Loading…
0 of 10 objectives have lessons · 0 studied · 0 secure
Lessons for this topic haven’t been written yet. The objectives below show exactly what the syllabus expects, so you can plan with them in the meantime.
What Cambridge says you should be able to do, in our words. Codes are the topic number plus the objective’s position.
Define the terms: (a) standard electrode (reduction) potential; (b) standard cell potential.
No lesson yet
Describe the standard hydrogen electrode.
No lesson yet
Describe methods used to measure the standard electrode potentials of: (a) metals or non-metals in contact with their ions in aqueous solution; (b) ions of the same element in different oxidation states.
No lesson yet
Calculate a standard cell potential by combining two standard electrode potentials.
No lesson yet
Use standard cell potentials to: (a) deduce the polarity of each electrode and hence explain/deduce the direction of electron flow in the external circuit of a simple cell; (b) predict the feasibility of a reaction.
No lesson yet
Deduce from E⦵ values the relative reactivity of elements, compounds and ions as oxidising agents or as reducing agents.
No lesson yet
Construct redox equations using the relevant half-equations.
No lesson yet
Predict qualitatively how the value of an electrode potential, E, varies with the concentrations of the aqueous ions.
No lesson yet
Use the Nernst equation, e.g. E = E⦵ + (0.059/z) log([oxidised species]/[reduced species]), to predict quantitatively how the value of an electrode potential varies with the concentrations of the aqueous ions.
Examples include Cu²⁺(aq) + 2e⁻ ⇌ Cu(s) and Fe³⁺(aq) + e⁻ ⇌ Fe²⁺(aq).
No lesson yet
Understand and use the equation ΔG⦵ = –nE⦵cell F.
No lesson yet