Ode Coyote wrote:

> Dissolved Compounds still remain those compounds and don't change into
> something else when the water is removed.
>  A free silver ion isn't likely to be very stable and very much wants to
> share an electron with something.

Solutions by their very nature are always neutral.  If you have an Ag+ ion,
there has to be a (-) ion to balance it. The two together will define the
compound.  For freshly made EIS the negative ion is the hydroxyl ion, IE OH-,
so the silver compound in EIS is actually silver hydroxide.  At higher
concentrations, silver hydroxide tends to become unstable, and will
spontaneouly convert to silver oxide.  This could be part of the aging process
that occurs when EIS sits, not sure.

>
>
>  Question:
>  Does it HAVE to "share", or can it's desires be passified as an 'onlooker'
> or 'groupie', so to speak?
> Can a free silver ion 'associate' [identify?] itself... around and with...
> a water molecules opposite valence oxygen componant and become at least
> 'more' stable  without actually becoming a 'compound' made from out of that
> water molecule? ...a protective attraction vs an absolute reaction..

A silver ion will tend to attact the OH portion of a water molecule, producing
silver hydroxide.  The remaining H will find a matching one, and form H2 which
may remain dissolved or be outgassed over time.

>
>
> Can a cluster of silver atoms that include one or more ions on it's surface
> to present an ionic 'appearance' to the water molecules also be included in
> such an attraction?

A cluster of silver atoms do often obtain a charge.  They are not ions per say
I don't believe but just a cluster with a charge.  The charge is referred to as
the zeta when it is measured. The higher the charge or zeta, the more stable
the colloidal portion is. If they have no charge, then they will precipitate.

Marshall

>
>
> Warning:  Any in depth explanation one way or the other will probably
> confuse me.
>  Simple answers?  Yes, no , maybe sometimes?
>
> Ode
>
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