Light sources. Excited gas atoms are the primaty source of radiation in combustion and discharge lamps. lamps is not continuous!
|
|
- Joseph Harper
- 5 years ago
- Views:
Transcription
1 Light sources Excited gas atoms are the primaty source of radiation in combustion and discharge lamps. Continuous spectrum: black body radiation Characteristic spectrum: emission lines Absorption lines The spectrum of discharge lamps is not continuous!
2 Atom models: Thomson and Rutherford Thomson model raisins in a cake Rutherford experiment
3 The Rutherford model m m The mass and charge are concentrated in the core.
4 The Bohr model of hydrogen atom Problems of the Rutherford s model: - electron should fall on the core synchrotron radiaton - does not explain why atomic spectra are not continous
5 Bohr model of hydrogen atom Balmer the lines in hydrogen spectrum Rydberg R H = m 1 Lyman ultraviolet spectrum n=2,3,4... Paschen, Brackett, Pfund, Humphrey series - infrared n =1,2,3... n>n
6 Bohr model principles 1. Electron moves on circular orbit around the atom. The electron energy is constant it does not emit radiation. 2. The electron can stay on orbits, for which the orbital angular momentum is equal the multiplicity of h/2p 3. Emission and absorption occurs, when the electron jumps between allowed orbits. The frequency of the radiation is related to the energy: E = h L n n h 2 n- quantum number
7 Bohr model electron energy L m u n e r n 2 n m u e n Ze rn r n n h 2 E( n) E ( n) E ( n) E( n) p m e Z n 0 2 e k 4 1 n=1 the basic state n= ionized state The wavelength is related to the quantum numbers: m e e c 2 1 n 2 1 m 2 R 1 R m e M R H
8 Bohr model hydrogen spectrum
9 Gaseous spectra Helium Neon Argon Krypton Xenon Mercury Sodium
10 Discharge lamps 1. Emission of electrons from the electrode (called a cathode) 2. These electrons knock out the electrons from nobel gas atoms 3. Avalanche ionization of gas, conductivity increases. 4. Electrons or excited atoms collide with mercury atoms. 5. In mercury, the electrons jump to higher energy levels 6. These electrons return to lower levels with emission of a photon 7. The UV light is converted to visible light in the lamp coating Electrodes of tungsten, either coated with a layer which decreases the work function ( cold cathode) or in the form of a incadescent wire ( hot cathode). Pressure of 0.3 bar - noble gas and mercury vapor. Fluorescent coating Power supply with a ballast. Initially, the lamp has a high resistance decreases upon ingition. The ballast decreases the current of the ignited lamp.
11 Discharge bulbs Inductor Starter (i.e. bimetallic)
12 Neon lights 1.Bending of a glass tube 2. Welding of electrodes on both ends 3. Removal of impurities under vacuum and using high current 4. Covering of electrodes with layer of BaO 2 low exit function, cold cathode 5. Evacuation of gas to 1/100 bar 5. Refill with noble gas or mercury vapor. Power supply: 3-15 kv, up to 100 ma.
13 HID lamps HID- High Intensity Discharge Ignition: ionization of xenone, the color correponds to xenon emission line. Heating: metal salt inside the bulb evaporate and are ionized increase of current. Continous work: the lamp reaches the target color. Powered by AC current, 85 V RMS, frequency of about 400 Hz. United States Department of Transportation Federal Highway Administration
14 Flame and its color Smoke unburnt carbon black. Gaseous burning: oxidation of smaller molecules C Burning of carbon black C. So called reducing flame. Still not enough oxygen to burn the fuel. Production of soot (carbon black) not enough oxygen to burn the fuel. Partial burning of gaseous fuel to carbon oxide and dioxide. Remaining fuel thermally decomposes to smaller molecules.
15 Frank-Hertz experiment
16 The characteristic spectrum of X-rays Moseley law lines K Shielding by the K shell
17 Luminescence Luminescence emission of light not related to thermal excitation. Also called cold light sources Only a portion of atoms emits light! Kinds and sources of luminescence: Chemiluminescence chemical reactions Electroluminescence electrical current Photoluminescence incident light Fluorescence Phosphorescence Mechanoluminescence mechanical stimulation Scyntillation ionizing radiation Thermoluminescence increase of temperature N. Rakov et al., Optical Materials Express 11 (2013) 1803
18 Chemiluminescence and bioluminescence Photo: David Mülheims
19 Photoluminescence Emission of light after absorption of light (infrared to UV) Fluorescence instant emission (time 10 8 s) Phosphorescene emission with delay (up to hours) By Maxim Bilovitskiy - Own work, CC BY-SA 4.0,
20 Phosphors Discharge lamps: calcium halofosphoranes activated by manganese - the emission centers related to manganese Phosphor material converts UV light to visible light.
