Introduction to Quantum Mechanics. and Quantum Numbers
|
|
|
- Toby Morrison
- 5 years ago
- Views:
Transcription
1 Introduction to Quantum Mechanics and Quantum Numbers
2 The Quantum Mechanical Model quantum mechanics: the application of quantum theory to explain the properties of matter, particularly electrons in atoms
3 Schrödinger s Standing Wave Erwin Schrödinger and Louis de Broglie found that an electron bound to a nucleus in an atom resembled a standing wave, so they began research on a description of the atom based on wave behaviour instead of particle behaviour.
4
5 Schrödinger and de Broglie took the idea of standing waves and applied it to the electron in a hydrogen atom. In their model, the electron is a circular standing wave around the nucleus. This circular standing wave consists of wavelengths that are multiples of whole numbers (n = 1, 2, 3, 4,...). Only certain circular orbits have a circumference into which a whole number of wavelengths can fit.
6 Any other orbits of the standing electron wave are not allowed because they would cause the standing wave to cancel out or collapse.
7 Orbitals and Probability Distributions Schrödinger s work on quantum mechanics led to his development of a mathematical equation, called the Schrödinger wave equation, that could be used to calculate electron energy levels. Orbital: the region around the nucleus where an electron has a high probability of being found
8 um/schr2.html
9 Werner Heisenberg came up with a statistical approach for locating electrons. To measure the location and speed of an object, you must be able to observe it. Heisenberg s Uncertainty Principle: the idea that it is impossible to know the exact position and speed of an electron at a given time
10 The best we can do is to describe the probability of finding an electron in a specific location. wave function: the mathematical probability of finding an electron in a certain region of space Quantum mechanics does not describe how an electron moves or even if it moves. It only tells us the statistical probability of finding the electron in a given location in an atom. The area or region where we are likely to find an electron is an orbital.
11 Using wave functions, physicists have created a three-dimensional electron probability density, which is a plot that indicates regions around the nucleus with the greatest probability of finding an electron. The electron probability density plot for a hydrogen electron in the ground state (lowest energy state) is spherical and is called the 1s orbital.
12 The greatest probability of finding the electron occurs at a distance r max from the nucleus. This distance is the same as the distance Bohr calculated for the radius of the first circular orbit of hydrogen s electron.
13 The two main ideas of the quantum mechanical model of the atom are that electrons can be in different orbitals by absorbing or emitting quanta of energy, and that the location of electrons is given by a probability distribution.
14 Quantum Numbers There are 4 quantum numbers (numbers that describe the quantum mechanical properties of orbitals; from the solutions to Schrödinger s wave equation)
15 The Principal Quantum Number (n) The integer, n, that Bohr used to label the orbits and energies describes a main shell of electrons, and is referred to today as the principal quantum number. Bohr s theory used only one quantum number, which is the main reason that it worked well for hydrogen but not for other atoms.
16
17 The Secondary Quantum Number, (l) Arnold Sommerfeld (1915) boldly employed elliptical orbits to extend the Bohr theory and successfully explain that the main lines of the bright-line spectrum for hydrogen were actually composed of more than one line.
18 He introduced the secondary quantum number, l, to describe additional electron energy sublevels, or subshells, that formed part of a main energy level. Using the analogy of a staircase for an energy level, this means that one of Bohr s main energy steps is actually a group of several little steps.
19 Notice that the number of sublevels equals the value of the principal quantum number.
20
21 The Magnetic Quantum Number, m l The scientific work of analyzing atomic spectra was still not complete. If a gas discharge tube is placed near a strong magnet, some single lines split into new lines that were not initially present. This observation was first made by Pieter Zeeman in 1897 and is called the normal Zeeman Effect.
22 He observed, for example, triplets where only one line existed without the magnetic field. The Zeeman effect was explained using another quantum number, the magnetic quantum number, m l, added by Arnold Sommerfeld and Peter Debye (1916). Their explanation was that orbits could exist at various angles. The idea is that if orbits are oriented in space in different planes, the energies of the orbits are different when the atom is near a strong magnet.
