NOTES: 5.3 Light and Atomic Spectra (more Quantum Mechanics!)
|
|
|
- Shawn Walton
- 5 years ago
- Views:
Transcription
1 NOTES: 5.3 Light and Atomic Spectra (more Quantum Mechanics!)
2 Light WAVE or PARTICLE?
3 Electromagnetic Radiation Electromagnetic radiation includes: -radio waves -microwaves -infrared waves -visible light -ultraviolet waves -x-rays -gamma rays
4 Electromagnetic Radiation according to the wave model, light consists of electromagnetic waves all EM waves travel in a vacuum at a speed of 3.0 x 10 8 m/s
5 Electromagnetic Radiation Electromagnetic radiation (radiant energy) is characterized by its: -WAVELENGTH (color): λ (Greek letter lambda) -FREQUENCY (energy): ν (Greek letter nu)
6 WAVES Wavelength = distance between successive crests measured in units of length (m, nm) Frequency = the # of crests passing a given point per second measured in # per sec, or s -1, or Hertz
7
8 NOTICE: as wavelength decreases, frequency (& therefore ENERGY) increases!
9
10 VISIBLE LIGHT: When sunlight or white light is passed through a prism, it gives the continuous spectrum observed in a rainbow. each color blends into the next in the order: red, orange, yellow, green, blue, indigo, violet RED LIGHT: longest wavelength, lowest freq. VIOLET LIGHT: shortest wavelength, highest freq.
11 Light and Electrons each element emits light when it is excited by an electric current passing through its gas or vapor the atoms first absorb energy, then lose the energy as they emit light passing light emission through a prism gives a unique atomic emission spectrum
12 Light and Electrons recall: white light gives a continuous spectrum atomic emission spectra: relatively few lines **this suggests the emission of very specific, exact frequencies of energy/light! each line corresponds to a specific amt. of energy being emitted!!
13 Bright Line Emission Spectrum The light emitted by an element when its electrons return to a lower energy state can be viewed as a bright line emission spectrum.
14 Light and Electrons the emission spectrum of each element is unique to that element emission spectra can be used to identify the components of an unknown compound **we can even discover the composition of far away stars by studying their emission spectra!! (stars are hot, glowing bodies of gases!) Wow Science is cool!
15 The Quantum Concept: according to classical physics, there is no limit to how small the energy gained or lost by an object can be so classical physics cannot explain emission spectra which only allows SOME amounts of energy, but not others enter: Max Planck! ( ) he wondered, what if light energy consists of little packets of energy called QUANTA?
16 The Quantum Concept: Einstein added the proposal we can describe light as composed of particles, or PHOTONS. each photon of light has a particular amount or packet of energy (a quantum). the amt. of energy (frequency) possessed by a photon depends on the color (wavelength) of the light.
17 The Quantum Concept & the Photoelectric Effect: Photons light quanta or packets of energy Photons can be observed indirectly through photoelectric effect PHOTOELECTRIC EFFECT - metals eject electrons called photoelectrons when light shines on them
18 The Quantum Concept & the Photoelectric Effect: HOWEVER, not all colors / frequencies of light will work on all metals! (because only specific frequencies, quanta, may be absorbed) in what ways do we use the energy of light to generate electricity??? -cars with photoelectric cells; solar-powered calculators; etc.
19 What does this have to do with electron arrangement in atoms? When all electrons are in the lowest possible energy levels, an atom is said to be in its GROUND STATE. When an atom absorbs energy so that its electrons are boosted to higher energy levels, the atom is said to be in an EXCITED STATE.
20 Electron States Ground state lowest energy level or n = 1 Excited state energy level of n = 2, 3, 4. energy levels are quantized (only certain values of electron energy are possible). QUANTA of energy are absorbed and then released when electrons drop from an excited state to a lower energy state Only electrons in transition from high to low energy levels emit energy in the form of light
21
22 Bright Line Emission Spectrum The light emitted by an element when its electrons return to a lower energy state can be viewed as a bright line emission spectrum.
Chapter 5 Electrons In Atoms
Chapter 5 Electrons In Atoms 5.1 Revising the Atomic Model 5.2 Electron Arrangement in Atoms 5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 Copyright Pearson Education, Inc., or its affiliates.
