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From: Jan K Labanowski <jlabanow-,-nd.edu>

--
Jan K. Labanowski, Ph.D.                   Tel. (574) 631-5465
Science Computing Facility                FAX (574) 631-9293
University of Notre Dame
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Notre Dame, IN 46556-5670










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--
Jan K. Labanowski, Ph.D.                   Tel. (574) 631-5465
Science Computing Facility                FAX (574) 631-9293
University of Notre Dame
225 Nieuwland Science Hall
Notre Dame, IN 46556-5670






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From chemistry-request@ccl.net Thu Jul  7 23:45:44 2005
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Subject: Symmetry breaking during CASSCF
From: <gustavo ## mercury.chem.pitt.edu>
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Dear CCL Readers,
     I have a planar conjugated organic molecule that, on paper, has D2h
symmetry. I am working with the hypothesis that the molecule is a
biradical singlet. I want to perform a CASSCF(2,2) on this molecule
to estimate the biradical character of this molecule. When I
calculate the molecule with the constraint that the molecule has D2h
symmetry, the calculation has severe convergence problems. If I
remove this constraint, the molecule distorts to a C2v symmetry and I
obtain a biradical character ~20%. I checked the orbitals being used
for the CASSCF calculation and they look right (one nonbonding and
another slightly antibonding).
     Is the situation described above correct? Can an organic molecule
have such a symmetry breaking as a result of a CASSCF calculation? Is
the molecule really a C2v system? Any suggestions are welcome.
     Thank you very much in advance for your help.
     Sincerely yours,
                                Gustavo L.C. Moura
                           gustavo ## mercury.chem.pitt.edu




From chemistry-request@ccl.net Thu Jul  7 21:39:02 2005
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Date: Thu, 07 Jul 2005 20:28:49 -0400
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To: chemistry !! ccl.net
Subject: Re: CCL: W:Solvation free energy for aromatic hydrocarbon
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Aromatic systems are weakly polar.  Certainly, compared to other groups 
in proteins --- hydroxyls, amides, carboxylic acids, amines and so on 
--- they are relatively hydrophobic.  However, they are significantly 
more polar than aliphatic hydrocarbons.  As you pointed out, this is 
borne out by the free energies of hydration, as well as by theoretical 
studies.  However, the interior of a protein is a vacuum, and is not 
even entirely hydrophobic (at minimum, there are buried back-bone 
amides).  Looking at transfer between water and octanol (a moderately 
non-polar enviroment), benzene falls out somwhere between propane and 
butane --- certainly preferring the more hydrophobic environment.  This 
all works out as a result of the balancing of enthalpic (both 
electrostatic and van der Waals, in molecular mechanics' terms) 
interactions between the solute and solvent and entropic terms resulting 
> from solvent structure.  More statistical frameworks (like 
hydrophobicity scales and the like)  are really just capturing the same 
underlying physics, which is why you'll often here people refering to 
them in the same language (e.g. the hydrophobic effect).

To give a quick example of how the vacuum to water transfer free energy 
may be negative, while the hydrophobic solvent to water transfer energy 
may be positive, just think about van der Waals interactions; there are 
none in vacuum, and plenty between an aromatic system in hydrophobic 
solvent.  The weak dielectric response of hydrophobic solvents (around 2 
at the very minimum) gives an added bonus, and as always, entropy is a 
hard one to deal with perfectly.

But in a nutshell, aromatic certainly do have favorable hydration free 
energies despite generally considered "hydrophobic".  It's not a 
misnomer, but more a difference in reference state.  Of course, every 
thing is always a little more complicated than what anyone tells you, 
but that's what makes it all fun.

+--------------------------------------------------------------------+
| David F. Green                           |                         |
| Postdoctoral Associate                   | Office: 617-253-5438    |
| Division of Bioengineering and Computer  | Mobile: 617-953-3922    |
|   Science & Artificial Intelligence Lab  | Fax:    617-252-1816    |
| Massachusetts Institute of Technology    |                         |
| 32 Vassar St., 32-211                    | E-mail: dfgreen !! mit.edu |
| Cambridge, MA 02139                      |                         |
+--------------------------------------------------------------------+


Chemical, , Bond wrote:
> Hi there,
> 
> I am confused with a single concept: what should be the sign for the solvation  free energy for a fragment like phenyl?  
> 
> There are many experimental data of solvation free energy for aromatic hydrocarbons, such as benzene, naphthalene, etc, but they are all negative surprisingly.  I looked at several papers with models of solvation energy, and their predictions all all have negative solvation energies for those compounds, just like the experiments.
> 
> Typically when a phenyl group is transfered from water into protein, we would like to say there is a negative(beneficial) desolvation energy, or the usual called hydrophobic effect.  And this has been used in tons of models for protein simulation or protein-ligand binding.  Note, in this context, the solvation energy (from gas into water) is positive! 
> 
> Is there something wrong over here?  Or just some artifact from the fitting?
> 
> Hope there would be some good comments.
> 
> Thanks a lot,
> Bond
> 
> 
> -= This is automatically added to each message by the mailing script =-
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From chemistry-request@ccl.net Fri Jul  8 01:33:33 2005
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Hi Bond,

the concepts of the solavtion models are right. You must take into 
account the van der Waals (vdW) energies, which to first order can be 
considered as a kind of vdWs surface energy.

