Textbook Question
Write the Lewis symbols for the ions in each ionic compound. c. CaI2
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Ch.9 - Chemical Bonding I: The Lewis Model
Chapter 9, Problem 43
What is the trend in the lattice energies of alkaline earth metal oxides? Here are the lattice energies (in kJ/mol): MgO -3795, CaO -3414, SrO -3217, BaO -3029.
Verified step by step guidance1
Identify the alkaline earth metals involved: magnesium (Mg), calcium (Ca), strontium (Sr), and barium (Ba).
Recognize that lattice energy is the energy required to separate one mole of an ionic solid into its gaseous ions.
Observe the given lattice energies: MgO (-3795 kJ/mol), CaO (-3414 kJ/mol), SrO (-3217 kJ/mol), BaO (-3029 kJ/mol).
Note the trend in lattice energies: as you move down the group from MgO to BaO, the lattice energy becomes less negative, indicating a decrease in lattice energy.
Understand that this trend is due to the increasing ionic size of the metal cations as you move down the group, which results in a decrease in the electrostatic attraction between the ions.
Related Practice
Textbook Question
Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Sr and Se b. Ba and Cl c. Na and S d. Al and O
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Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Ca and N b. Mg and I c. Ca and S d. Cs and F
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Textbook Question
Rubidium iodide has a lattice energy of -617 kJ/mol, while potassium bromide has a lattice energy of -671 kJ/mol. Why is the lattice energy of potassium bromide more exothermic than the lattice energy of rubidium iodide?
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Textbook Question
The lattice energy of CsF is -744 kJ/mol, whereas that of BaO is -3029 kJ/mol. Explain this large difference in lattice energy.
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Textbook Question
Use the Born–Haber cycle and data from Appendix IIB, Chapter 8 and this chapter to calculate the lattice energy of KCl. (ΔHsub for potassium is 89.0 kJ/mol.)
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