OCR UNIT 1: ELECTRONS, BONDING AND STRUCTURE all included

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1. What are three characteristics that ionic compounds have (when in a giant ionic structure)?

  • high boiling point, always conducts electricity and cannot dissolve in water
  • dissolve in water, low boiling point, can not conduct electricity
  • conduct electricity when molten or dissolved, have high boiling points, dissolve in water
  • always conducts electricity, low boiling point, cannot dissolve in water
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2. 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
  • 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
  • They make the bonding between atoms weaker

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

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

4. What is a covalent bond?

  • the electrostatic attraction between ions with the same charge
  • a shared pair of electrons
  • 1 shared electron
  • the electrostatic attraction between two oppositely charged ions

5. What is ionic bonding?

  • an electrostatic attraction between two oppositely charged ions
  • an electrostatic attraction between two ions with the same charge
  • the intermolecular forces between induced dipoles
  • the intermolecular forces caused by an electronegative N,F,O, a lone pair and a hydrogen

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