0 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1039

14.62 NiL+ + acetic acid

(pt)

(1.2 ± 0.1) x 104 0.015-

0.06 RT 4.85 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1039

14.63 NiL+ + 9,10-anthraquinone-2,6-disulphonate

(et)

(4.8 ± 0.5) x 10* 0.004 RT 7.0 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1039

14.64 NiL+ + 1,4—benzoquinone (et)

(4.8 ± 0.5) x 10® 0.004 RT 7.0 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1039

14.65 NiL+ + 3-benzoylpyridine (et)

(2.5 ± 0.3) x 108 0.004 RT 7.0 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1039

14.66 NiL+ + fluorescein

(et)

(3.2 ± 0.3) x 10® 0.004 RT 7.0 Pr Measured in the presence of 1 mol

dm^3 2-methyl-2-

propanol.

Tait..76-1039

14.67 NiL+ + methyl iodide

(et or Sn2)

(4.6 ± 0.5) x 108 0.01 RT 9.2 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1039

40
Table 14. Nickel(I) and nickel(III) reactions — Continued

No. Reaction A/dm3 mol 1 s

1 * / </°C PH Method Comments Ref.

M HN. NiL+

(L = 5,7,7,12,14,14-hexamethyl-l,4,8,l l-tetraazacyclotetradeca-4,1 1-diene). C7JH N)

14.68 NiL+ + Co(bpy)ss+ (1.3 ± 0.1) x 10» 0.016- RT 7.0 P

r Measured in the Tait.. 76-1039

(et) 0.028 presence of 1 mol

dm-3 2-methyl-2-

propanol. 14.69 NiL+ + (2.6 ± 0.3) x 10« 0.016- RT 7.0 P

r Measured in the Tait..76-1039 CoL'(OHa)(OH)2+

(et) 0.028 presence of 1 mol

dm-3 2-methyl-2-

propanol.

(L' = 5,7,7, 12, 14, 14—hexamethyl-l ,4,8, 1 l-tetraazacyclotetradeca-4, 1 1-diene). 14.70 NiL+ + Co(en)ss+ (et) (1.1 ± 0.1) x 10s 0.016- RT 7.0 P

r Measured in the Tait.. 76-1039

0.028 presence of 1 mol

dm-3 2-methyl-2-

propanol. 14.71 NiL+ + Co(NHs)«s+ (et) (1.9 ± 0.2) x 10s 0.016- RT 7.0 P

r Measured in the Tait.. 76-1039

0.028 presence of 1 mol

dm-3 2-methyl-2-

propanol. 14.72 NiL+ + CoL'(0H)2+

(et) (3.6 ± 0.4) x 107 0.016- RT 7.0 Pr Measured in the Tait..76-1039 0.028 presence of 1 mol

dm-3 2-methyl-2-

propanol.

(L' = 2,3,9,10-tetramethyl-l,4,8,l l-tetraazacyclotetradeca-l,3,8,10-tetraene). 14.73 NiL+ + Cr(bpy)ss+ (1.1 ± 0.1) x 108 0.016- RT 7.0 Pr Measured in the Tait.. 76-1039

0.028 presence of 1 mol

dm-3 2-methyl-2-

propanol. 14.74 NiL+ + Fe(bpy)ss+ (et) (2.2 ± 0.2) x 10s 0.016- RT 7.0 P

r Measured in the Tait..76-1039 0.028 presence of 1 mol

dm-3 2-methyl-2-

propanol. 14.75 NiL+ + HsO

+

(pt) (1.3 ± 0.1) xlO® 0.06-0.3 RT <1.25 Pr Reaction may involve proton transfer to the metal centre to give a hydrido complex

Tait.. 76-1039

14.76 NiL+ + HaPOr (pt) (2.4 ± 0.2) xlO* 0.01-0.1 RT 5.50 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait.. 76-1039

14.77 NiL+ + NaO (et or (1.8 ± 0.2) x 107 - RT 7.0 Pr Measured in the Tait.. 76-1039

0 at) presence of 1 mol

dm-3 2-methyl-2-

propanol. Reaction

possibly involves two electron oxidation to Nim complex. 14.78 NiL+ + Oa -> (1.7 ± 0.2) x 10* - RT 7.0 Pr Product transfers Tait.. 76-1039

NiL2+ + Oa”

41

an electron to

1 ,4—benzoquinone

but not menaquinone, and identified therefore as Oa

-

, although Oa adduct NiLOa+

, could conceivably react in same way.
Table 14. Nickel(I) and nickel(III) reactions — Continued

No. Reaction A/dm3 mol-1

s

1 * / t/°c pH Method Comments Ref.

14.79 NiL+ + Ru(NHs)a3+(et) (4.5 ± 0.5) x 103 0.016-

0.028 RT 7.0 P

r Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1039

14.80 NiL+ 4

Ru(NHs)5N03+

(et)

(3.5 ± 0.4) x 107 0.016-

0.028 RT 7.0 P

r Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait.76-1039

14.81 NiL+ 4 acetic acid

(pt)

(1.9 ± 0.2) x 10s 0.015-

0.06 RT 4.85 P

r Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait.76-1039

14.82 NiL+ 4 9,10-anthraquinone-2,6-disulphonate

(et)

(5.0 ± 0.5) x 10* 0.004 RT 7.0 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1039

14.83 NiL+ 4 1,4—benzoquinone

(et)

(3.8 ± 0.4) xlO* 0.004 RT 7.0 P

r Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait.76-1039

14.84 NiL+ + 3-benzoylpyridine (et)

(7.5 ± 0.8) x 10s 0.004 RT 7.0 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait..76-1039

14.85 NiL+ + eosin Y (et) (2.7 ± 0.3) x 10B 0.004 RT 7.0 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait.76-1039

14.86 NiL+ + fluorescein (et) (3.3 ± 0.3) x 10* 0.004 RT 7.0 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait.76-1039

14.87 NiL+ 4 methyl iodide

(et or Sn2)

Ni(l) radical complexes

(1.3 ± 0.1) x 108 0.01 RT 9.2 Pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol.

Tait.76-1039

14.88 NiCHaOH+ 4 H20 ->

Nia+ 4 CHsOH 4 OH"

7 s_1 RT nat Pr Products characterised by conductivity experiments.

Kelm...74-1037

14.89 NiCHaOH+ 4 HaOa (et?) 7.3 x 103 - RT nat Pr - Kelm.. .74-1037

14.90 NiCOa 4 HaO < 1 s

_1 - RT nat Pr - Kelm.. .74-1037

14.91 NiCaH4OH+ 4 HaO —

Nia+ 4 CaHsOH 4 OH"

5 s' 1 RT nat Pr Products characterised by conductivity experiments.

Kelm. ..74— 1037

14.92 NiCaH«OH+ 4 HaOa (et?) 2.3 x 104 - RT nat Pr - Kelm.. .74-1037

14.93 NiCOH(CHj)a+ 4 HaO < 1 s_l - RT nat Pr - Kelm...74—1037

14.94 NiCOH(CHs)a+ 4 HaOa 1.1 x 10« - RT nat Pr - Kelm. ..74— 1037

14.95 NiCaH40CaHB + 4 HaO < 1 s_1 - RT nat Pr - Kelm...74— 1037

14.96 NiCaH4 OCaHs+ 4 HaOa 1.3 x 103 - RT nat Pr - Kelm...74-1037

14.97 NiCsH»+ 4 HaO -

Nia+ 4 C5H10 4 OH49 s-1 RT nat Pr Products characterised by conductivity experiments.

Kelm.. .74-1037

14.98 NiCs H,+ 4 HaOa

(CsHs = cyclopentyl radical) NiOSNiOJP+

< 5x 10* RT nat Pr Kelm...74—1037

14.99 NiOa+ -+ Nia+ 4 Oa

_ 780 ± 80 s_1 - 25 ± 2 5.7 Pr Measured from the SeU.76-1134

rate of formation

of the nitroform anion in solutions contining tetra- nitromethane and 1 mol dm-3 2-methyl-2-

42 propanol.
TABLE 14. Nickel(I) and nickel(lll) reactions — Continued

No. Reaction A:/dm3 mol 1 s

1 “ / </°C pH Method Comments Ref.

14.100 NiOa+ + H

+ K = 2000 ± 1200 M"1 0.04 25 ± 2 3.0- P

r Measured from the pH Sell.76-1134 NiOaH

2+

(i.e. pX, = 3.2 ± 5.7 dependence of the

0.3) rate of formation of

the nitroform anion

in solutions containing tetranitromethane and

1 mol dm-3 2-methyl-2-

propanol. 14.101 NiOaH

2+ -> > 2800 s _1 25 ± 2 3.0 P

r Estimated from the SeU.76-1134

Ni2+ + HOa rate of formation

of the nitroform anion in solutions containing tetra- nitromethane and 1 mol dm-3 2-methyl-2-

propanol.

Ni(III) complexes 14.102 Nira(NHs)n + NaH« (4 ± 1) x 106 RT 11.3 P

r - Lati.72-0460 14.103 Nim(NHs)n + Nim(NHs)n 2k < 3.5 x 107 RT 11.3 P

r - Lati.72-0460

Rate constants for the decay of Nira(en)„ and Nim(gly)„ are given in tables III and IV respectively of ref. 72-0461.

These rate constants cannot be attributed to any specific reaction.

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

43
TABLE 15. Lead(I) reactions

No. Reaction k/dm* mol-1

s-1 “ / t/°C pH Method Comments Ref.

15.1 PbUPb+ + Cda+ < 107 RT nat pr Baxe..66-0848

15.2 Pb+ + Cr*+ < 107 - RT nat pr Baxe..66-0848

15.3 Pb+ + Nia+ < 107 - RT nat pr Baxe. .66-0848

15.4 Pb+ + 02 - 3.9 x 10® - RT nat pr Baxe. .66-0848

Pba+ + 02- Product transfers an electron to 1,4-

benzoquinone and

tentatively identified as Oj“. (Ref. 76-1134).

15.5 Pb+ + OH (et) 7.7 x 10® - RT nat pr Reinterpreted from Baxe..66-0848

data in ref. 66-0848

on decay of Pb+in the absence of OH scavengers. Principal competing reaction, Pb+ +

Pb+

, not taken into account. 15.6 Pb+ + Zna+ < 107

15.7 Pb1 + 1,4-benzo- (4.1 ± 0.8)x 10® quinone —* Pba+ +

( 1 ,4—benzoquinone)

-

15.8 Pb+ + menaquinone —* (3.7 ± 0.4) x 10® Pba+ + (menaquinone)

-

RT nat 25 ±2 6.3

RT 7.2

pr - Baxe..66-0848

pr Lead(II) acetate Sell.76-1134

salt used, Pb+ may be complexed

to acetate. Measured

from the rate of formation of the benzosemiquinone

product in the presence of 1 mol

dm-

* 2-methyl-2-

propanol. pr Measured by the Rao.75-1032

rate of formation Rao.73-1047

of the semiquinone

in the presence of

ca. 1 mol dm-* 2-methyl-2-propanol.

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

44
Table 16. Praseodymium(IV) reactions

No. Reaction k/ dm* mol 1 s

1 * / t/°C PH Method G>mments Ref.

16.1 Pr4+ + H,0

PrOH,+ + H

+ K — (7 ± 1) x 10 4 var

or pAT. = 3.1 ± 0.1 RT 1.95-

5.87 P

r Measured from effect of pH on absorption

of Pr(IV).

Fara.72-0066

16.2 PrTM + Br

-

(et or af) (1.2 ± 0.4) x 101 ® 0.75

[Pr,(SO«)s] RT nat P

r Fara.72-0066

16.3 PrTM + HaQa (H at ?) (8 ± 1) x 10« 0.75

[Pra(SO«)s] RT nat P

r “ Fara.72-0066

16.4 PrTM + HSO*-

(et or H at)

(2.0 ± 0.3) x 10« “ RT 2-3.8 Pr Fara.72-0066

16.5 PrTM + NO," (et?) (3 ± 1) x 107 0.75

tPr*(SO«)3] RT nat Pr Fara.72-0066

16.6 Priv + Priv

(see comments)

2k = (1.6 ± 0.8) x 10» RT 5.8 Pr Stable products of

reaction suggested

to be PrTM and

Oa. Initial product

possibly an oxo or hydroxo bridged

dipraseodymium species.

