# Methods of Calculating Ionization Energies of Multielectron (Five or More) Isoelectronic Atomic Ions

Authors: Peter F. Lang; Barry C. Smith
Journal: The Scientific World Journal
 (2013)

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## Abstract

We have previously used simple empirical equations to reproduce the literature values of the ionization energies of isoelectronic sequences of up to four electrons which gave very good agreement. We reproduce here a kinetic energy expression with corrections for relativity and Lamb shift effects which give excellent agreement with the literature values. These equations become more complex as the number of electrons in the system increases. Alternative simple quadratic expressions for calculating ionization energies of multielectron ions are discussed. A set of coefficients when substituted into a simple expression produces very good agreement with the literature values. Our work shows that Slater's rules are not appropriate for predicting trends or screening constants. This work provides very strong evidence that ionization energies are not functions of complete squares, and when calculating ionization energies electron transition/relaxation has to be taken into account. We demonstrate clearly that for particular isoelectronic sequences, the ionizing electrons may occupy different orbitals and in such cases more than one set of constants are needed to calculate the ionization energies.


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## Body

## 1. Introduction

We have previously proposed a simple empirical equation to reproduce the literature values of the ionization energies of one-electron [1] and two-electron [2] atomic ions with very good agreement. This was recently extended to calculate ionization energies and first electron affinities of three and four electron ions [3] which also gave very good agreement with the literature values. However, we used a potential energy approach in our equation which has no theoretical basis.With the development of quantum theory, the two-particle problem can be solved exactly, and the kinetic energy of the electron in a hydrogen atom or hydrogen-like ion can be calculated using the Schrödinger equation. In 1930, Dirac [4] produced an equation which included a relativistic correction for the electron energy levels. Lamb and Retherford [5–7] were able to show that there is a small shift (now known as the Lamb shift) in the energy levels of the hydrogen atom not included in the Dirac equation. When the Lamb shift is taken into account, the actual ionization energies of one electron atoms are slightly less than that calculated by the Dirac equation. The calculation of the Lamb shift now forms an essential part in the theoretical calculations of energy levels and ionization energies of one and two electron atomic ions [8, 9].In this work, we begin by showing the expressions with relativistic corrections to calculate ionization energies which give excellent agreement with the literature values. However, as the number of electrons in the sequence increases, the expressions become more and more complex and less predictable.  Hence, we discuss alternative simple equations to calculate energies of isoelectronic sequences in excess of five electrons and show that it is more practical to adopt a simple expression to reproduce ionization energies which still provide very good agreement with generally accepted values. To maintain our aim of simplicity, the expressions/equations only contain fundamental constants or values derived from fundamental constants and fairly simple numbers.


## 2. Sources of Data

Moore [10–13] provided very detailed tables of atomic energy levels and ionization potentials in wave numbers (cm−1) and values converted from wave numbers to electron volts (eV) (where 1 cm−1 equals 1.2398418 × 10−4 eV) for atoms and atomic ions with estimated experimental errors and references to original work. These remain the most extensive survey of ionization energies and are still quoted in recent publications. The CRC Handbook of Chemistry and Physics [14] contains comprehensive data from Moore and later sources but does not supply information on estimated uncertainties. The majority of published ionization energy data are now available on the National Institute of Standards and Technology web site (http://www.nist.gov/srd/). These compilations include values of ionization energies that are accurately measured as well as crude estimates.


## 3. Ionization Energies of the Hydrogen to Boron Isoelectronic Sequences

When an electron in a multielectron system is ionized, we assume that the ionization energy contains (Jk) the kinetic energy term; (Jl) the Lamb shift term, (Jt) the relaxation/transition energy term, and any residual interaction (Er) [2]. Therefore, the ionization energy can be represented as [15]
(1)1n2μ(Jk-Jl-Jt)+Er=Ek-El-Et+Er,
where n is the principal quantum number and μ is the reduced mass and are provided in Table 2. Ek, El, and Et represent Jk, Jl, and Jt multiplied by 1/n2μ, respectively. Jk, Jl, and Jt are multiplied by 1/n2μ because the electron ionized occurs in energy level n and it revolves around the centre of mass. A list of reduced masses are given in Table 2. It is common to present ionization energies in eV (electron volt). Calculated results in this work are converted to eV from Joules by using the relationship of 1 eV = 1.60217648 ×  10−19 J, any other figures in cm−1 are converted to eV by multiplying them with the value 0.00012398418.


