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The solid PCl5 exists as...

The solid `PCl_5` exists as

A

`PCl_(5)` molecules

B

`P_(2)Cl_(10)`

C

`[PCl_(4)]+[PCl_(6)]^(-)`

D

none

Text Solution

Verified by Experts

The correct Answer is:
C
Solid `PCl_(5)` exist as `[PCl_(4)]^(+) [PCl_(6)]^(-)` which are tetrahedral and octahedral respectively.
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Draw the structure of the following (i) HClO_3 (ii) H_2S_2O_8 ( b) Give reasons for the following (i) Above 1000 K sulphur shows paramagnetism. (ii)Although electron gain enthalpy of fluorine is less negative of chlorine ,yet flourine is a better oxidising agent than chlorine . (iii) In solid state PCl_5 exists as an ionic compound

Why does PCl_(5) exist as [PCl_(4)]^(+)[PCl_(6)]^(-) in the crystalline state?

Knowledge Check

  • In solid PCl_(5) exist as

    A
    `PCl_(3)`
    B
    `PCl_(4)^(+)`
    C
    `PCl_(6)^(-)`
    D
    `PCl_(4)^(+) and PCl_(6)^(-)`

  • In solid PCl_(5) exist as [PCl_(4)]^(+) [PCl_(6)]^(-) . The hybridisation is P is /are

    A
    `sp^(3)`
    B
    `sp^(3)d`
    C
    `sp^(3)d^(2)`
    D
    `sp^(3) d^(3)`

  • In the solid state PCl_5 exists as

    A
    `[PCl_4]^(-)` and `[PCl_6]^(+)` ions
    B
    covalent `PCl_5` molecules only
    C
    `[PCl_4]^(+)` and `[PCl_6]^(-)` ions
    D
    covalent `P_2Cl_(10)` molecules only

    • Similar Questions

    Explore conceptually related problems

    (a) In a polar solvenbt , PCl_(5) undergoes an ionization reaction as follows : 2 PCl_(5) hArrPCl_(4)^(+) + PCl_(6) ^(-) Wht will be the geometrical shape of each species present In the equalilbrium maxture ? (b) Why does PCl_(5) exist as [ PCl_(4)]^(+) [PCl_(6)]^(-) ?

    PCl_3 under goes hydrolysis to produce an oxoacid.It has formula In solid PCl, exist as

    In solid state PCl_(5) exists as ionic solid i.e., [X]^(+)[Y]^(-) , shapes of X^(+) and Y^(-) are respectively

    Regarding PCl_(5) correct statements are (i) In gaseous and liquid phase PCl_(5) has trigonal bipyramidal structure (ii) In the solid state PCl_(5) exists as an ionic solid, [PCl_(4)]^(+)[PCl_(6)]^(-) in which cation is octahedral and anion is tetrahedral (iii) In PCl_(5) , axial bonds are longer than equatorial bonds (iv) In PCl_(5) , all the five bonds are equal

    PCl_5 has trigonal pyramidal geometry with sp^3 d hybridisation in gases and liquid state but in solid state it exist as ionic compound. In crystalline state PCl_5 exists as.

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