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Chemical Bonding

Chemical Bonding. Molecular Geometry. Ch. 6 Sections 1-4 Review. In general, what determines whether atoms will form chemical bonds? Atoms will form a chemical bond if their potential energy is lowered in doing so. Describe the difference between ionic and covalent bonding.

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Chemical Bonding

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  1. Chemical Bonding Molecular Geometry

  2. Ch. 6 Sections 1-4 Review • In general, what determines whether atoms will form chemical bonds? Atoms will form a chemical bond if their potential energy is lowered in doing so. • Describe the difference between ionic and covalent bonding. Ionic bonds form as a result of the transfer of electrons between two atoms with a large difference in electronegativity. Covalent bonds form when electrons are shared between two atoms of similar or slightly different electronegativity.

  3. Ch. 6 Sections 1-4 Review • What types of bonds form between the following pairs of atoms: Ca-Cl, O-H, O-O? Ionic, polar covalent, nonpolar covalent • What is the meaning of the word polar, as applied to chemical bonding? Polar refers to bonds that have an uneven distribution of charge. • What type of bonding exists (ionic or covalent) in the compounds: NaCl, H2O, CH4? Ionic, covalent, covalent

  4. Ch. 6 Sections 1-4 Review • List 3 properties of ionic compounds. Hardness, brittleness, electrical conductivity in molten state, high melting and boiling points. • What accounts for the properties of ionic compounds listed above? Cations and anions are arranged in a crystal lattice. • Draw the Lewis dot diagram for C3H6.

  5. Ch. 6 Sections 1-4 Review • How are single, double, and triple covalent bonds different? One, two, and three pairs of electrons are shared; bond energy increases with the number of bonds and bond length decreases with the number of bonds. • Draw the Lewis dot structure for SO2. Show both resonance structures.

  6. Ch. 6 Sections 1-4 Review • What properties of metals contribute to their tendency to form metallic bonds? Most metals have unfilled outermost orbitals, low ionization energies, and low electronegativities. • What are some common properties of metals? Electrical and thermal conductivity, luster, malleability, ductility, high melting and boiling points

  7. Hybridization Hybridization – mixing of atomic orbitals of similar energy to produce new orbitals of equal energy

  8. Hybridization

  9. Intermolecular Forces • Covalent, ionic, and metallic bonds can be considered to be intra-molecular forces Intermolecular Forces- forces of attraction between molecules; weaker than covalent, ionic, and metallic bonds.

  10. Boiling Points and Bonding Types

  11. Boiling Points and Bonding Types

  12. Molecular Polarity • Molecular polarity depends on the polarity of the bonds that make up a compound and the molecular shape. • A dipole moment results when a polar molecule has a center for positive charge separate from a center for negative charge

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