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 due to the many strong covalent bonds, making them extremely hard materials that do not conduct electricity. Diamond, composed of carbon atoms with four other carbon atoms, has a melting point over 3,700 degrees Celsius, while silicon dioxide, made of silicon and oxygen, also requires significant energy to break its covalent bonds.

Insights

  • Giant covalent molecules such as diamond and silicon dioxide exhibit high melting and boiling points because of the multitude of strong covalent bonds they possess, demanding significant energy for bond breakage.
  • Diamond's exceptional hardness and high melting point of over 3,700 degrees Celsius stem from its structure of carbon atoms forming covalent bonds with four other carbon atoms, while silicon dioxide's similar properties are attributed to the strong covalent bonds between silicon and oxygen atoms within its structure.

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Recent questions

  • 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.
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