Chapter 4: The Electron
|
|
|
- Prudence Rice
- 5 years ago
- Views:
Transcription
1 Chapter 4: The Electron C. Goodman Doral Academy Preparatory High School, Based on a PowerPoint presentation by Sarah Temple By PresenterMedia.com
2 Section 4-1 Electromagnetic Spectrum Essential Questions 1. What is electromagnetic radiation, and what is the dual particle-wave nature of light? 2. Using the formulas c = λν and E = hν how can frequency, wavelength and energy of electromagnetic radiation be calculated?
3 Vocabulary 1. Electromagnetic radiation/ spectrum 2. Wavelength 3. Frequency 4. The speed of light: 3.00 x 10 8 m/s 5. Quantum (of energy) 6. Photon 7. Planck s constant x J*s 8. Absorption 9. Emission-line spectrum 10. Heisenberg Uncertainty Principle 11. Schrödinger wave equation 12. Quantum theory
4 The Wave Description of Light Electromagnetic radiation is a form of energy that exhibits wavelike behavior as it travels through space.
5 Blast from the Past: Waves Wavelength = λ (m) distance between corresponding points on adjacent waves. Frequency = ν (Hz or s -1 ) number of waves that pass a given point in a specific time, usually one second.
6 Electromagnetic Spectrum All forms of electromagnetic radiation, arranged by wavelength
7
8 Louis de Broglie Explained that electrons have a wave aspect, like light 1. They exist as particle-waves 2. They can exist at specific frequencies 3. These frequencies correspond to specific energies
9 What do all of these waves have in common? 1. They act like particles (photons), since they can travel through space 2. They travel at the speed of light: 3 x 10 8 m/s 3. They act like waves: each has a unique frequency and wavelength For more information about this topic, see es/wavpart2.html (if you don t want to write this down, look under the Chemistry topic in the links on my webpage)
10 What do electrons have to do with light and waves and frequencies??? When have contact with a wave from the EM spectrum, they absorb energy (absorption). The electron can t hold the energy The electron spits it back out (emission). This rejected energy is in the form of EM radiation it has a frequency and wavelength as well as energy. If its wavelength is within the visible light spectrum, you can even see the wave as a color!!! If it s not in the visible spectrum, you can still see it using a spectroscope
11 Emission and absorption Electrons absorb energy from EM radiation, and emit energy as EM radiation
12 Section 4-2 Quantum Theory Essential Questions 1. What is the quantum model of the atom? 2. How are quantum numbers used to describe orbitals and electrons?
13 Section 4-2 Vocabulary 1. Quantum theory 1. Heisenberg Uncertainty Principle 2. Schrödinger 2. Quantum numbers 1. Principal quantum number (n) 2. Angular momentum quantum number (l) 3. Magnetic quantum number (m) 4. Spin quantum number 3. Orbitals 1. s-orbital 2. p-orbital 3. d-orbital 4. f-orbital
14 It is impossible to determine simultaneously both the position and momentum of an electron or any other particle. From "The Development of the Uncertainty Principle", an audiotape produced by Spring Green Multimedia in the UniConcept Scientist Tapes series, 1974.
15 Schrödinger Wave Equation Developed an equation to explain electrons as waves Reconciled wave-particle duality of the electron
16 Quantum Model 1. Mathematically describes the wave properties of electrons and other very small particles 2. Wave functions only give you the probability of finding an electron in a given place
17 Orbitals Electrons travel in orbitals: a 3-dimensional region around the nucleus that indicates the probable location of an electron
18 Atomic Theory marches on Let s bring it down, and see where atomic theory has gone from Thomson to Heisenberg: F:\Chemistry Resource Disk\Powerpoints\Ch04\75063.html
19 Quantum Numbers Quantum numbers specify properties of atomic orbitals and the properties of electrons in orbitals
20 The Four Defined Quantum Numbers 1 st three describe the orbital in which an electron is located Principal main energy level (n) Angular momentum shape (l) Magnetic orientation (m) 4 th describes a state of the electron Spin
21 Principal Quantum Number (n) Main energy level of electron
22 How many electrons are possible per energy level? # e- = 2n 2 Where n=principal quantum #
23 Angular Momentum Quantum Number Symbol: l Indicates type of sublevel (sub shells) I.e. shape or orbital (s, p, d, f)
24 Angular Momentum Quantum Number Each energy level can contain a different number or sub-shells (orbital shapes) n = 1 s orbital n = 2 s, p orbitals n = 3 s, p, d orbitals n = 4 s, p, d, f orbitals
25 Magnetic Quantum Number Symbol = m Orientation of an orbital around the nucleus Refers to xyz axis
26 Magnetic Quantum Number Each orientation adds to the number of subshells available
27 Magnetic Quantum Number
28 Magnetic Quantum Number Each subshell can hold 2 e- So Orientations Can hold s orbital p orbital d orbital f orbital
29
30 Spin Quantum Number How the electron spins on an axis creating a magnetic field 2 spin states of an e-
31 Section 4-3 Electron Configuration Essential Questions 1. How are the Aufbau Principle, the Paulli Exclusion Principle, and Hund s rule used in determining an element s ground-state electron configuration? 2. How does one indicate an element s ground-state electron configuration using orbital notation, electron-configuration notation, and noble-gas notation?
