Zn has a much lower enthalpy of atomisation than V. The correct explanation is

ABoth use only the two 4s electrons, but V has a larger atomic number
BZn has more electrons and therefore stronger metallic bonding
CV has 3 unpaired 3d electrons that take part in metallic bonding along with the 4s electrons, while the $3 d^{10}$ shell of Zn does not
DZn uses its filled 3d electrons for strong bonding but V does not

Answer: C

V is

3 d^{3} 4 s^{2}

and can use its unpaired

3 d

electrons in addition to

4 s

in metallic bonding, giving a high enthalpy of atomisation. Zn is

3 d^{10} 4 s^{2}

with no unpaired d electrons, so only the

4 s^{2}

pair contributes and the bonding is weak. This is why Zn also has a low melting point.