Redox Chemistry

Redox Chemistry - 2. Use the trends in the periodic table...

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Redox Chemistry Redox (reduction/oxidation) chemistry deals with chemical reactions in terms of electron transfer. The origin comes from the reactions metals undergo: SnO 2 + C Sn + CO 2 Sn + O 2 SnO 2 In simplest form, a redox reaction simply involves a transfer of electrons. Cu 2+ + Mg Mg 2+ + Cu The substance that loses electrons is said to be oxidized . The substance that gains electrons is said to be reduced . L ose G ain E lectrons says El ectrons O xidation R eduction An substance that oxidizes another is called an oxidizing agent . An substance that reduced another is called a reducing agent . Oxidation Numbers: An oxidation number is the actual or assumed charge on an atom in a molecule or on an ion.
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Determining Oxidation Number: 1. Assume the most electronegative element has a full share of electrons pairs involved in any bond (ionic or covalent).
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Unformatted text preview: 2. Use the trends in the periodic table to help determine oxidation number. 3. Deduce other oxidation numbers from other oxidation numbers of elements in the compound or ion. Common Oxidation Numbers: Atom or Ion Oxidation Number Examples all atoms in elemental form. Na (s); Cl 2 hydrogen in all compounds. +1 H in HCl except in hydrides-1 H in LiH oxygen in all compounds-2 O in CO2 except in peroxides-1 O in H2O2 all monatomic ions charge on ion Fe 2+ is +2; Br-is 1 Elements: S 6 Pb O 2 Ionic Compounds: NaCl PbCl 4 SnO 2 Fe 2 O 3 Ions: NO 3-Cr 2 O 7 2-MnO 4-Covalent Compounds: CH 4 H 2 O NH 3 Unusual Cases: MgH 2 K 2 O 2 Carbon: CO CO 2 CO 3 2-CNO-C 2 H 2 CN-...
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Redox Chemistry - 2. Use the trends in the periodic table...

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