A) what are main two allotropes of carbon distinguish these two allotropes on basis of hardness and electrical conduction
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Diamond and graphite are both giant covalent substances made entirely of carbon atoms. Both have chemical formula , but they do not have a molecular formula.
Molecular structure
Diamond: Giant covalent structure, with each carbon covalently bonded to four other carbon atoms in a tetrahedral arrangement to form a rigid structure.
Graphite: It is also Giant covalent structure, with each carbon covalently bonded to three other carbon atoms in a hexagonal arrangement.
Hardness
Diamond: Extremely hard. Due to rigid, tetrahedral arrangement of carbon atoms.
Graphite: Soft. Layers of hexagonally arranged carbon atoms can slide over one another.
Electrical conductivity
Diamond: Insulator. Mobile electrons are absent. All four valence electrons are used in covalent bonds.
Graphite: Conductor. Three out of four valence electrons are used for covalent bonding with other carbon atoms. Remaining valence electrons can be delocalised across the planes of carbon atoms.
Molecular structure
Diamond: Giant covalent structure, with each carbon covalently bonded to four other carbon atoms in a tetrahedral arrangement to form a rigid structure.
Graphite: It is also Giant covalent structure, with each carbon covalently bonded to three other carbon atoms in a hexagonal arrangement.
Hardness
Diamond: Extremely hard. Due to rigid, tetrahedral arrangement of carbon atoms.
Graphite: Soft. Layers of hexagonally arranged carbon atoms can slide over one another.
Electrical conductivity
Diamond: Insulator. Mobile electrons are absent. All four valence electrons are used in covalent bonds.
Graphite: Conductor. Three out of four valence electrons are used for covalent bonding with other carbon atoms. Remaining valence electrons can be delocalised across the planes of carbon atoms.
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