HDTenEightyP/NetNews huggingface dataset:
From: tyadav@athena.mit.edu (Tapesh Yadav)
Subject: Re: "White" Carbon?  O4?
Organization: Massachusetts Institute of Technology
Date: Thu, 13 Aug 1992 16:08:50 GMT

===================================
 moroney@ramblr.enet.dec.com writes:
>The CRC Handbook, in their section on the elements describes an allotrope of
>carbon as "white" carbon, in addition to diamond and graphite allotropes. They
>devote a couple sentences to it and state that not much is known about it.
>Does this have anything to do with 'buckyballs'? They do not mention them, 
>in the latest edition.  Does anyone know anything about 'white' carbon beyond
>what's listed in the CRC?
>
>-Mike

 The latest issue of Phys Rev Lett, (Vol 69, No 3) carries a paper
 by Moshary et al. on something similar to this.
 
	C60 collapses to a new phase (transparent) of carbon at about 20 GPa.

 Earlier this year, Nature carried an article from france about
 C60 to diamond conversion at room temp + hi pres.

 I am unaware of any other C60 transform, yet.

T.Y.
----
tyadav@athena.mit.edu
From: forrest@cup.portal.com (Forrest H Bennett)
Newsgroups: sci.chem
Subject: Re: "White" Carbon?  O4?
Date: Thu, 13 Aug 92 12:39:22 PDT
Organization: The Portal System (TM)
Distribution: usa

>The CRC Handbook, in their section on the elements describes an allotrope of
>carbon as "white" carbon, in addition to diamond and graphite allotropes. The
>devote a couple sentences to it and state that not much is known about it.
>Does this have anything to do with 'buckyballs'? They do not mention them, ev
>in the latest edition.  Does anyone know anything about 'white' carbon beyond
>what's listed in the CRC?
 
To my knowledge there are 6 crystalline allotrops of Carbon: 
alph-graphite, beta-graphite, diamond, Lonsdaleite (also called 
hexagonal diamond), chaoite, and carbon-VI. I suppose that you 
could also count the Fullerenes C60, C70, C240, etc. Chaoite is 
white; I have a few numbers on it, what do you need?
       
Forrest
Newsgroups: sci.chem
From: vsummers@polaris.cv.nrao.edu (Vince Summers)
Subject: Re: the TRUTH about Methylene Chloride
Organization: National Radio Astronomy Observatory
	<1992Aug18.205552.16112@leland.Stanford.EDU>
Date: Wed, 19 Aug 1992 13:11:05 GMT

     No need for the (sic)----affect is the correct spelling.

Vince Summers
vsummers@polaris.cv.nrao.edu
From: dsmith@uoft02.utoledo.edu
Newsgroups: sci.chem
Subject: the TRUTH about Methylene Chloride
Date: 17 Aug 92 20:03:37 EST
Organization: University of Toledo, Computer Services

If they will forgive me, the following is taken from the Merck Index, 10th
Edition, page 869, item 5936, Methylene Chloride:

	Human Toxicity:  Narcotic in high concns.
	Use:  Solvent for cellulose acetate; degreasing and cleaning fluids,
	      as solvent in food processing.
	Therap Cat:  Pharmaceutical aid (solvent)

So, if all of you chemophobes and rumormongers don't mind - DON'T GO TALKING
ABOUT SOMETHING UNTIL YOU CHECK YOUR FACTS.  Obviously, as with any chemical
(which means any matter in the universe) too much is bad for you.  (Even
too much oxygen can hurt or kill you in the right circumstances.  Just ask
a scuba diver.)

I don't mind concern by uninformed or lay persons, or even those who think
they might know but aren't sure.  The worst enemy we have is ignorance.
But when chemists start passing bad information, that hurts everyone.  I
don't pretend to know everything, and I would not have put my two cents in,
but this subject was starting to get out of hand.  As a chemist and teacher,
I feel that the only way people and society will advance will be to take the
mystery out of (IMHO) simple sciences such as chemistry, since everything
is chemistry.

