Of the species, `NO, NO^(+), NO^(2+) and NO^(-)`, the one with minimum bond strength is :

Options

A. `NO^(-)`
B. `NO^(+)`
C. `NO^(2+)`
D. `NO`

Explanation

To determine which species among NO, NO⁺, NO²⁺, and NO⁻ has the minimum bond strength, we need to analyze the number of electrons in each species and calculate their bond orders. The bond strength is inversely related to the bond order; thus, a lower bond order indicates weaker bond strength.

### Step 1: Calculate the number of electrons in each species

1. **For NO (Nitric Oxide)**:
- Nitrogen (N) has 7 electrons.
- Oxygen (O) has 8 electrons.
- Total electrons = 7 + 8 = 15.

2. **For NO⁺ (Nitric Oxide Cation)**:
- Total electrons = 15 - 1 (due to +1 charge) = 14.

3. **For NO²⁺ (Nitric Dioxide Cation)**:
- Total electrons = 15 - 2 (due to +2 charge) = 13.

4. **For NO⁻ (Nitric Oxide Anion)**:
- Total electrons = 15 + 1 (due to -1 charge) = 16.

### Step 2: Determine the bond order for each species

The bond order can be calculated using the formula:
\[ \text{Bond Order} = \frac{\text{Number of bonding electrons} - \text{Number of antibonding electrons}}{2} \]

However, for simplicity, we can use the following relationship based on the number of electrons:
- For 14 electrons, bond order = 3.
- For 15 electrons, bond order = 2.5.
- For 13 electrons, bond order = 2.
- For 16 electrons, bond order = 1.5.

### Step 3: Compare the bond orders

- **NO**: 15 electrons → Bond order = 2.5
- **NO⁺**: 14 electrons → Bond order = 3
- **NO²⁺**: 13 electrons → Bond order = 2
- **NO⁻**: 16 electrons → Bond order = 1.5

### Step 4: Identify the species with minimum bond strength

The species with the lowest bond order is NO⁻, which has a bond order of 1.5. Therefore, it has the minimum bond strength.

### Final Answer:
The species with minimum bond strength is **NO⁻**.

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