1. Macromolecular / giant covalent Molecular / simple covalent
Ionic
Metallic
Covalent
Macromolecular / giant covalent
Molecular / simple covalent
Graphite
Diamond
Diagram of structure
Describe how the bonds are formed
Melting point & why?
Electrical conductivity & why?
Solubility & why?
Activity 1- Structure and properties research task

2. ANSWERS Ionic Sodium chloride Metallic Sodium Covalent Giant covalent
Simple covalent
Iodine
Graphite
Diamond
Diagram of structure
Describe how the bonds are formed
1 electron transferred from a sodium atom to a chlorine atom to make Na+ and Cl–.
Electrostatic attraction between ions of opposite charge and electrostatic repulsion between ions of similar charge.
Outer-shell electrons are delocalised to the bulk. Electrostatic attractions between the delocalised electrons and the metal ions and electrostatic repulsions between electrons and between the metal ions.
Each carbon forms three covalent bonds with three other carbon atoms (sharing of two outer-shell electrons). The fourth electron is delocalised across the graphite layer.
Weak intermolecular forces between adjacent layers.
Each carbon forms four single covalent bonds with four other carbon atoms (sharing of two outer-shell electrons).
A single covalent bond exists between iodine atoms, with each atom sharing one electron each.
Weak intermolecular forces between adjacent iodine molecules.
Melting point & why?
High because the strong electrostatic forces of attraction between oppositely charged ions require large amounts of energy (hence high temperature) to break.
High, because the strong electrostatic forces of attraction between the metal ions and the electrons require large amounts of energy (hence high temperature) to break.
High, because it is a giant lattice and large amounts of energy (hence high temperature) are required to break the strong covalent bonds.
Low, as the intermolecular forces between the molecules are weak, so require little energy (hence low temperature) to break.
Electrical conductivity & why?
Conducts electricity in liquid state and in solution due to the flow of ions.
Conducts electricity in the solid and molten state, due to flow of delocalised electrons.
Conducts electricity in the solid state due to the flow of delocalised electrons.
Does not conduct electricity – electrons are localised in covalent bonds.
Solubility in water & why?
Soluble: ions can form bonds with the polar water molecules.
Insoluble as not polar.
Slightly soluble in water as induced dipoles in iodine can form bonds with polar water molecules.