Self Assessment Checklist – Chemical Bonding

Knowing the learning objectives is the first step in acing Chemistry. Master the essential concepts and apply them to interesting Chemistry questions confidently. Topical syllabus objective checklists are available here for your self-assessment. These checklists are based on Cambridge O-level Syllabus. Conduct self assessment when you revise. Tick against objectives that you can confidently say ‘I Can Do It’. Revise objectives that you are unsure of. Knowing what you need to know builds confidence in tackling questions. 

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Self Assessment Checklist - Chemical Bonding

  I can do this!
aDescribe the stable electronic configuration of a noble gas.
bDeduce the physical and chemical properties of substances from their structures and bonding and vice versa.

Self Assessment Checklist - Ionic Bonding

  I can do this!
aDescribe the formation of ions by electron loss/gain in order to obtain the electronic configuration of a noble gas.

bDescribe the formation of ionic bonds between metals and non-metals, e.g. sodium chloride; magnesium chloride
cState that ionic compounds form giant lattices in which the ions are held by electrostatic attraction, e.g. sodium chloride (will not be required to draw diagrams of ionic lattices)
dDeduce the formula of an ionic compound from the charges on the ions and vice versa.
eDeduce the formula of an ionic compound from the diagram of its lattice structure, limited to binary compounds.
fRelate the physical properties (including electrical property) of ionic compounds to their lattice structure.

Self Assessment Checklist - Covalent Bonding

  I can do this!
aDescribe 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
bDescribe, using ‘dot-and-cross’ diagrams, the formation of covalent bonds between non-metallic elements
Example: Hydrogen, Oxygen, Water, Methane, Carbon Dioxide
cDeduce the arrangement of electrons in covalent molecules.
dCompare 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.
eCompare 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).
fRelate the physical properties (including electrical property) of covalent substances to their structure and bonding.

Self Assessment Checklist - Metallic Bonding

  I can do this!
aDescribe metals as a lattice of positive ions in a ‘sea of electrons’.
bRelate the physical properties of metals to their structure.
cRelate the electrical conductivity of metals to the mobility of the electrons in the structure.
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