HDTenEightyP/NetNews huggingface dataset:
From: jf41+@andrew.cmu.edu (Jonathan R. Ferro)
Newsgroups: sci.chem
Subject: Re: More on moderator
Date: 22 Jul 92 20:51:04 GMT
Organization: Carnegie Mellon, Pittsburgh, PA

The main reason so many people are against modification of existing
groups in general is that they have learned over time two simple facts
about long-term free-form discussions:

1.  Unwanted discussion topics will die of their own accord if enough
    people start talking about something else.

2.  When all is said and done, exhorting people to go elsewhere wastes
    more time and energy than just ignoring them.

It's that simple!  Really!

USENET is not an oligarchy or a democracy.  It is an enlightened
anarchy.  If you want to see it "working" you have to work it yourself.
Requests for "I would like to see a discussion on X" are decidedly
inferior to statements of "Here is what I'm doing with X" in this
environment.

As I posted in sci.astro last month, when meta-discussion on the
appropriateness of certain posts came up:
----------
Remember that this is a newsgroup, not an archive.
The way to interest people in what you are saying is to present it in a
useful and familiar fashion.  On USENET, that means adhering to general
posting standards:
- present your text in ragged-right single-spaced paragraphs, separated
  by blank lines; two spaces after sentence-ending punctuation; etc.
  (Yes, all the things you learned in typing class.)
- don't go over 70-75 columns in width
- try to get rid of trailing whitespace
- DON"T FORGET TO USE LOWER CASE ONCE IN A WHILE
- Your signature does not need to include your resume.  Four lines suffice!
----------

Finally, there's no use in trying to engage _specific_ people in
discussions like these, either by trying to introduce them to computers
in general or to this or that newsgroup or topic specifically.  My
research advisor hasn't read his email in over four years, but I don't
think he's hurting for letting that avenue of communication slide.  :-)

--
Jon Ferro		MIT Transportation Modelling Research Center (TMRC)
jf41+@andrew.cmu.edu	"We can hack it!"
SGNTR VRS VRSN 3.1B: Strppd nd cmprssd fr qckr trnsmssn! nfct yrs tdy!
Newsgroups: sci.chem
From: gchism@magnus.acs.ohio-state.edu (Grady W Chism)
Subject: FTIR for Schiff's base in proteins
Summary:  Help needed
Organization: The Ohio State University
Date: Thu, 30 Jul 1992 02:56:17 GMT

I am interested in the possibility of following Shiff base formation by FTIR. I
would like to do this for a protein solution heated in the presence of glucose.
Has anyone tried to do something similar? I would appreciate advice or 
references.
Thanks.
-- 
Grady W. Chism                     Email:gchism@magnus.acs.ohio-state.edu
Dept. of Food Science and Tech.    Voice:614-292-7719
Ohio State University              FAX:614-292-0218
2121 Fyffe Road, Columbus, OH 43210
Newsgroups: sci.chem
From: lchai@phoenix.Princeton.EDU (Liang Chai)
Subject: Re: Let's have a laugh
Originator: news@ernie.Princeton.EDU
Keywords: N2O
Organization: Princeton University
Date: Thu, 30 Jul 1992 02:02:21 GMT

In article <1992Jul24.070154.22216@alf.uib.no> ttt@cmi.no (Tore Tjomsland) writes:
>Is there anybody out there who knows how to
>make N2O ?
>
>Tore Tjomsland
>e-mail: ttt@cmi.no
>

Put metal (such as Zinc) into HNO3, you can get the gas mixture NO2, NO,
..., and the ratio depends on the concentration of the acid solution. AT
certain range, you can get mainly N2O.

Liang Chai
lchai@phoenix.princeton.edu
From: b_duke@darwin.ntu.edu.au (Brian Duke)
Newsgroups: sci.chem
Subject: Re: More on moderator
Date: 24 Jul 92 14:06:02 +0900

In article <cs_jh.504@cox.nsac.ns.ca>, cs_jh@cox.nsac.ns.ca (JEFF HOYLE) writes:
> Just so everyone knows......
> 
> My posting concerning a moderator was basically shot to pieces.  In all 8 
> people replied either to the newsgroup or to me by email.  All indicated 
> that they would vote AGAINST any form of moderation (no pun 
> intended !!!).  It seems that the discussion that I thought should not be in 
> sci.chem has gone away anyway!!
> 
> The problem that I see with a newsgroup like this one is that it is hard to 
> get chemists who are newbie computer users to access the newsgroup and get 
> involved when they see totally irrelevant discussions going on.  It just 
> seems to scare new users off!!!!  I have tried several times to get 
> colleagues to be involved with the group and this is one of the common 
> comments that I get from them.........

