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Topic: Don't know what to call it  (Read 2450 times)

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Offline Montegue

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Don't know what to call it
« on: June 07, 2013, 08:46:12 PM »
This compound is interesting.

[Cr(H20)4Cl2]Cl

By guessing, I break it into [Cr(H20)4Cl2]+ and Cl-.

I supposed that (H20)4 is neutral, but inside the square bracket, excluding (H20)4,
Cr+6 and Cl2- don't add up to +1 charge.

How come?
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Offline Corribus

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Re: Don't know what to call it
« Reply #1 on: June 07, 2013, 09:28:35 PM »
Why are you sure the chromium is +6?
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What men are poets who can speak of Jupiter if he were like a man, but if he is an immense spinning sphere of methane and ammonia must be silent?  - Richard P. Feynman

Offline Montegue

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Re: Don't know what to call it
« Reply #2 on: June 07, 2013, 11:19:33 PM »
Why not?
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Offline Corribus

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Re: Don't know what to call it
« Reply #3 on: June 07, 2013, 11:25:43 PM »
You answered that in your first post.
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What men are poets who can speak of Jupiter if he were like a man, but if he is an immense spinning sphere of methane and ammonia must be silent?  - Richard P. Feynman

Offline Arkcon

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Re: Don't know what to call it
« Reply #4 on: June 08, 2013, 10:11:23 AM »
The topic you're trying to understand is called co-ordination compounds. http://en.wikipedia.org/wiki/Coordination_complex  The Wikipedia article is a good starting point for this general concept -- strict ion charges don't apply to forming these compounds, the various ligands share their s and p orbitals with the central metal's d orbital.
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Offline Montegue

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Re: Don't know what to call it
« Reply #5 on: June 08, 2013, 12:07:41 PM »
Thank you, Arkcon. That's the answer I was looking for. It's very helpful. After I read it, I found that the oxidation state of Cr is +3 because of the total charge of the ligands.
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