Questions: The strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy. (A) C=N (B) C ≡ N (A,B) (C) C-C (D) C ≡ C (C,D) Submit Answer Retry Entire Group 8 more group attempts remaining

The strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds.

For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy.
(A) C=N
(B) C ≡ N
(A,B)
(C) C-C
(D) C ≡ C
(C,D)
Submit Answer
Retry Entire Group
8 more group attempts remaining

Transcript text: The strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy. (A) $\mathrm{C}=\mathrm{N}$ (B) $\mathbf{C} \equiv \mathrm{N}$ (A,B) $\square$ (C) C-C (D) $C \equiv C$ (C,D) $\square$ Submit Answer Retry Entire Group 8 more group attempts remaining

Solution

Solution Steps

Step 1: Understanding Bond Energy

Bond energy is the measure of bond strength in a chemical bond. It is the amount of energy required to break one mole of bonds in a substance in the gas phase. Generally, shorter bonds are stronger and have higher bond energies.

Step 2: Analyzing the First Pair

For the first pair:

(A) $\mathrm{C}=\mathrm{N}$ is a double bond.
(B) $\mathbf{C} \equiv \mathrm{N}$ is a triple bond.

Triple bonds are generally stronger and have higher bond energies than double bonds because they involve more shared electrons and are shorter.

Step 3: Analyzing the Second Pair

For the second pair:

(C) C-C is a single bond.
(D) $C \equiv C$ is a triple bond.

Again, triple bonds are stronger and have higher bond energies than single bonds due to the increased number of shared electrons and shorter bond length.