Chapter 7: Electrons in Atoms. Electromagnetic Radiation

Size: px
Start display at page:

Download "Chapter 7: Electrons in Atoms. Electromagnetic Radiation"

Transcription

1 Chapter 7: Electrons in Atoms Dr. Chris Kozak Memorial University of Newfoundland, Canada 1 Electromagnetic Radiation Electric and magnetic fields propagate as waves through empty space or through a medium. A wave transmits energy. 10 1

2 EM Radiation Low ν High ν 11 Frequency, Wavelength and Velocity Frequency (ν) in Hertz Hz or s -1. Wavelength (λ) in meters m. cm µm nm Å pm (10-2 m) (10-6 m) (10-9 m) (10-10 m) (10-12 m) Velocity (c) x 10 8 m s -1. c = λν λ = c/ν ν= c/λ 12 2

3 What is the frequency of light corresponding to blue light? λ = 473 nm. c = 2.998x10 8 m s -1. A. 1.58x10-15 s -1 B. 1.42x10-15 s -1 C. 6.33x10-14 s -1 D. 1.42x10-2 s -1 E. 1.42x10 2 s -1 F. 6.33x10 14 s -1 G. 1.42x10 15 s -1 H. 1.58x10 15 s -1 Electromagnetic Spectrum 14 3

4 Constructive and Destructive Interference 15 Refraction of Light 16 4

5 Atomic Spectra Hydrogen Helium Lithium Sodium Potassium 17 Atomic Spectra 18 5

6 Blackbody Radiation 3 phenomena confounded physicists at the turn of the 20 th century: 1) Atomic Spectra 2) Photoelectric effect 3) Blackbody radiation When a solid object is heated to 1000K, visible light is emitted. As T increases, intensity and wavelength change. Why? This is characteristic of blackbody radiation (a hypothetical body that absorbs and emits all frequencies of radiation). We see the colour and intensity of light increase in each of these increase K Embers in a fire 1500 K Stove heating element 2000 K 19 Light bulb filament Quantum Theory Blackbody Radiation: So, heated bodies emit light. In Blackbody Radiation, Intensity (I) is inversely proportional to wavelength (λ), or, it increases with increasing frequency (v). I proportional to 1/λ. Classical theory predicts continuous increase of intensity with frequency. However, in reality the intensity drops off after specific wavelengths. Max Planck, 1900: Energy, like matter, is discontinuous. ΔE = Δnhν E is energy, n is a positive integer, h = x J. s (Planck s constant) and ν is frequency in hertz (s -1 ) 20 6

7 What is the energy corresponding to blue light? λ = 473 nm h= x J s, c=2.998x10 8 m s -1. Δ E = h ν, ν = c / λ Enter your answer between 0 and 1000 kj mol -1 Rank Responses Other The Photoelectric Effect Light striking the surface of certain metals causes ejection of electrons Wave properties of light is unable to explain some observations ν > ν o threshold frequency (Light must have a minimum frequency or no current flows) ne - a I # of e - depends on intensity (Absence of Lag time. Current flow is immediate. The metal does not accumulate energy to eject the electron as predicted by wave theory) E k α ν kinetic energy depends on frequency (Wave theory says that amplitude, not frequency is responsible so any colour of light should be able to do this so long as it is bright enough. This can t be right!) 22 7

8 The Photoelectric Effect 23 The Bohr Atom Electrons move in circular orbits about the nucleus (like in classical physics) Fixed set of stationary states (allowed orbits) Governed by angular momentum: nh/2π, n=1, 2, 3. Energy packets (quanta) are absorbed or emitted when electrons change stationary states The integral values that are allowed are called quantum numbers The energy of an electron becomes increasingly negative the closer it gets to the nucleus according to E = -R H /n 2. R H is a constant Why is electron E a negative value? E = -R H n 2 R H = x J 24 8

9 Energy-Level Diagram ΔE = E f E i = 1 = R H ( ni 2 1 n f 2 -R H n f 2 -R H n i 2 ) = hν = hc/λ 25 Ionization Energy of Hydrogen 1 ΔE = R H ( ni 2 1 n f 2 ) = hν As n f goes to infinity for hydrogen starting in the ground state: 1 hν = R H ( ) = R ni 2 H This also works for hydrogen-like (1-electron) species such as He + and Li 2+ hν = -Z 2 RH Z is the nuclear charge (number of protons) 26 9

10 Great, but what do we really need to know? Calculate the energy, frequency and wavelength for any hydrogen atom transition Identify the wavelengths of the electromagnetic spectrum as being in the UV, visible or IR regions. You should be able to do Examples & 7.5 in Tro (and the practice examples) 27 Summary of Bohr s Atomic Theory Electrons are in motion around the nucleus (orbits) But, for circular orbits, electrons would possess angular momentum (acceleration) and therefore radiate energy! So, using Planck s quantum hypothesis, 1) Electrons move in fixed orbits around the nucleus 2) Fixed orbits (stationary states) mean properties of individual electrons will have unique values, for example, the angular momentum is quantized based on the orbit in which the electron resides. 3) Electrons only pass between allowed orbits. This means that fixed quanta of energy are involved. QUANTUM NUMBERS! 28 10

11 What is Bohr s Theory Good For? Approximations of the energy associated with transitions (movement) of electrons ONLY in ions with one electron! Can t explain: spectra of species with more than one electron effect of magnetic fields on emission spectra It is an uneasy mixture of classical and non-classical physics. Modern quantum theory replaced Bohr theory in Which of the following transi1ons emits a photon with the greatest wavelength? A. n=4 to n=2 B. n=2 to n=1 C. n=4 to n=3 11

12 Determine the energy of light emiaed by a hydrogen atom for the transi1on of an electron from n=3 to n=2. Input an answer in kj mol - 1. Rank Responses Other hap://snews.bnl.gov/popsci/atom1.jpg What is the energy of the photon emiaed associated when the electron in O 7+ undergoes a n=3 to n=2 transi1on Input an answer in kj mol - 1. Rank Responses Other hap:// Oxygen%20Spec%20sm.jpg 12

