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Halo students,

Do you find assigning Oxidation Number (or Oxidation States) to elements and then geting the correct chemical formulae of compounds very challenging, and often lost marks on it. Fret Not! In fact, assigning Oxidation Number to the elements and obtaining the subsequent chemical formulae of the compounds is easy if you observe the following rules:

• The oxidation numbers of an atom or the atoms in a neutral molecule must add up to zero.
• If an atom or molecule is ionic its oxidation number must add up to its overall charge.
• Alkali metal atoms (Group I) have an oxidation number equal to +1 within compounds.
• Alkali earth atoms (Group II) have an oxidation number of +2 within compounds.
• Halogens have -1 oxidation number within compounds.
• Hydrogen is always assigned a +1 oxidation number in compounds, except in metal hydrides (e.g. LiH) whereby the Li has a + 1 oxidation number while H adopts a -1 oxidation number.
• Oxygen is assigned an oxidation number of -2 in compounds except when It is found in Hydrogen Peroxide whereby each 0 atom has a -1 oxidation state.
• The sum of oxidation states of all the atoms in a molecule is equal to zero.
• The sum of oxidation states of all the atoms in a radical is equal to the charge on the ion.

Examples To Note:

N₂O      +1 state for N, -2 state for O

LiH         +1 state for Li, -1 state for H

H₂O₂      +1 state for H, -1 state for O
O₂         0 state for O
SO₄^2-       +6 state for S, -2 state for O

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• O Level Chemistry - Definition of Redox
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• Chemistry Question - Redox Reactions
• O Level Chemistry - More Questions on Redox

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