HDTenEightyP/NetNews huggingface dataset:
From: scotbri@flower.rosemount.com (Scott Brigham)
Subject: Soft Drink Ingredient
Originator: scotbri@flower
Organization: Rosemount, Inc.
Distribution: usa
Date: Tue, 15 Dec 1992 15:36:55 GMT

I was reading the label on my bottle of Schweppes Bitter Lemon
and noticed the last ingredient is "glycerol ester of wood rosin".
What is this and why am I drinking it?
=========================
 scotbri@rosemount.com  
 Scott Brigham  (AA0HU)
 St. Paul, MN  USA
=========================
From: whitbeck@equinox.unr.edu (Michael Whitbeck)
Newsgroups: sci.chem
Subject: oops! was phosphate buffer problem
Date: 17 Dec 92 01:55:51 GMT
Distribution: na
Organization: University of Nevada, Reno

In a previous post I plug'd-n-chug'd
an approximate solution to a problem/question
about a phosphate buffered solution.

While I quickly cross-checked the results re the
acid dissociation constants I didn't cross check
mass balance or charge balance (sheepish grin goes here)

So much for back of the envelop calculations!

Mike W.
Newsgroups: sci.chem
From: gay@selkirk.sfu.ca (Ian D. Gay)
Subject: Re: Acid-base equilibrium (triprotic)
Keywords: acid base equilibrium triprotic
Organization: Simon Fraser University, Burnaby, B.C., Canada
Date: Wed, 16 Dec 1992 20:05:33 GMT

whitbeck@equinox.unr.edu (Michael Whitbeck) writes:

>>How much of each solution will you use?
>>
>>You are given the following data:
>>_Acid_        _pKa_ _Ka_
>>H3PO4  2.148 7.11 * 10^-3
>>H2PO4  7.199 6.32 * 10^-8
>>HPO4        12.15 7.1  * 10^-13

>Using your Ka values...
>If you relax the 'free phosphate' restriction a bit
>then if you mix 0.53 liter of the H3PO4 with 0.47 liter of
>the Na3PO4 solution you should get (to 1 sig. fig :-)

>H3PO4 0.144e-4
>H2PO4 0.702
>HPO4 0.187
>PO4 0.112  (pretty close to .1!)
>H 0.157e-6  (~ 6.8 pH)

Unfortunately [H+][PO4---]/[HPO4--] is nowhere near to being equal to 
K3, with your proposed values, so this is not a solution of the 
equilibrium problem.

>Wheee... back in freshman chemistry again!

 D-, marking generously.
From: verhaar@accucx.cc.ruu.nl (Henk Verhaar)
Newsgroups: sci.chem
Subject: Re: Literature about CoMFA and QSAR
Date: 17 Dec 92 13:15:44 GMT
Organization: Academic Computer Centre Utrecht

In <1992Dec13.003238.1@hmcvax.claremont.edu> mulman@hmcvax.claremont.edu (Mike Ulman) writes:

>In article <1992Dec10.104719.8976@aragorn.unibe.ch>, braendle@iac.unibe.ch (Martin Braendle) writes:
>> Can anyone point me to introducing literature about Comparative Molecular
>> Field Analysis (CoMFA) and QSAR methods? Thank you.
>> 
>> Martin Braendle
>-- 

>If I understand you correctly, you are looking to a book that will introduced
>you to QSARs and how to start. Try:

>Martin, Y.C. "Quantitative Drug Design", Marcel Dekker, Inc., New York, 1978.

>In general, look for literature articles by Leo Hansch of Pomona College.

That should be Leo & Hansch. :)
Looking for Hansch & Leo might be even more useful.

There is a reasonably large body of literature on QSAR. For a more or less
uptodate overview, browse through recent issues of Quantitative Structure-
Activity Relationships, a journal published by VCH. One of the good things of
this journal, besides being a good one, is that they publish summaries of
related articles in other journals.

QS-AR has a reasonable number of papers on CoMFA as well. If your really
interested in CoMFA, maybe the appropriate sections in the SYBYL (by TRIPOS)
manuals might be worth reading.

Which field of QSAR are you interested in anyway? (I'm in QSAR in
environmental toxicology and chemistry; in my field CoMFA isn't all that
useful).

