Why is the oxide of si solid while the oxide of c is gas at room temperature?
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The oxide of carbon, CO2 and CO exist as simple melecular structure. The intermolecular forces of attraction between the molecules is the weak van der Waals force. Hence they have low melting and boiling points and at room temperature and atmospheric pressure , they exist as gas molecules.
The oxide of Si, that is SiO2 exist as giant covalent structure. The Si atom and oxygen are bonded together by strong covalent bond tetrahedrally forming a very big molecules. A large amount of energy is needed to break the covalent bonds as well as the giant structure.
That's why it has a very high melting and boiling points. Hence, it exists as solid at room temperature.
The oxide of Si, that is SiO2 exist as giant covalent structure. The Si atom and oxygen are bonded together by strong covalent bond tetrahedrally forming a very big molecules. A large amount of energy is needed to break the covalent bonds as well as the giant structure.
That's why it has a very high melting and boiling points. Hence, it exists as solid at room temperature.
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