Answer the question on the basis of passage given below:

Second period elements of p-Block differ from the rest of their group members due to their small atomic size, high electronegativity, high ionization enthalpy and absence of d-orbitals.

The elements from the second period like C, N, O have unique property of forming pa pa multiple bonds whereas other heavier elements of p-block form da pa multiple bonds. This changes the properties of second period elements to great extent. Also the single bond strength of the p-block elements with their own atoms gets affected by their atomic size and presence of lone pairs.

Inert pair effect also affects the properties of the p-Block elements especially for those elements which are present from 4th period onward and this happens due to poor screening effect of inner (n-1) d subshell electrons.

The decreasing order of melting point of the following elements will be:-

A. Nitrogen (N)

B. Phosphorus (P)

C. Arsenic (As)

D. Antimony (Sb)

E. Bismuth (Bi)

Choose the correct answer from the options given below:

As > Sb > Bi > P > N

The correct answer is option 1. As > Sb > Bi > P > N.

The given elements are:

C. Arsenic (As): Arsenic is a metalloid with both metallic and non-metallic properties. It has a relatively high melting point compared to the other elements listed. Arsenic exhibits metallic bonding, where its electrons are delocalized over the atomic lattice, contributing to the strength of the bonds. This strong metallic bonding results in a higher melting point for arsenic.

D. Antimony (Sb): Antimony is also a metalloid and follows arsenic in the decreasing order of melting points. It exhibits similar metallic properties to arsenic, with metallic bonding contributing to its melting point. While antimony has a lower melting point than arsenic, it still has a higher melting point than bismuth, phosphorus, and nitrogen.

E. Bismuth (Bi): Bismuth is a post-transition metal with weaker metallic bonding compared to arsenic and antimony. Although it still exhibits metallic properties, the metallic bonding in bismuth is weaker, leading to a lower melting point compared to arsenic and antimony.

B. Phosphorus (P): Phosphorus is a non-metal and exists in various allotropes, such as white phosphorus and red phosphorus. In its solid state, phosphorus forms covalent bonds between its atoms. These covalent bonds are relatively strong, resulting in a higher melting point compared to nitrogen.

A.Nitrogen (N): Nitrogen has the highest melting point among the given elements. Nitrogen exists as diatomic molecules (\(N_2\)) with triple bonds between nitrogen atoms. Breaking these strong covalent bonds requires a significant amount of energy, resulting in a higher melting point compared to the other elements listed.

In summary, the correct order of decreasing melting points is: As > Sb > Bi > P > N. This order is based on the strength of metallic bonding for arsenic and antimony, the weaker metallic bonding for bismuth, and the strength of covalent bonds for phosphorus and nitrogen.