23
24 Shapes and Orientations of Orbitals
25 The Spin Quantum Number, m s Paramagnetism is another kind of magnetism of substances and is recognized as a relatively weak attraction to a strong magnet. Paramagnetism refers to the magnetism of individual atoms; ferromagnetism is due to the magnetism of a collection of atoms.
26 Samuel Goudsmit and George Uhlenbeck, found that a fourth quantum number was necessary to account for the details of the emission spectra of atoms due to paramagnetism. Since they knew from classical physics that a spinning charge produces a magnetic moment, it seemed reasonable to assume that the electron could have two oppositely directed spin states
27 In 1925, Wolfgang Pauli, suggested that each electron spins on its axis. For an electron, the two spins are equal in magnitude but opposite in direction, and these are the only choices; i.e., the spin is quantized to two and only two values. This fourth quantum number is called the spin quantum number,m s, and is given values of either +1/2 or -1/2. Qualitatively, we refer to the spin as either clockwise or counterclockwise or as up or down.
28 Pauli s Exclusion Principle In a given atom, no two electrons can have the same set of four quantum numbers (n, l, m l, and m s ).
29 Summary of Quantum Numbers
--THE QUANTUM MECHANICAL MODEL
--THE QUANTUM MECHANICAL MODEL Bohr s Energy Levels Electrons reside in certain energy levels Each level represents a certain amount of energy Low Energy levels: closer to nucleus High Energy levels: farther
Electromagnetic 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
The 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
Physics 30 Lesson 34 Quantum Mechanics (optional reading)
Physics Lesson Quantum Mechanics (optional reading) This lesson is not a part of the Physics curriculum. However, this lesson completes the story of our current understanding of the electron structure
Line 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:
A 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
Chapter 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
Chapter 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,
Chapter 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,
Chapter 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
SCH4U: 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
Chapter 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
Chapter 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
ATOMIC STRUCRURE
ATOMIC STRUCRURE Long Answer Questions: 1. What are quantum numbers? Give their significance? Ans. The various orbitals in an atom qualitatively distinguished by their size, shape and orientation. The
Review Models of the Atom
Review Models of the Atom Copyright 2007 Pearson Benjamin Cummings. All rights reserved. Dalton proposes the indivisible unit of an element is the atom. Thomson discovers electrons, believed to reside
Light. 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
November 06, Chapter 7 Atomic Struture. CHAPTER 7 Atomic Structure. Oct 27 9:34 AM ATOMIC STRUCTURE. Oct 27 9:34 AM
CHAPTER 7 Atomic Structure ATOMIC STRUCTURE 1 The Wave Nature of Light Most subatomic particles behave as PARTICLES and obey the physics of waves. Visible light Ultravioletlight Wavelength Frequency (Hertz
CHEMISTRY 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
2) 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
Complete 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
Ch. 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
Chapter 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
QUESTION BANK ON ATOMIC STRUCTURE
CHEMISTRY QUESTION BANK ON ATOMIC STRUCTURE (QUANTAM NUMBERS) Q. Deduce the possible sets of four quantum number when n =. Q. What is the maximum number of electron that may be present in all the atomic
SECTION 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
Chapter 4 Section 2 Notes
Chapter 4 Section 2 Notes Vocabulary Heisenberg Uncertainty Principle- states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle. Quantum
Electronic 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
Electron 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.
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
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
Chapter 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
Unit 4. Electrons in Atoms
Unit 4 Electrons in Atoms When were most of the subatomic particles discovered? Who discovered densely packed nucleus surrounded by fast moving electrons? Rutherford s Model Major development Lacked detail
5.1 Light & Quantized Energy
5.1 Light & Quantized Energy Objectives: 1. Describe electromagnetic (EM) wave properties & measures 2. Relate visible light to areas of the EM spectrum with higher & lower energy 3. Know the relationship
Quantum Mechanical Model
Quantum Mechanical Model De Broglie De Broglie build upon Planck s observations of packets of light (photons) emit a distinctive quantum of energy. He proposed that the particles being emitted have particle
Chapter 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
Classical Theory of the Atom
QUANTUM CHEMISTRY Classical Theory of the Atom The electron is in a shell around nucleus at a certain distance (radius, r) Electron orbits (revolves) the nucleus, like the planets around the sun. r Hydrogen
CHAPTER 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
Surprise, surprise, surprise
Experiment Rutherford had two grad students, Marsden and Geiger. It was decided that Geiger would gain some practice by conducting a series of experiments with gold and alpha particles. The positively
Electronic 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
Outline 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
Ch 6 Atomic Spectra. Masterson & Hurley
Ch 6 Atomic Spectra Masterson & Hurley 1 Joule = 1 kg m 2 s 2 Ch 6.1 Light, Photon Energies, & Atomic Spectra What scientists know about light, scientists are able to explain the structure of the atom.