21 Phosphors Cathodoluminescence excitation by electron beam CRT TV receivers, oscilloscopes
22 Electron shells Electron shells K,L,M,N,O,P,Q 2n 2 electrons on a shell
23 The periodic table
Chapter 28. Atomic Physics
Chapter 28 Atomic Physics Quantum Numbers and Atomic Structure The characteristic wavelengths emitted by a hot gas can be understood using quantum numbers. No two electrons can have the same set of quantum
More informationLight Emission.
Light Emission www.physics.sfasu.edu/friedfeld/ch29lec.ppt Radio waves are produced by electrons moving up and down an antenna. Visible light is produced by electrons changing energy states in an atom.
More informationWhat are the six common sources of light?
What are the six common sources of light? Common light sources include incandescent, fluorescent, laser, neon, tungsten-halogen, and sodium-vapor bulbs. Objects that give off their own light are luminous.
More informationChapter 28. Atomic Physics
Chapter 28 Atomic Physics Sir Joseph John Thomson J. J. Thomson 1856-1940 Discovered the electron Did extensive work with cathode ray deflections 1906 Nobel Prize for discovery of electron Early Models
More informationAn element Is a substance that cannot be split into simpler substance. It is composed of discrete particles called atoms.
digitalteachers.co.ug Atomic structure Inorganic chemistry deals with the physical and chemical properties of the elements of the the periodic table. An element Is a substance that cannot be split into
More informationwhere n = (an integer) =
5.111 Lecture Summary #5 Readings for today: Section 1.3 (1.6 in 3 rd ed) Atomic Spectra, Section 1.7 up to equation 9b (1.5 up to eq. 8b in 3 rd ed) Wavefunctions and Energy Levels, Section 1.8 (1.7 in
More informationWe now realize that the phenomena of chemical interactions, and, ultimately life itself, are to be understood in terms of electromagnetism".
We now realize that the phenomena of chemical interactions, and, ultimately life itself, are to be understood in terms of electromagnetism". -Richard Feynman Quantum H Atom Review Radia Wave Function (1s):
More informationChapter 7: The Quantum-Mechanical Model of the Atom
C h e m i s t r y 1 A : C h a p t e r 7 P a g e 1 Chapter 7: The Quantum-Mechanical Model of the Atom Homework: Read Chapter 7. Work out sample/practice exercises Check for the MasteringChemistry.com assignment
More informationThe Bohr Model of the Atom
Unit 4: The Bohr Model of the Atom Properties of light Before the 1900 s, light was thought to behave only as a wave. Light is a type of electromagnetic radiation - a form of energy that exhibits wave
More informationATOMIC MODELS. Models are formulated to fit the available data. Atom was known to have certain size. Atom was known to be neutral.
ATOMIC MODELS Models are formulated to fit the available data. 1900 Atom was known to have certain size. Atom was known to be neutral. Atom was known to give off electrons. THOMPSON MODEL To satisfy the
More informationChapter 37 Early Quantum Theory and Models of the Atom
Chapter 37 Early Quantum Theory and Models of the Atom Units of Chapter 37 37-7 Wave Nature of Matter 37-8 Electron Microscopes 37-9 Early Models of the Atom 37-10 Atomic Spectra: Key to the Structure
More information1) Introduction 2) Photo electric effect 3) Dual nature of matter 4) Bohr s atom model 5) LASERS
1) Introduction 2) Photo electric effect 3) Dual nature of matter 4) Bohr s atom model 5) LASERS 1. Introduction Types of electron emission, Dunnington s method, different types of spectra, Fraunhoffer
More informationPHYS 202. Lecture 23 Professor Stephen Thornton April 20, 2006
PHYS 202 Lecture 23 Professor Stephen Thornton April 20, 2006 Reading Quiz The noble gases (He, Ne, Ar, etc.) 1) are very reactive because they lack one electron of being in a closed shell. 2) are very
More informationPHYS 202. Lecture 23 Professor Stephen Thornton April 25, 2005
PHYS 202 Lecture 23 Professor Stephen Thornton April 25, 2005 Reading Quiz The noble gases (He, Ne, Ar, etc.) 1) are very reactive because they lack one electron of being in a closed shell. 2) are very
More information2. Discrete means unique, that other states don t overlap it. 3. Electrons in the outer electron shells have greater potential energy.
