![Wave Mechanics ,[object Object],[object Object],[object Object],[object Object],L. de Broglie (1892-1987) for particles is called the de Broglie wavelength From previous lecture we know that, Light as well as heat energy exhibits both wave and particle nature under suitable conditions = Wave mechanical theory Therefore, mc = h / and for particles (mass)x(velocity) = h / ](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
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Lecture 7
- 1. Electronic configuration of Atom Lecture 7 Week 4
- 6. ORBITAL 2 is proportional to the probability of finding an e- at a given point. The three dimensional region within which there is higher probability that an e having certain energy will be found is called ORBITAL, The energy of e in an orbital is always same
- 8. Those are principal ( n ) , angular ( l ) , and magnetic ( m ) quantum numbers n l m principal 1, 2, 3, … size and energy angular momentum 0, 1, 2, …, ( n - 1) shape magnetic - l , …, l orientation
- 10. n = 1 l = 0 = (1s) n = 2 l = 0, 1 = (2s, 2p) n = 3 l = 0, 1, 2 = (3s, 3p, 3d) n = 4 l = 0, 1, 2, 3 = (4s, 4p, 4d, 4f) designated by letters l = 0 s orbital l = 1 p orbital l = 2 d orbital l = 3 f orbital Angular momentum quantum number ( l ) It is an integer from 0 to (n-1) It is related to the shape of the orbital
- 11. n = 1 l = 0 m = 0 n = 2 l = 0 m = 0 l = 1 m = -1 m = 0 m = 1 n = 3 l = 0 m = 0 l = 2 l = 1 m = -1 m = 0 m = 1 m = -2 m = -1 m = 0 m = 1 m = 2 s s p s p d 1 1 3 3 1 5 Magnetic quantum number ( l ) It is an integer from –l through 0 to +l It is prescribes the orientation of the orbital in space around nucleus
- 14. 1 s orbital spherical Shape of Atomic Orbital See Fig-7.17 of Silberg Chemistry Page 278
- 15. Shape of 2p Orbital dumbbell shape 3 p , 4 p , 5 p etc. are similar shapes but larger size
- 16. n = 3, l = 1 Orbitals (3p x 3p y 3p z )
- 17. 3 d orbitals cloverleaf larger n same shapes but size larger
- 18. Representation of 4f Orbitals
- 19. There are n 2 orbitals in the n th SHELL Also see Fig - 7.17 & Fig - 7.18 & Fig – 7.19 and Fig - 8.9of your reference Silberg Chemistry Book 2 1 3d n= 3
- 24. Electronic configuration No of e in sub shell Electronic configuration of shell 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 4f 14 2 10 6 14 10 2 2 6 6 2
- 27. The relation between orbital filling and the periodic table
- 29. Electron configurations in the first three periods.
- 30. Orbital occupancy for the first 10 elements, H through Ne.
- 31. Hund’s rule
- 34. A periodic table of partial ground-state electron configurations