According to MOT, two atomic orbitals overlap resulting in the formation of molecular orbital formed. Number of atomic orbitals overlapping together is equal to the molecule orbital formed. The two atomic orbital thus formed by LCAO (linear combination of atomic orbital) in the phase or in the different phase are known as bonding and antibonding molecular orbitals respectively. The energy of bonding molecular orbital is lower than that of the pure atomic orbitals by an amount `Delta`. This known as the stabilization energy. The enerby of antibonding molecular orbital in increased by `Delta'` (destabilisation energy).
Q. How many nodal plane is present in `sigma_(s and p)` bonding molecular orbital ?

Options

A. zero
B. `1`
C. `2`
D. `3`

Explanation

To determine the number of nodal planes present in sigma (σ) bonding molecular orbitals formed from s and p atomic orbitals, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Molecular Orbitals**:
- Molecular orbitals are formed by the linear combination of atomic orbitals (LCAO). When two atomic orbitals combine, they can form bonding or antibonding molecular orbitals.

2. **Identifying Sigma (σ) Bonding Molecular Orbitals**:
- Sigma (σ) bonding molecular orbitals are formed when atomic orbitals overlap along the internuclear axis. This can occur with s orbitals or p orbitals.

3. **Analyzing the Nodal Planes**:
- A nodal plane is defined as a region in a molecular orbital where the probability of finding an electron density is zero. In bonding molecular orbitals, the electron density is concentrated between the nuclei of the bonded atoms.

4. **Sigma (σ) Bonding from s Orbitals**:
- When two s orbitals overlap, they form a σ bonding molecular orbital. Since the s orbitals are spherical and symmetrical, there are no nodal planes in this bonding molecular orbital.

5. **Sigma (σ) Bonding from p Orbitals**:
- When two p orbitals overlap to form a σ bonding molecular orbital, they also do so along the internuclear axis. The overlap occurs in such a way that there is no region where the electron density is zero along the axis of overlap.

6. **Conclusion**:
- For both σ bonding molecular orbitals formed from s and p orbitals, there are **no nodal planes** present. Therefore, the answer to the question is that the number of nodal planes in σ_s and σ_p bonding molecular orbitals is **zero**.

### Final Answer:
The number of nodal planes present in σ_s and σ_p bonding molecular orbitals is **0**.

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