Complete Table 1.1 by naming the lattice structures of the crystalline solids of Mg, Si and P.
Fig. 1.1 shows the relative electrical conductivities of the Period 3 elements. Explain why conductivity rises from Na to Al and why P, S and Cl are non-conductors of electricity.
Write an equation, with state symbols, to represent the third ionisation energy of argon.
The differences in the third ionisation energy values shown in Fig. 1.2 are caused by differences in the attraction between the nucleus and the outer electron in each ion. State two factors that influence the strength of this attraction between the nucleus and the outer electron.
Use Fig. 1.2 to suggest which factor has the greatest effect on the size of the attraction between the nucleus and the outer electron. Explain your answer.
In the third ionisation energy of argon, the ion formed has the electronic configuration $1\text{s}^2\ 2\text{s}^2\ 2\text{p}^6\ 3\text{s}^2\ 3\text{p}^3$. Complete Fig. 1.3 so that it shows how the electrons are arranged in the orbitals of this ion.
Most Period 3 elements react with oxygen to make oxides. Write an equation for the reaction of phosphorus with oxygen.
Write an equation for the reaction of aluminium oxide with an excess of aqueous sodium hydroxide.
In the third ionisation energy of argon, the ion formed has the electronic configuration $1s^2\,2s^2\,2p^6\,3s^2\,3p^3$. Complete Fig. 1.3 so that it shows how the electrons are arranged in the orbitals of this ion.