The structure of phosphide ion is similar to that of

Options

A. Nitride ion
B. Chloride ion
C. Fluoride ion
D. Sodium ion

Explanation

To determine which ion has a structure similar to the phosphide ion (P³⁻), we need to analyze the electron configurations of the given ions and identify which one is isoelectronic with P³⁻.

### Step-by-Step Solution:

1. **Identify the Phosphide Ion:**
- The phosphide ion is represented as P³⁻.
- Phosphorus (P) has an atomic number of 15, which means a neutral phosphorus atom has 15 electrons.
- When it gains 3 electrons to form P³⁻, it has a total of 15 + 3 = 18 electrons.

2. **Analyze the Given Options:**
- **Option 1: Nitrite Ion (NO₂⁻)**
- Nitrogen (N) has an atomic number of 7 and oxygen (O) has an atomic number of 8.
- The nitrite ion has a total of 5 electrons from nitrogen and 12 from two oxygen atoms, giving a total of 17 electrons (not isoelectronic with P³⁻).

- **Option 2: Chloride Ion (Cl⁻)**
- Chlorine (Cl) has an atomic number of 17.
- The chloride ion gains 1 electron, resulting in 17 + 1 = 18 electrons (isoelectronic with P³⁻).

- **Option 3: Fluoride Ion (F⁻)**
- Fluorine (F) has an atomic number of 9.
- The fluoride ion gains 1 electron, resulting in 9 + 1 = 10 electrons (not isoelectronic with P³⁻).

- **Option 4: Sodium Ion (Na⁺)**
- Sodium (Na) has an atomic number of 11.
- The sodium ion loses 1 electron, resulting in 11 - 1 = 10 electrons (not isoelectronic with P³⁻).

3. **Conclusion:**
- The only ion that has the same number of electrons (18) as the phosphide ion (P³⁻) is the chloride ion (Cl⁻).
- Therefore, the structure of the phosphide ion is similar to that of the chloride ion.

### Final Answer:
The structure of the phosphide ion (P³⁻) is similar to that of the chloride ion (Cl⁻).