Question

compare the properties of diamond andg raphite

Answer 1

Diamonds have a 3d network of strong covalent bonds which makes it hard to break but Graphite has flat layers of carbon atoms held together by weak Van der Waal's forces which makes Graphite easily breakable

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Answer 2

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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.

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