Fara.72-0066

•If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

45
TABLE 17. Platinuni(I) and platinum(III) reactions

No. Reaction A/dm* mol-1

s -1 a / t/°C PH Method Comments Ref.

Pif Reactions

Pt1 from PtCU2~ +

17.1 Pt1 + N»0 (et or 0 at) < 4 x 10* - RT nat P

r - Ghos.69-0144

17.2 Pt1 + Oa (et or af) < 2 x 107 - RT nat P

r - Ghos.69-0144

17.3 Pt1 + Pt1 -+ Pt° + 'k' = (4.1 ± 0.5) 0.003 RT nat Pr Unclear whether Ghos.69-0144

ptn x 10® rate constants

refer to k or 2k. T = (3.15± 0.15) 0.013 RT nat P

r Measured in the Ghos.69-0144

x 10® presence of 0.1 mol

dm”® KQ.

'k' = ca. 2.5 x 0.018 RT 2 Pr - Ghos.69-0144

x 10® Products identified

in y-radiolysis

experiments (see ref. 62-0164).

Pt1 from Pt{CN)P~ + e,q 17.4 Pt1 + NaO (et or 0 at) (1.8 ± 0.25) x 107 - RT nat Pr - Ghos.69-0144

17.5 Pt1 + Oa (et or af) (3.5 ± 0.5) x 10® - RT nat Pr - Ghos.69-0144

Pt1 from PtLCl+ + e,q (L == diethylenetriamine). 17.6 Pt1 + Pt1 (? see 2k = (4.6 ± 2.0) 2 x 10"4 ca. nat Pr Rate constant Stor...75-1188 comments) x 107 25 represents decay of second transient produced from Pt11 + Caq- First transient decays by a first order reaction with

(2.3 ± 1.3) x 10®

s -1

, probably

associated with

the substitution of CT by H20.

Pt1 from PtLCl* + H(L = diethylenetriamine). 17.7 Pt1 + Pt1 (dis?) 2k = (6.8 ± 0.8) - ca. 2-3 Pr - Stor...75-1 188

x 10® 25

Pt1 from Pt{en)2a+ + e*. 17.8 Pt1 + Pt1 (dis?) 2k = (9.0 ± 0.8) 4 x 10-4

ca. nat Pr - Stor...75-1188

x 10® 25

Pt1 {from Pt(en)a2+ + H

17.9 Pt1 + Pt1 (dis?) 2k = (2.8 ± 0.6) - ca. 2-3 Pr - Stor.. .75-1 188

x 10® 25

Pt1 from PtLCl* + H (L = tetraethyldiethylenetriamine)

.

17.10 Pt1 + Pt1 (dis?) 2k = (1.3 ± 0.6) - ca. 2-3 Pr - Stor.. .75-1 188

x 10“ (!) PtTM Reactions PtTMfrom PtCU2- + Cla" 17.11 (PtTM)1 -> (PtTM)11 (3 ± 1) x 10s s"1 - ca. 0.3 Pr Reaction probably Stor...75-1188

(see comments for 25 associated with mechanism) change in number

of chloride ligands

and/or substitution of a

- by HiO.

Measured in the presence of 0.5 mol

dm"® HQ.

17.12 PtTM + Cun

(et) (1.5 ± 0.2) x 10® 0.5 ca. 0.3 Pr Measured in the Stor...75-1188 (HQ) 25 presence of 0.5 mol dm-

* HQ.

Cun in the form

of chloro complex.

46
TABLE 17. Platinum(I) and platinum(III) reactions — Continued

No. Reaction k/dm3 mol 1 9

1 • I t /°C pH Method Comments

17.13 PtTM + PtTM (dis) 2k = ca. 2 x 10» 0.5 ca. 0.3

(HC1) 25

17.14 PtTMfrom PtCU2~ + hv

PtTM + Fe2+(et) (2.8 ± 0.3) x 10® 2 x 10-3

17.15 PtTM + PtTM (dis) 2k = (4.6 ± 0.4) x 106 10 3 ca. 205.8

from PtClS' + OH

OH

1.8 x 10s s-1

2.0 x 105 s-1

RT nat

RT nat

2.0 x 10s s-1 RT nat

PtTMfrom Pt(en)i2+ + Cli 17.17 (PtTM)1 -> (PtTM)11 (1.3 ± 0.1) x 10s s _1

ca. 0.3 25

pr Rate constant is for the decay of

the second transient PtTM species,

(Ptm)u

in entry 17.11. Measured in the presence of

0.5 mol dm-3 HQ.

f.ph. From dependence of

rate constant for

this reaction on ionic strength charge on PtTM is -1, and identified therefore as PtCU

-

. Broszkiewicz and Grodkowski (ref. 76-1055) suggest however that the reaction observed under the conditions employed was

Cla" + Fea+ . Other

experiments give k =

(4.0 ± 0.6) x 10® dm3 mol-1

9-1 for Cla- +

Fe2+. f.ph. Rate constant cal- culated taking

€410 = 3.7 x 103 dm3 mol-1 cm

-1

.

pr Rate constant measured from

decay of reactant

at 450 nm.

pr Rate constant measured from

decay of reactant

at 450 nm.

pr Rate constant measured from

build-up of product at 400 nm.

Ligand reorganization mechanism

implied from similarity of products

of PtCL2- + OH

and PtCL2- + e»q

(ref. 68-0169).

pr Decay approxi- mates to two

consecutive first order processes

(see also 17.18). Measured in the presence of 0.5 mol dm-3 HQ.

Ref.

Stor... 75-1 188

Wrig.72-7088

Wrig.72-7088

Adam..68-0169

Ghos.69-0144

Adam..68-0169

Stor.. .75-1 188

47
TABLE 17. Platinum(I) and platinum(III) reactions — Continued

No. Reaction A/dm3 mol 1 s_1 * I t/° C PH Method Comments Ref.

17.18 (Pt111^—, (ptnyu 7.7 ± 0.8 s_1 _ ca. 0.3 Pr Measured in the Stor...75-1188 25 presence of 0.5 mol dm-3 HQ.

See also comments

under 17.17. 17.19 Pt® + Cu11 (et) (3.2 ± 0.7) x 10® 0.5 ca. 0.3 P

r Measured in the Stor...75-1188 (HQ) 25 presence of 0.5 mol dm-3 HQ.

17.20 PtTM -|- Fe11 (et) (2.5 ± 0.4) x 10* 0.5 ca. 0.3 Pr Measured in the Stor...75-1188 (HQ) 25 presence of 0.5 mol dm-3 HQ.

/*®from Pt(enW+ + OH

17.21 (PtTM)1 — (Ptm)u

(2.5 ± 0.2) x 105 - RT 4.0-7.0 P

r - Brod...76-1093

+ H

+

s" 1

(2.4 ± 0.3) x 10s

Q — 1 - RT 7.0-9.6 P

r - Brod...76-1093

17.22 (PtTM)4 + OH" -*

s (3.1 ± 0.5) x 1010 __ RT 7.0-9.6 P

r _ Brod...76-1093

(Ptm)U + Ha0

17.23 (PtTM)' + H

+ - (4.2 ± 0.9) x 10» - RT 4.0-7.

0

P

r - Brod. ..76-1093

(PtTM)111 17.24 (PtTM)11 + (1.5 ± 0.4) x 10* - RT 2.9-8.5 P

r Measured in the Brod...76-1093

(PtTM)11 (dis?) presence of (0-2) x 10-3 mol dm-3 Q".

(4.3 ± 2.8) x 10* - RT 4.0-9.

1

f.ph. Measured in the Brod. ..76-1093

presence of (0-1) x 10-5 mol dm-3 Q

-

. Unclear whether

these rate constants

refer to k or 2k. 17.25 ( Ptm)U + Cun < 104 - RT 6.3-6.6 Pr - Brod...76-1093

17.26 (Ptmju + (2.3 ± 0.2) x 108 - RT 6.3-6.6 Pr - Brod...76-1093

Fe(CN)6

4- (et) 17.27 (PtTM)11 + q2 < 105 - RT 6.3-6.6 Pr - Brod. ..76-1093 17.28 (PtTM)TM (6.6 ± 1 . 8) x 10s - RT 2.8-4.3 Pr Cf. entry 17.23 Brod...76-1093

(PtTM)1 + H

+ or pAT„ = 6.8 ± 0.2 17.29 (ppnjiu ? 28 ± 6 s"1 RT 2.8-4.3 Pr Reaction may be second order.

Brod.. .76-1093

17.30 (PtTM)11 + cr — (1.11 ± 0.09) x 10» - RT 3-4,5.

1

Pr - Brod. ..76-1093

(Ptm)lv

17.31 ( Ptm)iv + Cun

(2.7 ± 1.0) x 10s - RT 2.1 Pr Measured in the Brod.. .76-1093

(et?) presence of 5 x 10

~6 mol dm-3 Q“.

(3.2 ± 1.1) x 105 RT 2.0 f.ph. Measured in the presence of 0-0.5 mol dm-3 2-methyl2-propanol.

Mechanism of reaction may be complex as the

rate constants were

appreciably higher

(25-50%) at the lower [Cu11

] employed. 17.32 (PtTM)lv + 'k' = (5.7 ± 1.0) x 107 - RT 3.4 Pr Measured in the Brod.. .76-1093

(Ptnl

)lT (dis?) presence of 10-B mol dm-3 Q“. Rate

constant calculated taking £300 (Ptm)lT = 9070 dm3 mol-1 cm

-1

. 48
TABLE 17. Platinum(I) and platinum(III) reactions — Continued

No. Reaction A/dm3 mol 1 s

1 3 t/° C pH Method Comments Ref.

17.32 Cont. 'k' = (4.9 ± 1.9) x 107 RT 2.0 f.ph.

PtTMfrom tnzns-Pt(en)aClia+ + eaq or CHaCOHCHa

17.33 PtTM + PtTM (dis) 2k = (5.8 ± 1.0) x 107

PtTMfrom trans-Pt{en\iClia+ + H

17.34 PtTM + PtTM (dis) 2k = (8.8 ± 1.0) x 107

PfTMfrom trans-f,t{en)'2Cla2+ + ’CHiOH

17.35 PtTM + PtTM (dis) 2k = (1.04 ± 0.38) x 10*

Pf°from Pt(dien)Cl+ + CU~

17.36 PtTM + Cun (et) (3.2 ± 0.7) x 10*

17.37 PtTM + PtTM

(dis)

2k = (6.8 ± 1.6) x 10*

PtTMfrom Pt(dien) Cl+ + OH

17.38 (PtTM)1 -* (4.8 ± 0.8) x 10s

(Ptm)U

PtTMfrom PtLCl+ + Clt (L = tetraethyldiethylenetriamine). 17.39 PtTM + Cu11 (1.5 ± 0.4) x 107

17.40 PtTM + PtTM 2A = ca. 8 x 10*

PtTMfrom PtLCl+ + OH (L = tetraethyldiethylenetriamine). 17.41 (PtTM)1 (Pt111

)

11 1.8 ± 0.6 s_1

ca. 25

ca. 25

ca. 25

ca. 25

ca. 25

RT

ca. 25

ca. 25

ca. 25

0.3

0.3

nat

0.3

0.3

nat

P

r

P

r

P

r

P

r

Pr

P

r

P

r

Pr

Pr

Measured in the presence of (0-1) x 10-s mol dm-3

Cl~ and 0-0.5 mol

dm-3 2-methyl-2-

propanol. Rate

constant calculated taking €a«o(Ptm)lT = 9490 dm3 mol-1 cm

-1

. Unclear whether

these rate constants refer to k or 2k.

Measured in the presence of 2.6 mol dm-3 2-

propanol.

Measured in the presence of 0.11-

2 mol dm-3 2-methyl2-propanol.

Measured in the presence of 2-4

mol dm-3 methanol.

Measured in the presence of 0.5 mol dm-3 HQ.

Measured in the presence of 0.5 mol dm-3 HQ.

Rate constant

for initial decay

of PtTM transient. This process is followed by (i) an intermediate

process exhibiting

mixed order kinetics, and (ii) a slow second order decay

with 2k = (7.6 ±

0.6) x 10* dm3 mol-1

s"».

