Bonding and structures relation to properties of substances

• What are the three states of matter?

  Solid, liquid, and gas
• At what point do melting and freezing occur?

  At the melting point
• At what point do boiling and condensing occur?

  At the boiling point
• How does particle theory explain changes in states of matter?

  • Energy needed to change state depends on forces between particles.
  • Nature of particles depends on bonding and structure.
  • Stronger forces lead to higher melting and boiling points.
• What are the limitations of the simple particle model of matter?

  It assumes no forces, represents particles as solid spheres, and ignores particle interactions.
• How are the states of matter represented in chemical equations?

  Solid (s), liquid (l), gas (g), and aqueous (aq)
• What are the properties of ionic compounds?

  • Regular structures (giant ionic lattices) with strong electrostatic forces.
  • High melting and boiling points due to strong bonds.
  • Conduct electricity when melted or dissolved, but not when solid.
• What are the properties of small molecules?

  • Usually gases or liquids with low boiling and melting points.
  • Weak intermolecular forces broken during boiling or melting.
  • Do not conduct electricity due to lack of overall charge.
• What type of molecules do polymers consist of?

  Very large molecules
• What are the properties of polymers?

  • Atoms linked by strong covalent bonds.
  • Strong intermolecular forces make them solids at room temperature.
• What are giant covalent structures and their properties?

  • Solids with very high melting points.
  • Atoms linked by strong covalent bonds.
  • Bonds must be overcome to melt or boil.
  • Examples: diamond, graphite, and silicon dioxide.
• What are the properties of metals and alloys?

  • Metals have giant structures with strong metallic bonding.
  • High melting and boiling points.
  • Atoms can slide over each other, making metals malleable.
  • Alloys are harder than pure metals due to distorted layers.
• Why are metals good conductors of electricity and thermal energy?

  • Delocalised electrons carry electrical charge.
  • Delocalised electrons transfer thermal energy.