You just have to keep trying. Keep telling them about good discussions.
I sympathise, but moderating is not the answer. There should be more 
posts from chemistry academics and the group should not be left just to
computer ept staff and graduate students.
> 
> Does anyone have any suggestions?  I think that there are alot of good 
> questions being asked that require more input from practicing chemists to 
> help out.....  How do we get these people involved in a meaningful way with 
> out putting them off (as I indicated above).

Try starting lots of fascinating treads yourself.
> 
> One possibility I suppose would be the formation of another newsgroup 
> (sci.chemistry or something similar)

No! No! No!
> 
> I really would like to see this thing working .....
> 

It will. It will.
-- 
                  Brian Salter-Duke (Brian Duke)
School of Chemistry and Earth Sciences, Northern Territory University
        GPO Box 40146, Casuarina, NT 0811, Australia.
Phone 089-466702   FAX 089-410460    E-mail B_DUKE@DARWIN.NTU.EDU.AU
Newsgroups: sci.chem
From: gchism@magnus.acs.ohio-state.edu (Grady W Chism)
Subject: Oxygen monitoring
Organization: The Ohio State University
Date: Thu, 30 Jul 1992 02:53:34 GMT

I need to monitor the oxygen content in a vacuum line.  The stream will also 
have significant amounts of water vapor and volatile esters. Any suggestions?
Apologies for the previous faulty posting.
                               Thanks.
-- 
Grady W. Chism                     Email:gchism@magnus.acs.ohio-state.edu
Dept. of Food Science and Tech.    Voice:614-292-7719
Ohio State University              FAX:614-292-0218
2121 Fyffe Road, Columbus, OH 43210
Newsgroups: sci.chem
From: jb@falstaff.MAE.CWRU.Edu (Jim Berilla)
Subject: Re: Gold + ???
Organization: Case Western Reserve University, Cleveland, Ohio, USA
Distribution: usa
Date: Fri, 24 Jul 92 19:37:59 GMT

In article <1992Jul24.012839.28064@news.Hawaii.Edu>,
mike@uhunix.uhcc.Hawaii.Edu (Mike W. Burger) writes:

[about 15th century refining of gold]

A wonderful book to read about this subject is:

 AUTHOR       Agricola, Georg, 1494-1555.
 TITLE        De re metallica. Translated from the first Latin ed. of 1556,
                with biographical introd., annotations, and appendices upon the
                development of mining methods, metallurgical processes, geology
                , mineralogy & mining law from the earliest times to the 16th
                century, by Herbert Clark Hoover and Lou Henry Hoover.
 EDITION      [New ed.]
 IMPRINT      New York, Dover Publications, 1950.
 DESCRIPT'N   xxxi, 638 p. illus., facsim. 28 cm.
 NOTE         "A complete and unchanged reprint of the translation published by
                the Mining magazine, London, in 1912."
              Bibliography: p. 599-606.

The extraction process wasn't perfect.  I remember that some silver objects
from (supposedly) the 15th century were judged to be forgeries because the
silver lacked the impurities (gold and lead) which would have been present
if the silver had been refined with 15th century technology.
-- 
      Jim Berilla / jb@falstaff.MAE.cwru.edu / +1 216 368 6776
Newsgroups: sci.chem
From: billn@hpcvaac.cv.hp.com (bill nelson)
Subject: Re: Precipitating Aluminum out of Solution
Organization: Hewlett-Packard Company, Corvallis, Oregon USA
Date: Fri, 31 Jul 1992 06:43:15 GMT

knapp@spot.Colorado.EDU (David Knapp) writes:
: >
: >I would guess you need to do something like heating up an Aluminum
: >compound (Al2O3 or AlCl3, etc) until molten and then introducing a
: >more reactive metal (sodium, magnesium, potassium, etc), all in an
: >inert atmosphere of some sort. This should precipitate out Aluminum.
: 
: 
: Aluminum *can* be precipitated out of an aqueous soln in the form of a 'lake'.
: You can see it (Al(OH)3) by adding an organic dye like aluminon. This can
: be centrifuged and dried, but would  probably need to be heated in a hydrogen
: furnace to get back to metallic Al.