Physics and the Quantum Mechanical Model
chemistry 1 of 38 Mechanical Model Neon advertising signs are formed from glass tubes bent in various shapes. An electric current passing through the gas in each glass tube makes the gas glow with its
Write the electron configuration for Chromium (Cr):
Write the electron configuration for Chromium (Cr): Energy level Aufbau Principle Atomic orbital Quantum Hund s Rule Atomic number Electron Configuration Whole number Pauli Exlcusion Principle Quantum
Table 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
5.3. Physics and the Quantum Mechanical Model
Chemistry 5-3 Physics and the Quantum Mechanical Model Neon advertising signs are formed from glass tubes bent in various shapes. An electric current passing through the gas in each glass tube makes the
Unit 3. Chapter 4 Electrons in the Atom. Niels Bohr s Model. Recall the Evolution of the Atom. Bohr s planetary model
Unit 3 Chapter 4 Electrons in the Atom Electrons in the Atom (Chapter 4) & The Periodic Table/Trends (Chapter 5) Niels Bohr s Model Recall the Evolution of the Atom He had a question: Why don t the electrons
The ELECTRON: Wave Particle Duality. chapter 4
The ELECTRON: Wave Particle Duality chapter 4 What do we know about light? Before 1900 s scientists thought light behaved as a wave. This belief changed when it was discovered that light also has particle
Chapter 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
Chapter 5 Electrons In Atoms
Chapter 5 Electrons In Atoms 5.1 Revising the Atomic Model 5.2 Electron Arrangement in Atoms 5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 Copyright Pearson Education, Inc., or its affiliates.
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
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
c = 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
Electrons! Chapter 5
Electrons! Chapter 5 I.Light & Quantized Energy A.Background 1. Rutherford s nuclear model: nucleus surrounded by fast-moving electrons; no info on how electrons move, how they re arranged, or differences
The 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
Light, Electrons, and Energy. Pre-AP
Light, Electrons, and Energy Pre-AP Light Waves! Electromagnetic Frequency Light Phenomenon Light can act as a wave or as a particle, but most light-electron interactions use wave physics. = greek letter
Electrons, Energy, & the Electromagnetic Spectrum Notes Simplified, 2-D Bohr Model: Figure 2. Figure 3 UNIT 4 - ELECTRONS & ELECTRON ARRANGEMENT
Electrons, Energy, & the Electromagnetic Spectrum Notes Simplified, 2-D Bohr Model: Figure 1 UNIT 4 - ELECTRONS & ELECTRON ARRANGEMENT Figure 2 Figure 3 The energy is released as electromagnetic radiation.
Energy of Waves. What is the relationship between l, n and Energy?!
Chapter 5 Part 2 c = ln Practice! What is the wavelength of a microwave that has a frequency of 1.56 x 10 9 Hz? The red-colored light in a fireworks display might be produced when Strontium salts are heated.
Wavelength (λ)- Frequency (ν)- Which of the following has a higher frequency?
Name: Unit 5- Light and Energy Electromagnetic Spectrum Notes Electromagnetic radiation is a form of energy that emits wave-like behavior as it travels through space. Amplitude (a)- Wavelength (λ)- Which
Electromagnetic Radiation. is a form of energy that exhibits wavelike behavior as it travels through space.