Measured in the presence of 0.5 mol dm-3 HQ.

Measured in the presence of 0.5 mol dm-3 HQ.

Brod...76-1093

Stor... 75-1 188

Stor... 75-1 188

Stor.. .75-1188

Stor.. .75-1 188

Stor.. .75-1 188

Brod...76-1093

Stor.. .75-1 188

Stor.. .75-1 188

Brod. ..76-1093

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

49
Table 18. Rhodium(II) reactions

No. Reaction A/dm3 mol-1

s

1 * t/'C PH Method Comments Ref.

Rh(NHs)ti+ and related complexes 18.1 Rh(NHs)«a+ -|- HaO 3.5 x 109 s'1 Rh(NHs)sH2Oa+ + NH,

18.2 Rh(NHs)3Ha04+ + HaO — 40 s" 1 Rh(NHs)a(HaO)aa+ + NHS

18.3 Rh(NHs)«a+ + Oa — 3.1 x 10* OaRh(NHs)4a+

18.4 Rh(NHs)4a+ + 2k = ca. 1.2 x 107 Rh(NH3)«2+ (dis?)

18.5 Rh(NHs)4a+ + ca. 1.4 x 10* Rh(NH3)4Bra

+ -* Rh(NHs)«3+ + Rh(NHs)«Bra

RT 4.0

RT 4.0

RT 4.0

RT 4.0

RT 4.0

P

r

P

r

P

r

P

r

P

r

Rate constant measured by change in conductivity result- ing from NHs + H

+ —* NH4+

. Solutions contained also 0.5 mol dm-3 2-methyl-2-

propanol. Rate constant measured by change in conductivity result- ing from NHs + H

+ —*• NH4+

. Solutions contained also 0.5 mol dm-3 2-methyl2-propanol. Product characterised by coductivity measurements. Measured

in the presence

of 0.5 mol dm-3

2-methyl-2-propanol.

Estimated from dependence of chain length in the Rh(NHs)4a+ +

Rh(NHs)4Bra

+

reaction on dose

rate. Estimated from

initial conductivity change.

Measured in the presence of 0.5 mol dm-3 2-methyl2-propanol. Products inferred from chain reaction which ensues.

Lili..75-1128

Lili..75-1128

Lili.. 75-1128

Lili.. 75-1128

Lili..75-1128

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

50
Table 19. Ruthenium(I), (II), (III) and (IV) reactions

No. Reaction A/dm3 mol-1

s

1 * I t /°C pH Method Comments

Ru1 Ru(NH3)JV2+

19.1 Ru(NH,)5N/ + 2k = 2.7 x 10» < 6 x 20 ± 2 nat Ru(NHs)bN*+

(dis) 10"4

Ruu

19.2 Ru(NHs)bCT + HaO 4.7 ± 0.4 s” 1 Ru(NHs),Ha02+ + Cr20 nat

19.3 Ru(NHs)bH20

2+ + 1.0 x 103 3 x 10-4 Ru(NHs)sa2+ —

Ru(NHs)bC1 + + Ru(NHs)sH20

3+

20 nat

19.4 Ru(NHs)»N02+ + 02 7.6 x 10*

(et or af) RT -

19.5 Ru(NHs)5 N02+ + HaCC(CHs)aOH 3.7 x 10* -> Ru(NH,)5NO. CH2C(CH3)aOH2+ RT 1.0-10.3

19.6 Ru(NHs )bN0

2+ + 3 x 10" RT nat 02CH2 C(CHs)a0H

(af or et)

Rum

19.7 Ru(NHs)sNas+ + H20-+ 250 ± 20 s"1 - 20 ± 2 nat Ru(NHs)sOHa+ + H

+ + Na

270 ± 20 s_1 - 20 ± 2 nat

pr Deposit of mettallic ruthenium and molecular

nitrogen (G(Nj) = 1.25) formed

as stable products. Immediate

products of reaction unknown.

pr Product characterised by its absorption spectrum,

pr Products inferred from fact that radiation brings about complete

aquation of Ru(NHs)sQ2+

. pr

pr Measured in the presence of 0.1 - 2.0 mol dm-3 2-methyl-2-

propanol. Product characterised by elemental

microanalysis, ion exchange chromatography, and uvvisible, ir and nmr spectroscopy, pr Measured in the presence of

1 mol dm-3 2-

methyl-2-propanol.

pr Measured from

decay of Ru(NHs)sNas+

absorption. pr Measured from

the formation

of Ru(NHs)bOH2+. Ru product characterised by its absorption spectrum

G(Na) = 9.7 (=

2 G eaq + Goh) measured in yradiolysis experi- ments with NaO

saturated solutions.

Ref.

Baxe. 71-0234

Baxe..70-0178

Baxe. .70-0178

Armo.75-1049

Armo..75-1077

Armo..75-1077

Baxe.71-0234

Baxe.71-0234

51
TABLE 19. Ruthenium(I), (II), (III) and (IV) reactions — Continued

No. Reaction A/dms mol 1 s

1 • </'C pH Method Comments Ref.

RuTM (The precise nature of these complexes is uncertain; aU were formed by OH oxidation of the corresponding Rum complex). 19.8 Ru(NHs)«4+ +

Ru(NHa)«4+ (dis)

19.9 Ru(NH,)sas+

products

4.5 x 10® 3 x 10-s 20 nat pr Unclear whether Baxe..70-0178

rate constant

refers to k or

2k. A product

of this reaction

(possibly Ru(NHs)«5+

) decays by a first order process with

k = 0.75 s_I

. Further, slower

reactions ensue

before the formation

of the stable products, and these presumably are due

to aquation and

hydrolysis reactions. 2.5 x 10s s~l 3 x 10-s 20 nat pr The product of Baxe. .70-0178

this reaction undergoes two

further unimolecular reactions with

rate constants of 44 and 0.45 s-1

. These are probably

associated with aquation and hydrolysis reactions.

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

52
TABLE 20. Samarium(II) reactions

No. Reaction k/dm* mol 1 s

1 * / t/°C PH Method Comments Ref.

5i/ia+

.q 20.1 Sm2+ + BrO," (et) 7.1 x 108 0.015 RT nat P

r - Fara.72-0065

(7.0 ± 0.5)x 107 0.0375 RT 6 P

r - Pika. .73-1084

20.2 Sml+ + Co(en)ss+ < 1 x 108 0.06- RT 6 Pr - Fara. 73-0107

1.0 20.3 Sma+ + Co(NH,)5Br3+ 3.5 x 107 0.06 RT 6 P

r - Fara.73-0107

(et) 1.6 x 10s 1.0 RT 6 P

r Fara.73-0107

(NaC10«)

2.5 x 10» 1.0 RT 6 Pr - Fara.73-0107

(NaCl) 20.4 Sm2+ + Co(NHs)*Cla+ 3.8 x 107 0.06 RT 6 P

r - Fara.73-0107

(et) 1.7 x 108 1.0 RT 6 P

r Fara.73-0107

(NaC10«)

2.3 x 108 1.0 RT 6 Pr - Fara.73-0107 (NaQ)

20.5 Sma+ + Co(NHs)sCNa+ < 3.0 x 109 0.06 RT 6 Pr - Fara.73-0107

20.6 Sma+ + Co(NH,)Fa+ 2.5 x 107 0.06 RT 6 P

r - Fara.73-0107

(et) 1.1 x 108 1.0 RT 6 Pr - Fara.73-0107

(NaClOi)

1.8 x 108 1.0 RT 6 Pr - Fara.73-0107

(NaCl) 20.7 Sma+ + Co(NH3)5H2Os+ 6.0 x 108 0.3 RT - Pr - Fara.73-0107

(et) 8.8 x 108 1.0 RT - Pr - Fara.73-0107

(NaClOi)

2.6 x 107 1.0 RT - Pr - Fara.73-0107

(NaCl) 20.8 Sma+ + Co(NH,)5Ia+ (et) 5.8 x 107 0.06 RT 6 Pr - Fara.73-0107

20.9 Sma+ + Co(NHs)5Ns2+

(et) 7.8 x 107 0.06 RT 6 Pr - Fara.73-0107

2.5 x 108 0.5 RT 6 Pr - Fara.73-0107

(NaC10«) 20.10 Sm2+ + Co(NH3)5NCSa+ < 1.0 x 109 0.06 RT 6 Pr - Fara.73-0107 < 1.0 x 109 0.5 RT 6 Pr - Fara.73-0107 (NaC104) 20.11 Sma+ + Co(NH3).3+ < 1.0 x 10s 0.06 RT 6 Pr - Fara.73-0107

(et) 5.0 x 10s 1.0 RT 6 Pr Fara.73-0107

(NaCl) 20.12 Sma+ + Co(NH3)50Ha+ 1.5 x 107 0.3 RT - Pr - Fara.73-0107

(et) 5.0 x 107 1.0 RT Pr Fara.73-0107 (NaC104) 5.0 x 107 1.0 RT - Pr - Fara.73-0107

(NaCl) 20.13 Sma+ + CrO«a- (et) (4.0 ± 0.5) x 109 0.375 R1 6 Pr - Pika. .73-1084

20.14 Sm2+ + Cua+ (et) 8.3 x 107 0.015 RT nat Pr - Fara.72-0065

20.15 Sma+ + H203 (et) 3.5 x 107 0.015 RT nat Pr - Fara.72-0065

(6.7 ± 0.3) x 107 0.375 RT 6 Pr - Pika..73-1084

20.16 Sm2+ + Eu3+

(et) 7.5 x 108 0.015 RT nat Pr - Fara.72-0065

20.17 Sm2+ + I03“ (et) 4.9 x 107 0.015 RT nat Pr - Fara.72-0065

20.18 Sm2+ + MnC>4

-

(et) (4.7 ± 0.5) x 10* 0.375 RT 6 Pr - Pika.. 73-1084

6.5 x 10* 0.015 RT nat Pr - Fara. 72-0065

20.19 Sma+ + NOj~ (et) 1.1 x 10» -»0 RT nat Pr - Fara. 72-0065

(1.3 ± 0.2) x 10" 0.375 RT 6 Pr - Pika. .73-1084

20.20 Sm2+ + NO," (et) (1.5 ± 0.2) x 108 0.375 RT 6 Pr - Pika. .73-1084

2.0 x 10* 0.015 RT nat Pr - Fara. 72-0065

20.21 Sm2+ + N20 (et?) 2.0 x 10* 0.015 RT nat Pr - Fara.72-0065

53
Table 20. Samarium(II) reactions — Continued

No. Reaction k! dm* mol-1

s_1 “ / t/°C pH Method Comments Ref.

20.22 Sm1+ + O* (af or et) 3.9 x 10“ 0.015 RT nat P

r — Fara.72-0065

(4.2 ± 0.5) x 10* 0.375 RT 3-6 P

r - Pika..73-1084 20.23 Sma+ + OH (et) 6x 10* - RT nat P

r - Fara. 72-0065

(6.2 ± 0.8) x 10* 0.375 RT 3-6 P

r - Pika..73-1084

20.24 Sma+ + Ru(NHs)8Br*+ 1.5 x 10* 0.06 RT 6 P

r - Fara.73-0107

(et) 20.25 Sma+ + Ru(NHs)sCl2+ 1.5 x 10* 0.06 RT 6 P

r - Fara.73-0107

(et) 4.3 x 10* 1.0 RT 6 P

r Fara.73-0107 (NaClCM

6.5 x 10* 1.0 RT 6 P

r - Fara.73-0107

(NaCl) 20.26 Sma+ + Ru(NH,)5HsOs+ 6.5 x 107 0.3 RT 2 P

r - Fara.73-0107

(et) 1.8 x 10* 1.0 RT 2 P

r Fara.73-0107 (NaQ04) 1.3 x 10* 1.0 RT 2 P

r - Fara.73-0107

(NaCl) 20.27 Sma+ + Ru(NH3)5I a+

ca. 10* 0.06 RT 6 Pr - Fara.73-0107

(et) 20.28 Sma+ + Ru(NHs)sOHa+ 4.0 x 107 0.06 RT 6 Pr - Fara.73-0107

(et) 2.2 x 10* 1.0 RT 6 Pr Fara.73-0107 (NaQ04) 6.0 x 10* 1.0 RT 6 Pr - Fara.73-0107

(NaCl) 20.29 Sma+ + Ru(NHa)«s+ 2.5 x 107 0.06 RT 6 Pr - Fara.73-0107

(et) 2.0 x 10* 1.0 RT 6 Pr - Fara.73-0107 (NaQ04) 8.0 x 10* 1.0 RT 6 Pr - Fara.73-0107

(NaCl) 20.30 Sma+ + Yb*+

(et) 3.0 x 10* 0.015 RT nat Pr - Fara.72-0065

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

54
Table 21. Thallium(O) and (II) reactions

No. Reaction k/dm* mol-1

s-1 * / </‘C PH Method Comments Ref.

