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Chemical Bonding - Coggle Diagram

- - - - Simple covalent compounds have low melting and boiling points.
        Reason: Simple covalent compounds consist of small, discrete molecules. Thus, only a small amount of energy is need to overcome the weak intermolecular forces of attraction.
      - Simple covalent compounds are generally unable to conduct electricity in any state.
        Reason: Since simple covalent compounds are made up of small, discrete molecules, they have no free-moving ions or delocalised electrons to act as mobile charge carriers to conduct electricity.
      - Simple covalent compounds are mostly insoluble in water and usually soluble in organic solvents.
  - - - Each carbon atom of diamond is covalently bonded to another four carbon atoms in a repeated tetrahedral arrangement.
      - Properties of diamond
        
        Diamond has very high melting and boiling points.
        Reason: Diamond has a giant covalent structure. A large amount of energy is required to overcome the strong covalent bonds between the carbon atoms of diamond.
        
        Diamond is unable to conduct electricity.
        Reason: Each carbon atom of diamond uses up all four of its valence electrons to form covalent bonds with four other carbon atoms. Thus, there are no delocalised electrons to act as mobile charge carriers to conduct electricity.
        
        Diamond is very hard.
        Reason: A large amount of energy is required to overcome the strong intermolecular forces between the carbon atoms of diamond.
        
        Diamond is insoluble in both water and organic solvents.
    - - Each carbon atom of graphite is covalently bonded to another three carbon atoms in a repeated hexagonal arrangement. They form parallel layers, which are held together by weak intermolecular forces of attraction. Since only 3 out of 4 of the valence electrons of each carbon atom are involved in covalent bonding, the last valence electron is delocalised and can conduct electricity.
      - Properties of graphite
        
        Graphite has very high melting and boiling points.
        Reason: Graphite has a giant covalent structure. Thus, a large amount of energy is needed to overcome the strong covalent bonds between the carbons atoms of graphite.
        
        Graphite is able to conduct electricity.
        Reason: Each carbon atom uses 3 out of 4 of its valence electrons to form covalent bonds with 3 other carbon atoms. Each carbon atoms has one valence electron not used in covalent bonding, this electron is delocalised and can conduct electricity.
        
        Graphite is soft and slippery.
        Reason: The layers of carbon atoms of graphite are held together by weak intermolecular forces of attraction and can thus slide over each other.
        
        Graphite is insoluble in both water and organic solvents.