Atomic Transitions and Selection Rules
|
|
- Juniper Austin
- 5 years ago
- Views:
Transcription
1 Atomic Transitions and Selection Rules The time-dependent Schrodinger equation for an electron in an atom with a time-independent potential energy is ~ 2 2m r2 (~r, t )+V(~r ) (~r, We found that the solutions to this equation can be found via separation of variables and superposition: (~r, t )= X n c n n (~r )exp( ie n t/~) (n is shorthand for the set of quantum numbers that defines an eigenstate of the Hamiltonian)
2 Clicker Question (~r, t )= X n c n n (~r )exp( ie n t/~) What is the probability that an energy E i is measured? 1. c n 2. c i 3. c i 2 4. c i ψ i 2 5. c i E i 2
3 Clicker Question Suppose the energy is measured and the result is E 3. We now know that the quantum state is ψ 3, and that c n =0 for all values of n not equal to 3. If we wait a time t and then measure the energy again, what is the probability we will measure a value E n (for n not equal to 3)? 1. Zero! 2. Roughly zero for small values of t, but it increases with time. 3. Non zero and a constant value, regardless of the value of t.
4 Time-Dependent Potential Energy Now suppose the potential energy is given by V (~r, t )=V 0 (~r )+V 1 (~r, t ), where V 0 is the original potential energy associated with the atom and V 1 is some time-dependent perturbation (such as due to incident electromagnetic radiation). Now the solution to the time dependent Schrodinger equation will change, and since V 1 is time dependent, separation of variables will no longer work. If V 1 <<V 0, we call V 1 a perturbation. The idea is it still makes sense to think of the electron as being a superposition of eigenstates of V 0, but now the coefficients are time-dependent. (~r, t )= X n c n (t) n (~r )exp( ie n t/~) This means that transitions can occur.
5 Transitions and Selection Rules (~r, t )= X n c n (t) n (~r )exp( ie n t/~) Solving the time-dependent Schrodinger equation to determine c n (t) is well outside the scope of this class (take Atomic and Molecular Physics). It turns out that if the electron is initially in state i (c i (t=0) = 1 and c other (t=0) = 0), then the probability per unit time that a transition to state f occurs is given by where i!f / <f V 1 (~r Z, t ) i > 2, <f V 1 (~r, t ) i >= f V 1 i d 3 r For the case where V 1 is due to unpolarized radiation i!f = Z ~ 2 f~r i d 3 r (! if )
6 Example: 2s to 1s transition Consider the transition of hydrogen from 2s to 1s due to radiation polarized in the z-direction: Z 2 2!1 / 1z 2 d 3 r Z 100z 200 d 3 / Z 0 cos sin d Is this integral zero or non-zero? 1. Zero 2. Non-Zero
7 Selection Rules The selection rules for dipole transitions result from determining when the overlap integral is not zero: Z f ~r i d 3 r 6= 0 For hydrogen-like atoms (one electron), the resulting selection rules are: l = ±1 m l =0, ±1 For multi-electron atoms: J =0, ±1 M J =0, ±1 (J=0 to 0 not allowed) For ideal LS coupling S =0 M S =0 This implies that For 1-e transitions, L =0, ±1 l = ±1
8 Applications to Helium Due to ΔS=0, triplet states can t transition to singlet states. Metastable states: states that can t transition via the dipole transition. Forbidden Transitions. Transitions via magnetic dipole or electric quadrapole interactions.
