Electronic Structure

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Orbitals:

(http://www.google.co.uk/imgres?q=orbital+diagrams&um=1&hl=en&sa=N&rlz=1C1AFAB_enGB463GB463&biw=1366&bih=643&tbm=isch&tbnid=1zKh-g8udAwM6M:&imgrefurl=http://chemistry11-genius.blogspot.com/2011/05/electronic-structure-of-atom.html&docid=ekbHLS5nGhuIFM&imgurl=http://4.bp.blogspot.com/-fjQAZidF9Kc/Tb9KIl_jaOI/AAAAAAAAADs/-jdC7QhF7QM/s1600/ch9orbitals1.jpg&w=576&h=388&ei=MNKjUM-8OIa00QXHtYDwBw&zoom=1&iact=hc&vpx=944&vpy=165&dur=307&hovh=184&hovw=274&tx=113&ty=107&sig=106407783890754899411&page=1&tbnh=156&tbnw=239&start=0&ndsp=18&ved=1t:429,r:4,s:0,i:81)

  • All orbitals have space for 2 electrons
  • There is one s orbital on every shell (holding 2 electrons in the s subshell)
  • There are 3 p orbitals in every shell from the 2nd shell upward (holding 6 electrons in the p ubshell)
  • There are 5 d orbitals on every shell from the 3rd shell upward (holding 10 electrons in the d subshell)

Electrons do not like to be paired in an orbital and will go into a free one if available

If forced to pair, the electrons spin in opposite directin (up, down)

Sub shell notation is done like this:

1) The shell number (e.g 1)

2) The sub shell (e.g s)

3) The number of electrons in that subshell (e.g

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