State and explain the pattern in volatility of the halogens, from chlorine to iodine.
Explain why HI is the least thermally stable among HCl, HBr and HI.
The table gives the electronegativity values for hydrogen, fluorine and iodine. Explain, in terms of intermolecular forces, why HI has a lower boiling point than HF.
Iodine reacts with hot concentrated aqueous sodium hydroxide in the same way as chlorine. Write an equation for the reaction of iodine and hot aqueous sodium hydroxide.
$\text{CH}_3\text{I}$ can be prepared from methanol, $\text{CH}_3\text{OH}$. Identify a reagent that can convert $\text{CH}_3\text{OH}$ to $\text{CH}_3\text{I}$.
$1,2$-diiodoethane, $\text{CH}_2\text{ICH}_2\text{I}$, can be prepared by bubbling ethene into liquid iodine. Fully name the type of mechanism shown in this reaction.
Name J.
J reacts with NaOH(aq) to form K. Fully name the mechanism for the reaction of J with NaOH(aq) to form K.
$J$ reacts with $\text{NaOH}$ dissolved in ethanol to form a mixture of two alkenes, $L$ and $M$. Alkene $L$ is shown. In the box provided, draw the structure of $M$.
Explain why $L$ does not show geometrical (cis-trans) isomerism.
$L$ reacts with hot concentrated acidified $\text{KMnO}_4\text{(aq)}$ to form propanone and one other organic product. Identify the other organic product.
Propanone reacts with excess alkaline aqueous iodine. Complete and balance the equation for this reaction: $\text{CH}_3\text{COCH}_3 + \ldots \text{I}_2 + \ldots \text{OH}^- \rightarrow \ldots \text{CH}_3\text{COO}^- + \ldots \text{H}_2\text{O} + \ldots \text{I}^- + \ldots$.
State one observation that can be made in the reaction in (c)(vi).