Energy levels and atomic structures lectures chapter one
|
|
- Mervyn Peter Barker
- 5 years ago
- Views:
Transcription
1 Structure of Atom An atom is the smallest constituent unit of ordinary matter that has the properties of a element. Every solid, liquid, gas, and plasma is composed of neutral or ionized atoms. Atoms are very small; typical sizes are around 100 pm (a ten-billionth of a meter, in the short scale). An atom consists of a small, dense nucleus at the center, surrounded by electrons which orbit the nucleus. The nucleus contains more than 99% of the mass of an atom, but concentrates in an extremely small volume A nucleus contains two types of particles: protons and neutrons A proton has a positive electric change, equal and opposite to that of an electron. A neutron, about the same mass of a proton, has no electric charge. An atom has no net electric charge Development of Atomic Models Thomson model In the nineteenth century, Thomson described the atom as a ball of positive charge containing a number of electrons. Rutherford s Atomic Model In the early twentieth century, Rutherford showed that most of an atom's mass is concentrated in a small, positively charged region called the nucleus. Rutherford proposed that an atom has a positively charged core (nucleus) surrounded by the negative electrons. 1
2 Bohr Atomic model After Rutherford's discovery, Bohr proposed that electrons travel in definite orbits around the nucleus. Quantum mechanical model Modern atomic theory described the electronic structure of the atom as the probability of finding electrons within certain regions of space. Bohr Model of the Atom Fundamental postulates: The Danish physicist Niels Bohr, who first presented this model of the atom, based it on 3 fundamental postulates. (1) Electrons move around the nucleus in circular non-radiating orbits - called stationary states. However, they are not at rest! (2) An atom only emits or absorbs electromagnetic radiation when an electron makes a transition from one state to another. 2
3 (3) Only certain stationary states are allowed: those where the orbital angular momentum of the electron is given by and h is Planck's constant. where n is an integer 1 (n = 1, 2, 3 etc.) This is known as the quantization of angular momentum. The equation implies that an integer number of wavelengths fit round the orbit: whence since,, (de Broglie relation) Sizes Of Allowed Orbits Classically, for an orbiting electron (mass m, charge -e and speed v), the centripetal force is balanced by the electric (Coulomb) force: Energies of Allowed Orbits 3
4 The minus sign means energy is required to remove the electron This energy is called the binding energy. Substituting for r from Equation above gives the energies of other allowed states: Quantum Numbers And Energy Levels 4
5 Normally, the electron is in the lowest state (n = 1), the ground state. It can gain energy from electromagnetic radiation, collisions with other atoms, etc. and be promoted into one of the higher levels, i.e. to an excited state of the atom. Note: the energy gained must equal the energy required. If the electron acquires energy > 13.6 ev, it is liberated from the atom altogether. The atom is ionized. Energy Conservation And Spectral Lines An electron in an excited state normally returns very quickly to its ground state, either directly or via an intermediate state When the electron moves from its initial E i to its final E f state, a photon is emitted (or absorbed, if E i < E f.) The energy of the photon emitted (or absorbed) is given by energy conservation For hydrogen [ ] : where n i and n f (with n i > n f ) are the quantum numbers of the initial and final states. Possible decays from an n = 3 excited atomic state: 5
6 All these transitions correspond to discrete photon energies. A series of sharp spectral lines are produced. All these lines are in the ultra-violet region of the emission spectrum. They are called the Lyman Series. Electrons from states with n i > 2 can return, initially, to the first-excited state (n f = 2), emitting one photon and then to the ground state emitting a second photon, with E ph = 10.2 ev, which is part of the Lyman series. Photons from transitions to the first-excited, (n = 2) state of the hydrogen atom form another series of spectral lines. This series is in the visible part of the spectrum from yellow, for the lowest energy, to violet for the highest energies. It is called the Balmer Series. Problems with the Bohr Model The Bohr model applies only to one electron atoms. The Bohr model doesn t account for the observed spectra of multielectron elements or ions. The movement of electrons in atoms is much less clearly defined than Bohr allowed. 6
