$$Statement-I$$: All $$P-CI$$ bonds in $$PCI5$$ are equal in length.$$Statement-II$$: In vapour state $$PCl5$$ (PCI4)+$$ $$(PCI6)– .

Correct option is 4Both statement-I and statement-II are incorrect

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Statement-I: All P-CI bonds in PCI₅ are equal in length.
Statement-II: In vapour state PCl₅ (PCI₄)⁺ (PCI₆)^– .

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Both statement-I and statement-II are correct

Statement-I is correct and statement-II is incorrect

Statement-I is incorrect and statement-II is correct

Both statement-I and statement-II are incorrect

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detailed solution

Correct option is D

Both (A) and, (R) are false. PCl5 exists as (PCl4)+ (PCl6)– in solid state. in vapour form it exists as trigonal bipyramidal molecule with two axial P-Cl bonds equal in length and larger than other three equatorial P—Cl bonds.

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Statement-I: All P-CI bonds in PCI5 are equal in length.Statement-II: In vapour state PCl5 (PCI4)+ (PCI6)– .

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Statement-I: All P-CI bonds in PCI₅ are equal in length.
Statement-II: In vapour state PCl₅ (PCI₄)⁺ (PCI₆)^– .