Chapter 5 Electrons In Atoms
|
|
- Berenice Carson
- 5 years ago
- Views:
Transcription
1 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. All Rights Reserved. CHEMISTRY & YOU What gives gas-filled lights their colors? An electric current passing through the gas in each glass tube makes the gas glow with its own characteristic color. 2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
2 Light and Atomic Emission Spectra Light and Atomic Emission Spectra What causes atomic emission spectra? 3 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. The Nature of Light By the year 1900, there was enough experimental evidence to convince scientists that light consisted of waves. The amplitude of a wave is the wave s height from zero to the crest. The wavelength, represented by λ (the Greek letter lambda), is the distance between the crests. Light and Atomic Emission Spectra 4 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
3 The Nature of Light Light and Atomic Emission Spectra The frequency, represented by ν (the Greek letter nu), is the number of wave cycles to pass a given point per unit of time. The SI unit of cycles per second is called the hertz (Hz). 5 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. The Nature of Light Light and Atomic Emission Spectra The product of frequency and wavelength equals a constant (c), the speed of light. c = λν 6 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
4 Light and Atomic Emission Spectra The frequency (ν) and wavelength (λ) of light are inversely proportional to each other. As the wavelength increases, the frequency decreases. 7 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Light and Atomic Emission Spectra The Nature of Light According to the wave model, light consists of electromagnetic waves. Electromagnetic radiation includes radio waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays. All electromagnetic waves travel in a vacuum at a speed of m/s. 8 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
5 The Nature of Light Light and Atomic Emission Spectra The sun and incandescent light bulbs emit white light, which consists of light with a continuous range of wavelengths and frequencies. When sunlight passes through a prism, the different wavelengths separate into a spectrum of colors. In the visible spectrum, red light has the longest wavelength and the lowest frequency. 9 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Light and Atomic Emission Spectra The electromagnetic spectrum consists of radiation over a broad range of wavelengths. Low energy (λ = 700 nm) High energy (λ = 380 nm) Frequency ν (s -1 ) 3 x x x Wavelength λ (m) 10 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
6 Light and Atomic Emission Spectra Atomic Emission Spectra When atoms absorb energy, their electrons move to higher energy levels. These electrons lose energy by emitting light when they return to lower energy levels. 11 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Light and Atomic Emission Spectra Atomic Emission Spectra A prism separates light into the colors it contains. White light produces a rainbow of colors. Screen Light bulb Slit Prism 12 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
7 Sample Problem 5.2 Calculating the Wavelength of Light Calculate the wavelength of the yellow light emitted by a sodium lamp if the frequency of the radiation is Hz. 13 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Sample Problem Analyze List the knowns and the unknown. Use the equation c = λν to solve for the unknown wavelength. KNOWNS frequency (ν) = /s c = m/s UNKNOWN wavelength (λ) =? m 14 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
8 Sample Problem Calculate Solve for the unknown. Write the expression that relates the frequency and wavelength of light. c = λν 15 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Sample Problem Calculate Solve for the unknown. Rearrange the equation to solve for λ. c = λν λ = ν c Solve for λ by dividing both sides by ν: c ν = λν ν 16 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
9 Sample Problem Calculate Solve for the unknown. Substitute the known values for ν and c into the equation and solve. c λ = = 8 m/s = m ν /s 17 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. What is the frequency of a red laser that has a wavelength of 676 nm? 18 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
10 What is the frequency of a red laser that has a wavelength of 676 nm? c = λν ν = c ν = = 8 m/s λ /s = m c λ 19 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. The Quantum Concept and Photons The Quantum Concept and Photons How did Einstein explain the photoelectric effect? 20 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
11 The Quantum Concept and Photons The Quantization of Energy German physicist Max Planck ( ) showed mathematically that the amount of radiant energy (E) of a single quantum absorbed or emitted by a body is proportional to the frequency of radiation (ν). E ν or E = hν 21 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. The Quantum Concept and Photons The Quantization of Energy The constant (h), which has a value of J s (J is the joule, the SI unit of energy), is called Planck s constant. E ν E or E ν = or hνe = hν 22 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
12 The Quantum Concept and Photons The Photoelectric Effect Albert Einstein used Planck s quantum theory to explain the photoelectric effect. In the photoelectric effect, electrons are ejected when light shines on a metal. 23 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. The Quantum Concept and Photons The Photoelectric Effect To explain the photoelectric effect, Einstein proposed that light could be described as quanta of energy that behave as if they were particles. 24 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
