What are the oxidation states of the metal in $F e C l_{4}^{2 -}$ $FeCl_4^(2-)$ and $C r_{2} O_{7}^{2 -}$ $Cr_2O_7^(2-)$ ?

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What are the oxidation states of the metal in $F e C l_{4}^{2 -}$ $FeCl_4^(2-)$ and $C r_{2} O_{7}^{2 -}$ $Cr_2O_7^(2-)$ ?

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Answer 1 · 2017-05-28T06:43:22

We has $F e (I I +)$ $Fe(II+)$ , and $Cr(VI+).........$

Explanation:

$"Chromate ion"$ $-=$ $CrO_4^(2-)$ .

The typical oxidation state of oxygen is $-II$ , and it is here. And since the sum of the oxidation states equals the charge on the ion, which is $-2$ , $Cr_"oxidation number"+4xx(-2)=-2$

$Cr_"oxidation number"=Cr(VI+)$ .

What about $"dichromate"$ , $Cr_2O_7^(2-)$ ?

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What are the oxidation states of the metal in $F e C l_{4}^{2 -}$ $FeCl_4^(2-)$ and $C r_{2} O_{7}^{2 -}$ $Cr_2O_7^(2-)$ ?

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What are the oxidation states of the metal in FeCl_4^(2-)FeCl2−4FeCl_4^(2-) and Cr_2O_7^(2-)Cr2O2−7Cr_2O_7^(2-)?

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What are the oxidation states of the metal in $F e C l_{4}^{2 -}$ $FeCl_4^(2-)$ and $C r_{2} O_{7}^{2 -}$ $Cr_2O_7^(2-)$ ?