More or less accidentally, for water vdWs energy and surface tension 
(cavity formation free energy) almost cancel, so that hydration free 
energies of alkanes are very slightly positive. Since aromatics (due to 
the quadrupole moment) are slightly more polar than alkanes, hydration 
free energies of aromatics are slightly negative, as you say.

In a less polar solvent than water the cavitation free energy is much 
less positive (typically close to zero). Thus the solavtion free energy 
in such solvent would be much more negative that it is into water, and 
thus the ballance of the transfer of  aromatics from water to less polar 
solvents is much in favor of the non-polar solvent.

You can study these terms in detail in our solvation model COSMO-RS (see 
www.cosmologic.de).

Regards

Andreas

Chemical, , Bond wrote:

>Hi there,
>
>I am confused with a single concept: what should be the sign for the solvation  free energy for a fragment like phenyl?  
>
>There are many experimental data of solvation free energy for aromatic hydrocarbons, such as benzene, naphthalene, etc, but they are all negative surprisingly.  I looked at several papers with models of solvation energy, and their predictions all all have negative solvation energies for those compounds, just like the experiments.
>
>Typically when a phenyl group is transfered from water into protein, we would like to say there is a negative(beneficial) desolvation energy, or the usual called hydrophobic effect.  And this has been used in tons of models for protein simulation or protein-ligand binding.  Note, in this context, the solvation energy (from gas into water) is positive! 
>
>Is there something wrong over here?  Or just some artifact from the fitting?
>
>Hope there would be some good comments.
>
>Thanks a lot,
>Bond
>
>
>-= This is automatically added to each message by the mailing script =-
>To send e-mail to subscribers of CCL put the string CCL: on your Subject: line
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>
>
>
>
>
>
>
>  
>


-- 
-----------------------------------------------------------------------------
Dr. habil. Andreas Klamt
COSMOlogic GmbH&CoKG
Burscheider Str. 515
51381 Leverkusen, Germany

Tel.: +49-2171-73168-1  
Fax:  +49-2171-73168-9
e-mail: klamt _()_ cosmologic.de
web:    www.cosmologic.de
-----------------------------------------------------------------------------
COSMOlogic
        Your Competent Partner for
        Computational Chemistry and Fluid Thermodynamics
-----------------------------------------------------------------------------




From chemistry-request@ccl.net Fri Jul  8 05:28:04 2005
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Date: Fri, 08 Jul 2005 09:19:13 +0100
From: "Jamie Platts" <platts _()_ Cardiff.ac.uk>
To: <chemistry _()_ ccl.net>
Subject: Re: CCL: MP2 virial value
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Dear Pasikonik

You can obtain the virial value from -V/T = 1 - E/T. Both are reported by
Gaussian,
the energy as EUMP2 (or just MP2 in the archive summary), and the kinetic
energy
as KE, just below the multipole information. Make sure you use the "density"
keyword
or you'll probably get the HF value for KE.

As an example, values for Cl2 using MP2/6-311G* are

EUMP2 =    -0.91923578058246D+03
KE= 9.195031259365D+02
-V/T = 1.99971

Hope this helps,

Jamie

----------------------------------------------------------
  Jamie Platts
  School of Chemistry       Phone: +44 (0) 2920 874950
  Cardiff University            Email: platts _()_ cf.ac.uk
  Park Place                     FAX:   +44 (0) 2920 874030
  Cardiff CF10 3AT            www.cf.ac.uk/chemy

>>> drpasikonik _()_ yahoo.com 07/07/05 11:56 pm >>>
Hi everybody
Can anybody tell me how to obtain the virial (-V/T) value for the MP2
calculations in Gaussian?
There is no problem on the HF or DFT level, but this property is not listed for
MP2. How can I print it
 
Thank you in advance
 
Pasikonik

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From chemistry-request@ccl.net Fri Jul  8 10:47:44 2005
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To: chemistry _()_ ccl.net, mclaro2727 _()_ yahoo.com
Subject: Re: CCL: 3D to chemical name
Message-ID: <1120831136.42ce86a06b781 _()_ webmail.njit.edu>
Date: Fri, 08 Jul 2005 09:58:56 -0400 (EDT)
From: dnp5 _()_ njit.edu
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Hi Claro:

You can try ACD/ChemSketch 8.0 Freeware from the link below. 

http://www.acdlabs.com/download/chemsk.html

Deepangi

Quoting Tony Yuan <TYuan _()_ cambridgesoft.com>:

