Bonding

Bonding

1. Ionic

   • Involves the loss or gain of electrons
     • REDOX ( Reduction Oxidation )
     • OILRIG Oxidation Is Loss of electrons Reduction Is Gain of electrons
   • Between Non-Metals and metals
     • Non-Metals Commonly Groups 1+2
     • Metals Commonly Groups 6+7
   • Charged particles form (ions) because no. of protons and electrons are no longer equal
     • Therefore the + & - particles are strongly attracted - Electrostatic forces of attraction
       • Which gives ionic compound their high melting & boiling points
   • Common Examples:

2. Covalent

   • Involves the sharing of a pair of electrons
     • So atoms feel like they have a full shell
   • Between Non-Metals only
     • An example is di-atomic molocules
       • H2 - N2 - 02 - Cl2
   • There are strong bonds between the shared e- and the nuclei of the atoms
   • Some examples:
   • The forces of attraction or intermolecular forces are very weak
     • SO the melting and boiling points are very low as it takes little energy to break the intermolecular forces
       • As A result most molecular substances are a liquid or gas at room temp

3. Metallic

   • Metallic Bonding:
     • The substance is describes as having a sea of delocalised electrons
   • When bonding occurs the outer electron(s) become free or delocalised.
     • These electrons are not paired to any atom so can flow throughout the whole substance
       • WHich is why metallic compounds conduct electricity

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