CHAPTER 28 Quantum Mechanics of Atoms Units
|
|
- Colin Hood
- 5 years ago
- Views:
Transcription
1 CHAPTER 28 Quantum Mechanics of Atoms Units Quantum Mechanics A New Theory The Wave Function and Its Interpretation; the Double-Slit Experiment The Heisenberg Uncertainty Principle Philosophic Implications; Probability versus Determinism Quantum-Mechanical View of Atoms Quantum Mechanics of the Hydrogen Atom; Quantum Numbers Complex Atoms; the Exclusion Principle The Periodic Table of Elements X-Ray Spectra and Atomic Number Quantum Mechanics A New Theory Quantum mechanics incorporates wave-particle duality, and successfully explains energy states in complex atoms and molecules, the relative brightness of spectral lines, and many other phenomena. It is widely accepted as being the fundamental theory underlying all physical processes. Quantum mechanics is essential to understanding atoms and molecules, but can also have effects on larger scales. The Wave Function and Its Interpretation; the Double-Slit Experiment An electromagnetic wave has oscillating electric and magnetic fields. What is oscillating in a matter wave? This role is played by the wave function, Ψ. The square of the wave function at any point is proportional to the number of electrons expected to be found there. For a single electron, the wave function is the probability of finding the electron at that point. For example: the interference pattern is observed after many electrons have gone through the slits. If we send the electrons through one at a time, we cannot predict the path any single electron will take, but we can predict the overall distribution. 1
2 Werner Heisenberg Developed an abstract mathematical model to explain wavelengths of spectral lines Called matrix mechanics Other contributions Uncertainty Principle Nobel Prize in 1932 Atomic and nuclear models Forms of molecular hydrogen The Heisenberg Uncertainty Principle Combining, we find the combination of uncertainties: Quantum mechanics tells us there are limits to measurement not because of the limits of our instruments, but inherently. This is due to the wave-particle duality, and to interaction between the observing equipment and the object being observed. Imagine trying to see an electron with a powerful microscope. At least one photon must scatter off the electron and enter the microscope, but in doing so it will transfer some of its momentum to the electron. The uncertainty in the momentum of the electron is taken to be the momentum of the photon it could transfer anywhere from none to all of its momentum. In addition, the position can only be measured to about one wavelength of the photon. This is called the Heisenberg uncertainty principle. It tells us that the position and momentum cannot simultaneously be measured with precision. This relation can also be written as a relation between the uncertainty in time and the uncertainty in energy: This says that if an energy state only lasts for a limited time, its energy will be uncertain. It also says that conservation of energy can be violated if the time is short enough. 2
3 6 Example 1: An electron moves in a straight line with a constant speed v 1.10x10 m/ s which has been measured to a precision of 0.10%. What is the maximum precision with which its position could be simultaneously measured? p mv (9.11x10 kg)(1.10 x10 m/ s) 1.00x10 kg m/ s 27 The uncertainty is 10% - or p 1.0x10 kg m/ s 34 h 1.06x10 J s 7 x 1.1x10 m 27 p 1.0x10 kg m / s Example 2: What is the uncertainty in position, imposed by the uncertainty principle, on a 150-g baseball thrown at (42 1) m/ s? The uncertainty in speed is v 1 m / s p m v (0.150 kg)(1 m / s) 0.15 kg m / s 34 h 1.06x10 J s 34 x 7x10 m p.15 kg m / s Philosophic Implications; Probability versus Determinism The world of Newtonian mechanics is a deterministic one. If you know the forces on an object and its initial velocity, you can predict where it will go. Quantum mechanics is very different you can predict what masses of electrons will do, but have no idea what any individual one will. Quantum-Mechanical View of Atoms Since we cannot say exactly where an electron is, the Bohr picture of the atom, with electrons in neat orbits, cannot be correct. Quantum theory describes an electron probability distribution; this figure shows the distribution for the ground state of hydrogen: Quantum Mechanics of the Hydrogen Atom; Quantum Numbers There are four different quantum numbers needed to specify the state of an electron in an atom. 1. Principal quantum number n gives the total energy: 3
