CHEM 101 1nd Edition Lecture 26Outline of Last Lecture I. Quantum MechanicsII. Quantum NumbersOutline of Current Lecture I. Quantum MechanicsII. Quantum NumbersIII. Common Misconceptions about Orbital ShapesIV. Types of Atomic OrbitalsCurrent LectureI. Quantum Mechanicsa. Determined Wave Equationi. Defines energy of an electron in terms of wavesii. Composed of wave functions, trident1. Have radial and angular partsb. Consequences of Schrodinger’s Equation1. Only certain eve functions are allowed (quantization)2. Quantum numbers describe approximate location of e-II. Quantum Numbersa. Wave functions, or orbitals, describe the region of space where an electron can be found and are described by three quantum numbers n, l, mlb. Principle Quantum Number, ni. Defines energy level and size of the orbitalii. n - 1,2,3,..iii. Increasing n = higher E, larger orbitalc. Angular Momentum (Azimuthal) Quantum Number, li. Defines the shape of the orbitalii. l = 0,1,2; l = 0 s, l = 1 p, l = 2 dd. Magnetic Quantum Number mli. Defines the orientation of the orbitalii. ml = -l,…, -1, 0, 1,…, lIII. Common Misconceptions about Orbital Shapesa. Not an impenetrable surface in which the electron is "contained"b. Probability of finding the election is no the same throughout the volume 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.enclosed by the surfacec. Terms “electron cloud” and “electron distribution” imply that the election is a particle but the basic premise in quantum mechanics is that the electron is treated as a wave, not a particle.IV. Types of Atomic Orbitalsa. s Orbitalsi. Spherical in Shape1. No planar nodesa. No places e- can’t be2. Size of orbital increases, as n increasesii. l = 0iii. 1s1. Quantum Numbersa. n = 1b. l = 0c. ml = 0iv. 2s1. 3 points with a probability of 0a. Nucleusb. Outside Boundaryc. Inner Ring were 1s Orbital Ends2. Quantum Numbersa. n = 2b. l = 0c. ml = 0v. 3s1. 4 points with a probability of 0a. Nucleusb. Outside Boundaryc. 2 Inner Rings where 1s and 2s Orbitals Ends2. Quantum Numbers a. n = 3b. l = 0c. ml = 0b. p Orbitalsi. “Dumbbell” Shape1. 1 planar nodea. Node = plane formed by y axis and z axisb. px is along the x axis2. Size of orbital increases as n increaseii. l = 1iii. The 3 p orbitals lie 90 degrees apart in spaceiv. 2px Orbital1. Quantum Numbersa. n = 2b. l = 1c. ml = -1, 0, +1v. 3px Orbital1. 2 distances from the nucleus that have a probability of 0a. Nucleusb. Outside Boundaryc. Boundary between second and third energy level2. Quantum Numbersa. n = 3b. l = 1c. ml = -1, 0, +1c. d Orbitalsi. Double “Dumbbell” Shape or “Dumbbell/Donut” Shape1. 2 planar nodes thru nucleusii. l = 2iii. There are 5 d Orbitalsiv. Quantum Numbers1. n = 32. l = 23. ml = -2, -1, 0, 1, 2v. 3dxy Orbital1. Nodesa. x axis and z axisb. y axis and z axis2. Between the x and y axesvi. 3dxz Orbital1. Nodesa. x and yb. z and y2. Dumbbells in the space between the x and the z axesvii. 3dyz Orbital1. Nodesa. y and x axesb. z and z axes2. In the space between the intersection of y and z axeviii. 3dx2- y2 Orbital1. Centered on the x and y axesix. 3dz2 Orbital1. Dumbbell Donuta. Dumbbell is along the z axisb. The Donut goes around the x-y planed. f Orbitalsi. Triple “dumbbell” shape1. 3 planar nodesii. l = 3iii. There are 7 f orbitalsiv. Quantum Numbers1. n = 42. l = 33. ml = -3, -2, -1, 0, 1, 2,