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Oxidation state, also known as oxidation number, is a hypothetical charge that an atom would have if all bonds to atoms of different elements were 100% ionic. It is a concept used to track the theoretical transfer of electrons in chemical reactions, particularly in redox (reduction-oxidation) reactions. The oxidation state of an atom in a molecule or ion is determined by a set of rules. In its elemental form, an atom has an oxidation state of zero. For simple ions, the oxidation state is equal to the charge of the ion. Oxygen typically has an oxidation state of -2, except in peroxides where it is -1 and when bonded to fluorine. Hydrogen usually has an oxidation state of +1 when bonded to nonmetals and -1 when bonded to metals. The sum of the oxidation states of all atoms in a neutral molecule must equal zero, and in a polyatomic ion, it must equal the charge of the ion. Assigning oxidation states helps chemists understand electron movement and predict reaction products.