Bond Parameters

The problem requires determining the correct order of bond angles for the molecules , , , and . To resolve this, we must understand the molecular geometry and associated bond angles for each molecule:

: Silicon tetrachloride adopts a tetrahedral geometry, giving it bond angles of 109.5°.

: Sulfur trioxide has a trigonal planar shape, with bond angles of 120°.

: Ammonia exhibits a trigonal pyramidal shape due to a lone pair, resulting in a bond angle of approximately 107°.

: Mercury(II) chloride forms a linear structure, which leads to bond angles of 180°.

Given these geometries, the order from largest to smallest bond angles is:

• (180°)
• (120°)
• (109.5°)
• (107°)

Thus, the correct order is: .

To determine the bond angles b₁, b₂, b₃, we need to analyze the structure shown in the accompanying image. Bond angles are influenced by the hybridization and spatial arrangement of atoms in molecules.

1. Determine the electronic geometry and hybridization:
In molecules, bond angles depend on the hybridization state of the central atom. The typical angles are:

• sp³ hybridization → approximately 109.5°
• sp² hybridization → approximately 120°
• sp hybridization → 180°

2. Identify and match angles with options:
Given that the correct set of angles is 118°, 79°, 101°, and assuming the molecular structure contains distortions from ideal geometries:

• An angle of 118° could correspond to a slightly distorted sp² geometry.
• The small angle 79° may result from steric strain or a ring structure imposing sharp bond angles.
• The intermediate angle 101° may arise from a distorted tetrahedral or irregular trigonal geometry.

3. Conclusion:
Based on molecular geometry considerations and the provided data, the correct bond angle assignments are:
b₁ = 118°, b₂ = 79°, b₃ = 101°, indicating deviations from ideal hybridized geometries due to structural distortions.