5.3 – Lewis Structures
Octet Rule – chemical compounds tend to form so that each atom, by gaining, losing, or sharing
electrons, has an octet (8) of electrons in its highest occupied energy level.
*exceptions: Hydrogen (2), Boron (6)
Electron Dot Notation – an electron configuration in which only the valence electrons of an atom are
shown (these are indicated by dots placed around the element’s symbol).
*Draw the dot notation for the following:
1. Na 2. Mg 3. B 4. C 5. N 6. O 7. F
Lewis Structures – formulas in which atomic symbols represent nuclei, dot pairs or dashes represent
covalent bonds, and dots adjacent to one atomic symbol represent unshared electrons.
*example:
Multiple Covalent Bonds – atoms of some elements can often share more than one pair of electrons.
Multiple bonds have greater bond energies and are shorter than single bonds.
*example of a double bond
*example of a triple bond
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