> 
> 
> Try ChemDraw.  It can do 3D => 2D => Chemical Name.
> Also try ChemFinder.com and ChemACX.com, you can search suppliers by
> doing structure query.
> Chem3D can convert PDB files to MDL mol files and CDX files.
> 
> Good luck!
> 
> -----Original Message-----
> From: Computational Chemistry List [mailto:chemistry-request _()_ ccl.net]
> On
> Behalf Of Noel O'Boyle
> Sent: Thursday, July 07, 2005 4:01 AM
> To: chemistry _()_ ccl.net
> Cc: mclaro2727 _()_ yahoo.com
> Subject: CCL: 3D to chemical name
> Importance: Low
> 
> Dear Claro,
> 
> Many chemical don't have simple names, and many suppliers use
> different
> names
> for the same chemical. What you need is the supplier code for the
> chemical.
> It is sometimes possible (for example, on the sigma-aldrich webpage)
> to
> search
> the supplier's catalogue using the chemical formula, or by drawing the
> molecule
> on the web page.
> 
> A note of warning: often the ligand structures taken from pdb files
> contain
> just the carbon skeleton, and are missing protons and bond orders.
> Just
> to
> make your life easier :-)
> 
> Regards,
> Noel O'Boyle.
> 
> >-- Original Message --
> >Date: Wed, 6 Jul 2005 13:33:44 -0700 (PDT)
> >From: michelle claro <mclaro2727 _()_ yahoo.com>
> >Subject: CCL: 3D to chemical name 
> >To: chemistry _()_ ccl.net
> >Reply-To: chemistry _()_ ccl.net
> >
> >
> >Hello,
> > 
> >I have about 50 pdb structures (no protein in the pdb just the
> ligand)
> but
> >I need the chemical names in order to purchase them.  What is the
> easiest
> >way to get a chemical name from a pdb?  Thanks in advance.
> > 
> >M. Claro
> >
> >
> >__________________________________________________
> >Do You Yahoo!?
> >Tired of spam?  Yahoo! Mail has the best spam protection around 
> >http://mail.yahoo.com 
> 
> 
> 
> 
> 
> To send e-mail to subscribers of CCL put the string CCL: on your
> Subject: line
> 
> Send your subscription/unsubscription requests to:
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> 
> 
> 
> 
> 
> 
> 
> 
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From: Yvette Sturdy <yvette.sturdy _()_ chemistry.oxford.ac.uk>
Date: Fri, 8 Jul 2005 13:08:30 +0100 (BST)
To: chemistry _()_ ccl.net
Subject: Wilson B Matrix
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Dear All,

I'm having some problems obtaining the Wilson B matrix.

I have outputted it from Gamess. The package calculates the z matrix from
the cartesians correctly, but if i take the B matrix it gives and pre-multiply
the cartesians only the bond lengths come out correctly. Has anyone had
any experience with this? Or does anyone know of a code i can use to obtain
the B matrix?

(I've tried with gaussian98 and encounter similar problems)

Thanks.

Yvette.


-- 
Yvette Sturdy
Physical and Theoretical Chemistry Laboratory
University of Oxford



From chemistry-request@ccl.net Fri Jul  8 07:34:45 2005
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From: "Gustavo, L.C., Moura" <gustavo _()_ mercury.chem.pitt.edu>
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Dear CCL Readers,
     I have a planar conjugated organic molecule that, on paper, has D2h
symmetry. I am working with the hypothesis that the molecule is a
biradical singlet. I want to perform a CASSCF(2,2) on this molecule
to estimate the biradical character of this molecule. When I
calculate the molecule with the constraint that the molecule has D2h
symmetry, the calculation has severe convergence problems. If I
remove this constraint, the molecule distorts to a C2v symmetry and I
obtain a biradical character ~20%. I checked the orbitals being used
for the CASSCF calculation and they look right (one nonbonding and
another slightly antibonding).
     Is the situation described above correct? Can an organic molecule
have such a symmetry breaking as a result of a CASSCF calculation? Is
the molecule really a C2v system? Any suggestions are welcome.
     Thank you very much in advance for your help.
     Sincerely yours,
                                Gustavo L.C. Moura
                           gustavo _()_ mercury.chem.pitt.edu


From chemistry-request@ccl.net Fri Jul  8 05:13:23 2005
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Date: Fri, 08 Jul 2005 11:11:09 +0200
From: Pierre Archirel <pierre.archirel !! lcp.u-psud.fr>
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Dear Elmar,
I would say the issue you are refering to has nothing to do with PCM,
but is probably due to a DFT artifact, which is the wrong dissociation
of NaCl, even in the gas phase. Your asymptotic system is a singlet open 
shell,
with two electrons, alone in their orbitals. DFT poorly addresses this 
situation,
because of the approximative cancelation of the self interaction.
To check this:
1- verify that at the crude HF level, your long range PCM energy is the sum
of the PCM energies of the fragments.
2-  check if your (gas phase) long range B3LYP calculation yields
fragments with 0 charges. If not, DFT is of no help to you.
P.

__________________________________________________________

 Pierre Archirel
 Groupe de Chimie Thiorique
 Laboratoire de Chimie Physique      Tel: 01 69 15 63 86
 Bat 349                             Fax: 01 69 15 61 88
 91405 Orsay Cedex
 France                   pierre.archirel !! lcp.u-psud.fr
__________________________________________________________




From chemistry-request@ccl.net Fri Jul  8 00:13:51 2005
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From: Christopher Cramer <cramer ## chem.umn.edu>
Subject: Fwd: CCL: dissociation problem in PCM model ? 
Date: Thu, 7 Jul 2005 22:13:47 -0500
To: Elmar Gerwalin <elg ## chemie.uni-kl.de>
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Elmar,

    My textbook, Essentials of Computational Chemistry, actually has a  
specific section (11.4.4  Potentials of Mean Force and Solvent  
Structure) that mentions your problem. The issue is that continuum  
models like the PCM variants involve the definition of a solute cavity,  
typically defined as roughly the union of a set of van der Waals  
spheres on all of the atoms. If you pull your solute apart, breaking a  
bond, at some point you will exceed van der Waals contact and the poor  
program has to decide what to do. It is quite unpleasant to solve the  
Poisson equation with two cavities in a dielectric continuum... If  
memory serves, PCM leaves some sort of neck between the two for awhile,  
so that there is still a single cavity, but this clearly soon becomes a  
bad approximation, since there is really solvent there. At some point,  
the program probably just delivers an error message (and a cryptic one,  
too, no doubt).

