Oxidation Number
Oxidation Number Rules
- A few simple rules help guide you through the process of determining the oxidation number of any element
- Remember, you are determining the oxidation state of a single atom
Oxidation Numbers
- The oxidation state of an atom is the charge that would exist on an individual atom if the bonding were completely ionic
- It is like the electronic ‘status’ of an element
- Oxidation numbers are used to
- Tell if oxidation or reduction has taken place
- Work out what has been oxidised and/or reduced
- Construct half equations and balance redox equations
Oxidation Numbers of Simple Ions
Oxidation Rules Table
Molecules or Compounds
- In molecules or compounds, the sum of the oxidation number on the atoms is zero
Oxidation Number in Molecules or Compounds
- Because CO2 is a neutral molecule, the sum of the oxidation number must be zero
- For this, one element must have a positive oxidation number and the other must be negative
How do you determine which is the positive one?
- The more electronegative species will have the negative value
- Electronegativity increases across a period and decreases down a group
- O is further to the right than C in the periodic table so it has the negative value
- From its position in the periodic table and/or
- The other element(s) present in the formula
- The oxidation states of all other atoms in their compounds can vary
- By following the oxidation number rules, the oxidation state of any atom in a compound or ion can be deduced
- The position of an element in the periodic table can act as a guide to the oxidation number
Oxidation Numbers & the Periodic Table
- Test your understanding on the following examples:
Worked example
Deducing oxidation numbers
Give the oxidation number of the elements in bold in these compounds or ions:
a. P2O5
b. SO42-
c. H2S
d. Al2Cl6
e. NH3
f. ClO2-
Answers
Are oxidation numbers always whole numbers?
- The answer is yes and no
- When you try and work out the oxidation numbers of sulfur in the tetrathionate ion S4O62- you get an interesting result!
The oxidation number of sulfur in S4O62- is a fraction
- The fact that the oxidation number comes out to +2.5 does not mean it is possible to get half an oxidation number
- This is only a mathematical consequence of four sulfur atoms sharing +10 oxidation number
- Single atoms can only have an integer oxidation number, because you cannot have half an electron!
Roman numerals
- Roman numerals are used to show the oxidation states of transition metals which can have more than one oxidation state
- Iron can be both +2 and +3 so Roman numerals are used to distinguish between them
- Fe2+ in FeO is written as iron(II) oxide
- Fe3+ in Fe2O3 is written as iron(III) oxide