Explain why the elements Na to Al are good electrical conductors.
Explain why the elements P, S and Cl do not conduct electricity.
Fig. 2.1 shows how the melting point of the Period 3 elements Si to Cl changes across the period. The Period 3 elements Si to Cl are all non-metals. Explain why there is a large difference between the melting point of Si and the melting points of P, S and Cl.
Table 2.1 gives some information about several Period 3 chlorides. Row B gives the pH of the solution formed when the Period 3 chloride is added to water. Complete Table 2.1. You may use the following abbreviations: I = ionic, C = covalent, M = metallic, G = giant, S = simple.
Write an equation for the formation of $\mathrm{AlCl_3}$ from its elements.
Write an equation for the formation of $\mathrm{H_3PO_4}$ from $\mathrm{PCl_5}$.
Given the reversible reaction $\mathrm{S_2Cl_2(l) + Cl_2(g) \rightleftharpoons 2SCl_2(l)}$ and $\Delta H = -41\,\mathrm{kJ\,mol^{-1}}$, state what is meant by dynamic equilibrium.
Given the reversible reaction $\mathrm{S_2Cl_2(l) + Cl_2(g) \rightleftharpoons 2SCl_2(l)}$ and $\Delta H = -41\,\mathrm{kJ\,mol^{-1}}$, identify the condition needed to establish dynamic equilibrium.
$\mathrm{S_2Cl_2(l)}$ is yellow and $\mathrm{SCl_2(l)}$ is red. Given the equilibrium $\mathrm{S_2Cl_2(l) + Cl_2(g) \rightleftharpoons 2SCl_2(l)}$ and $\Delta H = -41\,\mathrm{kJ\,mol^{-1}}$, state what is observed and explain your answers when: (1) the equilibrium mixture is warmed gently; (2) the overall pressure of the equilibrium mixture is increased.
Aqueous $\mathrm{MgCl_2}$ reacts with aqueous $\mathrm{Na_2CO_3}$ to produce a white precipitate. When heated, the white precipitate breaks down by thermal decomposition. Construct an equation to show the reaction of aqueous $\mathrm{MgCl_2}$ with aqueous $\mathrm{Na_2CO_3}$. Use state symbols in your equation.
Identify the products of the thermal decomposition of the white precipitate.
State the trend in thermal stability of the Group 2 carbonates down the group.