13 The Quantum Concept and Photons The Photoelectric Effect These light quanta are called photons. Einstein s theory that light behaves as a stream of particles explains the photoelectric effect and many other observations. 25 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. The Quantum Concept and Photons The Photoelectric Effect These light quanta are called photons. Einstein s theory that light behaves as a stream of particles explains the photoelectric effect and many other observations. Light behaves as waves in other situations; we must consider that light possesses both wavelike and particle-like properties. 26 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
14 The Quantum Concept and Photons The Photoelectric Effect No electrons are ejected because the frequency of the light is below the threshold frequency. If the light is at or above the threshold frequency, electrons are ejected. If the frequency is increased, the ejected electrons will travel faster. 27 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. An Explanation of Atomic Spectra When an electron has its lowest possible energy, the atom is in its ground state. In the ground state, the principal quantum number (n) is Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
15 An Explanation of Atomic Spectra When an electron has its lowest possible energy, the atom is in its ground state. In the ground state, the principal quantum number (n) is 1. Excitation of the electron by absorbing energy raises the atom to an excited state with n = 2, 3, 4, 5, or 6, and so forth. A quantum of energy in the form of light is emitted when the electron drops back to a lower energy level. 29 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Quantum Mechanics The Heisenberg Uncertainty Principle The Heisenberg uncertainty principle states that it is impossible to know both the velocity and the position of a particle at the same time. 30 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
16 Quantum Mechanics The Heisenberg Uncertainty Principle The Heisenberg uncertainty principle states that it is impossible to know both the velocity and the position of a particle at the same time. This limitation is critical when dealing with small particles such as electrons. But it does not matter for ordinary-sized objects such as cars or airplanes. 31 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Quantum Mechanics To locate an electron, you might strike it with a photon. The electron has such a small mass that striking it with a photon affects its motion in a way that cannot be predicted accurately. The very act of measuring the position of the electron changes its velocity, making its velocity uncertain. Before collision: A photon strikes an electron during an attempt to observe the electron s position. After collision: The impact changes the electron s velocity, making it uncertain. 32 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
17 The Heisenberg uncertainty principle states that it is impossible to simultaneously know which two attributes of a particle? 33 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. The Heisenberg uncertainty principle states that it is impossible to simultaneously know which two attributes of a particle? velocity and position 34 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
18 Key Concepts and Key Equations When atoms absorb energy, their electrons move to higher energy levels. These electrons lose energy by emitting light when they return to lower energy levels. To explain the photoelectric effect, Einstein proposed that light could be described as quanta of energy that behave as if they were particles. The light emitted by an electron moving from a higher to a lower energy level has a frequency directly proportional to the energy change of the electron. 35 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Key Concepts and Key Equations Classical mechanics adequately describes the motions of bodies much larger than atoms, while quantum mechanics describes the motions of subatomic particles and atoms as waves. C = λν E = h ν 36 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
19 Glossary Terms amplitude: the height of a wave s crest wavelength: the distance between adjacent crests of a wave frequency: the number of wave cycles that pass a given point per unit of time; frequency and wavelength are inversely proportional to each other hertz: the unit of frequency, equal to one cycle per second 37 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Glossary Terms electromagnetic radiation: energy waves that travel in a vacuum at a speed of m/s; includes radio waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays spectrum: wavelengths of visible light that are separated when a beam of light passes through a prism; range of wavelengths of electromagnetic radiation 38 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
20 Glossary Terms atomic emission spectrum: the pattern formed when light passes through a prism or diffraction grating to separate it into the different frequencies of light it contains Planck s constant: the constant (h) by which the amount of radiant energy (E) is proportional to the frequency of the radiation (ν) photoelectric effect: the phenomenon in which electrons are ejected when light shines on a metal 39 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Glossary Terms photon: a quantum of light; a discrete bundle of electromagnetic energy that interacts with matter similarly to particles ground state: the lowest possible energy of an atom described by quantum mechanics Heisenberg uncertainty principle: it is impossible to know both the velocity and the position of a particle at the same time 40 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
21 BIG IDEA Electrons and the Structure of Atoms Electrons can absorb energy to move from one energy level to a higher energy level. When an electron moves from a higher energy level back down to a lower energy level, light is emitted. 41 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. END OF Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
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.
