Chapter 9 Chemical Bonding I: Lewis Theory. Outline Lewis Theory Types of Chemical Bonds Ionic Born-Haber Cycle Lattice Energy Covalent Electronegativity Lewis Structures Bond Energy Bond Length Metallic. Potential Energy versus Distance.
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Tro: Chemistry: A Molecular Approach, 2/e
Calculate the enthalpy of formation of sodium chloride from it’s elements. Given:
Na (s) → Na (g) +107.3 kJ/mol
Na (g) → Na+(g) + 1 e- +495.8 kJ/mol
½ Cl2 (g) → Cl (g) +122 kJ/mol
Cl (g) + 1 e- → Cl- (g) -348.6 kJ/mol
Na+ (g) + Cl- (g) → NaCl (s) -787 kJ/mol
Calculate the energy released in kJ/mol when sodium iodide is formed.
Na (s) + ½ I2 (s) → NaI (s)
The energy of vaporization of elemental sodium is 107 kJ/mol. The ionization energy of sodium is 486 kJ/mol. The sum of the enthalpies of dissociation and vaporization of elemental iodine is 214 kJ/mol and the electron affinity of iodine is -295 kJ/mol. The lattice energy of sodium iodide is -704 kJ/mol.
Calculate the energy released in kJ/mol when lithium hydride is formed. The heat of vaporization of elemental lithium is 161 kJ/mol, the ionization energy of lithium is 520 kJ/mol. The dissociation energy of hydrogen gas is 436 kJ/mol and the electron affinity of a gaseous hydrogen atom is -73 kJ/mol. The lattice energy of lithium hydride is -917 kJ/mol.
Determine the energy of formation of magnesium bromide. Given:
Mg (s) → Mg (g) +147.7 kJ/mol
Mg (g) → Mg+(g) + 1 e- +737.7 kJ/mol
Mg+(g) → Mg2+ (g) + 1 e- +1,450.7 kJ/mol Br2 (g) → 2 Br (g) +193 kJ/mol
Br (g) + 1 e- → Br- (g) -325 kJ/mol
Mg2+ (g) + 2 Br- (g) → MgBr2 (s) -2,440 kJ/mol
Approximate the ΔHrxn for the production of ammonia by the Haber process:
N2 (g) + 3 H2 (g) 2 NH3 (g)
Approximate the ΔHrxn for the combustion of methane:
CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)
Approximate the ΔHrxn for the halogenation of acetylene gas:
C2H2 (g) + 2 Cl2 (g) C2H2Cl4 (g)