CHAPTER 5: States of  Matter

1. The Gaseous State
2. The Liquid State
3. The Solid State
4. Ceramics
5. Conserving Materials

Learning outcomes:

• state the basic assumptions of the kinetic theory as applied to an ideal gas
• explain qualitatively in terms of intermolecular forces and molecular size:
  • the conditions necessary for a gas to approach ideal behaviour
  • the limitations of ideality at very high pressures and very low temperatures
• state and use the general gas equation pV = nRT in calculations, including the determination of   Mr
• describe, using a kinetic-molecular model: the liquid state, melting, vaporisation, vapour pressure.
• describe, in simple terms, the lattice structure of a crystalline solid which is:
  • ionic, as in sodium chloride, magnesium oxide
  • simple molecular, as in iodine
  • giant molecular, as in silicon(IV) oxide and the graphite and diamond allotropes of carbon
  • hydrogen-bonded, as in ice
  • metallic, as in copper

[the concept of the ‘unit cell’ is not required]

• explain the strength, high melting point and electrical insulating properties of ceramics in terms of their giant molecular structure
• relate the uses of ceramics, based on magnesium oxide, aluminium oxide and silicon(IV) oxide, to their properties (suitable examples include furnace linings, electrical insulators, glass, crockery).
• discuss the finite nature of materials as a resource and the importance of recycling processes
• outline the importance of hydrogen bonding to the physical properties of substances, including ice and water (for example, boiling and melting points, viscosity and surface tension).
• suggest from quoted physical data the type of structure and bonding present in a substance