Chemistry OCR 1.2.4 Electrons and the Periodic Table

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

  • the number of electrons stays the same
  • electrons are added
  • electrons are removed
  • the number of electrons is doubled
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2. 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

3. 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

4. What affect does the principal quantum number n, have on the energy level and distance of the shell from the nucleus?

  • the larger the value of the principal quantum number , the higher the energy level and the further the shell from the nucleus
  • the larger the value of the principal quantum number, the higher the energy level and the closer the shell is to the nucleus
  • the larger the value of the principal quantum, the lower the energy level and the closer the shell is to the nucleus
  • the principal quantum number has no affect on the energy level or distance of the shell from the nucleus

5. What is the relationship between the 4s sub-shell and the 3d sub-shell?

  • the 4s sub-shell has a lower energy level then the 3d sub-shell
  • the 4s sub-shell has equal energy level to the 3d sub-shell
  • the 3d sub-shell has a lower energy than the 4s sub-shell
  • they have no relationship

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