7 The uncertainty principle (1927) The Heisenberg s uncertainty principle says that you cannot determine the position and momentum of an electron at the same time. only probability of finding an electron with a given energy a given space. ( )( ) ( )( ) properties of light Light has different colours. Light can travel through a vacuum. Light can be reflected and refracted, Classification of Electromagnetic Radiation Dual properties of Light: (1) waves and (2) particles Light is an electromagnetic radiation wave, e.g, Young s double slit experiment Light is also a particle-like packet of energy - photon Light particle is called photon The energy of phone is related to the wavelength of light 7
8 Light has a dual personality; it behaves as a stream of particle like photons, but each photon has wavelike properties Particles of light are called photons Each photon has a particular energy is Planck s constant this relationship between the energy of a photon and the frequency or wavelength of the wave. An Equation For Matter Waves? De Broglie postulated that every particles has an associated wave of wavelength. An equation for matter waves is : 8
9 where m is the mass of the particle and v its speed. Equation is known as the de Broglie relation and the wavelength λ of the matter wave is called de Broglie wavelength. The dual aspect of matter is evident in the de Broglie relation. On the left hand side of Eq, λ is the attribute of a wave while on the right hand side the momentum p is atypical attribute of a particle. Planck s constant h relates the two attributes. Wave-Particle Duality Of Light Evidence for wave-nature of light Diffraction and interference Evidence for particle-nature of light Photoelectric effect Compton effect Wave-Particle Duality Of Matter Based on the idea that light and all other electromagnetic Radiation may be considered a particle or a wave nature, Louis de Broglie suggested that the same kind of duality must be applicable to matter If electromagnetic radiation behaves as a particle, de Broglie reasoned, why couldn t a particle in motion, such as an electron, behave as a wave? : 9
10 Wave-Particle Duality Of Light The phenomena of reflection, refraction, interference and diffraction can all be explained using the idea of light as a wave motion. Furthermore, the fact that light can be polarised indicates that the waves are transverse. The photoelectric effect however, requires an explanation which considers light and all other electromagnetic radiation as a particle motion (i.e. consisting of discrete packets of energy called photons). Note All physical entities can be described as waves or particles. The two models are linked by the following relationships : Wave functions Schrödinger: Replace the precise trajectory of particles by a wave function mathematical function that varies with position., a 10
11 physical interpretation of wave functions. Probability of finding a particle in a region is proportional to. Quantum mechanics acknowledges the wave-particle duality of matter by supposing that, a particle is distributed through space like a wave, rather than traveling along a definite path. The wave that in quantum mechanics replaces the classical concept of particle trajectory is called a wave function, ( psi ). Wave functions, are mathematical descriptions of the motion of electron waves as they vary with location and with time. is the probability density. To calculate the probability that a particle is in a small region in space multiply y 2 by the volume of the region. ( ) 11
Planck 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 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 informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change Chapter 5: Electrons in Atoms 5 Section 5.1 Section Section 5.3 Table Of Contents Light and Quantized Energy Electron Configuration Compare the wave and particle natures of
More informationLecture 11 Atomic Structure
Lecture 11 Atomic Structure Earlier in the semester, you read about the discoveries that lead to the proposal of the nuclear atom, an atom of atomic number Z, composed of a positively charged nucleus surrounded