More informationc = λν 10/23/13 What gives gas-filled lights their colors? Chapter 5 Electrons In Atoms
CHEMISTRY & YOU What gives gas-filled lights their colors? Chapter 5 Electrons In Atoms 5.1 Revising the Atomic Model 5. Electron Arrangement in Atoms 5.3 Atomic and the Quantum Mechanical Model An electric
More informationPhysics 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
More information5.3. 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
More informationThe 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
More informationNOTES: 5.3 Light and Atomic Spectra (more Quantum Mechanics!)
NOTES: 5.3 Light and Atomic Spectra (more Quantum Mechanics!) Light WAVE or PARTICLE? Electromagnetic Radiation Electromagnetic radiation includes: -radio waves -microwaves -infrared waves -visible light
More informationWrite 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
More informationTable of Contents Electrons in Atoms > Light and Quantized Energy > Quantum Theory and the Atom > Electron Configuration
Electrons in Atoms October 20, 2014 Table of Contents Electrons in Atoms > Light and Quantized Energy > Quantum Theory and the Atom > Electron Configuration 1 Electromagnetic Spectrum Electromagnetic radiation
More informationThe Bohr Model of the Atom
Unit 4: The Bohr Model of the Atom Properties of light Before the 1900 s, light was thought to behave only as a wave. Light is a type of electromagnetic radiation - a form of energy that exhibits wave
More informationElectrons! 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
More informationChapter 6. Quantum Theory and the Electronic Structure of Atoms Part 1
Chapter 6 Quantum Theory and the Electronic Structure of Atoms Part 1 The nature of light Quantum theory Topics Bohr s theory of the hydrogen atom Wave properties of matter Quantum mechanics Quantum numbers
More informationName 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
More informationName 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
More informationThe 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
More informationI understand the relationship between energy and a quanta I understand the difference between an electron s ground state and an electron s excited
NCCS 1.1.2 & 1.1.3 I understand the relationship between energy and a quanta I understand the difference between an electron s ground state and an electron s excited state I will describe how an electron
More informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change Chapter 5: Electrons in Atoms 5 Section 5.1 Section Section 5.3 Table Of Contents Light and Quantized Energy Electron Configuration Compare the wave and particle natures of
More informationChapter 7 Atomic Structure -1 Quantum Model of Atom. Dr. Sapna Gupta
Chapter 7 Atomic Structure -1 Quantum Model of Atom Dr. Sapna Gupta The Electromagnetic Spectrum The electromagnetic spectrum includes many different types of radiation which travel in waves. Visible light
More informationProperties of Light. Arrangement of Electrons in Atoms. The Development of a New Atomic Model. Electromagnetic Radiation CHAPTER 4
CHAPTER 4 Arrangement of Electrons in Atoms The Development of a New Atomic Model The Rutherford model was a great improvement over the Thomson model of the atom. But, there was one major question that
More informationUnit 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
More informationYellow. Strontium red white. green. yellow violet. green. red. Chapter 4. Arrangement of Electrons in Atoms. Table of Contents
Chapter 4 Arrangement of Electrons in Atoms Table of Contents Section 1 Section 2 Section 3 The Development of a New Atomic Model The Quantum Model of the Atom Electron Configurations Sodium Yellow Strontium
More informationChapter 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
More informationWavelength (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
More informationCh 7 Quantum Theory of the Atom (light and atomic structure)
Ch 7 Quantum Theory of the Atom (light and atomic structure) Electromagnetic Radiation - Electromagnetic radiation consists of oscillations in electric and magnetic fields. The oscillations can be described
More informationQuantum Theory of the Atom
The Wave Nature of Light Quantum Theory of the Atom Electromagnetic radiation carries energy = radiant energy some forms are visible light, x rays, and radio waves Wavelength ( λ) is the distance between
More informationEnergy 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.
