The Bohr model for the electrons
|
|
- Darren Logan
- 7 years ago
- Views:
Transcription
1 The Bohr model for the electrons Electronic structure how the electrons are arranged inside the atom Applying the quantum principle of energy Two parameters: Energy Position
2 Learning objectives Describe the basic principles of the Bohr model Distinguish between the classical view and the quantum view of matter Define atomic orbitals Distinguish between the Bohr orbit and atomic orbital Apply quantum numbers and atomic orbitals to building atoms and the periodic table Describe periodic trends in terms of electronic structure
3 Bohr s theory of the atom: applying photons to electronic structure Electrons occupy specific levels (orbits) and no others Orbits have energy and size Larger orbits are at higher energy Electron excited to higher level by absorbing photon Electron relaxes to lower level by emitting photon Photon energy exactly equals gap between levels
4 Size of energy gap determines Small energy gap, low frequency, long wavelength (red shift) High energy gap, high frequency, short wavelength (blue shift) photon energy
5 The full spectrum of lines for H Each set of lines in the H spectrum comes from transitions from all the higher levels to a particular level. The lines in the visible are transitions to the second level
6 The Bohr orbits Bohr orbits have quantum numbers n n = 1 (capacity 2) n = 2 (capacity 8) n = 3 (capacity 8)
7 Bohr orbits and the periodic table Elements in the same group have the same number of electrons in outer Bohr orbit
8 Successes and shortcomings of Bohr Couldn t explain why orbits were allowed Only successful agreement with experiment was with the H atom Introduced connection between spectra and electron structure Concept of allowed orbits is developed further with new knowledge Nonetheless, an important contribution, worthy of the Nobel prize
9 Electrons are waves too! Life at the electron level is very different Key to unlocking the low door to the secret garden of the atom lay in accepting the wave properties of electrons De Broglie wave-particle duality All particles have a wavelength wavelike nature. Significant only for very small particles like electrons or photons As mass increases, wavelength decreases Electrons have wavelengths about the size of an atom Electrons are used for studying matter electron microscopy
10 Electron microscopes can peer within waves interacting with matter
11 Heisenberg Uncertainty Principle: the illusive electron We can predict the motion of a ball; But not an electron: problems locating small objects
12 The Quantum Mechanics: waves of uncertainty System developed that incorporated these concepts and produced an orbital picture of the electrons No longer think of electrons as particles with precise location, but as waves which have probability of being in some region of the atom the orbital Impossible with the classical mechanics of Newton
13 Orbits become orbitals The Orbitron: a gallery of atomic orbitals and molecular orbitals
14 Orbitals are described by quantum numbers Each orbital has unique set 1s, 2p, 3d etc. Number describes energy Letter describes shape S zero dimensions P one dimension D two dimensions F three dimensions
15
16 Getting from the orbitals to the elements All elements have the same set Atomic number dictates how many are filled how many electrons are added Filling orbitals follows a fixed pattern: lowest energy ones first
17 Orbital energy levels in H and other elements
18 How many per orbital? Electrons share orbitals (only two allowed) A consequence of spin
19 How many electrons can be added to the orbitals 1s, 2s, 3s etc. 2 electrons 2p, 3p, 4p etc. 6 electrons 3d, 4d etc. 10 electrons 4f, 5f etc. 14 electrons
20 Add electrons to the orbitals lowest first 4s 4p 3d 3s 3p 2s 1s 2p H(z = 1)
21 Fill lowest orbital 4s 4p 3d 3s 3p 2s 1s 2p He(z = 2)
22 Begin next orbital 4s 4p 3d 3s 3p 2s 1s 2p Li(z = 3)
23 Fill 2s 4s 4p 3d 3s 3p 2s 1s 2p Be(z = 4)
24 Begin filling 2p 4s 4p 3d 3s 3p 2s 1s 2p B(z = 5)
25 Electrons don t like to pair 4s 4p 3d 3s 3p 2s 1s 2p C(z = 6)
26 4s 4p 3d 3s 3p 2s 1s 2p O(z = 8)
27 4s 4p 3d 3s 3p 2s 1s 2p F(z = 9)
28 Filled 2p neon unreactive 4s 4p 3d 3s 3p 2s 1s 2p Ne(z = 10)
29 Shape of the periodic table explained by orbital picture 2 groups 10 groups 6 groups 14 groups
30 Connecting the table with orbitals: elements per row matches capacity of orbitals
31 Simplifying with shells: echoes of Bohr orbits The orbitals with the same Principal Quantum number (1,2,3 etc) are grouped into shells Filled shells have special significance Filled shell 1 Filled shell 1 Unfilled shell 2 Filled shell 2
32 The periodic law and atomic size
33 Ionization energy and the periodic law Ionization energy is energy required to remove electron from the neutral atom
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 informationAtomic 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 informationLevel 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 informationPhotons. 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 information13- 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 informationName 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 informationChapter 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 informationTIME 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 informationWAVES 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 informationCHEM 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 informationChemistry 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 informationWave 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 informationNanoelectronics. 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 information5. 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 informationThe 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 informationElectrons 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 informationDO 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 informationSample 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 informationAtoms 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 informationArrangement 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 informationThe 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 informationMODERN 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 informationElectron 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 informationLight 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 informationHow 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 informationFrom lowest energy to highest energy, which of the following correctly orders the different categories of electromagnetic radiation?
