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I. Introduction to Bonding (p. 161 – 163)

Ch. 6 & 7 - Chemical Bonding. I. Introduction to Bonding (p. 161 – 163). A. Vocabulary. Chemical Bond attractive force between atoms or ions that binds them together as a unit bonds form in order to… decrease potential energy (PE) increase stability. A. Vocabulary. CHEMICAL FORMULA.

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I. Introduction to Bonding (p. 161 – 163)

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  1. Ch. 6 & 7 - Chemical Bonding I. Introduction toBonding(p. 161 – 163) C. Johannesson

  2. A. Vocabulary • Chemical Bond • attractive force between atoms or ions that binds them together as a unit • bonds form in order to… • decrease potential energy (PE) • increase stability C. Johannesson

  3. A. Vocabulary CHEMICAL FORMULA IONIC COVALENT Formula Unit Molecular Formula NaCl CO2 C. Johannesson

  4. A. Vocabulary COMPOUND more than 2 elements 2 elements Binary Compound Ternary Compound NaCl NaNO3 C. Johannesson

  5. A. Vocabulary ION 2 or more atoms 1 atom Monatomic Ion Polyatomic Ion Na+ NO3- C. Johannesson

  6. B. Types of Bonds COVALENT IONIC e- are transferred from metal to nonmetal e- are shared between two nonmetals Bond Formation Type of Structure true molecules crystal lattice Physical State liquid or gas solid Melting Point low high Solubility in Water yes usually not yes (solution or liquid) Electrical Conductivity no Other Properties odorous C. Johannesson

  7. B. Types of Bonds METALLIC e- are delocalized among metal atoms Bond Formation Type of Structure “electron sea” Physical State solid Melting Point very high Solubility in Water no yes (any form) Electrical Conductivity malleable, ductile, lustrous Other Properties C. Johannesson

  8. C. Bond Polarity • Most bonds are a blend of ionic and covalent characteristics. • Difference in electronegativity determines bond type. C. Johannesson

  9. C. Bond Polarity • Electronegativity • Attraction an atom has for a shared pair of electrons. • higher e-neg atom  - • lower e-neg atom + C. Johannesson

  10. C. Bond Polarity • Electronegativity Trend (p. 151) • Increases up and to the right. C. Johannesson

  11. C. Bond Polarity • Nonpolar Covalent Bond • e- are shared equally • symmetrical e- density • usually identical atoms C. Johannesson

  12. - + C. Bond Polarity • Polar Covalent Bond • e- are shared unequally • asymmetrical e- density • results in partial charges (dipole) C. Johannesson

  13. C. Bond Polarity • Nonpolar • Polar • Ionic C. Johannesson View Bonding Animations.

  14. C. Bond Polarity Examples: • Cl2 • HCl • NaCl 3.0-3.0=0.0 Nonpolar 3.0-2.1=0.9 Polar 3.0-0.9=2.1 Ionic C. Johannesson

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