77(0) 77J, 21.1 Tl° + HaOa - 5 x 10® - RT 0.1.5.2 7 Rate constant and Fara..71-0036

Tl+ + OH + OH" products deduced

from HaOa and Ha

yields in y-irradiated Tl1 solutions. < 107 - RT nat P

r - Fara..71-0036

21.2 Tl° + HO, - 1.3 x 1010 - RT 0.1,5.2 7 Rate constant and Fara..71-0036

Tl+ + HOj- products deduced

from HaOa and Ha

yields in y-irradiated Tl1 solutions. 21.3 Tl° + Oa - (1.0 ± 0.2) x 107 - RT nat P

r - Fara..71-0036

ti+ + or

21.4 Tl0 + Oa" -* 1.4 x 10# - RT 5.2 7 Rate constant and Fara..71-0036

Tl+ + Oa»- products deduced

from HaOa and Ha

yields in y-irradiated Tl1 solutions. 21.5 Tl0 + Tl+ ^ K = 2.3 x 10s AT 1 - RT 6.5 P

r Measured from the Cerc..66-0097

Tla

+

kt > 1010 RT 6.5 Pr effect of [Tl+

] on

the absorption due

to TV.

21.6 Tl° + Tln — (4.5 ± 1) x 10» - RT nat Pr Products deduced Fara..71-0036

T1+ + ni from HaOa and Ha

yields in y-irradiated Tl1 solutions. No account taken of

• the hydrolysis of Tl2+

(see entry 21.19). No account taken of competing reaction TV + Tln (see entry

21.12). 21.7 Tl° (?) + 1,4—benzo- 6* K o

cq - ca. 25 7.0 Pr Semiquinone product Rao.75-1032

quinone — Tl+ + (1,4—benzo- identified by its quinone)

-

77a+

absorption spectrum.

21.8 TV + HaOa — (7 ± 2) x 10« - RT nat Pr Products deduced Fara..71-0036

2T1+ + OH + OH" from HaOa and Ha

yields in y-irradiated Tl1 solutions. 21.9 Tla

+ + NaO (1.4 ± 0.2) x 107 - 25 nat Pr y-radiolysis studies SeU72-0844

(0 at or et) indicate that Na is one of the products

of this reaction. 21.10 Tla+ + Oa —

>

(1.0 ± 0.2) x 107 - RT nat Pr - Fara..71-0036

2T1+ + Oa" 1.2 x 107 - RT 0.1,5.2 7 Rate constant and Fara..71-0036

products deduced

from HaOa and Ha

yields in y-irradiated Tl1 solutions. 21.11 Tla

+ Tl° 4- Tl+

see entry 21.5

21.12 TV + Tln — (4.4 ± 0.9) x 10# -»0 RT nat Pr Products deduced Cerc..66-0097

3T1+

(4.5 ± 1) x 10# 0.0006 RT nat Pr from HaOa and Ha Fara..71-0036

yields in y-irradiated Tl1 solutions. (7.5 ± 1) x 10» 0.015 RT nat Pr No account taken of

the hydrolysis of

Tl+(see entry 21.19. 55
TABLE 21. Thallium(O) and (II) reactions — Continued

No. Reaction £/dms mol-1s

1 “ / t/°C PH Method Comments Ref.

21.13 Tla

+ + 1,4—dicyano- 2.7 x 10» _ RT P

r Organic product Robi.73-0121

benzene — 2T1+ + characterised by

( 1 ,4—dicyanobenzene) its absorption

spectrum.

Tla(Rate constants from pulse radiolysis and flash photolysis experiments only). 77J+ and TlOH+ 21.14 Tla+ + Coa+ kt = (6.2 ± 0.5) x 10s 0.75 25 0.6 f.ph. Evidence for Falc..74-7625

Tl+ + Co3+ products and equilibrium from conventional kinetic studies. 21.15 Tla+ + Cos+ -> (9.5 ± 0.5) x 10* 0.55 22 ± 2 0.3 f.ph. Evidence for Falc..75-7093

Tls+ + Coa+ products from

conventional kinetic

studies. 21.16 Tla+ + Fea+ -> (2.42 ± 0.1) x 106 0.30 14.7 0.6 f.ph. Evidence for pro- Falc..75-7093

Tl+ + Fea+

(2.50 ± 0.1) x 109 0.30 18.3 0.6 f.ph.

ducts from conventional kinetic

studies. Falc..75-7093

(2.53 ± 0.1) x 10s 0.30 20.7 0.6 f.ph. Falc..75-7093

(2.60 ± 0.1) x 109 0.30 24.8 0.6 f.ph. Falc..75-7093

(2.70 ± 0.1) x 10s 0.30 29.0 0.6 f.ph. Falc..75-7093

(2.73 ± 0.1) x 10* 0.30 33.9 0.6 f.ph. Falc..75-7093

(2.81 ± 0.1) x 10« 0.30 36.0 0.6 f.ph. Falc..75-7093

(2.91 ± 0.1) x 106 0.30 39.6 0.6 f.ph. Falc..75-7093 £a = 48 ± 2 kj mol"1 0.30 14-40 0.6 f.ph. Falc..75-7093

(6.7 ± 0.7) x 109 1 23 0 P

r Schw...74-1017

(HC10«) 21.17 Tla+ + Fes+ (1.1 ± 0.15) x 109 0.30 25 0.6 f.ph. Evidence for pro- Falc..74-7625

Tls+ + Fea+ ducts and equilibrium from conventional

kinetic studies. 21.18 Tla+ + HO, — (2.5 ± 1) x 10» - RT 1 P

r Estimated from ini- Cerc..66-0097

Tl+ + H

+ + Oa tial decay of Tln

in aerated solutions. 21.19 Tla+ + HaO pit = 4.6 ± 0.2 var 21 2-7 P

r Evidence for equili- O'Ne.75-1130

T10H+ + H

+

kf = 3.5 x 10s s -1 var 21 2-7 P

r brium from optical and

kT = (1.4 ± 0.5) x 1010 var 21 2-7 P

r conductivity measurements. 21.20 Tla+ + HaOa -> (2.8 ± 0.8) x 107 - RT 1 P

r Evidence for pro- Cerc..66-0097

Tl+ + HOa + H

+ ducts from HaOa and Ha yields in y-irradiated Tl1 solutions.

(see ref. 71-0036).

21.21 Tla+ + Mna+ — (1.9 ± 0.2) x 104 0.75 22 ± 3 0.3 f.ph. Evidence for pro- Falc..75-7093

Tl+ + Mns+ ducts from conventional kinetic studies etc. (see

ref. 75-7093). 21.22 Tln + Oa" 2 x 10l ° - RT 5.2 y Rate constant and Fara..7 1-0036

Tl1 + Oa products deduced

from HaOa and Ha

yields in y-irradiated Tl1 solutions. No account taken

of hydrolysis of Tla+ (see entry 21.19). 21.23 Tln + Tl° see entry 21.6 21.24 Tln + Tla+

see entry 21.12

56
Table 21. Thallium(O) and (II) reactions — Continued

No.

21.25

21.26

21.27

21.28

Reaction k!dm* mol 1 s

1 “ / t/° C pH Method Comments Ref.

Tl2+ + Tl2+ (dis) 2k = (3.8 ± 0.6) x 10* 1 23 0 P

r Measured from decay Schw...74-1017

(HC10«) of Tl2+ monitored

at 280 nm. Value

of €380 used to calculate rate constant

not given, but is ca. 3200 dm* mol-1 cm

-1

. 2k = (5.2 ± 0.5) x 10* 0.25 25 1 f.ph. Measured from decay Falc..74-7625 2k = (5.5 ± 0.5) x 10* 0.25 25 0.6 f.ph. of Tl2+ monitored 2k = (9.2 ± 0.9) x 10* 0.50 25 0.6 f.ph. at 270 nm. Rate 2k = (1.3 ± 0.1) x 10* 1.0 25 0.6 f.ph. constant calculated 2k = (1.2 ± 0.1) x 10* 1.0 25 0.3 f.ph. taking €370 = 5500

2k = (1.3 ± 0.1) x 10* 1.0 25 0 f.ph. dm* mol-1 cm

-1

. This E* == 7.9 ± 1.5 kj mol-1 15-45 f.ph. value was obtained by

interpolation from the measured spectrum of Tl2+ and the value of

€300 = 5400 dm* mol-1 cm

-1 measured by Cercek

et al (ref. 66-0097).

Note however that this

latter value was measured in solutions at pH ca. 6.5 and refers therefore to T10H+

(see entry 21.19). 2k/ €370 = (6.1 ± 0.6) 1 25 ± 2 0 f.ph. Measured in the pre- Burc.70-7309

x 104 cm s

1 (HC10«) sence of 5 x 10“* mol dm'

Tlm and 1 x 10-4 mol dm-

* Tl1

.

-3

2k/ €370 = (1.3 ± 0.2) 1 25 ± 2 0 f.ph. Measured in the pre- Burc.70-7309

x 10* cm s -1 (HC10«) sence of 5 x 10

-* mol dm-

* Tl111 and 5

x 10-2 mol dm-

* 2-

propanol.

T10H+ + T10H+ 2k == (4.6 ± 1.6) x 10* ca. 0 RT 6.5 pr Measured from decay Cerc..66-0097

(dis)

2k = 5 x 10* - RT > 5.5 P

r

of T10H+ monitored

at 260 nm. Rate

constant calculated taking €340 = 5400

dm* mol-1 cm

-1

. Extinction coefficient used to calculate rate constant

not given.

O'Ne.75-1130

Tl2+ + -CH20H (1.2 ± 0.3) x 104 - 23 ± 2 0.43 7 Estimated from the Burc.70-0336

(et or af) y-ray induced chain

reaction in Tln +

methanol solutions, taking *(nn + Tln

) = 5.5 x 10* dm* mol-1

s-1(see entry 21.25). Tl2+ + CHaC HOH (1.5 ± 0.4) x 104 - 23 ± 2 0.43 7 Estimated from the Burc.70-0336

(et or af) y-ray induced chain

reaction in Tln +

ethanol solutions, taking A(Tln + Tln

) = 5.5 x 10* dm* mol-1

s-1

(see entry 21.25). 57
Table 21. Thallium(O) and (II) reactions — Continued

No. Reaction k/ dm3 mol-1

s-1 a / t/° C pH Method Comments Ref.