From lowest energy to highest energy, which of the following correctly orders the different categories of electromagnetic radiation? From lowest energy to highest energy, which of the following correctly
More informationFlame 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 informationErnest Rutherford Atomic Model 1911. Plum Pudding Model J.J. Thomson 1897
1 The arrangement of electrons in an atom determine most of the chemical properties of that atom. Electrons are what actually do the reacting. Plum Pudding Model J.J. Thomson 1897 Ernest Rutherford Atomic
More informationCHEMSITRY 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 informationAP* 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 informationAtomic 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 informationElectrons 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 informationElements 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 informationMULTIPLE 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 informationAstronomy 110 Homework #04 Assigned: 02/06/2007 Due: 02/13/2007. Name:
Astronomy 110 Homework #04 Assigned: 02/06/2007 Due: 02/13/2007 Name: Directions: Listed below are twenty (20) multiple-choice questions based on the material covered by the lectures this past week. Choose
More informationChapter 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 informationElectron 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 informationElectron 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 informationUnit 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 informationName 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 informationHomework #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 informationThe 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 informationSection 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 informationQuestion: 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 informationThe Hydrogen Atom Is a Magnet. http://www.seed.slb.com/en/scictr/watch/gashydrates/detecting.htm
The Hydrogen Atom Is a Magnet Nuclear Magnetic Resonance Spectroscopy (NMR) Proton NMR A hydrogen nucleus can be viewed as a proton, which can be viewed as a spinning charge. As with any spinning charge,
More informationATOMS AND THE PERIODIC TABLE CHAPTER 3 PHYSICAL SCIENCE
ATOMS AND THE PERIODIC TABLE CHAPTER 3 PHYSICAL SCIENCE Chapter 3 Vocabulary Words (27 words) Nucleus Atomic number Proton Mass number Neutron Isotopes Electron Atomic mass unit (amu) Energy level Average
More informationMulti-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 informationCh. 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 informationObjectives. 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 information9/13/2013. 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 informationChem 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 informationAPS Science Curriculum Unit Planner
APS Science Curriculum Unit Planner Grade Level/Subject Chemistry Stage 1: Desired Results Enduring Understanding Topic 1: Elements and the Periodic Table: The placement of elements on the periodic table
More informationATOMIC 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 information6.7: Explaining the Periodic Table pg. 234
Unit C: Atoms, elements, and Compounds 6.7: Explaining the Periodic Table pg. 234 Key Concepts: 3. Elements are organized according to their atomic number and electron arrangement on the periodic table.
