In this I/GCSE Chemistry blog post, we will lookg at the different example of covalent bondings such as silicon and diamond.
Diamond (and Silicon)
- Each Carbon atom forms 4 strong covalent bonds with other atoms to give a tetrahedral structure.
High melting and boiling points
- A lot of energy is required to break the many strong bonds, hence the high melting and boiling points.
Hard Substance
- The many strong bonds each require a large force to break them.
Doesn't conduct electricity
- No free electrons to carry a current when a potential is applied.
- Insoluble
Graphite
- Each Carbon atoms forms 3 strong covalent bonds with other Carbon atoms, resulting in a layered structure.
- One spare electron is delocalised between the layers.
- The layers are held together by weak intermolecular forces.
High Melting and Boiling points
- The many strong bonds require a lot of energy to break, hence the high melting and boiling points.
Soft Substance
- Little force is needed to overcome the weak intermolecular forces.
Conducting Electricity
- The free delocalised electron is able to carry a current when a potential is applied.
That is all!
References:
https://www.google.com/url?sa=i&url=https%3A%2F%2Fwww.tutormyself.com%2Fedexcel-igcse-2017chem-150%2F&psig=AOvVaw3jug-TEo_dfVgOuXpS9nOY&ust=1629516896456000&source=images&cd=vfe&ved=0CAsQjRxqFwoTCOC3yNDVvvICFQAAAAAdAAAAABAD
https://www.google.com/url?sa=i&url=http%3A%2F%2Figcsechemisrtynotes.blogspot.com%2F2009%2F11%2Fdiamond-and-graphite-igcse-gcse.html&psig=AOvVaw2qVHWDHkUHR0kpyHu07lpl&ust=1629516976769000&source=images&cd=vfe&ved=0CAsQjRxqFwoTCNjZjvfVvvICFQAAAAAdAAAAABAJ