Question

The geometry around boron in the product ‘B’ formed from the following reaction is

• A. Trigonal planar
• B. Tetrahedral
• C. Pyramidal
• D. Square planar

Answer 1

The Correct Option is B

To determine the geometry around boron in the product 'B', we first need to understand the typical geometries associated with boron compounds. Boron commonly forms compounds where it exhibits sp² or sp³ hybridization, leading to different geometries depending on the type of bonds it forms.

1. **Trigonal Planar Geometry**: When boron is sp² hybridized, it typically forms a trigonal planar geometry. This is common in compounds such as borane (BH₃), where boron forms three sigma bonds.

2. **Tetrahedral Geometry**: For a tetrahedral geometry, boron must be sp³ hybridized, forming four sigma bonds. Typically, this arises when boron forms compounds with added coordination or when bonding is extended to include additional atoms or ligands.

In the context of the given reaction, the formation of the product 'B' with a tetrahedral geometry suggests that boron undergoes a change in its hybridization state. Usually, this change involves the acceptance of lone pairs or additional bonds, moving from a three-coordinate system to a four-coordinate one.

3. **Pyramidal Geometry**: This is generally not observed with boron due to its preference for electron-deficient bonding, which does not allow for the lone pair configuration that usually characterizes pyramidal geometries.

4. **Square Planar Geometry**: Square planar geometry is uncommon for boron. It is predominantly observed in transition metal complexes due to d-orbital participation, which boron lacks.

Given these possibilities, the most logical conclusion for boron in product 'B' to have a tetrahedral geometry requires examining its potential to expand its valence shell or coordinate sphere suitably. This could involve donor-atom interactions or reactions with electron-donating species.

Therefore, the product 'B' likely adopts a tetrahedral geometry due to sp³ hybridization, allowing it to maximize bonding capacity with surrounding atoms or groups.