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Unformatted text preview: 1s electron. 2p-orbital: When n = 2 , we have 2 possible values for . The first is = 0, or 2s orbital, which we just discussed above. The second possibility is = 1 or the 2 p orbital. For a given value of there are 2 + 1 possible m l values. So for = 1, we have m = -1, 0, +1 . These three values of m correspond to three different p-orbitals. P-orbitals look like dumbbells along each axis. Instead of a radial node, we have an angular node, which lies along the plane perpendicular to the axis in which the orbital lies. Since the energy, E , of each orbital is a function of only n , then all the n = 2 orbitals ( 2s , 2p x , 2p y , 2p z ) have the same energy. n = 3 orbitals: For the n=3 orbitals the possible quantum numbers are: n=3 =0 m =0 3s orbital n=3 =1 m =-1, 0, +1 3p orbitals n=3 =2 m =-2, -1, 0, +1, +2 3d orbitals...
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This note was uploaded on 10/13/2011 for the course CHEMISTRY 121 taught by Professor Staff during the Fall '10 term at Bangladesh University of Eng and Tech.
- Fall '10