HDTenEightyP/NetNews huggingface dataset:
From: rodenhiser@chem1.chem.dal.ca (RODENHEISER ANDREW)
Newsgroups: sci.chem
Subject: Re: Soft Drink Ingredient: Fluorescent Beer!
Date: 20 Dec 92 18:44:58 GMT
Organization: Dalhousie University, Halifax, Nova Scotia

In article <1992Dec18.181833.28302@netcom.com> howard@netcom.com (Howard Berkey) writes:
>From: howard@netcom.com (Howard Berkey)
>Subject: Re: Soft Drink Ingredient
>Date: Fri, 18 Dec 1992 18:18:33 GMT
>In article <A21067@F.maus.de> Sevo_Stille@f.maus.de (Sevo Stille) writes:
>>ornitz@kodak.kodak.com wrote in SCI.CHEM,A65354@HB
>>
>>While quinine in soft drinks may have been a useful trick to smuggle a malaria
>>prophylactic into the gin tonics of drunk colonial officers, it is hardly a
>>suitable flavour for todays soft drinks - stuff like tonic water and bitter
>>lemonades probably escaped from the drugstores into the bars during prohibition
>>and its "medical" applications of cocktails.
>
>It's still used in some tonic water, though.
>
>>True quinine tonic water (Schweppes Kenia still used to sell pretty strong
>>stuff some years ago...) has a strange blueish hue, which might be mimicked
>>with glycerol ester of wood rosin, to give quinine replacement tonics the
>>colour of the real stuff.
>
>Quinine is cool for drinks in a nightclub setting because it
>fluouresces with a pale blue color when exposed to UV light.  Fairly
>brightly, too.  Black lights in clubs can make it fluouresce.

So does a glass of draught beer, but only about the top inch because I 
presume the UV light is all absorbed after that distance.  A strange green/
purple tint in the yellow/brown liquid.  Any idea what compounds are 
responsible?

>-Howard
>-- 
>::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::
>Howard Berkey                       			   howard@netcom.com
>			  WARNING: Intel Inside
>... .. ...   ... .. ...   ... .. ...    ... .. ...   ... .. ...   ... .. ...

--
/KISS/Cooper/Seattle/Metal/MontyPython/DouglasAdams/NASCAR/Oldsmobiles
Andrew P. Rodenhiser,  Graduate Student   RODENHISER@CHEM1.CHEM.DAL.CA
Dalhousie  University,  Halifax,  N. S.,  Canada     APRODEN@AC.DAL.CA
Fluorescence  Probing  Studies  of  Polymer / Surfactant  Interactions
"Now I know why everything turns grey, but it's our own world we paint
And I want the brightest,  I want *fluorescent*.  Every day and night,
for the rest of my life.  Open your eyes, won't you?"--Faith. No More.
Newsgroups: sci.chem
From: dblackbu@alleg.edu (Dave Blackburn)
Subject: Re: Acid-base equilibrium (triprotic)
Organization: Allegheny College
Date: Wed, 16 Dec 1992 19:56:58 GMT

In article <c60a-gx.724486364@danube.Berkeley.EDU> c60a-gx@danube.Berkeley.EDU  
(Jeffrey Twu) writes:
>rmcory@uwovax.uwo.ca writes:
>>In article <c60a-gx.724438370@danube.Berkeley.EDU>,  
c60a-gx@danube.Berkeley.EDU (Jeffrey Twu) writes:
>>> Alright, I've been pondering over this question for the last few days,
>>> and have deduced it impossible to solve (with respect to the constraints,
>>> not the difficulty).  I would like your comments on it.
>>> 
>>> You are given four stock solutions, each one molar (1 mol/L) in their
>>> concentrations:  H3PO4, NaH2PO4, Na2HPO4, Na3PO4 (charges omitted).  From
>>> only these four solutions (no H2O lying around), you will make a buffer
>
>>Sorry, I'm afraid you have to have some H2O! Someone is pulling your leg.
>
>>> solution with the following restraints:
>>> 
>>> 1) pH = 6.8 (reasonably buffered around there)
>>> 2) total volume of new solution = 1 liter
>>> 3) Free phosphate concentration = [PO4] = 0.10 M
>
>>What is undoubtedly required here is ***TOTAL*** "phosphate" conc = 0.10 M, 
>>which in this case would be [H2PO4] + [HPO4] since at pH 6.8 the concs of
>>H3PO4 and PO4 would be negligible.
>
>>Otherwise, the problem is impossible, since [PO4] cannot be 0.10 M at pH  
6.8.
>
>>> 
>>> 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
>>> 
>>> Now, if this problem is actually impossible as written, would it be
>>> solvable if you removed one or more of the constraints?  (This question
>>> isn't part of the actual problem.)
>
>Ok, let's say you do allow total phosphate concentration = [H3PO4] +
>[H2PO4] + [HPO4] = 0.10 M ([PO4] negligible).  But, will we still need
>water to dilute?  (Remember, the total volume must be one liter.)
>
>Jeff
>+-Just remember:------------------------------------------------------------+
>|	Take it easy.							    |
>|		...and don't forget that human touch.	   	            |
>+<c60a-gx@danube.berkeley.edu>_________________________________<Jeffrey Twu>+

