Rules for assigning oxidation states
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Unit 9 - Redox Reactions
Last updated 7:05 PM on 8/28/23
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12 Terms
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atom in a free/elemental state
it’s oxidation state is 0
i.e. O2, Na, Cl2, HONCl BrIF
i.e. O2, Na, Cl2, HONCl BrIF
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group 1 metals
ALWAYS have a +1 oxidation state in their ions and compounds
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group 2 elements
ALWAYS have a +2 oxidation state in their ions and compounds
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aluminium (group 3)
has an oxidation state of +3 in the majority of its compounds
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when hydrogen is bonded to a non-metal
oxidation state of hydrogen is +1
i.e. HCl, HNO3
i.e. HCl, HNO3
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when hydrogen is bonded to a metal
oxidation state is -1
i.e. NaH, other metal hydrides
i.e. NaH, other metal hydrides
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oxygen
typically 2, (i.e. H2O and H2SO4)
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oxygen exception
in peroxides, oxygen oxidation state is -1
i.e. H2O2, hydrogen peroxide
i.e. H2O2, hydrogen peroxide
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fluorine
oxidation state is always 1 in all its compounds
i.e. LiF
i.e. LiF
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group 17 halogens
oxidation state is usually -1 in binary compounds (HI, NaCl, KBr) but in combination with oxygen, the oxidation state is positive
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neutral molecules
the sum of the oxidation states of ALL the atoms is zero
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polyatomic ions
the sum of the oxidation states of all the atoms equals the overall charge of the ion
Note 
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