Which is the following pairs of species have identical shapes ?

Options

A. `NO_(2)^(+) and NO_(2)^(-)`
B. `PCl_(5) and BrF_(5)`
C. `XeF_(4) and IC I_(4)^(-)`
D. `XeF_(4) and XeO_(4)`

Explanation

To determine which pairs of species have identical shapes, we will analyze each option step by step.

### Step 1: Analyze Option A (NO2+ and NO2-)
1. **NO2+ (Nitronium ion)**:
- Nitrogen has 5 valence electrons, and with a positive charge, it has 4 electrons.
- It forms 2 double bonds with oxygen (2 bond pairs).
- There are no lone pairs on nitrogen.
- **Shape**: Linear (due to 2 bond pairs and 0 lone pairs).

2. **NO2- (Nitrite ion)**:
- Nitrogen has 5 valence electrons, and with a negative charge, it has 6 electrons.
- It forms 1 double bond and 1 single bond with oxygen (2 bond pairs) and has 1 lone pair.
- **Shape**: Angular (due to 2 bond pairs and 1 lone pair).

**Conclusion for Option A**: The shapes are not identical (Linear vs. Angular).

### Step 2: Analyze Option B (PCl5 and BrF5)
1. **PCl5 (Phosphorus pentachloride)**:
- Phosphorus has 5 valence electrons and forms 5 bonds with chlorine (5 bond pairs).
- There are no lone pairs.
- **Shape**: Trigonal bipyramidal.

2. **BrF5 (Bromine pentafluoride)**:
- Bromine has 7 valence electrons and forms 5 bonds with fluorine (5 bond pairs) and has 1 lone pair.
- **Shape**: Square pyramidal (due to 5 bond pairs and 1 lone pair).

**Conclusion for Option B**: The shapes are not identical (Trigonal bipyramidal vs. Square pyramidal).

### Step 3: Analyze Option C (XeF4 and ICl4-)
1. **XeF4 (Xenon tetrafluoride)**:
- Xenon has 8 valence electrons and forms 4 bonds with fluorine (4 bond pairs) and has 2 lone pairs.
- **Shape**: Square planar (due to 4 bond pairs and 2 lone pairs).

2. **ICl4- (Iodine tetrachloride ion)**:
- Iodine has 7 valence electrons and with a negative charge, it has 8 electrons.
- It forms 4 bonds with chlorine (4 bond pairs) and has 2 lone pairs.
- **Shape**: Square planar (due to 4 bond pairs and 2 lone pairs).

**Conclusion for Option C**: The shapes are identical (Both are Square planar).

### Step 4: Analyze Option D
1. **Species in Option D**: (not specified in the transcript, but we can analyze based on common knowledge)
- Typically, if we consider a species with 4 bond pairs and 0 lone pairs (like CH4) and compare it with another species with 4 bond pairs and 2 lone pairs (like H2O), they will not have identical shapes.

**Conclusion for Option D**: The shapes are not identical.

### Final Answer:
The only pair of species that have identical shapes is **Option C: XeF4 and ICl4-**, both having a square planar shape.

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