21.29 Tl 2* + CH3 COHCH3 (9.4 ± 2.3) x 10s _ 23 ± 2 0.43 7 Estimated from the Burc.70-0336

(et or af) y-ray induced chain

reaction in Tln +

2-propanol solutions, taking A(Tln + Tln

) = 5.5 x 10* dm* mol-1

s-1(see entry 21.25). 21.30 Tla+ + anisole —

>

(5.0 ± 0.5) x 10* - 20 ± 2 4 P

r Radical cation pro- 0'Ne..75-1171

Tl+ + (anisole)+ duct characterised by its absorption and

esr spectra. 21.31 Tla+ + 1,2-dimeth- (6.0 ± 0. 6) x 10* - 20 ± 2 4 P

r Radical cation pro- 0'Ne..75-1171

oxybenzene —* Tl+ + duct characterised O'Ne..75-1086

(l,2-dimethoxybenzene)+ by its absorption and esr spectra. 21.32 T10H+ + 1,2-dimethoxy- 1.2 x 108 - RT > 4.7 P

r Radical cation pro- 0'Ne..75-1086

benzene — Tl+ + OH- + duct characterised

(l,2-dimethoxybenzene)+ by its absorption and esr spectra. 21.33 Tla+ + 1,3-dimethoxy- (8.0 ± 0. 8) x 10* - 20 ± 2 4 P

r Radical cation pro- 0'Ne..75-1171

benzene —*• Tl+ + (1,3- duct characterised dimethoxybenzene)+ by its absorption and esr spectra. 21.34 Tla+ + 1,4-dimethoxy- (6.5 ± 0.7) x 10* - 20 ± 2 4 P

r Radical cation pro- 0'Ne..75-1086

benzene —* Tl+ + duct characterised 0'Ne..75-1171

( 1 ,4-dimethoxybenzene)+ by its absorption and esr spectra. 21.35 T10H+ + 1,4—dimethoxy- 4.5 x 10* - RT > 4.7 P

r Radical cation pro- O'Ne..75-1086

benzene —*• Tl+ + OH- + duct characterised

( 1 ,4—dimethoxybenzene)+ by its absorption and esr spectra. 21.36 T10H+ + menaquinone slow - RT 6.8 P

r - Rao.73-1047

21.37 Tla+ + 1,2,3-trimethoxy- (3.2 ± 0.3) x 10* - 20 ± 2 4 P

r Radical cation pro- 0'Ne..75-1171

benzene —* Tl+ + (1,2,3- duct characterised trimethoxybenzene)+ by its absorption and

esr spectra. 21.38 Tla+ + 1,2,4—trimeth- (6.8 ± 0.7) x 10* - 20 ± 2 4 P

r Radical cation pro- 0'Ne..75-1171

oxybenzene —*• Tl+ + duct characterised (1,2,4—trimethoxybenzene)+ by its absorption and esr spectra. 21.39 Tla+ + 1,3,5-trimeth- (7.0 ± 0.7) x 10* - 20 ± 2 4 P

r Radical cation pro- 0'Ne..75-1171

oxybenzene —

Tl+ + duct characterised

( 1 ,3,5-trimethoxybenzene)+ by its absorption and esr spectra.

58
TABLE 21. Thallium(O) and (II) reactions — Continued

No. Reaction A/dm* mol 1 s

1 “ / </°C PH Method Comments Ref.

77n chloro-complexes 21.40 Tl*+ + cr T1C1+ K = (6.2 ± 0.7) 1 23 0 P

r Measured from ef- Dods.74—1038

x 104 dm* mol-1 (HC10«) feet of [Cl-

] on absorption spectrum

of Tln. A, = 9 x 10* 1 23 0 P

r Measured from rate Dods.74—1038

(HQO«) of attainment of

equilibrium. Ar = 1.4 x 10* s -1

1 (HC10«)

23 0 Pr

21.41 Tier + cr — K = (1.9 ± 0.4) 1 23 0 Pr Measured from ef- Dods.74-1038

TlCla x 10* dm* mol-1 (HC104) feet of [Cl-

] on

absorption spectrum

of Tln. 21.42 Ticia + cr K = 13 ± 3 dm* 1 23 0 Pr Measured from ef- Dods.74-1038

T1CU

- mol-1 (HCIO4) feet of [Cl -

] on

absorption spectrum

of Tln. 21.43 Tln + Tln

(dis) 2k = 5.38 x 10® 1 23 0 Pr [Cl-

] = 1 x 10

-* mol dm-* Dods.74-1038

2k = 5.58 x 10® 1 23 0 Pr [CT] = 9.7 x 10

-* mol dm-* Dods.74-1038

2k = 4.74 x 10® 1 23 0 Pr [Cl-

] = 0.1 mol

dm-® Dods.74-1038

2k = 3.70 x 10® 1 23 0 Pr [Cl -

] = 0.98 mol

dm-3 Dods.74-1038

Plus data at intermediate chloride concentrations.

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2A).

Table 22. Thulium(II) reactions

No. Reaction A/dm* mol 1 s

1 a / t/°C PH Method Comments Ref.

Tm\X

22.1 Tm*+ + OH (et) (7 ± 1) x 10® - RT 3-6 pr - Pika. .73-10

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

59
Table 23. Ytterbium(II) reactions

No. Reaction A/dm* mol-1

s

1 * / f/°C pH Method Comments Ref.

yjj, (Rate constants from pulse radiolysis studies only). 23.1 Yba+ + BrO,~ < 10* 0.015 RT nat P

r - Fara.72-0065

23.2 Yb,+ + Co(en)3s+ < 5 x 10* 0.06-1.0 RT 6 P

r - Fara.73-0107

23.3 Yba+ + Co(NH,)5Bra+ (et) 3.0 x 10* 0.06 RT 6 P

r - Fara.73-0107

1.4 x 107 1.0 RT 6 P

r - Fara.73-0107 (NaCICM

2.5 x 107 1.0 RT 6 P

r - Fara.73-0107

(NaCl) 23.4 Yba+ + Co(NH3)5a2+

(et) 4.3 x 10* 0.06 RT 6 P

r - Fara.73-0107

1.9 x 107 1.0 RT 6 Pr - Fara.73-0107 (NaQ04) 2.3 x 107 1.0 RT 6 P

r - Fara.73-0107

(NaCl) 23.5 Yba+ + Co(NHs)5CNa+ (et) 3.0 x 10* 0.06 RT 6 P

r - Fara.73-0107

23.6 Yba+ + Co(NH,)5 P+(et) 1.1 x 107 0.06 RT 6 P

r - Fara.73-0107

6.0 x 107 1.0 RT 6 Pr - Fara.73-0107 (NaQ04) 1.0 x 10* 1.0 RT 6 P

r - Fara.73-0107

(NaCl) 23.7 Yba+ + Co(NHs)5HaOa+ 2.2 x 10* 0.3 RT 2 Pr - Fara.73-0107

(et) 6.4 x 10* 1.0 RT 2 Pr - Fara.73-0107 (NaQ04) 23.8 Yba+ + Co(NH,)5N,a+ (et) 1.6 x 107 0.06 RT 6 Pr - Fara.73-0107

2.6 x 107 0.5 RT 6 Pr - Fara.73-0107 (NaC104) 23.9 Yba+ + Co(NH3)5NCSa+ < 5.0 x 10* 0.5 RT 6 Pr - Fara.73-0107 (NaC104) 23.10 Yba+ + Co(NHs)«s+ < 5.0 x 10* 0.06 RT 6 Pr - Fara.73-0107

23.11 Yba+ + Co(NHs)50Ha+ (et) 7.7 x 10* 0.3 RT 5.5. Pr - Fara.73-0107

1.9 x 107 1.0 RT 5.5 Pr - Fara.73-0107 (NaC104) 2.9 x 107 1.0 RT 5.5 Pr - Fara.73-0107

(NaCl) 23.12 Yba+ + Cua+ (et) 1.2 x 107 0.015 RT nat Pr - Fara.72-0065

23.13 Yba+ + HaOa (et) 9.1 x 10* 0.015 RT nat Pr - Fara.72-0065

23.14 Yba+ + IOj- (et) 2.1 x 10* 0.015 RT nat Pr - Fara.72-0065

23.15 Yba+ + MnOr (et) 8.3 x 107 0.015 RT nat Pr - Fara.72-0065

23.16 Yba+ + NOa“ (et) 4.7 x 107 0.015 RT nat Pr - Fara.72-0065

23.17 Yba+ + NO," (et) 3.6 x 10* 0.015 RT nat Pr - Fara.72-0065

23.18 Yba+ + NaO (et?) ca. 10* 0.015 RT nat Pr - Fara.72-0065

23.19 Yba+ 4- 0, (et or af) (6.3 ± 1) x 107 0.375 RT 2 Pr - Pika..73-1084

6.5 x 107 0.015 RT nat Pr - Fara.72-0065

23.20 Yba+ + OH (et) 3 x 10* 0.015 RT nat Pr - Fara.72-0065

(3.2 ± 0.3) x 10* 0.375 RT 2 Pr - Pika..73-1084

23.21 Yba+ + Ru(NH,)5Bra+ 3.3 x 107 0.06 RT 6 Pr - Fara 73-0107

(et) 23.22 Yba+ + Ru(NH,)5Cl2+

(et) 1.5 x 107 0.06 RT 6 Pr - Fara.73-0107

1.8 x 10* 1.0 RT 6 Pr - Fara.73-0107 (NaC104) 2.8 x 10* 1.0 RT 6 Pr - Fara.73-0107

(NaCl)

60
Table 23. Ytterbium(II) reactions — Continued

No. Reaction A/dm3 mol-1s

1 • / t/°C pH Method Comments Ref.

23.23 Yb*+ + Ru(NHj)8HjOs+ 1.0 x 107 0.3 RT 2 P

r - Fara.73-0107

(et) 2.9 x 107 1.0 RT 2 P

r - Fara.73-0107 (NaC104) 3.2 x 10" 1.0 RT 2 P

r - Fara.73-0107

(NaCl) 23.24 Yba+ + Ru(NH,)5Ia+ (et) ca. 108 0.06 RT 6 P

r - Fara.73-0107

23.25 Yb3+ + Ru(NHs)«s+ (et) 5.0 x 10* 0.06 RT 6 Pr - Fara.73-0107

4.5 x 107 1.0 RT 6 Pr - Fara.73-0107

(NaC10«)

3.0 x 10* 1.0 RT 6 Pr - Fara.73-0107

(NaCl) 23.26 Yba+ + Ru(NH,)5OHa+ 1.3 x 107 0.06 RT 6 Pr - Fara.73-0107

(et) 2.3 x 107 0.3 RT 6 Pr - Fara.73-0107

5.0 x 107 1.0 RT 6 Pr - Fara.73-0107 (NaQO«)

1.4 x 10* 1.0 RT 6 Pr - Fara.73-0107 (NaQ)

•If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2 k).

61
TABLE 24. Zinc(I) reactions

No. Reaction A/dm* mol 1 s-1 * / t/° C PH Method Comments Ref.

24.1 Zn\Q Zn+ + BrOs

-

(et) (2.1 ± 0.3) x 10* 0.08 RT nat Pr Meye.68-0855

24.2 Zn+ + Cda+ (et?) < 1 x 107 0.08 RT nat P

r The reason for the Meye.68-0855

24.3 Zn+

-I" ClOa

8.3 x 10s

< 3 x 10* 0.08

RT

RT

nat

nat

P

r

P

r

discrepancy between

these two values is not clear.

Baxe. .66-0848

Meye.68-0855

24.4 Zn+ + Coa+ < 3 x 10* 0.08 RT nat P

r - Meye.68-0855

24.5 Zn+ + Co(bpy)ss+ (et) 2.6 x 10* - RT nat pr - Baxe. .72-0381

24.6 Zn+ + Co(en)sa+ (et) (2.5 ± 0.4) x 10* 0.08 RT 5-6 Pr - Meye.69-0428

24.7 Zn+ + cw-Co(en)aQ2+ (1.91 ± 0.3) x 10® 0.08 RT 5-6 Pr - Meye.69-0428

24.8

(et) Zn+ + trans- (2.3 ± 0.3) x 10® 0.08 RT 5-6 Pr Meye.69-0428

24.9

Co(en)2Cl2+

(et) Zn+ + Co(en)jCOs+

(4.7 ± 0.7) x 10* 0.08 RT 5-6 Pr Meye.69-0428

24.10

(et) Zn+ + cis-Co(en)aFj+

(5.4 ± 0.8) x 10* 0.08 RT 5-6 Pr Meye.69-0428

24.11

(et) Zn+ + Co(en)aFHjOa+ (4.7 ± 0.7) x 10* 0.08 RT 5-6 Pr Meye.69-0428

24.12

(et) Zn+ + cw-Co(en)aNHjCla+ (1.47 ± 0.2) x 10* 0.08 RT 5-6 Pr Meye.69-0428

24.13

(et) Zn+ + cis- (2.7 ± 0.7) x 10* 0.08 RT 5-6 Pr Meye.69-0428

24.14

Co(en)aNHsNOaa+ (et) Zn+ + Co(NH3)«s+ (8.4 ± 1.3) x 10* 0.08 RT 5-6 Pr Meye.69-0248

