Chapter 20 - Electrochemistry
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what is reduction
gain of electrons
what is oxidation
loss of electrons
what happens to a reducing agent
it loses electron
what happens to an oxidising agent
it gains electrons
what is the anode
the negative elctrode
what is the cathode
the positive electrode
what is the convention for representing an electrochemical cell
the cathode on the right and anode on the left
what occurs at the anode in terms of electron transfer
oxidation
what occurs at the cathode in terms of electron transfer
reduction
what are the conditions for a standard elecctrode potential
298K, 100kPa, and 1moldm^-3
define a half cell
a metal dipped into a solution of its own ions
wwhat is a cell
two half cells connected together
how do electrons flow in a cell
from the anode to the cathode
which electrode is the stronger reducing agent
the anode
which electrode is the stronger oxidising agent
the cathode
what is the potential of a strong reducing agent
negative
what is the potential of a strong oxidising agent
positive
how is an electrodes potential measured
by connecting it to a hydrogen half cell and measuring the emf produced
what is purpose of the salt bridge
to allow ions from either solution to move between each half cell
what makes a suyitable salt for a salt bridge
the fact that it doesnt react with either solution in the half cells
how is a cell conventionally represented
the most oxidised species are the closest to the salt bridge, species of the same state are separated with a comma and species of different species are separated by a line the salt bridge is two lines
what must be used when the electrode material isnt a metal solid
platinum
what reaction occurs at the positive electrode of a lithium cell
Li+ + CoO2 + e- —> Li+[CoO2]-
what occurs at the negative electrode of a lithium cell
Li —> Li+ + e-