The type of hybridization of boron in diborane is

Options

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

Answer

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

### Step 1: Understand the Structure of Diborane
Diborane consists of two boron atoms and six hydrogen atoms. The structure can be visualized as having two boron atoms at the center with hydrogen atoms surrounding them. Each boron atom forms bonds with hydrogen atoms.

**Hint:** Visualize the molecular structure to identify how atoms are connected.

### Step 2: Count the Valence Electrons
Boron has three valence electrons (as it is in group 13 of the periodic table). In diborane, each boron atom will contribute its three valence electrons.

**Hint:** Remember that boron typically has three electrons available for bonding.

### Step 3: Determine Bonding in Diborane
In diborane, each boron atom forms:
- Two terminal B-H bonds (one with each of the two hydrogen atoms).
- One three-center two-electron bond, which involves the sharing of electrons between two boron atoms and one hydrogen atom.

**Hint:** Identify how many bonds each boron atom is involved in.

### Step 4: Calculate the Total Number of Bonds
Each boron atom in diborane effectively forms four bonds:
- Two with terminal hydrogen atoms.
- One with the other boron atom through the three-center bond.

**Hint:** Count the total number of bonds formed by each boron atom.

### Step 5: Determine Hybridization
To find the hybridization, we use the formula:
- Number of hybrid orbitals = Number of bonds + Lone pairs
In this case, each boron atom forms four bonds and has no lone pairs. Thus, the hybridization can be determined as:
- 4 bonds = sp³ hybridization.

**Hint:** Use the bond count to determine the type of hybridization.

### Conclusion
The type of hybridization of boron in diborane is **sp³**.

### Final Answer
The correct answer is **sp³ hybridization** for boron in diborane.

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