Section 12.4 Bonding in Solids

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Presentation transcript:

Section 12.4 Bonding in Solids

Bonding in Ionic and Metallic Solids In these sections… Control of ionic bond strength Determining lattice energy: Born-Haber Cycles Band Theory: Metallic bonding Band Theory: Semicondictors

Ionic Bonding Lattice Energy: Trends

Determining Lattice Energy: Born-Haber Cycles Conceptualize Ionic Compound Formation: Na(s) + ½ Cl2(g)  NaCl(s) H = -lattice energy Step 1. Vaporize Na(s) Na(s)  Na(g) Hosublimation = 107 kJ Step 2. Ionize Na(g) Na(g)  Na+(g) + e- Ionization Energy = 496 kJ Step 3. Break Cl-Cl bond (need only 1 Cl) ½ Cl-Cl(g)  Cl(g) ½ Cl-Cl Bond = ½ 242 kJ = 121kJ Step 4. Ionize Cl(g) Cl(g) + e-  Cl-(g) Electron Affinity = -349 kJ Step 5. Lattice Formation Na+(g) + Cl-(g)  NaCl(s) Energy = U, Lattice Energy Steps 1 through 5 = Hoformation (NaCl(s))= -411 kJ Solve for U = (-107 + -496 + -121 + 349 + -411) kJ = -786 kJ Lattice energy = 786 kJ/mol

Metallic Bonding: Band Theory

Metallic Bonding: Trends sim

Semiconductors: Band Theory

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