4 2. Orbital quantum number l gives the angular momentum; l can take on integer values from 0 to n The magnetic quantum number, m l, gives the direction of the electron s angular momentum, and can take on integer values from l to +l. This plot indicates the quantization of angular momentum direction for l = 2. The other two components of the angular momentum are undefined. 4. The spin quantum number, m s, this for an electron can take on the values +½ and -½. The need for this quantum number was found by experiment; spin is an intrinsically quantum mechanical quantity, although it mathematically behaves as a form of angular momentum. This table summarizes the four quantum numbers. The angular momentum quantum numbers do not affect the energy level much, but they do change the spatial distribution of the electron cloud. 4
5 Allowed transitions between energy levels occur between states whose value of l differ by one: Other, forbidden, transitions also occur but with much lower probability. Complex Atoms; the Exclusion Principle Complex atoms contain more than one electron, so the interaction between electrons must be accounted for in the energy levels. This means that the energy depends on both n and l. A neutral atom has Z electrons, as well as Z protons in its nucleus. Z is called the atomic number. Wolfgang Pauli Contributions include Major review of relativity Exclusion Principle Connect between electron spin and statistics Theories of relativistic quantum electrodynamics Neutrino hypothesis Nuclear spin hypothesis Complex Atoms; the Exclusion Principle In order to understand the electron distributions in atoms, another principle is needed. This is the Pauli Exclusion Principle: No two electrons in an atom can occupy the same quantum state. The quantum state is specified by the four quantum numbers; no two electrons can have the same set. This chart shows the occupied and some unoccupied states in He, Li, and Na. 5
6 Filling Shells As a general rule, the order that electrons fill an atom s subshell is: Once one subshell is filled, the next electron goes into the vacant subshell that is lowest in energy Otherwise, the electron would radiate energy until it reached the subshell with the lowest energy A subshell is filled when it holds 2(2l+1) electrons The Periodic Table The outermost electrons are primarily responsible for the chemical properties of the atom Mendeleev arranged the elements according to their atomic masses and chemical similarities The electronic configuration of the elements explained by quantum numbers and Pauli s Exclusion Principle explains the configuration Example 3: High-energy photons are used to bombard an unknown material. The strongest peak is found for X-rays emitted with energy of 66keV. Guess what the material is. The hydrogen transition n = 2 to n = 1 would yield about 10.2eV. Energy E is proportional to 2 2 Z or ( Z 1) because the nucleus is shielded by the one electron in a 1s state. So: ( 1) Z x ev eV 6.5x10 Z , and Z 82( lead ) 3 Example 4: What is the shortest wavelength X-ray photon emitted in an X-ray tube subjected to 50kV? 34 8 hc (6.63x10 J s)(3.0x10 m / s) 11 o 2.5x10 m 19 4 ev (1.6x10 C)(5.0x10 V ) So: 0.025nm 6
Chapter 38 Quantum Mechanics
Chapter 38 Quantum Mechanics Units of Chapter 38 38-1 Quantum Mechanics A New Theory 37-2 The Wave Function and Its Interpretation; the Double-Slit Experiment 38-3 The Heisenberg Uncertainty Principle
More informationA more comprehensive theory was needed. 1925, Schrödinger and Heisenberg separately worked out a new theory Quantum Mechanics.
