Multiple Choice
Which of the following correctly ranks the lattice energy of the salts NaCl, MgO, and KBr from highest to lowest?
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11. Bonding & Molecular Structure
Lattice Energy
Multiple Choice
Which of the following compounds would you expect to have the highest boiling point?
A
MgCl2
B
SrO
C
SrCl2
D
CsI
E
LiBr
Verified step by step guidance1
Step 1: Understand that boiling point is influenced by the strength of intermolecular forces. Ionic compounds typically have high boiling points due to strong ionic bonds.
Step 2: Consider the lattice energy, which is the energy required to separate one mole of a solid ionic compound into gaseous ions. Lattice energy is generally higher for compounds with smaller ions and higher charges.
Step 3: Compare the ionic charges and sizes of the given compounds. MgCl2, SrO, SrCl2, CsI, and LiBr all consist of ions with different charges and sizes.
Step 4: Analyze the charges: MgCl2 has Mg2+ and Cl-, SrO has Sr2+ and O2-, SrCl2 has Sr2+ and Cl-, CsI has Cs+ and I-, and LiBr has Li+ and Br-. Higher charges typically lead to higher lattice energy.
Step 5: Consider the ionic sizes: Smaller ions lead to higher lattice energy. Compare the sizes of the ions in each compound to determine which has the highest lattice energy, and thus the highest boiling point.
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