Silicon dioxide melts at 1710 ∘C1710\ ^\circ\text{C}1710 ∘C and sulfur dioxide melts at −72 ∘C-72\ ^\circ\text{C}−72 ∘C. Both substances contain covalent bonds. Which statement explains this difference?
Melting silicon dioxide overcomes weak forces between separate molecules
Melting sulfur dioxide overcomes covalent bonds throughout a giant structure
Melting silicon dioxide overcomes covalent bonds throughout a giant structure
Melting sulfur dioxide overcomes strong forces between oppositely charged ions
42 exam-style questions on AQA GCSE Chemistry 2.2 How bonding and structure are related to the properties of substances, covering 2.2.1a The three states of matter, 2.2.1b Limitations of the simple particle model, 2.2.2 State symbols in chemical equations, 2.2.3 Properties of ionic compounds, 2.2.4 Properties of small molecules, 2.2.5 Polymers, 2.2.6 Giant covalent structures, 2.2.7 Properties of metals and alloys, and 2.2.8 Metals as conductors. Each one has a worked solution and a mark scheme showing where the marks go.