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C3: Ionic bonding, metallic bonding and structure

Quiz by Oxford Revise Chemistry

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19 questions
Show answers
  • Q1
    What is an ion?
    atom/molecule that has gained or lost neutrons
    atom/molecule that has lost or gained electrons
    atom/molecule that shares electrons with another atom
    atom/molecule that has gained or lost protons
    60s
  • Q2
    Which kinds of elements can form ionic bonds?
    metals and elements
    metals and non-metals
    metals and metals
    non-metals and non-metals
    60s
  • Q3
    60s
  • Q4
    60s
  • Q5
    60s
  • Q6
    What is the force that holds oppositely charged ions together?
    electrostatic force of attraction
    electromagnetic force
    gravitational force
    magnetic force
    60s
  • Q7
    What is the name of a regular structure of alternating positive and negative ions, held together by the electrostatic force of attraction?
    giant covalent structure
    simple covalent
    simple ionic molecule
    giant ionic lattice
    60s
  • Q8
    Why do ionic substances have high melting points?
    electrostatic force of attraction between positive and negative ions is strong and requires lots of energy to break
    the ions in an ionic lattice are very closely packed together so require a lot of energy to pull them apart
    the electrostatic attraction between negative electrons is very strong and so requires a lot of energy melt them
    electrostatic force between positive neutrons and negative ions is strong and requires lots of energy to break
    60s
  • Q9
    Why don't ionic substances conduct electricity when solid?
    they contain non-metal elements which cannot conduct
    ions are fixed in position so cannot move, and there are no delocalised electrons
    ionic crystals cannot slide over each other and carry charge
    ions are not charged
    60s
  • Q10
    When can ionic substances conduct electricity?
    when frozen
    when melted or dissolved
    when evaporated
    when condensed
    60s
  • Q11
    Why do ionic substances conduct electricity when melted or dissolved?
    ions are free to move and carry charge
    there are delocalised electrons which can move and carry the charge
    electrons are free to slide over each other
    the non-metal ions become metals
    60s
  • Q12
    Which of these correctly describes the structure of a pure metal?
    layers of positive metal ions surrounded by free negative ions
    layers of metal atoms surrounded by delocalised electrons
    layers of positive metal ions surrounded by delocalised electrons
    layers of non metal atoms surrounded by delocalised electrons
    60s
  • Q13
    Describe the bonding in a pure metal.
    strong electrostatic forces of attraction between metal atoms and delocalised electrons
    strong magnetic forces of attraction between metal ions and delocalised electrons
    strong electrostatic forces of attraction between metal ions and delocalised electrons
    strong gravitational forces of attraction between metal ions and delocalised electrons
    60s
  • Q14
    Which one of these is NOT a property of a pure metal?
    malleable
    brittle
    high melting/boiling points
    good conductors of electricity
    60s
  • Q15
    Why are pure metals malleable?
    the lattice of positive ions can change shape without having to move the layers
    layers of positive ions can slide over each other easily
    layers of negative ions can easily slide over each other
    delocalised electrons make the metal malleable
    60s

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