8. ch08-Chemical Bonding General Concepts.pdf - Ch 8 Chemical Bonding General Concepts Brady Senese 5th Ed Index 8.1 Electron transfer leads to the

8. ch08-Chemical Bonding General Concepts.pdf - Ch 8...

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Ch. 8 Chemical Bonding: General Concepts Brady & Senese, 5th Ed
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Index 8.1. Electron transfer leads to the formation of ionic compounds 8.2. Lewis symbols help keep track of valence electrons 8.3. Covalent bonds are formed by electron sharing 8.4. Covalent bonds can have partial charges at opposite ends 8.5. The reactivities of metals and nonmetals can be related to their electronegativities 8.6. Drawing Lewis structures is a necessary skill 8.7. Resonance applies when a single Lewis structure fails
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8.1 Electron transfer leads to the formation of ionic compounds 3 Lattice Energy, U Compound Ions Lattice Energy (kJ mol −1 ) LiCl Li + and Cl 845 NaCl Na + and Cl 778 KCl K + and Cl 709 LiF Li + and F 1033 CaCl 2 Ca 2+ and Cl 2258 AlCl 3 Al 3+ and Cl 5492 CaO Ca 2+ and O 2- 3401 Al 2 O 3 Al 3+ and O 2- 15,916 Formation of gaseous ions from an ionic solid A x B y(s) →xB y+ (g) + yB x- (g)
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8.1 Electron transfer leads to the formation of ionic compounds 4 Born Haber Cycle for NaCl 2Na (s) + Cl 2(g) → 2NaCl (s) What has to happen? Sublime Na: ΔH sub = 107.8 kJ/mol Ionize Na: IE 1 = 495.4 kJ/mol Break Cl bond: ½( D Cl-Cl ) = 121.3 kJ/mol Ionize Cl: EA = -348.8 kJ/mol Form bond: -U = -787 kJ/mol
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