13 Two Ideas Leading to a New Quantum Mechanics Wave-Particle Duality Heisenberg s Uncertainty Principle 33 Fire Photon Torpedoes! Wave-Particle Duality. Einstein suggested particle-like properties of light could explain the photoelectric effect. But diffraction patterns suggest photons are wavelike. de Broglie, 1924 Small particles of matter may at times display wavelike properties. The concept of the photon! 34 13

14 de Broglie and Matter Waves E = mc 2 hν = mc 2 hν/c = mc = p p = h/λ Einstein s Relativity Equation Planck s Equation for Energy Rearrange to give momentum, p Momentum carried by a photon in relation to its wavelength! λ = h/p = h/mu The wavelength is related to the mass of the particle (particle property) If matter waves exist for small particles, then beams of particles should exhibit the characteristic properties of waves: diffraction. 35 X-Ray Diffraction Structure 1 Structure

15 The Uncertainty Principle Werner Heisenberg Δx Δp h 4π Δx is uncertainty in position Δp is uncertainty in momentum We cannot measure the exact position or exact momentum of a subatomic particle simultaneously WHY?! 37 Sample Problems 1. Some Diamonds appear yellow because they contain nitrogen compounds that absorb purple light with a frequency of 7.23 x Hz. Calculate the wavelength in nm of absorbed light. 2. Calculate the E of one photon of UV (λ = 1 x 10-8 m), visible (λ = 5 x 10-7 m) and IR (λ = 1 x 10-4 m) light. What do the answers indicate about the relationship between λ and E? 3. Calculate the Energy required to remove an electron from a hydrogen atom in its ground state. 4. Calculate the wavelength of the transition from n = 4 to n = 1 in Hydrogen (one of the Lyman series of transitions). 5. Calculate the de Broglie wavelengths of a 50 kg mass travelling at ¼ the speed of light and for a proton (m = x kg) travelling at this speed. What do these wavelengths say about the wave properties of matter in relation to their size? 38 15

16 Wave Mechanics Standing waves. Nodes do not undergo displacement. 2L λ =, n = 1, 2, 3 n 39 Wave Functions ψ, psi, the wave function. Should correspond to a standing wave within the boundary of the system being described. Particle in a box. ψ = 2 L nπ x sin L 40 16

17 Probability of Finding an Electron 41 Wave Functions for Hydrogen Schrödinger, 1927 Eψ = Hψ H (x,y,z) or H (r,θ,φ) ψ(r,θ,φ) = R(r) Y(θ,φ) R(r) is the radial wave function. Y(θ,φ) is the angular wave function

18 Principle Shells and Subshells Principle electronic shell, n = 1, 2, 3 Angular momentum quantum number, l = 0, 1, 2 (n-1) I = 0, s l = 1, p l = 2, d l = 3, f Magnetic quantum number, m l = - l -2, -1, 0, 1, 2 +l 43 Orbital Energies 44 18

19 9-8 Interpreting and Representing the Orbitals of the Hydrogen Atom. 45 s orbitals 46 19

20 p Orbitals 47 p Orbitals 48 20

21 d Orbitals 49 Electron Spin: A Fourth Quantum Number 50 21

22 Electronic Structure of the H atom We have 3 quantum numbers for H n = 1 l = 0 m l = 0 m s 1s orbital Only one type of orbital orientation/ symmetry Only one electron (can be either +1/2 or -1/2) Ground State Configuration: 1s 1 51 Which of the following best represents an orbital with principal and angular momentum quantum numbers 4 and 1, respec1vely? A. B. C. D. E. 22

23 Multi-electron Atoms Schrödinger equation was for only one e -. Electron-electron repulsion in multi-electron atoms. Assume they have Hydrogen-like orbitals (by approximation). 53 Electron Configurations Three Main Principles Aufbau process. Build up and minimize energy. Pauli exclusion principle. No two electrons can have all four quantum numbers alike. Hund s rule. Degenerate orbitals are occupied singly first and with parallel spins

24 Which of the following orbital designa1ons is impossible? A. n=2, l = 0, m l = 0 B. n=3, l = 0, m l = 0 C. n=3, l = 1, m l = 1 D. n=3, l = 2, m l = - 1 E. n=3, l = 3, m l = - 3 Which of the following sets of quantum numbers is NOT matched with the orbital designa1on. A. n=1, l = 0: a 1s orbital B. n=2, l = 0: a 2p orbital C. n=3, l = 0: a 3s orbital D. n=3, l = 1: a 3p orbital E. n=3, l = 2: a 3d orbital 24

25 Orbital Energies 57 How many electrons can have the following set of quantum numbers? Rank n = 3 Responses 6 Other Energy 5s 4s 3s 2s 4p 3p 2p 4p 4p 3p 3p 2p 2p 4d 4d 4d 4d 4d 3d 3d 3d 3d 3d 1s Multi-Electron Atom Atom 25

26 Orbital Filling for Atoms Only 59 Aufbau Process and Hund s Rule spdf notation: C (carbon) 1s 2 2s 2 2p 2 Expanded notation: 1s 2 2s 2 2p x1 p y

27 Filling p Orbitals (Electrons in Boxes) 61 Filling the d Orbitals 62 27

28 To which element does the following orbital filling diagram belong? A. C B. N C. Si D. P E. None of these. Which of the following is the condensed electron configura1on for chlorine? A. [Ne]3p7 B. [Ne]3s23p5 C. [Ne]3s23p6 D. [Ne]3s23d5 E. [Ne]3s23p33d2 Cl2(g) Cl2(l) 28

29 The electron configura1on for Ca is A. [Ar]3s 2 B. [Ar]3s4s C. [Ar]4s 2 D. [Ar]3s 4 E. [Ar]4p 2 The electron configura1on for Br is A. [Ar] 4s 2 3d 10 4p 5 B. [Ar] 4s 2 4d 10 4p 5 C. [Ar] 4s 2 5d 10 4p 5 D. [Ar] 5s 2 4d 10 5p 5 E. [Ar] 4s 2 5d 9 4p 6 29

