What are the oxidation states of the metal in #FeCl_4^(2-)# and #Cr_2O_7^(2-)#?

1 Answer
anor277
May 28, 2017

We has #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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