Oxidation Number (Edexcel AS Chemistry)

Revision Note

Test yourself
Philippa

Author

Philippa

Last updated

Defining Oxidation Number

  • There are three definitions of oxidation and reduction  used in different branches of chemistry
  • Oxidation and reduction can be used to describe any of the following processes

Definitions and Examples of Oxidation & Reduction

Electrochemistry OIL RIG Diagram, downloadable AS & A Level Chemistry revision notes

Use the acronym "Oil Rig" to help you remember the definitions of oxidation and reduction

Oxidation Number

  • The oxidation number 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

Worked example

What are the oxidation numbers of the elements in the following species?

a) C                b)  Fe3+                       c)  Fe2+

d) O2-             e)  He                          f)  Al3+

Answers:

a) 0     b) +3    c) +2   

d) -2    e) 0      f) +3

  • So, in simple ions, the oxidation numbers of the atom is the charge on the ion:
    • Na+, K+, H+ all have an oxidation number of +1
    • Mg2+, Ca2+, Pb2+ all have an oxidation number of +2
    • Cl, Br, I all have an oxidation number of -1
    • O2-, S2- all have an oxidation number of -2
  • Roman numerals are also used to indicate the oxidation state of ions
    • Iron(II) sulfate implies that the iron is in a +2 oxidation state, i.e. Fe2+ 
    • Iron(III) sulfate implies that the iron is in a +3 oxidation state, i.e. Fe3+ 
  • More complicated examples include other atoms / ions as part of the formula 
    • Potassium manganate(VII) implies that the manganese is in a +7 oxidation
    • Potassium manganate(VII) contains the potassium ion K+ and the manganate ion MnO4 
      • Since the oxygen in the manganate ion is in the -2 oxidation state, there is a total of -8 from the oxygen
      • The manganate ion has an overall -1 charge, which means that the manganese ion must be in the +7 oxidation state

Calculating Oxidation Numbers

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 number of a single atom
  • The oxidation number (ox.no.) refers to a single atom in a compound

Oxidation Number Rules Table

Electrochemistry Table 1_Oxidation Numbers, downloadable AS & A Level Chemistry revision notes

Molecules or Compounds

  • In molecules or compounds, the sum of the oxidation numbers on the atoms is zero

Oxidation Number in Molecules or Compounds

  • Because CO2 is a neutral molecule, the sum of the oxidation numbers 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

How do you determine the value of an element’s oxidation number?

  • From its position in the periodic table and / or
  • The other element(s) present in the formula
  • The oxidation numbers of all other atoms in their compounds can vary
  • By following the oxidation number rules, the oxidation number 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

You've read 0 of your 10 free revision notes

Unlock more, it's free!

Join the 100,000+ Students that ❤️ Save My Exams

the (exam) results speak for themselves:

Did this page help you?

Philippa

Author: Philippa

Expertise: Chemistry

Philippa has worked as a GCSE and A level chemistry teacher and tutor for over thirteen years. She studied chemistry and sport science at Loughborough University graduating in 2007 having also completed her PGCE in science. Throughout her time as a teacher she was incharge of a boarding house for five years and coached many teams in a variety of sports. When not producing resources with the chemistry team, Philippa enjoys being active outside with her young family and is a very keen gardener.