LEARNING OBJECTIVES

  • Adapt the Bohr model for hydrogen to many-electron atoms.
  • Identify periodic trends in ionization energy and atomic size. Explain these in terms of the men-in-well model.
  • Recognize that the adjective valence describes the electrons that are most readily lost during successive ionizations. Identify the number of valence electrons in atoms of the “representative elements”.
  • Recognize that at normal temperatures and pressures, for non-metals, the maximum number of valence electrons per atom is eight (with the exception of two for H and He).
  • Use the men-in-well model and the difference in attraction of valence electrons by the nuclei of metal and non-metal atoms to explain the formation of binary ionic compounds.
  • Show that the men-in-well model is not adequate to represent the formation of a covalent bond between non-metal atoms.
  • Compare strengths and weakness of various ways (molecular, line, structural) to represent covalent molecules.
  • Use Lewis diagrams to represent the sharing of valence electrons to form covalent bonds in compounds.

NOTES

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