9 Semi-Classical Model of Transitions Some insight to the nature of transitions can be obtained from a semi-classical model. Classically, we know that radiation is emitted when charged particles accelerate (due to a changing electric field inducing a magnetic field). The electric field can often be approximated by using the dipole moment: ~p = X i q i ~r i E ~ 1 3(~p ˆr)ˆr ~p 4 0 r 3 The Larmor formula gives the power of emitted radiation due to an accelerating charge: P = q2 a c 3
10 Semi-Classical Model of Dipole Transitions A harmonically oscillating dipole can be expressed as ~p = ~p 0 e iwt After expressing the acceleration in terms of the dipole moment, the Larmor formula P = µ 0! 4 p c Now, for quantum mechanics, the dipole moment is due to the electron cloud. ~p = e Z ~r (~r ) 2 d 3 r
11 Z Clicker Question ~p = e ~r (~r ) 2 d 3 r Is the dipole moment zero or non-zero if the electron is in a stationary state (with no time-dependent potential energy)? 1. zero, for any quantum state 2. zero for some, non-zero for other quantum states 3. non-zero for all quantum states
12 Z Clicker Question ~p = e ~r (~r ) 2 d 3 r Is the dipole moment zero or non-zero if the electron is in a stationary state (with no time-dependent potential energy)? 1. zero, for any quantum state 2. zero for some, non-zero for other quantum states 3. non-zero for all quantum states Thus stationary states don t emit any radiation, and again we see transitions don t occur if there is no time-dependent potential energy.
13 Semi-Classical Model of Dipole Transitions Now, due to the time-dependent potential energy, let s let the electron have a foot in both the initial and final states: (~r, t )=c i (t) i (~r )exp( ie i t/~)+c f (t) f exp( ie f t/~) ~p = e Inserting, we find where Z ~r (~r ) 2 d 3 r ~p = c i c f ~p 0 exp(i!t)+c i c f ~p 0 exp( i!t) ~p =2Re[c i c f ~p 0 exp(i!t)] Z ~p 0 = e i ~r f dv ~! = E i E f p 0 is the overlap integral. Determining when this integral is not equal to zero gives us the selection rules.
14 Spontaneous Emission Why does an excited atom, out in space, far from any source of electromagnetic radiation, de-excite?
15 GRE QUESTIONS
16
17 X-Ray Line Spectra Transitions of valence electrons result in UV, visible, infrared, and radio emission lines. Multi-electron atoms with a large value of Z can emit X-ray emission lines: If an electron from an inner shell is ejected (say due to a collision with a high-energy electron or photon), an electron from a higher energy state can jump into the hole. A cascade occurs due to the holes left behind by the jumping electrons.
18
19
20
21 generalizing (for other transitions): f = k 1 (Z k 2 )
Notes on x-ray scattering - M. Le Tacon, B. Keimer (06/2015)
Notes on x-ray scattering - M. Le Tacon, B. Keimer (06/2015) Interaction of x-ray with matter: - Photoelectric absorption - Elastic (coherent) scattering (Thomson Scattering) - Inelastic (incoherent) scattering
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 informationNotes on excitation of an atom or molecule by an electromagnetic wave field. F. Lanni / 11feb'12 / rev9sept'14
Notes on excitation of an atom or molecule by an electromagnetic wave field. F. Lanni / 11feb'12 / rev9sept'14 Because the wavelength of light (400-700nm) is much greater than the diameter of an atom (0.07-0.35
More informationOptical Spectroscopy 1 1. Absorption spectroscopy (UV/vis)
Optical Spectroscopy 1 1. Absorption spectroscopy (UV/vis) 2 2. Circular dichroism (optical activity) CD / ORD 3 3. Fluorescence spectroscopy and energy transfer Electromagnetic Spectrum Electronic Molecular
More informationFundamentals of Spectroscopy for Optical Remote Sensing. Course Outline 2009
Fundamentals of Spectroscopy for Optical Remote Sensing Course Outline 2009 Part I. Fundamentals of Quantum Mechanics Chapter 1. Concepts of Quantum and Experimental Facts 1.1. Blackbody Radiation and
More informationGlow-Sticks are Forbidden. Zachary G Wolfe. Department of Physics and Physical Oceanography. University of North Carolina Wilmington