Hope this helps

Henk-- 
Henk Verhaar <verhaar@cc.ruu.nl>

Research Institute of Toxicology - University of Utrecht
Dept of Environmental Toxicology

Where we find out just how much junk you can bear and still be (re)productive!
Newsgroups: sci.chem,sci.engr.chem,sci.misc,sci.chem,organomet
From: gcook@horus.cem.msu.EDU (Greg Cook|xxxxxx)
Subject: Re: sci.chem.organomet is ACTIVE NOW!!!!
Organization: Michigan State University
Date: Wed, 16 Dec 92 13:49:49 GMT

From article <cabku01.724435494@mailserv>, by cabku01@mailserv.zdv.uni-tuebingen.de (Hartwig Kuehbauch):
> 
> Finally --- we made it!!!
> 
> SCI.CHEM.ORGANOMET is active now!!!

I am glad to see this happen.  When I first suggested we start sci.chem
about 5 years ago, I envisioned a different chem group for each area.

I was thinking more along the lines of pchem, inorgchem, orgchem, and
analchem; but why not organomet?  I'm just surprised to see this one
be created first.

-----------------------------------------------------------------------
Gregory R. Cook                           gcook@horus.cem.msu.edu
Department of Chemistry                   cookgreg@student.msu.edu
Michigan State University                 cook@msucem.BITNET
From: sklar@picasso.ocis.temple.edu (Dave Sklar)
Newsgroups: sci.chem
Subject: Stable Orbitals: 1/2 full
Date: 13 Dec 92 04:09:48 GMT
Organization: Temple University
X-Newsreader: Tin 1.1 PL5


	The e- config. of Cr is [Ar]3d54s1, while it would be expected to
be [Ar]3d44s2.  This is so the 3d orbital can be half-filled, which is more
stable, apparently, than 4/10 filled.  Why is a half filled shell more
stable?  It seems intuitive, but intuition is pretty worthless inside an
atom.

	Dave
Newsgroups: sci.chem
From: Norbert Mueller <K360171@alijku11.edvz.uni-linz.ac.at>
Subject: Molfile format
X-Xxmessage-Id: <A7553BF3E0016205@nmueller.chemie.uni-linz.ac.at>
X-Xxdate: Wed, 16 Dec 92 19:02:59 GMT
Organization: Johannes Kepler Univ., Inst. of Chemistry
X-Useragent: Nuntius v1.1.1d12
Date: Wed, 16 Dec 1992 19:03:03 GMT

The Molfile data format has been placed in the public domain, as far
as I know from hearsay. Can someone please point me to a document that
explicitly states this and that gives a complete description of this
format ?

Thanks in advance.


Norbert M\ller
Institute of Chemistry
Johannes Kepler University
A-4040 Linz
Austria 
e-mail K360171@ALIJKU11.bitnet
       K360171@EDVZ.uni-linz.ac.at
       Norbert@soft.uni-linz.ac.at
Newsgroups: sci.chem
From: billn@hpcvaac.cv.hp.com (bill nelson)
Subject: Re: composition of "white" gold
Organization: Hewlett-Packard Company, Corvallis, Oregon USA
Date: Sun, 13 Dec 1992 09:46:16 GMT

giber@pollux.cs.uga.edu (Carolyn Giberson) writes:
: 
: White gold is a gold alloy, containing silver and nickel I think.

Nope. If there is silver in it, it is green gold. I am not sure what
nickel would do to the gold.

Bill
Newsgroups: sci.chem
From: cid@athena.mit.edu (Derek H Cedillo)
Subject: H2O Evaporation Calculation
Organization: Massachusetts Institute of Technology
Date: Sun, 13 Dec 1992 06:47:30 GMT

Help please,
I would like to know a method of calculating
the time it would take water to evaporate
in a given temp and humidity.
anyone have an equation or table or something
of the sorts.  Answers and Pointers
welcomed at: Cid@athena.mit.edu

Thanks a million!!!


Derek

-------------------------------------------------------------------
"He lived a life of going-to-do, 
   and died with nothing done"	       
		-J. Albery	     

In other words---JUST DO IT!
Newsgroups: sci.chem
From: hank@well.sf.ca.us (Hank Roberts)
Subject: Re: What is in those 'bubbling' lamps?
Keywords: lamps
Organization: Whole Earth 'Lectronic Link
Date: Wed, 16 Dec 1992 01:47:05 GMT


LavaLamps are still available, in several colors and sizes. Someone
on the net posted an address a few years ago, which I've lost; a phone
call to The Exploratorium Store (San Francisco, CA 415 561-0393 mail order)
will get you your choice.

