Question #30c1c

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Question #30c1c

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Answer 1 · 2014-11-05T06:30:11

The oxidation states of the $C_{2} O_{4}^{- 2}$ $C_2O_4^-2$ ion are
$C^{+ 3}$ $C^(+3)$ and $O^{- 2}$ $O^-2$ .

Explanation:

$C_{2} O_{4}$ $C_2O_4$ oxalate is a polyatomic ion with a charge of -2.

The oxygen atoms in this molecule have a oxidation state of -2, vecause oxygen is always a -2 charge. Since there are 4 atoms of oxygen the overall charge of the oxygen atoms is 4(-2) = -8.

Since the total charge of oxalate is -2 the charge created by the carbon atoms must be +6. (-8 +6 = -2) this means that each carbon atom must have an oxidation state of +3. (+6/2 = +3)

The oxidation states of the $C_{2} O_{4}^{- 2}$ $C_2O_4^-2$ ion are
$C^{+ 3}$ $C^(+3)$ and $O^{- 2}$ $O^-2$

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