Ch28 Quantum Mechanics of Atoms Bohr s model was very successful to explain line spectra and the ionization energy for hydrogen. However, it also had many limitations: It was not able to predict the line
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 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 informationChapter 28. Atomic Physics
Chapter 28 Atomic Physics Bohr s Correspondence Principle Bohr s Correspondence Principle states that quantum mechanics is in agreement with classical physics when the energy differences between quantized
More informationChapter 28 Quantum Mechanics of Atoms
Chapter 28 Quantum Mechanics of Atoms 28.1 Quantum Mechanics The Theory Quantum mechanics incorporates wave-particle duality, and successfully explains energy states in complex atoms and molecules, the
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 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 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 informationFinal Exam Tuesday, May 8, 2012 Starting at 8:30 a.m., Hoyt Hall Duration: 2h 30m
Final Exam Tuesday, May 8, 2012 Starting at 8:30 a.m., Hoyt Hall. ------------------- Duration: 2h 30m Chapter 39 Quantum Mechanics of Atoms Units of Chapter 39 39-1 Quantum-Mechanical View of Atoms 39-2
More informationBohr s Correspondence Principle
Bohr s Correspondence Principle In limit that n, quantum mechanics must agree with classical physics E photon = 13.6 ev 1 n f n 1 i = hf photon In this limit, n i n f, and then f photon electron s frequency
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 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 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 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 informationQuantum Mechanics of Atoms
Quantum Mechanics of Atoms Your theory is crazy, but it's not crazy enough to be true N. Bohr to W. Pauli Quantum Mechanics of Atoms 2 Limitations of the Bohr Model The model was a great break-through,
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 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 informationThe Electronic Structures of Atoms Electromagnetic Radiation The wavelength of electromagnetic radiation has the symbol λ.
CHAPTER 7 Atomic Structure Chapter 8 Atomic Electron Configurations and Periodicity 1 The Electronic Structures of Atoms Electromagnetic Radiation The wavelength of electromagnetic radiation has the symbol
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 informationFinal Exam. Tuesday, May 8, Starting at 8:30 a.m., Hoyt Hall.
Final Exam Tuesday, May 8, 2012 Starting at 8:30 a.m., Hoyt Hall. Summary of Chapter 38 In Quantum Mechanics particles are represented by wave functions Ψ. The absolute square of the wave function Ψ 2
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 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 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 informationPart One: Light Waves, Photons, and Bohr Theory. 2. Beyond that, nothing was known of arrangement of the electrons.
CHAPTER SEVEN: QUANTUM THEORY AND THE ATOM Part One: Light Waves, Photons, and Bohr Theory A. The Wave Nature of Light (Section 7.1) 1. Structure of atom had been established as cloud of electrons around
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 informationDevelopment of the Periodic Table. Chapter 5. Light and the EM Spectrum. Light
Chapter 5 Periodic Table Song Periodicity and Atomic Structure Development of the Periodic Table Mid-1800 s, several scientists placed known elements in order based on different criteria. Mendeleev s and
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 informationCOLLEGE PHYSICS. Chapter 30 ATOMIC PHYSICS
COLLEGE PHYSICS Chapter 30 ATOMIC PHYSICS Matter Waves: The de Broglie Hypothesis The momentum of a photon is given by: The de Broglie hypothesis is that particles also have wavelengths, given by: Matter
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 informationStructure of the atom
Structure of the atom What IS the structure of an atom? What are the properties of atoms? REMEMBER: structure affects function! Important questions: Where are the electrons? What is the energy of an electron?
More informationElectronic Structure of Atoms. Chapter 6
Electronic Structure of Atoms Chapter 6 Electronic Structure of Atoms 1. The Wave Nature of Light All waves have: a) characteristic wavelength, λ b) amplitude, A Electronic Structure of Atoms 1. The Wave
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 informationChapter 12: Phenomena
Chapter 12: Phenomena K Fe Phenomena: Different wavelengths of electromagnetic radiation were directed onto two different metal sample (see picture). Scientists then recorded if any particles were ejected
More informationUNIT 4 Electrons in Atoms. Advanced Chemistry 235 Lanphier High School Mr. David Peeler
UNIT 4 Electrons in Atoms Advanced Chemistry 235 Lanphier High School Mr. David Peeler Section 4.1 Models of the Atom OBJECTIVES: Identify the inadequacies in the Rutherford atomic model. Section 4.1 Models
More informationExplain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic radiation.