24.15

(et) Zn+ + Co(NHs)5Bra+ (2.6 ± 0.4) x 10* 0.08 RT 4.0 Pr Meye.69-0428

24.16

(et) Zn+ + Co(NHa)5aa+ (2.2 ± 0.3) x 10® 0.08 RT 5-6 Pr Meye.69-0428

24.17

(et) Zn+

-I- Co(NHs)5CNa+ (1.30 ± 0.2) x 10® 0.08 RT 5-6 Pr Meye.69-0428

24.18

(et) Zn+ + Co(NHs)sP+

(8.2 ± 1.2) x 10* 0.08 RT 5-6 Pr Meye.69-0428

24.19

(et) Zn+ + Co(NH3)5fumar- (1.2 ± 0.3) x 10® 0.08 RT 5-6 Pr Meye.69-0428

24.20

ate+(et) Zn+ + Co(NHs)5HaOs+ (1.56 ± 0.2) x 10® 0.08 RT 4.0 Pr Meye.69-0428

24.21

(et) Zn+ + Co(NH3)5OHa+ (1.10 ± 0.2) x 10® 0.08 RT 6.6 Pr Meye.69-0428

24.22

(et) Zn+ + Co(NH3)5N3a+ (1.49 ± 0.2) x 10® 0.08 RT 5-6 Pr Meye.69-0428

24.23

(et) Zn+ + Co(NH3)sNCSa+ (1.65 ± 0.2) x 10® 0.08 RT 5-6 Pr Meye.69-0428

24.24

(et) Zn+ + Co(NH3)B00CCH3a+ (5.0 ± 0.8) x 10* 0.08 RT 5-6 Pr Meye.69-0428

24.25

(et) Zn+ + Crs+ < 107 RT nat Pr Baxe..66-0848

24.26 Zn+ + CraCV

-

(et) (1.6 ± 0.2) x 1010 0.020* 25±2 nat Pr - Buxt..76-1072

24.27 Zn+ + Cua+ (et) (2.5 ± 0.4) x 10* 0.08 RT nat Pr - Meye.68-0855

24.28 Zn+ + HaOa —

(9.5 ± 2.0) x 10®

(1.80 ± 0.3) x 10®

0.4(ZnSO«)

RT

RT

5-8

nat

y

Pr

Measured by competition with NOs

-

. Rate constant cal- culated taking

k(Zn+ + NOD = 2.1 x 10* dm* mol-1

s_I

(see entry 24.33).

Fiti70-0117

Meye.68-0855 Zna+ + OH + OH" (2.3 ± 0.2) x 10® - 25±2 nat Pr Products inferred Buxt.76-1072

E, = 10.5 ± 1.0 nat Pr

from y-radiolysis

experiments (see

ref. 73-0039). Buxt..76-1072

kj mol 1

62
Table 24. Zinc(I) reactions — Continued

No. Reaction A/dm* mol-1

s-1 * / f/°C pH Method Comments Ref.

24.29 Zn+ + H,0+ < 10« 0.08 RT _

P

r _ Meye.68-0855

24.30 Zn+ + IOr (et) (3.6 ± 0.5) x 10* 0.08 RT nat P

r - Meye.68-0855

(1.7 ± 0.3) x IO10 0.4 RT 5-8 y Measured by com- Fiti70-0117

(ZnS04) petition with NOs

-

. Rate constant cal- culated taking

A(Zn+ + NOs

-

) =

2.1 x 10* dm* mol-1

s-1(see entry 24.33). 24.31 Zn+ + Nia+ (et) < 5x 10* 0.08 RT nat P

r - Meye.68-0855

5 x 107 - RT nat P

r - Baxe. .66-0848

24.32 Zn+ + NOr (et) (2.2 ± 0.3) x 10* 0.08 RT nat P

r - Meye.68-0855

24.33 Zn+ + NO," (et) (2.1 ± 0.3) x 10* 0.08 RT nat Pr - Meye.68-0855

24.34 Zn+ + NaO -> < 1.3 x 107 - RT nat P

r - Meye.68-0855

ZnO+ + Na (3.7 ± 0.4) x 107 - 25±2 nat P

r Products charac- Buxt..76-1072 Ea = 35.5 ± 1.4 kj - 1-30 nat P

r terised by their mol-1 absorption spectrum

(see ref. 76-1072)

and in y-radiolysis

experiments (see

ref. 73-0039). 24.35 Zn+

-f- Oa — (2.4 ± 0.4) x 10* - RT nat Pr - Meye.68-0855 Zna+ + Oa~ 3.3 x 10* - RT nat Pr - Baxe. .66-0848

Products characterised by their absorption spectrum

(see ref. 76-1072)

and reactivity with 1,4-benzoquinone (see

ref. 76-1134). 24.36 Zn+ + OH (et) 5.7 x 10* - RT nat Pr No correction made Baxe. .66-0848

for competing reaction Zn+ + Zn+

. ca. 8 x 10* 25±2 nat Pr Estimated from

decay of Zn+in the absence of OH

scavengers taking

into account competing reactions such

as Zn+ + Zn+

, Zn+ +

HsOa, OH + OH etc.

Buxt.75-1027

24.37 Zn+ + Pba+ (et) 4.0 x 10* - RT nat Pr - Baxe. .66-0848

24.38 Zn+ + Ru(bpy)ss+ (et) 2.5 x 10* - RT nat Pr - Baxe.72-0381

24.39 Zn+ + Ru(NHs)«*+

(et) (2.2 ± 0.3) x 10* 0.08 RT nat Pr - Navo.70-1229

24.40 Zn+

-f SaOg2 — (1.3 ± 0.1) x 10® 0.02* 25±2 nat Pr - BuxL.76-1072 Zna+ + SOr + SO«a- 24.41 Zn+ + Zn+ 2k < 8 x 10* 0.4 25±2 nat Pr Estimated from rate of decay of Zn+

in the presence of 2-

methyl-2-propanol.

Major competing reaction is Zn+ +

•CHaC(CH,)aOH.

Buxt.75-1027

24.42 Zn+ + allyl alcohol —> ca. 10® - 25 ±2 nat Pr Product characterized BuxL.76-1072

(Zn - aUyl alcohol)+ by its absorption spectrum.

63
TABLE 24. Zinc(I) reactions — Continued

No. Reaction k/ dm3 mol-1

s-1 * I t/°C pH Method Comments Ref.

24.43 Zn+ + benzophonone — 2.5 x 10® Zna+ + (benzophenone)

-

24.44 Zn+ + 1,4—benzo- (3.0 ± 0.6) 10® quinone — Zna+ +

( 1 ,4-benzoquinone)

“

4.8 x 10®

24.45 Zn+ + menaquinone — (3.8 ± 0.4) x 10® Zn*+ + (menaquinone)

-

Znl Complexes

RT 7.0

25±2 5.7

RT 7.0

RT 7.1

pr Measured in the presence of ca.

1 mol dm-3 2-

methyl-2-propanol.

Ketyl radical product characterised by its absorption

spectrum. pr Measured in the presence of 1 mol

dm-3 2-methyl-2-

propanol. Semiquinone product

characterised by

its absorption

spectrum. pr Measured in the presence of ca.

1 mol dm-3 2-

methyl-2-propanol.

pr Measured in the presence of ca.

1 mol dm-3 2-methyl2-propanol. Semiquinone product

characterised by

its absorption

spectrum.

ZnL+ (from ZnLa+ + CHjCO'CHj), L = hematoporphyrin (ix) (no reference made to number of protons involved with complex).

24.46 ZnL+ + ZnL+ - 'k' = (2.1 ± 0.4) x 103 0.1 RT

(ZnIV+

24.47 (ZnL)»2+ -> P 17 ± 2 s"1 0.1 RT

P — dihydroporphyrin

product < 0.14 s"1 0.1 RT

13 Pr

13

13

P

r

P

r

Unclear whether k

or 2k. Measured

in the presence of

1 mol dm-3 2-propanol. Dimerisation mechanism implied from subsequent

reactions (see entry 24.47) and

comparison with the products of reduction

of ZnLa+ in aprotic

solvents. Reaction suggested

to involve internal rearrangement. Reaction presumed

to involve splitting of dimer.

Rao.75-1032

SeU.76-1134

Rao.75-1032

Rao.73-1047,

Rao.75-1032

Hare. 74—1040

Hare.74—1040

Hare.74—1040

“If the data source gives no errors none are shown here but they should be assumed to be at least ±25% (or ±50% for 2k).

64
Table 25. Intramolecular electron transfer reactions for some metal complexes'

No. Reaction k! s“ l

b

/ t/°C pH Method Comments Ref.

25.1

Electron adducts (NH3)B CoIIV-00CC,H«N0a)- - 2.6 x 103 RT 7.0 P

r Simi..77-1027

25.2 (NH3)«CoI1(p-OOCC.H«NOa) (NH3)BCom(m-00CC«H4N0a)- - 1.5 x 102 . RT 7.0 P

r . Simi..77-1027

25.3 (NHa)BCoI1(m-OOCCBH«NOa) (NH3)BCoIII(o-OOCCeH«NOa)- — 4.0 x 101 RT 7.0 P

r Simi..77-1027

25.4 (NHs)BCoII(o-00CC6H«N0a) (NHs)BCoin(o-OOCCBH«N02H) - 9.5 x 103 RT 0.8 P

r Simi..77-1027

25.5 (NHs)BCoI1(o-OOCCBH«NOa) + H

+ (NHa)BCoin[2,4-OOCC«H«(NOa)a] - 3.5 x 104 RT 7.0 P

r Simi..77-1027

25.6

(NH3)BCon[2,4-00CC6H4(N0a)a] (NH3)BCom[3,5-OOCCBH«(NOa)a]- 1.3 x 102 RT 7.0 P

r Simi..77-1027

25.7 — (NHs)BCon[3,5-OOCC*H«(NOa)2] Cun(gluthathione_

) — (3.6 ± 0.3) RT 11 P

r Rate constant Fara.76-1016

25.8

Cu’(gluthathione)

Cu^lyjafgly

-

) —

x 103

(1.7 ± 0.3) RT 9 P

r

independent of [Cu11]: [glutathione] ratio in range 1:2 to 1:5 and of [Cu11] in the range

(1-10) x 10-4 mol

dm-3. Rate constant Fara.76-1016 CuI(gly)3 x 104 independent of

Hydroxyl radical adducts 25.9 (NH,)5Com00CC«H50H —

(NH,)8Con00CC,H«0H + H

+ Hydrogen atom adducts 25.10 (NHs)5Com00CC«H5H

(NH3)5ConOOCC«H«H + H

+

[Cu11

]: [gly] ratio in range

1:6 to 1:15 and

of [Cu11] in the range (1-10) x 10-4 mol dm-3

.

< 102

< 102

RT

RT

6.0 Pr

P

r

Cohe.71-0282

Cohe.71-0282

•Intramolecular electron transfer reactions of metallo-proteins and related systems not included..

bN.B. First order rate constants.

65
References

62-0164

64-

0133

65-

0385

65-0393

65-0394

65-

0799

66-

0097

66-

0848

67-

0019

67-

0062

68-

0066

68-0169

68-0302

68-0431

68-0435

68-

0855

69-

0144

69-0428

69-0434

69-0971

Haissinsky, M., Radiolysis of compounds of the noble metals in aqueous solution. I. Action of gamma rays on the chlorides of

Pt11 and PtTM in acid solution, RADIATION RES. 17(3): 274—85

(1962). Asmus, K.-D.; Henglein, A.; Ebert, M.; Keene, J.P., Pulsradiolytische Untersuchung schneller Reaktionen von

hydratisierten Elektronen, freien Radikalen und Ionen mit Tetranitromethan in waessriger Loesung, BER. BUNSENGES.

PHYS. CHEM. 68: 657-63 (1964). Baxendale, J.H.; Keene, J.P.; Stott, D.A., Determination of some fast reaction rates using the pulsed radiolysis of permanganate solutions. Pulse Radiolysis, Ebert, M.; Keene,

J.P.; Swallow, AJ.; Baxendale, J.H. (eds.), Acad. Press, N.Y., 1965, p. 107-15.

Baxendale, J.H.; Fielden, E.M.; Keene, J.P., Pulse radiolysis of Ag+

solutions. Ibid., p. 207-16.

Baxendale, J.H.; Fielden, E.M.; Keene, J.P., Formation of Cum

in the radiolysis of Cu2+ solutions. Ibid., p. 217-20.

