Silver, Ag, is a metal in the d-block of the Periodic Table.

1. (a)Silver can form compounds containing either Ag+ or Ag2+ ions. Explain why silver is a transition element.[1]
2. (b)(i)Table 1.1 gives data relevant to the Born–Haber cycle for silver(I) fluoride, AgF. Table 1.1 standard energy change value/kJ mol-1 first ionisation energy of silver +732 enthalpy change of atomisation of silver +289 enthalpy change of atomisation of fluorine +79 enthalpy change of formation of silver(I) fluoride -203 lattice energy of silver(I) fluoride -955 Write equations for the standard enthalpy changes described. Include state symbols. • standard enthalpy change of atomisation of silver • standard enthalpy change of formation of silver(I) fluoride[2]
3. (b)(ii)Define lattice energy.[2]
4. (b)(iii)Calculate the first electron affinity, EA₁, of fluorine, using data from Table 1.1. It may be helpful to draw a labelled energy cycle as part of the working for your answer. EA₁ = .............................................. kJ mol-1[2]
5. (c)(i)Use the data in Table 1.2 to calculate the enthalpy change of solution, ΔHsol, of AgF(s). Table 1.2 energy change at 298 K value/kJ mol-1 lattice energy of AgF(s) -955 enthalpy change of hydration of Ag+(g) -464 enthalpy change of hydration of F¯(g) -506 ΔHsol of AgF(s) = ...................................... kJ mol-1[1]
6. (c)(ii)Use your answer to (c)(i) to suggest whether AgF is soluble in water at 298K. Explain your answer.[1]
7. (d)(i)Table 1.3 shows some data relevant to the silver(I) halides, AgCl to AgI. Table 1.3 silver(I) halide first electron affinity of halogen/kJ mol-1 lattice energy /kJ mol-1 AgCl -349 -905 AgBr -325 -890 AgI -295 -876 Explain the trend in the first electron affinities of the halogens, Cl to I.[2]
8. (d)(ii)Explain the trend in the lattice energies of the silver(I) halides, AgCl to AgI.[1]
9. (e)(i)An electrochemical cell is constructed using the electrodes shown in Table 1.4. Table 1.4 electrode half-equation E°/V 1 AgCl(s) + e¯ ⇌ Ag(s) + Cl-(aq) +0.222 2 Cu2+(aq) + 2e¯ ⇌ Cu(s) +0.342 Calculate the standard cell potential, E°cell. Construct an equation for the overall cell reaction. E°cell = ...................................... V equation .......................................................................................................................................................................[2]
10. (e)(ii)In a different experiment, electrode 1 is set up using a saturated solution of KCl. Saturated KCl(aq) contains 36.0g of KCl per 100 cm³ of solution at 298K. The Nernst equation for electrode 1 is: E = E° + (0.059/Z) log (1/[Cl-(aq)]) Calculate the electrode potential, E, of electrode 1 under these conditions. E = ...................................... V[3]

This question uses a diagram from the original paper, which isn't shown here. Open the full paper from the past papers archive to see it.