    But, if you compute the separated species individually, then there  
is no problem at all. Each has a well defined cavity and is infinitely  
far from anything but solvent. The two calculations will not agree,  
since the cavities were defined very differently.

    The only widely used continuum model that does NOT suffer from this  
discontinuity in a potential of mean force owing to cavity separation  
is the Generalized Born model, which takes atomic radii as inputs but  
does not use them to construct a formal cavity and is smooth and  
continuous over all distances.

    If you would like to try a GB model, you are welcome to employ one  
of our SMx solvation models, freely available in a variety of codes,  
including SMxGAUSS, which can either read a Gaussian output file as  
input and run as a stand-alone code, or can be driven by G03 using the  
"external" keyword. See comp.chem.umn.edu/mccdir/software.htm for full  
details.

Best regards,

Chris

Begin forwarded message:

> From: Elmar Gerwalin <elg !! chemie.uni-kl.de>
> Date: July 7, 2005 3:29:35 PM CDT
> To: CHEMISTRY !! ccl.net
> Subject: CCL: dissociation problem in PCM model ?
> Reply-To: chemistry !! ccl.net
>
> Hi,
>
> I'm trying to describe dissociation processes in some small organic  
> molecules.
> Therefore, I'm using B3LYP+SCRF(C-PCM, solvent=methanol) single point  
> jobs to get the
> solvation energy at each step. Finally, a potential energy curve E(R)  
> is my goal.
> R is the bond distance I'm interested in; e.g. a C-O, C-Cl bond or ,  
> for testing purposes
> Na-Cl.
>
> But, unfortunately, wrong asymptotic behaviour (like a "size  
> inconsistency problem") is
> observed in all cases: the "supermolecule's" solvation energy at large  
> distances (10 or 20 A)
> is differing about more than 20 kcal/mole from the sum of the  
> solvation energies of the two ions.
>
> My question is: is the problem known (references ?)? How can be it be  
> accounted for ?
> Do I have to use specific energy terms given in gaussian's output  
> and/or male a correction to them ?
>
> Any help is appreciated.
>
> Bye,
>
> Yours,
>  Elmar
>
>
> --  
> ========================================================
> Elmar Gerwalin ,   University of Kaiserslautern,Germany
>                    Dept. of Theoretical Chemistry
>                    elg !! chemie.uni-kl.de
> ========================================================
>
>
> -= This is automatically added to each message by the mailing script =-
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>
>
>
>
>
--

Christopher J. Cramer
University of Minnesota
Department of Chemistry
207 Pleasant St. SE
Minneapolis, MN 55455-0431
--------------------------
Phone:  (612) 624-0859 || FAX:  (612) 626-2006
Mobile: (612) 597-5275
cramer !! pollux.chem.umn.edu
http://pollux.chem.umn.edu/~cramer
(website includes information about the textbook "Essentials
     of Computational Chemistry:  Theories and Models, 2nd Edition")


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Elmar,


   My textbook, Essentials of Computational Chemistry, actually has a
specific section (11.4.4  Potentials of Mean Force and Solvent
Structure) that mentions your problem. The issue is that continuum
models like the PCM variants involve the definition of a solute
cavity, typically defined as roughly the union of a set of van der
Waals spheres on all of the atoms. If you pull your solute apart,
breaking a bond, at some point you will exceed van der Waals contact
and the poor program has to decide what to do. It is quite unpleasant
to solve the Poisson equation with two cavities in a dielectric
continuum... If memory serves, PCM leaves some sort of neck between
the two for awhile, so that there is still a single cavity, but this
clearly soon becomes a bad approximation, since there is really
solvent there. At some point, the program probably just delivers an
error message (and a cryptic one, too, no doubt).


   But, if you compute the separated species individually, then there
is no problem at all. Each has a well defined cavity and is infinitely
far from anything but solvent. The two calculations will not agree,
since the cavities were defined very differently.


   The only widely used continuum model that does NOT suffer from this
discontinuity in a potential of mean force owing to cavity separation
is the Generalized Born model, which takes atomic radii as inputs but
does not use them to construct a formal cavity and is smooth and
continuous over all distances.


   If you would like to try a GB model, you are welcome to employ one
of our SMx solvation models, freely available in a variety of codes,
including SMxGAUSS, which can either read a Gaussian output file as
input and run as a stand-alone code, or can be driven by G03 using the
"external" keyword. See comp.chem.umn.edu/mccdir/software.htm for full
details.


Best regards,


Chris


Begin forwarded message:


<excerpt><bold><color><param>0000,0000,0000</param>From:
</color></bold>Elmar Gerwalin <<elg !! chemie.uni-kl.de>

<bold><color><param>0000,0000,0000</param>Date: </color></bold>July 7,
2005 3:29:35 PM CDT

<bold><color><param>0000,0000,0000</param>To:
</color></bold>CHEMISTRY !! ccl.net

<bold><color><param>0000,0000,0000</param>Subject: </color>CCL:
dissociation problem in PCM model ? 

<color><param>0000,0000,0000</param>Reply-To:
</color></bold>chemistry !! ccl.net


Hi,


I'm trying to describe dissociation processes in some small organic
molecules.

Therefore, I'm using B3LYP+SCRF(C-PCM, solvent=methanol) single point
jobs to get the 

solvation energy at each step. Finally, a potential energy curve E(R)
is my goal.

