Chemistry: Carbon Bonding and Properties
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Questions and Answers

What affects the strength of an ionic bond in terms of melting and boiling points?

  • Color of the compound
  • Number of ions present
  • Atomic weight of the ions
  • Size and charge of the ions (correct)

    • Which pairing would likely have a higher melting point according to the text?

  • Group 3 / Group 5 (3+, 5-)
  • Group 4 / Group 8 (4+, 8-)
  • Group 1 / Group 7 (1+, 7-)
  • Group 2 / Group 6 (2-, 2+) (correct)

    • Why do solid-state ionic compounds not conduct electricity?

  • Because they lack ions
  • The ions are too large to conduct
  • Due to the absence of free-moving ions
  • The lattice structure prevents ion movement (correct)

    • In what state do ionic compounds conduct electricity?

    <p>Liquid state or solution</p> Signup and view all the answers

    Which macromolecular structure is known for its high melting point?

    <p>Diamond</p> Signup and view all the answers

    What property makes graphite a good conductor of electricity?

    <p>Free-moving electrons between layers</p> Signup and view all the answers

    Why are metals typically hard?

    <p>As a result of strong electrostatic attraction between metal cations and delocalised electrons</p> Signup and view all the answers

    What needs to happen for atoms in a giant covalent structure to move through a solvent?

    <p>Strong covalent bonds need to be broken</p> Signup and view all the answers

    What is the main reason for the high melting and boiling points of metals?

    <p>Strong electrostatic attraction between metal cations and delocalised electrons</p> Signup and view all the answers

    Why is graphite an exception when it comes to solubility?

    <p>It has spare electrons</p> Signup and view all the answers

    In a metallic structure, what are the particles of the 3-D lattice surrounded by?

    <p>'Sea' of delocalised electrons</p> Signup and view all the answers

    What type of bonding is responsible for electrical conductivity in metals?

    <p>Metallic bonding</p> Signup and view all the answers

    Why do giant covalent structures have high melting and boiling points?

    <p>The lattice particles are atoms with strong covalent bonds that need a lot of energy to break</p> Signup and view all the answers

    Why is graphite able to conduct electricity?

    <p>The remaining valence electron on each carbon atom is delocalized and can move freely within the sheet</p> Signup and view all the answers

    What contributes to the hardness of macromolecular (giant covalent) structures?

    <p>Rigid 3-D structure holding surface atoms in place</p> Signup and view all the answers

    Why are melting and boiling points of giant covalent structures much higher than simple covalent structures?

    <p>All strong covalent bonds holding the giant lattice need to be broken, requiring a lot of energy</p> Signup and view all the answers

    What makes graphite a good lubricant?

    <p>Weak forces between the sheets allow easy sliding</p> Signup and view all the answers

    Why are giant covalent crystals considered insulators?

    <p>There are no charged particles in the lattice, as they consist of atoms</p> Signup and view all the answers

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