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Redox
the balance transfer of one of more electrons between chemical species
Reduction
the gain of one or more electrons from a chemical species
Oxidation
the loss of one or more electrons from a chemical species
Oxidising agent (oxidant)
causes another species to be oxidised
Causing another species to lose one or more electrons
It itself is undergoing reduction
Reducing agent (reductant)
causes another species to be reduced
Causing another species to gain one or more electrons
It itself is undergoing oxidation
Conjugate redox pairs
One pair is made up of the oxidising agent (reactant) and the species from when the oxidising agent is produced (product)
A and A+ is one pair
The other pair is the reducing agent (reactant) and the species from when the reducing agent is oxidised (product)
B+ and B is another pair
Oxidation rules
The oxidation state of a free element (an element by itself or bounded to itself) is always 0
Oxidation state of simple ion is equal to the charge of the ion
The sum of oxidation state in a neutral compound is 0
The sum of oxidation states in a polyatomic ion is equal to the charge of the ion
The normal oxidation state for hydrogen in a compound is +1 (except in metal hydrides, where it is -1)
The normal oxidation state for oxygen in a compound is -2 (except in peroxides, where it is -1)