That is the point. It would not be so difficult to precipitate some aluminum
compound. The problem is precipitating pure aluminum.

Bill
From: benjamin@munch.mmwb.ucsf.edu (Dennis Benjamin)
Newsgroups: sci.chem
Subject: Re: Problems with NICOLET spectrometer
Date: 23 Jul 92 15:53:03 GMT
Organization: UCSF Computer Graphics Lab

Whoops! having re-read the original article, it should be no problem
finding a kermit for an IBM PC, just use archie and look for a
directory named DOS or IBM
Newsgroups: sci.chem,sci.bio,sci.engr,soc.college,soc.college.grad
Newsgroups: sci.chem
Subject: Re p32 -> gammas
From: news@massey.ac.nz (USENET News System)
Date: Wed, 29 Jul 92 04:48:11 GMT
Organization: DSIR, Palmerston North, New Zealand


be wary of the 'plexiglass' shields. SOME have fairly high quantities of lead
incorporated into them and this (so i've been told) is the source of the 
problem. For most of the commonly used (in bio tracers anyway) isotopes, no
problem - but apparently the energy of the 32P is about right to produce the
xrays (?) mentioned from the Pb.

Comments ??? Is this True ?

	Bruce



Xref: sparky sci.chem:2715 comp.graphics:7998 comp.graphics.visualization:1139 bionet.neuroscience:352 bionet.xtallography:53 alt.graphics:303 alt.drugs:13268 alt.psychoactives:1026 sci.bio:2710 sci.med:14183 comp.org.eff.talk:4727 soc.college.grad:1611
From: carl@aoa.aoa.utc.com (Carl Witthoft)
Newsgroups: sci.chem,comp.graphics,comp.graphics.visualization,bionet.neuroscience,bionet.xtallography,alt.graphics,alt.drugs,alt.psychoactives,sci.bio,sci.med,comp.org.eff.talk,soc.college.grad
Subject: Re: CENSORED by SIGGRAPH: ( Xochi Speaks ) Psychedelic Educational Media
Keywords: Psychedelics
Date: 21 Jul 92 15:10:15 GMT
Organization: Adaptive Optics Associates

x
Nice try for the alltime crossposting record.
What a pile of useless dribble (or is that drivel).
Go away. Now. 
Thanks

-- 
Bobby Newmark, aka  Carl Witthoft @ Adaptive Optics Associates
aoa!carl@bbn.com  carl@aoa.utc.com
54 CambridgePark Drive, Cambridge,MA 02140 617-864-0201
**Just say NO to HMOs**
From: jf41+@andrew.cmu.edu (Jonathan R. Ferro)
Newsgroups: sci.chem
Subject: Re: moderator how is one appointed?
Date: 21 Jul 92 14:06:22 GMT
Article-I.D.: andrew.MeP8dSi00hYzQif0sg
Organization: Carnegie Mellon, Pittsburgh, PA

cs_jh@cox.nsac.ns.ca (JEFF HOYLE) writes:
> How does one go about seeking a moderator for a group?

The FAQ file "How to Create a New Newsgroup" has just been posted in
news.groups.  The file does state that the guidelines are "NOT intended
as guidelines for setting USENET policy other than group creations", but
so many people have gotten used to the procedure that it will be
unlikely that any other procedure can be agreed upon.

Note that there are three major factors working against consideration of
this change already:

1) Someone is going to have to agree to be the moderator of this group.
This is usually the hardest part of starting a moderated group.

2) Discussion of heirarchy changes tends to drown out real news.  If a
RFD is posted here you can expect to not see any continuing chemistry
discussion for 2-5 months.

3) Me.  I'm voting NO right now, and I don't expect my opinion to
change.  The value of the quick response time of a live newsgroup
outweighs the small inconvenience of having to skip over articles that I
am not interested in.

