Bonds

Bonds

Ionic Bonding
1. Between metals and non-metal atoms
2. Atoms gain full outer shells by losing or gaining electrons
3. Atoms form positive and negatively charged ions
4. Strong electrostatic forces of attraction between ions
5. Properties
  1. High melting and boiling points due to strong attraction between oppositely charged ions
  2. Conduct electricity when molten or dissolved in water due to mobile ions, however does not when a solid
Covalent bonding
1. Between non-metals atoms only
2. Atoms gain full outer shell by sharing electrons
3. Two types of covalent bonding
  1. Simple molecular
    1. Small group of atoms share electrons forming small molecules
    2. Each covalent bond is very strong
    3. Forces attraction between molecules is weak
    4. Properties
      1. Low melting and boiling points
        Due to the weak forces between molecules easily overcome
      2. Do not conduct electricity in any state
        Due to no mobile ions or delocalised electrons
  2. Giant Macromolecular
    1. Large number of atoms share electrons forming a giant macromolecule
    2. Many strong covalent bonds formed
    3. Two main examples of Giant Macromolecular bonds are both Carbon
      1. Diamond
        Each carbon atom form 4 strong covalent bonds
        High melting and boiling point due to many strong covalent bonds
        Very hard and strong
        Does not conduct electricity
        No free-moving ions or delocalised electrons
      2. Graphite
        Each carbon atom forms 3 strong covalent bonds
        Leaves a 'free' delocalised electron on the outer shell
        Conducts electricity
        Due to delocalised electron
        High melting and boiling point due to many strong covalent bonds
        Lubricant because of layered structure
        Weak forces between layers allow them to slide past each other
Metallic Bonding
1. Metals exist as a lattice of positively charged ions
2. Properties
  1. High melting and boiling points
    1. Due to strong attraction between ions and electrons
  2. Conducts electricity
    1. Due to delocalised outer shell electrons
  3. Malleable since mobile electrons allow planes of metal ions to move past each other without breaking apart
3. Outer shell electrons are delocalised
4. Strong attraction between positive ions and negative electrons

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