Chem 111 1st EditionLecture 8Outline of Last Lecture I. Study GuideOutline of Current Lecture I. Redox ReactionsCurrent LectureRedox Reaction: short for Reduction Oxidation reactionsReduction: gain of electronsOxidation: loss of electrons(Oxygen is common oxidizing agent, thus the name)Oxidation: −¿+¿+e¿Na−→ N a¿ (Na loses an electron)Reduction: −¿−→ Na+¿+e¿N a¿ (Na^+ gains an electron)Oxidation and Reduction always occur together!Zn(s)+2 Cu(N O3)2(aq)−→ zn(N O3)2(aq)+Cu(S)NIE : Zn(s)+C u+2(aq)−→ Z n+2(aq)+Cu(s)Z n0(s)+C u+2(aq)−→ Z n+2(aq)+C u0(s)Zn is oxidized, Zn reduces the Cu^2+, Cu^2+ is an oxidizing agent, Cu^2+ is ReducedMore redox reaction examplesCa+2 H2O−−→Ca(OH)2+H2Half Reaction: −¿Ca−→ C a+2+2 e¿Half Reaction: −¿+H2−¿−→ 2O H¿2 H2O+2 e¿How to recognize a redox reaction?Look for oxidation numbersEvery element in every substance in a reaction has an oxidation numberReview the rules on Table 4.4.1Some Important RulesRule #1: Each atom in a pure element has an oxidation number of zeroRule #2: A monoatomic ion has an oxidation number equal to the ion chargeThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Rule #6: The sum of the oxidation numbers for all atoms in an ion is equal to the overall charge on the ion. For a neutral compound, the sum of all of the oxidation numbers is equal to
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