Glow-Sticks are Forbidden Zachary G Wolfe Department of Physics and Physical Oceanography University of North Carolina Wilmington Abstract: Physics students learn early that certain electronic transitions
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 informationComplete nomenclature for electron orbitals
Complete nomenclature for electron orbitals Bohr s model worked but it lacked a satisfactory reason why. De Broglie suggested that all particles have a wave nature. u l=h/p Enter de Broglie again It was
More informationChapters 28 and 29: Quantum Physics and Atoms Questions & Problems
Chapters 8 and 9: Quantum Physics and Atoms Questions & Problems hc = hf = K = = hf = ev P = /t = N h h h = = n = n, n = 1,, 3,... system = hf photon p mv 8 ml photon max elec 0 0 stop total photon 91.1nm
More informationParticles and Waves Particles Waves
Particles and Waves Particles Discrete and occupy space Exist in only one location at a time Position and velocity can be determined with infinite accuracy Interact by collisions, scattering. Waves Extended,
More informationLecture 3: Helium Readings: Foot Chapter 3
Lecture 3: Helium Readings: Foot Chapter 3 Last Week: the hydrogen atom, eigenstate wave functions, and the gross and fine energy structure for hydrogen-like single-electron atoms E n Z n = hcr Zα / µ
More informationPreliminary Quantum Questions
Preliminary Quantum Questions Thomas Ouldridge October 01 1. Certain quantities that appear in the theory of hydrogen have wider application in atomic physics: the Bohr radius a 0, the Rydberg constant
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 informationThe Einstein A and B Coefficients
The Einstein A and B Coefficients Austen Groener Department of Physics - Drexel University, Philadelphia, Pennsylvania 19104, USA Quantum Mechanics III December 10, 010 Abstract In this paper, the Einstein
More informationArrangement of Electrons. Chapter 4
Arrangement of Electrons Chapter 4 Properties of Light -Light s interaction with matter helps to understand how electrons behave in atoms -Light travels through space & is a form of electromagnetic radiation
More informationMultielectron Atoms and Periodic Table
GRE Question Multielectron Atoms and Periodic Table Helium Atom 2 2m e ( 2 1 + 2 2) + 2ke 2 2ke 2 + ke2 r 1 r 2 r 2 r 1 Electron-electron repulsion term destroys spherical symmetry. No analytic solution
More informationDo Now: Bohr Diagram, Lewis Structures, Valence Electrons 1. What is the maximum number of electrons you can fit in each shell?
Chemistry Ms. Ye Name Date Block Do Now: Bohr Diagram, Lewis Structures, Valence Electrons 1. What is the maximum number of electrons you can fit in each shell? 1 st shell 2 nd shell 3 rd shell 4 th shell
More information2) The energy of a photon of light is proportional to its frequency and proportional to its wavelength.
Advanced Chemistry Chapter 13 Review Name Per Show all work Wave Properties 1) Which one of the following is correct? A) ν + λ = c B) ν λ = c C) ν = cλ D) λ = c ν E) νλ = c 2) The energy of a photon of
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 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 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 informationQuick Review. 1. Kinetic Molecular Theory. 2. Average kinetic energy and average velocity. 3. Graham s Law of Effusion. 4. Real Gas Behavior.
Quick Review 1. Kinetic Molecular Theory. 2. Average kinetic energy and average velocity. 3. Graham s Law of Effusion. 4. Real Gas Behavior. Emission spectra Every element has a unique emission spectrum
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 informationEx: N has 5 valence electrons, so it s Lewis structure would look like: N
Chemistry Ms. Ye Review: Bohr Model of the Atom Name Date Block Electrons are shown in concentric shells or energy levels around the nucleus o The first shell can hold up to o The second shell can hold
More informationLet s start with ionization energy - The minimum energy needed to remove and electron from an atom.
