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Chemistry 1211 Rules for Establishing Oxidation Numbers 1. Any uncombined atom, or any atom in a molecule of an element, is assigned an oxidation number of zero. Examples: N2, Cl2, C, Sn, S8 2. The oxidation number of a simple, monatomic ion is the same as the charge on the ion. Examples: Na+ is +1, Cu+2 is +2, Cu+ is +1, F¯ is -1. 3. The oxidation numbers of some common atoms are: a. Fluorine, the most electronegative element, is -1 in all fluorine containing compounds. b. In most oxygen containing compounds oxygen is -2. In peroxides (i.e. H2O2) each oxygen has an oxidation number of -1. In the compound OF2, the oxygen atom has an oxidation number of +2. c. Hydrogen usually has an oxidation number of +1 except in metallic hydrides where it then has an oxidation number of -1 Examples: HCl, hydrogen is +1; NaH, hydrogen is -1. d. The halogens, unless bonded to an element with a higher electronegativity, have an oxidation number of -1. Examples: NaCl, chlorine is -1; HClO4, chlorine is +7. 4. Since chemical compounds are neutral, it stands to reason that the algebraic sum of their oxidation numbers must equal zero. Examples: NaCl, sodium is +1, chlorine is -1, total is 0 CO2, carbon is +4, oxygen is -2 (so -4 for two), total is 0. 5. The sum of the oxidation numbers of atoms comprising a polyatomic ion equals the charge on the ionic group. Examples: SO4-2, sulfur is +6, oxygen is -2 (so -8 for four), total is -2. NH4+, nitrogen is -3, hydrogen is +1 (so +4 for four), total is +1.