More informationChapter 6: The Electronic Structure of the Atom Electromagnetic Spectrum. All EM radiation travels at the speed of light, c = 3 x 10 8 m/s
Chapter 6: The Electronic Structure of the Atom Electromagnetic Spectrum V I B G Y O R All EM radiation travels at the speed of light, c = 3 x 10 8 m/s Electromagnetic radiation is a wave with a wavelength
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 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 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 informationSECTION 2: QUANTUM THEORY AND THE ATOM CHAPTER 9: ELECTRONS IN ATOMS AND THE PERIODIC TABLE
SECTION 2: QUANTUM THEORY AND THE ATOM CHAPTER 9: ELECTRONS IN ATOMS AND THE PERIODIC TABLE Learning Goals Compare the Bohr and quantum mechanical models of the atom. Explain the impact of de Broglie s
More informationStellar Astrophysics: The Interaction of Light and Matter
Stellar Astrophysics: The Interaction of Light and Matter The Photoelectric Effect Methods of electron emission Thermionic emission: Application of heat allows electrons to gain enough energy to escape
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 informationSCH4U: History of the Quantum Theory
SCH4U: History of the Quantum Theory Black Body Radiation When an object is heated, it initially glows red hot and at higher temperatures becomes white hot. This white light must consist of all of the
More informationEarly Quantum Theory & Models of the Atom (Ch 27) Discovery of electron. Blackbody Radiation. Blackbody Radiation. J. J. Thomson ( )
Early Quantum Theory & Models of the Atom (Ch 27) Discovery of electron Modern physics special relativity quantum theory J. J. Thomson (1856-1940) measured e/m directly set-up was similar to mass spectrometer
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 7 Atomic Structure -1 Quantum Model of Atom. Dr. Sapna Gupta
Chapter 7 Atomic Structure -1 Quantum Model of Atom Dr. Sapna Gupta The Electromagnetic Spectrum The electromagnetic spectrum includes many different types of radiation which travel in waves. Visible light
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 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 informationChapter 6 Electronic structure of atoms
Chapter 6 Electronic structure of atoms light photons spectra Heisenberg s uncertainty principle atomic orbitals electron configurations the periodic table 6.1 The wave nature of light Visible light is
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 7. The Quantum- Mechanical Model of the Atom. Chapter 7 Lecture Lecture Presentation. Sherril Soman Grand Valley State University
Chapter 7 Lecture Lecture Presentation Chapter 7 The Quantum- Mechanical Model of the Atom Sherril Soman Grand Valley State University The Beginnings of Quantum Mechanics Until the beginning of the twentieth
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 informationCHAPTER 4. Arrangement of Electrons in Atoms
CHAPTER 4 Arrangement of Electrons in Atoms 4.1 Part I Development of a New Atomic Model 4.1 Objectives 1. Explain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic
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 informationYellow. Strontium red white. green. yellow violet. green. red. Chapter 4. Arrangement of Electrons in Atoms. Table of Contents
Chapter 4 Arrangement of Electrons in Atoms Table of Contents Section 1 Section 2 Section 3 The Development of a New Atomic Model The Quantum Model of the Atom Electron Configurations Sodium Yellow Strontium
More informationProperties of Light. Arrangement of Electrons in Atoms. The Development of a New Atomic Model. Electromagnetic Radiation CHAPTER 4
CHAPTER 4 Arrangement of Electrons in Atoms The Development of a New Atomic Model The Rutherford model was a great improvement over the Thomson model of the atom. But, there was one major question that
More informationAtomic Structure and the Periodic Table
Atomic Structure and the Periodic Table The electronic structure of an atom determines its characteristics Studying atoms by analyzing light emissions/absorptions Spectroscopy: analysis of light emitted
More informationQuantum Theory of the Atom
The Wave Nature of Light Quantum Theory of the Atom Electromagnetic radiation carries energy = radiant energy some forms are visible light, x rays, and radio waves Wavelength ( λ) is the distance between
