Hie-Joon Kim. Seoul National University. Experience. Representative Publications
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1 Hie-Joon Kim Professor Emeritus Seoul National University B.S. Chemistry, Seoul National University, Korea, 1970 Ph.D. Chemistry, University of Chicago, USA, 1977 Experience Professor, Department of Chemistry Seoul National University ( ) Chair Professor, Gw angju Institute of Science and Technology (2013-Present ) SNU Teaching Award (2007) Representative Publications Philosophical Questions Scientific Answ ers (Thinking Power Books, 2012) Chemistry of Life, Chemistry for Life (Free Academy, 2009)
2 Chapter 1 Bohr Model
3 INTRODUCTION The Bohr Model of Hydrogen: A Paradigm for the Structure of Atoms Excerpt s from Hydrogen by Rigden Niels Bohr ( )
4 1-1 Thomson s Electron When Niels Bohr received his doctorate in 1911, the world of physics was pregnant with potential. One of those whose discoveries prepared the field for Bohr and others was J.J. Thomson ( ), who in 1884, at the age of twenty- eight, became Cavendish Professor of Experimental Physics at the University of Cambridge, following in the steps of James Clerk Maxwell ( ) and Lord Rayleigh ( ). dia.org/wikipedia/com mons/5/57/james_cle rk_m axw ell.png media.org/w ikipedi a/commons/5/54/st rutt.jpg kimedia.org/wikip edia/ commons/th umb/c/c1/j.j_tho mson.jpg/205px- J.J_Thomson.jpg
5 1-1 Thomson s Electron With Thomson s discovery of the negatively charged electron, Prout s idea that atoms were built up from some common entity took on a new significance. William Prout For Prout, the common entity was hydrogen; in the years immediately following 1897, the common entity became the electron. mmons/thumb/5/52/prout_william_painti ng.jpg/220px-prout_william_painting.jpg
6 1-1 Thomson s Electron In 1903 J.J. Thomson asserted that hydrogen contains about a thousand electrons. In 1906, Thomson made perhaps his greatest contribution to the pursuit of an atomic model. H With several lines of reasoning, Thomson concluded that the number of electrons in an atom was approximately equal to an atom s atomic weight. On this basis, there would be only one electron in a hydrogen atom.
7 1-2 Rutherford s Nucleus Rutherford liked alpha particles. After all, he had discovered them in In 1908 he established that the alpha particle carried a double positive charge. kimedia.org/wiki pedia/commons/ d/ de/ernest_ruth erford_1908.jpg dia.org/wikipedia/com mons/thumb/7/79/alp ha_decay.svg/1280px- Alpha_Decay.svg.png
8 1-2 Rutherford s Nucleus Rutherford and his assistant Hans Geiger directed a well- defined beam of alpha particles at thin foils of aluminum and gold. Most of the alpha particles passed straight through the foil, but some of them were scattered through a small angle, especially from the foils composed of gold atoms.
9 1-2 Rutherford s Nucleus Rutherford made a suggestion to Ernest Marsden, an undergraduate who was helping Geiger. Rutherford s suggestion went something like this: Why don t you see if some alpha particles are scattered at large angles? w.chemistryexplained.com/images/ chfa_04_img0818.jpg In March 1911, this new model of the atom was conveyed to the community of science. Later, in October 1912, Rutherford used the term nucleus for the first time.
10 1-3 Bohr s Atom More than any other person, more than any other physicist, Bohr was the guiding spirit of the quantum revolution. Bohr s contribution to twentiethcentury physics is acknowledged by most physicists as second only to Albert Einstein s. w/wp-content/uploads /2015/04/EMC2- Facebook-Cover.jpg Einstein 1921 Nobel Physics Prize Bohr 1922 Nobel Physics Prize abe0fc6-26cdb33025b4deaf9c0 a6e9a3953d227.r43.cf 2.rackcdn.com/26C342 D0-389E-45CF-B45A- FF88C2995CDD.jpg
11 1-3 Bohr s Atom Following Rutherford, Bohr depicted the hydrogen atom to be a positively charged nucleus of very small dimensions and an electron describing closed orbits around it. Bohr used the term stationary orbits in which, he asserted, there is no energy radiation, thereby violating the established tenets of nineteenthcentury electromagnetism.