Doug Smith, Ph.D.
Assistant Professor of Chemistry
The University of Toledo

"The technology of a sufficiently advanced civilization is indistinguishable
from magic."
Newsgroups: sci.chem
From: LJ10717@LMSC5.IS.LMSC.LOCKHEED.COM
Subject: Synonym in Question?
Organization: Lockheed Missiles & Space Company, Inc.
Date: Wed, 12 Aug 92 21:33:01 GMT


Hi Sci.chem Netters,

I have a history question dealing with the material Silver Nitrate.  Does
anyone know why the synonym for this material is "Lunar Caustic"?

If so, please give enough detail for the basis of this chosen name for AgNO3.

Thanks in advance.

Note: In case anyone is wondering, a wager is pending in our orgn. for the one
who can yield enough information on this matter.

------------------------------------------------------------------------------
Diamond - lj10717@lmsc5.is.lmsc.lockheed.com      "After all, diamonds are a
                                                   girl's best friend!"
                                                     -MM
------------------------------------------------------------------------------



Newsgroups: sci.chem
From: vasisn@vccsouth30.its.rpi.edu (Niraj Vasishtha)
Subject: dissolution of PET and Nylons
Reply-To: vasisn@rpi.edu
Organization: Rensselaer Polytechnic Institute, Troy, NY.
Date: Fri, 21 Aug 1992 15:18:31 GMT


	I'm lokking for a solvent or a combination of two compatible solvents for the dissolution of PET, nylon -6 and -66. 
	would any shed some light on it. 


niraj vasishtha
vasisn@rpi.edu
From: aproden@ac.dal.ca (Andrew P. Rodenhiser)
Newsgroups: sci.chem
Subject: Re: airbags how do they work? Chemistry??
Date: 19 Aug 92 18:41:48 GMT
Organization: Dalhousie University, Halifax, Nova Scotia, Canada

In article <15AUG199212012653@juliet.caltech.edu>, natefrei@juliet.caltech.edu (Frei, Nathan A.) writes:
> In article <1992Aug14.201208.14279@engage.pko.dec.com>, moroney@ramblr.enet.dec.com writes...
>>In article <cs_jh.555@cox.nsac.ns.ca>, cs_jh@cox.nsac.ns.ca (JEFF HOYLE) writes...
>>>Some time ago I posted a request for info concerning the chemistry involved 
>>>in air bag inflation.  I did not get any useful responses.  Is there any one 
>>>out there who either knows and can explain the process or who has a leading 
>>>reference to this subject.
>> 
>>I believe they use sodium azide, which explodes producing a sudden large
>>volume of nitrogen gas.
>> 
>>Sodium Azide is NaN .
>>                   3
>>-Mike
> 
> That sounds right.  Incidentally, the rxn is highly exothermic (only logical,
> considering that it produces tens of liters of gas in milliseconds), meaning
> that a people suffer second or third degree burns from airbags.  Auto
> manufacturers (and most folks tend to agree) that this is a reasonable
> price for an increased survival rate.
> 
> If you want more info, why not write to the automakers?  I worked for GM for
> a summer, and they were only too eager too tell everybody about their airbags,
> since theirs are supposedly the coolest (they are only about 180 degrees C).
> 
> Nathan Frei
> 

All of this sounds perfectly correct to me as well.  Another suggestion is
to post to rec.autos.tech where I'm sure someone, maybe even a GM engineer
will have an answer.

P.S. Hi, Jeff.  I mentioned our previous conversation to Dr Kwak and he
most certainly did remember you.  He was also happy to see me discussing 
something useful on this net, as opposed to playing around! :)
Cheers,
-- 
~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~
Andrew Paul Rodenhiser   |  You are the only censor.
Department of Chemistry  |  If you don't like what I'm saying,
Dalhousie University     |  you have the choice.
Halifax, N.S. Canada     |  You can turn me off!
APRODEN@ac.dal.ca        |   --Alice Cooper, Lay Down & Die, Goodbye.
~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~
Newsgroups: sci.chem
From: kgraff@csd4.csd.uwm.edu (Kathy A Graff)
Subject: wi.forsale milw.general
Originator: kgraff@csd4.csd.uwm.edu
Organization: Computing Services Division, University of Wisconsin - Milwaukee
Distribution: wi
Date: Mon, 17 Aug 1992 12:27:34 GMT


Free to a good home:

     Back issues of Analytical Chemistry

Fill out your collection or begin a new one!