30 Light Emission Answers and Solutions for Chapter 30 Reading Check Questions 1. At these high frequencies, ultraviolet light is emitted. 2. Discrete means unique, that other states don t overlap it.
More informationA fluorescent tube is filled with mercury vapour at low pressure. After mercury atoms have been excited they emit photons.
Q1.(a) A fluorescent tube is filled with mercury vapour at low pressure. After mercury atoms have been excited they emit photons. In which part of the electromagnetic spectrum are these photons? What is
More informationEM SPECTRUM, WAVELENGTH, FREQUENCY, AND ENERGY WORKSHEET
EM SPECTRUM, WAVELENGTH, FREQUENCY, AND ENERGY WORKSHEET 1.) Look at the EM spectrum below to answer this question. As you move across the visible light spectrum from red to violet (A) Does the wavelength
More informationChapter 31 Atomic Physics
100 92 86 100 92 84 100 92 84 98 92 83 97 92 82 96 91 80 96 91 76 95 91 74 95 90 68 95 89 67 95 89 66 94 87 93 86 No. of Students in Range Exam 3 Score Distribution 25 22 20 15 10 10 5 3 2 0 0 0 0 0 0
More informationClassification of Electromagnetic Radiation
Light and Energy Electromagnetic Radiation Radiant energy that exhibits wavelength-like behavior and travels through space at the speed of light in a vacuum. Example: The sun light, energy used in microwave
More informationParticle nature of light & Quantization
Particle nature of light & Quantization A quantity is quantized if its possible values are limited to a discrete set. An example from classical physics is the allowed frequencies of standing waves on a
More informationAtomic Spectroscopy. Absorption and Emission Spectra. Lodovico Lappetito. SpettroscopiaAtomica - 15/07/2015 Pag. 1
Atomic Spectroscopy Absorption and Emission Spectra Lodovico Lappetito SpettroscopiaAtomica - 15/07/2015 Pag. 1 Table of Contents Atomic Spectra... 3 Diffraction Grating Spectrometer... 4 Spectral Lamps...
More informationCSUS Department of Chemistry Experiment 9 Chem. 1A
CSUS Department of Chemistry xperiment 9 Chem. 1A xp. 9 PR-Lab ASSIGNMNT Name: Lab Section (1) Use equation (2) [see the discussion on the next page] to calculate the energies of the ten lowest states
More informationPhysics 1C Lecture 29A. Finish off Ch. 28 Start Ch. 29
Physics 1C Lecture 29A Finish off Ch. 28 Start Ch. 29 Particle in a Box Let s consider a particle confined to a one-dimensional region in space. Following the quantum mechanics approach, we need to find
More informationChapter 37 Early Quantum Theory and Models of the Atom. Copyright 2009 Pearson Education, Inc.
Chapter 37 Early Quantum Theory and Models of the Atom Planck s Quantum Hypothesis; Blackbody Radiation Photon Theory of Light and the Photoelectric Effect Energy, Mass, and Momentum of a Photon Compton
More informationChapter Test B. Chapter: Arrangement of Electrons in Atoms. possible angular momentum quantum numbers? energy level? a. 4 b. 8 c. 16 d.
