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.

Among the elements mentioned below, some are not stable in their +3 oxidation state and undergoes disproportionation reactions easily

A. N

B. P

C. As

D. Sb

E. Bi

Choose the correct answer from the options given below:

N and P only

The correct answer is option 3. N and P only. 

Nitrogen typically forms compounds in various oxidation states ranging from -3 to +5. However, it is relatively unstable in the +3 oxidation state. Compounds of nitrogen in the +3 oxidation state, such as ammonia borane (\(NH_3BH_3\)), are not stable and can undergo disproportionation reactions. In disproportionation reactions, a single species simultaneously undergoes both oxidation and reduction. For nitrogen in the +3 oxidation state, it tends to either gain or lose electrons to form more stable nitrogen compounds in different oxidation states, rather than remaining in the +3 state.

Phosphorus shares a similar behavior with nitrogen. While phosphorus can form compounds in various oxidation states, it is relatively unstable in the +3 oxidation state. Compounds of phosphorus in the +3 oxidation state, such as phosphine (\(PH_3\)), are not stable and can readily undergo disproportionation reactions. Like nitrogen, phosphorus tends to undergo reactions where it gains or loses electrons to form more stable compounds in different oxidation states.

Arsenic (As), Antimony (Sb), and Bismuth (Bi) are more stable in their +3 oxidation states compared to nitrogen and phosphorus. Compounds of arsenic, antimony, and bismuth in the +3 oxidation state are relatively stable and do not undergo disproportionation reactions as readily as nitrogen and phosphorus. Arsenic, antimony, and bismuth compounds tend to maintain their +3 oxidation state without undergoing simultaneous oxidation and reduction reactions under normal conditions.

Therefore, the elements nitrogen and phosphorus exhibit a tendency to undergo disproportionation reactions due to the instability of their +3 oxidation states, while arsenic, antimony, and bismuth are more stable in their +3 oxidation states. This explains why only nitrogen and phosphorus are mentioned as elements that are not stable in their +3 oxidation state and undergo disproportionation reactions easily.