The characteristics of elements $\mathrm{X}, \mathrm{Y}$ and $Z$ with atomic numbers, respectively, 33, 53 and 83 are:  

The element $\mathrm{X}$ with atomic number $=33$, its electronic configuration of the atomic number will be $1{ \mathrm{s}}^{2}2{ \mathrm{s}}^{2}2{\mathrm{p}}^{6}3{ \mathrm{s}}^{2}3{\mathrm{p}}^{6}4{ \mathrm{s}}^{2}3{ \mathrm{d}}^{10}4{\mathrm{p}}^3$ So, its configuration is similar to 15th group and it has 5 valence electrons.

This group has nitrogen, phosphorus, arsenic, antimony, and bismuth as its members. Additionally, its first two elements are known to show non-metallic properties, while arsenic and antimony are known to show properties of metalloids and bismuth is metallic in nature.

The element $\text{Y}$ with atomic number $=53$ has an electronic configuration $1{ \mathrm{s}}^{2}2{ \mathrm{s}}^{2}2{\mathrm{p}}^{6}3{ \mathrm{s}}^{2}3{\mathrm{p}}^{6}3{ \mathrm{d}}^{10}4{ \mathrm{s}}^{2}4{\mathrm{p}}^{6}4{ \mathrm{d}}^{10}5{ \mathrm{s}}^{2}5{\mathrm{p}}^5$ which represents iodine.

lodine is a Group 17 element as it contains 7 valence electrons in its outermost shell. It is a nonmetal because it belongs to the halogen period. The element $\mathrm{Z}$ with atomic number $=83$ has a configuration $1{ \mathrm{s}}^{2}2{ \mathrm{s}}^{2}2{\mathrm{p}}^{6}3{ \mathrm{s}}^{2}3{\mathrm{p}}^{6}4{ \mathrm{s}}^{2}3{ \mathrm{d}}^{10}4{\mathrm{p}}^{6}5{ \mathrm{s}}^{2}4{ \mathrm{d}}^{10}5{\mathrm{p}}^{6}6{ \mathrm{s}}^{2}4{\mathrm{f}}^{14}5{ \mathrm{d}}^{10}6{\mathrm{p}}^3$

It lies in the p-block as its last electron lies in the $\mathrm{p}$-orbital. So, it is the only metal contained in Group 15.

Hence, the required option is D.