Silver can make compounds that contain either $\text{Ag}^+$ or $\text{Ag}^{2+}$ ions. Explain why silver is a transition element.
Table 1.1 contains the data needed for the Born-Haber cycle for silver(I) fluoride, $\text{AgF}$.
Write equations for the standard enthalpy changes given below. Include state symbols. • standard enthalpy change of atomisation of silver • standard enthalpy change of formation of silver(I) fluoride
Define lattice energy.
Calculate the first electron affinity, $EA_1$, of fluorine, using the data in Table 1.1. Drawing a labelled energy cycle may help you with your answer.
Use the information in Table 1.2 to calculate the enthalpy change of solution, $\Delta H_{sol}$, of $\text{AgF}$(s).
Use your answer to c(i) to suggest whether $\text{AgF}$ is soluble in water at $298\,\text{K}$. Explain your answer.
Explain the trend in the first electron affinities of the halogens, $\text{Cl}$ to $\text{I}$.
Explain the trend in the lattice energies of the silver(I) halides, $\text{AgCl}$ to $\text{AgI}$.
Calculate the standard cell potential, $E^\circ_{\text{cell}}$. Construct an equation for the overall cell reaction.
In another experiment, electrode 1 is prepared using a saturated KCl solution. Saturated KCl(aq) contains $36.0\,\text{g}$ of KCl per $100\,\text{cm}^3$ of solution at $298\,\text{K}$. The Nernst equation for electrode 1 is: $E = E^\circ + \frac{0.059}{z} \log \left( \frac{1}{[\text{Cl}^- (\text{aq})]} \right)$ Calculate the electrode potential, $E$, of electrode 1 under these conditions.