protons and electrons

very small charge (+-1.602 x 10^-19 C)

force per unit charge N/C opposite charges attract, like charges attract

ability of an electric field to do work on a charge (V=J/C) **important; need to know this and the unit**

when electrons are lost when oxidation number increases LEO

when electrons are gained losing/reducing oxidation number

electrochemical cells and types

system of electrodes (often metals) and electrolytes in which a chemical rxn generates or uses an electric current voltaic (galvanic) cell electrolytic cell

voltaic (galvanic) cell

an electrochemical cell that uses a SPONTANEOUS reaction to generate electric current

an electrochemical cell in which an external energy source drives a non spontaneous rxn “takes a nonspontaneous rxn and uses an external power source to drive the rxn”

when you split up a redox rxn and have 1 half rxn in one beaker and other rxn in other beaker portions of the voltaic cell where the separated half rxns take place

allows ions to flow and balance charge

how do ions flow in the salt bridge

anions flow toward the anode cations flow toward the cathode

to maintain charge balance not of electrons but rather ions i guess idk... electrons go via wire, not this i guess if we didnt do this, rxn would stop itself so theres no "charge buildup"

ability of the anode to lose e- Eox

ability of the cathode to gain e- Ered

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electrochemistry

Question	Answer
electrochemistry	study of oxidation-reduction reactions that involve the transfer of electrons
electric charge	property of matter (C) (COULOMB)
protons and electrons	very small charge (+-1.602 x 10^-19 C)
electric field	force per unit charge N/C opposite charges attract, like charges attract
electric potential	ability of an electric field to do work on a charge (V=J/C) important; need to know this and the unit
electric current	rate charge flow (A=C/s)
oxidation	when electrons are lost when oxidation number increases LEO
reduction	when electrons are gained losing/reducing oxidation number
electrochemical cells and types	system of electrodes (often metals) and electrolytes in which a chemical rxn generates or uses an electric current voltaic (galvanic) cell electrolytic cell
voltaic (galvanic) cell	an electrochemical cell that uses a SPONTANEOUS reaction to generate electric current
electrolytic cell	an electrochemical cell in which an external energy source drives a non spontaneous rxn “takes a nonspontaneous rxn and uses an external power source to drive the rxn”
redox rxn	transfer of electrons
half cells	when you split up a redox rxn and have 1 half rxn in one beaker and other rxn in other beaker portions of the voltaic cell where the separated half rxns take place
oxidation occurs at the	anode
reduction occurs at the	cathode
reduction does what to electrons	consumes electrons (+)
oxidation does what to electrons	produces electrons (-)
salt bridge	allows ions to flow and balance charge
how do ions flow in the salt bridge	anions flow toward the anode cations flow toward the cathode
salt bridge purpose	to maintain charge balance not of electrons but rather ions i guess idk... electrons go via wire, not this i guess if we didnt do this, rxn would stop itself so theres no "charge buildup"
oxidation potential	ability of the anode to lose e- Eox
reduction potential	ability of the cathode to gain e- Ered

Created by: user-1759191

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