Define what electronegativity is.
O and S are both in Group 16. Explain why their Pauling electronegativity values are different.
$\text{LiH}$ is ionic. Draw a dot-and-cross diagram for $\text{LiH}$. Show every electron.
Suggest the molecular shape of $\text{H}_2\text{S}$.
Write an equation to represent the first ionisation energy of $\text{H}$.
Explain why Table 1.1 gives no data for the second ionisation energy of $\text{H}$.
Give the full electronic configuration for $\mathrm{S}^{2+}(g)$.
$\text{CO}_2$ and $\text{SO}_2$ are acidic gases. Write an equation for how $\text{SO}_2$ reacts with $\text{H}_2\text{O}$.
Write an equation for how $\text{SO}_2$ reacts with $\text{NaOH}$.
Construct an equation for how $\text{CO}_2$ reacts with $\text{Mg(OH)}_2$.
Complete Table 1.2 by placing a tick ($\checkmark$) to indicate which compounds have molecules with an overall dipole moment.
At $150^{\circ}\text{C}$ and $103\,\text{kPa}$, every compound listed in Table 1.2 is gaseous. Under these conditions, $0.284\,\text{g}$ of one compound occupies a volume of $127\,\text{cm}^3$. Use this information to calculate the $M_r$ of the compound. Hence, identify the compound from those shown in Table 1.2. Show your working.