Aluminium nitride, AlN, is an ionic compound. It is used in electronic devices because it conducts heat well.
Aluminium has atomic number 13. Nitrogen has atomic number 7.
Give the electronic configuration of an aluminium ion.
Explain, in terms of electron transfer, how aluminium atoms and nitrogen atoms form aluminium nitride. Include the formulae of the ions formed in your answer.
Aluminium also forms an oxide. Deduce the formula of aluminium oxide. Explain your answer.
In moist air, aluminium nitride reacts slowly with water to form aluminium hydroxide, Al(OH)3\mathrm{Al(OH)_{3}}Al(OH)3, and ammonia, NH3\mathrm{NH_{3}}NH3.
Write the balanced equation for this reaction. State symbols are not required.
A sample of aluminium nitride reacts completely with water and produces 1.20 dm3\mathrm{dm^{3}}dm3 of ammonia gas at room temperature and pressure.
Calculate the mass of aluminium nitride in the sample.
Relative atomic masses: Al = 27, N = 14.
The volume of one mole of any gas at room temperature and pressure is 24 dm3\mathrm{dm^{3}}dm3.
56 exam-style questions on Edexcel GCSE Chemistry 2.3 Ionic bonding, covering 2.3.1 Ions and the formation of ionic bonds, 2.3.2 Naming and deducing formulae of ionic compounds, and 2.3.3 Giant ionic lattices. Each one has a worked solution and a mark scheme showing where the marks go.