Assertion: In crystal lattice, size of the cation is larger in a tetrahedral hole than in an octahedral hole.
Reason: The cations occupy more space than anions in crystal packing.

Both the assertion and reason is correct

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Assertion is correct but the reason is incorrect

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Assertion is incorrect but the reason is correct

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Both the assertion and reason are incorrect

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Solution

The correct option is D Both the assertion and reason are incorrect
In crystal lattice tetrahedral void is smaller than the octahedral void as
$Radius of tetrahedral void =0.225 R Radius of octahedral void =0.414 R$
Anions are larger in size than cations so anions occupy more space.

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Q. Assertion : In crystal lattice, the size of the cation is larger in a tetrahedral hole than in an octahedral hole.
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Assertion: In crystal lattice, size of the cation is larger in a tetrahedral hole than in an octahedral hole. Reason: The cations occupy more space than anions in crystal packing.

The correct option is D Both the assertion and reason are incorrectIn crystal lattice tetrahedral void is smaller than the octahedral void as Radius of tetrahedral void =0.225 RRadius of octahedral void =0.414 R Anions are larger in size than cations so anions occupy more space.

Assertion: In crystal lattice, size of the cation is larger in a tetrahedral hole than in an octahedral hole.
Reason: The cations occupy more space than anions in crystal packing.

The correct option is D Both the assertion and reason are incorrect
In crystal lattice tetrahedral void is smaller than the octahedral void as
$Radius of tetrahedral void =0.225 R Radius of octahedral void =0.414 R$
Anions are larger in size than cations so anions occupy more space.