"Not even a happy user, just someone who wants one for his birthday."
From: daniel@teer19.acpub.duke.edu (Daniel Crawford)
Newsgroups: sci.chem
Subject: SUMMER UNDERGRADUATE FELLOWSHIPS
Date: 18 Dec 92 15:17:25 GMT


                       The University of Georgia

               CENTER FOR COMPUTATIONAL QUANTUM CHEMISTRY

             Summer Research Fellowships for Undergraduates

LOCATION: The Center for Computational Quantum Chemistry, The University
of Georgia in Athens, Georgia.

DIRECTOR: Dr. Henry F. Schaefer, III.

RESEARCH: Each Summer Research Fellow will conduct an independent
research project under the guidance of a Senior Scientist and will
receive adequate training (lectures and computer workshops) in molecular
quantum mechanics and spectroscopy.  Research at the CCQC involves the
use and development of state-of-the-art theoretical methods to describe
the electronic structure of molecules.  A wide variety of chemical
problems have been examined using _ab initio_ methods such as
Self-Consistent Field, Configuration Interaction, and Coupled Cluster.

Some examples include: 
(1) silicon analogs of common hydrocarbon compounds;
(2) potential energy hypersurfaces governing elementary gas-phase
    chemical reactions;
(3) problems in physical organic chemistry, including carbenes and
    biradicals;
(4) hydrogen-bonded systems.

QUALIFICATIONS: Applicants should have completed their junior
undergraduate year and have outstanding academic credentials.
Successful candidates invariably have an interest in pursuing Ph.D.
studies in theoretical physical chemistry in the United States.

STIPENDS: $1300 per month for a 10-12 week period.  Up to $400 in travel
assistance will be provided.

APPLICATION DEADLINE: April 1, 1993


   Send Resume, Academic Transcript and Two Letters of Reference to:

		       	T. Daniel Crawford
	     Center for Computational Quantum Chemistry
	             The University of Georgia
		     Athens, Georgia 30602-2556

Note: Resumes will be accepted via E-mail; transcripts and letters of
reference must be sent via U.S. mail.

For e-mail replys and further information, write to:

           crawdad%sherman.ccqc.uga.edu@athena.cs.uga.edu
Newsgroups: sci.chem
From: gkm@cc.uow.edu.au (Glen K Moore)
Subject: What is in those 'bubbling' lamps?
Summary: I would like o build a large demonstation for a Science Centre
Keywords: lamps
Organization: University Of Wollongong
Date: Tue, 15 Dec 92 13:56:21 GMT

Many years ago lamps could be purchased where a coloured material (pink?)
was heated by a light below causing it to rise as a coloured 'blob' in
a liquid of a different colour. The blob changed shape and eventually sank
to be reheated and rise again.

1. What chemicals are used? (someone suggested glycerine)
2. Has anyone made a large one before?

Glen
gkmcc.uow.edu.au
Science Centre
Wollongong, Australia
Newsgroups: sci.chem,sci.electronics,sci.phys
From: aankrom@nyx.cs.du.edu (Anthony Ankrom)
Subject: All I want for Christmas/Khannuka...
Organization: Nyx, Public Access Unix @ U. of Denver Math/CS dept.
Date: Fri, 18 Dec 92 17:21:45 GMT


 I have recently been studying electrochemistry and I can't for the life
of me, find a decent Platinum electrode. Platinum foil 2.5 x 3.5 cm will 
do...
 (I thought about the p-toluene boronic acid that I needed too, but it
wouldn't fit in an envelope now would it?)

 Happy Holidays, 

St. Anthony, inventor of oat bran...
                    