Well, if each of your stock solutions is 1.0 M in X3PO4 (X= H or Na) then  
without dilution the total phosphate will be 1.0 M no matter which of the  
solutions you mix together. (Phosphate with the appropriate number of protons,  
or as the biochemists out there say, P-sub-i)
--

* Dave Blackburn  dblackbu@alleg.edu  flames to self@home.dev.null *          
* Chemistry, Macs, Hypercard, cats,  <>< religion, & the Dead      *
* (Anyone else who held these opinions would be as crazy as I am.) *
*   "Sometimes the songs that we hear are just songs of our own"   *
From: dl10696@ehsn4.cen.uiuc.edu (Dat Trieu Le)
Newsgroups: sci.chem
Subject: Re: White gold
Date: 14 Dec 92 20:05:35 GMT
Organization: University of Illinois at Urbana

billn@hpcvaac.cv.hp.com (bill nelson) writes:

>kenneth@davy.uio.no (Kenneth Ruud) writes:
>: In article <1992Dec9.072759.22917@ucsu.Colorado.EDU> lorenzo@spot.Colorado.EDU (Eric J. Lorenzo) writes:
>: >
>: >   What exactly is white gold?  Is it a naturally found metal?  It definately
>: >   costs more in jewelry form.
>: >
>: White gold is not found naturally as a metal, because it is an alloy made of
>: gold, nickel and palladium. Im'm afraid I don't know the exact composition in
>: percent, but perhaps somone out there can help?

>White gold usually contains either 25% platinum or 12% palladium.

>Bill

I was under the impression that the gold jewelers sell are alloys.
Pure gold is too soft and brittle to be used as jewelry. I guess
that's why American jewelers don't sell any purer than 18 karot gold.
But I was unaware of the alloys they actually use.
Newsgroups: sci.chem
From: rmcory@uwovax.uwo.ca
Subject: Re: phosphate buffer chemistry
Organization: University of Western Ont, London
Distribution: na
Date: Fri, 18 Dec 1992 01:34:52 GMT

