The melting points of the oxides of the third-period elements are given in parentheses: Na2O (1275°C), MgO (2800°C), Al2O3 (2045°C), SiO2 (1610°C), P4O10 (580°C), SO3 (16.8°C), Cl2O7 (91.5°C). Classify these solids in terms of crystal types. Na2O: ionic covalent molecular metallic. MgO: ionic covalent molecular metallic

Period 3 oxides, such as Na2O, MgO, and Al2O3, exhibit a range of bonding from ionic to covalent, influencing their melting points, electrical conductivity, and acid-base reactions with water. These compounds demonstrate the diverse chemical behavior of elements in the third period, with metal oxides being basic, non-metal oxides acidic, and ...

PCl3, PCl5, S2Cl2, Cl2 – all have simple molecular structures (covalently bonded molecules) held together by weak van der Waals’ forces, resulting in low melting and boiling points. S2Cl2 Cl2 molecules. NaCl dissolves in H2O to give a neutral solution …

2023年6月30日 · The structures: The metallic oxides on the left adopt giant structures of ions on the left of the period; in the middle, silicon forms a giant covalent oxide (silicon dioxide); the elements on the right form molecular oxides.

- Na2O, MgO and Al2O3: METAL oxides, so form GIANT IONIC LATTICES > high melting points due to strong electrostatic attractions between oppositely charged ions. - Al2O3: lower than expected due to COVALENT character: smaller difference in electronegativity between Al and O so O cannot attract electrons strongly, Al distorts electrons.

2009年4月16日 · • Na2O, MgO, Al2O3: Exist as ionic structure. A large amount of energy is required to break the strong electrostatic attraction forces between the ions in the lattice. • SiO2: Exist as giant covalent structure where Si and O atoms are held by covalent bonds. A lot of energy is required to break the strong covalent bonds.

An amphoteric oxide - reacts with both acids and alkalis e.g. Al2O3 and HCl: - Al2O3(s) + 6HCl(aq) 2AlCl3(aq) + 3H2O(l) e.g. Al2O3 and hot, concentrated NaOH: - Al2O3(s) + 2NaOH(aq) + 3H2O(l) 2NaAl(OH)4 (aq)

Describe Na2O, MgO, Al2O3 structure & bonding & why? Ionic Giant Lattice structures: strong forces of attraction between ions. Explain bonding in Al2O3? Due to electronegativity diff being less big OR the small aluminium ion with a high charge being able to get close to the oxide ion and distorting the oxide charge cloud.

This document is an A-level chemistry past paper from AQA, covering Period 3 elements and their oxides. It includes equations, observations, and melting point information for different compounds like Na2O, MgO, and others. It covers concepts like ionic and covalent bonding, and neutralization reactions. Full Transcript

MgO and Al2O3 have a higher melting point than Na2O since the charges are higher, resulting in a stronger attraction between the ions. SiO2 has a giant covalent structure and hence a high melting point. There are strong covalent bonds between all the atoms and thus lots of energy is required to break them.