--
          / N \   O                   Mi vsi smo krizhani,
         |   \ |  || Ph               chlani izbrani
         |   | |_O-C-C-OH             mesarskega ceha...
BZ        \ / /      Ph                            aankrom@nyx.cs.du.edu
From: koehler@secs.ucsc.edu
Newsgroups: sci.chem
Subject: Re: Extraction of THC from alcohol/THC solution
Date: 17 Dec 92 06:08:01 GMT
Reply-To: koehler@secs.ucsc.edu
Organization: UCSC Molecular Engineering Laboratory
NNTP-Posting-Host: moleng.ucsc.edu

MeCl2 and NaCl/H2O would be the scam the average pirate should chose!
Newsgroups: sci.chem
From: nasadk@vccnw05.its.rpi.edu (Kristopher Martin Nasadowski)
Subject: Buckyballs - X-Ray Crystallographic data
Summary: Anyone have C60 X-Ray Crystallographic Data?
Date: Wed, 16 Dec 1992 17:36:04 GMT

I'm interested in finding X-Ray crystallographic data for C 60.
Specifically, the x, y, and z coordinates and the size of the 
unit crystal. A literature search here has yielded nothing 
of value. If anyone could point me to a literature source 
or e-mail me the data, I'd be most appreciative....

Please respond by e-mail

Nazman
<nasadk@rpi.edu>
Newsgroups: sci.chem,rec.pyrotechnics
From: tony2@prefect.cc.bellcore.com (gozdz,antoni s)
Subject: glow sticks - where to get chemicals
Organization: Bellcore, Livingston, NJ
Distribution: world 
Date: Fri, 18 Dec 92 23:27:43 GMT

In article <1992Dec18.192350.1630@muddcs.claremont.edu> sbonds@jarthur.claremont.edu (007) writes:
>
*******************************
>Luminol, while fun, is NOT what is used in commercial lightsticks.  Luminol
>just doesn't last long enough.
>
>All of the material below is taken from a chemical demonstrations book for
>which, unfortunately, I do not have the bibliographic information.  It was
>titled something like "Chemical Demonstrations for Instructors", and was a
>four-volume set.
>
>Anyway, on to the meat of the matter.
>
>The oxidant is hydrogen peroxide contained in a phthalic ester solvent.  The
>concentration is very low, less than 0.5%.  The fluorescing solution consists
>of a phenyl oxalate ester and a fluorescent dye.  The dye used is 9,10-bis-
>(phenylethynyl)anthracene (for green) or 9,10-diphyenylanthracene (for blue).
>
>Here is the reaction sequence:
>
>1)  (Ph)-O-CO-CO-O-(Ph) + H2O2 --> (Ph)-O-CO-CO-O-OH + (Ph)-OH
>
>2)          (Ph)-O-CO-CO-O-OH  -->  O-O
>                                    | |    +  (Ph)-OH
>                                   OC-CO
>
>3)                 C2O4 + Dye  --> Dye* + 2CO2
>
>4)                        Dye* --> Dye + hv
>
>In 1) The hydrogen peroxide oxidizes the phenyl oxalate ester to a peroxyacid
>ester and phenol.  The unstable peroxyacid ester decomposes to the cyclic
>peroxy compound and more phenol in step 2).  The cyclic peroxy compound is
>again unstable and gives off energy to the dye as it decomposes to the very
>stable carbon dioxide.  The dye then radiates this energy as light.
>
>So far as I know the only way to get the dyes needed is to synthesize them
^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^
>yourself.  If anyone knows otherwise, please let me know!
^^^^^^^^^

Good news!

Earlier this year, I bought 
9,10-bis(phenylethynyl)anthracene from Fluka 
(cat. no. 15146).  It's not cheap - $19 for 0.1g.

Its (and 32 other analogs') synthesis and photochemistry
was reported by P. J. Hanhela and D. B. Paul in
Aust. J. Chem. 1984, 37, 553, and
ibid., 1981, 34, pp. 1669, 1687, 1701.
Its fluorescence quantum efficiency was 0.7-0.9!
In addition, the fluorescence wavelength could be
controlled over the range 420-670 nm 
by varying substituents. 

Tony

-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-
Antoni S. Gozdz                tel  (908) 758-2931  |  Bellcore  NVC 3X-261
tony2@prefect.cc.bellcore.com  FAX  (908) 741-2891  |  Red Bank, NJ 07701, USA
                           no .sig, strictly business
-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-
From: mancini@fysik.uu.se (Derrick C. Mancini)
Newsgroups: sci.chem
Subject: Re: composition of "white" gold
Followup-To: sci.chem
Date: 14 Dec 1992 15:21:23 GMT
Organization: Fysikum, Uppsala Universitet
Distribution: world
NNTP-Posting-Host: usx221.fysik.uu.se

In article <1992Dec13.094616.25458@hpcvaac.cv.hp.com>,
billn@hpcvaac.cv.hp.com (bill nelson) wrote:
> 
> giber@pollux.cs.uga.edu (Carolyn Giberson) writes:
> : 
> : White gold is a gold alloy, containing silver and nickel I think.
> 
> Nope. If there is silver in it, it is green gold. I am not sure what
> nickel would do to the gold.
> 
> Bill

Small amounts of nickel made be added for improved strength.  Silver-gold
alloy IS found naturally, it is not white gold (as Bill pointed out).  It
is called electrum and was known to the ancients as such.

