Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: al220007 on November 22, 2022, 04:47:37 PM
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I was calculating some oxidation states but I couldn't solve 3 of the compounds my teacher gave:
I know O has oxidation state equals -2 in all of them and Cl on the first compound hasn't oxidation state equals -1 because it's bonded with an O but now I'm stuck.
How should I solve them? Is there any rule I'm missing?
Thanks in advance! ;)
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Would writing these compound dissociated to ions help?
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I know O has oxidation state equals -2 in all of them and Cl on the first compound hasn't oxidation state equals -1 because it's bonded with an O but now I'm stuck.
In neutral compound (not cation or anion) sum of the all oxidations states is equal 0.
Cr(ClO3)3 is a salt, it dissociate to cation and anion.
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Would writing these compound dissociated to ions help?
I hope I did it right:
- Cr(ClO3)3 --> Cr3+ + 3ClO3-
- ZnSO4 --> Zn2+ + SO42-
- Al2(SO4)3 --> 2Al3+ + 3SO42-
Now I calculated the oxidation state of each one separatedly and I think the result it's correct!
Example with Cr(ClO3)3
3 + 3(5 + 3(-2)) = 0 | | | +3 = 3 | | | +5 - 2 = -1 |
Cr(ClO3)3 | | | Cr3+ | | | 3ClO3- |
I just need to review the ions charges.
Thank you <3
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Looks OK.