Question

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

	Column $I$		Colum $II$
(A)	Hydrogen $(H_2)$	(i)	$498.0kJmo{l}^{-}1$
(B)	Oxygen $(0_2)$	(ii)	$946.0kJmo{l}^{-}1$
(C)	Nitrogen $(N_2)$	(iii)	$435.8kJmo{l}^{-}$

• A. $\left(A\right)\to \left(i\right),\left(B\right)\to \left(ii\right),\left(C\right)\to \left(iii\right)$
• B. $\left(A\right)\to \left(iii\right),\left(B\right)\to \left(ii\right),\left(C\right)\to \left(i\right)$
• C. $\left(A\right)\to \left(i\right),\left(B\right)\to \left(iii\right),\left(C\right)\to \left(ii\right)$
• D. $\left(A\right)\to \left(iii\right),\left(B\right)\to \left(i\right),\left(C\right)\to \left(ii\right)$

Answer 1

Answer: (D)

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
$H—H<O=O<N\equiv N$