Electrons! Chapter 5
|
|
- Blaise Miles
- 6 years ago
- Views:
Transcription
1 Electrons! Chapter 5
2 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 in chemical behavior a. Example: Cl, Ar, K are #s 17, 18, consecutive atomic numbers, but very different properties -- why? 2. Early 1900s: scientists noticed that some elements produced light when placed in a flame a. Analyzing the specific light emitted showed that chemical behavior was related to electron arrangement
3 B. Light: Wave Nature 1. Wavelength (λ): distance between two neighboring crests or troughs a. unit: usually nanometers (1 x 10-9 m = 1 nm) 2. Frequency (ν): number of waves (measured in # of crests) which pass a given point each second a. unit: hertz (1 Hz = 1 wave/second), kilohertz, megahertz b. in mathematical calculations, use s -1 (1 s -1 = 1 Hz) 3. Amplitude: height of wave from origin to crest or origin to trough 4. Speed of light (c) = 3.00 x 10 8 m/s c = λν ^see p. 119
4 i. Example: A certain red light has a wavelength of 650 nm. What is its frequency? (BRINGIN BACK G.U.E.S.S) G: wavelength = 650 nm, c = 3.00 x 10 8 m/s, 1 Hz = 1 s -1 U: frequency (in Hz) E: c = λν can change to ν = c/λ S: 3.00 x 10 8 m 1 nm 1 1 Hz 1 s 1 x 10-9 m 650 nm 1 s -1 S: 4.62 x Hz
5 5. Electromagnetic (EM) radiation: form of energy released by EM processes that acts like a wave as it travels through space; consists of synchronized electric & magnetic fields a. Electromagnetic (EM) spectrum: spectrum of all EM radiation resulting from fluctuations or vibrations of charged particles (p. 120) i. Includes radio waves, microwaves, radar waves, infrared light, visible light (aka continuous spectrum), ultraviolet, X-rays, and gamma rays ii. Each part of the continuous spectrum corresponds to a specific wavelength & frequency, which are refracted at different angles -- produces colors (ROY G BIV)
6 Practice Problems: p. 121, #1-4
7 C. Light: Particle Nature 1. Wave model of light does not describe all of its interactions with matter, like iron emitting different wavelengths of light (colors) at different temperatures -- so how can these interactions be explained? 2. Max Planck (German physicist, 1890s) wanted to figure this out! a. Studied light emitted from heated objects b. Found that frequencies & energy changed in tiny, specific amounts, and matter can only gain or lose energy in these small amounts (quanta), NOT in any random amount c. Quantum: minimum amount of energy that can be gained or lost by an atom; plural quanta; also called photons d. All energy, including light, comes in quanta -- this is quantum theory e. Each color of light has a specific sized quanta; red is small, violet is large
8 3. Planck proposed a formula that expresses the energy of a single quantum (photon) of radiation of any given frequency E = energy (in joules) E = hν h = Planck s constant, x J s ν = frequency in s -1 a. Example: how much energy is contained in one quantum of a gamma ray? Frequency of gamma ray is 1 x Hz G: h = x J s, ν = 1 x Hz, 1 Hz = 1 s -1 U: energy (in joules) E: E = hν S: x J s 1 x Hz 1 s Hz S: x J b. Example 2: how much energy is contained in one quantum of a radio wave? Frequency of radio wave is 1 x 10 4 Hz
9 4. Albert Einstein (German physicist, 1905) studied the photoelectric effect: light of a certain frequency (color) shining upon a material & causing electrons to be discharged from the material a. Theoretically, a very lowfrequency light directed at a material for a long period of time will eventually accumulate & provide enough energy for the material to eject electrons BUT, that didn t happen -- why?
