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14 Cards in this Set
- Front
- Back
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Define 'Oxidation' |
The loss of electrons, resulting in an increase of oxidation state |
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Define 'Reduction' |
The gain of electrons, resulting in a decrease of oxidation state |
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What is a 'Reducing agent'? |
A species that reduces another species by donating one or more electrons, thus being itself oxidised. |
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What is an 'Oxidising agent'? |
A species that oxidises another species by removing one or more electrons, thus being itself reduced. |
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Define 'species' |
An atom, molecule or ion |
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An example of a redox equation is where Mg burns in oxygen: 2Mg + O2 ----> 2MgO Write reductive and oxidative half equations for this reaction |
Oxidative: Mg -----> Mg2+ +2e- Reductive: O2 + 4e- ----> 2O2- |
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What are the typical oxidation numbers of Oxygen and Hydrogen? |
Oxygen -2 Hydrogen +1 Exceptions: Oxygen is -1 in peroxides Hydrogen is -1 when combined with a less electronegative element e.g in KH |
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What is the oxidation number of H2 |
0 as it is in its elemental form |
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The sum of all the oxidation numbers in a neutral compound is...? |
0 |
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What is the oxidation number of nitrogen in the following: NH3 (NO2)- (NO3)- |
-3 in NH3 +3 in (NO2)- +5 in (NO3)- |
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Deduce the formula for Iron (III) Sulphate |
Fe is 3+, SO4 is 2- To give a neutral compound they must be in a 2:3 ratio Fe2(SO4)3 |
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Most chlorine based bleaches contain the ClO- ion. State the oxidation state of Cl in this compound and give its systematic name |
Cl is +1 Chlorate (1) |
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Fe (s) -----> Fe2+ (aq) + 2e- O2 (aq) + 2H2O (l) + 4e- -----> 4OH- (aq) |
2Fe (s) + O2 (aq) + 2H2O (l) -----> 4OH- (aq) + 2Fe2+ (aq) |
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What is the change in oxidation number of Chlorine is this reaction? KClO3 (S) ------> KCl (s) + 1.5O2 (g) |
From +5 to -1 |
