In solid state $P C l_{5}$ exist as an ionic solid $[P C l_{4}]^{+} [P C l_{6}]^{-}$ hybridisation state of cation and anion respectively :

Question

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Answer 1

In the solid state it exists as an ionic solid, $[P C l 4]^{+} [P C l 6]^{-}$ . The cation, $[P C l 4]^{+}$ is tetrahedral and $s p^{3}$ hybridised. The anion, $[P C l 6]^{-}$ is octahedral and is $s p^{3} d^{2}$ hybridised.

Answer 2

In the solid state it exists as an ionic solid,

[P C l 4]^{+} [P C l 6]^{-}

. The cation,

[P C l 4]^{+}

is tetrahedral and

s p^{3}

hybridised. The anion,

[P C l 6]^{-}

is octahedral and is

s p^{3} d^{2}

hybridised.

In solid state $P C l_{5}$ exist as an ionic solid $[P C l_{4}]^{+} [P C l_{6}]^{-}$ hybridisation state of cation and anion respectively :

$d s p^{2}, s p^{3} d^{2}$

$s p^{3}, s p^{3} d^{2}$

$s p^{3} d^{2}, s p^{3}$

$s p^{3} d^{2}, d s p^{2}$

In the solid state it exists as an ionic solid, $[P C l 4]^{+} [P C l 6]^{-}$ . The cation, $[P C l 4]^{+}$ is tetrahedral and $s p^{3}$ hybridised. The anion, $[P C l 6]^{-}$ is octahedral and is $s p^{3} d^{2}$ hybridised.

The hybrid states of phosphorous atoms in $P C l_{5}$ and $P B r_{3}$ in gaseous phase are $s p^{3} d$ . But in solid $P C l_{5}$ , phosphorous shows $s p^{3} d^{2}$ hybrid state. While $P$ in $P B r$ is in $s p^{3}$ hybrid state. This is because :

If $P C l_{5}$ exists, why $N C l_{5}$ does not?

What is the hybridization state of cation part of solid $P C l_{5}$ ?

$P C l_{5}$ is a covalent in gaseous and liquid states but ionic in solid state.

$P C l_{5}$ in solid state consists of tetrahedral $P C l_{4}^{+}$ cation and octahedral $P C l_{6}^{-}$ anion.

$N_{2} O_{5}$ is said to be ionic in solid state. Write the cation and anion in it and the hybridised state of N atom in cation.

Revise with Concepts

Compounds of Phosphorus - PCl3

Compounds of Phosphorus - PCl5

In solid state PCl5​ exist as an ionic solid [PCl4​]+[PCl6​]− hybridisation state of cation and anion respectively :

dsp2,sp3d2

sp3,sp3d2

sp3d2,sp3

sp3d2,dsp2

In the solid state it exists as an ionic solid, [PCl4]+[PCl6]−. The cation, [PCl4]+ is tetrahedral and sp3 hybridised. The anion, [PCl6]− is octahedral and is sp3d2 hybridised.

The hybrid states of phosphorous atoms in PCl5​ and PBr3​ in gaseous phase are sp3d. But in solid PCl5​, phosphorous shows sp3d2 hybrid state. While P in PBr is in sp3 hybrid state. This is because :

If PCl5​ exists, why NCl5​ does not?

What is the hybridization state of cation part of solid PCl5​?

PCl5​ is a covalent in gaseous and liquid states but ionic in solid state.

PCl5​ in solid state consists of tetrahedral PCl4+​ cation and octahedral PCl6−​ anion.

N2​O5​ is said to be ionic in solid state. Write the cation and anion in it and the hybridised state of N atom in cation.

Revise with Concepts

Compounds of Phosphorus - PCl3

Compounds of Phosphorus - PCl5

In solid state $P C l_{5}$ exist as an ionic solid $[P C l_{4}]^{+} [P C l_{6}]^{-}$ hybridisation state of cation and anion respectively :

$d s p^{2}, s p^{3} d^{2}$

$s p^{3}, s p^{3} d^{2}$

$s p^{3} d^{2}, s p^{3}$

$s p^{3} d^{2}, d s p^{2}$

In the solid state it exists as an ionic solid, $[P C l 4]^{+} [P C l 6]^{-}$ . The cation, $[P C l 4]^{+}$ is tetrahedral and $s p^{3}$ hybridised. The anion, $[P C l 6]^{-}$ is octahedral and is $s p^{3} d^{2}$ hybridised.

The hybrid states of phosphorous atoms in $P C l_{5}$ and $P B r_{3}$ in gaseous phase are $s p^{3} d$ . But in solid $P C l_{5}$ , phosphorous shows $s p^{3} d^{2}$ hybrid state. While $P$ in $P B r$ is in $s p^{3}$ hybrid state. This is because :

If $P C l_{5}$ exists, why $N C l_{5}$ does not?

What is the hybridization state of cation part of solid $P C l_{5}$ ?

$P C l_{5}$ is a covalent in gaseous and liquid states but ionic in solid state.

$P C l_{5}$ in solid state consists of tetrahedral $P C l_{4}^{+}$ cation and octahedral $P C l_{6}^{-}$ anion.

$N_{2} O_{5}$ is said to be ionic in solid state. Write the cation and anion in it and the hybridised state of N atom in cation.