This is the American Chemical Society publication which costs $8 each
for single back issues if you order from them.

They are yours for free if you can pick them up. If you are outside the
Milwaukee area, I can send them if you pre-pay shipping. I am moving and
need the space. Issues go back to 1977.

Kathy Graff
kgraff@csd4.csd.wum.edu
Phone: 229-4661, 649-3016, or 332-0546 (evenings)
From: fritz@hpfcbig.sde.hp.com (Gary Fritz (tmp))
Newsgroups: sci.chem
Subject: Common ingredients info
Date: 19 Aug 92 18:31:08 GMT
Article-I.D.: fc.Bt8u3x.CDx
Reply-To: Gary Fritz <fritz@hpfcbig.sde.hp.com>
Organization: HP SESD, Fort Collins, CO
X-Newsreader: Tin 1.1scd1 PL4

Hi all,

I'm not a regular in this group, but I suspected you folks might be the
best source for some information.  Thanks in advance for any pointers.

I'd like to do some research on the ingredients commonly found in products
everybody uses all the time, like shampoos, soaps, lotions, etc.  I've heard
enough rumors of nasty effects of sodium lauryl sulfate and similar common
ingredients that I'd like to do some looking on my own.

Only problem is, where to look?  The only sources I've found so far are,
shall we say, biased.  I'd appreciate pointers to any reference books
or other good sources that list all these sorts of ingredients and explain
what they do, what they're good for, and what dangers/hazards they carry
in language understandable to an intelligent but non-chemist person.

Thanks!
Gary
Newsgroups: sci.chem
From: houze@bach.udel.edu (Jonathan Bric Houze)
Subject: Re: Methylene Chloride
Organization: University of Delaware
Date: Wed, 19 Aug 1992 01:02:03 GMT

In article <1992Aug18.221806.3774@ucsu.Colorado.EDU> saastad@spot.Colorado.EDU (SAASTAD OLE) writes:
>
>The CH2Cl2 is in so low concentrations that it will be soluble in water.
>The solubility should be in the ppm range, maybe as low as ppb. It will 
>acumulate in fat, fish, birds, etc. In air it is broken down by reaction
>with atmospheric OH radical. It does not destroy ozone.
>
>-- 
>Ole W Saastad  
I can assure you that methylene chloride is much more soluble in water
than you suggest (ppm, ppb). At the lab I work at, there has been much
grief due to the fact that methylene chloride has been getting into the
waste water in the hundreds of ppm (maybe even thousands of ppm, but at
that point, it is easier to talk percentages). The volatility of methylene
chloride is so great that dry ice traps have to be installed on the
water aspirator vacuum lines. This condenses the methylene chloride
before it gets to the water and sends discharge levels even higher. 

Also, in the turbulent environment in ocean surf, it is possible that
the methylene chloride could be churned into an emulsion. I have long
and grievous experience with methylene chloride forming emulsions
when trying to use it as an extraction solvent.

Finally, as noted in previous posts, methylene chloride is metabolised
in the body, so it probably wouldn't accumulate to any appreciable
degree up the food chain.

						Jonathan Houze 
						houze@bach.udel.edu
From: Ligon@macgw1.ge.com (Woody Ligon)
Newsgroups: sci.chem
Subject: Re: Methylene Chloride
Date: 19 Aug 92 14:02:57 GMT
Distribution: usa
Organization: GE-CRD

In article <1992Aug18.221806.3774@ucsu.Colorado.EDU>, saastad@spot.Colorado.EDU (SAASTAD OLE) writes:
> 
 The solubility should be in the ppm range, maybe as low as ppb. It will 
> acumulate in fat, fish, birds, etc. In air it is broken down by reaction
> with atmospheric OH radical. It does not destroy ozone.
> 
> -- 
> Ole W Saastad  
> Dept. of Chemistry University of Oslo Norway.
> Now at University of Colorado at Boulder / CIRES ,  Atmospheric Chemistry.
> 
> 

Anyone who has done a liquid/liquid extraction with CH2Cl2/H2O should realize
 that this material is remarkably soluble in water.  I don't have the number 
handy but the chem rubber handbook gives it a "partially soluble). Partially 
soluble usually means low percent levels-- not ppm.

