Boron with hydrogen forms a number of hydrides which are known are boranes. These hydrides are classified into closoboranes and nidobarances. The simplest hydride of boron is diborane. Boron apart from having `(2c, 2e)` bonds also contain `(3c, 2e)` bonds.
Boron in diborane is___hydridised.

Options

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

Answer

To determine the hybridization of boron in diborane (B2H6), we can follow these steps:

### Step 1: Understand the Structure of Diborane
Diborane is a compound consisting of two boron atoms and six hydrogen atoms. The formula for diborane is B2H6.

### Step 2: Identify the Hybridization of Boron
In diborane, each boron atom forms bonds with hydrogen atoms and also participates in a unique bonding arrangement known as a 3-center 2-electron bond (often referred to as a "banana bond").

### Step 3: Determine the Electron Configuration of Boron
Boron has an atomic number of 5, which gives it the electron configuration of 1s² 2s² 2p¹. In the excited state, one of the 2s electrons can be promoted to a 2p orbital, resulting in the configuration of 2s¹ 2p².

### Step 4: Analyze Bond Formation
In diborane, each boron atom forms:
- 3 single bonds with hydrogen atoms (2 center 2 electron bonds).
- 1 additional bond that is a 3-center 2-electron bond involving both boron atoms and one hydrogen atom.

### Step 5: Determine the Hybridization
To accommodate these bonds, the boron atoms undergo hybridization. Each boron atom forms four equivalent bonds (three with hydrogen and one with the other boron atom). This requires sp³ hybridization, as it involves four equivalent hybrid orbitals.

### Conclusion
Thus, the hybridization of boron in diborane (B2H6) is **sp³**.

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