(Disclaimer: If I am wrong, I am not surprised!)

Derrick C. Mancini
Fysiska Institutionen  -  Uppsala Universitet
Box 530  S751 21  Uppsala  Sverige
mancini@fysik.uu.se
---------------------------------------------
"Are we having fun yet?"  -  Zippy
From: jctwu@soda.berkeley.edu (Jeffrey Twu)
Newsgroups: sci.chem
Subject: Re: phosphate buffer chemistry
Date: 18 Dec 1992 21:57:46 GMT
Organization: U.C. Berkeley, CS Undergraduate Association
Distribution: na
NNTP-Posting-Host: soda.berkeley.edu
Summary: The final word...
Keywords: phosphate buffer chemistry acid base equilibrium

For all those still following the thread, I've checked with the
originators of the problem and got an official word:  The question was
poorly worded, and when they said you were only allowed those four stock
phosphate solutions, they expected you to know that water was also
permitted.

In addition, "phosphate concentration" did represent _total_ phosphate
concentration, not just free ion concentration.

And I guess:
>Prof. Robert M. Cory, Chemistry Dept, U. Western Ontario, London N6A 5B7 CANADA
>Office (519)679-2111x6339; Home (519)472-8866; FAX (519)661-3022; cory@uwo.ca

... can say, "I told you so!"  (Hmm... I guess I can't expect too much
from Berkeley professors.)

Thanks!

Jeff
-- 
+-Just remember:------------------------------------------------------------+
|	Take it easy.							    |
|		...and don't forget that human touch.	   	            |
+<c60a-gx@danube.berkeley.edu>_________________________________<Jeffrey Twu>+
Newsgroups: sci.chem
From: billn@hpcvaac.cv.hp.com (bill nelson)
Subject: Re: Arsenic Trioxide
Organization: Hewlett-Packard Company, Corvallis, Oregon USA
Date: Sun, 13 Dec 1992 10:22:11 GMT

vxc15931@vax1.mankato.msus.edu writes:
: What are the steps in preparing arsenic trioxide from metallic arsenic?
: The procedures that I know require the extraction of white arsenic (trioxide)
: from lead ore.  Can anyone suggests a more simplified approach?

Nope - that is the procedure. Heat arsenical pyrite ore in oxygen to obtain
crude As2O3. Purify the crude oxide by dissolving in HCl and distilling off
the AsCl3. Remove any residual SbCl3 by shaking the distillate in concentrated
HCl. The dissolve the AsCl3 in boiling H2O - the pure oxide will crystalize
out on cooling.

Or, you might simply purchase it from a chemical supply. It is used as a 
chemical reagent.

LD50 in rats is 138mg/Kg.

Bill
Newsgroups: sci.chem,rec.pyrotechnics
From: sbonds@jarthur.claremont.edu (007)
Subject: Re: Glow Sticks
Keywords: Glow
Organization: Lacking
Date: Fri, 18 Dec 1992 19:23:50 GMT

In article <18DEC199202083549@zeus.tamu.edu> wdb3926@zeus.tamu.edu (BRUTON, WILLIAM DANIEL) writes:
>(carey treesh) writes...
>> .....
>> ...  From what I know about it, the H202 is mixed with some sort of 
>> thing called and "ester oxolate".  The dye is also mixed with some kinda ester
>> I think.  

This is correct.  I never saw the post you said you'd send off, so I thought
I'd explain for all the curious people out there.

I've crossposted to rec.pyrotechnics since this subject often pops up there,
too.

>An earlier post said that luminol and H2O2 are used in some "Glow-Stix".
>I see that Central Scentific has some luminol for about $15/gallon...

Luminol, while fun, is NOT what is used in commercial lightsticks.  Luminol
just doesn't last long enough.

All of the material below is taken from a chemical demonstrations book for
which, unfortunately, I do not have the bibliographic information.  It was
titled something like "Chemical Demonstrations for Instructors", and was a
four-volume set.