## 4. The Relativistic, Lamb Shift, Electron Transition/Relaxation, and Residual Corrections

The energy of an electron moving in a Bohr orbit can be represented by(2)movo2a0=q1q2(4πεoa02),
where mo is the electron rest mass, vo is the velocity of the electron, q1q2 stand for the charges of the electron and nucleus, εo is the permittivity of a vacuum, and a0 is the Bohr radius. The velocity vo of the electron in the hydrogen atom can be calculated from the above relationship and is equal to 2.1876913 × 106 m/sec. The velocity v of the electron in successive atoms of the one-electron series increases by Z times where Z is the atomic/proton number or v=voZ. When there is more than one electron in the system, we assume that the velocity of the electron changes by (Z-S) where S is the screening constant for that electron.The theory of relativity [16] points out that the mass m of a moving particle is given by the expression m=mo/((1-v2/c2)) where mo is the rest mass of particle.  Expansion of this expression gives
(3)m=mo(1+12v2c2+38v4c4+516v6c6+⋯),
therefore it follows that (1/2)mv2=(1/2)mov2(1+(1/2)v2/c2+(3/8)v4/c4+(5/16)v6/c6+⋯).The kinetic energy components including relativistic correction for a one-electron atom at an equilibrium position (when the relativistic correction is half that of the maximum) are then(4)12mov2+0.5(14mov4c2+316mov6c4).
The ionization energy of a one-electron atom is then
(5)I=μ(12mov2+0.5(14mov4c2+316mov6c4)-El).The Lamb shift is usually computed by highly complex formulas which require lengthy computer routines to compute [17]. We assume (without theoretical justification) that the Lamb shift is a relativistic charge, mass, and size ratio effect. The reduced mass calculation [18] implicitly assumes that the electron and nucleus are point charges. But they have a finite size hence there needs to be an extra component in the reduced mass calculation. The energy reduction to take account of reduced mass is not simply me/(me+mp)((1/2)movo2) but should include a function of the charge and the ratio of nuclear to atomic size, and this component is calculated by the following expression:
(6)El=(meme+mp)(α2.67)(12movo2)(Z-S)3.2A1/3,
where me is the electron mass, mp is the proton mass, and the factor for the reduced mass correction for hydrogen is me/(me+mp). The size of the nucleus increases roughly proportional to A1/3 [19]. α is the fine structure constant, and (α/2.67) is a crude approximation of the square root of the ratio of nuclear to atomic size for hydrogen, and A is the mass number of the atom. In a one electron system, S is zero.After an electron is ionized, one or more of the remaining electron(s) is/are attracted more closely to the nucleus. The attractive energy between the proton and the remaining electron(s) changes because of the change in screening experienced by the remaining electron(s) before and after ionization, [15] and this transition/relaxation energy is a function of
(7)n24(12mo(vo(Z-S1))2-12mo(vo(Z-S2))2),
where S1 is the screening constant for the remaining electron(s) after ionization and S2 is the screening constant for the remaining electron(s) before ionization.In the helium system, there are two electrons and both occupy the 1s orbital. Since each electron occupies half of the space and each is repelled by only one other electron (here we have assumed that the two electrons act as in a two-particle problem and are equivalent), the screening constant is a half (0.5).  After ionization, there is zero screening.In the lithium series, the electron that is ionized occupies a higher (2s) orbital and is shielded by two 1s electrons, and the screening increases by 1 to 1.5. The extra screening experienced by the two inner electrons in the 1s orbital increases to 0.625 and which is an increase by 1/8 or 0.125 rather than 0.5 because the third electron occupies a different orbital and in a different electron shell (i.e., 0.5 of 0.5 of 0.5). After ionization, only two electrons are left in the system and the screening reduces to just 0.5.In the beryllium series, the electron that is ionized occupies the 2s orbital. Since there are four electrons and each moving in an elliptical orbit, each may at any time interact differently with the other three electrons. The screening of the fourth electron increases by a half to 2, and the other electron in the 2s orbital experiences a