Reaction 1 gives $\mathrm{Ca(NO_3)_2}$ plus one further product. Name the other product.
Write an equation for the thermal decomposition of $\mathrm{Ca(NO_3)_2(s)}$.
State the trend in the thermal stability of the Group 2 nitrates down the group.
In reaction 3, excess $\mathrm{CO_2}$ is bubbled through water containing $\mathrm{CaCO_3}$. A solution of $\mathrm{Ca(HCO_3)_2(aq)}$ is produced. Construct an equation for reaction 3.
Describe how $\mathrm{Ca(OH)_2}$ is used in agriculture.
In reaction 4, calcium carbide, $\mathrm{CaC_2}$, is made from $\mathrm{CaO}$. $\mathrm{CaC_2}$ contains the $\mathrm{C_2^{2-}}$ anion. Each carbon atom in $\mathrm{C_2^{2-}}$ is $sp$ hybridised. Describe how $sp$ hybridised orbitals are formed.
Sketch a diagram showing how two $sp$ hybrid orbitals can make a sigma ($\sigma$) bond.
The flowchart presents some reactions of $\text{CaC}_2$.
Reaction 5 can be used to make $\text{NH}_3$. $\text{CaCN}_2 + 3\text{H}_2\text{O} \rightarrow \text{CaCO}_3 + 2\text{NH}_3$ Calculate the minimum mass, in tonnes, of calcium cyanamide, $\text{CaCN}_2$, that is required to produce $1.50 \times 10^6$ tonnes of $\text{NH}_3$. Show your working. $1$ tonne $= 1.00 \times 10^6\ \text{g}$.
Draw the structures of the organic products formed in the reactions below: $\text{CH}_3\text{CH}_2\text{Br}$ with $\text{NaCN}$ dissolved in ethanol, then $\text{H}_2\text{SO}_4$(aq) heated under reflux. A carbonyl compound reacted with $\text{NaCN}$ and $\text{HCN}$.