In diborane `(B_(2)H_(6))`, the bond formed between B and B is called :

Options

A. sigma bond
B. 2-centre 2-electron bond
C. banana bond
D. coordinate bond

Explanation

To determine the type of bond formed between the two boron atoms in diborane (B₂H₆), we need to analyze the structure and bonding characteristics of the molecule.

### Step-by-Step Solution:

1. **Understanding the Structure of Diborane (B₂H₆)**:
- Diborane consists of two boron (B) atoms and six hydrogen (H) atoms. The molecular structure can be visualized as having two boron atoms at the center with hydrogen atoms surrounding them.

2. **Valence Electrons**:
- Each boron atom has 3 valence electrons. Therefore, in diborane, the two boron atoms together contribute a total of 6 valence electrons.

3. **Bonding with Hydrogen**:
- Each boron atom forms bonds with three hydrogen atoms. In BH₃ (the boron hydride unit), boron uses its three valence electrons to form three single covalent bonds with hydrogen atoms.

4. **Boron-Boron Bond**:
- In diborane, there are two boron atoms. The bonding between these two boron atoms is unique. Each boron atom has an empty p-orbital, and they share two electrons to form a bond. This bond is not a typical single bond; instead, it involves the sharing of two electrons between the two boron atoms.

5. **Nature of the Boron-Boron Bond**:
- The bond formed between the two boron atoms in diborane is called a **"three-center two-electron bond"**. This type of bond involves three atoms (the two boron atoms and one hydrogen atom) sharing two electrons.

6. **Conclusion**:
- Therefore, the bond formed between the two boron atoms in diborane (B₂H₆) is classified as a **three-center two-electron bond**.