screening of between 1.5 and 2 and is 1.75. After ionization of the fourth electron, the screening experienced by the third electron drops back to 1.5.For the boron system, the outermost electron occupies a new orbital and the screening increases by 1 to 3. The screening of the fourth electron increases by 0.25 to 2.25, and after ionization the screening reduces back to 2.We assume that there are two opposite and competing residual electron-electron interactions, and this is discussed in detail in previous work and is not fully reproduced here [15]. In summary, there are temporary asymmetric distributions of electrons (e.g., they may be nearer to each other or further apart than average). The first type (when they are nearer to each other) is residual electron-electron repulsion which reduces slightly the energy required to ionize the electron, and this reduction diminishes very rapidly because with each successive ionization the size of the electron orbit/shell becomes smaller and the electrons become much more tightly bound to the nucleus. The reduction in energy resulting from this interaction is expressed by
(8)Er1=(12movo2)QIα((Z-(I-1))!).The opposite and competing electron-electron interaction occurs when there are more than two electrons in the system. In a three electron system, two electrons occupy the 1s orbital and one occupies the 2s orbital. The instantaneous asymmetric distribution of electrons produces an effect which result in the 2s electron being screened slightly less than 0.5 from each of the 1s electrons. The result is that one of the electrons is temporarily attracted to the nucleus a bit more than expected and hence increases the amount of energy required to remove it from the atom/ion. This is represented by(9)Er2=1n2(12movo2(Z-S)2)αQII2,
and the total residual electron interaction energy change is
(10)Er=(-(12movo2)QIα((Z-(I-1))!)+1n2(12movo2(Z-S)2)αQII2).Symbols and values of constants shown in all the expressions in this work are given in Table1. QI is the number of electron-electron interactions before ionization and QII is the number of electron-electron interactions after ionization.Table 1
Symbols, conversion factors, and constants (to 9 significant figures).
Symbol/constant
Value/comment/definition
α
0.00729735254
I
Number of electrons remaining after ionization
eV
1 electron volt = 1.60217648 × 10−19 Joules
n
Principal quantum number
v
Electron velocity
Q
Number of residual electron-electron interactions
A
Mass number
µ
Reduced mass (see Table8 for individual values)
S
Screening constant for the ionizing electron
S
1
Screening for the remaining electron(s) after ionization
S
2
Screening for the remaining electron(s) before ionization
Z
Proton number (nuclear charge)
c
Velocity of light 2.99792458 × 108 ms−1
m
e
Electron rest mass 9.10938215 × 10−31 kg
m
p
Proton rest mass 1.67262164 × 10−27 kg
q
Electron charge 1.60217649 × 10−19 C
h
Planck’s constant 6.62606896 × 10−34 Js
ε
o
8.85418782 × 10−12 Fm−1Table 2
Coefficients/constants for calculating ionization energies of multielectron ions.
Z
(
1
)
(
2
)
(
3
)
(
4
)
Screening constants
Coefficienta
Coefficientb
Reduced mass*
B
3
0.318
0.032
0.999939550
C
3.5
0.572
0.490
0.999954670
N
4
0.842
1.170
0.999961152
O
5
0.716
0.731
0.999966015
F
5.5
1.054
2.357
0.999971388
Ne
6
1.318
3.520
0.999972825
Na
7
2.222
11.809
0.999976377
Mg
7.5
2.344
12.925
0.999977367
Al
8.5
2.882
21.124
0.999979889
Si
9
3.012
22.521
0.999980614
P
9.5
3.194
24.599
0.999982497
S
10.5
2.850
22.194
0.999983051
Cl
11
2.968
23.026
0.999983571
Ar
11.5
3.306
27.683
0.999986454
**
Screening constants
Coefficienta
Coefficientb
Reduced mass
K
11
2.968
23.026
0.999986113
Ca
11.5
3.306
27.683
0.999986467
Sc
13.5
3.366
30.828
0.999988489
Ti
14
3.832
38.481
0.999989186
V
14.5
4.542
51.618
0.999989405
Cr
15
5.138
62.763
0.999990000
Mn
15.5
5.658
73.472
0.999990188
Fe
16.5
5.850
82.119
0.999990702
Co
17
4.484
57.749
0.999990708
*Reduced masses are calculated from atomic number 5 to atomic number 26; for ions above atomic number 26, the reduced mass of atomic 26 is used since the differences between reduced masses at high atomic numbers are too small to show any differences in the calculated results.
**From the potassium series, the constants apply to calculating ionization energies from the third ionization energy (i.e., third ionization of potassium, fourth ionization of calcium, etc.).