Gordon, S., Ibid., p

285.

Cercek, B.; Ebert, M.; Swallow, AJ., Novel valence states of thallium as studied by pulse radiolysis, J. CHEM. SOC. PT. A

(5): 612-5 (1966). Baxendale, J.H.; Keene, J.P.; Stott, D.A., Reactions and relative potentials of some metal ions in unstable valence states, CHEM.

COMMUN. 715-16 (1966). Konstantatos, J.; Katakis, D., The radiolysis of concentrated

neutral sodium perchlorate aqueous solutions, J. PHYS. CHEM.

71(4): 979-83 (1967). Buxton, G.V.; Dainton, F.S.; Thielens, G., Kinetics of reactions of the hydrated electron, CHEM. COMMUN (4): 201 (1967). Dainton, F.S.; Wiseall, B., Reactions of nitrosodimethylaniline with free radicals, TRANS. FARADAY SOC. 64(3): 694—705

(1968). Adams, G.E.; Broszkiewicz, R.B.; Michael, B.D., Pulse

radiolysis studies on stable and transient complexes of platinum, TRANS. FARADAY SOC. 64(5): 1256-64 (1968). Ghosh-Mazumdar, A.S.; Hart, EJ., A pulse radiolysis study of

bivalent and zerovalent gold in aqueous solutions, ADVAN.

CHEM. SER. 81: 193-209 (1968). Pukies, J.; Roebke, W.; Henglein, A., Pulsradioytische Unter- suchung einiger Elementarprozesse der Silberreduktion, BER. BUNSENGES. PHYS. CHEM. 72(7): 842-7 (1968). Pukies, J.; Roebke, W., Pulsradioytische Untersuchung der Reduktion des Ag+-Ions in ammoniakalischer Loesung, BER. BUNSENGES. PHYS. CHEM. 72(9/10): 1101-5 (1968). Meyerstein, D.; Mulac, W.A., Reductions by monovalent zinc, cadmium, and nickel cations, J. PHYS. CHEM. 72(3): 784—8

(1968). Ghosh-Mazumdar, A.S.; Hart, EJ., Electron pulse radiolysis of aqueous tetrachloro and tetracyano complexes of Pt11

, INT. J. RADIAT. PHYS. CHEM. 1: 165-76 (1969). Meyerstein, D.; Mulac, W.A., Reduction of cobalt(III) complexes

by monovalent zinc, cadmium, and nickel ions in aqueous

solutions, J. PHYS. CHEM. 73(4): 1091-5 (1969). Jayson, G.G.; Keene, J.P.; Stirling, D.A.; Swallow, AJ., Pulseradiolysis study of some unstable complexes of iron, TRANS.

FARADAY SOC. 65(561): 2453-64 (1969).

Taylor, R.S.; Sykes, A.G., Preparation, spectrum, and stability of indium(I) in aqueous solution, J. CHEM. SOC. PT. A 2419-

23 (1969).

70-0117 Fiti, M., La cinetique de competition dans 1' etude des

intermediaires instables. I. Les ions Co+

, Mn+, Zn+, Cd+

et Ni+

, REV. ROUM. CHIM. 15(1): 77-85 (1970). 70-0178 Baxendale, J.H.; Rodgers, M.AJ.; Ward, M.D., Radiolysis of aqueous solutions of ruthenium (III) hexa-ammine and

chloropenta-ammine, J. CHEM. SOC. PT. A (8): 1246-50

(1970). 70-0336 Burchill, C.E.; Hickling, G.G., Radiation-induced oxidation of

alcohols by Tl(IH) in acid aqueous solution, CAN. J. CHEM.

48(16): 2466-73 (1970). 70-0512 Barker, G.C.; Fowles, P., Pulse radiolytic induced transient

electrical conductance in liquid solutions. Part 3. Radiolysis of aqueous solutions of some inorganic systems, TRANS.

FARADAY SOC. 66(7): 1661-9 (1970). 70-0580 Baxendale, J.H.; Koulkes-Pujo, A.-M., Une etude par radiolyse

pulse sur l'espece transitoire Au II, J. CHIM. PHYS. 67(9): 1602-7 (1970). 70-1228 Meyerstein, D.; Mulac, W.A., The effect of ligands on the chemical properties of monovalent cadmium ions, INORG.

CHEM. 9(7): 1762-6 (1970). 70-1229 Navon, G.; Meyerstein, D., The reduction of ruthenium(III)

hexaammine by hydrogen atoms and monovalent zinc, cadmium, and nickel ions in aqueous solutions, J. PHYS.

CHEM. 74(23): 4067-70 (1970). 70-7309 Burchill, C.E.; Wolodarsky, W.H., The photo-chemistry of aqueous solutions of Tl(III) perchlorate, CAN. J. CHEM.

48(19): 2955-9 (1970).

70-

7726 Thornton, A.T.; Laurence, G.S., The rates of oxidation of Fe2+

, Mn2+

, and Co+ by Bra

-

radical ions, CHEM. COMMUN. 443—4

(1970).

71-

0036 Faraggi, M.; Zehavi, D.; Anbar, M., Effect of thallous ions on

the yields of hydrogen and hydrogen peroxide in radiolyzed aqueous solutions, TRANS. FARADAY SOC. 67: 2057—

(1971). 71-0097 Venerable, G.D.II; Halpern, J., Pulse radiolysis of aqueous

solutions of pentacyanocobaltate(II). The detection and

characterization of pentacyanocobaltate(I), J. AMER. CHEM.

SOC. 93(9): 2176-9 (1971). 71-0174 Meyerstein, D., Trivalent copper. I. A pulse radiolytic study of

the chemical properties of the aquo complex, INORG. CHEM.

10(3): 638-41 (1971). 71-0234 Baxendale, J.H.; Mulazzani, Q.G., A study of the oxidation and

reduction of Ru(NHs)sNa2+ by y- and electron pulse radiolysis,

J. INORG. NUCL. CHEM. 33(3): 823-30 (1971). 71-0282 Cohen, H.; Meyerstein, D., Oxidation of benzoatopentaamminecobalt(III) by hydroxyl radicals, J. AMER. CHEM. SOC. 93(17): 4179-83 (1971)

71-

0775 Meyerstein, D., Trivalent copper. II. A pulse radiolytic study of

the formation and decomposition of amino complexes, INORG.

CHEM. 10(10): 2244-0 (1971).

72-

0065 Faraggi, M.; Tendler, Y., Pulse radiolysis in lanthanide aqueous

solutions. I. Formation spectrum and chemical properties of

divalent europium, ytterbium, and samarium ions, J. CHEM.

PHYS. 56(7): 3287-93 (1972). 72-0066 Faraggi, M.; Feder, A., Pulse radiolysis studies in lanthanide aqueous solutions. II. Formation, spectrum and some chemical

properties of praseodymium(IV) in aqueous solution. J. CHEM.

PHYS. 56(7): 3294-7 (1972). 72-0290 Faraggi, M.; Amozig, A., Pulse radiolysis of metallic ions in aqueous solutions. I. Pulse radiolysis in Hg2+ and Hgj2+ ions in

66
aqueous solutions, INT. J. RADIAT. PHYS. CHEM. 4(3): 353-

8 (1972). 72-0381 Baxendale, J.H.; Fiti, M., Transient species in the reactions of some pyridyl complex ions with hydrated electrons, J. CHEM.

SOC. DALTON TRANS. (18): 1995-8 (1972). 72-0460 Lati, J.; Meyerstein, D., Trivalent nickel. I. A pulse radiolytic

study of the formation and decomposition of the ammoniacal

complex in aqueous solution, INORG. CHEM. 11(10): 2393-7

(1972). 72-0461 Lati, J.; Meyerstein, D., Trivalent nickel. II. A pulse radiolytic

study of the formation and decomposition of the ethylenediamine and glycine complexes in aqueous solution, INORG. CHEM. 11(10): 2397-401 (1972). 72-0844 Sellers, R.M., Ph.D. Thesis, Univ. of Leeds, 1972.

72-

7088 Wright, R.C.; Laurence, G.S., Production of platinum(III) by

flash photolysis of PtCl«2-

, J. CHEM. SOC., CHEM. COMMUN.

(3): 132-3 (1972)

73-

0038 Jayson, G.G.; Parsons, B.J.; Swallow, A.J., Oxidation of ferrous

ions by perhydroxyl radicals, J. CHEM. SOC, FARADAY

TRANS. 1 69(1): 236-42 (1973). 73-0039 Buxton, G.V.; Dainton, F.; McCracken, D.R., Radiation chemical study of the reaction of Ni+

, Co+ and Cd+ with NaO. Evidence of the formation of a hyperoxidised state by oxygen atom transfer, J. CHEM. SOC, FARADAY TRANS. 1 69(1): 243-54 (1973). 73-0043 Nazhat, N.B.; Asmus, K.-D., Reduction of mercuric chloride by

hydrated electrons and reducing radicals in aqueous solutions. Formation and reactions of HgCl, J. PHYS. CHEM. 77(5): 614—

20 (1973). 73-0107 Faraggi, M.; Feder, A., Electron-transfer reactions of cobalt(III) and ruthenium(III) ammines with europium(II), ytterbium(II), and samarium(II) in aqueous solutions, INORG. CHEM. 12(1): 236-41 (1973). 73-0121 Robinson, E.A.; Schulte-Frohlinde, D., Pulse radiolysis of 1,4—

dicyanobenzene in aqueous solutions in the presence and

absence of thallium(I) ions, J. CHEM. SOC. FARADAY

TRANS. 1 69(4): 707-18 (1973). 73-0122 Jayson, G.G.; Parsons, B.J.; Swallow, A.J., Appearance of

sulphatoferric complexes in the oxidation of ferrous sulphate

solutions. A study by pulse radiolysis, J. CHEM. SOC. FARADAY TRANS. 1 69(6): 1079-89 (1973). 73-1047 Rao, P.S.; Hayon, E., One-electron redox reactions of free

radicals in solution. Rate of electron transfer processes of quinones, BIOCHIM. BIOPHYS. ACTA 292: 516-33 (1973). 73-1053 Farhataziz; Mihalcea, I.; Sharp, L.J.; Hentz, R.R. Pulse

radiolysis of liquids at high pressures. IV. Hydrogen-atom

reactions in aqueous 0.1M HC10« solutions, J. CHEM. PHYS.

59(5): 2309-15 (1973). 73-1057 Ellis, J.D.; Green, M.; Sykes, A.G.; Buxton, G.V.; Sellers, R.M.,

Pulse radiolysis of titanium(III) and other metal(III) ions in the presence of formic acid, J. CHEM. SOC., DALTON TRANS.

(16): 1724-8 (1973). 73-1066 Broszkiewicz, R.K., Pulse radiolysis studies on complexes of

iridium, J. CHEM. SOC, DALTON TRANS. (17): 1799-802

(1973). 73-1080 Fujita, S.; Horii, H.; Taniguchi, S., Pulse radiolysis of mercuric

ion in aqueous solutions, J. PHYS. CHEM. 77(24): 2868-71

(1973). 73-1084 Pikaev, A.K.; Sibirskaya, G.K.; Spitsyn, V.I., Study of divalent samarium, europium, thulium, ytterbium, and of tetravelent praseodymium ions by pulse radiolysis in aqueous solution, DOKL. PHYS. CHEM. (ENGL. TRANSL.) 209(4-6): 339-42

(1973), Transl. from DOKL. AKAD. NAUK SSSR 209(5): 1154-7 (1973). 73-

1104 Rao, P.S.; Hayon, E., Rate constants of electron transfer processes in solution: Dependence on the redox potential of the

acceptor, NATURE(LONDON) 243: 344-6 (1973).

74—

1017 Schwarz, H.A.; Comstock, D.; Yandell, J.K.; Dodson, R.W., A

pulse radiolysis study of thallium(II) in aqueous perchloric acid

solutions, J. PHYS. CHEM. 78(5): 488-93 (1974). 74—1037 Kelm, M.; Lilie, J.; Henglein, A.; Janata, E., Pulse radiolytic study of Ni+

. Nickel-carbon bond formation, J. PHYS. CHEM.

