In which of the following bond angle is maximum?
— To determine the bond angle, we need to consider the hybridization and molecular geometry of each species.
To determine the bond angle, we need to consider the hybridization and molecular geometry of each species. The presence of lone pairs significantly affects bond angles.
Step 1: Analyze the hybridization and geometry of NH3
In NH3, nitrogen is sp3 hybridized. It has three bond pairs and one lone pair. The geometry is trigonal pyramidal, and due to the lone pair-bond pair repulsion, the bond angle is approximately 107°.
Step 2: Analyze the hybridization and geometry of NH4+
In NH4+, nitrogen is sp3 hybridized. It has four bond pairs and no lone pairs. The geometry is tetrahedral, and the bond angle is ideally 109.5°.
Step 3: Analyze the hybridization and geometry of H2O
In H2O, oxygen is sp3 hybridized. It has two bond pairs and two lone pairs. The geometry is bent or V-shaped, and due to two lone pair-bond pair repulsions, the bond angle is approximately 104.5°.
Step 4: Analyze the hybridization and geometry of SCl2
In SCl2, sulfur is sp3 hybridized. It has two bond pairs and two lone pairs. Similar to H2O, the geometry is bent or V-shaped. The bond angle is approximately 103° (due to larger size of Cl atoms and lone pair repulsions).
Step 5: Compare the bond angles
- NH3: ~107°
- NH4+: 109.5°
- H2O: ~104.5°
- SCl2: ~103°
Comparing these values, NH4+ has the maximum bond angle.
Correct Answer: (B)