## 5. Ionization Energies of One and Two Electron Ions

There is only one electron andn is 1, the formula for calculating the ionization energy is
(11)I1=μ(me(me+mp)(α2.67)(12movo2)(Z)3.212mov2+0.5(14mov4c2+316mov6c4)-(meme+mp)(α2.67)(12movo2)(Z)3.2A1/3).
The one-electron ionization energies calculated by (11) when compared with the ionization energies published in the CRC Handbook of Chemistry and Physics agree to 99.999% or better in the majority of cases. The biggest absolute difference is 0.086 eV (to 3 decimal places) from a calculated value of 5469.95 eV or 0.00164% [15].The ionization energy of a two electron system is (Ek-El-Et+Er), where
(12)El=μ((meme+mp)(α22/3)(12movo2)(Z-0.5)3.2A1/3);Et=0.25μ(12mo(vo(Z))2-12mo(vo(Z-0.5))2);Er=(-(12movo2)α((Z)!)).
Since, for simplicity, we have not applied a relativistic correction to Et we have made a crude approximation of reducing the relativistic correction in Ek by another 5% to 0.45 (rather than 0.5) and where v is (vo(Z-0.5)), so it is
(13)Ek=μ(12mov2+0.45(14mov4c2+316mov6c4)).When compared to theCRC Handbook of Chemistry and Physics the majority of values differ by less than 0.01%, the largest absolute difference is 0.216 eV from a calculated value of 2437.846 eV or 0.0089%.


## 6. Ionization Energies of Three-, Four-, and Five-Electron Ions

The ionization energy of a three-, four-, and five electron system is(14)(Ek-El-Et+Er),
where
(15)El=0.25μ((meme+mp)(α22/3)(12movo2)(Z-0.5)3.2A1/3);Et=μ(12mo(vo(Z-S1))2-12mo(vo(Z-S2))2);Er=((-(12movo2)QIα((Z-(I-1))!)+1n2(12movo2(Z-S)2)αQII2Qα((Z-(I-1))!))).
As with the two-electron system, we have not applied a relativistic correction to Et but we have made a crude approximation of reducing the relativistic correction in Ek by 5% to 0.45 and where v is (vo(Z-S)), so that the expression becomes
(16)Ek=0.25μ(12mov2+0.45(14mov4c2+316mov6c4)).
The agreement with the literature values of ionization energies is 99% or better in all cases. It is evident from the above discussion that as the number of electrons in the system increases the equations get more complicated and it is difficult to determine the various corrections.


