- 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.