redox reactions
- Created by: Margaret Hobart
- Created on: 05-05-21 16:56
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- REDOX reactions
- oxidation
- oxidising agent
- a substance that oxidises another substance and is itself reduced
- e- acceptors
- the species being reduced is the oxidising agent
- loss of e-
- increase oxidation state
- oxidising agent
- reduction
- reducing agent
- a substance that reduces another substance and is itself reduced
- loses e-
- the species being oxidised is the reducing agent
- gain of e-
- REDOX
- e- transferred from reducing gent to oxidising agent
- oxidation
- oxidising agent
- a substance that oxidises another substance and is itself reduced
- e- acceptors
- the species being reduced is the oxidising agent
- loss of e-
- increase oxidation state
- oxidising agent
- disproportionation reaction
- the same species is both oxidised and reduced
- decrease the oxidation state
- reducing agent
- REDOX
- e- transferred from reducing gent to oxidising agent
- disproportionation reaction
- the same species is both oxidised and reduced
- half equations
- shows only reduction or oxidation process
- oxidation states
- common oxidation states
- group 1 metals always +1
- group 2 metals always +2
- oxygen usually -2
- except in peroxides and F2O
- hydrogen usually +1
- in metal hydroxides it's -1
- fluorine always -1
- chlorine usually -1
- except in compounds with O or F
- roman numerals indicate oxidation state e.g. Fe (III)
- tells you the number of e- accepted or donated
- charge on an ion tell you the oxidisation state
- common oxidation states
- oxidation
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