## 7. Alternative Simple Equations to Calculate Ionization Energies

Besides the more complicated equations shown above, ionization energies can be calculated with simpler expressions but not so precise. A simple formula is sometimes used to calculate ionization energies. It often takes the form of [20]
(17)I=(1n*2)hcRH(Z-S)2,
where RH is the Rydberg constant for hydrogen (R∞, the Rydberg constant for infinite mass is equivalent to 13.6059 eV), n* is an “effective” quantum number, Z is the atomic number, and S is the screening constant based on Slater’s rules [21] which enable approximations of analytic wave functions to be constructed for rough estimates [22]. Equation (17) makes a very simplistic assumption that when an electron is removed from an atom or ion, the atom/ion remains unchanged except for the removal of that electron. We believe that it is incorrect to use equations like (17) (where the ionization energy is considered as a function of a complete square) to calculate energies in isoelectronic series. For multielectron systems, we need to consider electron transition/relaxation and other smaller components which may influence the ionization energy of an electron.In a multielectron system, the main components of the energy change during ionization are the electron-proton energy or(Z-S)2 and the electron relaxation energy (or kn2[((Z-S1)2-(Z-S2)2)] where k is a constant dependent on the particular shell/orbital, S1 and S2 represent the screening constants of the remaining electrons after and before the electron is ionized). In most cases, the electron-proton energy component alone accounts for 90% or more of the energy change and together with the relaxation energy can represent more than 95% of the total energy change.  If factors which in total contribute only a small percentage of the energy change, such as residual repulsion, pairing or exchange energies are excluded, the expression for calculating the ionization energy can be approximated to
(18)I=(1n2)Rμhc×{(Z-S)2-0.25n2[((Z-S1)2-(Z-S2)2)]}.
This can be expanded to become
(19)I=(1n2)Rμhc{(Z2-2ZS+S2)-k[(Z2-2ZS1+S12)-(Z2-2ZS2+S22)]}.
Since in the second half of expression (19) the Z2 term cancels out, only 2Z(S1-S2) and (S22-S12) are left. 2Z(S1-S2) can be reduced to aZ, and (S22-S12) becomes a constant b. This can be rearranged and simplified to
(20)I=(1n2)Rμhc{(Z2-2ZS+S2)-aZ+b},
where a and b are constants for each isoelectronic system, n is the principal quantum number, and, unlike (17), expression (20) is not a complete square.We have formulated the following rules for working out screening (shielding) constants:(1) for each additional electron in the system, the screening increases by 0.5 unless (2) the electron to be ionized occupies a new orbital such as from beryllium to boron when it increases by 1 and (3) to account for the pairing effect, such as from nitrogen to oxygen, the screening constant increases by 1. For example, for the carbon system, the screening increases by 0.5 units to 3.5 and increases by a further 0.5 to 4 for nitrogen but increases to 5 for oxygen.We made different estimates of the screening constantsS2 and S1 and obtained various values of a and b. We then selected the values that give the best results and a list of screening constants, coefficients a and b and reduced masses as shown in Table 2. They are used with equation (20) to calculated the ionization energies of isoelectronic sequences from five electrons.The values calculated from expression (20) are presented for the first six appropriate members of each series for the following two reasons.  Firstly, as we have already shown [14], ionization energies of the first few members of isoelectronic sequences are the most precise. Sometimes, only the first four or five members of a series are experimentally measured and uncertainties increase further along a series. Secondly, our results are compared with ionization energies with those compiled in the CRC Handbook of Chemistry and Physics, and for many isoelectronic series with more than twenty electrons, only a limited number of values are available for each sequence. Some of these values are given to many significant figures and some only to two or three significant figures because uncertainties can be of the order of 1 eV or higher.  Since, as with previous work, all our results are rounded to three decimal places we have decided that where the CRC Handbook of Chemistry and Physicshas provided values with more than three decimal places they are rounded to three decimal places in the tables.


