anonymous
  • anonymous
Which of the following quantum number combinations is not allowed in an atom? n = 2, l = 0, m subscript l = 0 n = 3, l = 2, m subscript l = -1 n = 6, l = 5, m subscript l = -4 n = 1, l = 0, m subscript l = 1
Chemistry
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chestercat
  • chestercat
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anonymous
  • anonymous
The last one my friend. m subscript l is comprised between +l and -l: if l is 0 m can only be 0
anonymous
  • anonymous
In fact the orbital l=0 is the energy sublivel 's', shaped like a sphere, (the level m subcript l indicate the orientation in space, and a sphere "l=0" can only have one orientation in 3d space)
Photon336
  • Photon336
n is the principle quantum number can be any whole integer; \[M _{L} \] = orientation. L = shape of your orbital \[s = \pm \frac{ 1 }{2 }\] this is our spin

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Photon336
  • Photon336
|dw:1441645957399:dw| our spin can either be up or down, and each orbital the box can hold a maximum of 2 electrons. if you have If I remember correctly \[m_{L} = \pm l\] so if you have l = 2 for instance m_{L} can take on any value from positive L to negative L.
Photon336
  • Photon336
a typical P orbital; starts at n = 2 say we have L = 1 Ml can be +1 -1 or 0 EACH orbital holds 2 electrons so if we have 3 possible orientations P_{x} P_{y} P_{z} which can hold a maximum of 2 electrons. A p orbital can hold 6 electrons. so 2 for each. the P_{x} y and z come from mL which can be less than or equal to L but not greater than L. Remember L gives us the shape of the orbital, while n tells us what energy level we're at. FYI the periodic table is organized based on energy levels. |dw:1441646127733:dw|

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