In article <5101@equinox.unr.edu>, whitbeck@equinox.unr.edu (Michael Whitbeck) writes:
> for those following the thread on the 
> phosphate buffer problem I posted a guestimate solution
> but failed to check all the balancing equations for
> reasonableness (e.g. mass and charge)- that was my last
> word on the subject (till now)
> 
> here is a basic program that I just 
> used to cross-check mass and charge balance, etc on
> the answer I had posted earlier:
> 
> 10 X1 =  1.44347E-05   REM H3PO4 at equilibrium
> 20 X2 = 0.701707   REM H2PO4 at equilibrium
> 30 X3 = 0.186543   REM HPO4 at equilibrium
> 40 X4 = 0.111736   REM PO4 at equilibrium
> 50 X5 =  1.57200E-07   REM H ion at equilibrium
> 60 X6 = 0.53		REM initial added H3PO4
> 70 X7 = 1-X6		REM initial added Na3PO4
> 80 c1 =  7.11000E-03	REM equilibrium constants
> 90 c2 =  6.32000E-08
> 100 c3 =  7.10000E-13
> 110 R1 = C1*X1-X5*X2   REM checks on equilibria
> 120 R2 = C2*X2-X5*X3   REM checks on equilibria
> 130 R3 = C3*X3-X5*X4   REM checks on equilibria
> 140 R4 = 3*X7+X5-X2-2*X3-3*X4  REM check charge balance
> 150 R5 = X6+X7-X1-X2-X3-X4  REM check mass balance
> 160 PRINT R1,R2,R3
> 170 PRINT R4,R5
>>run
> -1.10308E-07 -2.93246E-08 -1.75649E-08 
> -8.42800E-07 -4.34700E-07 
> 
> if these results fall into the category
> of close-enough then the answer to the
> original poster's question remains
> YEP! you can get the specified solution as
> long as you aren't too fussy about free PO4 being
> 0.11M vs 0.1M
> 
> previously I said all this was neglecting volume change on 
> mixing and activity coefficients. I should also
> add that given such a conc'd solution ion-pair formation
> might also be significant.  
> 
> Mike W.
-- 

This is nonsense! If [PO4] = 0.1 M, we have:

K3 = 7.1E-13 = [H3O+][PO4]/[HPO4] = (10E-6.8)(0.1)/[HPO4]

so [HPO4] = 22,300 M !

NOT!!!


--------------------------------------------------------------
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
From: James_J_Kowalczyk@cup.portal.com
Newsgroups: sci.chem
Subject: Re: Glow Sticks  -- sci.chem FAQ?
Date: Tue, 15 Dec 92 22:30:30 PST
Organization: The Portal System (TM)
Distribution: world

wdb3926@zeus.tamu.edu (BRUTON, WILLIAM DANIEL) writes:

>Glow Sticks...
>
>You know those liquid filled cylinders that you can buy at camping stores?
>When you break a small capsule in the center of the plasitc stick
>by bending the cylinder the capsule breaks and two liquids mix and
>give off a bright green glow....bright enough to read by...
>
>Any idea what the two liquids are?
>
>Dan


This is not a flame, but since this question comes up in sci.chem
about once a month, has anyone considered created a FAQ for sci.chem?
(If there is one, sorry. :)  

Jim Kowalczyk                      James_J_Kowalczyk@cup.portal.com
From: det@phlan.sw.stratus.com (David Toland)
Newsgroups: sci.chem
Subject: Re: GRE Question
Date: 16 Dec 1992 13:45:04 GMT
Organization: Stratus Computer, Software Engineering
NNTP-Posting-Host: phlan.sw.stratus.com

In article <1992Dec16.043711.24096@news.cs.brandeis.edu> st891425@pip.cc.brandeis.edu writes:
>Are minute amounts of H3PO4 used in soft drinks?

I don't know if I'd call the quantity of phosphoric acid in some soft drinks
"minute".  On my can of Diet Coke sitting here, it's listed *before*
the preservatives, the natural flavors and the caffeine.

Ever wonder why mixtures of carbonated water and syrup were called
"phosphates" in the old soda counters?  Also, now you've got some idea
why Coke is so good for cleaning rust off of nails.




-- 
--------------------------------------------------------------------------
All opinions are MINE MINE MINE, and not necessarily anyone else's.
det@phlan.sw.stratus.com   |  "Laddie, you'll be needin' something to wash
                           |  that doon with."
From: root@admin.mport.COM (admin)
Newsgroups: sci.chem
Subject: Re: Phenyl acetone.
Date: 11 Dec 92 22:46:29 GMT
Organization: Microport Inc., Scotts Valley, CA 95066 US of A



>Now that brings up another point.  Isn't there a class of opiate
>antagonists (or agonists, whichever is the right word) that are very
>closely related to their agonist (or antagonist) cousins?  So on one
>hand you can have a large degree of structural freedom while still
>having similar activity; but on the other, a large change in activity
>can come about from a small structural change.  I suppose this is one
>of those things that makes pharmacology and biochemistry interesting.
>-- 
>David J. Heisterberg (djh@osc.edu)       What men value is not rights

===================

I seem to remember that in the semi-synthetic (morphine based) opiates,
the group attached to the Nitrogen can drastically change the
agonist/antagonist properties.  An Allyl group makes it strongly
antagonistic if I remember right, a methyl = morphine (??)  Anyone
remember anything along these lines?

