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3.1.7 Oxidation and Reduction (Oxidation states (used to see what has been…
3.1.7 Oxidation and Reduction
Oxidation
process of losing electrons
gain of oxygen
loss of hydrogen
oxidising agent is an electron acceptor
Reduction
process of gaining electrons
loss of oxygen
gain of hydrogen
reducing agent is an electron donor
Oxidation states
used to see what has been oxidised and what has been reduced in a redox reaction; also called oxidation numbers
every element in its uncombined state has an oxidation state of zero
H: always +1 (except metal hydride when it is -10)
Group 1: always +1
Group 2: always +2
Al: always +3
O: -2 (except peroxides when it is -1 and in OF₂ when it is +2)
F: always -1
Cl: -1 (except in compounds with F and O where it is positive)
sum of oxidation states in a compound is 0
sum of oxidation states of a complex ion equals the charge on the ion
in c compound, the most electronegative element always has a negative oxidation state
Half equations
combine half equations
add water to balance oxygens
add H⁺ ions to balance hydrogens
add electrons to balance charge
Sammer Sheikh