At room temperature fluorine and chlorine are gases, bromine is a liquid and iodine is a solid. State how volatility changes down Group 17.
Explain why this pattern occurs.
Iodine, $\text{I}_2$, is displaced from $\text{NaI(aq)}$ by chlorine, $\text{Cl}_2$. Write an equation for this reaction.
Silver nitrate solution, $\text{AgNO}_3(aq)$, is added to separate solutions of $\text{NaI}$ and $\text{NaCl}$. Precipitates form. Excess aqueous ammonia is then added to both precipitates. Complete the table with the colour and name of the precipitate produced in each reaction, and with what happens when excess aqueous ammonia is added to each precipitate.
Write an ionic equation, including state symbols, to show the reaction taking place when $\text{AgNO}_3(aq)$ is added to $\text{NaI(aq)}$.
Solid $\text{NaI}$ reacts with concentrated sulfuric acid to give purple fumes of $\text{I}_2\text{(g)}$ and hydrogen sulfide gas, $\text{H}_2\text{S\,(g)}$. By contrast, when solid $\text{NaCl}$ reacts with concentrated sulfuric acid, the only gas formed is $\text{HCl\,(g)}$. Explain why concentrated sulfuric acid reacts differently with $\text{NaI}$ and with $\text{NaCl}$. Your answer should mention the role of the sulfuric acid in each case.
Explain what is meant by oxidising agent in terms of electron transfer.
Suggest an equation for the reaction between chlorine and water.
Write an equation for the reaction between chlorine and hot aqueous sodium hydroxide. Use oxidation numbers to explain why this counts as a redox reaction.