Assessment Chapter Test B Chapter: Arrangement of Electrons in Atoms PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question
More informationProfessor K. Atomic structure
Professor K Atomic structure Review Reaction- the formation and breaking of chemical bonds Bond- a transfer or sharing of electrons Electrons Abbreviated e - What are they? How were they discovered? Early
More informationEinstein. Quantum Physics at a glance. Planck s Hypothesis (blackbody radiation) (ultraviolet catastrophe) Quantized Energy
Quantum Physics at a glance Quantum Physics deals with the study of light and particles at atomic and smaller levels. Planck s Hypothesis (blackbody radiation) (ultraviolet catastrophe) Quantized Energy
More informationChapter 28 Assignment Solutions
Chapter 28 Assignment Solutions Page 770 #23-26, 29-30, 43-48, 55 23) Complete the following concept map using these terms: energy levels, fixed electron radii, Bohr model, photon emission and absorption,
More informationExperiment 3 Electromagnetic Radiation and Atom Interaction
Experiment 3 Electromagnetic Radiation and Atom Interaction B OBJECTIVES To be familiar with the relationship between emission line spectra and the energy levels of electrons in various atoms. B INTRODUCTION
More informationAtomic Spectra Introduction
Atomic Spectra Introduction: Light and all other electromagnetic radiation is energy that is emitted in the form of waves. Thus light behaves like a wave, and the energy of light varies with the wavelength
More informationAtomization. In Flame Emission
FLAME SPECTROSCOPY The concentration of an element in a solution is determined by measuring the absorption, emission or fluorescence of electromagnetic by its monatomic particles in gaseous state in the
More informationChapter 5. The Electromagnetic Spectrum. What is visible light? What is visible light? Which of the following would you consider dangerous?
Which of the following would you consider dangerous? X-rays Radio waves Gamma rays UV radiation Visible light Microwaves Infrared radiation Chapter 5 Periodicity and Atomic Structure 2 The Electromagnetic
More informationPhysics and the Quantum Mechanical Model
chemistry 1 of 38 Mechanical Model Neon advertising signs are formed from glass tubes bent in various shapes. An electric current passing through the gas in each glass tube makes the gas glow with its
More informationTHE NATURE OF THE ATOM. alpha particle source
chapter THE NATURE OF THE ATOM www.tutor-homework.com (for tutoring, homework help, or help with online classes) Section 30.1 Rutherford Scattering and the Nuclear Atom 1. Which model of atomic structure
More informationOPAC 101 Introduction to Optics
OPAC 101 Introduction to Optics Topic 2 Light Sources Department of http://www1.gantep.edu.tr/~bingul/opac101 Optical & Acustical Engineering Gaziantep University Sep 2017 Sayfa 1 Light Sources: maybe
More informationUNIT : QUANTUM THEORY AND THE ATOM
Name St.No. Date(YY/MM/DD) / / Section UNIT 102-10: QUANTUM THEORY AND THE ATOM OBJECTIVES Atomic Spectra for Hydrogen, Mercury and Neon. 1. To observe various atomic spectra with a diffraction grating
More information1 The Cathode Rays experiment is associated. with: Millikan A B. Thomson. Townsend. Plank Compton
1 The Cathode Rays experiment is associated with: A B C D E Millikan Thomson Townsend Plank Compton 1 2 The electron charge was measured the first time in: A B C D E Cathode ray experiment Photoelectric
More informationExperiment 24: Spectroscopy
Experiment 24: Spectroscopy Figure 24.1: Spectroscopy EQUIPMENT High Voltage Power Supply Incandescent Light Source (3) Gas Discharge Tubes: 1. Helium 2. Hydrogen 3. Unknown Element Spectrometer Felt (1)
More informationUnit 3. Chapter 4 Electrons in the Atom. Niels Bohr s Model. Recall the Evolution of the Atom. Bohr s planetary model
Unit 3 Chapter 4 Electrons in the Atom Electrons in the Atom (Chapter 4) & The Periodic Table/Trends (Chapter 5) Niels Bohr s Model Recall the Evolution of the Atom He had a question: Why don t the electrons
More informationDuncan. Electrons, Energy, & the Electromagnetic Spectrum Notes Simplified, 2-D Bohr Model: Figure 1. Figure 2. Figure 3
Electrons, Energy, & the Electromagnetic Spectrum Notes Simplified, 2-D Bohr Model: Figure 1 Figure 2 Figure 3 Light Calculation Notes Here s how the type/form of EM radiation can be determined The amount
More information5.3. Physics and the Quantum Mechanical Model
Chemistry 5-3 Physics and the Quantum Mechanical Model Neon advertising signs are formed from glass tubes bent in various shapes. An electric current passing through the gas in each glass tube makes the
More informationBecause light behaves like a wave, we can describe it in one of two ways by its wavelength or by its frequency.