-rbd


=*=*=*=*=*=*=*=*=*=*=*=*========*=*=*=*=*=*=*=========*=*=*=*=*=*=*=*=*=*=*=*=*=
Richard ducman Ducoty                                          Microport Inc.
duc@mport.com                                                  Scotts Valley, CA
root@mport.com                                                 408.438.8649
From: Erik@tdkt.kksys.com (Erik Jacobson)
Newsgroups: sci.chem
Subject: FidoNet dupes from my sight...
Date: 15 Dec 92 23:56:14 GMT

I will not be reading sci.chem for responses.  I will monitor news.admin, but
would appreciate it if messages were sent to me in e-mail.  This will be my only
posting in sci.chem.

I hesitated to reply to these messages because I was afraid it would make things
WORSE, not better.  Some people urged me to post, so I decided to throw one in
here.

My sight did, in fact, throw a bunch of messages into sci.chem.  It was a one
time thing.  It happened in one big bunch -- only once.  So, it is NOT STILL
HAPPENING.  It was a one time thing... I was not home while the bunch got sent
out, so I wasn't able to catch them.

This reason it happened was because I was switching mail tossers, and one of the
conversion programs (to convert setup) didn't convert the setup very nicely.  A
bunch of Fidonet areas got thrown into a directory along with usenet areas. 
They all got scanned out as sci.chem messages, once.  As soon as I noticed the
problem, I fixed it.

I am sorry for the problems this may have caused.  It is my understanding that
people are still talking about this issue as if it is still happening.  It
isn't!  It happened in one batch one evening, and stopped there.  People who are
posting that it is still happening are just quoting old messages.

I guess I will try to monitor news.admin for a while to answer any questions. I
would appreciate it if the responses were posted in e-mail, however.

One more comment.  I got punished for all of this.  At least 100 e-mail messages
got thrown at my sight.  One person sent an e-mail reply to every fidonet
message that was thrown into sci.chem.  I bet there are a lot of confused
FidoNet users out there wondering where this strange message came from out of
the blue telling them to stop posting stuff in sci.chem.

Erik... I suppose you could say a news admin?  Heh

 * Origin: Dark Knight's Table - N0SVX - Minnetonka, MN (1:282/31)
From: howard@netcom.com (Howard Berkey)
Newsgroups: sci.chem
Subject: test-ignore
Date: 12 Dec 1992 14:51:44 -0600
Organization: UTexas Mail-to-News Gateway
NNTP-Posting-Host: cs.utexas.edu

:)

-- 
::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::::
Howard Berkey                       			   howard@netcom.com
			       I Am Electro
... .. ...   ... .. ...   ... .. ...    ... .. ...   ... .. ...   ... .. ...
From: ivan@erich.triumf.ca (Ivan D. Reid)
Newsgroups: sci.chem
Subject: Re: C 60 TRUNKATED ICOSAEDRAL COORDINATES
Date: 17 Dec 1992 10:04 PST
Organization: TRIUMF: Tri-University Meson Facility
Distribution: world
NNTP-Posting-Host: erich.triumf.ca
News-Software: VAX/VMS VNEWS 1.41    

In article <36023@sophia.inria.fr>, laurent@cenerg.cma.f writes...
>Because I am a bad mathematician and especially a lazy, I am looking
>for coordinates of nodes of a trunkated icosadreal (C 60 atoms) to visualize 
>the molecule in 3 D with a computer programm, I have.
> 
	This also in response to an earlier request for C60 atomic coordinates
(which I didn't post due to a lost transAtlantic link at the crucial moment).
The theoretical coordinates as well as those deduced from neutron scattering
are in WIF David et (many) al., Nature 353, 147 (12 September 1991).

Ivan Reid, Paul Scherrer Institute, CH.     			ivan@cvax.psi.ch
From: ralf@ark.abg.sub.org (Ralf Stephan)
Newsgroups: sci.chem
Subject: Re: *****GET OUT OF THIS NEWSGROUP!!!*****
Date: 11 Dec 92 13:59:00 GMT
Organization: Not Very Ltd.