Electromagnetic Radiation is a form of energy that exhibits wavelike behavior as it travels through space. What are the 7 forms of electromagnetic radiation, in order of INCREASING wavelength? gamma rays
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
The Theory of Electromagnetism
Notes: Light The Theory of Electromagnetism James Clerk Maxwell (1831-1879) Scottish physicist. Found that electricity and magnetism were interrelated. Moving electric charges created magnetism, changing
Frequency: the number of complete waves that pass a point in a given time. It has the symbol f. 1) SI Units: Hertz (Hz) Wavelength: The length from
Frequency: the number of complete waves that pass a point in a given time. It has the symbol f. 1) SI Units: Hertz (Hz) Wavelength: The length from the one crest of a wave to the next. I. Electromagnetic
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
Ch. 5 Notes - ELECTRONS IN ATOMS NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 5 Notes - ELECTRONS IN ATOMS NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 5.1 Notes I. Light and Quantized Energy A. The Wave Nature of Light 1) the wave
Ch. 4 Notes - ELECTRONS IN ATOMS NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 4 Notes - ELECTRONS IN ATOMS NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Light and Quantized Energy A. The Wave Nature of Light 1) the wave nature of
10/4/2011. Tells you the number of protons
Atomic Structure The arrangement of the subatomic particles within the atom determines the chemical properties of the elements How they interact with one another The types of ions and structures that they
Ch 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
The Sine Wave. You commonly see waves in the environment. Light Sound Electricity Ocean waves
The Sine Wave Mathematically, a function that represents a smooth oscillation For example, if we drew the motion of how the weight bobs on the spring to the weight we would draw out a sine wave. The Sine
General Chemistry by Ebbing and Gammon, 8th Edition
Chem 1045 General Chemistry by Ebbing and Gammon, 8th Edition George W.J. Kenney, Jr Last Update: 26-Mar-2009 Chapter 7: Quantum Theory of the Atom These Notes are to SUPPLIMENT the Text, They do NOT Replace
I 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
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
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
The Atom & Unanswered Questions:
The Atom & Unanswered Questions: 1) Recall-Rutherford s model, that atom s mass is concentrated in the nucleus & electrons move around it. a) Doesn t explain how the electrons were arranged around the
Name Date Class ELECTRONS IN ATOMS
Name _ Date Class 5 ELECTRONS IN ATOMS SECTION 5.1 MODELS OF THE ATOM (pages 127 132) This section summarizes the development of atomic theory. It also explains the significance of quantized energies of
Unit 3: Electron configuration and periodicity
Unit 3: Electron configuration and periodicity Group 1 BOHR MODELS Group 18 H Group 2 Group 13 Group 14 Group 15 Group 16 Group 17 He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca His theory couldn t
Chapter 5 Light and Matter
Chapter 5 Light and Matter Stars and galaxies are too far for us to send a spacecraft or to visit (in our lifetimes). All we can receive from them is light But there is much we can learn (composition,
ASTRONOMY 161. Introduction to Solar System Astronomy. Class 9
ASTRONOMY 161 Introduction to Solar System Astronomy Class 9 Light Monday, January 29 Look, but don t touch. - Astronomers Motto Light: Key Concepts (1) Visible light is just one form of electromagnetic
Chapter 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
History of the Atomic Model
Chapter 5 Lecture Chapter 5 Electronic Structure and Periodic Trends 5.1 Electromagnetic Radiation Learning Goal Compare the wavelength, frequency, and energy of electromagnetic radiation. Fifth Edition
Do Now: Bohr Diagram, Lewis Structures, Valence Electrons 1. What is the maximum number of electrons you can fit in each shell?
Chemistry Ms. Ye Name Date Block Do Now: Bohr Diagram, Lewis Structures, Valence Electrons 1. What is the maximum number of electrons you can fit in each shell? 1 st shell 2 nd shell 3 rd shell 4 th shell
Bohr. Electronic Structure. Spectroscope. Spectroscope
Bohr Electronic Structure Bohr proposed that the atom has only certain allowable energy states. Spectroscope Using a device called a it was found that gaseous elements emitted electromagnetic radiation
Ch 9 Electrons in Atoms & the Periodic Table Study Sheet Acc. Chemistry SCANTRON. Name /99. 3) Light is a type of matter. 3)
Ch 9 Electrons in Atoms & the Periodic Table Study Sheet Acc. Chemistry SCANTRON Name /99 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. 1) When the elements are arranged
Atomic Structure Part II. Electrons in Atoms
Atomic Structure Part II Electrons in Atoms Radiant energy travels in the form of waves that have both electrical and magnetic properties. These electromagnetic waves can travel through empty space, as
Introduction. Electromagnetic Waves. Electromagnetic Waves
Introduction Much of the information we know about electrons comes from studies of interactions of light and matter. In the early 1900 s, scientists discovered that light has properties of both a wave
Name Class Date ELECTRONS AND THE STRUCTURE OF ATOMS
Electrons in Atoms ELECTRONS AND THE STRUCTURE OF ATOMS 5.1 Revising the Atomic Model Essential Understanding of an atom. An electron s energy depends on its location around the nucleus Reading Strategy
The ELECTRON: Wave Particle Duality
