Ionic bonding, metallic bonding, and structure

• What is an ion?


  Atom that has lost or gained electrons
• What kinds of elements form ionic bonds?

  Metals and Non-metals
• What charges do ions from Groups 1 and 2 form?

  Group 1 forms 1+ Group 2 forms 2+
• What charges do ions from Groups 6 and 7 form?

  Group 6 forms 2- Group 7 forms 1-
• Name the force that holds oppositely charged ions together

  Electrostatic force of attraction
• Describe the structure of a giant ionic lattice

  Regular structure of alternating positive and negative ions, held together by the electrostatic force of attraction
• Why do ionic substances have high melting points?

  Electrostatic force of attraction between positive and negative ions is strong and requires lots of energy to break
• Why don't ionic substances conduct electricity when solid?

  Ions are fixed in position so cannot move, and there are no delocalised electrons
• When can ionic substances conduct electricity?

  when melted or dissolved
• Why do ionic substances conduct electricity when melted or dissolved?

  Ions are free to move and carry charge
• Describe the structure of a pure metal

  Layers of positive metal ions surrounded by delocalised electrons
• Describe the bonding in a pure metal

  strong electrostatic forces of attraction between metal ions and delocalised electrons
• What are four properties of pure metals?

  Malleable, High melting/boiling points, good conductors of electricity, good conductors of thermal energy
• Explain why pure metals are malleable

  Layers can slide over each other easily
• Explain why metals have high melting and boiling points

  Electrostatic force of attraction between positive metal ions and delocalised electrons is strong and requires a lot of energy to break
• Why are metals good conductors of electricity and of thermal energy?

  Delocalised electrons are free to move through the metal
• What is an alloy?


  Mixture of a metal with atoms of another element
• Explain why alloys are harder than pure metals

  Different sized atoms disturb the layers, preventing them from sliding over each other