Here is the overall reaction of a mercury oxide dry cell: zn + hgo --> zno + hg. in this reaction, which of the following gets oxidized?

a. hg

b. o

c. zn

d. hgo

Zinc is oxidized because it starts as a metal with an oxidation state of zero and ends up as an atom bound to oxygen. Oxygen has two bonds, so the oxidation state of Zinc would be 2. The Mercury is therefore reduced because it undergoes the opposite process. This is a REDOX reaction, and the two half-reactions are: 

Zn -> Zn(+2) + 2e(-) 
Hg(+2) + 2e(-) -> Hg

The answer to your question is C. I hope that this is the answer that you were looking for and it has helped you.

Part -1

Electrode A - Mg(s)

Electrode B -

Part-2

Option -C

Part - 3

Electrons flow from electrode -A to electrode -B.

Explanation:

Part-1

Electrode A is

Electrode B is

Part-2

From the electrode, magnesium looses two electrons and chlorine gains two electrons. Therefore, balanced redox equation for the voltaic cell is as follows.

Part-3

ions flow from the left to right.

ions flow from the right to left.

Therefore, Electrons flow from electrode -A to electrode -B.