32 Section 4-3 Vocabulary 1. Electron configuration 2. Ground state 3. Aufbau Principle 4. Paulli Exclusion Principle 5. Hund s Rule 6. Orbital notation 7. Electron-configuration notation 8. Noble-gas notation
33 Electron Configuration The arrangement of electrons in an atom Lowest-energy arrangement is called the element s ground-state electron configuration 192d/video-v1.mp4
34 Rules Governing Electron Configurations There are three rules for electron configuration: 1. Aufbau principle 2. Paulli Exclusion Principle 3. Hund s Rule
35 1 st Rule Governing Electron Configurations Aufbau principle The rule of placing electrons within atomic orbitals (within subshells) 1. Electrons are placed in the lowest energetically available subshell 2. An orbital can hold at most 2 electrons
36
37 Filling order mnemonic
38 How do I remember the order of the subshells? Use your handy-dandy periodic table!!!
39 2 nd Rule Governing Electron Configurations Define: Paulli Exclusion Principle No two electrons in the same atom can have the same set of four quantum numbers NOT Each orbital can only contain 2 electrons with opposite spin states 1 s 2
40 3 rd Rule Governing Electron Configurations Hund s Rule 1. Every orbital in a subshell is singly occupied (i.e. with only one electron) before any of the orbital get two electrons 2. All electrons in singly occupied orbitals have the same spin
41 3 rd Rule Governing Electron Configurations Yes No
42 Examples What are the orbital notations for hydrogen and helium? Carbon? Oxygen?
43 More examples
44 Please take out your Orbital Notation Practice worksheet, and let s make it happen! PRACTICE TIME!!!
45 Writing Electron Configurations Orbital Notation Electron- Configuration Notation example = Al 1s 2 2s 2 2p 6 3s 2 3p 1
46
47 Writing Electron Configurations Noble-Gas Notation Condensing electron-configuration notation [Ne] 3s 2 3p 1 where [Ne] = 1s 2 2s 2 2p 6 So normal electron-configuration: 1s 2 2s 2 2p 6 3s 2 3p 1
48
49
50
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
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
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
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
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
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
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 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
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
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
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
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
Name 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
Chapter 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
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
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
Provide a short and specific definition in YOUR OWN WORDS. Do not use the definition from the book. Electromagnetic Radiation
Name: Provide a short and specific definition in YOUR OWN WORDS. Do not use the definition from the book Additional Notes: Electromagnetic Radiation Electromagnetic Spectrum Wavelength Frequency Photoelectric
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
CHAPTER 5 Electrons in Atoms
CHAPTER 5 Electrons in Atoms 5.1 Light & Quantized Energy Was the Nuclear Atomic model incomplete? To most scientists, the answer was yes. The arrangement of electrons was not determined > Remember...the
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
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
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
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:
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
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
Light, Waves, and Electrons
Light, Waves, and Electrons Light: Travels 1. 2. Light Waves Wavelength Frequency Electromagnetic Spectrum Speed of light The product of frequency of a wave and wavelength = the speed of light Calculate
Atomic Structure and Periodicity
p. 99 p. 98 p. 98 Electromagnetic Spectrum Image Atomic Structure and Periodicity Chemistry Zumdahl Chapter 7 Properties of Light Electromagnetic Radiation: a form of energy that exhibits wavelike behavior
Terms to Know. 10.Angular quantum number 11.Magnetic quantum number 12.Spin quantum number
Terms to Know 1. Photon 2. Atomic emission spectrum 3. Ground state 4. Atomic orbital 5. Aufbau principle 6. Pauli exclusion principle 7. Hunds rule 8. Electron configuration 9. Principle quantum number
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
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
Honors Chemistry Unit 3 ELECTRONS IN ATOMS
Honors Chemistry Unit 3 ELECTRONS IN ATOMS I. RADIATION A. Particles 1. alpha particle - helium nucleus with 2 protons, 2 neutrons 2. beta particle - electron or positron ejected from nucleus B. Energy
Name Date Class MODELS OF THE ATOM
Name Date Class 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
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
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
Chapter 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,
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
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
Quantum 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
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
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.
