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METALLIC BOND bond found in metals; holds metal atoms together very strongly

METALLIC BOND bond found in metals; holds metal atoms together very strongly. Metallic Bond. Formed between atoms of metallic elements Electron cloud around atoms Good conductors at all states, lustrous, very high melting points Examples; Na, Fe, Al, Au, Co.

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METALLIC BOND bond found in metals; holds metal atoms together very strongly

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  1. METALLIC BONDbond found in metals; holds metal atoms together very strongly

  2. Metallic Bond • Formed between atoms of metallic elements • Electron cloud around atoms • Good conductors at all states, lustrous, very high melting points • Examples; Na, Fe, Al, Au, Co

  3. Ionic Bond, A Sea of Electrons

  4. Metals Form Alloys Metals do not combine with metals. They form Alloys which is a solution of a metal in a metal. Examples are steel, brass, bronze and pewter.

  5. C. Polyatomic Ions • NH4+ 1 N × 5e- = 5e- 4 H × 1e- = 4e- 9e- H H N H H - 1e- 8e- - 8e- 0e- C. Johannesson

  6. D. Resonance Structures • Molecules that can’t be correctly represented by a single Lewis diagram. • Actual structure is an average of all the possibilities. • Show possible structures separated by a double-headed arrow. C. Johannesson

  7. O O S O O O S O O O S O D. Resonance Structures • SO3 C. Johannesson

  8. 6 electrons in the : : : : : : valence shells of boron F C l and aluminum : : : F B : C l A l : : : : F : : C l : : Boron trifluoride Exceptions to the Octet Rule • Molecules containing atoms of Group 3A elements, particularly boron and aluminum Aluminum chloride

  9. Exceptions to the Octet Rule • Atoms of third-period elements have 3d orbitals and may expand their valence shells to contain more than 8 electrons • phosphorus may have up to 10

  10. Exceptions to the Octet Rule • sulfur, another third-period element, forms compounds in which its valence shell contains 8, 10, or 12 electrons

  11. A. VSEPR Theory • Valence Shell Electron Pair Repulsion Theory • Electron pairs orient themselves in order to minimize repulsive forces. C. Johannesson

  12. Lone pairs repel more strongly than bonding pairs!!! A. VSEPR Theory • Types of e- Pairs • Bonding pairs - form bonds • Lone pairs - nonbonding e- C. Johannesson

  13. Bond Angle A. VSEPR Theory • Lone pairs reduce the bond angle between atoms. C. Johannesson

  14. B. Determining Molecular Shape • Draw the Lewis Diagram. • Tally up e- pairs on central atom. • double/triple bonds = ONE pair • Shape is determined by the # of bonding pairs and lone pairs. Know the 8 common shapes & their bond angles! C. Johannesson

  15. BeH2 C. Common Molecular Shapes 2 total 2 bond 0 lone LINEAR 180° C. Johannesson

  16. C. Common Molecular Shapes 3 total 3 bond 0 lone BF3 TRIGONAL PLANAR 120° C. Johannesson

  17. C. Common Molecular Shapes 3 total 2 bond 1 lone SO2 BENT <120° C. Johannesson

  18. C. Common Molecular Shapes 4 total 4 bond 0 lone CH4 TETRAHEDRAL 109.5° C. Johannesson

  19. C. Common Molecular Shapes 4 total 3 bond 1 lone NH3 TRIGONAL PYRAMIDAL 107° C. Johannesson

  20. C. Common Molecular Shapes 4 total 2 bond 2 lone H2O BENT 104.5° C. Johannesson

  21. C. Common Molecular Shapes 5 total 5 bond 0 lone PCl5 TRIGONAL BIPYRAMIDAL 120°/90° C. Johannesson

  22. C. Common Molecular Shapes 6 total 6 bond 0 lone SF6 OCTAHEDRAL 90° C. Johannesson

  23. D. Examples • PF3 4 total 3 bond 1 lone TRIGONAL PYRAMIDAL 107° C. Johannesson

  24. D. Examples • CO2 2 total 2 bond 0 lone LINEAR 180° C. Johannesson

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