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Unformatted text preview: 1s electron. 2porbital: When n = 2, we have 2 possible values for ℓ. The first is ℓ = 0, or 2s orbital, which we just discussed above. The second possibility is ℓ = 1 or the 2 p orbital. For a given value of ℓ there are 2 ℓ + 1 possible m l values. So for ℓ = 1, we have m ℓ = 1, 0, +1. These three values of m ℓ correspond to three different porbitals. Porbitals 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 ℓ=0 m ℓ =0 3s orbital n=3 ℓ=1 m ℓ =1, 0, +1 3p orbitals n=3 ℓ=2 m ℓ =2, 1, 0, +1, +2 3d orbitals For much nicer threedimensional renderings of all the atomic orbitals visit Mark Winter's Orbitron site ....
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This note was uploaded on 07/31/2008 for the course CHY 152 taught by Professor Foucher during the Winter '08 term at Ryerson.
 Winter '08
 FOUCHER

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