1e. A brief comparison of types of bonding and structure of substances related to their physical properties

(best studied as you work through Parts 2 to 5)

PRACTICAL RESEARCH - investigating the properties of a variety of compounds

You can learn how to classify different types of elements and compounds in terms of their structure and bonding by investigating their:

melting points and boiling points, solubility in water and electrical conductivity (as solids and in solution) of substances such as sodium chloride, magnesium sulphate, hexane, liquid paraffin, silicon(IV) oxide, copper sulphate, and sucrose (sugar).

You can do simple experiments as well as looking up their properties in data books to decide the nature of their structure and chemical bonding involved.

Comparing substances based on the type of bonding holding the atoms together

Property \ bond type	Ionic	Covalent - relatively small molecules	Covalent - giant structures	Metallic giant structure
Examples	Sodium chloride, magnesium oxide	hydrogen, chlorine, ammonia, carbon dioxide, water, wax	carbon - diamond, silicon, silicon dioxide	copper, iron, gold, sodium
'Picture' of the structure . ~3D except only 2D for metal
Bonding in structure	Giant lattice of oppositely charged ions strongly attracted to each other	Relatively few atoms strongly bonded together to form individual molecules - mutual attraction to electrons between the nuclei	Giant lattice of many atoms bonded together to form (usually) an extended 3D network.	Giant lattice of many atoms (actually positive ions) bonded together by attraction to free moving negative electrons between them
Physical state at room temperature	All solid	Gas, liquid or solid	All solid	All solid (except liquid mercury)
Melting/boiling points	All relatively high	Relatively low	Relatively high	Mostly high
Electrical conduction	Solid NO, When molten or dissolved in water YES - ions free to move	Poor or not at all - little or NO free ions or electrons to carry an electric current	Very poor or not at all - graphite an exception - does have delocalised electrons in each layer	All good conductors - all have free delocalised electrons to carry an electric charge current through the giant lattice

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