The ELECTRON: Wave Particle Duality No familiar conceptions can be woven around the electron. Something unknown is doing we don t know what. -Sir Arthur Eddington The Nature of the Physical World (1934)
The Development of Atomic Theory
The Development of Atomic Theory Democritus (400 BC) John Dalton (1803) J.J. Thomson (1897) Ernest Rutherford (1911) James Chadwick (1932) - suggested that matter is composed of indivisible particles called
EXPERIMENT 17: Atomic Emission
EXPERIMENT 17: Atomic Emission PURPOSE: To construct an energy level diagram of the hydrogen atom To identify an element from its line spectrum. PRINCIPLES: White light, such as emitted by the sun or an
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
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
Atomic Spectra & Electron Energy Levels
CHM151LL: ATOMIC SPECTRA & ELECTRON ENERGY LEVELS 1 Atomic Spectra & Electron Energy Levels OBJECTIVES: To measure the wavelength of visible light emitted by excited atoms to calculate the energy of that
Atomic Structure Part II Electrons in Atoms
Atomic Structure Part II Electrons in Atoms Radiant energy travels in the form of waves that have both electrical and magnetic properties. These electromagnetic waves can travel through empty space, as
Properties 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
Arrangement of Electrons. Chapter 4
Arrangement of Electrons Chapter 4 Properties of Light -Light s interaction with matter helps to understand how electrons behave in atoms -Light travels through space & is a form of electromagnetic radiation
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
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
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
Chapter 4 Electron Configurations
Chapter 4 Electron Configurations Waves Today scientists recognize light has properties of waves and particles Waves: light is electromagnetic radiation and travels in electromagnetic waves. 4 Characteristics
Chapter 5. Electrons in Atoms
Chapter 5 Electrons in Atoms Warm - Up What kind of light causes you to sunburn? Why does only this type of light burn your skin and not other light? What does sunscreen do on a chemical level? Today s
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
Properties of Light and Atomic Structure. Chapter 7. So Where are the Electrons? Electronic Structure of Atoms. The Wave Nature of Light!
Properties of Light and Atomic Structure Chapter 7 So Where are the Electrons? We know where the protons and neutrons are Nuclear structure of atoms (Chapter 2) The interaction of light and matter helps
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
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
Duncan. Electrons, Energy, & the Electromagnetic Spectrum Notes Simplified, 2-D Bohr Model: Figure 1. Figure 2. Figure 3
Electrons, Energy, & the Electromagnetic Spectrum Notes Simplified, 2-D Bohr Model: Figure 1 Figure 2 Figure 3 Light Calculation Notes Here s how the type/form of EM radiation can be determined The amount
CHEMISTRY - TRO 4E CH.7 - THE QUANTUM-MECHANICAL MODEL OF THE ATOM
!! www.clutchprep.com CONCEPT: THE NATURE OF LIGHT Visible light represents a small portion of the continuum of radiant energy known as. The visible light spectrum ranges from to. Its wave properties of
9/16/08 Tuesday. Chapter 3. Properties of Light. Light the Astronomer s Tool. and sometimes it can be described as a particle!
9/16/08 Tuesday Announce: Observations? Milky Way Center movie Moon s Surface Gravity movie Questions on Gravity from Ch. 2 Ch. 3 Newton Movie Chapter 3 Light and Atoms Copyright (c) The McGraw-Hill Companies,
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.
LIGHT AND THE QUANTUM MODEL
LIGHT AND THE QUANTUM MODEL WAVES Wavelength ( ) - length of one complete wave Frequency ( ) - # of waves that pass a point during a certain time period hertz (Hz) = 1/s Amplitude (A) - distance from the
Electrons, 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
The Structure of the Atom Review
The Structure of the Atom Review Atoms are composed of PROTONS + positively charged mass = 1.6726 x 10 27 kg NEUTRONS neutral mass = 1.6750 x 10 27 kg ELECTRONS negatively charged mass = 9.1096 x 10 31
Background: The Electromagnetic Spectrum
Background: The Electromagnetic Spectrum Wavelength (λ) in meters wavelength decreasing 10 4 10 2 10 0 10-2 10-4 10-6 10-8 10-10 10-12 10-14 microwaves ultraviolet Gamma rays Radio waves AM 10 4 Shortwave
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
Atomic Spectra Introduction
Atomic Spectra Introduction: Light and all other electromagnetic radiation is energy that is emitted in the form of waves. Thus light behaves like a wave, and the energy of light varies with the wavelength
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
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:
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
Atomic Notes.notebook. January 15, Recall the models of the atom we have discussed thus far:
Atomic Notes.notebook January 15, 2014 Dec 17 10:59 AM Recall the models of the atom we have discussed thus far: Dalton solid neutral sphere Thomson plum pudding model Rutherford planetary model Rutherford
Modern 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
Name Date Class MODELS OF THE ATOM
5.1 MODELS OF THE ATOM Section Review Objectives Identify inadequacies in the Rutherford atomic model Identify the new assumption in the Bohr model of the atom Describe the energies and positions of electrons
The 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
Review: Properties of a wave
Radiation travels as waves. Waves carry information and energy. Review: Properties of a wave wavelength (λ) crest amplitude (A) trough velocity (v) λ is a distance, so its units are m, cm, or mm, etc.