10 b. Einstein found that when the intensity of light of a particular wavelength was reduced, fewer electrons were ejected, & vice versa i. Based on wave theory, less intense light should cause electrons to be ejected with lower kinetic energy, & vice versa ii. However, electrons emitted at lower intensities still had the same kinetic energy as when the intensity was greater iii.conclusions: Light has both wave & particle properties Light consists of photons: particles of EM radiation carrying a quantum of energy (plain English: light is a stream of tiny bundles of energy) Photons have their own specific energy for a given wavelength; at minimum, one photon possesses the energy necessary to eject an electron from a material
11 Practice Problems: p. 124, #5-6 Homework: p. 126, #7-12
12 Homework Answers p ) 3.61 x J 4) 8.48 x J p a) 4.19 x J 6a) gamma ray or X ray 5b) 6.29 x J 6b) infrared 5c) 6.96 x J 6c) ultraviolet p speed, wavelength, frequency, amplitude; EM waves travel at c 8. Wave model treats light as an EM wave; particle model treats it as comprised of photons. Wave model couldn t explain photoelectric effect, color of hot objects, & emission spectra. 9. A quantum is the minimum amount of energy that can be lost or gained by an atom; matter loses or gains energy in multiples of the quantum 10. Continuous spectrum contains all colors, emission spectra contains only specific colors 11. Einstein proposed that EM radiation has a wave-particle nature, that the energy of a photon depends on the frequency of the radiation, and that a photon s energy is given by E photon = hv 12. a: 3 (radio waves) b: 1 (gamma rays) c: 1 (gamma rays)
13 D. Light Spectra 1. Light is not always absorbed or emitted by a material continuously, as the wave model would suggest -- instead, it is often emitted in bursts by excited electrons 2. Atomic emission spectrum: frequencies of light emitted by a given material a. When substances are passed through a flame, they glow a particular color (example: copper - green, sodium - yellow) b. When this light is passed through a prism & divided, a series of colored lines appears called spectral lines c. Each element has a unique set of lines it produces, so atomic emission spectra (the sets of lines) can be used to identify elements d. Example: hydrogen s emissions spectrum, p. 126
14 II. Quantum Theory & the Atom A.Bohr s Model 1. Proposed a quantum atomic model that explained why atomic emission spectra are only made up of certain frequencies of light, not all continuously 2. Key points: a. There are certain definite orbits in which electrons can travel b. An electron in a given orbit has a certain definite amount of energy c. The greater the distance from the nucleus, the greater the energy of the electron d. Possible electron orbits are called energy levels e. An electron can gain energy from various sources, causing it to jump to a higher level f. When an electron drops to a lower energy level, it loses energy in the form of a photon of radiation g. Energy of the photon corresponds to the difference in energy levels h. An electron cannot drop into an energy level which already holds its maximum number of electrons
15 3. Also mapped out energy levels a. Lowest energy level is called the ground state b. When an atom gains energy, it enters an excited state Bohr described 7 possible excited states/energy levels of hydrogen & assumed it was the same for other atoms c. Atom gains energy electrons jump to higher energy levels d. Atom loses energy in the form of a photon of EM radiation electrons fall back to a lower energy level e. Amount of energy photon carries is determined by the difference in energy levels when an electron falls from an upper level to a lower level ΔE = E higher-energy orbit E lower energy orbit = E photon = hf
16 B. Quantum-Mechanical Model 1. Bohr s model explained hydrogen well, but not really other elements; primarily his ideas of quantized energy & energy levels were correct & expanded upon by several scientists 2. Louis de Broglie suggested that all moving particles have wave properties a. de Broglie equation: λ = h/mv wavelength of any particle is equal to Planck s constant divided by mass times velocity b. He was correct! 3. Heisenberg s uncertainty principle: there is always some uncertainty as to the location & velocity of an electron it is impossible to know both simultaneously 4. Schrödinger treated electron as a wave & came up with an equation to describe its wave-like behavior confirmed electron has both wave & particle properties 5. Wave model predicts that electrons will be found in an atomic orbital: a 3D region around the nucleus
17 C. Hydrogen s Atomic Orbitals 1. Principal quantum number (n): indicates sizes & energies of atomic orbitals a. Corresponds to the energy levels suggested by Bohr (1,2,3,4,5,6,7) called principal energy levels b. Electrons may be found in each energy level of an atom (7 shown on the periodic table) c. Largest possible number of electrons possible in any one level is 2n 2 2. Energy sublevels: contained within principal energy levels a. Number of sublevels contained within each principal energy level = n b. All electrons in each energy level do not have the same energy as earlier assumed c. Determines the shape of the electron cloud d. Four types of sublevels are possible, each with a defined shape & number of electrons: s sharp : lowest sublevel p principal : second sublevel d diffuse : third sublevel f fundamental : fourth sublevel 2e - (1 pair) 6e - (3 pair) 10e - (5 pair) 14e - (7 pair)
18 Copy in notes: Table 5-1 Figure 5-10 a & b
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
More informationChapter 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 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 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 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 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 informationChapter 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 informationLight. October 16, Chapter 5: Electrons in Atoms Honors Chemistry. Bohr Model
Chapter 5: Electrons in Atoms Honors Chemistry Bohr Model Niels Bohr, a young Danish physicist and a student of Rutherford improved Rutherford's model. Bohr proposed that an electron is found only in specific
More informationCHAPTER 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 information5.1 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
More informationLIGHT 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
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 informationArrangement 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