> >>You know who you are.
> 
> Is it a software glitch, or is it enemy action?
> 
> Maybe it's a Turing Test.

Even worse:  Fidonet at its best.


--
*******************************************************************************
int a=10000,b,c=2800,d,e,f[2801],g;main(){for(;b-c;)f[b++]=a/5;for(;d=0,g=c*2;c
-=14,printf("%.4d",e+d/a),e=d%a)for(b=c;d+=f[b]*a,f[b]=d%--g,d/=g--,--b;d*=b);}
Newsgroups: sci.chem
From: ornitz@kodak.kodak.com (Barry Ornitz)
Subject: Re: Soft Drink Ingredient
Followup-To: sci.chem
Keywords: wood rosin, brominated vegetable oil, turpentine, lemon oil
Organization: Eastman Chemical Company
Distribution: usa
Date: Wed, 16 Dec 92 16:43:25 GMT

In article <1992Dec15.153655.15312@rosevax.rosemount.com> 
scotbri@flower.rosemount.com (Scott Brigham) writes:
>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?

At one time, the late Larry Lippman discussed this.  Unfortunately I did not
save the post, so I am not sure of the following answer.  Larry discussed both
glycerol esters and brominated vegetable oil, another common ingredient in
non-cola soft drinks.  His answer had to do with making the drink opalescent
(somewhat cloudy) to mimic natural fruit juices.

Another possibility is that the glycerol ester of wood rosin may be a 
saponification agent to enhance the solubility of lemon oils in water.  Lemon
oil itself is commercially obtained from turpentine distillation so there may
be a connection here. [I once toured the Glidden (paint)/Durkee (flavorings)
plant in Jacksonville, FL.  They also made peppermint and spearmint oils,
perfume bases, and other interesting products as well as turpentine from tall
oils obtained from paper mills.]

I hope someone else has the true purpose and will post it.
						Barry
 -----------------
|  ___  ________  |    Dr. Barry L. Ornitz          WA4VZQ
| |  / /        | |    Eastman Chemical Company
| | / /         | |    ECC Research Laboratories, Engineering Research Div.
| |< < K O D A K| |    Process Instrumentation Research Laboratory
| | \ \         | |    P. O. Box 1972, Building 167B
| |__\ \________| |    Kingsport, TN  37662  (615/229-4904, FAX 615/229-4558)
|                 |    INTERNET:   ornitz@kodak.com
 -----------------
Newsgroups: sci.chem
Subject: Re: Arsenic Trioxide
From: vxc15931@vax1.mankato.msus.edu
Date: 11 Dec 92 13:58:20 -0600
Organization: Mankato State University

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?

And no, I don't intend to poison anyone (although I am tempted).  I need a 
sample for a lab demonstration of the Marsh test.  This is for a 
law enforcement class in forensic chemistry.

Thanks in advance!

==================
Jose' R.C. Cruz
Graduate Assistant
Mankato State University
Mankato, MN

==================

"Eliminate the impossible.  Whatever remains, though highly improbable, 
 must be the truth."

              - Sherlock Holmes
From: slp9c@cc.usu.edu
Newsgroups: sci.chem
Subject: Alternative refregrents !
Date: 17 Dec 92 16:30:59 MDT
Organization: Utah State University

Hi everybody,
		
		I would appreciate it a lot if some one
has any information on alternative refregrents, i.e.,
alternative to freon.  I know of methyl chloride as being
used as refregrent, but I was wondering if there are any
other compounds.
	
		Thanks in advance for your help,

Jasmail Singh
From: whitbeck@equinox.unr.edu (Michael Whitbeck)
Newsgroups: sci.chem
Subject: Re: Soft Drink Ingredient
Date: 15 Dec 92 22:51:26 GMT
Distribution: usa
Organization: University of Nevada, Reno

In article <1992Dec15.153655.15312@rosevax.rosemount.com> scotbri@flower.rosemount.com (Scott Brigham) writes:
>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
>=========================

wood rosin is obtained from the extraction of pine
stumps with naptha followed by distillation. The
raw material is graded by color and consists of a
mixture of high mol. wt. acids, abietic acid may
dominate [the mixture may often be referref to as
abietic acid]. The glycerol ester is of course the
product from reacting the acids with glycerol.

