Chemistry OCR 1.2.4 Electrons and the Periodic Table

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1. According to the Aufbau principle when does the 4s sub-shell fill?

  • at the same time as the orbitals in the 3d sub-shell
  • before the orbitals in the 3d sub-shell
  • after the orbitals in the 3d sub-shell
  • it doesn't fill at all
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2. The Periodic Table is structured in blocks of 2,6,10 and 14 elements, linked to....

  • shells
  • sub-shells
  • orbitals
  • atoms

3. 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?

  • 1s^2 1s^2 2p^4
  • 1s^2 2s^2 2p^6
  • (^ indicates subscript) 1s^2 2s^2 2p^4
  • 1s^2 2s^2 2p^3

4. How can the electronic configuration be abbreviated?

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

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

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

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