30 The electron configura1on for Mo is A. [Kr] 4s 2 3d 4 B. [Kr] 4s 2 4p 4 C. [Kr] 5s 2 5d 4 D. [Kr] 5s 2 4d 4 E. [Kr] 5s 1 5d 5 The electron configura1on for Sn is A. [Kr] 4s 2 3d 10 5p 2 B. [Kr] 5s 2 4d 10 5p 2 C. [Kr] 5s 2 5d 10 5p 2 D. [Kr] 5s 2 4d 10 5p 2 E. [Kr] 5s 2 6d 5 5p 2 30

31 Which of the following represents an excited state electron configura1on? A. C A.. B.. B. N C.. D.. C. O E.. D. Si 2s 2s 2s 3s 2p 2p 2p 3p E. P 3s 3p 8-12 Electron Configurations and the Periodic Table 70 31

Atomic Structure: Chapter Problems

Atomic Structure: Chapter Problems Atomic Structure: Chapter Problems Bohr Model Class Work 1. Describe the nuclear model of the atom. 2. Explain the problems with the nuclear model of the atom. 3. According to Niels Bohr, what does n stand

More information

TIME OF COMPLETION NAME SOLUTION DEPARTMENT OF NATURAL SCIENCES. PHYS 3650, Exam 2 Section 1 Version 1 October 31, 2005 Total Weight: 100 points

TIME OF COMPLETION NAME SOLUTION DEPARTMENT OF NATURAL SCIENCES. PHYS 3650, Exam 2 Section 1 Version 1 October 31, 2005 Total Weight: 100 points TIME OF COMPLETION NAME SOLUTION DEPARTMENT OF NATURAL SCIENCES PHYS 3650, Exam 2 Section 1 Version 1 October 31, 2005 Total Weight: 100 points 1. Check your examination for completeness prior to starting.

More information

CHEM 1411 Chapter 5 Homework Answers

CHEM 1411 Chapter 5 Homework Answers 1 CHEM 1411 Chapter 5 Homework Answers 1. Which statement regarding the gold foil experiment is false? (a) It was performed by Rutherford and his research group early in the 20 th century. (b) Most of

More information

Name Date Class ELECTRONS IN ATOMS. Standard Curriculum Core content Extension topics

Name Date Class ELECTRONS IN ATOMS. Standard Curriculum Core content Extension topics 13 ELECTRONS IN ATOMS Conceptual Curriculum Concrete concepts More abstract concepts or math/problem-solving Standard Curriculum Core content Extension topics Honors Curriculum Core honors content Options

More information

Wave Function, ψ. Chapter 28 Atomic Physics. The Heisenberg Uncertainty Principle. Line Spectrum

Wave Function, ψ. Chapter 28 Atomic Physics. The Heisenberg Uncertainty Principle. Line Spectrum Wave Function, ψ Chapter 28 Atomic Physics The Hydrogen Atom The Bohr Model Electron Waves in the Atom The value of Ψ 2 for a particular object at a certain place and time is proportional to the probability

More information

Atomic Structure Ron Robertson

Atomic Structure Ron Robertson Atomic Structure Ron Robertson r2 n:\files\courses\1110-20\2010 possible slides for web\atomicstructuretrans.doc I. What is Light? Debate in 1600's: Since waves or particles can transfer energy, what is

More information

Chapter 18: The Structure of the Atom

Chapter 18: The Structure of the Atom Chapter 18: The Structure of the Atom 1. For most elements, an atom has A. no neutrons in the nucleus. B. more protons than electrons. C. less neutrons than electrons. D. just as many electrons as protons.

More information

Arrangement of Electrons in Atoms

Arrangement of Electrons in Atoms CHAPTER 4 PRE-TEST 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 following orbital

More information

Photons. ConcepTest 27.1. 1) red light 2) yellow light 3) green light 4) blue light 5) all have the same energy. Which has more energy, a photon of:

Photons. ConcepTest 27.1. 1) red light 2) yellow light 3) green light 4) blue light 5) all have the same energy. Which has more energy, a photon of: ConcepTest 27.1 Photons Which has more energy, a photon of: 1) red light 2) yellow light 3) green light 4) blue light 5) all have the same energy 400 nm 500 nm 600 nm 700 nm ConcepTest 27.1 Photons Which

More information

13- What is the maximum number of electrons that can occupy the subshell 3d? a) 1 b) 3 c) 5 d) 2

13- What is the maximum number of electrons that can occupy the subshell 3d? a) 1 b) 3 c) 5 d) 2 Assignment 06 A 1- What is the energy in joules of an electron undergoing a transition from n = 3 to n = 5 in a Bohr hydrogen atom? a) -3.48 x 10-17 J b) 2.18 x 10-19 J c) 1.55 x 10-19 J d) -2.56 x 10-19

More information

PHOTOELECTRIC EFFECT AND DUAL NATURE OF MATTER AND RADIATIONS

PHOTOELECTRIC EFFECT AND DUAL NATURE OF MATTER AND RADIATIONS PHOTOELECTRIC EFFECT AND DUAL NATURE OF MATTER AND RADIATIONS 1. Photons 2. Photoelectric Effect 3. Experimental Set-up to study Photoelectric Effect 4. Effect of Intensity, Frequency, Potential on P.E.

More information

Chapter 7. Electron Structure of the Atom. Chapter 7 Topics

Chapter 7. Electron Structure of the Atom. Chapter 7 Topics Chapter 7 Electron Structure of the Atom Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Chapter 7 Topics 1. Electromagnetic radiation 2. The Bohr model of

More information

Chem 1A Exam 2 Review Problems

Chem 1A Exam 2 Review Problems Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?

