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. What are Van Der Waals Forces?

  • any intermolecular force
  • ionic attraction
  • electrostatic attraction between temporary dipoles and induced dipoles caused by movement of electrons in atoms and molecules.
  • shared pair of electrons

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

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

4. What is dative covalent bonding?

  • When there are more than 8 electrons in outer shell
  • When there are less than 8 electrons in outer shell
  • When both electrons come from one atom
  • When atoms share more than one pair of electron e.g. in N2

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

  • 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
  • They make the melting point lower because it stops the positive ions being attracted togther
  • Because the shared pair of electrons create a strong intermolecular force

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