#5.2.3a
explanation and use of the terms oxidising agent and reducing agent (see also 2.1.5 Redox)
#5.2.3b
construction of redox equations using half-equations and oxidation numbers
#5.2.3c
interpretation and prediction of reactions involving electron transfer
#5.2.3d
the techniques and procedures used when carrying out redox titrations including those involving Fe2+/MnO4– and I2/S2O32− (see also 2.1.5e–f)
#5.2.3e
structured and non-structured titration calculations, based on experimental results of redox titrations involving:
(i) Fe2+/MnO4– and I2/S2O32−
(ii) non-familiar redox systems
Non-structured titration calculations could be examined in the context of both acid–base and redox titrations (see also 2.1.4d–e).
#5.2.3f
use of the term standard electrode (redox) potential, Eθ, including its measurement using a hydrogen electrode
Eθ data will be provided on examination papers.
#5.2.3g
the techniques and procedures used for the measurement of cell potentials of:
(i) metals or non-metals in contact with their ions in aqueous solution
(ii) ions of the same element in different oxidation states in contact with a Pt electrode
For measurement of standard cell potentials, ions of the same element can have concentrations of 1 mol dm–3 or be equimolar.
PAG8
#5.2.3h
calculation of a standard cell potential by combining two standard electrode potentials
#5.2.3i
prediction of the feasibility of a reaction using standard cell potentials and the limitations of such predictions in terms of kinetics and concentration
#5.2.3j
application of principles of electrode potentials to modern storage cells
Details of storage cells and required equations will be provided. Relevant electrode potentials and other data will be supplied.
#5.2.3k
explanation that a fuel cell uses the energy from the reaction of a fuel with oxygen to create a voltage and the changes that take place at each electrode.
Recall of fuel cells and equations will not be required. Relevant electrode potentials and other data will be supplied.