Edexcel A Level Chemistry:復習筆記2.1.3 Redox & Disproportionation
Disproportionation
Disproportionation reactions
- A?disproportionation?reaction?is a reaction in which the same species is simultaneously oxidised and reduced
Example of a disproportion reaction in which the same species (chlorine in this case) has been both oxidised and reduced
Using Oxidation Numbers
Worked Example
Balancing disproportionation reactions
Balance the disproportionation reaction which takes place when chlorine is added to hot concentrated aqueous sodium hydroxide. The products are Cl-?and ClO3-?ions and water
Answer
Step 1:?Write the unbalanced equation and identify the atoms that change in oxidation number:
Step 2:?Deduce the oxidation number changes:
Step 3:?Balance the oxidation number changes:
Step 4:?Balance the charges
Step 5:?Balance the atoms
Worked Example
Oxidation and reduction
In each of the following equations, state which reactant has been oxidised and which has been reduced.
- Na++ Cl-?→? NaCl
- Mg + Fe2+? →? Mg2+?+ Fe
- CO + Ag2O? →? 2Ag + CO2
Answer 1:
-
- Oxidised: Cl-?as the oxidation state has increased by 1
- Reduced: Na+?as the oxidation state has decreased by 1
Answer 2:
-
- Oxidised: Mg as the oxidation state has increased by 2
- Reduced: Fe2+?as the oxidation state has decreased by 2
Answer 3:
-
- Oxidised: C as it has gained oxygen
- Reduced: Ag as it has lost oxygen
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