## 8. Ionization Energies from Five- to Eighteen-Electron Isoelectronic Atomic Ions

Ionization energies reported in theCRC Handbook for five to eighteen electronic series (first six members) are given in Table 3. Values of ionization energies calculated using our coefficients are provided in Table 4. Percentage differences between our values and values published by the CRC Handbook as listed in Table 5 show that all values agree to 98% or better. Just over 76%, the calculated values agree to 99% or better.Table 3
Ionization energies (eV) of isoelectronic series from theCRC Handbook (5 to 18 electron sequences)—first six members of each series.
Z
(
2
)
(
3
)
(
4
)
(
5
)
(
6
)
(
7
)
First
Second
Third
Fourth
Fifth
Sixth
B
8.298
24.383
47.449
77.414
114.243
157.930
C
11.260
29.601
54.936
87.140
126.210
172.180
N
14.534
35.121
62.708
97.120
138.400
186.760
O
13.618
34.971
63.450
98.910
141.270
190.490
F
17.423
40.963
71.620
109.266
153.825
205.270
Ne
21.565
47.286
80.144
119.992
166.767
220.421
Na
5.139
15.035
28.448
45.142
65.025
88.053
Mg
7.646
18.829
33.493
51.444
72.595
97.030
Al
5.896
16.346
30.203
47.222
67.800
91.009
Si
8.152
19.770
34.790
53.465
75.020
99.400
P
10.487
23.338
39.610
59.810
82.660
108.780
S
10.360
23.814
40.740
60.910
84.500
110.680
Cl
12.968
27.630
45.806
67.270
91.650
119.530
Ar
15.760
31.630
50.913
73.489
99.300
128.130Table 4
Ionization energies (eV) of isoelectronic series calculated using expression 23 and coefficients/constants from Table2 (5 to 18 electron sequences).
Z
(
2
)
(
3
)
(
4
)
(
5
)
(
6
)
(
7
)
First
Second
Third
Fourth
Fifth
Sixth
B
8.306
24.231
46.959
76.490
112.824
155.960
C
11.252
29.715
54.980
87.049
125.920
171.595
N
14.544
35.490
63.238
97.790
139.144
187.302
O
13.616
34.990
63.167
98.148
139.930
188.517
F
17.419
41.045
71.475
108.706
152.741
203.579
Ne
21.564
47.693
80.626
120.361
166.900
220.241
Na
5.090
15.336
28.606
44.900
64.217
86.558
Mg
7.629
19.203
33.801
51.422
72.066
95.734
Al
5.907
16.668
30.452
47.260
67.091
89.945
Si
8.092
20.168
35.267
53.390
74.536
98.706
P
10.489
23.802
40.138
59.497
81.880
107.287
S
10.347
24.179
41.035
60.915
83.818
109.745
Cl
12.955
28.121
46.310
67.523
91.760
119.020
Ar
15.760
31.926
51.116
73.330
98.567
126.828Table 5
Percentage difference between values shown in Tables3 and 4.
Z
(
2
)
(
3
)
(
4
)
(
5
)
(
6
)
(
7
)
First
Second
Third
Fourth
Fifth
Sixth
B
−0.1
0.6
1.0
1.2
1.2
1.2
C
0.1
−0.4
−0.1
0.1
0.2
0.3
N
−0.1
−1.0
−0.8
−0.7
−0.5
−0.3
O
0.0
−0.1
0.4
0.8
0.9
1.0
F
0.0
−0.2
0.2
0.5
0.7
0.8
Ne
0.0
−0.9
−0.6
−0.3
−0.1
0.1
Na
1.0
−2.0
−0.6
0.5
1.2
1.7
Mg
0.2
−2.0
−0.9
0.0
0.7
1.3
Al
1.3
−2.0
−0.8
−0.1
1.0
1.2
Si
0.7
−2.0
−1.4
0.1
0.6
0.7
P
0.0
−2.0
−1.3
0.5
0.9
1.4
S
0.1
−1.5
−0.7
0.0
0.8
0.8
Cl
0.1
−1.8
−1.1
−0.4
−0.1
0.4
Ar
0.0
−0.9
−0.4
0.2
0.7
1.0