More informationUnit 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
More informationName 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
More informationLight. October 16, Chapter 5: Electrons in Atoms Honors Chemistry. Bohr Model
Chapter 5: Electrons in Atoms Honors Chemistry Bohr Model Niels Bohr, a young Danish physicist and a student of Rutherford improved Rutherford's model. Bohr proposed that an electron is found only in specific
More informationThe 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
More informationCHEMISTRY - 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
More informationLight, 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
More informationElectrons in Atoms. Section 5.1 Light and Quantized Energy Section 5.2 Quantum Theory and the Atom Section 5.3 Electron Configuration
Electrons in Atoms Section 5.1 Light and Quantized Energy Section 5.2 Quantum Theory and the Atom Section 5.3 Electron Configuration Click a hyperlink or folder tab to view the corresponding slides. Exit
More informationCalendar. 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
More informationLecture 11 Atomic Structure
Lecture 11 Atomic Structure Earlier in the semester, you read about the discoveries that lead to the proposal of the nuclear atom, an atom of atomic number Z, composed of a positively charged nucleus surrounded
More informationElectromagnetic 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
More informationElectrons 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.
More informationProperties 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
More informationName 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
More informationWAVE NATURE OF LIGHT
WAVE NATURE OF LIGHT Light is electromagnetic radiation, a type of energy composed of oscillating electric and magnetic fields. The fields oscillate perpendicular to each other. In vacuum, these waves
More information10/4/2011. 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
More informationChapter 5. The Electromagnetic Spectrum. What is visible light? What is visible light? Which of the following would you consider dangerous?
Which of the following would you consider dangerous? X-rays Radio waves Gamma rays UV radiation Visible light Microwaves Infrared radiation Chapter 5 Periodicity and Atomic Structure 2 The Electromagnetic
More informationCHAPTER 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
More informationElectronic structure of atoms
Chapter 1 Electronic structure of atoms light photons spectra Heisenberg s uncertainty principle atomic orbitals electron configurations the periodic table 1.1 The wave nature of light Much of our understanding
More informationConceptual Physics Fundamentals
Conceptual Physics Fundamentals Chapter 15: QUANTUM THEORY This lecture will help you understand: The Photoelectric Effect Absorption Spectra Fluorescence Incandescence Lasers Wave-Particle Duality Particles
More informationBohr. 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
More information2) The energy of a photon of light is proportional to its frequency and proportional to its wavelength.
Advanced Chemistry Chapter 13 Review Name Per Show all work Wave Properties 1) Which one of the following is correct? A) ν + λ = c B) ν λ = c C) ν = cλ D) λ = c ν E) νλ = c 2) The energy of a photon of
More informationSupplemental Activities. Module: Atomic Theory. Section: Electromagnetic Radiation and Matter - Key
Supplemental Activities Module: Atomic Theory Section: Electromagnetic Radiation and Matter - Key Introduction to Electromagnetic Radiation Activity 1 1. What are the two components that make up electromagnetic
More informationBellwork: Calculate the atomic mass of potassium and magnesium
Bellwork: Calculate the atomic mass of potassium and magnesium Chapter 5 - electrons in atoms Section 5.1: Revising the atomic model What did Ernest Rutherford think about electrons? In Rutherford s model,
More informationElectrons in Atoms. Section 5.1 Light and Quantized Energy
Name Date Class 5 Electrons in Atoms Section 5.1 Light and Quantized Energy In your textbook, read about the wave nature of light. Use each of the terms below just once to complete the passage. amplitude
More informationEXPERIMENT 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
More informationThe Electron Cloud. Here is what we know about the electron cloud:
The Electron Cloud Here is what we know about the electron cloud: It contains the subatomic particles called electrons This area accounts for most of the volume of the atom ( empty space) These electrons
More informationChapter 6 Electronic Structure of Atoms
Chapter 6 Electronic Structure of Atoms What is the origin of color in matter? Demo: flame tests What does this have to do with the atom? Why are atomic properties periodic? 6.1 The Wave Nature of Light
More informationAP Chemistry. Chapter 6 Electronic Structure of Atoms
AP Chemistry Chapter 6 Electronic Structure of Atoms Section 6.1 Wave Nature of Light When we say "light," we generally are referring to visible light a type of electromagnetic radiation But actually Visible
More informationChapter 7. The Quantum Mechanical Model of the Atom
Chapter 7 The Quantum Mechanical Model of the Atom The Nature of Light:Its Wave Nature Light is a form of electromagnetic radiation composed of perpendicular oscillating waves, one for the electric field
More informationElectrons, 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.
