Which set of compounds in the following pair of ionic compounds has the higher lattice energy?
(I) KCl or MgO (II) LiF or LiBr (III) MgF2 or NaCl
KCl,LiBr,MgF2
MgO,LiBr,MgF2
MgO,LiF,NaCl
MgO,LiF,MgF2
A
MgO,LiF,NaCl
B
MgO,LiF,MgF2
C
KCl,LiBr,MgF2
D
MgO,LiBr,MgF2
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Solution
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Lattice energy depends upon two factors:
charge on ion (greater the charge higher is the lattice energy)
size of ion (smaller the size of ion greater is the lattice energy)
Among KCl and MgO, K has charge +1 and Mg has charge +2. Also, K+ has larger ionic radii than Mg+2. So, both the factors add up and the lattice energy of MgO is higher than KCl.
LiF and LiBr have the same cation and same ionic charge. So lattice energy depends upon the size of anion. F− is smaller than Br−, therefore, lattice energy of LiF is higher than LiBr.
MgF2 has a charge +2 while NaCl has a charge +1. Therefore, lattice energy of MgF2 is higher than NaCl.
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Which set of compounds in the following pair of ionic compounds has the higher lattice energy?
(I) KCl or MgO (II) LiF or LiBr (III) MgF2 or NaCl
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Q2
Arrange the following in increasing lattice energy: LiF,LiBr,LiI.