Write a net ionic equation for the following: Acidified solutions of sodium dichromate and copper (I) bromide are mixed?
I know that the #Cr_2O_7^{2-}# will reduce to #Cr^{3+}# , but what isn't immediately obvious to me is why #Cu^+# is oxidized into #Cu^{2+}# how do we know necessarily that the copper oxidizes, and that it specifically oxidizes to copper(II).
There was also another problem where #Fe^{2+}# was oxidized to #Fe^{3+}# . In general, how do we know whether or not the metals oxidize, and what specifically they oxidize to.
I know that the
There was also another problem where
1 Answer
Well, usually these redox equations follow standard protocols....
Explanation:
Here, we know that red-orange dichromate ion, a potent oxidant, is reduced to green
And for every reduction there is a corresponding oxidation...
And so for the final redox process we take...
....the which I think is balanced with respect to mass and charge...