25-26 RedoxLandscape

25-26 RedoxLandscape - ELECTROCHEMISTRY Electrochemistry...

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CH112 LRSVDS Electrochem part 1 1 Electrochemistry involves the relationship between electrical energy and chemical energy. OXIDATION-REDUCTION REACTIONS SPONTANEOUS REACTIONS _____________________ Examples: voltaic cells, batteries. NON-SPONTANEOUS REACTIONS _____________________ Examples: electrolysis, electrolytic cells. QUANTITATIVE ASPECTS OF ELECTROCHEMICAL REACTIONS ELECTROCHEMISTRY CH112 LRSVDS Electrochem part 1 2 Oxidation/Reduction
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CH112 LRSVDS Electrochem part 1 3 OXIDATION-REDUCTION Oxidation = ___________________. An oxidizing agent is a substance that causes oxidation (and is itself reduced). Reduction = __________________. A reducing agent is a substance that causes reduction (and is itself oxidized). LAnOx and GRedCat! LAnOx: L ose electrons / An ode / Ox idized GRedCat: G ain electrons / Red uced / Cat hode CH112 LRSVDS Electrochem part 1 4 Rules for determining Oxidation States 1. Oxidation state of atom in elemental form is zero. e.g. Cl 2 O 2 P 4 C(s) S 8 2. The oxidation number of a monatomic ion equals its charge. 3. Some elements have “common” oxidation numbers that can be used as reference in determining the oxidation numbers of other atoms in the compound. Alkali metals +1 Alkaline earth metals +2 Fluorine –1 O usually –2 (peroxides (-1) & superoxides possible) H usually +1 (Hydrides: metal-H compounds (–1)) Cl, Br, I almost always –1 4. Sum of oxidation numbers is equal to overall charge of molecule or ion: For a neutral compound the sum of oxidation numbers equals zero. For a polyatomic ion, the sum of the oxidation numbers is equal to the charge on the ion.
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25-26 RedoxLandscape - ELECTROCHEMISTRY Electrochemistry...

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