Domanda del libro di testo
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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Ch.10 - Chemical Bonding I: The Lewis Model
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 10, Problema 49
Use the Born–Haber cycle and data from Appendix IIB, Chapter 9 and this chapter to calculate the lattice energy of LiBr. (ΔHsub for lithium is 138 kJ>mol.)
Guida verificata passo dopo passo1
Identify the steps involved in the Born–Haber cycle for LiBr, which include sublimation of lithium, ionization of lithium, dissociation of bromine, electron affinity of bromine, and formation of LiBr from gaseous ions.
Write the equation for the sublimation of lithium: \( \text{Li(s)} \rightarrow \text{Li(g)} \) with \( \Delta H_{\text{sub}} = 138 \text{ kJ/mol} \).
Write the equation for the ionization of gaseous lithium: \( \text{Li(g)} \rightarrow \text{Li}^+(g) + e^- \) and use the ionization energy from the appendix.
Write the equation for the dissociation of bromine: \( \frac{1}{2} \text{Br}_2(g) \rightarrow \text{Br}(g) \) and use the bond dissociation energy from the appendix.
Write the equation for the formation of LiBr from gaseous ions: \( \text{Li}^+(g) + \text{Br}^-(g) \rightarrow \text{LiBr(s)} \) and solve for the lattice energy using Hess's law by summing all the enthalpy changes.
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Born-Haber Cycle
The Born-Haber cycle is a thermodynamic cycle that relates the lattice energy of an ionic compound to its formation enthalpy and the energies involved in the formation of gaseous ions. It combines several steps, including sublimation, ionization, and electron affinity, to calculate the lattice energy indirectly. This cycle is essential for understanding how ionic compounds form and the energy changes associated with these processes.
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03:49
Born Haber Cycle
Lattice Energy
Lattice energy is the energy released when gaseous ions combine to form an ionic solid, or conversely, the energy required to separate one mole of an ionic solid into its gaseous ions. It is a measure of the strength of the ionic bonds in the solid and is influenced by the charges of the ions and the distance between them. Higher lattice energy indicates stronger ionic interactions and greater stability of the ionic compound.
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00:49Lattice Energy
Enthalpy Changes
Enthalpy changes refer to the heat content changes during chemical reactions or phase changes at constant pressure. In the context of the Born-Haber cycle, various enthalpy changes such as sublimation, ionization, and electron affinity are used to calculate the overall enthalpy change for the formation of an ionic compound. Understanding these enthalpy changes is crucial for accurately determining the lattice energy and predicting the stability of ionic compounds.
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02:34Enthalpy of Formation
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Use the Born–Haber cycle and data from Appendix IIB and Table 10.3 to calculate the lattice energy of MgO. (ΔHsub for magnesium is 137 kJ/mol; IE1 and IE2 for magnesium are 738 kJ/mol and 1450 kJ/mol, respectively; EA1 and EA2 for O are −141 kJ/mol and 744 kJ/mol, respectively.)