Light We can use different terms to describe light: Color Wavelength Frequency Light is composed of electromagnetic waves that travel through some medium. The properties of the medium determine how light
More information3. Particle nature of matter
3. Particle nature of matter 3.1 atomic nature of matter Democrit(us) 470-380 B.C.: there is only atoms and empty space, everything else is mere opinion (atoms are indivisible) Dalton (chemist) 180: chemical
More informationChapter 27 Early Quantum Theory and Models of the Atom Discovery and Properties of the electron
Chapter 27 Early Quantum Theory and Models of the Atom 27-1 Discovery and Properties of the electron Measure charge to mass ratio e/m (J. J. Thomson, 1897) When apply magnetic field only, the rays are
More informationAtomic Spectra. d sin θ = mλ (1)
Atomic Spectra Objectives: To measure the wavelengths of visible light emitted by atomic hydrogen and verify that the measured wavelengths obey the empirical Rydberg formula. To observe emission spectra
More informationNPTEL/IITM. Molecular Spectroscopy Lectures 1 & 2. Prof.K. Mangala Sunder Page 1 of 15. Topics. Part I : Introductory concepts Topics
Molecular Spectroscopy Lectures 1 & 2 Part I : Introductory concepts Topics Why spectroscopy? Introduction to electromagnetic radiation Interaction of radiation with matter What are spectra? Beer-Lambert
More information3 - Atomic Absorption Spectroscopy
3 - Atomic Absorption Spectroscopy Introduction Atomic-absorption (AA) spectroscopy uses the absorption of light to measure the concentration of gas-phase atoms. Since samples are usually liquids or solids,
More informationModern Atomic Theory. Chapter Rutherford s Atom Electromagnetic Radiation. Rutherford showed: Questions left unanswered:
Copyright 2004 by Houghton Mifflin Company. Modern Atomic Theory Chapter 10 All rights reserved. 1 10.1 Rutherford s Atom Rutherford showed: Atomic nucleus is composed of protons (positive) and neutrons
More informationEmission Spectroscopy
Objectives Emission Spectroscopy Observe spectral lines from a hydrogen gas discharge tube Determine the initial and final energy levels for the electronic transitions associated with the visible portion
More informationAtomic Spectroscopy. Objectives
Atomic Spectroscopy Name Objectives explain the difference between emission and absorption spectra calculate the energy of orbits in the Bohr model of hydrogen calculate E for energy transitions in the
More informationQuantum and Atomic Physics - Multiple Choice
PSI AP Physics 2 Name 1. The Cathode Ray Tube experiment is associated with: (A) J. J. Thomson (B) J. S. Townsend (C) M. Plank (D) A. H. Compton 2. The electron charge was measured the first time in: (A)
More informationOptical Spectroscopy and Atomic Structure. PHYS 0219 Optical Spectroscopy and Atomic Structure 1
Optical Spectroscopy and Atomic Structure PHYS 0219 Optical Spectroscopy and Atomic Structure 1 Optical Spectroscopy and Atomic Structure This experiment has four parts: 1. Spectroscope Setup - Your lab
More informationTHE UNIVERSITY OF QUEENSLAND DEPARTMENT OF PHYSICS PHYS2041 ATOMIC SPECTROSCOPY
THE UNIVERSITY OF QUEENSLAND DEPARTMENT OF PHYSICS PHYS2041 ATOMIC SPECTROSCOPY Warning: The mercury spectral lamps emit UV radiation. Do not stare into the lamp. Avoid exposure where possible. Introduction
More informationExperiment #9. Atomic Emission Spectroscopy
Introduction Experiment #9. Atomic Emission Spectroscopy Spectroscopy is the study of the interaction of light with matter. This interaction can be in the form of the absorption or the emission of electromagnetic
More informationParticle Detectors and Quantum Physics (2) Stefan Westerhoff Columbia University NYSPT Summer Institute 2002
Particle Detectors and Quantum Physics (2) Stefan Westerhoff Columbia University NYSPT Summer Institute 2002 More Quantum Physics We know now how to detect light (or photons) One possibility to detect
More informationSCH4C Practice WS Unit 1
Name: Class: Date: SCH4C Practice WS Unit 1 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The special band of light waves that the human eye can detect
More informationChemistry 212 ATOMIC SPECTROSCOPY
Chemistry 212 ATOMIC SPECTROSCOPY The emission and absorption of light energy of particular wavelengths by atoms and molecules is a common phenomenon. The emissions/absorptions are characteristic for each
More informationAtomic Theory. H. Cannon, C. Clapper and T. Guillot Klein High School
Atomic Theory Unit 3 Development of the Atomic Theory 1. Where is the mass of the atom concentrated? 2. What is located in the nucleus? 3. What is the negative particle that orbits the nucleus? 4. What
More information5.111 Lecture Summary #5 Friday, September 12, 2014
5.111 Lecture Summary #5 Friday, September 12, 2014 Readings for today: Section 1.3 Atomic Spectra, Section 1.7 up to equation 9b Wavefunctions and Energy Levels, Section 1.8 The Principle Quantum Number.
