Chlorine reacts with silicon to make silicon(IV) chloride. Describe the appearance of silicon(IV) chloride at room temperature and pressure. State its structure and bonding.
Samples of magnesium chloride and phosphorus(V) chloride are placed into separate beakers of cold water. Complete Table 3.1. Ignore temperature changes when you consider the observations for these reactions.
State the reagent and conditions needed for sodium chlorate(V) to form from $\text{Cl}_2\text{(g)}$.
Explain why the reaction in (c)(i) is called a disproportionation reaction. Your answer should mention the relevant species and their oxidation numbers.
State the conditions needed for chlorine to react with methane.
One of the products in the reaction is $\text{CH}_2\text{Cl}_2$, and this goes on to form $\text{CHCl}_3$. Complete Table 3.2 to show the mechanism details for the formation of $\text{CHCl}_3$ from $\text{CH}_2\text{Cl}_2$.
$\text{CHCl}_3$ and HF are used to make $\text{CHClF}_2$ in a substitution reaction. Write an equation for this reaction.
$X$ is a product of the substitution reaction that occurs when $\text{CHClF}_2$ reacts with $\text{Br}_2$. There is only one naturally occurring isotope of fluorine, $^{19}\text{F}$. The mass spectrum of $X$ shows molecular ion peaks at $m/e = 164$, $166$ and $168$. Complete Table 3.3 to show all the molecular ions responsible for each peak.