CHM-1045 Lecture Notes - Lecture 11: Photon, Quantum Number, Bohr Model

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ultramarinefrog201

20 Nov 2017

School

FSU

Department

Chemistry and Biochemistry

Course

CHM-1045

Professor

Cameroun Robert

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Document Summary

Chm 1045- lecture 11- electromagnetic spectrum and electron configuration. Wave periodic movement that transport energy from one point in space to another. Equation: c= c is the speed of light= 3. 0 e8m/s. Wavelength : wavelength is the distance between two consecutive peaks or troughs in a wave. Frequency : is the number of wave cycles that pass a specified point in. space in a specified amount of time. Amplitude: the magnitude of the wave"s displacement. related to the intensity of the wave, which for light is the brightness, and for sound is the loudness. Quantization: in which only discrete values from a more general set of continuous values of some property are observed. A blackbody: is a convenient, ideal emitter that approximates the behavior of many materials when heated. Equation: e(energy)= hv(frequency) h is plank constants= 6. 626e-34 joule second. Wave-particle duality: at a deep fundamental level still not fully understood, light is both wavelike and particle-like.

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LIGHT LAB SPRING 2018 CHEM 1430 Ill. Quantization of Electromagnetic Radiation In 1894, the German physidist, Max Plank, was working for a utility company to maximize visible light output from incandescent lamps using minimum power. Based on theoretical considerations, Planck postulated that electromagnetic energy could only be emitted at discrete values, rather than the continuum of predicted by classical physics, as multiples of the frequency of the radiation. Planck's Postulate took the mathematical form: EÂ·hv where the energy emitted, in Joules, is the product of a constant, h, known as Planck's Constant, and the frequency of the radiation, v. Planck's Postulate was experimentally verified and h found to have the value of 6.626 x 1034 Js(Joule seconds). The idea that electromagnetic radiation energy had specific frequency dependent energy was termed a "quantum of action," a distressing finding for the dlassically trained Planck. Despite his objections, Planck adopted this quantization of energy as a last resort to reconcile experiment with theory. This discovery set the stage for the early understanding of atomic structure, led to the term "photon" to describe the packet of energy carried by light waves, led to an understanding of the photoelectric effect, eventually leading to the development of general quantum theory Planck's Relationship, in combination with the tight equation, c the energy of a photon from frequency or wavelength. Î» w, allow expressions to be written to calculate ACTIVITY 4: QUANTIZATION OF THE ENERGY OF RADIATION To practice cakculations with Planck's Relationship, complete the following table, showing work with units in the right mest column, Convert given frequency to energy or given wavelength to energy. Take the value for Planck's Constant, h, to be 6.626 x 10"Js, show a calculation string include dimensions, reporting the final value to the proper number of significant figures Spectral Region Wavelength Frequency Energy in J/photon Show Calculation String Î» in meters v in s or cps X-ray 6.0 x 10"m Blue light 4.5 x 10m Infrared 4.1 x 10" cps Microwave 7.3 x 101 cps Radio Wave 3.0x 10 m IV. Bohr's Quantum Model for the Hydrogen Atom Ernest Rutherford's Gold Foil Experiment of 1911 demonstrated the nuclear structure of the atom. Questions remained as to how electrons were arranged in the atom. The most common belief called for the negatively charged the late 19h century recognized a particle (an electron) traveling around a body (the positively charged nucleus) would continuously radiate energy, slowing over time, eventually falling into the nucleus. Matter would collapse. Page 8 of 12

CHM-1045 Lecture Notes - Lecture 11: Photon, Quantum Number, Bohr Model

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