More informationChapter 5 Models of the Atom
Chapter 5 Models of the Atom Atomic Models Rutherford used existing ideas about the atom and proposed an atomic model in which the electrons move around the nucleus. However, Rutherford s atomic model
More informationProf. Jeff Kenney Class 5 June 1, 2018
www.astro.yale.edu/astro120 Prof. Jeff Kenney Class 5 June 1, 2018 to understand how we know stuff about the universe we need to understand: 1. the spectral analysis of light 2. how light interacts with
More informationThe Bohr Model Bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.
5.1 The Development of Atomic Models Rutherford s atomic model could not explain the chemical properties of elements. Rutherford s atomic model could not explain why objects change color when heated. The
More informationCDO AP Chemistry Unit 5
1. a. Calculate the wavelength of electromagnetic radiation that has a frequency of 5.56 MHz. b. Calculate the frequency of electromagnetic radiation that has a wavelength equal to 667 nm. 2. Electromagnetic
More informationEarly Quantum Theory and Models of the Atom
Early Quantum Theory and Models of the Atom Electron Discharge tube (circa 1900 s) There is something ( cathode rays ) which is emitted by the cathode and causes glowing Unlike light, these rays are deflected
More informationAtomic Spectra for Atoms and Ions. Light is made up of different wavelengths
Atomic Spectra for Atoms and Ions What will you be doing in lab next week? Recording the line spectra of several different substances in discharge tubes. Recording the line spectra of several ions from
More informationSPARKS CH301. Why are there no blue fireworks? LIGHT, ELECTRONS & QUANTUM MODEL. UNIT 2 Day 2. LM15, 16 & 17 due W 8:45AM
SPARKS CH301 Why are there no blue fireworks? LIGHT, ELECTRONS & QUANTUM MODEL UNIT 2 Day 2 LM15, 16 & 17 due W 8:45AM QUIZ: CLICKER QUESTION Which of these types of light has the highest energy photons?
More informationEXPERIMENT 17: Atomic Emission
EXPERIMENT 17: Atomic Emission PURPOSE: To construct an energy level diagram of the hydrogen atom To identify an element from its line spectrum. PRINCIPLES: White light, such as emitted by the sun or an
More informationLECTURE 23 SPECTROSCOPY AND ATOMIC MODELS. Instructor: Kazumi Tolich
LECTURE 23 SPECTROSCOPY AND ATOMIC MODELS Instructor: Kazumi Tolich Lecture 23 2 29.1 Spectroscopy 29.2 Atoms The first nuclear physics experiment Using the nuclear model 29.3 Bohr s model of atomic quantization
More informationWorksheet 2.1. Chapter 2: Atomic structure glossary
Worksheet 2.1 Chapter 2: Atomic structure glossary Acceleration (in a mass spectrometer) The stage where the positive ions are attracted to negatively charged plates. Alpha decay The emission of an alpha
More informationBohr. Electronic Structure. Spectroscope. Spectroscope
Bohr Electronic Structure Bohr proposed that the atom has only certain allowable energy states. Spectroscope Using a device called a it was found that gaseous elements emitted electromagnetic radiation
More informationLECTURE # 19 Dennis Papadopoulos End of Classical Physics Quantization Bohr Atom Chapters 38 39
PHYS 270-SPRING 2011 LECTURE # 19 Dennis Papadopoulos End of Classical Physics Quantization Bohr Atom Chapters 38 39 April 14, 2011 1 HOW TO MEASURE SPECTRA Spectroscopy: Unlocking the Structure of Atoms
More informationSpectroscopy. Hot self-luminous objects light the Sun or a light bulb emit a continuous spectrum of wavelengths.
