REVISION ELECTROCHEMISTRY OXIDATION Oxidation is a loss of
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REVISION ELECTROCHEMISTRY
OXIDATION • Oxidation is a loss of electrons • The oxidation number increases • E. g. • Electrodes where oxidation take place will reduce in mass • We write the oxidation reaction ‘upside-down’ from the table • Reducing agent ANODE The electrode where oxidation takes place
REDUCTION • Reduction is a gain of electrons • The oxidation number decreases • E. g. • Electrodes where reduction take place will increase in mass • We write the reduction reaction ‘right-way-round’ from the table • Oxidising agent CATHODE The electrode where reduction takes place
ELECTROLYTE solution/liquid/dissolved substance that conducts electricity through the movement of ions.
TABLE OF STANDARD REDUCTION POTENTIALS
STANDARD CONDITIONS •
CELL POTENTIALS •
GALVANIC CELL a cell in which chemical energy is converted into electrical energy. A galvanic (voltaic) cell has self-sustaining electrode reactions
SPONTATEOUS REACTIONS
SALT BRIDGE Its function is to maintain ELECTRICAL neutrality
CELL NOTATION • The H 2|H+ half-cell is treated just like any other half-cell. . • Cell terminals (electrodes) are written on the outside of the cell notation. • Active electrodes reducing agent | oxidised species || oxidising agent | reduced species • Inert electrodes (usually Pt or C): Pt | reducing agent | oxidised species || oxidising agent | reduced species | Pt Example: Pt | Cℓ-(aq) |Cℓ 2(g) || F 2(g) | F-(aq) | Pt
ELECTROLYTIC CELL a cell in which electrical energy is converted into chemical energy. ELECTROLYSIS The chemical process in which electrical energy is converted to chemical energy OR the use of electrical energy to produce a chemical change.
ELECTROLYTIC CELL
ELECTROPLATING
ELECTROPLATING
REFINING OF COPPER
REFINING OF COPPER
CHLOOR-ALKALI INDUSTRY
CHLOOR-ALKALI INDUSTRY
RECOVERY OF ALUMINIUM
RECOVERY OF ALUMINIUM
Oxidize Anode negative Reduce Cathode positive
Wants to oxidize ‘upside down’ Wants to reduce ‘rightside up’
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