Chapter 17: Electrochemistry Flashcards
(21 cards)
oxidation numbers
assessment of how the electronic environment of its atoms is different in comparison to the pure element
redox reaction
reduction-oxidation reaction
involves transfer of electrons
oxidized species
loss of electrons
increase in oxidation number
reduced species
gain of electrons
decrease in oxidation number
oxidizing agent
oxidizes other species by accepting electrons
reducing agent
reduces other species by donating electrons
Galvanic cell
electrochemical cell in which a spontaneous redox reaction takes place
chemical -> electrical energy
half cell
component of a cell that contains the redox conjugate pair of a reactant
anode
half cell in which oxidation takes place
cathode
half cell in which reduction takes place
salt bridge
completes the electrical circuit
balances out the charges in the half-cells
cell notation
symbolic representation of the chemical reactions and reactants in a cell
anode | solution || solution | cathode
inert electrode
electrode that conducts electrons to and from the reactants in a half-cell but not itself oxidized or reduced
active electrode
electrode that participates in the reaction of a half cell
potential
- measured of the energy that accompanies charge transfer
- driving force for charge transfer in redox reactions
- difference in potential between the two half cells is measured
V = J/C
cell potential
difference in the potentials of the cathode half-cell and the anode half-cell
standard electrode potential
potential measured for a cell when X is the cathode and SHE is the anode
standard reduction potential
electrode potential measured at standard state conditions
Faraday’s constant
charge on one mol of e-
Nernst equation
relates the potential of a redox system to its composition
concentration cell
galvanic cell consisting of half-cells with identical composition but differing concentrations