Hot self-luminous objects light the Sun or a light bulb emit a continuous spectrum of wavelengths. In contract, light emitted in low=pressure gas discharge contains only discrete individual wavelengths,
More informationA World of Color. Session 2. OLLI at Illinois Spring D. H. Tracy
A World of Color Session 2 OLLI at Illinois Spring 2018 D. H. Tracy Course Outline 1. Overview, History and Spectra 2. Nature and Sources of Light 3. Eyes and Color Vision 4. Origins of Colors of Things
More informationEP225 Lecture 31 Quantum Mechanical E ects 1
EP225 Lecture 31 Quantum Mechanical E ects 1 Why the Hydrogen Atom Is Stable In the classical model of the hydrogen atom, an electron revolves around a proton at a radius r = 5:3 10 11 m (Bohr radius)
More informationThe energy of the emitted light (photons) is given by the difference in energy between the initial and final states of hydrogen atom.
Lecture 20-21 Page 1 Lectures 20-21 Transitions between hydrogen stationary states The energy of the emitted light (photons) is given by the difference in energy between the initial and final states of
More informationGeneral Physics (PHY 2140)
General Physics (PHY 140) Lecture 33 Modern Physics Atomic Physics Atomic spectra Bohr s theory of hydrogen http://www.physics.wayne.edu/~apetrov/phy140/ Chapter 8 1 Lightning Review Last lecture: 1. Atomic
More informationChapter 5 Light and Matter
Chapter 5 Light and Matter Stars and galaxies are too far for us to send a spacecraft or to visit (in our lifetimes). All we can receive from them is light But there is much we can learn (composition,
More informationReview: Properties of a wave
Radiation travels as waves. Waves carry information and energy. Review: Properties of a wave wavelength (λ) crest amplitude (A) trough velocity (v) λ is a distance, so its units are m, cm, or mm, etc.
More informationParadigm Shift: Development of Current Atomic Theory Spectroscopy and Energy Levels in Atoms. OR, Show me the Electrons!
Lecture 2 362 January 16, 2019 Paradigm Shift: Development of Current Atomic Theory Spectroscopy and Energy Levels in Atoms OR, Show me the Electrons! Color Red Yellow White Green Blue Violet Metal Flame
More informationRAY OPTICS 6. DISPERSION POINTS TO REMEMBER
Y OPTICS 6. DISPESION POINTS TO EMEMBE. Dispersion : a) The splitting of white light into constituent colours is called dispersion and the band of colours is called spectrum. b) Dispersion of light was
More informationArrangement of Electrons in the Atom
Arrangement of Electrons in the Atom Bohr s Study of Atomic Spectra When white light is passed through a prism, the white light is broken up into an array of colours. This spread of colours is called a
More informationis the minimum stopping potential for which the current between the plates reduces to zero.
Module 1 :Quantum Mechanics Chapter 2 : Introduction to Quantum ideas Introduction to Quantum ideas We will now consider some experiments and their implications, which introduce us to quantum ideas. The
More informationChapter 39. Particles Behaving as Waves
Chapter 39 Particles Behaving as Waves 39.1 Electron Waves Light has a dual nature. Light exhibits both wave and particle characteristics. Louis de Broglie postulated in 1924 that if nature is symmetric,
More information8. Which of the following could be an isotope of chlorine? (A) 37 Cl 17 (B) 17 Cl 17 (C) 37 Cl 17 (D) 17 Cl 37.5 (E) 17 Cl 37
Electronic Structure Worksheet 1 Given the following list of atomic and ionic species, find the appropriate match for questions 1-4. (A) Fe 2+ (B) Cl (C) K + (D) Cs (E) Hg + 1. Has the electron configuration:
More informationCHAPTER 27 Quantum Physics
CHAPTER 27 Quantum Physics Units Discovery and Properties of the Electron Planck s Quantum Hypothesis; Blackbody Radiation Photon Theory of Light and the Photoelectric Effect Energy, Mass, and Momentum
More informationHomework on spectroscopy, colors, and light. Answers should be entered on a Scantron form given out in class. This exercise is worth 20 points.