Energy 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:
Chemistry 11. Unit 8 Atoms and the Periodic Table Part II Electronic Structure of Atoms
Chemistry 11 Unit 8 Atoms and the Periodic Table Part II Electronic Structure of Atoms 2 1. Atomic number and atomic mass In the previous section, we have seen that from 50 to 100 years after Dalton proposed
AP Chemistry A. Allan Chapter 7 Notes - Atomic Structure and Periodicity
AP Chemistry A. Allan Chapter 7 Notes - Atomic Structure and Periodicity 7.1 Electromagnetic Radiation A. Types of EM Radiation (wavelengths in meters) 10-1 10-10 10-8 4 to 7x10-7 10-4 10-1 10 10 4 gamma
E J The electron s energy difference between the second and third levels is J. = J
The wavelength of light emitted is 654 nm. = c f c 3.00 10 8 m/s f c 3.00 108 m 1s 6.54 10 7 m f 4.59 4.59 10 14 z 1 s 10 14 The frequency of the light emitted is 4.59 10 14 z. E hf h 6.63 10 34 J/z E
Electronic 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
Chapter 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
Atomic 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
XI STD-CHEMISTRY LESSON: ATOMIC STRUCTURE-I
XI STD-CHEMISTRY LESSON: ATOMIC STRUCTURE-I 1.Define Atom All matter is composed of very small particles called atoms 2.Define Orbital The nucleus is surrounded by electrons that move around the nucleus
Chapter 6 Electronic Structure of Atoms. 許富銀 ( Hsu Fu-Yin)
Chapter 6 Electronic Structure of Atoms 許富銀 ( Hsu Fu-Yin) 1 The Wave Nature of Light The light we see with our eyes, visible light, is one type of electromagnetic radiation. electromagnetic radiation carries
2.4. Quantum Mechanical description of hydrogen atom
2.4. Quantum Mechanical description of hydrogen atom Atomic units Quantity Atomic unit SI Conversion Ang. mom. h [J s] h = 1, 05459 10 34 Js Mass m e [kg] m e = 9, 1094 10 31 kg Charge e [C] e = 1, 6022
CHEMISTRY. 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:
Final 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
Physics 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
Electrons 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
The Bohr Model Bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.
5.1 The Development of Atomic Models Rutherford s atomic model could not explain the chemical properties of elements. Rutherford s atomic model could not explain why objects change color when heated. The
CHEM 103 Spectroscopy and the Quantum Mechanical Model
CHEM 103 Spectroscopy and the Quantum Mechanical Model Lecture Notes April 6, 2006 Prof. Sevian Agenda Emission spectroscopy How the quantum mechanical model explains it Where quantum mechanics breaks
Chapter 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
Development 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
Chapter 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
COLLEGE 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
UNIT 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
Chapter 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
UNIT 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
CHAPTER 28 Quantum Mechanics of Atoms Units
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;
THE 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
CHAPTER 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
Atomic Structure. Part 3: Wave-Mechanical Model of the Atom. Key Question: How does the wave mechanical model explain the location of electrons?