Also I don't think it accumulates. Instead it is metabolized rather quickly. 
The product, however, (at least in humans) is carbon monoxide if I remember 
correctly.  This is the reason people are strongly cautioned not to use CH2Cl2 b
based paint strippers without adequate ventilation. 

Woody Ligon   
Standard Disclaimer applies.



Woody Ligon   Standard Disclaimer applies.
From: graham@latrobe.edu.au (Graham Vincent)
Newsgroups: sci.chem
Subject: zeolites
Date: 18 Aug 92 02:01:32 GMT
Organization: La Trobe University, Victoria, Australia


Hi There Netters,
		Does anyone out there know of any storys behind the 
story of the development of zeolites as catalysts. e.g any serendipity that
occured in the lab, accidents that lead to breakthroughs, good quotes
by the developers e.t.c. The information is to brighten up an
essay on usefull compounds of silicon.

	If there is an interest in the responses I will post a summary.

Thanks in advance, 
			Graham.

-- 
__________________________________________________
			|
Graham Vincent		|  It doesn't matter if
La Trobe University,	| it is acuurate or not;
Bundoora, 3083,		|
VIC,			|  Just as long as it 
Australia.		|   looks pretty.           
graham@nmriris.latrobe  |
	.edu.au		|
________________________|__________________________
From: mssmith@afterlife.ncsc.mil (M. Scott Smith)
Newsgroups: sci.chem
Subject: Mystery Pizza Ingredient
Date: 20 Aug 92 21:30:27 GMT
Organization: The Great Beyond


To all:

I recently wrote an article asking about a "mystery" preservative I saw
on the packaging of some frozen pizza.  I received several responses, and
I'm grateful for the information:

--------------------------------

>Calcium propionate is the calcium salt of propionic acid. (or to be IUPAC
>about it, propanoic acid). Its formula is Ca(C H O ) .
>                                              3 5 2 2
>
>
>                        Ca(O C-CH -CH )     might give you a better idea
>                            2    2   3 2     what it looks like.
>
> As to why the name was fearured on the package so prominently,
> I have no idea. . . .
>
>                                                Jonathan Houze
>                                                houze@bach.udel.edu

--------------------------------

> Hi,
>    Calcium proprionate is the calcium salt of a naturally-occuring
> carboxylic acid.  It is found in foods like Swiss cheese.  It inhibits
> the formation of molds -- a good thing, since mycotoxins can be
> *very* nasty.  So, although preservatives like this don't sound very
> tasty, perhaps having them there in low levels is better than the
> alternative (which might be food poisoning!).
>
> Hope this helps,
>
> Carolyn Giberson
> giber@pollux.cs.uga.edu
> University of Georgia

--------------------------------

> Hi. If you want to read a nifty book about food additives and a million other
> things get hold of Ben Selinger's Chemistry in the Marketplace-A Consumer
> Guide, 4th Edn. Harcourt Brace Jovanovich, 1989. It may not mention calcium
> propionate explicitly but it will point you in the direction of a few
> good references.
>
> Andrea Sella
> UCL Chemistry
> aka ucca245@ucl.ac.uk

--------------------------------

So, that about wraps it up.  I can now live a little easier eating the pizza,
although I frankly like Pizza Hut better anyway.  :)  Thanks again for the
replies!