## 9. Ionization Energies from Nineteen- to Twenty-Seven-Electron Isoelectronic Sequences

Treatment of ionization energies of isoelectronic with nineteen electrons or more are different and more complicated. This is because, from atomic number nineteen, the electron to be ionized is in period 4 of the periodic table and such an isoelectronic system includes ionization of s or d electrons [23]. We have demonstrated that for the transition metals or lanthanide [24] elements, the ionization process is complicated and, in the majority of cases, d or f electrons are not removed in the first or second ionization. For example, consider the potassium, calcium, scandium, and titanium series (isoelectronic series with 19, 20, 21, and 22 electrons resp.). For the potassium series (19-electron isoelectronic), the first ionization of potassium and the second ionization of calcium both involve removal of a 4s electron. But the third ionization of scandium and the fourth ionization of titanium (which are in the same isoelectronic series) involve removal of a 3d electron.  For the calcium series (20-electron isoelectronic), the first ionization of calcium and the second ionization of scandium involve removal of a 4s electron whereas the third ionization of titanium involves removal of a 3d electron. Similarly with the scandium and titanium series, for the first two members of the series, the energy change is the energy required to ionize a 4s electron but from the third member of the series onwards the energy change is the energy for ionizing a 3d electron (a more detailed discussion is provided in a previous work [23]). Equation (20) shows that ionization is a function of 1/n2. Therefore, for the 19, 20, 21, and 22 isoelectronic series, the correct fraction or decimal for 1/n2 to use is 1/16 (or 0.0625) for the first two members of the series but 1/9 (or 0.11111) for the remainder of the series. Hence, for the above reasons, it is incorrect to use a single set of coefficients to calculate the energies of an isoelectronic sequence which may involve removal of electrons in different orbitals.We believe that there is little value calculating the first and second ionization energies of sequences beginning with the potassium. From the potassium series onwards, the third ionization energy requires a different set of coefficients. For example, for the potassium series, a set of coefficients is used to calculate the third ionization energy of potassium, the fourth ionization energy of calcium, and the fifth ionization energy of scandium, and so on because a 3p electron is ionized in all cases. For the scandium series, the third ionization of scandium, the fourth ionization of titanium, and the fifth ionization of vanadium and so on can be calculated using one set of coefficients since in all cases a 3d electron is ionized. However, the third ionization energy of the potassium series and the third ionization energy of the calcium series are identical to the fifth ionization of the chlorine and argon series, respectively. Hence, these two series will not be repeated in Tables6 and 7.Table 6
Ionization energies (eV) of isoelectronic series from the CRC.
Z
(
2
)
(
3
)
(
4
)
(
5
)
(
6
)
(
7
)
Third
Fourth
Fifth
Sixth
Seventh
Eighth
Sc
24.757
43.267
65.282
90.635
119.203
151.060
Ti
27.492
46.709
69.460
95.600
124.980
157.800
V
29.311
49.160
72.400
99.100
128.900
162.000
Cr
30.960
51.200
75.000
102.000
133.000
166.000
Mn
33.668
54.800
79.500
108.000
139.000
174.000
Fe
30.652
51.300
76.060
103.000
134.000
169.900
Co
33.500
54.900
79.800
108.000
140.900
N/ATable 7
Ionization energies (eV) of isoelectronic series using (20) and constants/coefficients in Table 2*.
Z
(
2
)
(
3
)
(
4
)
(
5
)
(
6
)
(
7
)
Third
Fourth
Fifth
Sixth
Seventh
Eighth
Sc
24.780
43.879
66.002
91.149
119.319
150.513
Ti
27.479
47.386
70.316
96.270
125.247
157.248
V
29.330
49.676
73.044
99.436
128.852
161.291
Cr
30.917
51.873
75.853
102.856
132.882
165.932
Mn
33.670
55.351
80.056
107.785
138.537
172.313
Fe
30.642
52.034
76.448
103.887
134.349
167.834
Co
33.509
55.453
80.421
108.413
139.428
N/A
*Ionization energy of isoelectronic series starting from the third ionization energy of the appropriate series.We have calculated the ionization energies up to the cobalt series (which contains five appropriate published values for comparison) because beyond the cobalt series there are fewer and fewer published values available for use in comparison. Ionization energies of isoelectronic series reported in theCRC Handbook for sequences from scandium to cobalt (for each series beginning with the third ionization energy) are given in Table 6. Values of ionization energies calculated using our coefficients are provided in Table 7. Percentage differences between our values and values in the CRC Handbookas listed in Table 8 show that all calculated values agree to 98%, or better and just under 83% of the values agree to 99% or better.Table 8
Percentage difference between values shown in Tables6 and 7.
Z
(
2
)
(
3
)
(
4
)
(
5
)
(
6
)
(
7
)
Third
Fourth
Fifth
Sixth
Seventh
Eighth
Sc
−0.1
−1.4
−1.1
−0.6
−0.1
0.4
Ti
0.0
−1.4
−1.2
−0.7
−0.2
0.3
V
−0.1
−1.0
−0.9
−0.3
0.0
0.4
Cr
0.1
−1.3
−1.1
−0.8
0.1
0.0
Mn
0.0
−1.0
−0.7
0.2
0.3
1.0
Fe
0.0
−1.4
−0.5
−0.9
−0.3
1.2
Co
0.0
−1.0
−0.8
−0.4
1.0
N/A


