Syllabus Objectives – Chemical Bonding

Self Assessment Checklist

Bonding I can do this!
(a) Describe the stable electronic configuration of a noble gas.
(b) Deduce the physical and chemical properties of substances from their structures and bonding and vice versa.

 

Ionic Bonding I can do this!
(a) Describe the formation of ions by electron loss/gain in order to obtain the electronic configuration of a noble gas.  
(b) Describe the formation of ionic bonds between metals and non-metals, e.g. NaCl; MgCl2.
(c) State that ionic compounds form giant lattices in which the ions are held by electrostatic attraction, e.g. NaCl (will not be required to draw diagrams of ionic lattices)
(d) Deduce the formula of an ionic compound from the charges on the ions and vice versa.
(e) Deduce the formula of an ionic compound from the diagram of its lattice structure, limited to binary compounds.  
(f) Relate the physical properties (including electrical property) of ionic compounds to their lattice structure.  

 

Covalent bonding I can do this!
(a) Describe the formation of a covalent bond by the sharing of a pair of electrons in order to gain the electronic configuration of a noble gas
(b) Describe, using ‘dot-and-cross’ diagrams, the formation of covalent bonds between non-metallic elements, e.g. H2; O2; H2O; CH4; CO2.
(c) Deduce the arrangement of electrons in covalent molecules.
(d) Compare the structure of simple molecular substances, e.g. methane; iodine, with those of giant molecular substances, e.g. poly(ethene); sand (silicon dioxide); diamond; graphite in order to deduce their properties.
(e) Compare the bonding and structures of diamond and graphite in order to deduce their properties such as electrical conductivity, lubricating or cutting action (will not be required to draw the structures).
(f) Relate the physical properties (including electrical property) of covalent substances to their structure and bonding.

 

Metallic bonding I can do this!
(a) Describe metals as a lattice of positive ions in a ‘sea of electrons’.
(b) Relate the physical properties of metals to their structure.
(c) Relate the electrical conductivity of metals to the mobility of the electrons in the structure.