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Which of the following has a geometry di...

Which of the following has a geometry different from the other three species (having the same geometry) ?

A

`BF_(4)^(-)`

B

`SO_(4)^(2-)`

C

`XeF_(4)`

D

`PH_(4)^(+)`

Text Solution

AI Generated Solution

The correct Answer is:
To determine which of the given species has a geometry different from the others, we will analyze the geometries of each compound step-by-step. ### Step 1: Analyze BF4⁻ (Boron Tetrafluoride Ion) 1. **Central Atom**: Boron (B) 2. **Valence Electrons**: Boron has 3 valence electrons. 3. **Bonds**: In BF4⁻, boron forms 4 bonds with fluorine atoms. Since boron can only accommodate 3 electrons normally, it accepts an electron from one of the fluorine atoms, resulting in a negative charge. 4. **Steric Number Calculation**: - Sigma bonds: 4 (one for each B-F bond) - Lone pairs: 0 - Steric Number = 4 + 0 = 4 5. **Hybridization**: sp³ 6. **Geometry**: Tetrahedral ### Step 2: Analyze SO4²⁻ (Sulfate Ion) 1. **Central Atom**: Sulfur (S) 2. **Valence Electrons**: Sulfur has 6 valence electrons. 3. **Bonds**: In SO4²⁻, sulfur forms 4 bonds with oxygen atoms (two double bonds and two single bonds with negative charges). 4. **Steric Number Calculation**: - Sigma bonds: 4 (one for each S-O bond) - Lone pairs: 0 - Steric Number = 4 + 0 = 4 5. **Hybridization**: sp³ 6. **Geometry**: Tetrahedral ### Step 3: Analyze XeF4 (Xenon Tetrafluoride) 1. **Central Atom**: Xenon (Xe) 2. **Valence Electrons**: Xenon has 8 valence electrons. 3. **Bonds**: In XeF4, xenon forms 4 bonds with fluorine atoms and has 2 lone pairs of electrons. 4. **Steric Number Calculation**: - Sigma bonds: 4 (one for each Xe-F bond) - Lone pairs: 2 - Steric Number = 4 + 2 = 6 5. **Hybridization**: sp³d² 6. **Geometry**: Octahedral (Shape: Square Planar due to lone pairs) ### Step 4: Analyze PH4⁺ (Phosphonium Ion) 1. **Central Atom**: Phosphorus (P) 2. **Valence Electrons**: Phosphorus has 5 valence electrons. 3. **Bonds**: In PH4⁺, phosphorus forms 4 bonds with hydrogen atoms and carries a positive charge. 4. **Steric Number Calculation**: - Sigma bonds: 4 (one for each P-H bond) - Lone pairs: 0 - Steric Number = 4 + 0 = 4 5. **Hybridization**: sp³ 6. **Geometry**: Tetrahedral ### Conclusion - **BF4⁻**: Tetrahedral - **SO4²⁻**: Tetrahedral - **XeF4**: Octahedral (Square Planar shape) - **PH4⁺**: Tetrahedral **Final Answer**: The species with a geometry different from the others is **XeF4**. ---

To determine which of the given species has a geometry different from the others, we will analyze the geometries of each compound step-by-step. ### Step 1: Analyze BF4⁻ (Boron Tetrafluoride Ion) 1. **Central Atom**: Boron (B) 2. **Valence Electrons**: Boron has 3 valence electrons. 3. **Bonds**: In BF4⁻, boron forms 4 bonds with fluorine atoms. Since boron can only accommodate 3 electrons normally, it accepts an electron from one of the fluorine atoms, resulting in a negative charge. 4. **Steric Number Calculation**: - Sigma bonds: 4 (one for each B-F bond) ...
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