In which of the following, the geometry is not correctly given?

Options

A. `PH_(3):" Trigonal pyramidal"`
B. `SiH_(4):"Tetrahedral"`
C. `ClF_(3):"Trigonal planar"`
D. `SF_(4):"Square planar"`

Explanation

To determine which of the given geometries is not correctly assigned, we need to analyze the hybridization and molecular geometry of each compound mentioned in the question. Let's go through each option step by step.

### Step 1: Analyze PH3 (Phosphine)
1. **Valence Electrons Calculation**:
- Phosphorus (P) is in Group 15, so it has 5 valence electrons.
- There are 3 hydrogen (H) atoms, each contributing 1 electron.
- Total = 5 (from P) + 3 (from H) = 8 electrons.
- Hybridization = (8 / 2) = 4 → sp³ hybridization.

2. **Bond Pairs and Lone Pairs**:
- Bond pairs = 3 (P-H bonds).
- Lone pairs = 1 (remaining electron pair on phosphorus).

3. **Geometry**:
- With 3 bond pairs and 1 lone pair, the geometry is **trigonal pyramidal**.
- The given geometry is correct.

### Step 2: Analyze SiH4 (Silane)
1. **Valence Electrons Calculation**:
- Silicon (Si) is in Group 14, so it has 4 valence electrons.
- There are 4 hydrogen atoms.
- Total = 4 (from Si) + 4 (from H) = 8 electrons.
- Hybridization = (8 / 2) = 4 → sp³ hybridization.

2. **Bond Pairs and Lone Pairs**:
- Bond pairs = 4 (Si-H bonds).
- Lone pairs = 0.

3. **Geometry**:
- With 4 bond pairs and no lone pairs, the geometry is **tetrahedral**.
- The given geometry is correct.

### Step 3: Analyze ClF3 (Chlorine trifluoride)
1. **Valence Electrons Calculation**:
- Chlorine (Cl) is in Group 17, so it has 7 valence electrons.
- There are 3 fluorine (F) atoms.
- Total = 7 (from Cl) + 3 (from F) = 10 electrons.
- Hybridization = (10 / 2) = 5 → sp³d hybridization.

2. **Bond Pairs and Lone Pairs**:
- Bond pairs = 3 (Cl-F bonds).
- Lone pairs = 2 (remaining pairs on chlorine).

3. **Geometry**:
- With 3 bond pairs and 2 lone pairs, the geometry is **trigonal bipyramidal**.
- The shape is **T-shaped**.
- The given geometry is incorrectly stated as **trigonal planar**.

### Step 4: Analyze SF4 (Sulfur tetrafluoride)
1. **Valence Electrons Calculation**:
- Sulfur (S) is in Group 16, so it has 6 valence electrons.
- There are 4 fluorine atoms.
- Total = 6 (from S) + 4 (from F) = 10 electrons.
- Hybridization = (10 / 2) = 5 → sp³d hybridization.

2. **Bond Pairs and Lone Pairs**:
- Bond pairs = 4 (S-F bonds).
- Lone pairs = 1.

3. **Geometry**:
- With 4 bond pairs and 1 lone pair, the geometry is **trigonal bipyramidal**.
- The shape is **seesaw**.
- The given geometry is incorrectly stated as **square planar**.

### Conclusion
The geometries that are not correctly given are for ClF3 and SF4. Therefore, the answer to the question is that the geometries for both ClF3 and SF4 are incorrectly stated.