--
Jon Ferro		MIT Transportation Modelling Research Center (TMRC)
jf41+@andrew.cmu.edu	"We can hack it!"
SGNTR VRS VRSN 3.1B: Strppd nd cmprssd fr qckr trnsmssn! nfct yrs tdy!
From: mgray1@metz.une.edu.au (Matthew GRAY)
Newsgroups: sci.chem
Subject: Schiff base synth.
Date: 30 Jul 92 09:34:06 GMT


I've been trying to make some analogous Schiff bases ( ketimines, imines, azomethines) of the form HO-C6H4-N=C-R(R'), either m- or p- on the phenol ring.
I have a prep for HOC6H4-N=C(Me)2, made by disolving p-aminophenol (p-hydroxyaniline) in acetone, and leaving in the fridge for a few days (also works with m-).
I've tried this with other ketones such as Et2C=O, Me(Pr)C=O, Me(Bu)C=O, as well as under more forcing conditions eg refluxing Me(Ph)C=O (~200 degrees) with conc H2SO4. Nothing in between seems to work either. 
Can anybody help me?
				Matthew Gray
				University of New England
				mgray1@metz.une.oz.au
From: berry@a.chem.upenn.edu (Don Berry)
Newsgroups: sci.chem
Subject: Re: Precipitating Aluminum out of Solution
Date: 22 Jul 92 18:26:17 GMT
Organization: University of Pennsylvania

In article <1992Jul22.172939.18139@ccu.umanitoba.ca>, cweiss@ccu.umanitoba.ca (christopher gene weiss) writes:
> 
> I've been looking for ways to precipitate reasonably fine aluminum metal
> out of a simple solution. I've considered dissolving aluminum metal in strong
> acid and then trying some sort of redox to precipitate it but I can't think
> of a decent reaction. Can anybody help me on this? Thanks.

   Your problem is essentially the same problem which delayed the
industrial scale use of aluminum for so long - Aluminum is a very
reactive, electropositive metal, and attempts to reduce Al salts in
most solutions instead lead to reduction of the solvent (i.e. you
get electrolysis of water.)  This may be more obvious if you extend
the problem and consider attempting to produce sodium metal by reducing
an aqueous NaCl solution.

   Incidentally, electrolysis of Al was originally performed in
molten NaAlCl4, but the big breakthrough was the use of molten
"Cryolite" (Na3AlF6) as solvent (it melts at "only" ca. 1000 deg C).

    Sorry, but generation of fine Al metal from a "simple" solution
doesn't seem likely.

Don Berry

Xref: sparky sci.chem:2735 sci.bio:2726 sci.engr:1848 soc.college:3463 soc.college.grad:1613
Newsgroups: sci.chem,sci.bio,sci.engr,soc.college,soc.college.grad
Subject: Re: Getting a PhD without being a grad student
From: A.S.Chamove@massey.ac.nz (A.S. Chamove)
Date: Thu, 23 Jul 92 00:55:06 GMT
Organization: Massey University, Palmerston North, New Zealand
X-Reader: NETNEWS/PC Version 2c

Several universities in the UK and in NZ will award PhDs solely on
the basis of a portfolio of published work plus an oral exam on that
work (to show that you really understand it).  It is NOT restricted
to staff at the university and anyone can apply for such a thing. The
reason is that PhDs in the UK are certificates of competence to do
research. 
The critical thing is to have a coherent body of work--say 5 papers
on development of the same topic. You will also have to find a
supervisor who will agree to be supervison, and that is someone with
an interest in the area. That should be no problem. 
My PhD was such a creature:
Chapter 1:Response to novel objects by monkeys of different dominance ranks.
Chapter 2:Monkeys entering groups at different dominance ranks.
Chapter 3:Monkeys changing dominance ranks.
chapter 4:Expression of dominance in darkness.
Chapter 5:A new behavioural recording system.
Chapter 6:Dominance history and learned levels of aggression.


-- 
-----------------------------------------------------------------
Arnold Chamove
Massey University Psychology
Palmerston North, New Zealand
From: dernis@binah.cc.brandeis.edu
Subject: Re: conductivity units
Reply-To: dernis@binah.cc.brandeis.edu
Organization: Brandeis University
Date: Thu, 23 Jul 1992 19:31:03 GMT

Siemens and Ohms are inverses of each other.  Thus your current units are
really Siemens per centimeter.   If you would like just Siemens you need
more information, namely, the length of material whose conductivity is
in question.  Just multiply by the length expressed in cm.

You may also come across Ohm -1 Cm-2, for membranes and other two dimensional\
conductors.  In that case multiply by the area.  

I hope this helped.

