CHEM 232 Lecture Notes - Lecture 4: Valence Electron, Lewis Structure, Noble Gas
Document Summary
Structural formula of polyatomic anions: count the total number of valence electron. Total= 18 electrons: use single covalent bonds to connect the atoms. O-n-o: beginning with the atom attached to the central atom, add the remaining electrons to complete octets. If the central atom does not have an octet, move pairs of nonbonding electron attached atoms to form multiple bonds with the central atom. Do so until the central atom has an octet. Isomers= different compounds with the same molecular formula. Electronegativity= ability of an element to attract bonding electrons: transfer of electrons- ionic bonds. Forms neutral salts (ion pairs) in network crystal lattices. Occurs between atoms of differing electronegativity (differences > 1. 9: sharing electrons- covalent bonds. Forms discrete molecules (each bond= 2 shared electrons) Occurs between atoms of similar electronegativity (differences 0 1. 9) Polar bonds: covalent bonds with unequal sharing of electrons. *bonds between atoms differing electronegativity (0. 5- 1. 9) *