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Write the Lewis structure for each molecule. d. CH4
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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 50
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.)
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Identify the steps involved in the Born–Haber cycle for the formation of MgO from its elements in their standard states.
Write the equation for the sublimation of solid magnesium to gaseous magnesium: \( \text{Mg(s)} \rightarrow \text{Mg(g)} \) with \( \Delta H_{\text{sub}} = 137 \text{ kJ/mol} \).
Write the equations for the ionization of gaseous magnesium: \( \text{Mg(g)} \rightarrow \text{Mg}^+(g) + e^- \) with \( \text{IE}_1 = 738 \text{ kJ/mol} \) and \( \text{Mg}^+(g) \rightarrow \text{Mg}^{2+}(g) + e^- \) with \( \text{IE}_2 = 1450 \text{ kJ/mol} \).
Write the equations for the electron affinity of oxygen: \( \text{O(g)} + e^- \rightarrow \text{O}^-(g) \) with \( \text{EA}_1 = -141 \text{ kJ/mol} \) and \( \text{O}^-(g) + e^- \rightarrow \text{O}^{2-}(g) \) with \( \text{EA}_2 = 744 \text{ kJ/mol} \).
Use Hess's law to combine these steps with the formation of MgO from its ions to solve for the lattice energy: \( \text{Mg}^{2+}(g) + \text{O}^{2-}(g) \rightarrow \text{MgO(s)} \).
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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 its constituent ions. It involves several steps, including the sublimation of the metal, ionization energy, electron affinity, and the formation of the ionic lattice. This cycle allows for the calculation of lattice energy indirectly by using known enthalpy changes.
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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 forces between the ions in an ionic compound. Higher lattice energy indicates stronger ionic bonds, which typically results in higher melting and boiling points for the compound.
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00:49Lattice Energy
Ionization Energy and Electron Affinity
Ionization energy (IE) is the energy required to remove an electron from a neutral atom in the gas phase, while electron affinity (EA) is the energy change that occurs when an electron is added to a neutral atom. In the context of the Born-Haber cycle, these energies are crucial for determining the energy changes associated with forming cations and anions from their respective atoms, which are essential steps in calculating lattice energy.
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01:34Electron Affinity
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