R is the bond distance I'm interested in; e.g. a C-O, C-Cl bond or ,
for testing purposes

Na-Cl.


But, unfortunately, wrong asymptotic behaviour (like a "size
inconsistency problem") is 

observed in all cases: the "supermolecule's" solvation energy at large
distances (10 or 20 A) 

is differing about more than 20 kcal/mole from the sum of the
solvation energies of the two ions.


My question is: is the problem known (references ?)? How can be it be
accounted for ?

Do I have to use specific energy terms given in gaussian's output
and/or male a correction to them ?


Any help is appreciated.


Bye,


Yours,

 Elmar



-- 

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

Elmar Gerwalin ,   University of Kaiserslautern,Germany

                   Dept. of Theoretical Chemistry

                   elg !! chemie.uni-kl.de    

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



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</excerpt>--


Christopher J. Cramer

University of Minnesota

Department of Chemistry

207 Pleasant St. SE

Minneapolis, MN 55455-0431

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

Phone:  (612) 624-0859 || FAX:  (612) 626-2006

Mobile: (612) 597-5275

cramer !! pollux.chem.umn.edu

http://pollux.chem.umn.edu/~cramer

(website includes information about the textbook "Essentials

    of Computational Chemistry:  Theories and Models, 2nd Edition")



--Apple-Mail-1-751306894--



From chemistry-request@ccl.net Thu Jul  7 22:47:31 2005
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Date: Thu, 07 Jul 2005 21:52:29 -0400
From: Jose Gascon <jose.gascon !! yale.edu>
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To: chemistry !! ccl.net
Subject: Re: CCL: dissociation problem in PCM model ?
References: <20050707202935.GA10202 !! pc1.chemie.uni-kl.de>
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Elmar, as I understand, DFT cannot be used to calculate dissociation 
energies.
Consider just the case of H2+ (the most trivial molecule). Here you will get
the wrong assimptotic value. In fact Hartree-Fock will give you the 
exact answer.
This is an intrinsic problem given by the fact that the density 
functionals are not
known exactly. In the case of H2+ this results in an electron that can 
literally interact
with itself.
My suggestion is to use MP2 or QCISD if you can afford it.
Best, jose

Elmar Gerwalin wrote:

>Hi,
>
>I'm trying to describe dissociation processes in some small organic molecules.
>Therefore, I'm using B3LYP+SCRF(C-PCM, solvent=methanol) single point jobs to get the 
>solvation energy at each step. Finally, a potential energy curve E(R) is my goal.
>R is the bond distance I'm interested in; e.g. a C-O, C-Cl bond or , for testing purposes
>Na-Cl.
>
>But, unfortunately, wrong asymptotic behaviour (like a "size inconsistency problem") is 
>observed in all cases: the "supermolecule's" solvation energy at large distances (10 or 20 A) 
>is differing about more than 20 kcal/mole from the sum of the solvation energies of the two ions.
>
>My question is: is the problem known (references ?)? How can be it be accounted for ?
>Do I have to use specific energy terms given in gaussian's output and/or male a correction to them ?
>
>Any help is appreciated.
>
>Bye,
>
>Yours,
> Elmar
>
>
>  
>

-- 
Jose A. Gascon - Postdoctoral Associate
Department of Chemistry - (203)432-5911; jose.gascon !! yale.edu
Yale University
P.O. Box 208107
New Haven, CT 06520-8107.




From chemistry-request@ccl.net Fri Jul  8 02:56:07 2005
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From: "Xavier ASSFELD" <Xavier.Assfeld !! cbt.uhp-nancy.fr>
To: <chemistry !! ccl.net>
Subject: RE: dissociation problem in PCM model ? 
Date: Fri, 8 Jul 2005 08:55:41 +0200
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Hey,

This is because of the cavity! At equilibrium distance, your system is in
one cavity, but at large distance two cavities are needed. Continuum models
are able to handle one cavity, not two. I'm not aware of program able to
take care of that.
Yours.



			       ...Xav

Pr. Xavier Assfeld             Xavier.Assfeld !! cbt.uhp-nancy.fr
Chimie et Biochimie theoriques T: (33) 3 83 68 43 82
Faculte des Sciences           F: (33) 3 83 68 43 71
54506 Vandoeuvre, France       http://www.cbt.uhp-nancy.fr

