Question

In the molecules \( {CH}_4 \), \( {NF}_3 \), \( {NH}_4^+ \) and \( {H}_2{O} \),

• A. The number of lone pairs are the same.
• B. All have the same hybridization of the central atom.
• C. The bond angles are the same.
• D. The number of bond pairs are the same.

Hint:

Molecules with \( sp^3 \) hybridization have a tetrahedral geometry. In molecules like \( {CH}_4 \), \( {NF}_3 \), \( {NH}_4^+ \), and \( {H}_2{O} \), the central atom exhibits \( sp^3 \) hybridization, although the number of bond pairs and lone pairs may vary.

Answer 1

The Correct Option is B

Let us examine the hybridization of the central atoms in each molecule: - \( {CH}_4 \): The central atom is carbon, which has 4 bond pairs and no lone pairs. This gives it an \( sp^3 \) hybridization. - \( {NF}_3 \): The central atom is nitrogen, which has 3 bond pairs and 1 lone pair. This gives it an \( sp^3 \) hybridization. - \( {NH}_4^+ \): The central atom is nitrogen, which has 4 bond pairs and no lone pairs due to the positive charge. This also gives it an \( sp^3 \) hybridization. - \( {H}_2{O} \): The central atom is oxygen, which has 2 bond pairs and 2 lone pairs. This gives it an \( sp^3 \) hybridization. Thus, all these molecules have \( sp^3 \) hybridization on their central atoms. 
Therefore, the correct option is B. 
- Option A: This is incorrect because the number of lone pairs is not the same for all molecules. 
- Option C: This is incorrect because the bond angles are not the same for all molecules. For example, \( {CH}_4 \) has 109.5° bond angles, while \( {H}_2{O} \) has 104.5° bond angles. 
- Option D: This is incorrect because the number of bond pairs is different for each molecule. 
Thus, the correct answer is Option B.