Chemistry OCR 1.2.4 Electrons and the Periodic Table

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1. Using the structured blocks, you can work out the electronic configurationof any element using the Periodic Table. Oxygen is the 4th element in the 2p-block. What would be its electonic configuration?

  • (^ indicates subscript) 1s^2 2s^2 2p^4
  • 1s^2 2s^2 2p^6
  • 1s^2 2s^2 2p^3
  • 1s^2 1s^2 2p^4
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2. What would be the electronic configuration of an iron Fe, atom and an iron 2+ ion, Fe2+?

  • Atom: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6 Fe2+ ion: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^6
  • Atom: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6 Fe2+ ion: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^4
  • the electronic configuration of an iron atom would be the same as that of an iron 2+ ion

3. When negative ions are formed, what happens to the electrons in the highest energy orbitals?

  • the number of electrons is doubled
  • electrons are added
  • the number of electrons stays the same
  • electrons are removed

4. The Periodic Table is structured in blocks of 2,6,10 and 14 elements, linked to....

  • shells
  • atoms
  • sub-shells
  • orbitals

5. How can the electronic configuration be abbreviated?

  • to show the last half of its electronic configuration
  • to show just the outer shell of the element
  • it can not be abbreviated
  • to show just the inner shell of the element

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