X> -----Message d'origine-----
X> De : Computational Chemistry List [mailto:chemistry-request !! ccl.net]De
X> la part de Elmar Gerwalin
X> Envoye : jeudi 7 juillet 2005 22:30
X> A : CHEMISTRY !! ccl.net
X> Objet : CCL: dissociation problem in PCM model ?
X>
X>
X> Hi,
X>
X> I'm trying to describe dissociation processes in some small
X> organic molecules.
X> Therefore, I'm using B3LYP+SCRF(C-PCM, solvent=methanol) single
X> point jobs to get the
X> solvation energy at each step. Finally, a potential energy curve
X> E(R) is my goal.
X> R is the bond distance I'm interested in; e.g. a C-O, C-Cl bond
X> or , for testing purposes
X> Na-Cl.
X>
X> But, unfortunately, wrong asymptotic behaviour (like a "size
X> inconsistency problem") is
X> observed in all cases: the "supermolecule's" solvation energy at
X> large distances (10 or 20 A)
X> is differing about more than 20 kcal/mole from the sum of the
X> solvation energies of the two ions.
X>
X> My question is: is the problem known (references ?)? How can be
X> it be accounted for ?
X> Do I have to use specific energy terms given in gaussian's
X> output and/or male a correction to them ?
X>
X> Any help is appreciated.
X>
X> Bye,
X>
X> Yours,
X>  Elmar
X>
X>
X> --
X> ========================================================
X> Elmar Gerwalin ,   University of Kaiserslautern,Germany
X>                    Dept. of Theoretical Chemistry
X>                    elg !! chemie.uni-kl.de
X> ========================================================
X>
X>
X> -= This is automatically added to each message by the mailing script =-
X> To send e-mail to subscribers of CCL put the string CCL: on your
X> Subject: line
X> and send your message to:  CHEMISTRY !! ccl.net
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From chemistry-request@ccl.net Fri Jul  8 11:16:43 2005
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To: chemistry/at/ccl.net
Cc: Elmar Gerwalin <elg/at/chemie.uni-kl.de>
Subject: Re: CCL: Fwd: dissociation problem in PCM model ?
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Dear Elmar, dear Chris,

just as a note, COSMO at least in its newer implementations as in 
TURBOMOLE should also give a rather reasonable and additive result for 
the solvation energies in such cases. Nevertheless, you must take into 
account that at low values of epsilon some of the electrostatic 
interaction of the parts is left, especially if hey are ions. So it is 
reasonable that you do not just get the sum of the energies of the 
individually solvated parts, unless the distance is very large. But I 
agree, that the problem you are reporting most likely does not result 
> from this end.

Regards

Andreas

Christopher Cramer wrote:

> Elmar,
>
> My textbook, Essentials of Computational Chemistry, actually has a 
> specific section (11.4.4 Potentials of Mean Force and Solvent 
> Structure) that mentions your problem. The issue is that continuum 
> models like the PCM variants involve the definition of a solute 
> cavity, typically defined as roughly the union of a set of van der 
> Waals spheres on all of the atoms. If you pull your solute apart, 
> breaking a bond, at some point you will exceed van der Waals contact 
> and the poor program has to decide what to do. It is quite unpleasant 
> to solve the Poisson equation with two cavities in a dielectric 
> continuum... If memory serves, PCM leaves some sort of neck between 
> the two for awhile, so that there is still a single cavity, but this 
> clearly soon becomes a bad approximation, since there is really 
> solvent there. At some point, the program probably just delivers an 
> error message (and a cryptic one, too, no doubt).
>
> But, if you compute the separated species individually, then there is 
> no problem at all. Each has a well defined cavity and is infinitely 
> far from anything but solvent. The two calculations will not agree, 
> since the cavities were defined very differently.
>
> The only widely used continuum model that does NOT suffer from this 
> discontinuity in a potential of mean force owing to cavity separation 
> is the Generalized Born model, which takes atomic radii as inputs but 
> does not use them to construct a formal cavity and is smooth and 
> continuous over all distances.
>
> If you would like to try a GB model, you are welcome to employ one of 
> our SMx solvation models, freely available in a variety of codes, 
> including SMxGAUSS, which can either read a Gaussian output file as 
> input and run as a stand-alone code, or can be driven by G03 using the 
> "external" keyword. See comp.chem.umn.edu/mccdir/software.htm for full 
> details.
>
> Best regards,
>
> Chris
>
> Begin forwarded message:
>
>     *From: *Elmar Gerwalin <elg/at/chemie.uni-kl.de>
>     *Date: *July 7, 2005 3:29:35 PM CDT
>     *To: *CHEMISTRY/at/ccl.net
>     *Subject: CCL: dissociation problem in PCM model ?
>     Reply-To: *chemistry/at/ccl.net
>
>     Hi,
>
>     I'm trying to describe dissociation processes in some small
>     organic molecules.
>     Therefore, I'm using B3LYP+SCRF(C-PCM, solvent=methanol) single
>     point jobs to get the
>     solvation energy at each step. Finally, a potential energy curve
>     E(R) is my goal.
>     R is the bond distance I'm interested in; e.g. a C-O, C-Cl bond or
>     , for testing purposes
>     Na-Cl.
>
>     But, unfortunately, wrong asymptotic behaviour (like a "size
>     inconsistency problem") is
>     observed in all cases: the "supermolecule's" solvation energy at
>     large distances (10 or 20 A)
>     is differing about more than 20 kcal/mole from the sum of the
>     solvation energies of the two ions.
>
>     My question is: is the problem known (references ?)? How can be it
>     be accounted for ?
>     Do I have to use specific energy terms given in gaussian's output
>     and/or male a correction to them ?
>
>     Any help is appreciated.
>
>     Bye,
>
>     Yours,
>     Elmar
>
>
>     -- 
>     ========================================================
>     Elmar Gerwalin , University of Kaiserslautern,Germany
>     Dept. of Theoretical Chemistry
>     elg/at/chemie.uni-kl.de
>     ========================================================
>
>
>
>     To send e-mail to subscribers of CCL put the string CCL: on your
>     Subject: line
>
>
>     Send your subscription/unsubscription requests to:
>     CHEMISTRY-REQUEST/at/ccl.net
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>     please
>
>
>
>
>
>
>
>
> -- 
>
> Christopher J. Cramer
> University of Minnesota
> Department of Chemistry
> 207 Pleasant St. SE
> Minneapolis, MN 55455-0431
> --------------------------
> Phone: (612) 624-0859 || FAX: (612) 626-2006
> Mobile: (612) 597-5275
> cramer/at/pollux.chem.umn.edu
> http://pollux.chem.umn.edu/~cramer
> (website includes information about the textbook "Essentials
> of Computational Chemistry: Theories and Models, 2nd Edition")
>
>