More informationThe Photoelectric Effect
The Photoelectric Effect Light can strike the surface of some metals causing an electron to be ejected No matter how brightly the light shines, electrons are ejected only if the light has sufficient energy
More informationLecture 6 - Atomic Structure. Chem 103, Section F0F Unit II - Quantum Theory and Atomic Structure Lecture 6. Lecture 6 - Introduction
Chem 103, Section F0F Unit II - Quantum Theory and Atomic Structure Lecture 6 Light and other forms of electromagnetic radiation Light interacting with matter The properties of light and matter Lecture
More informationChapter 7 QUANTUM THEORY & ATOMIC STRUCTURE Brooks/Cole - Thomson
Chapter 7 QUANTUM THEORY & ATOMIC STRUCTURE 1 7.1 The Nature of Light 2 Most subatomic particles behave as PARTICLES and obey the physics of waves. Light is a type of electromagnetic radiation Light consists
More informationCh 7 Quantum Theory of the Atom (light and atomic structure)
Ch 7 Quantum Theory of the Atom (light and atomic structure) Electromagnetic Radiation - Electromagnetic radiation consists of oscillations in electric and magnetic fields. The oscillations can be described
More informationI understand the relationship between energy and a quanta I understand the difference between an electron s ground state and an electron s excited
NCCS 1.1.2 & 1.1.3 I understand the relationship between energy and a quanta I understand the difference between an electron s ground state and an electron s excited state I will describe how an electron
More informationThe Photoelectric Effect
Stellar Astrophysics: The Interaction of Light and Matter The Photoelectric Effect Methods of electron emission Thermionic emission: Application of heat allows electrons to gain enough energy to escape
More informationPreview. Atomic Physics Section 1. Section 1 Quantization of Energy. Section 2 Models of the Atom. Section 3 Quantum Mechanics
Atomic Physics Section 1 Preview Section 1 Quantization of Energy Section 2 Models of the Atom Section 3 Quantum Mechanics Atomic Physics Section 1 TEKS The student is expected to: 8A describe the photoelectric
More informationPhysics 126 Practice Exam #4 Professor Siegel
Physics 126 Practice Exam #4 Professor Siegel Name: Lab Day: 1. Light is usually thought of as wave-like in nature and electrons as particle-like. In which one of the following instances does light behave
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 informationPhysical Electronics. First class (1)
Physical Electronics First class (1) Bohr s Model Why don t the electrons fall into the nucleus? Move like planets around the sun. In circular orbits at different levels. Amounts of energy separate one
More informationElectrons in Atoms. Section 5.1 Light and Quantized Energy Section 5.2 Quantum Theory and the Atom Section 5.3 Electron Configuration
Electrons in Atoms Section 5.1 Light and Quantized Energy Section 5.2 Quantum Theory and the Atom Section 5.3 Electron Configuration Click a hyperlink or folder tab to view the corresponding slides. Exit
More informationWAVE NATURE OF LIGHT
WAVE NATURE OF LIGHT Light is electromagnetic radiation, a type of energy composed of oscillating electric and magnetic fields. The fields oscillate perpendicular to each other. In vacuum, these waves
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 informationLecture PowerPoints. Chapter 27 Physics: Principles with Applications, 7th edition Giancoli
Lecture PowerPoints Chapter 27 Physics: Principles with Applications, 7th edition Giancoli This work is protected by United States copyright laws and is provided solely for the use of instructors in teaching
More informationSECTION A Quantum Physics and Atom Models
AP Physics Multiple Choice Practice Modern Physics SECTION A Quantum Physics and Atom Models 1. Light of a single frequency falls on a photoelectric material but no electrons are emitted. Electrons may
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 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 informationTable of Contents Electrons in Atoms > Light and Quantized Energy > Quantum Theory and the Atom > Electron Configuration
Electrons in Atoms October 20, 2014 Table of Contents Electrons in Atoms > Light and Quantized Energy > Quantum Theory and the Atom > Electron Configuration 1 Electromagnetic Spectrum Electromagnetic radiation
