Match the bond enthalpies given in column II with the molecules given in column I and mark the appropriate choice.
Column I
Column II
a.
Hydrogen $$\left( {{H_2}} \right)$$
1.
$$498.0\,kJ\,mo{l^{ - 1}}$$
b.
Oxygen $$\left( {{O_2}} \right)$$
2.
$$946.0\,kJ\,mo{l^{ - 1}}$$
c.
Nitrogen $$\left( {{N_2}} \right)$$
3.
$$435.8\,kJ\,mo{l^{ - 1}}$$
A.
a - 1, b - 2, c - 3
B.
a - 3, b - 2, c - 1
C.
a - 1, b - 3, c - 2
D.
a - 3, b - 1, c - 2
Answer :
a - 3, b - 1, c - 2
Solution :
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
i.e., $$H - H < O = O < N \equiv N$$
Releted MCQ Question on Inorganic Chemistry >> Chemical Bonding and Molecular Structure
Releted Question 1
The compound which contains both ionic and covalent bonds is