M. Scott Smith
--| mssmith@afterlife.ncsc.mil
  | umsmith@mcs.drexel.edu
Newsgroups: sci.chem
From: natefrei@juliet.caltech.edu (Frei, Nathan A.)
Subject: Re: Common ingredients info
News-Software: VAX/VMS VNEWS 1.41    
Organization: California Institute of Technology
Date: Thu, 20 Aug 1992 03:51:00 GMT

In article <Bt8u3x.CDx@fc.sde.hp.com>, Gary Fritz <fritz@hpfcbig.sde.hp.com> writes...
>Hi all,
> 
>I'm not a regular in this group, but I suspected you folks might be the
>best source for some information.  Thanks in advance for any pointers.
> 
>I'd like to do some research on the ingredients commonly found in products
>everybody uses all the time, like shampoos, soaps, lotions, etc.  I've heard
>enough rumors of nasty effects of sodium lauryl sulfate and similar common
>ingredients that I'd like to do some looking on my own.
> 
>Only problem is, where to look?  The only sources I've found so far are,
>shall we say, biased.  I'd appreciate pointers to any reference books
>or other good sources that list all these sorts of ingredients and explain
>what they do, what they're good for, and what dangers/hazards they carry
>in language understandable to an intelligent but non-chemist person.
> 
>Thanks!
>Gary

For a reasonably brief and intelligible description, look in _The New York 
Public Library Desk Reference_.  A better idea, though, would probably be to
get _The Merck Index_, or some such reference, and find a chemist to interpret,
since most non-scientist's books on the subject that I've seen are biased
one way or another (the reason for their publication was usually to "expose"
something or other, or to point out all the "lies" perpetrarted by someone
else).

Nate

Newsgroups: sci.chem
From: vsummers@polaris.cv.nrao.edu (Vince Summers)
Subject: An Interesting Question
Organization: National Radio Astronomy Observatory
Distribution: sci.chem
Date: Fri, 21 Aug 1992 18:18:04 GMT

     Despite the controversy concerning creation and evolution on other
postings, an interesting question arises that can be discussed without
bringing up these other side issues.
     You PHYSICAL CHEMISTS out there---no----maybe you DOCTORS of 
physical chemistry---to what extent can the earth be considered its
own universe for entropy considerations?  Must it be considered as an
integral part of the universe, or can it be a good at least first order
approximation of a separate universe as far as entropy is concerned?

Vince Summers,organic chemist

vsummers@polaris.cv.nrao.edu
Newsgroups: sci.chem
From: robin@ruchem.ru.ac.za
Newsgroups: sci.chem
Subject: supercritical water
Date: 21 Aug 92 08:23:22 GMT
Article-I.D.: hippo.1992Aug21.082153.25406
Reply-To: robin@ruchem.ru.ac.za
Organization: Rhodes University, Grahamstown, SA

Hi chempeople! Anyone interested in reactions in supercritical H2O?
T>375C,P>220Bar. I want to exchange ideas on design of pressure
vessel, T and P monitoring etc. Email to robin@ruchem.ru.ac.za to
save net overload (?)
Robin English
From: forrest@cup.portal.com (Forrest H Bennett)
Newsgroups: sci.chem
Subject: Re: "White" Carbon?  O4?
Date: Fri, 14 Aug 92 00:19:48 PDT
Organization: The Portal System (TM)
Distribution: usa
  <63979@cup.portal.com>

The only source of info on nonstandard Carbon allotrops that I've 
been able to find is two paragraphs and a hypothetical phase 
diagram from:
 
    "Chemistry of the Elements" pp 305, 308
    N. N. Greenwood and A. Earnshaw
    copyright 1984, reprinted 85, 86, 89
    Pergamon Press
                                       
lonsdaleite: "hexagonal wurtize-like lattice", "can be prepared at 
room temperature by static pressure along the c-axis of a single 
crystal of alpha-graphite, though it must be heated above 1000 
under pressure to stabilize it", density calc 3.51g cm^-3.
 
chaoite: white allotrope, "can be synthesized as white dendrites of 
hexagonal symmetry by the sublimation etching of pyrolytic graphite 
under free vaporization conditions above ~2000 C and at low 
pressure (~10^-4mmHg).", calculated density 3.43 g cm^-3.
 
carbon-VI: hexagonal allotrope, "obtained in 72 together with 
chaoite when graphic carbons were heated resistively or 
radiateively at ~2300 C under any pressure of argon in the range 
1-^-4mmHg to 1 atm; laster heating was even more effective", 
density > 2.9g cm^03.
 
chaoite & carbon-VI: "detailed crystal structures" ... "have not 
yet been determined but they appear to be based on a carbyne-type 
motif" (alternating single and triple bonds); ... "both are much 
more resistent to oxidation and reduction than graphite is and 
their properties are closer to those of diamond. Indeed, it now 
seems likely that there is a sequence of at least 6 stable carbyne 
allotropes in the region between stable graphite (2300 C) and the 
mp of carbon (~3500 C at 2*10^4 Pa)..."
 