Preview Objectives Properties of Light Wavelength and Frequency The Photoelectric Effect The Hydrogen-Atom Line-Emission Spectrum Bohr Model of the Hydrogen Atom Photon Emission and Absorption Section
More informationCHAPTER 5. The Structure of Atoms
CHAPTER 5 The Structure of Atoms Chapter Outline Subatomic Particles Fundamental Particles The Discovery of Electrons Canal Rays and Protons Rutherford and the Nuclear Atom Atomic Number Neutrons Mass
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 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 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 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 informationCHAPTER STRUCTURE OF ATOM
12 CHAPTER STRUCTURE OF ATOM 1. The spectrum of He is expected to be similar to that [1988] H Li + Na He + 2. The number of spherical nodes in 3p orbitals are [1988] one three none two 3. If r is the radius
More informationQuantum Mechanics & Atomic Structure (Chapter 11)
Quantum Mechanics & Atomic Structure (Chapter 11) Quantum mechanics: Microscopic theory of light & matter at molecular scale and smaller. Atoms and radiation (light) have both wave-like and particlelike
More informationRecall the Goal. What IS the structure of an atom? What are the properties of atoms?
Recall the Goal What IS the structure of an atom? What are the properties of atoms? REMEMBER: structure affects function! Important questions: Where are the electrons? What is the energy of an electron?
More informationPHYSICS 102N Spring Week 12 Quantum Mechanics and Atoms
PHYSICS 102N Spring 2009 Week 12 Quantum Mechanics and Atoms Quantum Mechanics 1. All objects can be represented by waves describing their propagation through space 2. The wave length is λ=h/p and frequency
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 informationLecture PowerPoint. Chapter 28 Physics: Principles with Applications, 6 th edition Giancoli
Lecture PowerPoint Chapter 28 Physics: Principles with Applications, 6 th edition Giancoli 2005 Pearson Prentice Hall This work is protected by United States copyright laws and is provided solely for the
More informationAtomic Structure Chapter 4
Atomic Structure Chapter 4 Outline A History of the Atomic Model Electron Structure of the Atom Useful Element Notations Early Thoughts on the Structure of Matter Before the invention of high powered microscopes,
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 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 informationSparks CH301. Quantum Mechanics. Waves? Particles? What and where are the electrons!? UNIT 2 Day 3. LM 14, 15 & 16 + HW due Friday, 8:45 am
Sparks CH301 Quantum Mechanics Waves? Particles? What and where are the electrons!? UNIT 2 Day 3 LM 14, 15 & 16 + HW due Friday, 8:45 am What are we going to learn today? The Simplest Atom - Hydrogen Relate
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 informationChapter 7. Wave Behavior of Electrons
Chapter 7 Wave Behavior of Electrons 2-Slit Interference If electrons behave only like particles, there should only be two bright spots on the target However, electrons actually present an interference
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 informationQuantum Theory and the Electronic Structure of Atoms
Quantum Theory and the Electronic Structure of Atoms Chapter 7 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Properties of Waves Wavelength ( ) is the distance
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 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 informationChapter 7 The Quantum-Mechanical Model of the Atom
Chapter 7 The Quantum-Mechanical Model of the Atom Electron Energy electron energy and position are complimentary because KE = ½mv 2 for an electron with a given energy, the best we can do is describe
More informationPHYSICS DOUGLAS C. GIANCOLI
