Bohr’s Successes and failures: The wave nature of the electron The Photon and Quantum • Read 192-194 (up to “The significance. ..”) • Introduced to the concept of the photon • light is still traveling as a wave, but not as an unlimited one Like this Not this • The energy of a photon is: E = hv • I.e. energy is dependent upon frequency • Pg. 219 - 220, Q. 6.12, 6.19, 6.21, 6.23 Explaining the line spectrum • Read remainder of pg. 194 • The jumps between orbitals have different energies (like jumping between different steps on a staircase) • Energy dictates frequency (E = h ν ) • frequency dictates type of EM radiation, or type of colour • Conclusion: the different lines of the spectra are explained by the different energies between orbitals The Bohr model of the atom • Recall that Bohr added to Rutherford’s model the idea of fixed shells • Evidence for Bohr’s Theory came from the existence of line spectra • However, Bohr had difficulty explaining other observations
This is the end of the preview. Sign up
access the rest of the document.
This note was uploaded on 04/12/2011 for the course CHEM 1010 taught by Professor Marshall during the Spring '11 term at North Texas.