8CHM11509 full lecture - CHM 115 Dr. Hilkka Kenttmaa...

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Unformatted text preview: CHM 115 Dr. Hilkka Kenttmaa Lecture 8 Reading was: 8.6-8.7 The Structure of Atoms and Molecules Lecture 9: same Next lab: Determination of NaOH concentration Bohrs Planetary Model Bohrs model based on Bohr orbits of electrons explained the line spectrum of the H atom but not other atoms. This model also fails to explain various characteristics of atoms, including bonding and periodicity The Wave Behavior of Matter Knowing that light has particle nature, it seems reasonable to ask if matter has wave nature. This question was answered by Louis de Broglie. Using Einsteins and Plancks equations, de Broglie derived: mv h = E = h E = mc 2 = c / h = mc 2 h (c/ ) = mc 2 h / = mc mv h = c = speed of light; replace with speed of particle = v The momentum, mv , is a particle property, whereas is a wave property. Therefore, in one equation, de Broglie summarized the concepts of waves and particles: any moving particle has . However, in order to measure , mv must be very small because h is small. mv h = 6 Question # 1 Which of the following particles are most likely to show wave-like behavior? (a) carbon atoms (b) particles (c) protons (d) electrons (e) photons Erwin Schrdinger (1887-1961): comprehensive theory of the behavior of electrons in atoms Electron can be described as a wave (de Broglie)...
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This note was uploaded on 02/06/2012 for the course CHM 115 taught by Professor Towns during the Spring '08 term at Purdue University-West Lafayette.

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8CHM11509 full lecture - CHM 115 Dr. Hilkka Kenttmaa...

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