Quiz 5 – Chemistry – Flashcards
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| oxidized |
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| lose electrons |
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| reduced |
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| gain electrons |
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| Oxidation number during oxidation |
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| increases |
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| oxidation number during reduction |
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| decrease |
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| half reaction electrons during oxidation |
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| electrons are products |
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| half reaction electrons during reduction |
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| electrons as reactants |
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| oxygen during oxidation |
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| oxygen added |
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| oxygen during reduction |
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| oxygen lost |
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| Rule 1: oxidation state of free elements |
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| 0 |
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| Rule 2: oxidation state of monatomic ions |
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| equal to their charge |
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| Rule 3: sum of atoms oxidation states in a compound |
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| equal zero |
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| Rule 4a: Group I metals have an oxidation state |
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| of +1 in their compounds |
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| Rule 4b: Group II metals have an oxidation state |
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| of +2 in their compounds |
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| Rule 5: nonmetals |
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| nonmetals have oxidation states according to the table, F=-1,H=+1, O=-2, group 7a=-1, group 6a=-2,group 5a=-3 |
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| reducing agent |
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| reactant that reduces an element in another reactant, contains the element that is oxidized |
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| oxidizing agent |
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| reactant that oxidizes an element in another reactant, contains the element that is reduced |
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| Anode electrode |
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| where oxidation occurs loses weight positive end of battery attracts anions |
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| Cathode electrode |
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| where reduction occurs attracts cations negative end of battery gains weight where plating takes place |
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| 1Amp (current) = 1 Coulomb of charge = |
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| 1 A = 6.242 x 10^18 electrons per second? |
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| 1 volt |
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| 1 J per Coulomb of charge |
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| electromotive forcel |
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| Amount of force pushing the electrons through the wire |
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| cell potential |
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| difference in potential energy between the anode and the cathode in a voltaic cell standard emf, Eocell |
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| inert electrode |
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| does not participate in reaction, but just provides a surface |
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| half-reaction with a strong tendency to occur |
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| large positive half-cell potential |
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| how electrons will flow when two half-cells are connected |
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| half-reaction with the stronger tendency will occurire |
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| standard hydrogen electrodels = |
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| = 0 v |
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| stronger tendency toward reduction than the SHE |
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| + value for Ered |
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| stronger tendency toward oxidation than the SHE |
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| - value for Ered |
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| For oxidation half-reaction |
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| Eoxi = - Ered |
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| Ecell = |
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| Eoxidation + Ereduction |
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| spontaneous reactionion |
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| Free energy change G < 1 (negative) E > 1 (positive) K > 1 |
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| G= -RTlnKB= |
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| =-nFEcell |
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| free energy change (G^o)= |
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| =G + RTlnQ |
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| E = |
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| E^o -(0.0592/n)logQ |
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| Concentration Cellsnion |
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| Electrons will flow from the electrode in the less concentrated solution to the electrode in the more concentrated solution |
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| ElectrolysisTlnQ |
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| using electrical energy to break a compound apartrire |
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| Corrosion |
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| spontaneous oxidation of a metal by chemicals in the environmentl |
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| Rust |
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| Fe2O3*nH2O;B |
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| Rust |
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| Fe2O3*nH2O;B |
