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Electrons in Atoms III. Quantum Model of the Atom Quantum Numbers Four Quantum Numbers: Specify the “address” of each electron in an atom UPPER LEVEL Quantum Numbers 1. Principal Quantum Number ( n ) • Energy level • Relative Size of the orbital • n = # of sublevels in that energy level • n2 = # of orbitals in the energy level • 2n2 = total # of electrons in that energy level Quantum Numbers 2. Angular Momentum Quantum # ( l ) • Is equal to… (n-1) •Energy sublevel •Shape of the orbital s p d f Quantum Numbers 3. Magnetic Quantum Number ( ml ) Orientation of orbital can be (–l to +l) Specifies the exact orbital within each sublevel Quantum Numbers px py pz Quantum Numbers n = # of sublevels per energy level n2 = # of orbitals per energy level Orbitals per sublevel: 1 s, 3 p, 5 d, 7 f Quantum Numbers Orbitals combine to form a spherical shape. 2px 2py 2s 2pz Quantum Numbers 4. Spin Quantum Number ( ms ) Electron spin +½ or -½ An orbital can hold 2 electrons that spin in opposite directions. Quantum Numbers No two electrons in an atom can have the same 4 quantum numbers. Each e- has a unique “address”: 1. Principal # 2. Ang. Mom. # 3. Magnetic # 4. Spin # energy level sublevel (s,p,d,f) orbital electron Questions If n = 3, what l values are available? If n = 2, how many orbital's are possible? If 32 electrons fit into a energy level, what is the lowest possible energy level? If l = 2, what sublevel is the electron in, and how many orbital's are present? 0, 1, 2 4 4 d, 5 orbital's in that sublevel