As soon as I locate it, I'm hoping to find more info in:
 
    "Structural Inorganic Chemistry"
    Oxford University Press 1975
 
Forrest
Newsgroups: sci.chem
From: jbrown@magnus.acs.ohio-state.edu (James S Brown)
Subject: Dissolving rubber?
Organization: The Ohio State University
Date: Fri, 21 Aug 1992 02:06:41 GMT

I am not a chemist, in fact I probably couldn't even play one on T.V., but I 
was wondering about something and ran across this newsgroup. Anyway, can rubber
be dissolved? And if so, by what? I realize this is probably a dumb
question, perhaps too general to respond to in simple terms, but if anyone 
could give it a shot, it would be appreciated!

Thanks in advance,

  Laurie

jbrown@magnus.acs.ohio-state.edu
From: blu@cellar.org (Dan Reed)
Newsgroups: sci.chem
Subject: Help!  I need an answer!
Date: 19 Aug 92 19:57:53 GMT
Organization: The Cellar BBS and public access system

Is Dipotasium (sp) Phosphate, harmful to aluminum?

My cars life depends on it.

PLEASE respond VIA mail..

----- 
 Dan Reed (Blu-Max) blu@cellar.org - AutoCad Geek - VW Lover - InlineSkater 
68 Cougar XR-7, 89 VW Golf, 72 Honda CL360Twin, Ti/99/4a, Vextrex, Timex
From: krm@sdc.boeing.com (Keith Michaels)
Newsgroups: sci.chem
Subject: converting gypsum into sheetrock
Date: 16 Aug 92 20:18:51 GMT

I recently saw on "This Old House" a factory tour of a sheetrock factory.
The process decribed was very simple: the gypsum is mined in an open pit,
crushed, mixed with water, and formed continuously into sheets.
The reaction is obviously exothermic, as the soft sheetrock is warm to 
the touch.

What prevents this reaction from occurring when rain falls on the exposed
gypsum in the pit?  If the reaction is just a hydration of CaSO4, why isn't
it reversable?  There must be more to it than what was shown.
/*-------------------------------------------------------------*
 * Keith R. Michaels                | The Boeing Company       *
 * internet: krm@sdc.boeing.com     | Seattle, WA.             *
 * Disclaimer: Yes.                                            *
 *-------------------------------------------------------------*/
From: saj@chinet.chi.il.us (Stephen Jacobs)
Newsgroups: sci.chem
Subject: Re: Chemistry/Pizza
Summary: Mold inhibitor, mostly
Date: 20 Aug 92 14:36:31 GMT
Organization: Chinet - Public Access UNIX

In article <1992Aug19.215548.29819@afterlife.ncsc.mil> mssmith@afterlife.ncsc.mil (M. Scott Smith) writes:
>   Needless to say, I was just curious to know what this calcium propionate
>stuff is..  (I don't remember it from first year chemistry at college.)  Why
>do they note its presence so liberally on the packaging?

Propionates are generally used to inhibit mold growth (a big problem with 
stuff that goes through a bunch of freeze-thaw cycles.  A person can get 
real discouraged watching what happens to frozen pizza between manufacture
and eating).  It mostly works 'just because.'  But consider that most 
organisms are well-adapted to digesting fatty acids with an even number of
carbon atoms.  Propionic acid gums up the works in some molds, and at least
slows them down.

If that pizza contained meat, it falls under USDA labelling regulations.
Nobody bothers to try to make sense of them anymore.  

                                      Steve
Newsgroups: sci.chem