More information

WAVES AND ELECTROMAGNETIC RADIATION

WAVES AND ELECTROMAGNETIC RADIATION WAVES AND ELECTROMAGNETIC RADIATION All waves are characterized by their wavelength, frequency and speed. Wavelength (lambda, ): the distance between any 2 successive crests or troughs. Frequency (nu,):

More information

Unit 2: Chemical Bonding and Organic Chemistry

Unit 2: Chemical Bonding and Organic Chemistry Chemistry AP Unit : Chemical Bonding and Organic Chemistry Unit : Chemical Bonding and Organic Chemistry Chapter 7: Atomic Structure and Periodicity 7.1: Electromagnetic Radiation Electromagnetic (EM)

More information

Sample Exercise 6.1 Concepts of Wavelength and Frequency

Sample Exercise 6.1 Concepts of Wavelength and Frequency Sample Exercise 6.1 Concepts of Wavelength and Frequency Two electromagnetic waves are represented in the margin. (a) Which wave has the higher frequency? (b) If one wave represents visible light and the

More information

Chemistry 102 Summary June 24 th. Properties of Light

Chemistry 102 Summary June 24 th. Properties of Light Chemistry 102 Summary June 24 th Properties of Light - Energy travels through space in the form of electromagnetic radiation (EMR). - Examples of types of EMR: radio waves, x-rays, microwaves, visible

More information

AP* Atomic Structure & Periodicity Free Response Questions KEY page 1

AP* Atomic Structure & Periodicity Free Response Questions KEY page 1 AP* Atomic Structure & Periodicity ree Response Questions KEY page 1 1980 a) points 1s s p 6 3s 3p 6 4s 3d 10 4p 3 b) points for the two electrons in the 4s: 4, 0, 0, +1/ and 4, 0, 0, - 1/ for the three

More information

How To Understand Light And Color

How To Understand Light And Color PRACTICE EXAM IV P202 SPRING 2004 1. In two separate double slit experiments, an interference pattern is observed on a screen. In the first experiment, violet light (λ = 754 nm) is used and a second-order

More information

The Phenomenon of Photoelectric Emission:

The Phenomenon of Photoelectric Emission: The Photoelectric Effect. The Wave particle duality of light Light, like any other E.M.R (electromagnetic radiation) has got a dual nature. That is there are experiments that prove that it is made up of

More information

CHEMSITRY NOTES Chapter 13. Electrons in Atoms

CHEMSITRY NOTES Chapter 13. Electrons in Atoms CHEMSITRY NOTES Chapter 13 Electrons in Atoms Goals : To gain an understanding of : 1. Atoms and their structure. 2. The development of the atomic theory. 3. The quantum mechanical model of the atom. 4.

More information

DO PHYSICS ONLINE FROM QUANTA TO QUARKS QUANTUM (WAVE) MECHANICS

DO PHYSICS ONLINE FROM QUANTA TO QUARKS QUANTUM (WAVE) MECHANICS DO PHYSICS ONLINE FROM QUANTA TO QUARKS QUANTUM (WAVE) MECHANICS Quantum Mechanics or wave mechanics is the best mathematical theory used today to describe and predict the behaviour of particles and waves.

More information

Review of the isotope effect in the hydrogen spectrum

Review of the isotope effect in the hydrogen spectrum Review of the isotope effect in the hydrogen spectrum 1 Balmer and Rydberg Formulas By the middle of the 19th century it was well established that atoms emitted light at discrete wavelengths. This is in

More information

The Advanced Placement Examination in Chemistry. Part I Multiple Choice Questions Part II Free Response Questions Selected Questions from1970 to 2010

The Advanced Placement Examination in Chemistry. Part I Multiple Choice Questions Part II Free Response Questions Selected Questions from1970 to 2010 The Advanced Placement Examination in Chemistry Part I Multiple Choice Questions Part II Free Response Questions Selected Questions from1970 to 2010 Atomic Theory and Periodicity Part I 1984 1. Which of

More information

Chemistry 2 Chapter 13: Electrons in Atoms Please do not write on the test Use an answer sheet! 1 point/problem 45 points total

Chemistry 2 Chapter 13: Electrons in Atoms Please do not write on the test Use an answer sheet! 1 point/problem 45 points total Chemistry 2 Chapter 13: Electrons in Atoms Please do not write on the test Use an answer sheet! 1 point/problem 45 points total 1. Calculate the energy in joules of a photon of red light that has a frequency

More information

CHAPTER 8 PRACTICE TEST QUESTIONS (END OF CHAPTER 7 TOO)

CHAPTER 8 PRACTICE TEST QUESTIONS (END OF CHAPTER 7 TOO) CHAPTER 8 PRACTICE TEST QUESTIONS (END OF CHAPTER 7 TOO) Information that most likely will be on the front cover of your exam: h i Z 2 ΔE = @ 2.18 x 10 @ 18 f Z 2 f J j @ k n f 2 n i 2 1. Which of the

More information

Name period AP chemistry Unit 2 worksheet Practice problems

Name period AP chemistry Unit 2 worksheet Practice problems Name period AP chemistry Unit 2 worksheet Practice problems 1. What are the SI units for a. Wavelength of light b. frequency of light c. speed of light Meter hertz (s -1 ) m s -1 (m/s) 2. T/F (correct

More information

3. What would you predict for the intensity and binding energy for the 3p orbital for that of sulfur?

3. What would you predict for the intensity and binding energy for the 3p orbital for that of sulfur? PSI AP Chemistry Periodic Trends MC Review Name Periodic Law and the Quantum Model Use the PES spectrum of Phosphorus below to answer questions 1-3. 1. Which peak corresponds to the 1s orbital? (A) 1.06

More information

Chapter 9: ELECTRONS IN ATOMS AND THE PERIODIC TABLE

Chapter 9: ELECTRONS IN ATOMS AND THE PERIODIC TABLE Chapter 9: ELECTRONS IN ATOMS AND THE PERIODIC TABLE Problems: 1-3, 13-15, 19, 23-25, 31-32, 43, 45-46, 49c, 50a, 50b, 57c, 58 (b,c,d), 61-62, 69, 71-74, 77-88, 91-94 9.5 LIGHT: Electromagnetic Radiation

More information

Electron Configuration Worksheet (and Lots More!!)

