(a) (i) Define standard electrode potential. (ii) State two factors that affect the value of standard electrode potential. (iii) Give two uses of the values...

(a)(i) The standard electrode potential, E°, is the potential of a half-cell measured relative to the standard hydrogen electrode under standard conditions: temperature 298 K, ion concentration 1.0 mol dm⁻³, and gas pressure 1 atm.

(ii) Two factors which affect electrode potential are:

1. concentration of ions in the electrolyte;
2. temperature.

(iii) Standard electrode potentials are used to:

1. predict the direction or feasibility of a redox reaction;
2. calculate the e.m.f. of an electrochemical cell.

(iv) A correctly labelled electrochemical cell is shown below.

Cell notation: \[\text{Zn(s)}\;|\;\text{Zn}^{2+}\text{(aq, 1 mol dm}^{-3}\text{)}\;||\;\text{Cu}^{2+}\text{(aq, 1 mol dm}^{-3}\text{)}\;|\;\text{Cu(s)}\] Zinc is the anode (negative electrode) where oxidation occurs, while copper is the cathode (positive electrode) where reduction occurs.

(v)

(b)(i)

1. Oxidation is the loss of electrons.
2. An oxidizing agent is a substance that accepts electrons and causes another substance to be oxidized.

(ii) In acidic solution, the balanced ionic equation is:

(c)

(d) Hydrogen bonding is the strong intermolecular attraction between a hydrogen atom covalently bonded to nitrogen, oxygen, or fluorine in one molecule and a lone pair of electrons on nitrogen, oxygen, or fluorine in a neighbouring molecule.