chapter 19
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| Electrochemistry | the area of chemistry that deals with the interconversion of electrical energy and chemical energy
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| Elecrochemistry involves: | 1. using electricity to maker chemical reactions and 2. using chemical reactions to produce electricity
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| electrochemical processes are? | oxidation- reduction reactions in which energy released by a spontaneous reactions is converted to electricity and electrical energy is used to cause a non spontaneous reaction to occur
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| oxidation | is a half reaction in which you lose e-
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| reduction | is a half reaction in which you gain e-
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| oxidation numbers | the charge an atom would have in a molecule (or in an ionic compound) if electrons were completely transferred
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| Free elements in an uncombined state have an oxidation number of? | zero
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| in mono-atomic ions the oxidation number is? | equal to the charge on the ion
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| The oxidation number of oxygen is usually? | -2. In H2O2 and O2(2-) it -1.
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| the oxidation number of hydrogen is | +1, except when it is bonded to metals in binary compounds, it is -1.
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| The oxidation number of group 1A metals is: | +1
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| The oxidation number of group IIA metals is: | +2
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| Fluorine's oxidation number is always: | -1
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| The sum of the oxidation numbers of all the atoms in a molecule is equal to? | the charge on the molecule or atom.
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| Anode | the electrode at which oxidation occurs, it positive
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| Cathode | the electrode at which reduction occurs, it negative
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| Half-cell reactions | redox reactions
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| voltometer | measures the difference in electrical potential between the anode and cathode
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| Galvanic Cells | an apparatus for generating electricity through the use of a spontaneous reaction
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| What does the subscript "o" denote? | Standard state condition
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| Cell voltage | the difference in electrical potential between the anode and the cathode
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| Double lines denote? | a salt bridge
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| Standard reduction potential (E0)- | is the voltage associated with a reduction reaction at an electrode when all solutes are 1M and all gases are at 1 atm
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| Standard emf (E0Cell) | E0cell= E0cathode- E0anode
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| The more positive E0 | the greater the tendency for the substance to be reduced
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| are half cell reactions reversible? | yes
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| the sign of E0 changes when? | the reaction is reversed
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| Changing the stoichiometric coefficients of a half-cell reaction does what? | It does not change the value of E0
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| Energy (joules)= | change(coulomb) x voltage(volts)
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| Faraday constant (F)= | the charge of one mole of electrons
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| ΔG is negative K>1 E0cell= | positive, favors the formation of products
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| ΔG is positive K<1 E0cell= | negative, favors the formation of reactants
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| Concentration cell- | a galvanic cell from two half-cells composed of the same material but differing in ion concentrations
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| Membrane potential- | is the electrical potential that exists across the membrane of various kinds of cells including muscle and nerve cells
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| Nerst equations | E=-(0.0257V/n) lnQ
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| Battery- | a galvanic cell, or series of combined galvanic cells, that can be used as a source of direct electrical current at a constant voltage. Are self contained and require no salt bridge.
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| Leclanche' cell | the most common battery, with no fluid component
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| Mercury Battery | used in medicine, provides consistent voltage
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| Lead storage battery | used in automobiles, consists of 6 identical cells joined in a series, and is rechargeable
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| Solid state Lithium battery | Rechargeable, long-lasting, very light. It is used in cell phones, cameras, and laptops.
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| Fuel Cell- | is an electrochemical cell that requires a continuous supply of reactants to keep functioning.
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| Corrosion- | the deterioration of metals bu an electrochemical process
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| Passivation- | process by which the surface of iron metal is made inactive by treating it with a strong oxidizing agent to for a thin oxide layer
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| Cathodic protection- | process in which a metal that is to be protected from erosion is made the cathode in that amounts to a galvanic cell
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| electrolytic cell- | an apparatus for carrying out electrolysis
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| Electrolysis- | the process on which electrical energy is used top cause a non-spontaneous chemical reaction to occur
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| overvoltage- | the difference between the electrode potential and the actual voltage required to cause electrolysis
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