Electron Configuration Worksheet (and Lots More!!) Electron Configuration Worksheet (and Lots More!!) Brief Instructions An electron configuration is a method of indicating the arrangement of electrons about a nucleus. A typical electron configuration

More information

SAMPLE EXAM 2 FALL 2012 SOLUTIONS Chemistry 11, Fall 2007 Exam II November 15, 2007 7:30 PM 9:30 PM

SAMPLE EXAM 2 FALL 2012 SOLUTIONS Chemistry 11, Fall 2007 Exam II November 15, 2007 7:30 PM 9:30 PM Name: SOLUTIONS III, IV, and V Section (circle): 1 2 3 4 5 SAMPLE EXAM 2 FALL 2012 SOLUTIONS Chemistry 11, Fall 2007 Exam II November 15, 2007 7:30 PM 9:30 PM As always, full credit will not be given unless

More information

Electromagnetic Radiation

Electromagnetic Radiation Chapter 7 A Quantum Model of Atoms Chapter Objectives: Understand the relationships between wavelength, frequency, and energy of light. Understand the origin of atomic line spectra. Learn how the quantum

More information

Light as a Wave. The Nature of Light. EM Radiation Spectrum. EM Radiation Spectrum. Electromagnetic Radiation

Light as a Wave. The Nature of Light. EM Radiation Spectrum. EM Radiation Spectrum. Electromagnetic Radiation The Nature of Light Light and other forms of radiation carry information to us from distance astronomical objects Visible light is a subset of a huge spectrum of electromagnetic radiation Maxwell pioneered

More information

CHAPTER 11: MODERN ATOMIC THEORY

CHAPTER 11: MODERN ATOMIC THEORY CHAPTER 11: MODERN ATOMIC THEORY Active Learning Questions: 1-2, 8-10, 14-18; End-of-Chapter Problems: 3-9, 11-13, 16, 18, 20-36, 45-54, 56-64, 66b, 67, 69-91, 98, 101-102, 108, 110, 113, 116, 11.2 ELECTROMAGNETIC

More information

Level 3 Achievement Scale

Level 3 Achievement Scale Unit 1: Atoms Level 3 Achievement Scale Can state the key results of the experiments associated with Dalton, Rutherford, Thomson, Chadwick, and Bohr and what this lead each to conclude. Can explain that

More information

MODERN ATOMIC THEORY AND THE PERIODIC TABLE

MODERN ATOMIC THEORY AND THE PERIODIC TABLE CHAPTER 10 MODERN ATOMIC THEORY AND THE PERIODIC TABLE SOLUTIONS TO REVIEW QUESTIONS 1. Wavelength is defined as the distance between consecutive peaks in a wave. It is generally symbolized by the Greek

More information

3) Of the following, radiation has the shortest wavelength. A) X-ray B) radio C) microwave D) ultraviolet E) infrared Answer: A

3) Of the following, radiation has the shortest wavelength. A) X-ray B) radio C) microwave D) ultraviolet E) infrared Answer: A 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 Answer: E 2) The wavelength of light emitted from a traffic light having a frequency of 5.75 1014 Hz is.

More information

Electron Orbits. Binding Energy. centrifugal force: electrostatic force: stability criterion: kinetic energy of the electron on its orbit:

Electron Orbits. Binding Energy. centrifugal force: electrostatic force: stability criterion: kinetic energy of the electron on its orbit: Electron Orbits In an atom model in which negatively charged electrons move around a small positively charged nucleus stable orbits are possible. Consider the simple example of an atom with a nucleus of

More information

Quantum Mechanics and Atomic Structure 1

Quantum Mechanics and Atomic Structure 1 Quantum Mechanics and Atomic Structure 1 INTRODUCTION The word atom is derived from the Greek word, atomos, which means uncut or indivisible. It was Dalton (1808) who established that elementary constituents

More information

Nanoelectronics. Chapter 2 Classical Particles, Classical Waves, and Quantum Particles. Q.Li@Physics.WHU@2015.3

Nanoelectronics. Chapter 2 Classical Particles, Classical Waves, and Quantum Particles. Q.Li@Physics.WHU@2015.3 Nanoelectronics Chapter 2 Classical Particles, Classical Waves, and Quantum Particles Q.Li@Physics.WHU@2015.3 1 Electron Double-Slit Experiment Q.Li@Physics.WHU@2015.3 2 2.1 Comparison of Classical and

More information

Electrons In Atoms Mr. O Brien (SFHS) Chapter 5 Standard 1D

Electrons In Atoms Mr. O Brien (SFHS) Chapter 5 Standard 1D Electrons In Atoms Mr. O Brien (SFHS) Chapter 5 Standard 1D Electrons in Atoms (std.1d) What are Bohr Models? planetary model in which the negatively-charged electrons orbit a small, positively-charged

More information

5. The Nature of Light. Does Light Travel Infinitely Fast? EMR Travels At Finite Speed. EMR: Electric & Magnetic Waves

5. The Nature of Light. Does Light Travel Infinitely Fast? EMR Travels At Finite Speed. EMR: Electric & Magnetic Waves 5. The Nature of Light Light travels in vacuum at 3.0. 10 8 m/s Light is one form of electromagnetic radiation Continuous radiation: Based on temperature Wien s Law & the Stefan-Boltzmann Law Light has

More information

Question: Do all electrons in the same level have the same energy?

Question: Do all electrons in the same level have the same energy? Question: Do all electrons in the same level have the same energy? From the Shells Activity, one important conclusion we reached based on the first ionization energy experimental data is that electrons

More information

Chapter 2. Quantum Theory

Chapter 2. Quantum Theory Chapter 2 Quantum Theory 2.0 Introduction 2.6 Orbital Shapes, Signs, and Sizes 2.1 The Nature of Light 2.7 Electron Configurations 2.2 Quantization 2.8 Quantum Theory and the Periodic Table 2.3 Bohr Model

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Practice Questions - Chapter 7 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which one of the following represents an impossible set of

More information

Chapters 21-29. Magnetic Force. for a moving charge. F=BQvsinΘ. F=BIlsinΘ. for a current

Chapters 21-29. Magnetic Force. for a moving charge. F=BQvsinΘ. F=BIlsinΘ. for a current Chapters 21-29 Chapter 21:45,63 Chapter 22:25,49 Chapter 23:35,38,53,55,58,59 Chapter 24:17,18,20,42,43,44,50,52,53.59,63 Chapter 26:27,33,34,39,54 Chapter 27:17,18,34,43,50,51,53,56 Chapter 28: 10,11,28,47,52