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 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 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 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 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 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 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 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 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. 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 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 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 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 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 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 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 informationDo 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
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 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 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 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 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 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 informationChapter 6. Electronic Structure of Atoms
Chapter 6 Electronic Structure of Atoms 6.1 The Wave Nature of Light Made up of electromagnetic radiation. Waves of electric and magnetic fields at right angles to each other. Parts of a wave Wavelength
More 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 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 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 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 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 informationThe 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
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 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 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 informationDuncan. 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
More informationChapter 8: Electrons in Atoms Electromagnetic Radiation
Chapter 8: Electrons in Atoms Electromagnetic Radiation Electromagnetic (EM) radiation is a form of energy transmission modeled as waves moving through space. (see below left) Electromagnetic Radiation
More informationChapter 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 informationChapter 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
More informationSCH4U: History of the Quantum Theory
SCH4U: History of the Quantum Theory Black Body Radiation When an object is heated, it initially glows red hot and at higher temperatures becomes white hot. This white light must consist of all of the
More informationChemistry 111 Dr. Kevin Moore
Chemistry 111 Dr. Kevin Moore Black Body Radiation Heated objects emit radiation based on its temperature Higher temperatures produce higher frequencies PhotoElectric Effect Light on a clean metal surface
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 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 informationThe 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
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 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 informationPart One: Light Waves, Photons, and Bohr Theory. 2. Beyond that, nothing was known of arrangement of the electrons.
CHAPTER SEVEN: QUANTUM THEORY AND THE ATOM Part One: Light Waves, Photons, and Bohr Theory A. The Wave Nature of Light (Section 7.1) 1. Structure of atom had been established as cloud of electrons around
More informationChapter 6: 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 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 informationHistory 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
More informationElectron Arrangement - Part 1
Brad Collins Electron Arrangement - Part 1 Chapter 8 Some images Copyright The McGraw-Hill Companies, Inc. Properties of Waves Wavelength (λ) is the distance between identical points on successive waves.
More informationThe 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)
More informationOutline Chapter 9 The Atom Photons Photons The Photoelectron Effect Photons Photons
Outline Chapter 9 The Atom 9-1. Photoelectric Effect 9-3. What Is Light? 9-4. X-rays 9-5. De Broglie Waves 9-6. Waves of What? 9-7. Uncertainty Principle 9-8. Atomic Spectra 9-9. The Bohr Model 9-10. Electron
More informationChapter 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 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 informationAtoms, 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
More informationChapter 7: The Quantum-Mechanical Model of the Atom
C h e m i s t r y 1 A : C h a p t e r 7 P a g e 1 Chapter 7: The Quantum-Mechanical Model of the Atom Homework: Read Chapter 7. Work out sample/practice exercises Check for the MasteringChemistry.com assignment
More informationProvide 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
More informationExplain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic radiation.
Preview Objectives Properties of Light Wavelength and Frequency The Photoelectric Effect The Hydrogen-Atom Line-Emission Spectrum Bohr Model of the Hydrogen Atom Photon Emission and Absorption Section
More informationCHAPTER 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
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 informationChapter 7. The Quantum Mechanical Model of the Atom
Chapter 7 The Quantum Mechanical Model of the Atom Quantum Mechanics The Behavior of the Very Small Electrons are incredibly small. Electron behavior determines much of the behavior of atoms. Directly
More informationAtomic Structure and Periodicity. AP Chemistry Ms. Grobsky
Atomic Structure and Periodicity AP Chemistry Ms. Grobsky Food For Thought Rutherford s model became known as the planetary model The sun was the positivelycharged dense nucleus and the negatively-charged
More informationEinstein. Quantum Physics at a glance. Planck s Hypothesis (blackbody radiation) (ultraviolet catastrophe) Quantized Energy
Quantum Physics at a glance Quantum Physics deals with the study of light and particles at atomic and smaller levels. Planck s Hypothesis (blackbody radiation) (ultraviolet catastrophe) Quantized Energy
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 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 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 informationHonors Unit 6 Notes - Atomic Structure
Name: Honors Unit 6 Notes - Atomic Structure Objectives: 1. Students will have a general understanding of the wave nature of light and the interrelationship between frequency, wavelength, and speed of
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 information