Given below are two statements :
Statement I : The N-N single bond is weaker and longer than that of P-P single bond
Statement II : Compounds of group 15 elements in +3 oxidation states readily undergo disproportionation reactions.
In the light of the above statements, choose the correct answer from the options given below

To determine the correct answer, we analyze both statements using the chemical properties and periodic trends of Group 15 elements.

The first statement asserts that the $$N-N$$ single bond is weaker and longer than the $$P-P$$ single bond. Nitrogen has a much smaller atomic radius than phosphorus, resulting in significant lone pair-lone pair repulsions between the two bonded nitrogen atoms. These repulsions weaken the $$N-N$$ single bond, making it less stable than the $$P-P$$ bond. However, because nitrogen atoms are smaller than phosphorus atoms, the $$N-N$$ bond is shorter, not longer, than the $$P-P$$ bond. Therefore, Statement I is false.

The second statement claims that compounds of Group 15 elements in the $$+3$$ oxidation state readily undergo disproportionation reactions. While certain compounds such as $$HNO_2$$ and $$H_3PO_3$$ can undergo disproportionation under suitable conditions, this behavior is not common to all Group 15 elements. As we move down the group, the inert pair effect becomes increasingly significant, stabilizing the $$+3$$ oxidation state, particularly for heavier elements such as bismuth. Consequently, $$Bi^{3+}$$ compounds are relatively stable and do not readily disproportionate. Hence, Statement II is also false.

Therefore, both statements are incorrect.

Correct Answer: Both Statement I and Statement II are false.