Hybridisation of Boron in `B_(2)H_(6)` molecule is :

Options

A. `sp^(2)`
B. `sp^(3)`
C. `sp^(3)d`
D. sp

Explanation

To determine the hybridization of boron in the \( B_2H_6 \) molecule, we can follow these steps:

### Step 1: Determine the Valence Electrons of Boron
Boron (B) has an atomic number of 5, which means it has 5 electrons. The electron configuration of boron is \( 1s^2 2s^2 2p^1 \). In the outermost shell (the second shell), boron has 3 valence electrons (2 from the 2s orbital and 1 from the 2p orbital).

**Hint:** Count the number of valence electrons for the central atom in the molecule.

### Step 2: Analyze the Structure of \( B_2H_6 \)
The \( B_2H_6 \) molecule consists of 2 boron atoms and 6 hydrogen atoms. Each boron atom forms bonds with three hydrogen atoms, leading to the formation of two \( BH_3 \) units.

**Hint:** Identify how many hydrogen atoms are bonded to each boron atom.

### Step 3: Consider the Hybridization of One \( BH_3 \) Unit
In the \( BH_3 \) unit, boron is bonded to three hydrogen atoms. To form these bonds, boron undergoes hybridization. The three valence electrons of boron can be excited to form three equivalent hybrid orbitals.

**Hint:** Think about how many bonds are formed and how many orbitals are needed for bonding.

### Step 4: Determine the Hybridization Type
Boron in \( BH_3 \) hybridizes to form three \( sp^2 \) hybrid orbitals. This involves mixing one \( s \) orbital and two \( p \) orbitals to create three \( sp^2 \) hybrid orbitals, which are arranged in a trigonal planar geometry.

**Hint:** Recall the geometry associated with different types of hybridization (e.g., \( sp \), \( sp^2 \), \( sp^3 \)).

### Step 5: Consider the Overall Structure of \( B_2H_6 \)
In \( B_2H_6 \), the two boron atoms are connected through a pair of shared electrons (a bridge), which means they also have an empty p orbital that can overlap with the other boron's empty p orbital. This results in the formation of a three-dimensional structure.

**Hint:** Visualize how the hybridized orbitals interact with each other and with hydrogen atoms.

### Conclusion
Thus, the hybridization of boron in \( B_2H_6 \) is \( sp^3 \) because each boron atom effectively uses four orbitals (three \( sp^2 \) for bonding with hydrogen and one empty p orbital for bridging).

**Final Answer:** The hybridization of boron in \( B_2H_6 \) is \( sp^3 \).