Chemistry - CHEMICAL BONDING Question with Solution | TestHub

From the given valence electrons:

A = B (2nd period, 5 valence e⁻), D = N (6 valence e⁻), E = O (6 valence e⁻).

A₂⁺ = B₂⁺ → Bond order = 1.5

D₂ = N₂ → Bond order = 3

E₂ = O₂ → Bond order = 2

E₂²⁻ = O₂²⁻ → Bond order = 1

Bond length is inversely proportional to bond order. Hence: N₂ (D₂) < O₂ (E₂) < O₂²⁻ (E₂²⁻).

Therefore:

(A) True: D₂ has shorter bond length than E₂.

(B) True: A₂⁺ (BO = 1.5) and D₂⁺ (N₂⁺, BO = 2.5) have comparable bond lengths in the given trend question.

(C) False.

(D) False, because in B₂⁺ the electron is removed from a π(2p) degenerate MO, not a non-degenerate MO.