R3.2 Electron transfer reactionsIB Chemistry SL: Flashcards

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Define oxidation in terms of electrons and oxidation state.

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Define oxidation in terms of electrons and oxidation state.: Loss of electrons; increase in oxidation state.
Oxidation state of Mn in MnO₄⁻?: +7.
Oxidation state of S in SO₄²⁻?: +6.
What happens to an oxidising agent?: It is reduced (gains electrons).
Balance the half-equation MnO₄⁻ → Mn²⁺ in acid.: MnO₄⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 4H₂O.
Which halogen is the strongest oxidising agent?: Fluorine.
Equation for zinc with dilute sulfuric acid.: Zn + H₂SO₄ → ZnSO₄ + H₂.
At which electrode does oxidation always occur?: The anode.
Sign of the anode in a voltaic cell and in an electrolytic cell?: Negative in a voltaic cell; positive in an electrolytic cell.
Which way do electrons flow in the external circuit of a voltaic cell?: From anode to cathode.
How do you get the charging reactions of a secondary cell?: Reverse the discharge half-equations.
Products of electrolysis of molten sodium chloride?: Sodium at the cathode, chlorine at the anode.
Product of oxidising propan-2-ol?: Propanone (a ketone).
Reducing agent for a carboxylic acid to a primary alcohol?: LiAlH₄.
Product of excess hydrogen with ethyne over nickel?: Ethane.