Day 7: Electrochemistry
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Oxidation
Loss of electrons (LEO)
Reduction
Gain of electrion (GER)
States of oxidation: 1
Elements in their elemental form are in the zero oxidation state (i.e. O2/O3)
States of oxidation: 2
Group 1 metals are +1 and Group 2 metals are +2
States of oxidation: 3
Hydrogen is +1 except when bonded to metals (when it’s -1)
States of oxidation: 4
Transition elements must be determined by context (except Al = +3, Zn= +2, Cd=+2, Ag= +1)
States of oxidation: 5
The most electronegative elements get their typical oxidation state
States of oxidation: 6
The last element not assigned balances the charge of the compound/ion
Oxidizing agent gets ________________ and reducing agent gets ______________
Reduced/ Oxidized
Elements or compounds are
oxidized/reduced
Compounds only
act as reducing/oxidizing agents
The anode is always
the site of oxidation (an Ox)
The cathode is always
the site of reduction (red cat)
Electrons always flow from
anode to cathode
Anions flow to the _______ and cations to the _____ through a salt bridge
Anode/Cathode
In the galvanic/voltaic (spontaneous) cells (Ecell>0)
the cathode is (+) and the anode is (-)
In electrolytic (non-spontaneous) cells (Ecell
cathode is (-) and anode is (+)
For metal/metal salt solution cells the cathode ________ and the anode ______
Gains mass/ Loses Mass
Galvanic cells _____ electricity
produce
Electrolytic cells______ electricity
consume, electricity forces non-spontaneous reaction to occur
Salt bridge
Completes curcuit, flow keeps solution netural
Flow is always from the
Anode to cathode
Standard Cell potentials
E(o) cell = E(o) reduction + E(o) oxidation
Standard Hydrogen Electrode (SHE) has a potential of
0.00V