Mitchell Dernis
From: cfthb@ux1.cts.eiu.edu (Howard Black)
Newsgroups: sci.chem
Subject: Re: Schiff base synth.
Date: 31 Jul 92 15:23:56 GMT
Article-I.D.: ux1.1992Jul31.152356.13012
Organization: Eastern Illinois University

In article <1524@grivel.une.edu.au> mgray1@metz.une.edu.au (Matthew GRAY) writes:
>
>I've been trying to make some analogous Schiff bases ( ketimines, imines, azomethines) of the form HO-C6H4-N=C-R(R'), either m- or p- on the phenol ring.
>I have a prep for HOC6H4-N=C(Me)2, made by disolving p-aminophenol (p-hydroxyaniline) in acetone, and leaving in the fridge for a few days (also works with m-).
>I've tried this with other ketones such as Et2C=O, Me(Pr)C=O, Me(Bu)C=O, as well as under more forcing conditions eg refluxing Me(Ph)C=O (~200 degrees) with conc H2SO4. Nothing in between seems to work either. 
>Can anybody help me?
>				Matthew Gray
>				University of New England
>				mgray1@metz.une.oz.au
>

    You don't say whether you successfully performed the reaction with
acetone, just that you tried the prep with other ketones.  I usually advise
my students to try to reproduce literature reactions before attempting to
extend them to untested substrates.

    In any case, problems with Schiff base formation usually arise from
unfavorable equilibria, that is, the water produced causes hydrolysis of
the imine back to the starting materials.  You might try molecular sieves,
a Dean-Stark trap (for higher-boiling ketones), etc.


-- 
   ******************************************************************
     Howard Black                             cfthb@ux1.cts.eiu.edu
     Department of Chemistry                  Eastern Illinois Univ. 
Newsgroups: sci.chem
From: tnfisher@nyx.cs.du.edu (tim fisher)
Subject: Removing water of hydration from fluorotitanate ??
Organization: Nyx, Public Access Unix @ U. of Denver Math/CS dept.
Date: Wed, 29 Jul 92 14:27:57 GMT

I am preparing a fluorotitante compound, calcium hexafluorotitanate,
CaTiF6 which will be reduced with Ca metal to produce Ti metal and CaF2
slag byproduct. We react TiO2 (anatase) with 48 pct HF acid (very
exothermic reaction) to make a TiF4 in solution, then precipitate the 
CaTiF6 by adding CaCO3 calcium carbonate to the solution. We then filter
the product and dry it initially at 100 degrees celcius, then for 3 days
at 195 degree celcius.

Thge initial fluorotitante produced (before drying) is a fully hydrated
CaTiF6 * 2H2O . After drying, we can only get down to a oxygen content of
about 0.8 wt pct. We have tried drying in inert atmosphere, various
temperatures, and have dried the powder under flowing HF gas at elevated
temperatures. Any oxygen in the calcium fluorotitanate powder will
contaminate the Ti metal produced.

Does anyone have any suggestions to remove the remaining water of
hydration?

Please post or e-Mail me at gfisher@alrc.usbm-ccn.gov . 

Thanks in Advance

Tim Fisher  US Bureau of Mines
                  Albany Research Center
                  Albany, Oregon
ph. 503-967-5854
internet: gfisher@alrc.usbm-ccn.gov












































Newsgroups: sci.chem
From: lchai@phoenix.Princeton.EDU (Liang Chai)
Subject: Re: silver oxidation
Originator: news@ernie.Princeton.EDU
Organization: Princeton University
Date: Sun, 26 Jul 1992 00:29:34 GMT

In article <posakony.711583503@unixg.ubc.ca> posakony@unixg.ubc.ca (Jeffrey Posakony) writes:
>
>A friend of mine recently posed this question to me.  Since I was unable to 
>answer it, I told him I'd put it to the net.  So here goes.  My friend wears 
>a chain with a Sterling silver pendant around his neck.  The pendant turns
>black over a short period of time (presumably a silver oxide coating).  This
>did not occur when he was living in Hong Kong, but only began after he came
>to Vancouver, British Columbia in Canada.  What might be the source of 
>the 'selective' oxidation?  It seems odd to me that the
>same thing did not occur in Hong Kong, since Hong Kong, according to him,
>has much more air pollution.  Vancouver lies next to the waters of the
>Pacific Ocean and is less humid than Hong Kong, if that helps any.  Might
>it even be something related to the change of food?   
>
>I would appreciate any ideas that anyone might have.  Please send all 
>responses directly to:   posakony@unixg.ubc.ca  


It looks to me that it might be silver sulfid (Ag2S). I cannot figure
out 
where the sulfer comes from and this is only for your information. It may
be wrong.

