How is the structure of a diamond similar to the structure of graphite?
Besides, what type of structure does a diamond have?
Answer: Diamond is organised in a giant lattice structure with strong covalent bonds between carbon atoms. Each carbon atom forms 4 bonds. Explanation: Each carbon atom has four electrons in its outer shell, all of which form covalent bonds which are strong and hard to break.
Also, how does the structure of diamond affect its properties? Properties and uses The three-dimensional arrangement of carbon atoms, held together by strong covalent bonds, makes diamond very hard. Diamond has a very high melting point because a large amount of energy is needed to overcome the many strong covalent bonds.
In this regard, what is the structure of graphite?
Graphite has a giant covalent structure consisting of layers of carbon atoms. Carbon atoms have 4 valence electrons that are available for bonding. In graphite, each carbon atom is covalently bonded to 3 other carbon atoms. Therefore, every carbon atom has 1 electron that is not used for bonding.
What are the properties of diamond and graphite?
The physical properties of graphite
- has a high melting point, similar to that of diamond.
- has a soft, slippery feel, and is used in pencils and as a dry lubricant for things like locks.
- has a lower density than diamond.
- is insoluble in water and organic solvents - for the same reason that diamond is insoluble.