-- 
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COSMOlogic GmbH&CoKG
Burscheider Str. 515
51381 Leverkusen, Germany

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From chemistry-request@ccl.net Fri Jul  8 11:06:35 2005
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To: chemistry/at/ccl.net
Subject: Re: CCL: W:Solvation free energy for aromatic hydrocarbon
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I believe the confusion lies in the fact that a protein environment is not 
well described by assuming it is the same as the gas phase.  That phenyl 
group in the protein is still "solvated" by the surrounding protein.  The 
important energetic measure in that case is not the (de)solvation energy 
of the phenyl group in water, but the differential solvation energy of the 
phenyl group between water and the protein environment.

Given a standard state of 1M concentration in the gas phase and solution 
phase, and 298K, benzene has the following experimental solvation 
energies: -0.9 kcal/mol in water, -4.0 kcal/mol in n-hexane, and -4.6 
kcal/mol in benzene.

So you can see that transferring a benzene molecule from water to some 
hydrocarbon-like environment is exothermic by ~3-4 kcal/mol, and for 
similar reasons there is a negative (beneficial) energetic effect of 
transfering the phenyl ring from water into the protein environment.

Dave Giesen





"Chemical, , Bond" <chemicalbond001/at/yahoo.com>
Sent by: "Computational Chemistry List" <chemistry-request/at/ccl.net>
07/07/2005 04:07 PM
Please respond to chemistry

 
        To:     chemistry/at/ccl.net
        cc: 
        Subject:        CCL: W:Solvation free energy for aromatic hydrocarbon


Hi there,

I am confused with a single concept: what should be the sign for the 
solvation  free energy for a fragment like phenyl? 

There are many experimental data of solvation free energy for aromatic 
hydrocarbons, such as benzene, naphthalene, etc, but they are all negative 
surprisingly.  I looked at several papers with models of solvation energy, 
and their predictions all all have negative solvation energies for those 
compounds, just like the experiments.

Typically when a phenyl group is transfered from water into protein, we 
would like to say there is a negative(beneficial) desolvation energy, or 
the usual called hydrophobic effect.  And this has been used in tons of 
models for protein simulation or protein-ligand binding.  Note, in this 
context, the solvation energy (from gas into water) is positive! 

Is there something wrong over here?  Or just some artifact from the 
fitting?

Hope there would be some good comments.

Thanks a lot,
Bond


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From chemistry-request@ccl.net Fri Jul  8 12:54:39 2005
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From: "Jim Kress" <ccl_nospam$at$kressworks.com>
To: <chemistry$at$ccl.net>
Subject: RE: dissociation problem in PCM model ? 
Date: Fri, 8 Jul 2005 12:54:06 -0400
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As I understand your problem, you are trying to determine the E vs R curve
for the dissociation of a bond.  You have also found that the energy you get
at large R is inconsistent with what you expected with respect to the
expected dissociation products.  For example, in NaCl you find it does not
dissociate to Na + Cl but instead it dissociates to Na+ + Cl-.

Assuming my understanding is correct, what you have encountered is a classic
problem with HF or DFT (single determinant) wave function application.  This
is discussed in detail in the Computational Chemistry books by Jensen, by
Cramer, etc.

You need to use a different method to properly describe this dissociation.
Generalized Valence Bond (GVB) methods were developed by Goddard et al to do
this.  They are implemented in PCGAMESS (and GAMESS) and are reasonably
straightforward to apply.  You can also do a two configuration MCSCF or some
other size consistent approach that provides proper dissociation.

My preference in doing this for purposes like yours, is to use GVB.  If you
want some help contact me off the list.

Jim

> -----Original Message-----
> From: Jose Gascon [mailto:jose.gascon$at$yale.edu] 
> Sent: Thursday, July 07, 2005 9:52 PM
> To: chemistry$at$ccl.net
> Subject: CCL: dissociation problem in PCM model ? 
> 
> 
> Elmar, as I understand, DFT cannot be used to calculate 
> dissociation energies.
> Consider just the case of H2+ (the most trivial molecule). 
> Here you will get the wrong assimptotic value. In fact 
> Hartree-Fock will give you the exact answer.
> This is an intrinsic problem given by the fact that the 
> density functionals are not known exactly. In the case of H2+ 
> this results in an electron that can literally interact with itself.
> My suggestion is to use MP2 or QCISD if you can afford it.
> Best, jose
> 
> Elmar Gerwalin wrote:
> 
> >Hi,
> >
> >I'm trying to describe dissociation processes in some small 
> organic molecules.
> >Therefore, I'm using B3LYP+SCRF(C-PCM, solvent=methanol) 
> single point 
> >jobs to get the solvation energy at each step. Finally, a 
> potential energy curve E(R) is my goal.
> >R is the bond distance I'm interested in; e.g. a C-O, C-Cl bond or , 
> >for testing purposes Na-Cl.
> >
> >But, unfortunately, wrong asymptotic behaviour (like a "size 
> >inconsistency problem") is observed in all cases: the 
> "supermolecule's" 
> >solvation energy at large distances (10 or 20 A) is 
> differing about more than 20 kcal/mole from the sum of the 
> solvation energies of the two ions.
> >
> >My question is: is the problem known (references ?)? How can 
> be it be accounted for ?
> >Do I have to use specific energy terms given in gaussian's 
> output and/or male a correction to them ?
> >
> >Any help is appreciated.
> >
> >Bye,
> >
> >Yours,
> > Elmar
> >
> >
> >  
> >
> 
> --
> Jose A. Gascon - Postdoctoral Associate
> Department of Chemistry - (203)432-5911; jose.gascon$at$yale.edu 
> Yale University P.O. Box 208107 New Haven, CT 06520-8107.
> 
> 
> 
> 
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From chemistry-request@ccl.net Fri Jul  8 16:16:19 2005
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Date: Fri,  8 Jul 2005 16:17:35 -0300
From: khunter[at]mta.ca
To: CHEMISTRY[at]ccl.net
Subject: CCL Macromodel conformation search
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Was wondering if it was possible to do a conformational search with Macromodel 
where one is changing the puckering in a five membered ring.