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
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
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
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
Electrons 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
Arrangement 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
Key Equations. Determining the smallest change in an atom's energy.
ATOMIC STRUCTURE AND PERIODICITY Matter and Energy Key Equations λν = c ΔE = hν Relating speed of a wave to its wavelength and frequency. Determining the smallest change in an atom's energy. H( λ =R n
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
C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 6 THE PERIODIC TABLE & ATOMIC STRUCTURE INSTR : FİLİZ ALSHANABLEH
C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 6 THE PERIODIC TABLE & ATOMIC STRUCTURE 0 1 INSTR : FİLİZ ALSHANABLEH CHAPTER 6 THE PERIODIC TABLE & ATOMIC STRUCTURE The Electromagnetic Spectrum The Wave
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
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
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
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
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
I. 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
3. States that an electron occupies the lowest available energy orbital.
Name: Score: 32 / 32 points (100%) Unit 3 Matching (1 point each) Match the electron configuration filling rule with the statements that best describe it Each choice will be used 3 times a Aufbau s Principle
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
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
Chapter 5. Arrangement of Electrons in Atoms
Chapter 5 Arrangement of Electrons in Atoms Light Dual Nature of Light: Light can act like, and as particles. Light is one type of which is a form of Energy that has wavelike behaviour Other types of em
Goals for Today. Clarify some Rydberg Concepts Absorption vs. emission
Note: Due to recent changes the exam 2 material for these slides ends at Ionization Energy Exceptions. You can omit Lewis Structures through General Formal Charge Rules. CH301 Unit 2 QUANTUM NUMBERS AND
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 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
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
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
Quantum Theory & Electronic Structure of Atoms. It s Unreal!! Check your intuition at the door.
Quantum Theory & Electronic Structure of Atoms It s Unreal!! Check your intuition at the door. 1 Quantum Theory of the Atom Description of the atom and subatomic particles. We will focus on the electronic
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
Chapter 4. Development of a New Model
Chapter 4 Development of a New Model Electrons behave like particles in some experiments, and like waves in others. The electron's 'wave/particle duality' has no real analogy in the everyday world. The
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.
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
Academic Chemistry Chapter 5 Electrons in Atoms Notes
Academic Chemistry Chapter 5 Electrons in Atoms Notes Name Date ATOMIC MODEL See Atomic Model Timeline worksheet for specifics. ELECTRONS Quantum Mechanical (QM) Model- This is the currently accepted model
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
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. 4 Sec. 1-2, Ch. 3 sec.6-8 ENERGY CHANGES AND THE QUANTUM THEORY THE PERIODIC TABLE
Ch. 4 Sec. 1-2, Ch. 3 sec.6-8 ENERGY CHANGES AND THE QUANTUM THEORY THE PERIODIC TABLE What Makes Red Light Red? (4.1) Electromagnetic Radiation: energy that travels in waves (light) Waves Amplitude: height
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
4.2 WHERE are the electrons in the { atom???? QUANTUM NUMBERS
4.2 WHERE are the electrons in the { atom???? QUANTUM NUMBERS Bohr s Model Contradicts Common Sense If only certain orbits with definite energies are allowed and the electrons constantly gives off radiation,
Chapter 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
General Chemistry. Contents. Chapter 9: Electrons in Atoms. Contents. 9-1 Electromagnetic Radiation. EM Radiation. Frequency, Wavelength and Velocity
General Chemistry Principles and Modern Applications Petrucci Harwood Herring 8 th Edition Chapter 9: Electrons in Atoms Philip Dutton University of Windsor, Canada N9B 3P4 Contents 9-1 Electromagnetic
#9 Modern Atomic Theory Quantitative Chemistry
Name #9 Modern Atomic Theory Quantitative Chemistry Student Learning Map Unit EQ: What is the current model of the atom? Key Learning: The current model of the atom is based on the quantum mechanical model.