Anyway, on to the meat of the matter.

The oxidant is hydrogen peroxide contained in a phthalic ester solvent.  The
concentration is very low, less than 0.5%.  The fluorescing solution consists
of a phenyl oxalate ester and a fluorescent dye.  The dye used is 9,10-bis-
(phenylethynyl)anthracene (for green) or 9,10-diphyenylanthracene (for blue).

Here is the reaction sequence:

1)  (Ph)-O-CO-CO-O-(Ph) + H2O2 --> (Ph)-O-CO-CO-O-OH + (Ph)-OH

2)          (Ph)-O-CO-CO-O-OH  -->  O-O
                                    | |    +  (Ph)-OH
                                   OC-CO

3)                 C2O4 + Dye  --> Dye* + 2CO2

4)                        Dye* --> Dye + hv

In 1) The hydrogen peroxide oxidizes the phenyl oxalate ester to a peroxyacid
ester and phenol.  The unstable peroxyacid ester decomposes to the cyclic
peroxy compound and more phenol in step 2).  The cyclic peroxy compound is
again unstable and gives off energy to the dye as it decomposes to the very
stable carbon dioxide.  The dye then radiates this energy as light.

So far as I know the only way to get the dyes needed is to synthesize them
yourself.  If anyone knows otherwise, please let me know!

  -- 007

-- 
 000   000  7777 | sbonds@jarthur.claremont.edu
0   0 0   0   7  |----------------------------------------------------------- 
0   0 0   0  7   |        Childhood is short...
 000   000   7   |                    ...but immaturity is forever.
From: fparnold@bach.udel.edu (Frederick P Arnold)
Newsgroups: sci.chem
Subject: FORTICON8 EHT program.
Date: 11 Dec 92 19:54:57 GMT
Distribution: sci.chem
Organization: University of Delaware

Hello.  Recently we acquired a copy of the FORTICON8 extended huckel theory 
program, but do not possess any documentation.  Does anybody by perchance have
a manual (or at least a specification of the various options) for this program 
online?  Secondly, we are possibly interested in scattered wave Xa
calculations, and are therefore looking for a program.  If anyone has one 
available, or pointers to one they've used and trust, that information would
be appreciated.

Thank you for your time.  We're trying to get some qualitative work done, being
as the organometallic systems of interest are too big to do by Hartree-Fock 
methods on our VAX.
						-fred
Newsgroups: sci.chem
From: rajat@sunny3.che.clarkson.edu (Rajat Kapoor)
Subject: Re: vanadium dioxide
Organization: Clarkson University
Date: Wed, 16 Dec 1992 16:16:35 GMT

From article <143532@lll-winken.LLNL.GOV>, by cec@imager (Charles Cunningham):
> Does anybody know how to make a single-crystal piece of vanadium dioxide?
> 
> Also, is anybody familiar with some way to get an atomically flat surface
> on VO2?


The closest I came making flat (not atomic) V2O4 platelets was by 
annealing commercial V2O5 crystals at 785 C for 4 days, and washing off
light particles by methanol and drying.  XRD showed very sharp [001]
peak and a weak [002] peaks. The intensity of other planes were
negligible.

Kapoor

 
Newsgroups: sci.chem
From: lc2b+@andrew.cmu.edu (Lawrence Curcio)
Newsgroups: sci.chem
Subject: Re: intro. quant. chem.
Date: 12 Dec 92 05:26:57 GMT
Article-I.D.: andrew.0f_UH1K00WB7QTI49=
Organization: Doctoral student, Urban and Public Affairs, Carnegie Mellon, Pittsburgh, PA

I had an earlier edition of Levine. From my own experience, it's about
as lucid a piece as you're going to find. Levine had a way of planting
ideas in your head - making you think you're the first one to think of
them, and then addressing them in the next chapter :(

The hardest part of QM, though, is the math. I recommend _Applied
Differential Equations_ by Murray R. Spiegel as an extremely simple and
practical reference. Also, _Advanced Calculus_ by Angus Taylor is a calc
book one can crack in the middle and read. I don't recommend either of
these volumes as texts (Spiegel is too simple, and Taylor is too wordy),
but they serve as great quick-and-dirty supplements.

Oh Yes! Use a computer whenever possible, turn your work paper 90
degrees before you start figuring, and buy plenty of pencils.

Good luck!
Newsgroups: sci.chem