understand the terms ‘oxidation’ and ‘reduction’ in terms of electron transfer, applied to s-, p- and d-block elements

Introduction to redox equilibria

understand the terms ‘oxidation’ and ‘reduction’ in terms of changes in oxidation number, applied to s-, p- and d-block elements

Introduction to redox equilibria

know what is meant by the term ‘standard electrode potential’, E^θ

Standard electrode potentials

know that the standard electrode potential, E^θ, refers to conditions of:

i) 298 K temperature
ii) 100 kPa pressure of gases
iii) 1.00 mol dm^-3 concentration of ions

Standard electrode potentials

know the features of the standard hydrogen electrode and understand why a reference electrode is necessary

Standard hydrogen electrode

understand that different methods are used to measure standard electrode potentials of:

i) metals or non-metals in contact with their ions in aqueous solution
ii) ions of the same element with different oxidation numbers

Standard electrode potentials

CORE PRACTICAL 10: Investigating some electrochemical cells

Combining half-cells

be able to calculate a standard emf, E^θ_cell, by combining two standard electrode potentials

Combining half-cells

be able to write cell diagrams using the conventional representation of half-cells

Standard electrode potentials

understand the importance of the conditions when measuring the electrode potential, E

Standard electrode potentials

be able to predict the thermodynamic feasibility of a reaction using standard electrode potentials

Combining half-cells

understand that E^θ_cell is directly proportional to the total entropy change and to ln K for a reaction

Combining half-cells

understand the limitations of predictions made using standard electrode potentials, in terms of kinetic inhibition and departure from standard conditions

Combining half-cells

know that standard electrode potentials can be listed as an electrochemical series

Standard electrode potentials

understand how disproportionation reactions relate to standard electrode potentials

Combining half-cells

understand the application of electrode potentials to storage cells

Storage cells

understand that the energy released on the reaction of a fuel with oxygen is utilised in a fuel cell to generate a voltage

Knowledge that methanol and other hydrogen-rich fuels are used in fuel cells is expected.

Fuel cells

know the electrode reactions that occur in a hydrogen-oxygen fuel cell

Knowledge of hydrogen-oxygen fuel cells with both acidic and alkaline electrolytes is expected.

Fuel cells

be able to carry out both structured and non-structured titration calculations including Fe²⁺/MnO₄⁻, and I₂/S₂O₃²⁻

Redox titrations

understand the methods used in redox titrations

Redox titrations

CORE PRACTICAL 11: Redox titration

Redox titrations