Question

Match the bond enthalpies given in column II with the molecules given in column I and mark the mark the appropriate choice.

Column I	Column II
(A) Hydrogen$(H_{2})$	(i) $498.0KJmol^{- 1}$
(B) Oxygen $(O_{2})$	(ii) $946.0KJmol^{- 1}$
(C) Nitrogen $(N_{2})$	(iii) $435.8KJmol^{- 1}$

• A. (A) $\rightarrow$ (i), (B) $\rightarrow$ (ii), (C) $\rightarrow$ (iii)
• B. (A) $\rightarrow$ (iii), (B) $\rightarrow$ (ii), (C) $\rightarrow$ (i)
• C. (A) $\rightarrow$ (i), (B) $\rightarrow$ (iii), (C) $\rightarrow$ (ii)
• D. (A) $\rightarrow$ (iii), (B) $\rightarrow$ (i), (C) $\rightarrow$ (ii)

Answer 1

Answer: (D)

(A) $\rightarrow$ (iii), (B) $\rightarrow$ (i), (C) $\rightarrow$ (ii)

Answer 2

: The order of bond enthalpies of the bonds is given as, Bond order $\propto$Bond enthalpy

Hence, single bond enthalpy < double bond enthalpy < triple bond enthalpy

$H - H < O = O < N \equiv N$