Early Quantum Theory In what may seem like an abrupt change of pace, we will now drop our periodic table with its focus on practical chemistry of elements and start working on the background needed to
More informationAtomic Structure and Processes
Chapter 5 Atomic Structure and Processes 5.1 Elementary atomic structure Bohr Orbits correspond to principal quantum number n. Hydrogen atom energy levels where the Rydberg energy is R y = m e ( e E n
More informationGilbert Kirss Foster. Chapter3. Atomic Structure. Explaining the Properties of Elements
Gilbert Kirss Foster Chapter3 Atomic Structure Explaining the Properties of Elements Chapter Outline 3.1 Waves of Light 3.2 Atomic Spectra 3.3 Particles of Light: Quantum Theory 3.4 The Hydrogen Spectrum
More informationLecture 3: Light absorbance
Lecture 3: Light absorbance Perturbation Response 1 Light in Chemistry Light Response 0-3 Absorbance spectrum of benzene 2 Absorption Visible Light in Chemistry S 2 S 1 Fluorescence http://www.microscopyu.com
More informationPhotochemical principles
Chapter 1 Photochemical principles Dr. Suzan A. Khayyat 1 Photochemistry Photochemistry is concerned with the absorption, excitation and emission of photons by atoms, atomic ions, molecules, molecular
More informationX-Rays from Atoms. These are called K α X-rays See table 29.1 for the energy of K α X-rays produced by some elements. Section 29.3
X-Rays from Atoms The highest photon energy available in a hydrogen atom is in the ultraviolet part of the electromagnetic spectrum Other atoms can emit much more energetic photons larger Z, more electric
More informationElectromagnetic Radiation. Chapter 12: Phenomena. Chapter 12: Quantum Mechanics and Atomic Theory. Quantum Theory. Electromagnetic Radiation
Chapter 12: Phenomena Phenomena: Different wavelengths of electromagnetic radiation were directed onto two different metal sample (see picture). Scientists then recorded if any particles were ejected and
More informationPHYS 172: Modern Mechanics Fall 2009
PHYS 172: Modern Mechanics Fall 2009 Lecture 14 Energy Quantization Read 7.1 7.9 Reading Question: Ch. 7, Secs 1-5 A simple model for the hydrogen atom treats the electron as a particle in circular orbit
More informationWhich of the following classes of electromagnetic waves will not ionise neutral atoms?
1 In an experiment to demonstrate the photoelectric effect, a charged metal plate is illuminated with light from different sources. The plate loses its charge when an ultraviolet light source is used but
More informationNon-stationary States and Electric Dipole Transitions
Pre-Lab Lecture II Non-stationary States and Electric Dipole Transitions You will recall that the wavefunction for any system is calculated in general from the time-dependent Schrödinger equation ĤΨ(x,t)=i
More informationAtomic Structure & Radiative Transitions
Atomic Structure & Radiative Transitions electron kinetic energy nucleus-electron interaction electron-electron interaction Remember the meaning of spherical harmonics Y l, m (θ, ϕ) n specifies the
More informationAST 105 Intro Astronomy The Solar System. MIDTERM II: Tuesday, April 5 [covering Lectures 10 through 16]
AST 105 Intro Astronomy The Solar System MIDTERM II: Tuesday, April 5 [covering Lectures 10 through 16] REVIEW Light as Information Bearer We can separate light into its different wavelengths (spectrum).
