Bonding

2.4 Ionic bonding
(a) *describe the formation of ions by electron loss/gain in order to obtain the electronic configuration of an inert gas
Read p87-92
(b) *describe the formation of ionic bonds between metals and non-metals, e.g. NaCl; MgCl₂
Read p93-94

(c) *state that ionic materials contain a giant lattice in which the ions are held by electrostatic attraction, e.g. NaCl (candidates will not be required to draw diagrams of ionic lattices)
Read p96
(d) deduce the formulae of other ionic compounds from diagrams of their lattice structures, limited to binary compounds
Read p94-95
(e) relate the physical properties (including electrical property) of ionic compounds to their lattice structure
Read p97-99

2.5 Covalent bonding
(a) *describe the formation of a covalent bond by the sharing of a pair of electrons in order to gain the electronic configuration of an inert gas
Read p102

(b) describe, using ‘dot-and-cross’ diagrams, the formation of covalent bonds between non-metallic elements, e.g. H₂; Cl₂; O₂; HCl; N₂; H₂O; CH₄; C₂H₄; CO₂
Read p102-105
(c) deduce the arrangement of electrons in other covalent molecules
Read p106
(d) relate the physical properties (including electrical properties) of covalent compounds to their structure and bonding
Read p106-112

2.6 Metallic bonding
(a) *describe metals as a lattice of positive ions in a ‘sea of electrons’
Read p113

(b) *relate the malleability of metals to their structure and the electrical conductivity of metals to the mobility of the electrons in the structure
Read p113