| Themes > Science > Chemistry > General Chemistry > Atomic Structure > Electronic Structures of Atoms > Atomic Structure Index > Electron capacity of shells, subshells and orbitals |
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An individual orbital is denoted by a distinct n,l and ml value. Two electrons can fit into each orbital: one with ms = +1/2 and the other -1/2. A sublevel is denoted by n and l, and has a set of orbitals denoted by ml For an l=0 (s) sublevel, there is only one possible ml value and thus only one orbital, ml = 0, so an l = 0 sublevel can hold only two electrons. An l = 1 (p) sublevel has three orbitals, one with ml = 1, one with ml = 0 and one with ml = -1. Each of these orbitals can hold two electrons each, so an l=1 (p) sublevel can hold 6 total electrons. For l=2 (d sublevel), there are five orbitals (ml = 2,1,0,-1,-2), each can hold two electrons, so the d sublevel can hold a total of 10 electrons. l=3 (f sublevel) has seven orbitals (ml = 3,2,1,0,-1,-2,-3) and so can hold a total of 14 electrons. A principle level can hold as many electrons as the sum of it's sublevels. For n=1, there is only one possible l value, l=0. An l=0 shell has 2 electrons, so the principle quantum level n=1 holds only two electrons. For n=2, there are two possible l values, l=0 and l=1. l=0 sublevels hold 2 electrons, l=1 hold 6, so the n=2 principle level can hold a total of 8 electrons. Example: A h orbital is a possible solution of the Schrodinger equation, although no ground state atom has electrons that reside in this sublevel. An h sublevel has l = 5. How many electrons can an h orbital hold? Solution: If a sublevel has l=5, then there are 11 distinct orbitals, with the ml values 5,4,3,2,1,0,-1,-2,-3,-4,-5. Each can hold two electrons, so a total of 22 electrons can fit in an h orbital. |
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