More informationThe Atom. Result for Hydrogen. For example: the emission spectrum of Hydrogen: Screen. light. Hydrogen gas. Diffraction grating (or prism)
The Atom What was know about the atom in 1900? First, the existence of atoms was not universally accepted at this time, but for those who did think atoms existed, they knew: 1. Atoms are small, but they
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 informationConceptual Physics Fundamentals
Conceptual Physics Fundamentals Chapter 15: QUANTUM THEORY This lecture will help you understand: The Photoelectric Effect Absorption Spectra Fluorescence Incandescence Lasers Wave-Particle Duality Particles
More informationLesson 11: Quantum Model of the Atom. See portions of Chapter 4 Section 2 of your textbook (pp )
Lesson 11: Quantum Model of the Atom See portions of Chapter 4 Section 2 of your textbook (pp 98-104) Atomic Models J.J. Thompson discovery of the electron, electrons in all atoms Millikan confirmed negative
More informationChapter 6. Electronic Structure of Atoms
Chapter 6 Electronic Structure of Atoms 6.1 The Wave Nature of Light Made up of electromagnetic radiation. Waves of electric and magnetic fields at right angles to each other. Parts of a wave Wavelength
More informationHistorical Background of Quantum Mechanics
Historical Background of Quantum Mechanics The Nature of Light The Structure of Matter Dr. Sabry El-Taher 1 The Nature of Light Dr. Sabry El-Taher 2 In 1801 Thomas Young: gave experimental evidence for
More informationElectronic structure the number of electrons in an atom as well as the distribution of electrons around the nucleus and their energies
Chemistry: The Central Science Chapter 6: Electronic Structure of Atoms Electronic structure the number of electrons in an atom as well as the distribution of electrons around the nucleus and their energies
More information298 Chapter 6 Electronic Structure and Periodic Properties of Elements
98 Chapter 6 Electronic Structure and Periodic Properties of Elements 6. The Bohr Model By the end of this section, you will be able to: Describe the Bohr model of the hydrogen atom Use the Rydberg equation
More informationMystery #3 Emission Spectra of Elements. Tube filled with elemental gas. Voltage can be applied across both ends, this causes the gas to emit light
Mystery #3 Emission Spectra of Elements Tube filled with elemental gas. Voltage can be applied across both ends, this causes the gas to emit light Line Spectra Copyright The McGraw-Hill Companies, Inc.
More informationChapter 6. Quantum Theory and the Electronic Structure of Atoms Part 1
Chapter 6 Quantum Theory and the Electronic Structure of Atoms Part 1 The nature of light Quantum theory Topics Bohr s theory of the hydrogen atom Wave properties of matter Quantum mechanics Quantum numbers
More informationChapter 7. The Quantum Mechanical Model of the Atom
Chapter 7 The Quantum Mechanical Model of the Atom The Nature of Light:Its Wave Nature Light is a form of electromagnetic radiation composed of perpendicular oscillating waves, one for the electric field
More informationEarlier we learned that hot, opaque objects produce continuous spectra of radiation of different wavelengths.
Section7: The Bohr Atom Earlier we learned that hot, opaque objects produce continuous spectra of radiation of different wavelengths. Continuous Spectrum Everyone has seen the spectrum produced when white
More informationOutline Chapter 9 The Atom Photons Photons The Photoelectron Effect Photons Photons
Outline Chapter 9 The Atom 9-1. Photoelectric Effect 9-3. What Is Light? 9-4. X-rays 9-5. De Broglie Waves 9-6. Waves of What? 9-7. Uncertainty Principle 9-8. Atomic Spectra 9-9. The Bohr Model 9-10. Electron
More informationElectronic structure of atoms
Chapter 1 Electronic structure of atoms light photons spectra Heisenberg s uncertainty principle atomic orbitals electron configurations the periodic table 1.1 The wave nature of light Much of our understanding
More informationChapter 6. Electronic Structure of Atoms. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 6 John D. Bookstaver St. Charles Community College Cottleville, MO Waves To understand the electronic structure of atoms, one must understand the nature of electromagnetic
More informationElectronic Structure. of Atoms. 2009, Prentice-Hall, Inc. Electronic Structure. of Atoms. 2009, Prentice-Hall, Inc. Electronic Structure.