Atoms and Periodic Properties
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Unit 01 (Chp 6,7): Atoms and Periodic Properties John D. Bookstaver St. Charles Community College
Chapter 11. What subatomic particles do you get to play with? Protons Neutrons Eletrons
Chapter 11 What subatomic particles do you get to play with? Protons Neutrons Eletrons changes the element isotopes: only mass is different what we play with in chemistry Bohr Model of the Atom electrons
UNIT TWO TEST HISTORY OF ATOM, STRUCTURE OF ATOM, ATOMIC MASS CARBON-12
KEY Review Sheet: UNIT TWO TEST HISTORY OF ATOM, STRUCTURE OF ATOM, ATOMIC MASS 1. Know which isotope is the standard for the atomic mass unit. CARBON-12 2. Know what the difference in masses of isotopes
Chapter 6. Electronic. Electronic Structure of Atoms Pearson Education
Chapter 6 Laser: step-like energy transition 6.1 The Wave Nature of Light 6.2 Quantized Energy and Photons 6.3 Line Spectra and the Bohr Model 6.4 The Wave Behavior of Matter 6.5 Quantum Mechanics and
The 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
Accounts 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
ATOMIC STRUCTURE. Wavelength and Frequency
ATOMIC STRUCTURE Wavelength and Frequency WAVELENGTH AND FREQUENCY The Wave Nature of Light Electromagnetic Radiation aka. Radiant energy or light A form of energy having both wave and particle characteristics
Georgia Institute of Technology CHEM 1310 revised 10/8/09 Spring The Development of Quantum Mechanics. ν (nu) = frequency (in s -1 or hertz)
The Development of Quantum Mechanics Early physicists used the properties of electromagnetic radiation to develop fundamental ideas about the structure of the atom. A fundamental assumption for their work
White Light. Chapter 7 Electron Structure of the Atom
Chapter 7 Electron Structure of the Atom Electromagnetic Radiation and Energy The Bohr Model of the Hydrogen Atom The Modern Model of the Atom Periodicity of Electron Configurations Valence Electrons for
Remember Bohr s Explanation: Energy Levels of Hydrogen: The Electronic Structure of the Atom 11/28/2011
The Electronic Structure of the Atom Bohr based his theory on his experiments with hydrogen he found that when energy is added to a sample of hydrogen, energy is absorbed and reemitted as light When passed
Chapter 9: Electrons in Atoms
General Chemistry Principles and Modern Applications Petrucci Harwood Herring 8 th Edition Chapter 9: Electrons in Atoms Philip Dutton University of Windsor, Canada N9B 3P4 Prentice-Hall 2002 Prentice-Hall
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
Q1 and Q2 Review large CHEMISTRY
Q1 and Q2 Review large CHEMISTRY Multiple Choice Identify the choice that best completes the statement or answers the question. 1. E = hv relates the following a. Energy to Planck s constant & wavelength
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
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY All matter is made of atoms. There are a limited number of types of atoms; these are the elements. (EU 1.A) Development of Atomic Theory Atoms are so small
Chapter Test B. Chapter: Arrangement of Electrons in Atoms. possible angular momentum quantum numbers? energy level? a. 4 b. 8 c. 16 d.
Assessment Chapter Test B Chapter: Arrangement of Electrons in Atoms PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question
WEEK 2: 4 SEP THRU 10 SEP; LECTURES 4-6
Learning Objectives Energy: Light as energy Describe the wave nature of light, wavelength, and frequency using the equation c = λν What is meant by the particle nature of light? Calculate the energy of
Chemistry 121: Atomic and Molecular Chemistry Topic 3: Atomic Structure and Periodicity
Text Chapter 2, 8 & 9 3.1 Nature of light, elementary spectroscopy. 3.2 The quantum theory and the Bohr atom. 3.3 Quantum mechanics; the orbital concept. 3.4 Electron configurations of atoms 3.5 The periodic
Electronic Structure and the Periodic Table. Unit 6 Honors Chemistry
Electronic Structure and the Periodic Table Unit 6 Honors Chemistry Wave Theory of Light James Clerk Maxwell Electromagnetic waves a form of energy that exhibits wavelike behavior as it travels through
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
CRHS Academic Chemistry Unit 4 Electrons. Notes. Key Dates
Name Period CRHS Academic Chemistry Unit 4 Electrons Notes Key Dates Quiz Date Exam Date Lab Dates Notes, Homework, Exam Reviews and Their KEYS located on CRHS Academic Chemistry Website: https://cincochem.pbworks.com
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