CHEM 121 Lecture Notes - Lecture 9: Oxidation State, Chemical Equation, Oxidizing Agent
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Neutralization reactions: most neutralization reactions produce water, not all, but most, net ionic equation for strong acids and bases, h+ (aq) + oh- (aq) --> h2o(l) Net ionic equations look different for weak acids: redox reactions, oxidation-reduction reactions, reaction by electron transfer, oxidation. Loss of electrons: reduction, gain of electrons, half reactions. Identifying redox: using oxidation numbers, reducing agent, only found on the reactant side. The reactant that participates in oxidation: the atom that increases its oxidation number and causes reduction in another atom, oxidizing agent, only found on the reactant side. The reactant that participates in reduction: the atom that decreases the oxidation number and causes oxidation in another atom, an easy way to spot a redox reaction is if there is an element in the equation, activity. The ability of a metal to give up electrons (aq) ---> zn2+ (aq) + cu(s: ex) zn(s) + cu2, half reactions, cu2+
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