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Diamond is harder than graphite because of –
- a)difference in layers of atoms
- b)tetrahedral structure of diamond
- c)difference of crystalline structures
- d)None of these
Correct answer is option 'A'. Can you explain this answer?
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Diamond is harder than graphite because of –a)difference in laye...
Diamond is harder than graphite because diamond has a more complex structure. Diamond's structure is like many pentagons connected together, each pentagon sharing a side with another pentagon or each pentagon sharing a point with another pentagon. All the points are linked together in some way. Graphite's structure is very loose, with its bonds forming layers.
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Diamond is harder than graphite because of –a)difference in laye...
The difference in their atomic structure. Diamond is made up of carbon atoms arranged in a rigid, three-dimensional lattice structure, where each carbon atom is bonded to four neighboring carbon atoms through strong covalent bonds. This arrangement creates a strong and stable structure, making diamond extremely hard.
On the other hand, graphite is made up of carbon atoms arranged in layers, where each carbon atom is bonded to three neighboring carbon atoms in a hexagonal pattern. These layers are held together by weak, non-covalent bonds called van der Waals forces, which allow the layers to slide over each other easily. This layered structure gives graphite its soft and slippery nature.
The difference in atomic structure between diamond and graphite is what makes diamond harder than graphite. In diamond, the strong covalent bonds between carbon atoms make it difficult for the structure to be deformed or scratched, resulting in its hardness. In contrast, the weak van der Waals forces in graphite allow the layers to easily slide over each other, making it soft and easily erasable.
Therefore, the atomic structure, specifically the type of bonding between atoms, is the main reason why diamond is harder than graphite.
On the other hand, graphite is made up of carbon atoms arranged in layers, where each carbon atom is bonded to three neighboring carbon atoms in a hexagonal pattern. These layers are held together by weak, non-covalent bonds called van der Waals forces, which allow the layers to slide over each other easily. This layered structure gives graphite its soft and slippery nature.
The difference in atomic structure between diamond and graphite is what makes diamond harder than graphite. In diamond, the strong covalent bonds between carbon atoms make it difficult for the structure to be deformed or scratched, resulting in its hardness. In contrast, the weak van der Waals forces in graphite allow the layers to easily slide over each other, making it soft and easily erasable.
Therefore, the atomic structure, specifically the type of bonding between atoms, is the main reason why diamond is harder than graphite.
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