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 6 Section 1 6: The Marathon Adapted from: John D. Bookstaver St. Charles Community College
More informationThe Wave Nature of Light Made up of. Waves of fields at right angles to each other. Wavelength = Frequency =, measured in
Chapter 6 Electronic Structure of Atoms The Wave Nature of Light Made up of. Waves of fields at right angles to each other. Wavelength = Frequency =, measured in Kinds of EM Waves There are many different
More informationLearning Objectives and Worksheet I. Chemistry 1B-AL Fall 2016
Learning Objectives and Worksheet I Chemistry 1B-AL Fall 2016 Lectures (1 2) Nature of Light and Matter, Quantization of Energy, and the Wave Particle Duality Read: Chapter 12, Pages: 524 526 Supplementary
More informationAtomic Structure Discovered. Dalton s Atomic Theory. Discovery of the Electron 10/30/2012
Atomic Structure Discovered Ancient Greeks Democritus (460-362 BC) - indivisible particles called atoms Prevailing argument (Plato and Aristotle) - matter is continuously and infinitely divisible John
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 informationWe also find the development of famous Schrodinger equation to describe the quantization of energy levels of atoms.
Lecture 4 TITLE: Quantization of radiation and matter: Wave-Particle duality Objectives In this lecture, we will discuss the development of quantization of matter and light. We will understand the need
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 informationChemistry is in the electrons
Chemistry is in the electrons Electronic structure arrangement of electrons in atom Two parameters: Energy Position The popular image of the atom is incorrect: electrons are not miniature planets orbiting
More informationc = λν 10/23/13 What gives gas-filled lights their colors? Chapter 5 Electrons In Atoms
CHEMISTRY & YOU What gives gas-filled lights their colors? Chapter 5 Electrons In Atoms 5.1 Revising the Atomic Model 5. Electron Arrangement in Atoms 5.3 Atomic and the Quantum Mechanical Model An electric
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 informationProblems with the atomic model?
Modern Atomic Theory- Electronic Structure of Atoms DR HNIMIR-CH7 Where should (-) electrons be found? Problems with the atomic model? First, a Little About Electromagnetic Radiation- Waves Another Look
More informationLine spectrum (contd.) Bohr s Planetary Atom
Line spectrum (contd.) Hydrogen shows lines in the visible region of the spectrum (red, blue-green, blue and violet). The wavelengths of these lines can be calculated by an equation proposed by J. J. Balmer:
More informationQUANTUM MECHANICS Chapter 12
QUANTUM MECHANICS Chapter 12 Colours which appear through the Prism are to be derived from the Light of the white one Sir Issac Newton, 1704 Electromagnetic Radiation (prelude) FIG Electromagnetic Radiation
More informationQuantum Theory of Light
King Saud University College of Applied Studies and Community Service Department of Natural Sciences Quantum Theory of Light General Physics II PHYS 111 Nouf Alkathran nalkathran@ksu.edu.sa Outline Definition
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 informationChapter 7. The Quantum Mechanical Model of the Atom
Chapter 7 The Quantum Mechanical Model of the Atom Quantum Mechanics The Behavior of the Very Small Electrons are incredibly small. Electron behavior determines much of the behavior of atoms. Directly
More informationAP Physics Study Guide Modern Physics I. Atomic Physics and Quantum Effects 1. Who is generally credited with the discovery of the electron?