More information

IONISATION ENERGY CONTENTS

IONISATION ENERGY CONTENTS IONISATION ENERGY IONISATION ENERGY CONTENTS What is Ionisation Energy? Definition of t Ionisation Energy What affects Ionisation Energy? General variation across periods Variation down groups Variation

More information

Bohr's Theory of the Hydrogen Atom

Bohr's Theory of the Hydrogen Atom OpenStax-CNX module: m42596 1 Bohr's Theory of the Hydrogen Atom OpenStax College This work is produced by OpenStax-CNX and licensed under the Creative Commons Attribution License 4.0 Abstract Describe

More information

Arrangement of Electrons in Atoms

Arrangement of Electrons in Atoms CHAPTER 4 Arrangement of Electrons in Atoms The emission of light is fundamentally related to the behavior of electrons. Neon Walkway The Development of a New Atomic Model T he Rutherford model of the

More information

2. John Dalton did his research work in which of the following countries? a. France b. Greece c. Russia d. England

2. John Dalton did his research work in which of the following countries? a. France b. Greece c. Russia d. England CHAPTER 3 1. Which combination of individual and contribution is not correct? a. Antoine Lavoisier - clarified confusion over cause of burning b. John Dalton - proposed atomic theory c. Marie Curie - discovered

More information

Homework #10 (749508)

Homework #10 (749508) Homework #10 (749508) Current Score: 0 out of 100 Description Homework on quantum physics and radioactivity Instructions Answer all the questions as best you can. 1. Hewitt10 32.E.001. [481697] 0/5 points

More information

Elements in the periodic table are indicated by SYMBOLS. To the left of the symbol we find the atomic mass (A) at the upper corner, and the atomic num

Elements in the periodic table are indicated by SYMBOLS. To the left of the symbol we find the atomic mass (A) at the upper corner, and the atomic num . ATOMIC STRUCTURE FUNDAMENTALS LEARNING OBJECTIVES To review the basics concepts of atomic structure that have direct relevance to the fundamental concepts of organic chemistry. This material is essential

More information

Flame Tests & Electron Configuration

Flame Tests & Electron Configuration Flame Tests & Electron Configuration INTRODUCTION Many elements produce colors in the flame when heated. The origin of this phenomenon lies in the arrangement, or configuration of the electrons in the

More information

The quantum understanding of pre-university physics students

The quantum understanding of pre-university physics students The quantum understanding of pre-university physics students Gren Ireson Department of Education, Loughborough University, Loughborough, Leicestershire LE11 3TU, UK Students in England and Wales wishing

More information

Chapter 2: Atomic Structure and Chemical Bonding

Chapter 2: Atomic Structure and Chemical Bonding Chapter 2: Atomic Structure and Chemical Bonding Materials Molecules Atoms Atoms = protons (p) + neutrons (n) + electrons (e) Protons and neutrons are made of quarks Quantitative measurements need units:

More information

Energy. Mechanical Energy

Energy. Mechanical Energy Principles of Imaging Science I (RAD119) Electromagnetic Radiation Energy Definition of energy Ability to do work Physicist s definition of work Work = force x distance Force acting upon object over distance

More information

9/13/2013. However, Dalton thought that an atom was just a tiny sphere with no internal parts. This is sometimes referred to as the cannonball model.

9/13/2013. However, Dalton thought that an atom was just a tiny sphere with no internal parts. This is sometimes referred to as the cannonball model. John Dalton was an English scientist who lived in the early 1800s. Dalton s atomic theory served as a model for how matter worked. The principles of Dalton s atomic theory are: 1. Elements are made of

More information

Electrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set

Electrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set Electrons in Atoms & Periodic Table Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Electrons in Atoms & Periodic Table 2 Study Guide: Things You

More information

ATOMIC SPECTRA. Apparatus: Optical spectrometer, spectral tubes, power supply, incandescent lamp, bottles of dyed water, elevating jack or block.

ATOMIC SPECTRA. Apparatus: Optical spectrometer, spectral tubes, power supply, incandescent lamp, bottles of dyed water, elevating jack or block. 1 ATOMIC SPECTRA Objective: To measure the wavelengths of visible light emitted by atomic hydrogen and verify the measured wavelengths against those predicted by quantum theory. To identify an unknown

More information

Atomic Calculations. 2.1 Composition of the Atom. number of protons + number of neutrons = mass number

Atomic Calculations. 2.1 Composition of the Atom. number of protons + number of neutrons = mass number 2.1 Composition of the Atom Atomic Calculations number of protons + number of neutrons = mass number number of neutrons = mass number - number of protons number of protons = number of electrons IF positive

More information

Multi-electron atoms

Multi-electron atoms Multi-electron atoms Today: Using hydrogen as a model. The Periodic Table HWK 13 available online. Please fill out the online participation survey. Worth 10points on HWK 13. Final Exam is Monday, Dec.

More information

Main properties of atoms and nucleus

Main properties of atoms and nucleus Main properties of atoms and nucleus. Atom Structure.... Structure of Nuclei... 3. Definition of Isotopes... 4. Energy Characteristics of Nuclei... 5. Laws of Radioactive Nuclei Transformation... 3. Atom

More information

Atoms Absorb & Emit Light

Atoms Absorb & Emit Light Atoms Absorb & Emit Light Spectra The wavelength of the light that an element emits or absorbs is its fingerprint. Atoms emit and absorb light First Test is Thurs, Feb 1 st About 30 multiple choice questions

More information

Does Quantum Mechanics Make Sense? Size

Does Quantum Mechanics Make Sense? Size Does Quantum Mechanics Make Sense? Some relatively simple concepts show why the answer is yes. Size Classical Mechanics Quantum Mechanics Relative Absolute What does relative vs. absolute size mean? Why

More information

Unit 3 Study Guide: Electron Configuration & The Periodic Table

Unit 3 Study Guide: Electron Configuration & The Periodic Table Name: Teacher s Name: Class: Block: Date: Unit 3 Study Guide: Electron Configuration & The Periodic Table 1. For each of the following elements, state whether the element is radioactive, synthetic or both.

