Identify the incorrect statement about PCl5:
- PCl5 possesses two different Cl – P – Cl bond angles
- All five P – Cl bonds are identical in length
- PCl5 exhibits sp3d hybridisation
- PCl5 consists of five P – Cl (sigma) bonds
The Correct Option is B
Solution and Explanation
To determine the incorrect statement about PCl5, let's analyze each option based on the chemical structure and properties of phosphorus pentachloride (PCl5).
-
Statement: PCl5 possesses two different Cl – P – Cl bond angles.
Explanation: PCl5 has a trigonal bipyramidal structure, where three chlorine atoms are in an equatorial plane, and two are in axial positions. This results in two distinct Cl – P – Cl bond angles: 120° in the equatorial plane and 90° between the axial and equatorial positions. -
Statement: All five P – Cl bonds are identical in length.
Explanation: Given the trigonal bipyramidal geometry, the equatorial P – Cl bonds are shorter than the axial P – Cl bonds because of electron cloud repulsion and spatial arrangement. Thus, not all P – Cl bonds are identical in length. Therefore, this statement is incorrect. -
Statement: PCl5 exhibits sp3d hybridisation.
Explanation: The central phosphorus atom in PCl5 undergoes sp3d hybridization to accommodate five chlorine atoms, forming a trigonal bipyramidal shape. -
Statement: PCl5 consists of five P – Cl (sigma) bonds.
Explanation: In PCl5, each P – Cl bond is a sigma bond, making up a total of five sigma bonds connecting phosphorus to the chlorine atoms.
Conclusion: The statement "All five P – Cl bonds are identical in length" is incorrect because of the nature of the trigonal bipyramidal structure leading to bond length differences between axial and equatorial positions.
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