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Which of the following compounds has the highest lattice energy?

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Question: Which of the following compounds has the highest lattice energy?

Options:

  1. NaCl
  2. MgO
  3. KBr
  4. CaF2

Correct Answer: MgO

Solution: 

Lattice energy increases with charge and decreases with size. MgO has a higher charge (2+) compared to NaCl (1+), KBr (1+), and CaF2 (2+ but larger size).

Which of the following compounds has the highest lattice energy?

Practice Questions

Q1
Which of the following compounds has the highest lattice energy?
  1. NaCl
  2. MgO
  3. KBr
  4. CaF2

Questions & Step-by-Step Solutions

Which of the following compounds has the highest lattice energy?
  • Step 1: Understand what lattice energy is. It is the energy released when ions come together to form a solid ionic compound.
  • Step 2: Know that lattice energy increases with the charge of the ions. Higher charges mean stronger attractions between the ions.
  • Step 3: Know that lattice energy decreases with the size of the ions. Larger ions are further apart, which weakens the attraction.
  • Step 4: Compare the charges of the compounds: MgO has Mg(2+) and O(2-), NaCl has Na(1+) and Cl(1-), KBr has K(1+) and Br(1-), and CaF2 has Ca(2+) and F(1-).
  • Step 5: Identify that MgO has the highest charge (2+) compared to NaCl and KBr (1+) and CaF2 (2+ but larger size).
  • Step 6: Conclude that MgO has the highest lattice energy because it has the highest charge and is not larger than CaF2.
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