Electrochemistry

electrode where the oxidation half-reaction takes place

galvanic cell in which the electrical work is used as a source of electrical power

electrode where the reduction half-reaction takes place

method of protecting a metal by sacrificing another metal as an anode in a galvanic cell

path through which electrons flow

process by which metals oxidize and return from a reduced form to their natural oxidation state

galvanic cell in which the electrolytes exist as pastes

flow of electric charge

amount of work required to move one charged particle from one point to another

voltage between two points when a charged particle is moved between them

branch of science that studies chemical reactions that cause electrons to move, resulting in the transfer of electrical charge

electrical conductor through which current enters or leaves an electrochemical cell

process of using electric current to do work on a chemical cell against its electric potential

ionic solution that can be decomposed by electricity

electrochemical cell that requires electrical energy to drive a nonspontaneous redox reaction

charge of one mole of electrons (96,485 C/mol)

device that generates electrical power through the ionization of hydrogen or another molecule

electrochemical cell formed when metal strips connected by a wire are immersed in different solutions of a redox reaction and the solutions are connected by a salt bridge

shorthand method of describing the setup of a galvanic cell

process that coats a metal with zinc as a sacrificial anode

electrode that does not take part in a chemical reaction but serves only to transfer electrons

equation used to find the cell potential under conditions that are not standard, given as $E=E^\circ-\frac{RT}{nF}\ln Q$

half-reaction showing oxidation (electron loss) of a species

half-reaction showing reduction (electron gain) of a species

anode made of a metal coupled to a more valuable metal, which it protects as part of a galvanic cell that undergoes galvanic corrosion

inert connection between the two half-cells, composed of either a glass tube filled with an inert salt solution or a strip of filter paper soaked in an inert salt solution, that transfers ions between the half-cells

potential difference between the cathode and the anode under standard conditions

platinum electrode in 1 M H⁺(aq) solution with bubbled hydrogen gas at 1 atm of pressure

tendency of the species to be reduced under standard conditions