78(9): 882-7 (1974). 74—1038 Dodson, R.W.; Schwarz, H.A., Pulse radiolysis studies of

chloride complexes of thallium(II). Absorption spectra and

stability constants of T1C1+

, T1CL, and T1C13, J. PHYS. CHEM.

78(9): 892-9 (1974). 74—1040 Harel, Y.; Meyerstein, D., On the mechanism of reduction of porphyrins. A pulse radiolytic study, J. AMER. CHEM. SOC.

96(9): 2720-7 (1974). 74—1072 Mulazzani, Q.G.; Ward, M.D.; Semerano, G.; Emmi, S.S.; Giordani, P., Gamma and pulse radiolysis of

tetracyanonickelate(II) anion in aqueous solution, INT. J. RADIAT. PHYS. CHEM. 6(3): 187-201 (1974). 74—1104 Laurence, G.S.; Thornton, A.T., Kinetics of oxidation of transition-metal ions by halogen radical anions. ?art. IV. The

oxidation of vanadium(II) and chromium(II) by diiodide, dibromide, and dichloride ions generated by pulse radiolysis, J. CHEM. SOC., DALTON TRANS. (11): 1142-8 (1974). 74—1142 Cohen, H.; Meyerstein, D., Ultraviolet-visible spectrum, and

kinetics of formation and decomposition, of pentaaquahydridochromium(III) and chromium(II) in aqueous

perchlorate solutions: A pulse-radiolysis study, J. CHEM. SOC.,

DALTON TRANS. (23): 2559-64 (1974). 74—1146 Cohen, H.; Meyerstein, D., Chromium-carbon bonds in aqueous

solutions. A pulse radiolytic study, INORG. CHEM. 13(10): 2434-43 (1974).

74—

7265 Falcinella, B.; Felgate, P.D.; Laurence, G.S., Aqueous chemistry

of thallium(II). Part I. Kinetics of reaction of thallium(II) with

cobalt(II) and iron(II) ions and oxidation-reduction potentials of

thallium(II), J. CHEM. SOC., DALTON TRANS. 1367-73

(1974).

75-

1027 Buxton, G.V.; Sellers, R.M., Pulse radiolysis study of monovalent cadmium, cobalt, nickel and zinc in aqueous

solution. Pt. 1. Formation and decay of the monovalent ions, J. CHEM. SOC., FARADAY TRANS. I 71(3): 558-68 (1975). 75-1032 Rao, P.S.; Hayon, E., One electron oxidation of odd-valent

metal ions in solution, J. PHYS. CHEM. 79(9): 865-8 (1975). 75-1044 Fujita, S.; Horii, H.; Mori, T.; Taniguchi, S., Pulse radiolysis of mercuric oxide in neutral aqueous solutions, J. PHYS. CHEM.

79(10): 960-4 (1975). 75-1049 Armor, J.N.; Hoffman, M.Z., Reactivity of coordinated nitrosyls. IV. One-electron reduction of ruthenium nitrosylpentaammine

(3 +) ion in aqueous solution, INORG. CHEM. 14(2): 444—6

(1975). 75-1064 Kelm, M.; Lilie, J.; Henglein, A., Pulse radiolytic investigation of the reduction of cadmium(II) ions, J. CHEM. SOC.,

FARADAY TRANS. 1 71(5): 1132-42 (1975). 75-1077 Armor, J.N.; Furman, R.; Hoffman, M.Z., Reactivity of coordinated nitrosyls. V. Generation and characterization of a ruthenium(II) alkylnitroso complex, J. AMER. CHEM. SOC.

97(7): 1737-42 (1975). 75-1086 O'Neill, P.; Steenken, S.; Schulte-Frohlinde, D., Formation of

radical cations from 1,2— and 1,4—dimethoxybenzene by

67
75-1092

75-1128

75-1130

75-1153

75-1171

75-1188

75-1203

75-1215

75-1218

75-

7093

76-

1001

76-1003

electron transfer to Tla+ and Ag2+ in aqueous solution. A pulse

radiolysis and in situ radiolysis EPR study, ANGEW. CHEM.

INT. ED. ENGL. 14(6): 430-1 (1975)

Meyerstein, D., Kinetics of complexation of copper(I) ions with maleate and fumarate in aqueous solutions. A pulse radiolytic

study, INORG. CHEM. 14(7): 1716-7 (1975).

Lilie, J.; Simic, M.G.; Endicott, J.F., Chemical behavior of rhodium(II)-ammine complexes generated by the pulse

radiolytic one-electron reduction of rhodium(III) ammines,

INORG. CHEM. 14(9): 2129-33 (1975).

O'Neill, P.; Schulte-Frohlinde, D., Evidence for formation of a (T10H)+ complex, J. CHEM. SOC., CHEM. COMMUN. (10): 387-8 (1975).

Barkatt, A., Rabani, J., Kinetics of spur reactions of electrons in ethylene glycol-water glassy ice. A pulse radiolytic study, J. PHYS. CHEM. 79(24): 2592-7 (1975).

O'Neill, P.; Steenken, S.; Schulte-Frohlinde, D., Formation of

radical cations of methoxylated benzenes by reaction with OH

radicals, Tla+

, Aga+, and S04 “ in aqueous solution. An optical and conductometric pulse radiolysis and in situ radiolysis electron spin resonance study, J. PHYS. CHEM. 79(25): 2773-

9 (1975).

Storer, D.K.; Waltz, W.L.; Brodovitch, J.C.; Eager, R.L., A

pulse radiolysis study of some platinum(II) and platinum(IV)

complex ions in aqueous solutions. The formation and

characterization of platinum(I) and platinum(III) transients, INT. J. RADIAT. PHYS. CHEM. 7(6): 693-704 (1975).

Fujita, S.; Horii, H.; Mori, T.; Taniguchi, S., Pulse radiolysis of Hg(CN)a in aqueous solutions, BULL. CHEM. SOC. JPN.

48(11): 3067-72 (1975).

Ilan, Y.A.; Czapski, G.; Ardon, M., The formation of CrOaa+ in the reaction of Cra+ + Oa in aqueous acid solutions, ISR. J. CHEM. 13(1): 15-21 (1975). Pikaev, A.K.; Sibirskaya, G.K.; Spitsyn, V.I., Pulsed radiolysis of aqueous solutions of compounds of divalent mercury, DOKL.

PHYS. CHEM. (ENGL. TRANSL.) 224(1-3): 994-7 (1975). Translated from DOKL. AKAD. NAUK SSSR 224(3): 638-41

(1975).

Falcinella, B.; Felgate, P.D.; Laurence, G.S., Aqueous chemistry

of thallium(Il) with manganese(II), iron(II), and cobalt(I) ions, J. CHEM. SOC., DALTON TRANS. (1): 1-9 (1975).

Tait, A.M.; Hoffman, M.Z.; Hayon, E., The reactivity of

cobalt(I) complexes containing unsaturated macrocyclic ligands

in aqueous solution, J. AMER. CHEM. SOC. 98(1): 86-93

(1976). Baxendale, J.H.; Garner, C.D.; Senior, R.G.; Sharpe, P., The

reduction of molybdenum(II) trifluoroacetate by pulse radiolysis

in methanol, J. AMER. CHEM. SOC. 98(2): 637-8 (1976).

76-1016 Faraggi, M.; Leopold, J.G., Pulse radiolysis studies of electrontransfer reaction in molecules of biological interest. II. The

reduction of Cu(II)-peptide complexes, RADIAT. RES. 65(2): 238-49 (1976). 76-1039 Tait, A.M.; Hoffman, M.Z.; Hayon, E., Reactivity of nickel(I) and copper(I) complex containing 14—membered macrocyclic

ligands in aqueous solution, INORG. CHEM. 15(4): 934—9

(1976). 76-1042 Jungbluth, H.; Beyrich, J.; Asmus, K.-D., Reduction of mercuric halides and pseudohalides in aqueous solution. Formation and some physicochemical properties of HgCl, HgBr,

Hgl, HgSCN, and HgCN radical molecules, J. PHYS. CHEM.

80(10): 1049-53 (1976). 76-1055 Broszkiewicz, R.K.; Grodkowski, J., Pulse radiolysis studies on

aqueous systems PtCV'-Cl

- and PtCLa~-Br

-

, INT. J. RADIAT. PHYS. CHEM.8(3): 359-65 (1976). 76-1072 Buxton, G.V.; Sellers, R.M.; McCracken, D.R., Pulse radiolysis

study of monovalent cadmium, cobalt, nickel and zinc in aqueous solution. Part 2. Reactions of the monovalent ions, J. CHEM. SOC., FARADAY TRANS. 1 72(6): 1464-76 (1976). 76-1087 Fujita, S.; Horii, H.; Mori, T.; Taniguchi, S., Pulse radiolysis of HgBra in aqueous solutions, BULL. CHEM. SOC. JPN. 49(5): 1250-3 (1976). 76-1093 Brodovitch, J.C.; Storer, D.K.; Waltz, W.L.; Eager, R.L., A

pulse radiolysis and flash photolysis study of the formation and

characterization of platinum(III) amine complex ions, INT. J. RADIAT. PHYS. CHEM. 8(4): 465-75 (1976). 76-1134 Sellers, R.M.; Simic, M.G., Pulse radiolysis study of the

reactions of some reduced metal ions with molecular oxygen in aqueous solution, J. AMER. CHEM. SOC. 98(20): 6145-50

(1976).

76-

1186 Buxton, G.V.; Green, J.C.; Sellers, R.M., Oxidation of

copper(I)-olefin complexes in aqueous solution by oxygen and

hydrogen peroxide, J. CHEM. SOC., DALTON TRANS. (21): 2160-5 (1976).

77-

0121 Buxton, G.V.; Sellers, R.M., The radiation chemistry of metal

ions in aqueous solution, COORD. CHEM. REV. 22(3): 195-

274 (1977). 77-1027 Simic, M.G.; Hoffman, M.Z.; Brezniak, N.V.; Kinetics of ligand-to-metal intramolecular electron transfer in cobalt(III)- ammine complexes containing a coordinated radical, J. AMER.

CHEM. SOC. 99(7): 2166-72 (1977). 77-1500 Buxton, G.V.; Green, J.C., Reactions of some simple a- and

/3-hydroxyalkyl radicals with Cu*f and Cu+ ions in aqueous

solution, J. CHEM. SOC., FARADAY TRANS. 1 74: 697-714

(1978).

U. S. GOVERNMENT PRINTING OFFICE : 1978-253-601

68
NBS-114A (REV. 7-73)

U.S. DEPT. OF COMM. 1 . PUB LIC ATION OR RE PORT NO. 2. Gov’t Accession

BIBLIOGRAPHIC DATA NSRDS-NBS 62

3. Recipient’s Accession No.

4. TITLE AND SUBTITLE

COMPILATION OF RATE CONSTANTS FOR THE REACTIONS OF METAL IONS

IN UNUSUAL VALENCY STATES

5. Publication Date June 1978

6. Performing Organization Code

7. AUTHOR(S)

George V. Buxton and Robin M. Sellers

8. Performing Organ. Report No.

9. PERFORMING ORGANIZATION NAME AND ADDRESS

NATIONAL BUREAU OP STANDARDS

DEPARTMENT OF COMMERCE

WASHINGTON, D.C. 20234

10. Project/Task/Work Unit No.

11. Contract/Grant No.

12. Sponsoring Organization Name and Complete Address (Street, City, State, ZIP)

Same as Item 9.

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Covered

N/A

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15. SUPPLEMENTARY NOTES

Library of Congress Catalog Card Number: 78-816

16. ABSTRACT (A 200-word or less factual summary of most significant information. If document includes a significant

bibliography or literature survey, mention it here.)

Kinetic data have been compiled for reactions of uncommon oxidation states of metals

which are produced by radiolysis of aqueous solutions of metal ions. Most of the

reaction rates are for transient species, and the rates were determined by pulse

radiolysis; some data were obtained by flash photolysis and gamma radiolysis. Metal

ions from Groups IB, I I B , I I I A , IVA, VIB, VI I B , VI I IB , and the lanthanides are included in the compilation.

17. KEY WORDS (six to twelve entries; alphabetical order; capitalize only the first letter of the first key word unless a proper name; separated by semicolons)

Aqueous solution; chemical kinetics; complex ions; electron transfer; metal ions;

radiation chemistry; rates; transients.

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