Bonding in which of the following diatomic molecule (s) becomes (s) stronger , on the basis of MO Theory , by removal of an electron?
(A) `NO`
(B) `N_(2)`
(C )`O_(2)`
(D) `C_(2)`
(E )`B_(2)`

Options

A. (A),(B)and (C ) only
B. (B) (C ),(E ) only
C. (A),(C ) only
D. (D) only

Explanation

To determine which diatomic molecule's bonding becomes stronger upon the removal of an electron, we will analyze the bond orders of the given molecules using Molecular Orbital (MO) Theory. The bond order is a measure of the strength of a bond; a higher bond order indicates a stronger bond.

### Step-by-Step Solution:

1. **Identify the Molecules**: The molecules we need to analyze are NO, N₂, O₂, C₂, and B₂.

2. **Calculate Initial Bond Orders**:
- **NO**: The bond order is calculated as 2.5.
- **N₂**: The bond order is 3.
- **O₂**: The bond order is 2.
- **C₂**: The bond order is 2.
- **B₂**: The bond order is 1.

3. **Remove One Electron**: We will now consider the effect of removing one electron from each molecule:
- **NO⁺**: The bond order increases to 3.
- **N₂⁺**: The bond order decreases to 2.5.
- **O₂⁺**: The bond order increases to 2.5.
- **C₂⁺**: The bond order decreases to less than 1.5.
- **B₂⁺**: The bond order decreases to less than 0.5.

4. **Compare Bond Orders After Removal**:
- **NO⁺**: Bond order = 3 (increased from 2.5)
- **N₂⁺**: Bond order = 2.5 (decreased from 3)
- **O₂⁺**: Bond order = 2.5 (increased from 2)
- **C₂⁺**: Bond order < 1.5 (decreased from 2)
- **B₂⁺**: Bond order < 0.5 (decreased from 1)

5. **Determine Which Bonds Become Stronger**:
- A bond order increase indicates a stronger bond.
- NO and O₂ show an increase in bond order after the removal of an electron.

### Conclusion:
The diatomic molecules whose bonding becomes stronger upon the removal of an electron are **NO** and **O₂**.