Which of the following compounds has the highest lattice energy?
Practice Questions
1 question
Q1
Which of the following compounds has the highest lattice energy?
NaCl
MgO
KBr
CaF2
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).
Questions & Step-by-step Solutions
1 item
Q
Q: Which of the following compounds has the highest lattice energy?
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).
Steps: 6
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.
