chapter 3

chapter 3

ionic bonding
1. metal and non metal
  1. metals lose electrons to form a stable ion
  2. non metals ions gain electrons to form stable ions
2. strong electrostatic forces of attraction between oppositley charged ions in an ionic compound
  1. regular lattice structure
3. use the charges to work out the formula of the ionic compound
4. conduct electricity when molten/ in solution
covalent bonding
1. non metals
2. a shared pair of electrons
  1. very strong as a lot of energy is needed to overcome the electrostatic forces of attraction
3. diamond and graphite
  1. allotropes
    1. same state but different structures
  2. DIAMOND
    1. each carbon atom forms 4 strong covalent bonds
    2. tetrahedral structure
      1. giant covalent
  3. GRAPHITE
    1. 3 covalent bonds between each carbon atom
      1. layers
        hexagonal structure
      2. between each layer is delocalised electrons which allow the layers to slide
metallic bonding
1. just metals ;)
2. electrons in the outer shell become delocalized
  1. +ve metal ions (cations) are held together by a sea of delocalised -ve electrons
    1. strong electrostatic forces
3. mallelable and ductile
  1. metal cations slide over each other if enough force is applied
4. magnesium
  1. hexagonal packed structure
    1. alternate layers
Coordinate bonding
1. 'dative covalent bond'
  1. just like a covalent bond but both electrons are donated from one atom
2. to form there must be a lone pair of electrons in one atom and a vacant orbital in the other atom
shapes
1. linear
  1. 180
  2. 2 bonding pairs
2. trigonal planar
  1. 120
  2. 3 bonding pairs
3. tetrahedral
  1. 109.5
  2. 4 bonding pairs
4. trigonal bipyramidal
  1. 90 and 120
  2. 5 bonding pairs
5. octahedral
  1. 90
  2. 6 bonding pairs
6. strength of repulsion
  1. lone pair : lone pair
    1. lone pair : bonding pair
      1. bonding pair : bonding pair

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