The extremely high melting point of diamond (carbon) may be explained by the :

network covalent bonds

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ionic bonds

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hydrogen bonds

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Van der Waal's forces

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none of the above

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Solution

The correct option is A network covalent bonds
Diamond has a giant molecular structure. Each carbon atom is covalently bonded to four other carbon atoms. A lot of energy is needed to separate the atoms in diamond. This is because covalent bonds are strong, and diamond contains very many covalent bonds. This makes diamond's melting point and boiling point very high.

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Explain the following :

(a) Electrovalent compounds conduct electricity in molten or aqueous state.

(b) Electrovalent compounds have a high melting point and boiling point while covalent compounds have low melting and boiling points.

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