Astr. 170B1 Due Sept. 20 Professors Rieke Homework on spectroscopy, colors, and light. Answers should be entered on a Scantron form given out in class. This exercise is worth 20 points. 1. Is the spectrum
More information2101 Atomic Spectroscopy
2101 Atomic Spectroscopy Atomic identification Atomic spectroscopy refers to the absorption and emission of ultraviolet to visible light by atoms and monoatomic ions. It is best used to analyze metals.
More informationReview: Light and Spectra. Absorption and Emission Lines
1 Review: Light and Spectra Light is a wave It undergoes diffraction and other wave phenomena. But light also is made of particles Energy is carried by photons 1 Wavelength energy of each photon Computer
More informationHigher -o-o-o- Past Paper questions o-o-o- 3.4 Spectra
Higher -o-o-o- Past Paper questions 1991-2010 -o-o-o- 3.4 Spectra 1992 Q37 The diagram below shows the energy levels for the hydrogen atom. (a) Between which two energy levels would an electron transition
More informationChem 105 Fri 22 Oct 2010
Chem 105 Fri 22 Oct 2010 1) Chapter 6 - Atomic Structure Hour Exam 2 will be returned Monday 10/22/2010 1 Mark your calendar: Hour Exam 3 (Ch 6, 7, 8) is Friday, Nov. 12. 10/22/2010 2 10/22/2010 3 Chap.
More information10/27/2017 [pgs ]
Objectives SWBAT explain the relationship between energy and frequency. SWBAT predict the behavior of and/or calculate quantum and photon energy from frequency. SWBAT explain how the quantization of energy
More information2.1- CLASSICAL CONCEPTS; Dr. A. DAYALAN, Former Prof & Head 1
2.1- CLASSICAL CONCEPTS; Dr. A. DAYALAN, Former Prof & Head 1 QC-2 QUANTUM CHEMISTRY (Classical Concept) Dr. A. DAYALAN,Former Professor & Head, Dept. of Chemistry, LOYOLA COLLEGE (Autonomous), Chennai
More informationATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY All matter is made of atoms. There are a limited number of types of atoms; these are the elements. (EU 1.A) Development of Atomic Theory Atoms are so small
More informationPlanck s Quantum Hypothesis Blackbody Radiation
Planck s Quantum Hypothesis Blackbody Radiation The spectrum of blackbody radiation has been measured(next slide); it is found that the frequency of peak intensity increases linearly with temperature.
More informationFinal Exam: Thursday 05/02 7:00 9:00 pm in STEW 183
Final Exam: Thursday 05/02 7:00 9:00 pm in STEW 183 Covers all readings, lectures, homework from Chapters 17 through 30 Be sure to bring your student ID card, calculator, pencil, and up to three onepage
More informationStudy On the Capacitance Between Orbitals and Atoms Modeling
Study On the Capacitance Between Orbitals and Atoms Modeling Ali A. Elabd *, El-Sayed M. El-Rabaie, Abdel-Aziz T. Shalaby Faculty of Electronic Engineering, 32952 Menouf, Minoufiya University, Egypt. In
More informationChapter 6 Electronic Structure of Atoms
Chapter 6 Electronic Structure of Atoms What is the origin of color in matter? Demo: flame tests What does this have to do with the atom? Why are atomic properties periodic? 6.1 The Wave Nature of Light
More informationChapters 31 Atomic Physics
Chapters 31 Atomic Physics 1 Overview of Chapter 31 Early Models of the Atom The Spectrum of Atomic Hydrogen Bohr s Model of the Hydrogen Atom de Broglie Waves and the Bohr Model The Quantum Mechanical
More information2) The number of cycles that pass through a stationary point is called A) wavelength. B) amplitude. C) frequency. D) area. E) median.
Chemistry Structure and Properties 2nd Edition Tro Test Bank Full Download: http://testbanklive.com/download/chemistry-structure-and-properties-2nd-edition-tro-test-bank/ Chemistry: Structure & Properties,
More informationAtoms, Electrons and Light MS. MOORE CHEMISTRY
Atoms, Electrons and Light MS. MOORE CHEMISTRY Atoms Remember Rutherford??? What did he discover with his gold foil experiment. A: Atoms contain a dense nucleus where the protons and neutrons reside. ATOMS
More information