S EVE N T H PHYSICS E DI T I O N PRINCIPLES WITH APPLICATIONS DOUGLAS C. GIANCOLI Boston Columbus Indianapolis New York San Francisco Upper Saddle River Amsterdam Cape Town Dubai London Madrid Milan Munich
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 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 informationChapter 7 Problems: 16, 17, 19 23, 26, 27, 30, 31, 34, 38 41, 45, 49, 53, 60, 61, 65, 67, 75, 79, 80, 83, 87, 90, 91, 94, 95, 97, 101, 111, 113, 115
Chapter 7 Problems: 16, 17, 19 23, 26, 27, 30, 31, 34, 38 41, 45, 49, 53, 60, 61, 65, 67, 75, 79, 80, 83, 87, 90, 91, 94, 95, 97, 101, 111, 113, 115 117, 121, 122, 125a Chapter 7 Atomic Structure and Periodicity
More informationChapter 8. Structure of Atom
Chapter 8 Structure of Atom Synopsis Energy propagates as electromagnetic waves and can have a wide variety of wavelengths. The entire range of wavelengths is known as the electromagnetic spectrum. Max
More informationEnergy and the Quantum Theory
Energy and the Quantum Theory Light electrons are understood by comparing them to light 1. radiant energy 2. travels through space 3. makes you feel warm Light has properties of waves and particles Amplitude:
More informationIntroduction to Quantum Mechanics. and Quantum Numbers
Introduction to Quantum Mechanics and Quantum Numbers The Quantum Mechanical Model quantum mechanics: the application of quantum theory to explain the properties of matter, particularly electrons in atoms
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 informationPART 2 Electronic Structure and the Periodic Table. Reference: Chapter 7 8 in textbook
PART 2 Electronic Structure and the Periodic Table Reference: Chapter 7 8 in textbook 1 Early Atomic Models 2 Thomson s 1904 Model of the Atom Plumb Pudding Model He discovered the electron, a discovery
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 informationCHAPTER 5 ATOMIC STRUCTURE SHORT QUESTIONS AND ANSWERS Q.1 Why it is necessary to decrease the pressure in the discharge tube to get the cathode rays? The current does not flow through the gas at ordinary
More informationArrangement of Electrons in Atoms
CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. In what way does the photoelectric effect support the particle theory
More informationChapter 7. DeBroglie Waves Heisenberg s Uncertainty Quantum Numbers Electron Configuration
Chapter 7 DeBroglie Waves Heisenberg s Uncertainty Quantum Numbers Electron Configuration Are Electrons Particles or Waves? De Broglie (1892 1987) If electromagnetic radiation behaves as a particle, could
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 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 informationPeriodicity and the Electronic Structure of Atoms 國防醫學院生化學科王明芳老師
Periodicity and the Electronic Structure of Atoms 國防醫學院生化學科王明芳老師 2018-10-2 1 2 Light and the Electromagnetic Spectrum Electromagnetic energy ( light ) is characterized by wavelength, frequency, and amplitude.
More informationAtomic Structure Ch , 9.6, 9.7
Ch. 9.2-4, 9.6, 9.7 Magnetic moment of an orbiting electron: An electron orbiting a nucleus creates a current loop. A current loop behaves like a magnet with a magnetic moment µ:! µ =! µ B " L Bohr magneton:
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 informationElectrons and Periodic Behavior. Cartoon courtesy of NearingZero.net
Electrons and Periodic Behavior Cartoon courtesy of NearingZero.net Wave-Particle Duality JJ Thomson won the Nobel prize for describing the electron as a particle. His son, George Thomson won the Nobel
More informationElectron Arrangement - Part 1
Brad Collins Electron Arrangement - Part 1 Chapter 8 Some images Copyright The McGraw-Hill Companies, Inc. Properties of Waves Wavelength (λ) is the distance between identical points on successive waves.
