Answer the question on the basis of passage given below:
Nitrogen differs from rest of the members of group 15 due to its small size, high electronegativity, high ionization enthalpy and non-availability of d orbitals. Nitrogen has unique ability to form \(p\pi -p\pi \) multiple bonds with itself and with other elements having small size and high electronegativity. Heavier elements of this group do not form \(p\pi -p\pi \) bonds as their atomic orbitals are so large and diffuse that they cannot have effective overlapping.
Group 15 elements forms oxides of type \(E_2O_3\). Acidic oxides are formed by
A. Bi
B. Sb
C. P
D. As
E. N
Choose the correct answer from the options given below:
Answer & explanation
Correct answer: option 3
The correct answer is Option (3) → C and E only
All Group 15 elements form oxides of the type E2O3 and E2O5. As metallic character increases down the group, the acidic character of the oxides decreases:
(A) Bi — False. \( \ce{Bi2O3} \) is predominantly basic.
(B) Sb — False. \( \ce{Sb2O3} \) is amphoteric.
(C) P — True. \( \ce{P2O3} \) (\( \ce{P4O6} \)) is purely acidic.
(D) As — False. \( \ce{As2O3} \) is amphoteric.
(E) N — True. \( \ce{N2O3} \) is purely acidic.
Note: This question is from the pre-rationalised NCERT book (2022-23). The topic is not there in the latest NCERT book (2026-27), and it is also out of the CUET 2026 syllabus.
NCERT (Pre-rationalised edition, 2022-23):
Reactivity towards Oxygen – “All these elements form two types of oxides: E2O3 and E2O5. The oxide in the higher oxidation state of the element is more acidic than that of lower oxidation state. Their acidic character decreases down the group. The oxides of the type E2O3 of nitrogen and phosphorus are purely acidic, that of arsenic and antimony amphoteric and those of bismuth is predominantly basic.”