Redox Reactions Flashcards
Redox Reaction
Pair of simultaneous oxidation and reduction reactions in which electrons are exchanged between reactants
Oxidation
Loss - a chemical species loses one or more electrons
Reduction
Gain - a chemical species gains one or more electrons
Oxidising Agent
Is reduced, enables other species to be oxidised
Reducing Agent
Is oxidised, enables other species to be reduced
Pure Elements
Oxidation state of 0
Group 1 (Alkali) Metals
Oxidation state of +1 in a compound
Group 2 (Alkaline earth) Metals
Oxidation state of +2 in a compound
Hydrogen
Oxidation state of +1 except for in a metal hydrite, oxididation state of -1
Oxygen
Oxidation state of -2 except for peroxide, oxidation state of -1
Electrochemical Cells
Utilise redox reactions to produce an electric current, purify metal alloys or coat one metal layer onto another
Voltaic (Galvanic) Cell
Utilises spontaneous redox reactions to create an electric current, half reactions are seperated, connecting leads attached to electrodes and salt bridge creates closed circuit
Anode
Negative charge, source of electrons, oxidation occurs
Salt Bridge
Anions travel towards anode, cations travel towards cathode
Cathode
Positive, gains electrons, reduction occurs