Redox (OCR A Level Chemistry)

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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

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 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-

AnswersElectrochemistry Table 2_Oxidation Numbers, downloadable AS & A Level Chemistry revision notes

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

Redox Reactions & Equations

  • Metals can react with acid to form a salt and hydrogen

Metal + acid → salt + hydrogen

  •  During this reaction, there are changes in oxidation number 
    • This means that the reaction can be classified as a redox reaction

Worked example

Explain why each of the following reactions is a redox reaction:

  1. Zinc + hydrochloric acid → zinc chloride + hydrogen
  2. Magnesium + sulfuric acid → magnesium sulfate + hydrogen

Answer 1

Step 1: Write the balanced symbol equation

    • Zn + 2HCl → ZnCl2 + H2 

Step 2: Deduce the changes in oxidation number

    • Zinc - starts at 0, changes to +2
    • Hydrogen - starts at +1, changes to 0
    • Chlorine - remains at -1 throughout

Step 3: Explain which species is reduced / oxidised

    • Zinc is oxidised as its oxidation number increases from 0 to +2
    • Hydrogen is reduced as its oxidation number decreases from +1 to 0

Answer 2

Step 1: Write the balanced symbol equation

    • Mg + H2SO4 → MgSO4 + H2 

Step 2: Deduce the changes in oxidation number

    • Magnesium - starts at 0, changes to +2
    • Hydrogen - starts at +1, changes to 0
    • Sulfate ion - remains at -2 throughout

Step 3: Explain which species is reduced / oxidised

    • Magnesium is oxidised as its oxidation number increases from 0 to +2
    • Hydrogen is reduced as its oxidation number decreases from +1 to 0

Examiner Tip

Remember that oxidation number increases in oxidation reactions and decreases in reductions reactions

If you are asked to explain why a reaction is a redox reaction, you should always talk about one of the following:

  • Gain / loss of oxygen
  • Gain / loss of hydrogen
  • Gain / loss of electrons
  • Changes in oxidation numbers

Simply saying that a reaction is a redox reaction because "reduction and oxidation happen at the same time" is describing, not explaining

Interpreting Redox

We can identify the oxidation and reducing agents in a reaction by using the oxidation state.

  • For example
Zn (s) + H2SO4 (aq) → ZnSO4 (aq) + H(g)
           
  • If we look at zinc, Zn, in the reaction above we can see that it increases from 0 to +2 in zinc sulfate, ZnSO4  
  • An increase in oxidation number indicates oxidation has occured
  • Therefore zinc is the reducing agent
  • If we look at sulfuric acid, H2SO4, the oxidation state of hydrogen has decreased from +1 to 0 in H2
  • A decrease in oxidation number indicates reduction has occurred 
  • Therefore sulfuric acid is the oxidising agent 

Worked example

Identify the oxidising agent and reducing agent in the following reaction:

2NH3 + NaClO → N2H4 + NaCl + H2O

Answer
Step 1:
Deduce the oxidation numbers of nitrogen and chlorine in the equation (hydrogen = +1, oxygen = -2, sodium = +1                                   
   N in NH3 is -3
   Cl in NaClO is +1
   N in N2H4 is -2
   Cl in NaCl is -1
                

Step 2

Identify which species has been oxidised and which has been reduced by looking at the oxidation numbers
   Nitrogen is increasing in oxidation number, therefore has been oxidised
   
Chlorine is decreasing in oxidation number, therefore has been reduced

Step 3

Identify the oxidising and reducing agent 
   NH3 is the reducing agent (it has been oxidised itself)
   NaClO is the oxidising agent (it has been reduced itself) 

Remember, the whole species is the reducing agent, not just the element (e.g. NH3 is the reducing agent, not N on its own) 

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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.