More information

Quantum Phenomena and the Theory of Quantum Mechanics

Quantum Phenomena and the Theory of Quantum Mechanics Quantum Phenomena and the Theory of The Mechanics of the Very Small Waseda University, SILS, Introduction to History and Philosophy of Science . Two Dark Clouds In 1900 at a Friday Evening lecture at the

More information

Ch. 9 - Electron Organization. The Bohr Model [9.4] Orbitals [9.5, 9.6] Counting Electrons, configurations [9.7]

Ch. 9 - Electron Organization. The Bohr Model [9.4] Orbitals [9.5, 9.6] Counting Electrons, configurations [9.7] Ch. 9 - Electron Organization The Bohr Model [9.4] Orbitals [9.5, 9.6] Counting Electrons, configurations [9.7] Predicting ion charges from electron configurations. CHEM 100 F07 1 Organization of Electrons

More information

Physical Science Study Guide Unit 7 Wave properties and behaviors, electromagnetic spectrum, Doppler Effect

Physical Science Study Guide Unit 7 Wave properties and behaviors, electromagnetic spectrum, Doppler Effect Objectives: PS-7.1 Physical Science Study Guide Unit 7 Wave properties and behaviors, electromagnetic spectrum, Doppler Effect Illustrate ways that the energy of waves is transferred by interaction with

More information

6.5 Periodic Variations in Element Properties

6.5 Periodic Variations in Element Properties 324 Chapter 6 Electronic Structure and Periodic Properties of Elements 6.5 Periodic Variations in Element Properties By the end of this section, you will be able to: Describe and explain the observed trends

More information

Infrared Spectroscopy: Theory

Infrared Spectroscopy: Theory u Chapter 15 Infrared Spectroscopy: Theory An important tool of the organic chemist is Infrared Spectroscopy, or IR. IR spectra are acquired on a special instrument, called an IR spectrometer. IR is used

More information

Electron Arrangements

Electron Arrangements Section 3.4 Electron Arrangements Objectives Express the arrangement of electrons in atoms using electron configurations and Lewis valence electron dot structures New Vocabulary Heisenberg uncertainty

More information

Physics 30 Worksheet # 14: Michelson Experiment

Physics 30 Worksheet # 14: Michelson Experiment Physics 30 Worksheet # 14: Michelson Experiment 1. The speed of light found by a Michelson experiment was found to be 2.90 x 10 8 m/s. If the two hills were 20.0 km apart, what was the frequency of the

More information

Indiana's Academic Standards 2010 ICP Indiana's Academic Standards 2016 ICP. map) that describe the relationship acceleration, velocity and distance.

Indiana's Academic Standards 2010 ICP Indiana's Academic Standards 2016 ICP. map) that describe the relationship acceleration, velocity and distance. .1.1 Measure the motion of objects to understand.1.1 Develop graphical, the relationships among distance, velocity and mathematical, and pictorial acceleration. Develop deeper understanding through representations

More information

A-level PHYSICS (7408/1)

A-level PHYSICS (7408/1) SPECIMEN MATERIAL A-level PHYSICS (7408/1) Paper 1 Specimen 2014 Morning Time allowed: 2 hours Materials For this paper you must have: a pencil a ruler a calculator a data and formulae booklet. Instructions

More information

Objectives. PAM1014 Introduction to Radiation Physics. Constituents of Atoms. Atoms. Atoms. Atoms. Basic Atomic Theory

Objectives. PAM1014 Introduction to Radiation Physics. Constituents of Atoms. Atoms. Atoms. Atoms. Basic Atomic Theory PAM1014 Introduction to Radiation Physics Basic Atomic Theory Objectives Introduce and Molecules The periodic Table Electronic Energy Levels Atomic excitation & de-excitation Ionisation Molecules Constituents

More information

Chapter 28 Atomic Physics

Chapter 28 Atomic Physics 614 Chapter 28 Atomic Physics GOALS After you have mastered the contents of this chapter, you will be able to achieve the following goals: Definitions Define each of the following terms and use it in an

More information

CHAPTER 9 ATOMIC STRUCTURE AND THE PERIODIC LAW

CHAPTER 9 ATOMIC STRUCTURE AND THE PERIODIC LAW CHAPTER 9 ATOMIC STRUCTURE AND THE PERIODIC LAW Quantum mechanics can account for the periodic structure of the elements, by any measure a major conceptual accomplishment for any theory. Although accurate

More information

Experiment #12: The Bohr Atom. Equipment: Spectroscope Hydrogen and Helium Gas Discharge Tubes, Holder, and Variac Flashlight

Experiment #12: The Bohr Atom. Equipment: Spectroscope Hydrogen and Helium Gas Discharge Tubes, Holder, and Variac Flashlight Experiment #12: The Bohr Atom Purpose: To observe the visible spectrum of hydrogen and helium and verify the Bohr model of the hydrogen atom. Equipment: Spectroscope Hydrogen and Helium Gas Discharge Tubes,

More information

Advanced Quantum Physics

Advanced Quantum Physics Advanced Quantum Physics Aim of the course Building upon the foundations of wave mechanics, this course will introduce and develop the broad field of quantum physics including: Quantum mechanics of point

More information

18.2 Comparing Atoms. Atomic number. Chapter 18

18.2 Comparing Atoms. Atomic number. Chapter 18 As you know, some substances are made up of only one kind of atom and these substances are called elements. You already know something about a number of elements you ve heard of hydrogen, helium, silver,

More information

Boardworks AS Physics

Boardworks AS Physics Boardworks AS Physics Vectors 24 slides 11 Flash activities Prefixes, scalars and vectors Guide to the SI unit prefixes of orders of magnitude Matching powers of ten to their SI unit prefixes Guide to

More information

Blackbody radiation derivation of Planck s radiation low

Blackbody radiation derivation of Planck s radiation low Blackbody radiation derivation of Planck s radiation low 1 Classical theories of Lorentz and Debye: Lorentz (oscillator model): Electrons and ions of matter were treated as a simple harmonic oscillators

