The correct order of the lattice energies of the following ionic compounds is:

N a C l > M g B r_{2} > C a O > A l_{2} O_{3}

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A l_{2} O_{3} > M g B r_{2} > C a O > N a C l

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M g B r_{2} > A l_{2} O_{3} > C a O > N a C l

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A l_{2} O_{3} > C a O > M g B r_{2} > N a C l

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Solution

The correct option is D $A l_{2} O_{3} > C a O > M g B r_{2} > N a C l$
As we move across the period,charge density of cation increases thus lattice energy increases.
$N a^{+} < M g^{2 +} < A l^{3 +}$
As we move down, the size increases which results in decrease of lattice energy.
$L i^{+} < N a^{+} < K^{+}$
In this question, we have following cations ( $N a^{+}, M g^{2 +}, A l^{3 +}, C a^{2 +}$ ) which can be arranged according to their lattice energies as
$N a^{+} < M g^{2 +} < C a^{2 +} < A l^{3 +}$
Therefore , order of lattice energy of ionic compound
$A l_{2} O_{3} > C a O > M g B r_{2} > N a C l$

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