CH-1010 Chapter Notes - Chapter 3: Rydberg Constant, Stationary Point, Ionic Radius

41 views14 pages

lavenderantelope86

1 Sep 2016

School

Department

Course

Professor

For unlimited access to Textbook Notes, a Class+ subscription is required.

Document Summary

In addition to giving us powerful insights into the composition and behavior of atoms, quantum theory has forever altered our sense of what we can really know about the word around us. According to quantum theory, our world at the atomic level is governed by rules that are different from those that apply to the macroscopic world. Distribution patterns of electrons provide a theoretical framework that explains the properties of the elements, including their tendencies to form ions with characteristic positive or negative charges, and their interactions to form compounds. Classical physics predicts that negatively charged electrons orbiting a positively charged nucleus should lose energy and eventually spiral into it. To understand the stability of atoms, we need to study how atoms interact with a form of energy called radiant energy or electromagnetic radiation that make up the electromagnetic spectrum. Some forms have much more energy than visible light.

Related Questions

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

CH-1010 Chapter Notes - Chapter 3: Rydberg Constant, Stationary Point, Ionic Radius

Document Summary

Get access

Related Documents

CH-1010 Chapter Notes - Chapter 3: Joseph Von Fraunhofer, Johann Jakob Balmer, Fraunhofer Lines

CH-1010 Chapter Notes - Chapter 3: Uncertainty Principle, Electromagnetic Spectrum, Fraunhofer Lines

CH-1010 Lecture Notes - Lecture 5: William Hyde Wollaston, Electromagnetic Spectrum, Electric Field

Related Questions