Question

Which of the following bonds requires the largest amount of bond energy to dissociate the atom concerned
A.\[H - H\] bond in hydrogen
B.\[C - C\] bond in methane
C.\[N \equiv N\] bond in nitrogen
D.\[O = O\] bond in oxygen
E.\[C - C\] bond in ethane

Answer 1

Hint: The bond-dissociation energy is defined as the standard enthalpy change when a bond is broken down.
It is an estimation of strength.

Complete step by step solution:Largely chemical conversion is all about the formation and dissociation of bonds.
Chemical bonds are built when electrostatic forces between atoms undergo combination. Chemical bonds can simply be broken down with the application of energy.
The bond dissociation energy is the quantity of energy required to break up a chemical bond. It refers to the amount of energy needed to provide a chemical bond between two molecules.
It is a path to specify how powerful a chemical bonding is.
It is identical to the bond energy level, especially in diatomic compounds.
The bond dissociation energies of covalent bonds are weak.
Here in this question, we have to find out which of the following bonds requires the largest amount of bond energy to dissociate the atom concerned.
The N≡N bond in nitrogen has the highest bond dissociation energy as it is a strong triple bond.
Its bond energy is 945 KJ/mol.

So, option C is correct.

Note: Bond dissociation energy is a state function and therefore does not rely on the way by which it occurs.
For chemical reactions, the addition and subtraction of bond dissociation energies for bonds created and bonds broken in a chemical reaction can be calculated using Hess's Law.