Explain how the Group 17 elements act as oxidising agents.
Write an equation to show the reaction in which $\text{Cl}_2$ oxidises aluminium metal.
A student heats equal amounts of $\text{I}_2(g)$ and $\text{H}_2(g)$ in a sealed flask, then allows the contents to cool. State what you observe during the reaction.
Both $\text{Cl}_2$ and $\text{Br}_2$ react with $\text{NH}_3$ to form $\text{N}_2$ and a hydrogen halide, HX. $3\text{X}_2 + 2\text{NH}_3 \rightarrow \text{N}_2 + 6\text{HX}$, where $\text{X} = \text{Cl}$ or $\text{Br}$. The relative bond strengths of X-X and H-X are what make the enthalpy changes of the two reactions different. Describe and explain the difference in the X-X bond strengths of $\text{Cl}_2$ and $\text{Br}_2$.
Describe the relative thermal stabilities of HCl and HBr.
Define enthalpy change of formation, $\Delta H_f$.
Table 1.1 supplies data relevant to the reaction of $\text{Cl}_2(g)$ with $\text{NH}_3(g)$. Use the data in Table 1.1 to calculate the enthalpy change of the reaction of $\text{Cl}_2(g)$ with $\text{NH}_3(g)$. Give your answer in $\text{kJ mol}^{-1}$.
When $\text{I}_2$ reacts with $\text{NH}_3$, $\text{NI}_3$ is formed. Predict the shape of a molecule of $\text{NI}_3$. Explain your answer.
Complete Table 1.2.
Suggest an identity for the species that produces each observation in the reaction of NaI with concentrated $\text{H}_2\text{SO}_4$. black solid; yellow solid; effervescence.
Table 1.3 provides some information about $\text{MgCl}_2$ and $\text{SiCl}_4$. Explain the difference between the electrical conductivity of liquid $\text{MgCl}_2$ and of liquid $\text{SiCl}_4$. Refer to bonding and relevant particles in your answer.
Suggest the pH of the solutions that form when each chloride is added to water. $\text{MgCl}_2$ ________ $\text{SiCl}_4$ ________