Chem 121 1st Edition Lecture 8Outline of Last Lecture I. The Nature of MatterII. Atomic Spectrum of HydrogenIII. The Bohr Model of HydrogenIV. The Wave Nature of MatterV. Quantum Mechanics and the AtomVI. Atomic OrbitalsVII. Quantum OrbitalsOutline of Current Lecture II. Quantum NumbersIII. Orbital ShapesCurrent LectureQuantum Numbers- To describe an orbital it needs 3 sets of quantum numbers. - How many shapes are allowed is determined by n.- Shape of orbital is determined by l.- Bohr Model helps to link orbital with energy level- Why is 1p not on the table? Because it is not allowed based on the rule. If n=1, n≠1Orbital Shapes- S orbitals (l=0) o Shape: sphereo Spherical node- region where zero probability in finding e-o Tunneling effect (Penetration effect): e- found in region closer to nucleus- P orbitals (l=1)o Shape: Dumb-bell e- spend time in both lobeso Orientation: lies along the axeso Nodal Plane: perpendicular orientation axis, zero probability in finding e-o n required: n greater than or equal to 2o 3 orbitals (2l+1)- D orbitals (l=2)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.o Shape: four-leaf clover (except dz2) o Orientation: lies in planeso 2 Nodal planes (except dz2) o n required: n is greater than or equal to 3o 5 orbitals (2l+1)- F orbitals (l=3)o Shape: 8 lobeso 3 nodal planeso n required: n is greater than or equal to 4o 7 orbitals (2l+1) The more nodal planes, the more the lobes, the more restrained the e- in space, the less space it occupies, the more energetic the orbital The larger the n the farther electrons are from the
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