More information

Nuclear Magnetic Resonance

Nuclear Magnetic Resonance Nuclear Magnetic Resonance NMR is probably the most useful and powerful technique for identifying and characterizing organic compounds. Felix Bloch and Edward Mills Purcell were awarded the 1952 Nobel

More information

where h = 6.62 10-34 J s

where h = 6.62 10-34 J s Electromagnetic Spectrum: Refer to Figure 12.1 Molecular Spectroscopy: Absorption of electromagnetic radiation: The absorptions and emissions of electromagnetic radiation are related molecular-level phenomena

More information

The Periodic Table; Chapter 5: Section 1 - History of the Periodic Table Objectives: Explain the roles of Mendeleev and Moseley in the development of

The Periodic Table; Chapter 5: Section 1 - History of the Periodic Table Objectives: Explain the roles of Mendeleev and Moseley in the development of The Periodic Table; Chapter 5: Section 1 - History of the Periodic Table Objectives: Explain the roles of Mendeleev and Moseley in the development of the periodic table. Describe the modern periodic table.

More information

- thus, the total number of atoms per second that absorb a photon is

- thus, the total number of atoms per second that absorb a photon is Stimulated Emission of Radiation - stimulated emission is referring to the emission of radiation (a photon) from one quantum system at its transition frequency induced by the presence of other photons

More information

Practice final for Basic Physics spring 2005 answers on the last page Name: Date:

Practice final for Basic Physics spring 2005 answers on the last page Name: Date: Practice final for Basic Physics spring 2005 answers on the last page Name: Date: 1. A 12 ohm resistor and a 24 ohm resistor are connected in series in a circuit with a 6.0 volt battery. Assuming negligible

More information

Solar Energy. Outline. Solar radiation. What is light?-- Electromagnetic Radiation. Light - Electromagnetic wave spectrum. Electromagnetic Radiation

Solar Energy. Outline. Solar radiation. What is light?-- Electromagnetic Radiation. Light - Electromagnetic wave spectrum. Electromagnetic Radiation Outline MAE 493R/593V- Renewable Energy Devices Solar Energy Electromagnetic wave Solar spectrum Solar global radiation Solar thermal energy Solar thermal collectors Solar thermal power plants Photovoltaics

More information

Kinetic Molecular Theory. Chapter 5. KE AVE and Average Velocity. Graham s Law of Effusion. Chapter 7. Real Gases

Kinetic Molecular Theory. Chapter 5. KE AVE and Average Velocity. Graham s Law of Effusion. Chapter 7. Real Gases hapter 5 1. Kinetic Molecular Theory. 2. Average kinetic energy and velocity. 3. Graham s Law of Effusion. 4. Real gases and the van der Waals equation. Kinetic Molecular Theory The curves below represent

More information

Physics 111 Homework Solutions Week #9 - Tuesday

Physics 111 Homework Solutions Week #9 - Tuesday Physics 111 Homework Solutions Week #9 - Tuesday Friday, February 25, 2011 Chapter 22 Questions - None Multiple-Choice 223 A 224 C 225 B 226 B 227 B 229 D Problems 227 In this double slit experiment we

More information

Experiment #5: Qualitative Absorption Spectroscopy

Experiment #5: Qualitative Absorption Spectroscopy Experiment #5: Qualitative Absorption Spectroscopy One of the most important areas in the field of analytical chemistry is that of spectroscopy. In general terms, spectroscopy deals with the interactions

More information

It takes four quantum numbers to describe an electron. Additionally, every electron has a unique set of quantum numbers.

It takes four quantum numbers to describe an electron. Additionally, every electron has a unique set of quantum numbers. So, quantum mechanics does not define the path that the electron follows; rather, quantum mechanics works by determining the energy of the electron. Once the energy of an electron is known, the probability

More information

Calculating particle properties of a wave

Calculating particle properties of a wave Calculating particle properties of a wave A light wave consists of particles (photons): The energy E of the particle is calculated from the frequency f of the wave via Planck: E = h f (1) A particle can

More information

Section 11.3 Atomic Orbitals Objectives

Section 11.3 Atomic Orbitals Objectives Objectives 1. To learn about the shapes of the s, p and d orbitals 2. To review the energy levels and orbitals of the wave mechanical model of the atom 3. To learn about electron spin A. Electron Location

More information

Lecture 3 September 14, 2009 Atomic Models: Rutherford & Bohr

Lecture 3 September 14, 2009 Atomic Models: Rutherford & Bohr Welcome to 3.091 Lecture 3 September 14, 2009 Atomic Models: Rutherford & Bohr 1 Periodic Table Quiz 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37

More information

Instructors Guide: Atoms and Their Isotopes

Instructors Guide: Atoms and Their Isotopes Instructors Guide: Atoms and Their Isotopes Standards Connections Connections to NSTA Standards for Science Teacher Preparation C.3.a.1 Fundamental structures of atoms and molecules. C.3.b.27 Applications

More information

Bohr model of hydrogen

Bohr model of hydrogen Chapter 3 Bohr model of hydrogen Figure 3.1: Democritus The atomic theory of matter has a long history, in some ways all the way back to the ancient Greeks (Democritus - ca. 400 BCE - suggested that all

More information

Review for Test 3. Polarized light. Action of a Polarizer. Polarized light. Light Intensity after a Polarizer. Review for Test 3.

Review for Test 3. Polarized light. Action of a Polarizer. Polarized light. Light Intensity after a Polarizer. Review for Test 3. Review for Test 3 Polarized light No equation provided! Polarized light In linearly polarized light, the electric field vectors all lie in one single direction. Action of a Polarizer Transmission axis

More information

PHYSICS PAPER 1 (THEORY)

PHYSICS PAPER 1 (THEORY) PHYSICS PAPER 1 (THEORY) (Three hours) (Candidates are allowed additional 15 minutes for only reading the paper. They must NOT start writing during this time.) ---------------------------------------------------------------------------------------------------------------------

More information

Semester Exam Practice Questions

Semester Exam Practice Questions Name: Class: _ Date: _ Semester Exam Practice Questions Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following is not a material? a. air

More information