This preview has intentionally blurred sections. Sign up to view the full version.
View Full DocumentThis preview has intentionally blurred sections. Sign up to view the full version.
View Full Document
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 ....
View
Full Document
 Winter '08
 FOUCHER
 Atomic orbital, Electron Orbital Shapes, Mark Winter

Click to edit the document details