Why are you drinking it? -- I don't know; does it
taste good?


My *guess* is that it either contributes to the
texture or the bitter taste of the beverage.

Mike W.
Newsgroups: sci.chem
From: nkjrm@taxus.uib.no (Rolf Manne)
Subject: Re: Stable Orbitals: 1/2 full
Organization: University of Bergen
Date: Wed, 16 Dec 1992 09:34:42 GMT

In article <1992Dec13.040948.7448@cronkite.ocis.temple.edu> sklar@picasso.ocis.temple.edu (Dave Sklar) writes:


>       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

The standard explanation why half-filled shells are preferred involves also
the fact that the electrons have to be in the high-spin state, i.e. 
all electron spins parallel. The Pauli exclusion principle then makes the
electrons avoid each other more than if some electrons had different spins. 

The above is a paraphrase of one of Hund's rules, formulated by German
physicist Friedrich Hund in the late 1920's. You find it in texts of
quantum mechanics.

Rolf Manne
e-mail Rolf.Manne@uib.no
Newsgroups: sci.chem
From: kim@Lise.Unit.NO (Kim Gunnar St|vring \yhus)
Subject: Re: TIME HAS INERTIA
Organization: Norwegian Institute of Technology
Date: Sat, 19 Dec 92 22:15:39 GMT

Warning to new readers of Abians postings concerning his principle.

If you post something about his principle, no matter how polite you
formulate it, the usual thing for Abian is to either answer rudely and with
no real content, or ignore you.

It has been proven that his principle is informationless, unusable, and not
science, but he still lingers on in this newsgroup.

Abian feeds on replies. Please don't feed him.

Kim0
From: schindler@rz-berlin.mpg.de
Newsgroups: sci.chem
Subject: Re: Stable Orbitals: 1/2 full
Date: 15 Dec 92 11:59:03 +0100
Organization: Rechenzentrum MPG Berlin

In article <Bz9p7E.Asq@news.cso.uiuc.edu>, dl10696@ehsn4.cen.uiuc.edu (Dat Trieu Le) writes:
> sklar@picasso.ocis.temple.edu (Dave Sklar) writes:
> 
> 
>>	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
> 
> Maybe it has something to do with the the geometry of the d-orbitals.
> The d-orbitals appear to be some complex 3-dim figure. Each orbital,
> by the Valence Electron Repulsion, are as far apartfrom each other
> as possible. There are 5 d-orbitals. If 4 of them are half-filled,
> then they would be applying lots of force and crowd over the unfilled
> orbital and thus making the d-orbitals less stable. Thus, if all 5
> orbitals are unfilled, then there is equilibrium among the d-orbitals,
> since all orbitals have one electron and are of the same energy level.
> 

My naive explanation why Cr 3d5 4s1 is more favorable than 3d4 4s2 is
that the spin spin pairing energy for the 4s level is larger than the
difference between 4s and 3d. 

just my two pence - Michael Schindler.
From: gsteckel@vergil.Eng.Sun.COM (Geoff Steckel - Sun BOS Hardware CONTRACTOR)
Newsgroups: sci.chem
Subject: Re: Soft Drink Ingredient
Date: 16 Dec 1992 20:13:08 GMT
Organization: Omnivore Technology, Newton, MA (617) 332-9252
Distribution: usa
NNTP-Posting-Host: vergil.east.sun.com

>In article <5079@equinox.unr.edu> whitbeck@equinox.unr.edu (Michael Whitbeck) writes:
>>>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?

I believe that this ingredient is used to produce cloudiness in the beverage.
You're supposed to believe that cloudiness is from lemon squeezings.
(Pine squeezings!?)

--
	geoff steckel (gwes@trilobyte.com, gwes@wjh12.harvard.EDU)
Disclaimer: I am not affiliated with Sun Microsystems, despite the From: line.
This posting is entirely the author's responsibility.
Newsgroups: sci.chem