More informationChapter 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
More informationChapter 7. Quantum Theory and Atomic Structure
Chapter 7 Quantum Theory and Atomic Structure Outline 1. The Nature of Light 2. Atomic Spectra 3. The Wave-Particle Duality of Matter and Energy 4. The Quantum-Mechanical Model of the Atom 3 September
More information2) The number of cycles that pass through a stationary point is called A) wavelength. B) amplitude. C) frequency. D) area. E) median.
Chemistry Structure and Properties 2nd Edition Tro Test Bank Full Download: http://testbanklive.com/download/chemistry-structure-and-properties-2nd-edition-tro-test-bank/ Chemistry: Structure & Properties,
More informationExplain how Planck resolved the ultraviolet catastrophe in blackbody radiation. Calculate energy of quanta using Planck s equation.
Objectives Explain how Planck resolved the ultraviolet catastrophe in blackbody radiation. Calculate energy of quanta using Planck s equation. Solve problems involving maximum kinetic energy, work function,
More informationChapter 7. The Quantum- Mechanical Model of the Atom. Chapter 7 Lecture Lecture Presentation. Sherril Soman Grand Valley State University
Chapter 7 Lecture Lecture Presentation Chapter 7 The Quantum- Mechanical Model of the Atom Sherril Soman Grand Valley State University The Beginnings of Quantum Mechanics Until the beginning of the twentieth
More informationUNIT 4 Electrons in Atoms. Advanced Chemistry 235 Lanphier High School Mr. David Peeler
UNIT 4 Electrons in Atoms Advanced Chemistry 235 Lanphier High School Mr. David Peeler Section 4.1 Models of the Atom OBJECTIVES: Identify the inadequacies in the Rutherford atomic model. Section 4.1 Models
More informationThe 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
More informationGeneral 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
More informationEnergy and the Quantum Theory
Energy and the Quantum Theory Light electrons are understood by comparing them to light 1. radiant energy 2. travels through space 3. makes you feel warm Light has properties of waves and particles Amplitude:
More informationChapter 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
More informationElectromagnetic 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.
More informationThe 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
More informationChapter 6 - Electronic Structure of Atoms
Chapter 6 - Electronic Structure of Atoms 6.1 The Wave Nature of Light To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation Visible light is an example
More informationChapter 7 QUANTUM THEORY & ATOMIC STRUCTURE Brooks/Cole - Thomson
Chapter 7 QUANTUM THEORY & ATOMIC STRUCTURE 1 7.1 The Nature of Light 2 Most subatomic particles behave as PARTICLES and obey the physics of waves. Light is a type of electromagnetic radiation Light consists
More informationBackground: 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
More informationDemocritus 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
More informationPart One: Light Waves, Photons, and Bohr Theory. 2. Beyond that, nothing was known of arrangement of the electrons.