More informationInformation in Radio Waves
Summative Assessment: Natural Sources of Radio Performance expectation: Develop and use a model of two objects interacting through electric or magnetic fields to illustrate the forces between objects and
More informationChapter 29 Atomic Physics. Looking Ahead. Slide 29-1
Chapter 29 Atomic Physics Looking Ahead Slide 29-1 Atomic Spectra and the Bohr Model In the mid 1800s it became apparent that the spectra of atomic gases is comprised of individual emission lines. Slide
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 informationTheory of optically thin emission line spectroscopy
Theory of optically thin emission line spectroscopy 1 Important definitions In general the spectrum of a source consists of a continuum and several line components. Processes which give raise to the continuous
More informationPHYS 219 General Physics: Electricity, Light and Modern Physics
PHYS 219 General Physics: Electricity, Light and Modern Physics Final exam is scheduled on Thursday May 2 @ 8 10 AM In Physics 112 It will cover five Chapters 25, 27, 28, 29, and 30. Review lecture notes,
More informationPhotoionized Gas Ionization Equilibrium
Photoionized Gas Ionization Equilibrium Ionization Recombination H nebulae - case A and B Strömgren spheres H + He nebulae Heavy elements, dielectronic recombination Ionization structure 1 Ionization Equilibrium
More informationAtomic Structure. Standing Waves x10 8 m/s. (or Hz or 1/s) λ Node
Atomic Structure Topics: 7.1 Electromagnetic Radiation 7.2 Planck, Einstein, Energy, and Photons 7.3 Atomic Line Spectra and Niels Bohr 7.4 The Wave Properties of the Electron 7.5 Quantum Mechanical View
More informationAtoms. Radiation from atoms and molecules enables the most accurate time and length measurements: Atomic clocks
Atoms Quantum physics explains the energy levels of atoms with enormous accuracy. This is possible, since these levels have long lifetime (uncertainty relation for E, t). Radiation from atoms and molecules
More informationCollisionally Excited Spectral Lines (Cont d) Diffuse Universe -- C. L. Martin
Collisionally Excited Spectral Lines (Cont d) Please Note: Contrast the collisionally excited lines with the H and He lines in the Orion Nebula spectrum. Preview: Pure Recombination Lines Recombination
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 informationLecture 6: The Physics of Light, Part 1. Astronomy 111 Wednesday September 13, 2017
Lecture 6: The Physics of Light, Part 1 Astronomy 111 Wednesday September 13, 2017 Reminders Star party tonight! Homework #3 due Monday Exam #1 Monday, September 25 The nature of light Look, but don t
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 informationHarmonic Potential with Gaussian Barrier Model for Ammonia Inversion
Harmonic Potential with Gaussian Barrier Model for Ammonia Inversion Frank Rioux Department of Chemistry College of St. Benedict St. John's University Abstract The umbrella inversion in ammonia is modeled
More informationAccounts for certain objects being colored. Used in medicine (examples?) Allows us to learn about structure of the atom
1.1 Interaction of Light and Matter Accounts for certain objects being colored Used in medicine (examples?) 1.2 Wavelike Properties of Light Wavelength, : peak to peak distance Amplitude: height of the
More informationCHEM6416 Theory of Molecular Spectroscopy 2013Jan Spectroscopy frequency dependence of the interaction of light with matter
CHEM6416 Theory of Molecular Spectroscopy 2013Jan22 1 1. Spectroscopy frequency dependence of the interaction of light with matter 1.1. Absorption (excitation), emission, diffraction, scattering, refraction
More informationAtomic spectra of one and two-electron systems
Atomic spectra of one and two-electron systems Key Words Term symbol, Selection rule, Fine structure, Atomic spectra, Sodium D-line, Hund s rules, Russell-Saunders coupling, j-j coupling, Spin-orbit coupling,
More informationI 2 Vapor Absorption Experiment and Determination of Bond Dissociation Energy.