From chemistry-request@ccl.net Fri Jul  8 14:30:34 2005
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Subject: RE: W:Symmetry breaking during CASSCF 
Date: Fri, 8 Jul 2005 14:29:43 -0400
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Jahn-Teller effect, perhaps?   Does the D2h geometry have degenerate orbitals which become non-degenerate once the symmetry is broken?

--David Shobe, Ph.D., M.L.S.
S|d-Chemie, Inc.
phone (502) 634-7409
fax (502) 634-7724

Don't bother flaming me: I'm behind a firewall.



-----Original Message-----
From: Computational Chemistry List [mailto:chemistry-request|at|ccl.net] On Behalf Of Gustavo, L.C., Moura
Sent: Friday, July 08, 2005 7:35 AM
To: chemistry|at|ccl.net
Subject: CCL: W:Symmetry breaking during CASSCF 

Dear CCL Readers,
     I have a planar conjugated organic molecule that, on paper, has D2h symmetry. I am working with the hypothesis that the molecule is a biradical singlet. I want to perform a CASSCF(2,2) on this molecule to estimate the biradical character of this molecule. When I calculate the molecule with the constraint that the molecule has D2h symmetry, the calculation has severe convergence problems. If I remove this constraint, the molecule distorts to a C2v symmetry and I obtain a biradical character ~20%. I checked the orbitals being used for the CASSCF calculation and they look right (one nonbonding and another slightly antibonding).
     Is the situation described above correct? Can an organic molecule have such a symmetry breaking as a result of a CASSCF calculation? Is the molecule really a C2v system? Any suggestions are welcome.
     Thank you very much in advance for your help.
     Sincerely yours,
                                Gustavo L.C. Moura
                           gustavo|at|mercury.chem.pitt.edu


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Subject: RE: W:Solvation free energy for aromatic hydrocarbon 
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From: "Shobe, David" <dshobe|at|sud-chemieinc.com>
To: <chemistry|at|ccl.net>
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1. Although benzene and water are immiscible in the sense that if you put 50 mL H2O and 50 mL C6H6 in a vessel, close it, and shake vigorously, you will get two liquid phases, not one.   However, there is an appreciable amount of water in the benzene phase, and an appreciable amount of benzene in the water phase. This  experimental evidence suggests that the free energy change from vapor phase* to a dilute solution in water is negative, but the free energy change from the liquid benzene phase to a more concentrated aqueous solution is positive.

2. The movement of the phenyl group from solution to protein is not DEsolvation; instead solvation by water is replaced with more favorable solvation by the protein.  

3. Phenyl groups (in this context) don't usually migrate by themselves; they are attached to some molecule.  So the positive solvation energy of the phenyl group may actually represent the difference between the solvation energy of alanine v. phenylalanine, or of some other pair of molecules differing by a phenyl group.

--David Shobe, Ph.D., M.L.S.
S|d-Chemie, Inc.
phone (502) 634-7409
fax (502) 634-7724

Don't bother flaming me: I'm behind a firewall.

*The experiment uses liquid benzene but under ambient conditions the liqud-vapor equilibrium favors the liquid.  If vapor to liquid is negative and liquid to dilute aq. soln. is negative, then vapor to dilute aq. soln. is negative also. 

-----Original Message-----
From: Computational Chemistry List [mailto:chemistry-request|at|ccl.net] On Behalf Of Chemical, , Bond
Sent: Thursday, July 07, 2005 4:08 PM
To: chemistry|at|ccl.net
Subject: CCL: W:Solvation free energy for aromatic hydrocarbon 

Hi there,

I am confused with a single concept: what should be the sign for the solvation  free energy for a fragment like phenyl?  

There are many experimental data of solvation free energy for aromatic hydrocarbons, such as benzene, naphthalene, etc, but they are all negative surprisingly.  I looked at several papers with models of solvation energy, and their predictions all all have negative solvation energies for those compounds, just like the experiments.

Typically when a phenyl group is transfered from water into protein, we would like to say there is a negative(beneficial) desolvation energy, or the usual called hydrophobic effect.  And this has been used in tons of models for protein simulation or protein-ligand binding.  Note, in this context, the solvation energy (from gas into water) is positive! 

Is there something wrong over here?  Or just some artifact from the fitting?

Hope there would be some good comments.

Thanks a lot,
Bond


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