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Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:
- a)undergoes sp2 hybridization and forms three sigma bonds with three neighbouring carbon atoms
- b)undergoes sp3 hybridization
- c)is tetrahedrally bonded
- d)is free from van der Waals force
Correct answer is option 'A'. Can you explain this answer?
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Graphite is a much better conductor of heat and electricity than diamo...
Undergoes sp2 hybridization and forms three sigma bonds with three neighbouring carbon atoms.
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Graphite is a much better conductor of heat and electricity than diamo...
Explanation:
Each carbon atom in graphite undergoes sp2 hybridization and forms three sigma bonds with three neighboring carbon atoms, creating a hexagonal lattice structure. This allows for the formation of delocalized π bonds above and below the plane of the carbon atoms, which are responsible for the high electrical conductivity of graphite.
Reasoning:
- In sp2 hybridization, each carbon atom uses one s orbital and two p orbitals to form three equivalent sp2 hybrid orbitals.
- These sp2 hybrid orbitals then overlap with the sp2 hybrid orbitals of neighboring carbon atoms to form strong sigma bonds.
- The remaining p orbital on each carbon atom overlaps sideways to form delocalized π bonds, which allow for the movement of electrons along the planes of graphite.
Comparison with Diamond:
- In contrast, each carbon atom in diamond undergoes sp3 hybridization, forming four sigma bonds with neighboring carbon atoms in a tetrahedral arrangement.
- The lack of delocalized π bonds in diamond restricts the movement of electrons, resulting in poor electrical conductivity compared to graphite.
Therefore, the sp2 hybridization and delocalized π bonds in graphite are the key factors that contribute to its superior conductivity compared to diamond.
Each carbon atom in graphite undergoes sp2 hybridization and forms three sigma bonds with three neighboring carbon atoms, creating a hexagonal lattice structure. This allows for the formation of delocalized π bonds above and below the plane of the carbon atoms, which are responsible for the high electrical conductivity of graphite.
Reasoning:
- In sp2 hybridization, each carbon atom uses one s orbital and two p orbitals to form three equivalent sp2 hybrid orbitals.
- These sp2 hybrid orbitals then overlap with the sp2 hybrid orbitals of neighboring carbon atoms to form strong sigma bonds.
- The remaining p orbital on each carbon atom overlaps sideways to form delocalized π bonds, which allow for the movement of electrons along the planes of graphite.
Comparison with Diamond:
- In contrast, each carbon atom in diamond undergoes sp3 hybridization, forming four sigma bonds with neighboring carbon atoms in a tetrahedral arrangement.
- The lack of delocalized π bonds in diamond restricts the movement of electrons, resulting in poor electrical conductivity compared to graphite.
Therefore, the sp2 hybridization and delocalized π bonds in graphite are the key factors that contribute to its superior conductivity compared to diamond.
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Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:a)undergoes sp2 hybridization and forms three sigma bonds with three neighbouring carbon atomsb)undergoes sp3 hybridizationc)is tetrahedrally bondedd)is free from van der Waals forceCorrect answer is option 'A'. Can you explain this answer?
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Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:a)undergoes sp2 hybridization and forms three sigma bonds with three neighbouring carbon atomsb)undergoes sp3 hybridizationc)is tetrahedrally bondedd)is free from van der Waals forceCorrect answer is option 'A'. Can you explain this answer? for Defence 2024 is part of Defence preparation. The Question and answers have been prepared according to the Defence exam syllabus. Information about Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:a)undergoes sp2 hybridization and forms three sigma bonds with three neighbouring carbon atomsb)undergoes sp3 hybridizationc)is tetrahedrally bondedd)is free from van der Waals forceCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Defence 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:a)undergoes sp2 hybridization and forms three sigma bonds with three neighbouring carbon atomsb)undergoes sp3 hybridizationc)is tetrahedrally bondedd)is free from van der Waals forceCorrect answer is option 'A'. Can you explain this answer?.
Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:a)undergoes sp2 hybridization and forms three sigma bonds with three neighbouring carbon atomsb)undergoes sp3 hybridizationc)is tetrahedrally bondedd)is free from van der Waals forceCorrect answer is option 'A'. Can you explain this answer? for Defence 2024 is part of Defence preparation. The Question and answers have been prepared according to the Defence exam syllabus. Information about Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:a)undergoes sp2 hybridization and forms three sigma bonds with three neighbouring carbon atomsb)undergoes sp3 hybridizationc)is tetrahedrally bondedd)is free from van der Waals forceCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Defence 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:a)undergoes sp2 hybridization and forms three sigma bonds with three neighbouring carbon atomsb)undergoes sp3 hybridizationc)is tetrahedrally bondedd)is free from van der Waals forceCorrect answer is option 'A'. Can you explain this answer?.
Solutions for Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:a)undergoes sp2 hybridization and forms three sigma bonds with three neighbouring carbon atomsb)undergoes sp3 hybridizationc)is tetrahedrally bondedd)is free from van der Waals forceCorrect answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for Defence.
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ample number of questions to practice Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:a)undergoes sp2 hybridization and forms three sigma bonds with three neighbouring carbon atomsb)undergoes sp3 hybridizationc)is tetrahedrally bondedd)is free from van der Waals forceCorrect answer is option 'A'. Can you explain this answer? tests, examples and also practice Defence tests.
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