CHEM103 Lecture 2: Unit1 pages 12-37 Sep 6

• School: University of Alberta
• Department: Chemistry
• Course: CHEM103
• Professor: Mariusz Klobukowski

Document Summary

The bohr model of the h atom (1913) Bohr used (a) rutherford nuclear model (b) classical orbits (c) planck"s quanta. [according to classical electrodynamics they would radiate energy] 2 some orbits are special no emission of radiation (stationary orbits) 3 an electron can jump from one stationary orbit to another emitting/absorbing radiation; the energy difference is proportional to frequency of radiation. 1-13: n = 1, 2, a quantum number, radius of the orbit is proportional to n2 r n. 2 rn = a0 n2 a0= 0. 529 . = 52. 9 10 12 m = 52. 9 pm (bohr radius: energy of an electron on an orbit is proportional to 1/n2. 1-14: ground state: lowest energy, n = 1, excited state, any n > 1: absorption of energy needed for the electron jump n = 1 n > 1, energy change during excitation: 2 n: most negative: n = 1. Visualization of bohr(cid:2)s model of the h atom [fig.