12 1-3 Bohr s Atom Bohr placed a quantum condition on the energy; namely, he asserted that only certain energies are permitted. Elect ron The larger the energy state of the hydrogen atom, the bigger the orbit. Proton 1 2 3
13 1-3 Bohr s Atom From his model, Bohr was able to calculate the radii of the various orbits and thus, from the radius of the smallest orbit, he could calculate the diameter of the hydrogen atom and hence, its size meters The dimension of the hydrogen atom, as Bohr calculated from his model, was 1.1 A (1.1 x 10-8 cm).
14 1-4 Hydrogen Line Spectrum Bohr brought one more basic idea to his treatment of the hydrogen atom, an amazing and a portentous idea: he proposed a mechanism to account for the spectrum of an atom Balmer pload.wi kimedia. org/wiki pedia/ co mmons/ 5/51/Bal mer.jpeg ν 3 = (1/2 2 1/3 2 ) s -1 ν 4 = (1/2 2 1/4 2 ) s -1 ν 5 = (1/2 2 1/5 2 ) s -1 ν 6 = (1/2 2 1/6 2 ) s -1
15 1-4 Hydrogen Line Spectrum In keeping with the 1900 work of Max Planck, Bohr expressed the energy difference between two of his allowed states in the hydrogen atom in terms of Planck s constant and the frequency of light. reew ebs.com /kienitz/imag es/planck.jpg n = 3 n = 2 n = 1 +Ze E = hf Max Planck 1918 Nobel Physics Prize E 3 E 2 = hf
16 1-4 Hydrogen Line Spectrum Bohr wrote an explicit expression for the specific energies of the allowed states of the hydrogen atom, where m = mass of the electron, e = the electric charge of the electron, h = Planck s constant, and n = an integer. At some point during this process, Balmer s formula came to Bohr s attention, and it became immediately clear. The clue for Bohr may well have been the appearance of n 2 in the denominators of both Balmer s formula and his expression. E n = 2π 2 me 4 /n 2 h 2 11 λλ = RR EE = ZZ22 mmmm hh 22 ε nn 22 = nn 22 eeee
17 1-5 Quantum Revolution After Bohr s model, his reputation grew to enormous proportions not so much as the consequence of the papers he wrote, but as a consequence of the influence he exerted on others. In , quantum mechanics, a new physics that brought understanding to the world of the atom, was created. In that great period of physics, wrote Victor Weisskopf, Bohr and his men touched the nerve of the universe. pload.wi kimedia. org/wiki pedia/ co mmons/ f/f4/heis enberg, Werner_ 1926.jp eg upload. wikime dia.org /wikipe dia/ co mmons /4/43/P auli.jpg ad.wikimedi a.org/wikip edia/ comm ons/thumb/ c/ cf/dirac_4.jpg/162px- Dirac_4.jpg m/ learningabroad/assets_c/20 13/05/IMG_3469[1]-thumb- 480x jpg g/wikipedia/commons/1/1a/ Heisenbergbohr.jpg
18 1-5 Quantum Revolution nuclear model ~ 400 BC line spectrum 1859 quantum theory Bohr model 1913 wave mechanics atomic physics quantum chemistry 1939 chemical bonding octet rule
19 Review Helium is doing well With two electrons in the first shell. After fluorine comes neon And after chlorine comes argon With eight electrons in the second shell. The rule is called octet Though for helium it is duet.
20 Life in The Universe THANK YOU
Hie-Joon Kim. Professor Emeritus Seoul National University. Experience. Representative Publications
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