Name Chemistry Atomic Structure Essential Question: How was the structure of the atom determined? Vocabulary: bright-line spectrum electron configuration excited state ground state orbital wave-mechanical
PAPER No. : 8 (PHYSICAL SPECTROSCOPY) MODULE No. : 8 (ALKALI METAL SPECTRA)
Subject Chemistry Paper No and Title Module No and Title Module Tag 8 and Physical Spectroscopy 8: Alkali metal spectra CHE_P8_M8 TABLE OF CONTENTS 1. Learning Outcomes 2. Introduction 3. Multi-electron
Physical 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
Electrons 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
Chapter 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
Chapter 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
ATOM atomov - indivisible
Structure of matter ATOM atomov - indivisible Greek atomists - Democrite and Leukip 300 b.c. R. Bošković - accepts the concept of atom and defines the force J. Dalton - accepts the concept of atom and
Old and new quantum theory
Old and new quantum theory Faults of the Bohr model: - gives only position of the lines and not the intensity - does not explain the number of electrons on each orbit - gives innacurate results for atoms
Calendar. October 23, Chapter 5 Notes Waves.notebook Waves vocab waves ws. quiz PSAT. Blank. elements test. demo day
Calendar Sunday Monday Tuesday Wednesday Thursday Friday Saturday 13 14 Waves vocab waves ws 20 PSAT make notecards 7th 15 21 22 quiz 16 23 17 24 27 28 29 30 31 elements test demo day Blank 1 The Nature
Topic 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...
PHYS 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
Unit 8 Building Atoms with Quantum Leaps
Oh boy... Sam Beckett (from Quantum Leap) Unit 8 Building Atoms with Quantum Leaps Physicists Put Atom in Two Places at Once This was the headline in the science section of the New York Times on May 28,
Explain 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
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
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.
Electronic 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
The 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
Chapter 7. Quantum Theory and the Electronic Structure of Atoms
Chapter 7 Quantum Theory and the Electronic Structure of Atoms This chapter introduces the student to quantum theory and the importance of this theory in describing electronic behavior. Upon completion
Quantum Theory and Electron Configurations
Chapter 5 Chapter 5 Quantum Theory and Electron Configurations It s all about color In terms of atomic models, so far: Dalton (1803) = Tiny, solid particle Thomson (1897) = Plum Pudding model Electrons
The 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
CHAPTER 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
Electrons hold the key to understanding why substances behave as they do. When atoms react it is their outer pars, their electrons, that interact.
Electronic Structure of Atoms The Wave Nature of Light Electrons hold the key to understanding why substances behave as they do. When atoms react it is their outer pars, their electrons, that interact.
The Hydrogen Atom. Dr. Sabry El-Taher 1. e 4. U U r
The Hydrogen Atom Atom is a 3D object, and the electron motion is three-dimensional. We ll start with the simplest case - The hydrogen atom. An electron and a proton (nucleus) are bound by the central-symmetric
Atoms, 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
Chapter 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
Chapter 5: Electrons in Atoms
Chapter 5: Electrons in Atoms Models of the Atom Rutherford used existing ideas about the atom and proposed an atomic model in which the electrons move around the nucleus, like the planets move around
Chapter 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
PHYS 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
Chapter 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
Quantum Mechanical Model of the Atom. Honors Chemistry Chapter 13
Quantum Mechanical Model of the Atom Honors Chemistry Chapter 13 Let s Review Dalton s Atomic Theory Thomson s Model Plum Pudding Rutherford s Model Bohr s Model Planetary Quantum Mechanical Model cloud
Chapter 28. Atomic Physics
Chapter 28 Atomic Physics Quantum Numbers and Atomic Structure The characteristic wavelengths emitted by a hot gas can be understood using quantum numbers. No two electrons can have the same set of quantum
Chapter 7. Characteristics of Atoms. 7.1 Electromagnetic Radiation. Chapter 7 1. The Quantum Mechanical Atom. Atoms: How do we study atoms?
Chapter 7 The Quantum Mechanical Atom 1 Characteristics of Atoms Atoms: possess mass contain positive nuclei contain electrons occupy volume have various properties attract one another combine to form
AP 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
Yellow. 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
The Nature of Energy
The Nature of Energy For atoms and molecules, one does not observe a continuous spectrum, as one gets from a white light source.? Only a line spectrum of discrete wavelengths is observed. 2012 Pearson
CHAPTER 4 10/11/2016. Properties of Light. Anatomy of a Wave. Components of a Wave. Components of a Wave
Properties of Light CHAPTER 4 Light is a form of Electromagnetic Radiation Electromagnetic Radiation (EMR) Form of energy that exhibits wavelike behavior and travels at the speed of light. Together, all