Reduced oxidation oxidation number the charge the

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Unformatted text preview: tance; It is reduced itself reduced Oxidation Oxidation Number The charge the atom would have in a molecule (or an ionic compound) if electrons were completely transferred 1. Free elements (uncombined state) have an oxidation number of zero. Oxidation Na, Be, K, Pb, H2, O2, P4 number : zero zero 2. In monoatomic ions, the oxidation number is equal to the monoatomic the Fe = +3 +3 charge on the ion. Li +1 Li = +1 Li+ ; Fe3+; O2-, Fe O = -2 3. The oxidation number of oxygen in compounds is usually –2. 3. oxygen In H2O2 and O22- it is –1. and 4. The oxidation number of hydrogen is +1 except when it is 4. hydrogen +1 bonded to metals in binary compounds, its oxidation number is –1 in this case. in esp : NaH +1 II +2 fluorine 5. Group IA metals are +1, IIA metals are +2 and fluorine is always –1. 6. The sum of the oxidation numbers of all the atoms in a sum all molecule or ion is equal to the charge on the molecule or ion charge on Oxidation numbers of all the atoms in HCO3- ? +1 +4 −2 − H CO 3 +1 ? H ClO 2 2− ? Cr O 2 7 +3 −2 H ClO 2 −2 2 − +6 Cr O 2 7 Single Replacement Reactions All single replacement reactions are redox reactions The single element is considered “more active” or higher in the “activity series” than the one in the compound. Reducing Reducing agent Hydrogen Hydrogen is more more active than copper copper Oxidation half reactions 0 +2 H 2 + CuO oxidizing agent 0 +1 → Cu + H 2O Reduction half reactions The more active an element is, the easier for it to lose electrons more easier Activity Series of Metals in aqueous solution Balancing Redox Equations Esp: The oxidation of Fe2+ to F...
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This document was uploaded on 02/26/2014.

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