## 10. Discussion

We have used a simple quadratic expression in this work. We have not considered exchange and orbital energies (20) and have ignored any residual interactions or relativistic corrections, which for multielectron systems are difficult to apply. Hence, it is not surprising that the agreement with some of the generally accepted values is less than 99%. However, some of the differences between the calculated values and CRC Handbook values are less than the experimental uncertainties. However, as we have shown above, equations for solving ionization energies can be very complicated and the results may be unpredictable as the number of electrons in an isoelectronic series increases. Therefore, we believe that there is a strong case to use a simple quadratic expression rather than trying to create complex equations to calculate ionization energies.Although Slater’s rules are still cited in recent publications [25] as adequate for predicting most periodic trends, it has been pointed out that the rules are unreliable when orbitals with a total quantum number of 4 [26] is reached (e.g., a 3p orbital has a principal quantum number of 3, orbital quantum number of 1, and magnetic quantum number of 1, and spin quantum number of 1⁄2 already has a total quantum number of 5). Equation (17) and Slater’s rules are based on simple assumptions and are unable to account for many different features of ionization energies across the periodic table. We have also shown that ionization energies are not functions of simple complete squares [23], and Slater’s rules cannot account for the complex patterns in ionization energies shown in our previous work [24].


## 11. Conclusion

Ionization energies calculated by a kinetic energy approach with simple relativistic and Lamb shift corrections give remarkable agreement with generally accepted values for one- to five-electron isoelectronic series. However, for multielectron isoelectronic series with five or more electrons, there is no accepted methodology for calculating relativistic corrections. Therefore, it is practical and more manageable to use a simple quadratic expression to calculate ionization energies which still give very good agreement with generally accepted values. We have not attempted to calculate ionization energies of sequences beyond cobalt because there are few sequences where a long series of data are available. We believe that expression (20) can be used to calculate ionization energies of any multielectron isoelectronic series assuming that sensible coefficients are applied. It is evident that an equation based on (17) (or function of a complete square such as (Z-S)2) is not the correct representation of the energy change when an electron is ionized. We have also demonstrated that it is incorrect to use a single set of constants/coefficients to calculate the ionization energies of some isoelectronic series such as the potassium, calcium, or scandium series.Since a great many of the experimental measurements of ionization energies were done over half a century ago, and some of the published values are extrapolated/interpolated, or estimates with fairly large uncertainties there is also a strong case for new measurements to be undertaken and reliability of some of the currently accepted values to be reexamined.



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