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Chapter 6 Study Guide

by: Sairal

Chapter 6 Study Guide Chem 113

Marketplace > Arizona State University > Chemistry > Chem 113 > Chapter 6 Study Guide
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This notes cover chapter 6 of Chemistry, the Central Science.
CHM 113
Study Guide
Chemistry, notes, Study Guide
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This 2 page Study Guide was uploaded by Sairal on Thursday March 31, 2016. The Study Guide belongs to Chem 113 at Arizona State University taught by Trovitch in Spring 2016. Since its upload, it has received 63 views. For similar materials see CHM 113 in Chemistry at Arizona State University.


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Date Created: 03/31/16
● Wavelength and Frequencies of Light  ○ Electronic stru describes the arrangement and energies of electrons around  the atom  ○ Electromagnetic radi​(aka radiation energy ­ Ex. visible light) moves through  a vacuum at the speed of c=2.99 x 1 m/s  ■ EM radiation has electric and magnetic components that vary in a  wavelength fashion periodically  ■ These waves allow it to be described i​ avelengt​nd  frequenc­ these two are interrelated  ● Quantized Energy and Photons  ○ Planck proposed that the minimum amount of radiant energy that an object can  gain or lose is related to the frequency of E=hv adiation: ​ ○ This smallest unit is c​uantumof energy  ○ Planck’s Const is described​ and is 6.626 x 10​ J­s  ○ Energy is quantized, meaning it can only have certain allowed values  ○ Photoelectric e ­ Einstein used quantum theory to explain this, which is the  emission of electrons from metal surfaces when exposed to light  ■ He proposed th​hoton​are quantized energy packets in light  ● Each photon carries ene​=hv E ● Bohr Model of the Hydrogen Atom  ○ Spectrum­ when light is dispersed into its component wavelengths it produces a  spectrum.  ○ Continuous spectr occurs when a spectrum contains all wavelengths  ○ Line spectr occurs when only certain wavelengths are present in a spectrum  ○ In the Bohr Model the energy of the electron in a hydrogen atom depends on the  value of the quantum num​,called t​rinciple quantum number  ■ The value ​​must be a positive integer  ■ Each value n​corresponds to a different specif​c energy, E n ■ Energy of the atom increasnincreases  ■ Ground sta​is the lowest energy at n=1 ­ othern arexcited  states  ■ Light is emitted when an electron drops in energy while light is absorbed  when an electron goes from a lower energy to a higher energy state  ■ The frequency of light emitted or absorbed i​​equals the  difference in energy between two allowed states  ● Wave Behavior of Matter  ○ De Brogl said matter should exhibit wave­light properties, a hypothesis of  matter wavewas proved to be experimentally by observing diffraction of  elements  ○ An object has a characteristic wavelength that de​omentum, mv:  wavelength = h/mv  ○ Discovery of wave properties of the electron led to​ncertainty s u principle  ○ There is a limit to the accuracy with which the position and momentum of particle  can be measured simultaneously. We we know one with better certainty, we  know the other with less.  ● Quantum Mechanics and Orbitals  ○ In the quantum mechanical model of the hydrogen atom behavior of the electron  is described by mathematical functiwave functions  ○ Each allowed wave function has precisely known energy, but the location of the  electron cannot be determined exactly, but there is a possibility that it will be in a  particular point in space which is given​robability density  ○ Electron densi distribution is a map of the probability of finding the electron at  all points in space  ○ Orbital ­ allowed wave functions of the hydrogen atom  ■ Described as a number and a letter which corresponds to values of three  quantum numbers  ■ Angular momentum quantum number,  , indicated b​, p, d and on  corresponding to the values of 0, 1, 2, 3  ● L defines the shape of the orbital  ● For a given value ​, can have integer values ranging from 0 to  (n­1).  ■ The magnetic quantum number, ml​ describes the orientation of the orbital  in space.  ● For a given value , ml​an have integral values ranging f om ­l​ to, including 0.  


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