write a balanced half - reaction describing the oxidation of aqueous chromium(ii) cations to aqueous…

Explanation:

Step1: Determine the oxidation state change

Chromium goes from +2 (in (Cr^{2+})) to +4 (in (Cr^{4+})). The change in oxidation state is (+4-(+2) = + 2).

Step2: Write the basic form of the half - reaction

The basic form is (Cr^{2+}\to Cr^{4+}).

Step3: Balance the charge

Since the oxidation state of Cr increases by 2, we need to balance the charge by losing 2 electrons. So the balanced half - reaction is (Cr^{2+}\to Cr^{4+}+2e^{-}).

Answer:

(Cr^{2+}\to Cr^{4+}+2e^{-})