OCR UNIT 1: ELECTRONS, BONDING AND STRUCTURE all included

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  • Created by: carys ☺
  • Created on: 14-05-13 15:16

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

  • They make the bonding between atoms weaker
  • Because the shared pair of electrons create a strong intermolecular force
  • 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
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2. What are three characteristics that ionic compounds have (when in a giant ionic structure)?

  • always conducts electricity, low boiling point, cannot dissolve in water
  • conduct electricity when molten or dissolved, have high boiling points, dissolve in water
  • dissolve in water, low boiling point, can not conduct electricity
  • high boiling point, always conducts electricity and cannot dissolve in water

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

  • 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.
  • a high attraction between the electron and the nucleus
  • the ability to remove all the electrons from the outer shell in an exothermic process

4. What charge does the Sulfate SO4 ion carry?

  • 2-
  • 4-
  • 4+
  • 2+

5. What is a covalent bond?

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

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