I 2 Vapor Absorption Experiment and Determination of Bond Dissociation Energy. What determines the UV-Vis (i.e., electronic transitions) band appearance? Usually described by HOMO LUMO electron jump LUMO
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 informationHonors Unit 6 Notes - Atomic Structure
Name: Honors Unit 6 Notes - Atomic Structure Objectives: 1. Students will have a general understanding of the wave nature of light and the interrelationship between frequency, wavelength, and speed of
More informationATOMIC AND LASER SPECTROSCOPY
ALAN CORNEY ATOMIC AND LASER SPECTROSCOPY CLARENDON PRESS OXFORD 1977 Contents 1. INTRODUCTION 1.1. Planck's radiation law. 1 1.2. The photoelectric effect 4 1.3. Early atomic spectroscopy 5 1.4. The postulates
More informationChapter 6 - Electronic Structure of Atoms
Chapter 6 - Electronic Structure of Atoms 6.1 The Wave Nature of Light To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation Visible light is an example
More informationModels of the Atom. Spencer Clelland & Katelyn Mason
Models of the Atom Spencer Clelland & Katelyn Mason First Things First Electrons were accepted to be part of the atom structure by scientists in the1900 s. The first model of the atom was visualized as
More informationGeorgia Institute of Technology CHEM 1310 revised 10/8/09 Spring The Development of Quantum Mechanics. ν (nu) = frequency (in s -1 or hertz)
The Development of Quantum Mechanics Early physicists used the properties of electromagnetic radiation to develop fundamental ideas about the structure of the atom. A fundamental assumption for their work
More informationPAPER No. : 8 (PHYSICAL SPECTROSCOPY) MODULE No. : 5 (TRANSITION PROBABILITIES AND TRANSITION DIPOLE MOMENT. OVERVIEW OF SELECTION RULES)
Subject Chemistry Paper No and Title Module No and Title Module Tag 8 and Physical Spectroscopy 5 and Transition probabilities and transition dipole moment, Overview of selection rules CHE_P8_M5 TABLE
More informationChapter4: Quantum Optical Control
Chapter4: Quantum Optical Control Laser cooling v A P3/ B P / C S / Figure : Figure A shows how an atom is hit with light with momentum k and slows down. Figure B shows atom will absorb light if frequency
More information量子力学 Quantum mechanics. School of Physics and Information Technology
量子力学 Quantum mechanics School of Physics and Information Technology Shaanxi Normal University Chapter 9 Time-dependent perturation theory Chapter 9 Time-dependent perturation theory 9.1 Two-level systems
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 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 informationBasic Physical Chemistry Lecture 2. Keisuke Goda Summer Semester 2015
Basic Physical Chemistry Lecture 2 Keisuke Goda Summer Semester 2015 Lecture schedule Since we only have three lectures, let s focus on a few important topics of quantum chemistry and structural chemistry
More informationElectromagnetic Radiation. is a form of energy that exhibits wavelike behavior as it travels through space.
Electromagnetic Radiation is a form of energy that exhibits wavelike behavior as it travels through space. What are the 7 forms of electromagnetic radiation, in order of INCREASING wavelength? gamma rays
More informationEmission of Light & Atomic Models 1
Emission of Light & Atomic Models 1 Objective At the end of this activity you should be able to: o Explain what photons are, and be able to calculate their energies given either their frequency or wavelength.
More informationElectromagnetic radiation simply a stream of photons (a bundle of energy) What are photons???
