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Question

Which of the following pairs is not the correct order of lattice energy?

A
KCl>MgO
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B
AlN>MgO
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C
CaO>BaO
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D
MgCO3>CaCO3
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Solution

The correct option is A KCl>MgO
As the charge on the ions (cations and anions) increase, the lattice energy increases, and it decreases when the size of the ions (cations and anions) increases.

a) Size: K+>Mg2+
Charge: +1<+2
Size: Cl>O2
Charge: 1<2
Thus, the lattice energy of MgO is greater than KCl.

b) Size: Al3+<Mg2+
Charge: +3>+2
Size: N3>O2
Charge: 3>2
Here, the charge factor dominates and hence the lattice energy of AlN is greater than MgO.

c) Size: Ca2+<Ba2+
Charge: +2=+2
Size: O2=O2
Charge: 2=2
The lattice energy of CaO is greater than BaO.

d) Size: Mg2+<Ca2+
Charge: +2=+2
Size: CO23=CO23
Charge: 2=2
The lattice energy of MgCO3 is greater than the CaCO3.

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