Chem 1320 1st Edition Lecture 18Outline of Last Lecture I. Newton II. Hydrogen AtomOutline of Current Lecture I. OrbitalsII. Quantum NumbersIII. Pauli Exclusion Principal IV. Aufban Principal V. Electron ConfigurationsCurrent LectureI. Orbitals S-orbitals: n, l=0, ml= 0P- orbitals: l=1, ml= -1,0,1D-orbitals: l=2, ml= -2,-1,0,1,2There are three different shapes of orbitals starting with the smallest (1s) medium (2s) and largest (3s). II. Quantum numbersQuantum numbers are an extra electron label. The Stem and Gerlach Experiment was on electron spin. m8= electron spin qn. The permitted values are ½ & -1/2. The significance accounts for electrons in atoms that interacts with magnetic fields. These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.III. Pauli Exclusion PrincipalThis principal explains the orbital occupation constraints. No two electrons can have the same four quantum numbers in an atom. A shell is all the electrons with the same principal qn. A subshell is all the electrons with the same n & l. An orbital is all the electrons with the same n, l, & ml. IV. The Aufban PrincipalThis principal is the order of filling orbitals to give the lowest energy configuration. This includes the ground state or ground electronic state. 1s2s 2p3s 3p 3d4s 4p 4d 4f5s 5p 5d 5f 5g6s 6p 6d 6f 6g 6h7s 7p 7d 7f 7g 7h…….8s 8p 8d 8f 8g 8h…….V. Electron ConfigurationsH: (Z=1) = 1s1 (core electron)He: (Z=2) = 1s2 (core electron)Li: (Z=3) = 1s22s1Be: (Z=4) = 1s22s2B: (Z=5) = 1s22s22p1C: (Z=6) = 1s22s22p2N: (Z=7) =1s22s22p3O: (Z=8) =1s22s22p4F: (Z=9) =1s22s22p5Ne: (Z=10) =1s22s22p6Na: (Z=11) =1s22s22p63s1TIP: to max the spin put the up arrow in each box first and then go back and put the down arrow. Hunds Rule states that the lowest energy state maximizes the
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