GCSE Chemistry Revision "Diamond and Silicon Dioxide"
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Giant covalent molecules like diamond and silicon dioxide have high melting and boiling points because of the numerous strong covalent bonds they contain. These molecules, such as diamond composed of carbon and silicon dioxide made of silicon and oxygen, exhibit exceptional hardness and inability to conduct electricity due to their unique covalent bonds.
Insights
- Giant covalent molecules like diamond and silicon dioxide exhibit high melting and boiling points because of the multitude of strong covalent bonds they possess, necessitating significant energy for bond breakage.
- Diamond's exceptional hardness and inability to conduct electricity stem from its unique structure of carbon atoms forming covalent bonds with each other, while silicon dioxide's similar properties are attributed to the strong covalent bonds between silicon and oxygen atoms.
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What are giant covalent molecules?
Large molecules with millions of covalent bonds.
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Summary
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"High Melting Points of Giant Covalent Molecules"
- Giant covalent molecules like diamond and silicon dioxide have millions of covalent bonds, leading to high melting and boiling points due to the significant energy required to break these bonds.
- Diamond, composed of carbon atoms forming covalent bonds with four other carbon atoms, is extremely hard with a melting point over 3,700 degrees Celsius. It cannot conduct electricity as all outer electrons are in covalent bonds.
- Silicon dioxide, made of silicon and oxygen covalently bonded, also has a high melting and boiling point due to its numerous strong covalent bonds, requiring substantial energy to break them for melting.
