CHEM 107 Lecture Notes - Lecture 48: Covalent Bond, Bond Order, Nonmetal
Document Summary
Covalent bonds are formed between atoms that share electrons (nonmetal + nonmetal) Number of electron pairs being shared by a pair of atoms. Three atoms sharing 3 pairs of electrons (6 total) Shorter and strong than comparable single or double bonds. A roadmap to lewis structures: determine the total number of electrons to use in structure. This equals the sum of the valence electrons for each of the atoms in the molecule. If the molecule is an anion, add the number of the anion charge to the electron count. If the molecule is a cation, subtract the number of the cation charge from the electron count. Cn- = 4 + 5 + 1 = 10e- Cf4 = 4 + 28 = 32e: arrange atoms appropriately. Carbon is always in the middle, hydrogen would never be. Think about how many bonds each atom can form. H and all group 7 elements can only form 1 bond, so they are always terminal.
