In the solid state PCl-5- exists as-PCl-4- and -PCl-6- ionscovalent PCl-5- molecules only-PCl-4- and -PCl-6- ionscovalent P-2-Cl-10- molecules only

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Toppr Admin · Accepted Answer

In the solid state- PCl5 prefers to exist as oppositely charged ion like -PCl4- and -PCl6-x2212- as ionic bonding enhances the crystalline nature- The shape is more stable in the ionic form as it forms the tetrahedral and octahedral shape-

In the solid state $P C l_{5}$ exists as:
$[P C l_{4}]^{-}$ and $[P C l_{6}]^{+}$ ions
covalent $P C l_{5}$ molecules only
$[P C l_{4}]^{+}$ and $[P C l_{6}]^{-}$ ions
covalent $P_{2} C l_{10}$ molecules only

In the solid state, $P C l_{5}$ prefers to exist as oppositely charged ion like $[P C l_{4}]^{+}$ and $[P C l_{6}]^{-}$ as ionic bonding enhances the crystalline nature. The shape is more stable in the ionic form as it forms the tetrahedral and octahedral shape.

In the solid state PCl5 exists as:[PCl4]− and [PCl6]+ ionscovalent PCl5 molecules only[PCl4]+ and [PCl6]− ionscovalent P2Cl10 molecules only

In the solid state, PCl5 prefers to exist as oppositely charged ion like [PCl4]+ and [PCl6]− as ionic bonding enhances the crystalline nature. The shape is more stable in the ionic form as it forms the tetrahedral and octahedral shape.

In the solid state $P C l_{5}$ exists as:
$[P C l_{4}]^{-}$ and $[P C l_{6}]^{+}$ ions
covalent $P C l_{5}$ molecules only
$[P C l_{4}]^{+}$ and $[P C l_{6}]^{-}$ ions
covalent $P_{2} C l_{10}$ molecules only

In the solid state, $P C l_{5}$ prefers to exist as oppositely charged ion like $[P C l_{4}]^{+}$ and $[P C l_{6}]^{-}$ as ionic bonding enhances the crystalline nature. The shape is more stable in the ionic form as it forms the tetrahedral and octahedral shape.