Quantum 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
Electromagnetic spectrum Electromagnetic radiation
Chapter 4 Section 1 Electromagnetic spectrum includes all the different wave lengths of radiation. Electromagnetic radiation is a form of energy that exhibits wave like behavior as it travels through space.
Bohr Diagram, Lewis Structures, Valence Electrons Review 1. What is the maximum number of electrons you can fit in each energy level or shell?
AP Chemistry Ms. Ye Name Date Block Bohr Diagram, Lewis Structures, Valence Electrons Review 1. What is the maximum number of electrons you can fit in each energy level or shell? 1 st shell 2 nd shell
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
The Electromagnetic Spectrum
The Electromagnetic Spectrum Outcomes: http://www.avclub.com/article/marvel-made-its-own-movies-ang-lee-offered-idiosyn-204118 Qualitatively describe the electromagnetic spectrum in terms of frequency,
Chapter 5 Models of the Atom
Chapter 5 Models of the Atom Atomic Models Rutherford used existing ideas about the atom and proposed an atomic model in which the electrons move around the nucleus. However, Rutherford s atomic model
Democritus and Leucippus Matter is made up of indivisible particles Dalton - one type of atom for each element. Greek Idea
Electrons in Atoms Democritus and Leucippus Matter is made up of indivisible particles Dalton - one type of atom for each element Greek Idea Thomson s Model Discovered electrons Atoms were made of positive
Electromagnetic Radiation
Electromagnetic Radiation aka Light Properties of Light are simultaneously wave-like AND particle-like Sometimes it behaves like ripples on a pond (waves). Sometimes it behaves like billiard balls (particles).
Chapter 7. Part I Dr. Stone Stan State
Chapter 7 Part I Dr. Stone Stan State 1 2 Electromagnetic Radiation Perpendicular oscillating fields: Electric: PET scan: gamma rays X-rays Visible light Infrared (heat) Microwaves Magnetic MRI = magnetic
5.111 Lecture Summary #3 Monday, September 8, 2014
5.111 Lecture Summary #3 Monday, September 8, 2014 Reading for today: Section 1.2 and Section 1.4 with a focus on pgs 10-12 (4 th ed or 5 th ed). Read for Lecture 4: Section 1.5 The Wave-Particle Duality
The Quantum Mechanical Atom
The Quantum Mechanical Atom CHAPTER 7 Chemistry: The Molecular Nature of Matter, 6 th edition By Jesperson, Brady, & Hyslop CHAPTER 8: Quantum Mechanical Atom Learning Objectives q Light as Waves, Wavelength
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
The Nature of Light. We have a dual model
Light and Atoms Properties of Light We can come to understand the composition of distant bodies by analyzing the light they emit This analysis can tell us about the composition as well as the temperature
Chemistry 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
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
The Death of Classical Physics. The Rise of the Photon
The Death of Classical Physics The Rise of the Photon A fundamental question: What is Light? James Clerk Maxwell 1831-1879 Electromagnetic Wave Max Planck 1858-1947 Photon Maxwell's Equations (1865) Maxwell's
The relationship between these aspects is described by the following equation: E = hν =
1 Learning Outcomes EXPERIMENT A10: LINE SPECTRUM Upon completion of this lab, the student will be able to: 1) Examine the line spectrum of the hydrogen atom. 2) Calculate the frequency and energy of the
LIGHT. Question. Until very recently, the study of ALL astronomical objects, outside of the Solar System, has been with telescopes observing light.
LIGHT Question Until very recently, the study of ALL astronomical objects, outside of the Solar System, has been with telescopes observing light. What kind of information can we get from light? 1 Light
1. The most important aspects of the quantum theory.
Lecture 5. Radiation and energy. Objectives: 1. The most important aspects of the quantum theory: atom, subatomic particles, atomic number, mass number, atomic mass, isotopes, simplified atomic diagrams,