Electromagnetic radiation simply a stream of photons (a bundle of energy) What are photons??? no mass travel in a wave like pattern move at the speed of light contain a certain amount (or bundle) of energy
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 informationNuclear Decays. Alpha Decay
Nuclear Decays The first evidence of radioactivity was a photographic plate, wrapped in black paper and placed under a piece of uranium salt by Henri Becquerel on February 26, 1896. Like many events in
More informationCHM Physical Chemistry II Chapter 12 - Supplementary Material. 1. Einstein A and B coefficients
CHM 3411 - Physical Chemistry II Chapter 12 - Supplementary Material 1. Einstein A and B coefficients Consider two singly degenerate states in an atom, molecule, or ion, with wavefunctions 1 (for the lower
More informationChapter 9. Blimps, Balloons, and Models for the Atom. Electrons in Atoms and the Periodic Table. Hindenburg. Properties of Elements Hydrogen Atoms
Chapter 9 Electrons in Atoms and the Periodic Table Blimps, Balloons, and Models for the Atom Hindenburg Blimps, Balloons, and Models for the Atom Properties of Elements Hydrogen Atoms Helium Atoms 1 Blimps,
More informationChapter 3. Electromagnetic Theory, Photons. and Light. Lecture 7
Lecture 7 Chapter 3 Electromagnetic Theory, Photons. and Light Sources of light Emission of light by atoms The electromagnetic spectrum see supplementary material posted on the course website Electric
More informationChapter 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 informationElectrons, Energy, & the Electromagnetic Spectrum Notes
Electrons, Energy, & the Electromagnetic Spectrum Notes Bohr Model Diagram Interpretation What form of EM radiation is released when an electron in a hydrogen atom falls from the 5 th energy level to the
More informationc = l Light: The Cosmic Messenger 1/23/18
Reading for today s and Thur class: ASTR 1040 Stars & Galaxies SDO: Post-flare ejection from solar surface Prof. Juri Toomre TAs: Peri Johnson, Ryan Horton Lecture 3 Tues 23 Jan 2018 zeus.colorado.edu/astr1040-toomre
More informationThe Zeeman Effect in Atomic Mercury (Taryl Kirk )
The Zeeman Effect in Atomic Mercury (Taryl Kirk - 2001) Introduction A state with a well defined quantum number breaks up into several sub-states when the atom is in a magnetic field. The final energies
More information2. Electric Dipole Start from the classical formula for electric dipole radiation. de dt = 2. 3c 3 d 2 (2.1) qr (2.2) charges q
APAS 50. Internal Processes in Gases. Fall 999. Transition Probabilities and Selection Rules. Correspondence between Classical and Quantum Mechanical Transition Rates According to the correspondence principle
More informationSemiconductor Physics and Devices
Introduction to Quantum Mechanics In order to understand the current-voltage characteristics, we need some knowledge of electron behavior in semiconductor when the electron is subjected to various potential
More informationLight. October 14, ) Exam Review 2) Introduction 3) Light Waves 4) Atoms 5) Light Sources
Light October 14, 2002 1) Exam Review 2) Introduction 3) Light Waves 4) Atoms 5) Light Sources Waves You know of many types of waves water, sound, seismic, etc A wave is something oscillating back and
More informationX Rays must be viewed from space used for detecting exotic objects such as neutron stars and black holes also observing the Sun.
6/25 How do we get information from the telescope? 1. Galileo drew pictures. 2. With the invention of photography, we began taking pictures of the view in the telescope. With telescopes that would rotate
More informationB2.III Revision notes: quantum physics
B.III Revision notes: quantum physics Dr D.M.Lucas, TT 0 These notes give a summary of most of the Quantum part of this course, to complement Prof. Ewart s notes on Atomic Structure, and Prof. Hooker s
More informationPhysics GRE: Atomic Physics. G. J. Loges 1. University of Rochester Dept. of Physics & Astronomy. xkcd.com/658/
Physics GRE: Atomic Physics G. J. Loges 1 University of Rochester Dept. of Physics & Astronomy xkcd.com/658/ 1 c Gregory Loges, 2016 Contents 1 Bohr Model 1 2 Atomic Structure 1 3 Selection Rules 2 4 Blackbody
More informationMie vs Rayleigh. Sun
Mie vs Rayleigh Sun Chemists Probe Various Energy Levels of Molecules With Appropiate Energy Radiation It is convenient (and accurate enough for our purposes) to treat a molecule or system of molecules
More informationChapter 29: Maxwell s Equation and EM Waves. Slide 29-1
Chapter 29: Maxwell s Equation and EM Waves Slide 29-1 Equations of electromagnetism: a review We ve now seen the four fundamental equations of electromagnetism, here listed together for the first time.
More informationProperties of Light and Atomic Structure. Chapter 7. So Where are the Electrons? Electronic Structure of Atoms. The Wave Nature of Light!