AP Physics Study Guide Modern Physics I. Atomic Physics and Quantum Effects 1. Who is generally credited with the discovery of the electron? 2. What was it that J. J. Thomson actually measured? 3. Regarding
More informationCHM 111 Unit 7 Sample Questions
Name: Class: Date: As you work these problems, consider and explain: A. What type of question is it? B. How do you know what type of question it is? C. What information are you looking for? D. What information
More informationChapter 6: Electronic Structure of Atoms
Chapter 6: Electronic Structure of Atoms Learning Outcomes: Calculate the wavelength of electromagnetic radiation given its frequency or its frequency given its wavelength. Order the common kinds of radiation
More informationChapter 4. Table of Contents. Section 1 The Development of a New Atomic Model. Section 2 The Quantum Model of the Atom
Arrangement of Electrons in Atoms Table of Contents Section 1 The Development of a New Atomic Model Section 2 The Quantum Model of the Atom Section 3 Electron Configurations Section 1 The Development of
More informationCHEMISTRY. Chapter 6 Electronic Structure of Atoms
CHEMISTRY The Central Science 8 th Edition Chapter 6 Electronic Structure of Atoms Kozet YAPSAKLI Who are these men? Ancient Philosophy Who: Aristotle, Democritus When: More than 2000 years ago Where:
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 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 informationI. Multiple Choice Questions (Type-I)
I. Multiple Choice Questions (Type-I) 1. Which of the following conclusions could not be derived from Rutherford s α -particle scattering experiement? (i) Most of the space in the atom is empty. (ii) The
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 information29:006 FINAL EXAM FRIDAY MAY 11 3:00 5:00 PM IN LR1 VAN
L 33 Modern Physics [1] 29:006 FINAL EXAM FRIDAY MAY 11 3:00 5:00 PM IN LR1 VAN Introduction- quantum physics Particles of light PHOTONS The photoelectric effect Photocells & intrusion detection devices
More informationTHE EDUCARE (SIROHI CLASSES) TEST SERIES 2018
THE EDUCARE (SIROHI CLASSES) TEST SERIES 2018 XII PHYSICS TEST MODERN PHYSICS NAME-... DATE-.. MM- 25 TIME-1 HR 1) Write one equation representing nuclear fusion reaction. (1) 2) Arrange radioactive radiations
More informationAtomic Structure and Periodicity. AP Chemistry Ms. Grobsky
Atomic Structure and Periodicity AP Chemistry Ms. Grobsky Food For Thought Rutherford s model became known as the planetary model The sun was the positivelycharged dense nucleus and the negatively-charged
More informationAtomic Structure and Periodicity
p. 99 p. 98 p. 98 Electromagnetic Spectrum Image Atomic Structure and Periodicity Chemistry Zumdahl Chapter 7 Properties of Light Electromagnetic Radiation: a form of energy that exhibits wavelike behavior
More informationAn electron can be liberated from a surface due to particle collisions an electron and a photon.
Quantum Theory and the Atom the Bohr Atom The story so far... 1. Einstein argued that light is a photon (particle) and each photon has a discrete amount of energy associated with it governed by Planck's
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 informationChapter 8: Electrons in Atoms Electromagnetic Radiation
Chapter 8: Electrons in Atoms Electromagnetic Radiation Electromagnetic (EM) radiation is a form of energy transmission modeled as waves moving through space. (see below left) Electromagnetic Radiation
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 informationPhysics 1C Lecture 29B
Physics 1C Lecture 29B Emission Spectra! The easiest gas to analyze is hydrogen gas.! Four prominent visible lines were observed, as well as several ultraviolet lines.! In 1885, Johann Balmer, found a
More informationElectromagnetic Radiation All electromagnetic radiation travels at the same velocity: the speed of light (c), m/s.
Chapter 6 Electronic Structure of Atoms Waves To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation. The distance between corresponding points on
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 informationLight. October 16, Chapter 5: Electrons in Atoms Honors Chemistry. Bohr Model
Chapter 5: Electrons in Atoms Honors Chemistry Bohr Model Niels Bohr, a young Danish physicist and a student of Rutherford improved Rutherford's model. Bohr proposed that an electron is found only in specific
More informationLecture 4. The Bohr model of the atom. De Broglie theory. The Davisson-Germer experiment
Lecture 4 The Bohr model of the atom De Broglie theory The Davisson-Germer experiment Objectives Learn about electron energy levels in atoms and how Bohr's model can be used to determine the energy levels
More informationThe Electron Cloud. Here is what we know about the electron cloud:
The Electron Cloud Here is what we know about the electron cloud: It contains the subatomic particles called electrons This area accounts for most of the volume of the atom ( empty space) These electrons
More informationModern Atomic Theory
Modern Atomic Theory In science, often times chemical or physical behavior can not be seen with the naked eye (nor with the use of some other device). Consequently, an understanding and explanation of
More information