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Chemical Bonding

This section explores the different types of chemical bonds including ionic, covalent, and metallic bonds. It also covers the concept of Lewis symbols and the octet rule, as well as the energetics and lattice energy of ionic bond formation. The differences between ionic and covalent bonding are discussed, along with the significance of single, double, and triple bonds.

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Chemical Bonding

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  1. Chemical Bonding Sections 8.1-8.3

  2. Objectives • Identify types of chemical bonds • Revisit Lewis symbols • Analyze ionic bonding • Compare and contrast ionic and covalent bonding • Identify single, double, and triple bonds

  3. Chemical bond Ionic bond Covalent bond Metallic bond Lewis symbol Octet rule Lattice energy Lewis structure Single bond Double bond Triple bond Bond length Key Terms

  4. Chemical Bonds • Strong attachment between two atoms/ions • 3 Types • Ionic: 8.2 • Covalent: 8.3 • Metallic: Chap 23

  5. Lewis Symbols • Another name for electron-dot symbols • Named for American chemist • Shows only valence electrons • REVIEW: Nitrogen, Oxygen, Bromine

  6. Octet Rule • Atoms tend to gain, lose, or share electrons to get 8 valence electrons • Full s and p • Many exceptions BUT good framework

  7. Ionic Bonding • Electrons transferred from atom to atom • Cation and anion formed • Electrostatic forces exist between ions of opposite charge

  8. Ex: NaCl Na + Cl  Na+ + [ Cl ]- Each has an octet Na+ :2s22p6 Cl- : 3s23p6

  9. Energetics of Ionic Bond Formation • Formation is very exothermic • Lose of electron is endothermic • Gain of electron is exothermic • Attraction of opposite charges releases energy when stabilized

  10. Lattice Energy • Measure of stabilization • Energy required to completely separate a mole of a solid ionic compound into its gaseous ions • Table 8.2 page 305 + if separating - if forming

  11. Magnitude of Lattice Energy • Charge of ions • Ionic size • Arrangement of solids

  12. Trends • Lattice Energy as charge of ions and radii

  13. Transition Metals

  14. Polyatomic Ions • Do not forget about them! • They are often anion (or cation for NH4+) of ionic compounds

  15. Covalent Bonding • Majority of substances • Sharing of pairs of electrons

  16. Ionic vs. Covalent

  17. Lewis Structure • Electron-dot diagrams for molecules • Dots represent lone pairs of electrons • A line represents shared electrons

  18. Lewis Structures H-H H ö: H

  19. Multiple Bonds • Single bond- 1 pair of electrons are shared • Double bond- 2 pairs are shared • Triple bond- 3 pairs are shared

  20. Single Bond

  21. Double Bond

  22. Triple Bond

  23. Bond Length • Distance between nuclei of atoms in a bond • Decreases as number of shared pairs increases

  24. Homework • 8.8-8.24 and 8.30-8.34 on page 336-337 • Black problems only • Due Monday 3/23

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