Liang Chai
lchai@phoenix.princeton.edu
From: pk03+@andrew.cmu.edu (Paul Karol)
Newsgroups: sci.chem
Subject: Re: Re p32 -> gammas
Date: 29 Jul 92 06:39:17 GMT
Article-I.D.: andrew.geReqJO00WBKE24ltS
Organization: Carnegie Mellon, Pittsburgh, PA

Concerning Pb x-rays from P-32 betas in plexiglass...

First, I'm surprised to hear that plexiglass has Pb.  Is it beyond the
trace level?  If not, its presence won't be too influential.

Second, again I point out that the average energy lost by the beta per
interaction is 32 eV.  The Pb x-rays that would be of concern are the
result of removing inner electrons, from the K or L shells, which
requires (very roughly) 80,000 and 10,000 eV respectively.  The valence
shell electrons are bound by only 7-20 eV and the resulting x-rays would
be 'soft' and much more prevalent.

Paul J. Karol
Nuclear Chemist
Newsgroups: sci.chem
From: sjpitts@leland.Stanford.EDU (steven pitts)
Subject: Re: Making Pickles Glow
Organization: DSG, Stanford University, CA 94305, USA
Date: Wed, 22 Jul 92 16:00:19 GMT

In article <1992Jul22.041111.18839@samba.oit.unc.edu> Alan.Tai@bbs.oit.unc.edu (Alan Tai) writes:
>Well, this morning, to I ran the experiment, passing 18 volts through
>a dill, turned out lights...and saw nothing unusual besides the usual
>sparks between the contacts and the pickle.  The pickle was about as
>dull as the counter it was on.

As I recall from a brief note about this last fall in Chemical and
Engineering News, the "electric pickle" trick is usually done with 110 V
AC current which offers a possibile explanation of why you didn't see
the effect.  As to the origin of the orange glow, I believe it is
thought to be sodium D-line emission.  I seem to recall that the
electric pickle is a favorite of Mr. Wizard (Frank Herbert) and has
caught the attention of Professor Shakashiri (sp?) of the University of
Wisconsin Department of Chemistry.  

If anyone can offer a good explanation as to the origin of sodium D-line
emission from the pickle, I'd be happy to hear it.  I seem to recall
someone hypothesizing gas pockets forming inside the pickle in which
neutral sodium vapor may exist from reduction of sodium cation which
certainly abounds in a dill pickle.

I think the "electric pickle" might offer an amusing alternative to a
gas discharge lamp as a light source for demonstrating discrete spectral
lines in the classroom.

Steve Pitts
Graduate Student
Department of Chemistry
Stanford University
From: eddie@csa2.lbl.gov (EDWARD J MOLER)
Newsgroups: sci.chem
Subject: Re: Making Pickles Glow
Date: 23 Jul 92 01:58:54 GMT
Organization: Lawrence Berkeley Laboratory - Berkeley, CA, USA
Distribution: world
Reply-To: eddie@csa2.lbl.gov
NNTP-Posting-Host: 128.3.254.197
News-Software: VAX/VMS VNEWS 1.3-4   

In article <1992Jul22.041111.18839@samba.oit.unc.edu>, Alan.Tai@bbs.oit.unc.edu (Alan Tai) writes...
>Someone recently posted that running a current through a pickle made
..
>    Has anyone else tried this?  Is this glowing bit for real?  If so,
>what could I be doing wrong?  This could be a great addition to our
>magic show :-).  Thanx.
> 
>           internet:  bbs.oit.unc.edu or 152.2.22.80


	Yes, I've done it with 110 AC wall current.  The pickle glows
yellow from the classic sodium D-lines.  As to the actual excitation
mechanism....

						Eddie Moler
						EJMOLER@LBL.GOV
From: hayesgb@wkuvx1.bitnet
Newsgroups: sci.chem
Subject: Metalation of Aryl Systems
Date: 23 Jul 92 12:23:36 CDT
Organization: Western Kentucky University, Bowling Green, KY

I am searching for information on procedures for metalating mono, and
disubstituted aryl ring systems.  Any information that anyone has would be
greatly appreciated.