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 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 informationAP Chemistry. Chapter 6 Electronic Structure of Atoms
AP Chemistry Chapter 6 Electronic Structure of Atoms Section 6.1 Wave Nature of Light When we say "light," we generally are referring to visible light a type of electromagnetic radiation But actually Visible
More informationElectrons in Atoms. Section 5.1 Light and Quantized Energy
Name Date Class 5 Electrons in Atoms Section 5.1 Light and Quantized Energy In your textbook, read about the wave nature of light. Use each of the terms below just once to complete the passage. amplitude
More informationTest Bank for General Chemistry Atoms First 2nd Edition by John E. McMurry and Robert C. Fay
Test Bank for General Chemistry Atoms First 2nd Edition by John E. McMurry and Robert C. Fay Link download full: https://digitalcontentmarket.org/download/test-bank-for-general-chemistry-atoms-f irst-2nd-edition-by-mcmurry-and-fay/
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 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 informationUNIT 1: STRUCTURE AND PROPERTIES QUANTUM MECHANICS. Development of the Modern Atomic Theory
UNIT 1: STRUCTURE AND PROPERTIES QUANTUM MECHANICS Development of the Modern Atomic Theory Problems with the Bohr Model Bohr s theory only fit the observed spectra of hydrogen. In addition, the Bohr model
More informationRadiation and the Atom
Radiation and the Atom PHYS Lecture Departamento de Física Instituto Superior de Engenharia do Porto cav@isep.ipp.pt Overview SI Units and Prefixes Radiation Electromagnetic Radiation Electromagnetic Spectrum
More informationChapter 6. of Atoms. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 6 John D. Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice Hall,
More informationChapter 6. of Atoms. Waves. Waves 1/15/2013
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 6 John D. Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice Hall,
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 informationCh. 7 The Quantum Mechanical Atom. Brady & Senese, 5th Ed.
Ch. 7 The Quantum Mechanical Atom Brady & Senese, 5th Ed. Index 7.1. Electromagnetic radiation provides the clue to the electronic structures of atoms 7.2. Atomic line spectra are evidence that electrons
More informationAtom Physics. Chapter 30. DR JJ UiTM-Cutnell & Johnson 7th ed. 1. Model of an atom-the recent model. Nuclear radius r m
Chapter 30 Atom Physics DR JJ UiTM-Cutnell & Johnson 7th ed. 1 30.1 Rutherford Scattering and the Nuclear Atom Model of an atom-the recent model Nuclear radius r 10-15 m Electron s position radius r 10-10
More informationThe early periodic table based on atomic weight. (Section 5.1) Lets review: What is a hydrogen atom? 1 electron * nucleus H 1 proton
PERIODICITY AND ATOMIC STRUCTURE CHAPTER 5 How can we relate the structure of the atom to the way that it behaves chemically? The process of understanding began with a realization that many of the properties
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 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 informationCHAPTER I Review of Modern Physics. A. Review of Important Experiments
CHAPTER I Review of Modern Physics A. Review of Important Experiments Quantum Mechanics is analogous to Newtonian Mechanics in that it is basically a system of rules which describe what happens at the
More informationAtomic Structure and Atomic Spectra
Atomic Structure and Atomic Spectra Atomic Structure: Hydrogenic Atom Reading: Atkins, Ch. 10 (7 판 Ch. 13) The principles of quantum mechanics internal structure of atoms 1. Hydrogenic atom: one electron
More informationName Class Date. Chapter: Arrangement of Electrons in Atoms
Assessment Chapter Test A Chapter: Arrangement of Electrons in Atoms In the space provided, write the letter of the term that best completes each sentence or best answers each question. 1. Which of the
More informationCHAPTER 4 Arrangement of Electrons in Atoms
CHAPTER 4 Arrangement of Electrons in Atoms SECTION 1 The Development of a New Atomic Model OBJECTIVES 1. Explain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic
More informationTopic 12: Quantum numbers. Heisenberg, Schrodinger, Quantum Theory, Quantum numbers, Practice
Topic 12: Quantum numbers Heisenberg, Schrodinger, Quantum Theory, Quantum numbers, Practice Quantum Mechanics We left off by saying Bohr s model only explained the electron arrangement of Hydrogen...
More information