Properties of Light and Atomic Structure Chapter 7 So Where are the Electrons? We know where the protons and neutrons are Nuclear structure of atoms (Chapter 2) The interaction of light and matter helps
More informationSpectral Resolution. Spectral resolution is a measure of the ability to separate nearby features in wavelength space.
Spectral Resolution Spectral resolution is a measure of the ability to separate nearby features in wavelength space. R, minimum wavelength separation of two resolved features. Delta lambda often set to
More informationψ s a ˆn a s b ˆn b ψ Hint: Because the state is spherically symmetric the answer can depend only on the angle between the two directions.
1. Quantum Mechanics (Fall 2004) Two spin-half particles are in a state with total spin zero. Let ˆn a and ˆn b be unit vectors in two arbitrary directions. Calculate the expectation value of the product
More informationChemistry 3502/4502. Final Exam Part I. May 14, 2005
Advocacy chit Chemistry 350/450 Final Exam Part I May 4, 005. For which of the below systems is = where H is the Hamiltonian operator and T is the kinetic-energy operator? (a) The free particle
More informationΨ t = ih Ψ t t. Time Dependent Wave Equation Quantum Mechanical Description. Hamiltonian Static/Time-dependent. Time-dependent Energy operator
Time Dependent Wave Equation Quantum Mechanical Description Hamiltonian Static/Time-dependent Time-dependent Energy operator H 0 + H t Ψ t = ih Ψ t t The Hamiltonian and wavefunction are time-dependent
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 informationSo far, we considered quantum static, as all our potentials did not depend on time. Therefore, our time dependence was trivial and always the same:
Lecture 20 Page 1 Lecture #20 L20.P1 Time-dependent perturbation theory So far, we considered quantum static, as all our potentials did not depend on time. Therefore, our time dependence was trivial and
More informationAtomic Structure Part II Electrons in Atoms
Atomic Structure Part II Electrons in Atoms Radiant energy travels in the form of waves that have both electrical and magnetic properties. These electromagnetic waves can travel through empty space, as
More information= λ. Light: The Cosmic Messenger. Continuing Topics for Today 1/24/17. Your account on Mastering Astronomy. ASTR 1040 Stars & Galaxies
REMINDER Your account on Mastering Astronomy ASTR 1040 Stars & Galaxies SDO: Post-flare ejection from solar surface Prof. Juri Toomre TAs: Piyush Agrawal, Connor Bice Lecture 3 Tues 24 Jan 2017 zeus.colorado.edu/astr1040-toomre
More informationChapter 4 Arrangement of Electrons in Atoms. 4.1 The Development of a New Atomic Model
Chapter 4 Arrangement of Electrons in Atoms 4.1 The Development of a New Atomic Model Properties of Light Electromagnetic Radiation: EM radiation are forms of energy which move through space as waves There
More informationCONTENTS. vii. CHAPTER 2 Operators 15
CHAPTER 1 Why Quantum Mechanics? 1 1.1 Newtonian Mechanics and Classical Electromagnetism 1 (a) Newtonian Mechanics 1 (b) Electromagnetism 2 1.2 Black Body Radiation 3 1.3 The Heat Capacity of Solids and
More informationUGC ACADEMY LEADING INSTITUE FOR CSIR-JRF/NET, GATE & JAM PHYSICAL SCIENCE TEST SERIES # 4. Atomic, Solid State & Nuclear + Particle
UGC ACADEMY LEADING INSTITUE FOR CSIR-JRF/NET, GATE & JAM BOOKLET CODE PH PHYSICAL SCIENCE TEST SERIES # 4 Atomic, Solid State & Nuclear + Particle SUBJECT CODE 05 Timing: 3: H M.M: 200 Instructions 1.
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 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 informationReview of Optical Properties of Materials
Review of Optical Properties of Materials Review of optics Absorption in semiconductors: qualitative discussion Derivation of Optical Absorption Coefficient in Direct Semiconductors Photons When dealing
More information