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In a binary compound, atoms of element A form a hcp structure and those of element M occupy 2/3 of the tetrahedral voids of the hcp structure. The formula of the binary compound is :

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A crystal is made up of metal ions 'M

_{1}' and 'M_{2}' and oxide ions. Oxide ions form a ccp lattice structure. The cation 'M_{1}' occupies 50% of octahedral voids and the cation 'M_{2}' occupies 12.5% of tetrahedral voids of oxide lattice. The oxidation numbers of 'M_{1}' and 'M_{2}' are, respectively :3

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An element crystallises in a face-centred cubic (fcc) unit cell with cell edge $$a$$. The distance
between the centres of two nearest octahedral voids in the crystal lattice is :

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A diatomic molecule X

(Avogadro constant (N

_{2}has a body-centred cubic (bcc) structure with a cell edge of 300 pm. The density of the molecule is 6.17 g cm^{–3}. The number of molecules present in 200 g of X_{2}is :(Avogadro constant (N

_{A}) = 6 $$ \times $$ 10^{23}mol^{–1})Questions Asked from Solid State (MCQ (Single Correct Answer))

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