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Covalent Bonding

Covalent Bonding. Sharing. Covalent Bonding. A form of chemical bonding where electrons are shared so that each atom has a complete valence shell One particle of a covalent compound is called a molecule. Types of Bonds. Single bond – 2 electrons (1 pair) are shared.

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Covalent Bonding

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  1. Covalent Bonding Sharing

  2. Covalent Bonding • A form of chemical bonding where electrons are shared so that each atom has a complete valence shell • One particle of a covalent compound is called a molecule.

  3. Types of Bonds • Single bond – 2 electrons (1 pair) are shared. • Double bond – 4 electrons (2 pairs) are shared. • Triple bond – 6 electrons (3 pairs) are shared.

  4. Other Names for Bond Types • A single bond is a sigma bond. • Double and triple bonds contain pi bonds. • Double = 1 sigma, 1 pi • Triple = 1 sigma, 2 pi

  5. Naming Binary Covalent Compounds • Identification = Use this system with nonmetal-nonmetal pairs • If the compound contains a metal, it is likely an ionic compound – use the other set of rules for those compounds. Naming Rule • First word = prefix + 1st element name • Second word = prefix + 2nd element name with –ide ending

  6. mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- Prefixes Exception: Use mono on the second word only, never the first word.

  7. Examples – Writing Names • N2O • SiF4 • N2O5 • NH3

  8. Examples – Writing Formulas • sulfur trioxide • dihydrogen monoxide

  9. VSEPR Theory • Valence Shell Electron Pair Repulsion Theory • Electron pairs orient themselves in order to minimize repulsive forces. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  10. Lone pairs repel more strongly than bonding pairs!!! VSEPR Theory • Types of e- Pairs • Bonding pairs - form bonds • Lone pairs - nonbonding electrons Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  11. Bond Angle VSEPR Theory • Lone pairs reduce the bond angle between atoms. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  12. Know the 8 common shapes & their bond angles! 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. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  13. B A B BeH2 Common Molecular Shapes 2 total 2 bond 0 lone LINEAR 180° Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  14. H2O Common Molecular Shapes 4 total 2 bond 2 lone BENT 104.5° Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  15. SO2 Common Molecular Shapes 3 total 2 bond 1 lone BENT <120° Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  16. B A B B BF3 Common Molecular Shapes 3 total 3 bond 0 lone TRIGONAL PLANAR 120° Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  17. B A B B B CH4 Common Molecular Shapes 4 total 4 bond 0 lone TETRAHEDRAL 109.5° Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  18. NH3 Common Molecular Shapes 4 total 3 bond 1 lone TRIGONAL PYRAMIDAL 107° Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  19. Ba PCl5 Be A Be Be Ba Common Molecular Shapes 5 total 5 bond 0 lone TRIGONAL BIPYRAMIDAL 120°/90° Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  20. SF6 B B B A B B B Common Molecular Shapes 6 total 6 bond 0 lone OCTAHEDRAL 90° Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  21. F P F F Examples • PF3 4 total 3 bond 1 lone TRIGONAL PYRAMIDAL 107° Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  22. OCO Examples • CO2 2 total 2 bond 0 lone LINEAR 180° Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

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