CHAPTER SEVEN: QUANTUM THEORY AND THE ATOM Part One: Light Waves, Photons, and Bohr Theory A. The Wave Nature of Light (Section 7.1) 1. Structure of atom had been established as cloud of electrons around
More informationCh. 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
More informationChapter 6 Electronic structure of atoms
Chapter 6 Electronic structure of atoms light photons spectra Heisenberg s uncertainty principle atomic orbitals electron configurations the periodic table 6.1 The wave nature of light Visible light is
More informationElectronic structure the number of electrons in an atom as well as the distribution of electrons around the nucleus and their energies
Chemistry: The Central Science Chapter 6: Electronic Structure of Atoms Electronic structure the number of electrons in an atom as well as the distribution of electrons around the nucleus and their energies
More informationNovember 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
More information5.111 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
More informationChapter 38. Photons Light Waves Behaving as Particles
Chapter 38 Photons Light Waves Behaving as Particles 38.1 The Photoelectric Effect The photoelectric effect was first discovered by Hertz in 1887, and was explained by Einstein in 1905. The photoelectric
More informationChapter 4. Table of Contents. Section 1 The Development of a New Atomic Model. Section 2 The Quantum Model of the Atom
Arrangement of Electrons in Atoms Table of Contents Section 1 The Development of a New Atomic Model Section 2 The Quantum Model of the Atom Section 3 Electron Configurations Section 1 The Development of
More informationCHEMISTRY - ZUMDAHL 8E CH.7 - ATOMIC STRUCTURE & PERIODICITY.
!! 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
More informationDevelopment of the Periodic Table. Chapter 5. Light and the EM Spectrum. Light
Chapter 5 Periodic Table Song Periodicity and Atomic Structure Development of the Periodic Table Mid-1800 s, several scientists placed known elements in order based on different criteria. Mendeleev s and
More informationChapter 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,
More informationChapter 6 Electronic Structure of Atoms
Chapter 6. Electronic Structure of Atoms NOTE: Review your notes from Honors or regular Chemistry for the sequence of atomic models and the evidence that allowed scientists to change the model. If you
More informationQuantum Theory of the Atom
Quantum Theory of the Atom The Wave Nature of Light A wave is a continuously repeating change or oscillation in matter or in a physical field. Light is also a wave. It consists of oscillations in electric
More informationChapter 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
More informationCRHS 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
More informationAccounts for certain objects being colored. Used in medicine (examples?) Allows us to learn about structure of the atom
1.1 Interaction of Light and Matter Accounts for certain objects being colored Used in medicine (examples?) 1.2 Wavelike Properties of Light Wavelength, : peak to peak distance Amplitude: height of the
More informationCh. 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
More informationUnit 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
More informationAtomic Structure and the Periodic Table
Atomic Structure and the Periodic Table The electronic structure of an atom determines its characteristics Studying atoms by analyzing light emissions/absorptions Spectroscopy: analysis of light emitted
More informationElectrons, Energy, & the Electromagnetic Spectrum Notes
Electrons, Energy, & the Electromagnetic Spectrum Notes Bohr Model Diagram Interpretation What form of EM radiation is released when an electron in a hydrogen atom falls from the 5 th energy level to the
More informationThe Structure of the Atom
CHAPTER 5 The Structure of the Atom 5.4 Light and Spectroscopy 460 370 BC 1808 1870 1897 1910 1925 Today Democritus Atomism Dalton Modern atomic theory Crookes Cathode rays Thomson Discovery of the electron
More informationElectronic Structure of Atoms. Chapter 6
Electronic Structure of Atoms Chapter 6 Electronic Structure of Atoms 1. The Wave Nature of Light All waves have: a) characteristic wavelength, λ b) amplitude, A Electronic Structure of Atoms 1. The Wave
More informationChapter 6: The Electronic Structure of the Atom Electromagnetic Spectrum. All EM radiation travels at the speed of light, c = 3 x 10 8 m/s
Chapter 6: The Electronic Structure of the Atom Electromagnetic Spectrum V I B G Y O R All EM radiation travels at the speed of light, c = 3 x 10 8 m/s Electromagnetic radiation is a wave with a wavelength
More informationIntroduction. 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
More informationThe 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
More informationThe Duality of Light. Electromagnetic Radiation. Light as a Wave
In this unit, you will be introduced to the dual nature of light, the quantum theory and Bohr s planetary atomic model. The planetary model was an improvement on the nuclear model and attempted to answer
More informationLecture 6 - Atomic Structure. Chem 103, Section F0F Unit II - Quantum Theory and Atomic Structure Lecture 6. Lecture 6 - Introduction
Chem 103, Section F0F Unit II - Quantum Theory and Atomic Structure Lecture 6 Light and other forms of electromagnetic radiation Light interacting with matter The properties of light and matter Lecture
More informationCHAPTER 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
More informationAtomic 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
More information