The Question is from neet-chemistry chemical-bonding hybridisation, and it was created by the author A.RAMA NAGESWARARAO

Question

Which of the following statements is INCORRECT regarding the hybridisation of $PCl_5$ in the gaseous and solid states?

A.RAMA NAGESWARARAO · Accepted Answer

## CORE INFORMATION
✓ **Answer**: A
## CONCEPT FRAMEWORK
	**Primary Concept**: Hybridisation and Molecular Geometry
	**Related Topics**: VSEPR theory, Bonding in phosphorus compounds
	**Prerequisites**: Lewis structures, Valence Bond Theory
## SOLUTION PATHWAY
**Given Information**:
	We are analyzing the hybridization of phosphorus in $PCl_5$ in gaseous and solid states.
**Method & Steps**:
	1. **Gaseous $PCl_5$**: 
		Reasoning: In the gaseous state, $PCl_5$ exists as a trigonal bipyramidal molecule.
		Formula/Rule: To form five bonds with five chlorine atoms, phosphorus utilizes one 3s, three 3p, and one 3d orbital, resulting in $sp^3d$ hybridization.
	2. **Solid $PCl_5$**: 
		Working: In the solid state, $PCl_5$ exists as an ionic compound, formulated as $[PCl_4]^+[PCl_6]^-$.
		Key Point: The cation $[PCl_4]^+$ has a tetrahedral geometry, and the anion $[PCl_6]^-$ has an octahedral geometry.
	3. **Hybridization in Solid State**:
		Result: The cation $[PCl_4]^+$ exhibits $sp^3$ hybridization, while the anion $[PCl_6]^-$ exhibits $sp^3d^2$ hybridization.
		Verification: This is consistent with the observed geometries.
 ## OPTION ANALYSIS
[A] :x: Incorrect. Phosphorus undergoes $sp^3d$ hybridization in the gaseous state, but $sp^3$ and $sp^3d^2$ hybridization in the solid state.  Thus, this statement is false.
[B] ✓: Correct. Phosphorus in gaseous $PCl_5$ has $sp^3d$ hybridization.
[C] ✓: Correct.  In solid $PCl_5$, phosphorus exists as $[PCl_4]^+$ ($sp^3$) and $[PCl_6]^-$ ($sp^3d^2$).
[D] :x: Incorrect. While $[PCl_6]^-$ part has $sp^3d^2$ hybridization, it's not the only hybridization present in the solid state; $[PCl_4]^+$ has $sp^3$ hybridization.
 ## LEARNING AIDS
	**Common Mistakes**:
		1. Assuming the same hybridization in all states: Remember that hybridization can change depending on the state of matter.
		2. Ignoring the ionic nature of solid $PCl_5$:  Don't just consider the molecular formula; consider the actual ionic structure in the solid state.
	**Quick Tips**:
		1. Relate geometry to hybridization: Trigonal bipyramidal is $sp^3d$, tetrahedral is $sp^3$, and octahedral is $sp^3d^2$.
		2. Remember the ionic structure of $PCl_5$:  Solid $PCl_5$ exists as $[PCl_4]^+[PCl_6]^-$.

A.RAMA NAGESWARARAO · Answer

The correct Option is "Phosphorus undergoes $sp^3d$ hybridisation in both the gaseous and solid states"

A.RAMA NAGESWARARAO · Answer

Phosphorus undergoes $sp^3d$ hybridisation in the gaseous state

A.RAMA NAGESWARARAO · Answer

Phosphorus undergoes $sp^3$ and $sp^3d^2$ hybridisation in the solid state

A.RAMA NAGESWARARAO · Answer

Phosphorus undergoes $sp^3d^2$ hybridisation in the solid state

NEET Chemistry Chemical Bonding and Molecular Structure Hybridisation MCQs

Select Topic

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

NEET Subjects

Our Bots

Company