I was making more of a guess than anything about the number of bonds
attached to the chromate. I thought that since most molecules are more
stable with a certain number of bonds (i.e. Oxygen with 2, carbon with 4)
that chromate would be the same way... I do realize that since chrominum
is a transition metal that it might be a little different. Anyone else
have any thoughts??
On Wed, 11 Dec 1996 hilleskl@plu.edu wrote:
>
> Kari,
>
> I was wondering if you could explain why the number of bonds on the
> chromate molecules you mentioned in your message below would affect the
> stability of the molecule.
>
> Kristina
>
> On Wed, 11 Dec 1996, Kari Fosser wrote:
>
> >
> > I'm not sure if this has been answered yet, but to answer your question,
> > the ester is not isolated because its surrounded by water molecules.
> > Since they are all around its very likely that the water will attack the
> > ester to form the ketone. As for stability: the chromate ester has 7
> > bonds compared to the chromic acid (6) and chromate ion (4 +electron pair)
> > That probably has something to do with the ester's unstability.
> >
> > Kari
> >
> > On Tue, 10 Dec 1996 johnstsl@plu.edu wrote:
> >
> > > On page 476 in Solomons below the mechanism for the formation of the
> > > chromate ester, it states that the chromate ester is "unstable and is not
> > > isolated". Does anyone know why this is? The atoms around the Cr
> > > in the chromium ester seem to have nearly the same structure as the atoms
> > > surrounding the Cr in the chromium ion. Does this matter?
> > >
> > > thanks! =)
> > >
> > > JOHNSTSL@PLU.EDU
> > >
> > >
> >
> >
>
>