Construct an equation that represents the second ionisation energy of argon.
The graph plots successive ionisation energies for argon. Extend the graph by predicting the eighth and ninth ionisation energies of argon. Mark each point with a cross ($\times$).
The energy value needed to remove the first electron from an argon atom has been circled on the graph. Sketch the shape of the orbital that contains this electron.
Chlorine is a diatomic gas, $\text{Cl}_2(\text{g})$. A sample of $\text{Cl}_2(\text{g})$ was produced in a chemical reaction. It had a volume of $20.0\,\text{cm}^3$ when measured at $404\,\text{kPa}$ and $25\,^{\circ}\text{C}$. Calculate the mass, in grams, of $\text{Cl}_2(\text{g})$ produced. For this calculation, assume chlorine behaves as an ideal gas under these conditions.
Calculate how many chlorine atoms are present in this sample of $\text{Cl}_2(\text{g})$. You may want to use your answer to (d)(i). If you cannot work out an answer to (d)(i), use $0.36\,\text{g}$ of $\text{Cl}_2$. This is not the correct answer.
$\text{Cl}_2(\text{g})$ is not an ideal gas under these conditions. Explain why $\text{Cl}_2(\text{g})$ becomes even less ideal at: • very high pressures • very low temperatures.