Define first ionisation energy.
State and explain how first ionisation energy changes as Group I is descended.
Suggest how this trend helps account for the rise in reactivity as the Group is descended.
In a redox reaction, $0.83\,\text{g}$ of lithium reacted with water to produce $0.50\,\text{dm}^3$ of aqueous lithium hydroxide according to the equation $2\text{Li}(s) + 2\text{H}_2\text{O}(l) \rightarrow 2\text{LiOH}(aq) + \text{H}_2(g)$. Calculate the amount, in moles, of lithium that reacted.
In a redox reaction, $0.83\text{ g}$ of lithium reacted with water to produce $0.50\text{ dm}^3$ of aqueous lithium hydroxide. $\text{2Li(s)} + \text{2H}_2\text{O(l)} \rightarrow \text{2LiOH(aq)} + \text{H}_2\text{(g)}$
Calculate the volume of hydrogen formed at room temperature and pressure.
Calculate the concentration, in $\text{mol dm}^{-3}$, of the $\text{LiOH(aq)}$ produced.
When heated in chlorine, every alkali metal reacts to make the corresponding chloride. Describe the observations when sodium is heated in chlorine and write a balanced equation for the reaction.