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1. What is a covalent bond?

  • a shared pair of electrons
  • the electrostatic attraction between ions with the same charge
  • the electrostatic attraction between two oppositely charged ions
  • 1 shared electron
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2. What affects ionisation energy?

  • the shape and size of an atom
  • nuclear charge, distance from nucleus and sheilding
  • only nuclear charge
  • distance from the nucleus, shielding and intermolecular forces

3. What is the definition of the first ionisation energy?

  • a high attraction between the electron and the nucleus
  • the ability to remove all the electrons from the outer shell in an exothermic process
  • the energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms to form one mole of gaseous 1+ ions.
  • the energy needed to remove 1 electron from each ion in 1 mole of gaseous 1+ ions to form one mole of gaseous 2+ ions.

4. How do the delocalised electrons in metallic bonding effect the melting point?

  • They make the melting point lower because it stops the positive ions being attracted togther
  • They make the bonding between atoms weaker
  • The more electrons there are, the stronger the bonding will be and the higher the meling point because the positive metal ions will have more electrons to be attracted to
  • Because the shared pair of electrons create a strong intermolecular force

5. What is the equation for the second ionisation of oxygen?

  • O2- (g) -> O2+ (g) + H2O
  • O+ (g) -> O2+ (g) + e-
  • O2+ (g) -> O3+ (g) + e-
  • O+ (l) -> O2+ (g) + e- (s)


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