Unit 4: Chemical Bonding and Molecular Structure Chapter 6 Notes ...

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6.4 Metallic Bonding I. The Metallic Bond Model A. Metallic Bonding 1. The chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons B. Electron Delocalization in Metals 1. Vacant p and d orbitals in metal's outer energy levels overlap, and allow outer electrons to move freely throughout the metal 2. Valence electrons do not belong to any one atom II. Metallic Properties A. Metals are good conductors of heat and light B. Metals are shiny 1. Narrow range of energy differences between orbitals allows electrons to be easily excited, and emit light upon returning to a lower energy level C. Metals are Malleable 1. Can be hammered into thin sheets D. Metals are ductile 1. Ability to be drawn into wire a. Metallic bonding is the same in all directions, so metals tend not to be brittle E. Metals atoms organized in compact, orderly crystalline patterns F. Different metallic elements (and carbon) can be mixed to form alloys 1. Sterling silver a. Ag = 92.5%, Cu = 7.5% 2. Brass a. Cu = 60%, Zn = 40% 6.5 Molecular Geometry A. VSEPR theory 1. valence-‐shell, electron-‐pair repulsion 2. states that repulsion between the sets of valence-‐level electrons surrounding an atom causes these sets to be oriented as far apart as possible 3. shared pairs of electrons will be as far apart from each other as possible B. Unshared Electron Pairs 1. Lone pairs (unshared electron pairs) occupies space around the atom just as bonding pairs do. 2. Lone pairs have a relatively greater effect on geometry than shared pairs (Have greater repusive forces & tend to compress the angles between bonding pairs) C. Double and triple bonds are treated in the same way as single bonds D. Polyatomic ions are treated similarly to molecules.
E. Molecular Polarity 1. The uneven distribution of molecular charge 2. A dipole is created by equal but opposite charges that are separated by a short distance. 3. The direction of the dipole is from the positive pole to its negative pole 4. A dipole is represented by an arrow with a head pointing toward the negatie pole and a crossed tail situated at the positive pole.
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Page 3 and 4: 2. can not be broken up by d
Page 5: A. Resonance Structure: bonding

Unit 4: Chemical Bonding and Molecular Structure Chapter 6 Notes ...

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