redox reactions

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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
    • 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
        • disproportionation reaction
          • the same species is both oxidised and reduced
      • decrease the oxidation state
    • 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

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