Write properties of diamond and graphite and how are they different from each other?
Answers
Answer:
The difference between diamond and carbon is given below.
Diamond Graphite-
It has crystalline nature
It has layered structure
Each C is sp
hybridzed and forms 4 covalent bonds with neighboring C atoms.
Each C atom is sp
2
hybridized and forms 3 sigma bonds with 3 other C atoms. Fourth electron forms pi bond.
The geometry is tetrahedral.
The geometry is planar
C-C bond length is 154 pm
C-C bond length is 141.5 pm
It has rigid covalent boning which is difficult to break.
It is soft. Its layers can be separated easily.
It is an electrical insulator.
It is good conductor of electricity.
Explanation:
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Answer
Graphite and diamond are both covalent bonds (made up of non-metal elements only) made from the element carbon, and they both are arranged in a regular lattice structure, but they do differ in many different ways..
Graphite has a hexagonal layered sheet, and it has 1 carbon atom connected or linked to 3 other carbon atoms, so it has 1 free delocalised electron and therefore graphite conducts electricity.
Diamonds have a tetrahedral arrangement, and 1 carbon atom is connected to 4 other carbon atoms, but there are no any delocalised electrons in diamonds, so diamonds don't conduct electricity, Diamonds are also one of the hardest substances on earth because of their tetrahedral structure.