Chemistry - With OWLv2 MindTap Access
10th Edition
ISBN: 9781337537735
Author: ZUMDAHL
Publisher: CENGAGE L
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Textbook Question
Chapter 8, Problem 63E
Consider the following energy changes:
∆E(kJ/mol) | |
Mg(g)→ Mg+(g) + e− | 735 |
Mg+ (g) → Mg2+(g) + e− | 1445 |
O(g) + e− → + O− (g) | −141 |
O−(g) + e− → O2− (g) | 878 |
Magnesium oxide exists as Mg2+O2− and not as Mg+O−. Explain.
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Check out a sample textbook solutionStudents have asked these similar questions
Draw the energy diagram of the reaction: Na(s) + ½Cl2 → NaCl.
Enthalpy (kJ/mol)
Na(s) → Na(g) +108
Na(g) → Na+(g) + e +496
½ Cl2 →Cl(g) +121
Cl(g) + e → Cl-(g) -349
Use the data in the table below to calculate the lattice energy of KCI.
K(s) → K(g)
K(g) → K+ (g) + e¯
Cl₂(g) → Cl(g)
Cl(g) + e Cl¯ (g)
→
K(s) + ½Cl₂(g) → KCl(s)
155.2
90.0 kJ/mol
418.8 kJ/mol
122 kJ/mol
-349 kJ/mol
-437 kJ/mol
1. Below is a list of enthalpy changes for the Born-Haber cycle for the formation of solid LiF from Li(s) and F(g). Use these data to determine the lattice energy for the formation LiF(s). Li(s) → Li(g) ΔH1 = +162 kJ/mol Li(g) → Li+(g) + e- ΔH2 = +520.2 kJ/molF2(g) → 2F(g) ΔH3 = 154 kJ/mol F(g) + e- → F-(g) ΔH4 = -328 kJ/molLi(s) + 1/2F2(g) → LiF(s) ΔHf = -612 kJ/mol
Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer.
a. 1371 kJ/mol
b. -1371 kJ/mol
c. 1043 kJ/mol
d. -1043 kJ/mol
Chapter 8 Solutions
Chemistry - With OWLv2 MindTap Access
Ch. 8 - Distinguish between the terms electronegativity...Ch. 8 - When an element forms an anion, what happens to...Ch. 8 - Define the term lattice energy. Why,...Ch. 8 - Explain how bond energies can be used to estimate...Ch. 8 - Prob. 5RQCh. 8 - Explain the terms resonance and delocalized...Ch. 8 - Define formal charge and explain how to calculate...Ch. 8 - Give two requirements that should be satisfied for...Ch. 8 - Consider the following compounds: CO2, SO2, KrF2,...Ch. 8 - Explain the electronegativity trends across a row...
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