More information- particle with kinetic energy E strikes a barrier with height U 0 > E and width L. - classically the particle cannot overcome the barrier
Tunnel Effect: - particle with kinetic energy E strikes a barrier with height U 0 > E and width L - classically the particle cannot overcome the barrier - quantum mechanically the particle can penetrated
More informationMolecular Spectroscopy:
: How are some molecular parameters determined? Bond lengths Bond energies What are the practical applications of spectroscopic knowledge? Can molecules (or components thereof) be identified based on differences
More informationLecture 3: Optical Properties of Bulk and Nano. 5 nm
Lecture 3: Optical Properties of Bulk and Nano 5 nm The Previous Lecture Origin frequency dependence of χ in real materials Lorentz model (harmonic oscillator model) 0 e - n( ) n' n '' n ' = 1 + Nucleus
More informationInfrared 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 informationUnit 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 informationExperiment #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 informationHeisenberg Uncertainty
Heisenberg Uncertainty Outline - Heisenberg Microscope - Measurement Uncertainty - Example: Hydrogen Atom - Example: Single Slit Diffraction - Example: Quantum Dots 1 TRUE / FALSE A photon (quantum of
More informationEnergy. 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 informationKinetic 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 information2. 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 informationName Class Date. spectrum. White is not a color, but is a combination of all colors. Black is not a color; it is the absence of all light.
Exercises 28.1 The Spectrum (pages 555 556) 1. Isaac Newton was the first person to do a systematic study of color. 2. Circle the letter of each statement that is true about Newton s study of color. a.
More informationSyllabus for Chem 359: Atomic and Molecular Spectroscopy
Syllabus for Chem 359: Atomic and Molecular Spectroscopy Instructors: Dr. Reinhard Schweitzer- Stenner and Ms. Siobhan E. Toal Of#ice: Disque 605/Disque 306 Tel: (215) 895-2268 Email: rschweitzer- stenner@drexel.edu
More informationChapter 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 informationPart I: Principal Energy Levels and Sublevels
Part I: Principal Energy Levels and Sublevels As you already know, all atoms are made of subatomic particles, including protons, neutrons, and electrons. Positive protons and neutral neutrons are found
More information18.2 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 informationQuantum 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 informationSAMPLE 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 informationElectromagnetic 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 informationChapters 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 informationWhat does Quantum Mechanics tell us about the universe?
Fedora GNU/Linux; L A TEX 2ǫ; xfig What does Quantum Mechanics tell us about the universe? Mark Alford Washington University Saint Louis, USA More properly: What do experiments tell us about the universe?
More informationThe Electromagnetic Spectrum
INTRODUCTION The Electromagnetic Spectrum I. What is electromagnetic radiation and the electromagnetic spectrum? What do light, X-rays, heat radiation, microwaves, radio waves, and gamma radiation have
More informationDoes 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 informationTHE CURRENT-VOLTAGE CHARACTERISTICS OF AN LED AND A MEASUREMENT OF PLANCK S CONSTANT Physics 258/259
DSH 2004 THE CURRENT-VOLTAGE CHARACTERISTICS OF AN LED AND A MEASUREMENT OF PLANCK S CONSTANT Physics 258/259 I. INTRODUCTION Max Planck (1858-1947) was an early pioneer in the field of quantum physics.
More informationSection 6 Raman Scattering (lecture 10)
Section 6 Scattering (lecture 10) Previously: Quantum theory of atoms / molecules Quantum Mechanics Valence Atomic and Molecular Spectroscopy Scattering The scattering process Elastic (Rayleigh) and inelastic
More informationNoble Gases. Outline Nobel Gas Elements Radon and Health Chemistry Homework
Radon and Other Noble Gases The elements in the last column of the periodic table are all very stable, mono-atomic gases. Until 1962, they were called inert gases because they did not react with other
More informationSSO Transmission Grating Spectrograph (TGS) User s Guide
SSO Transmission Grating Spectrograph (TGS) User s Guide The Rigel TGS User s Guide available online explains how a transmission grating spectrograph (TGS) works and how efficient they are. Please refer
More informationPhysics 441/2: Transmission Electron Microscope
Physics 441/2: Transmission Electron Microscope Introduction In this experiment we will explore the use of transmission electron microscopy (TEM) to take us into the world of ultrasmall structures. This
More informationHow To Understand The Measurement Process
April 24, 2015 Exam #3: Solution Key online now! Graded exams by Monday! Final Exam Monday, May 4 th, 10:30 a.m. Room: Perkins 107 1 A Classical Perspective A classical view will help us understand the
More informationLecture 3: Optical Properties of Bulk and Nano. 5 nm
Lecture 3: Optical Properties of Bulk and Nano 5 nm First H/W#1 is due Sept. 10 Course Info The Previous Lecture Origin frequency dependence of χ in real materials Lorentz model (harmonic oscillator model)
More informationDetermination of Molecular Structure by MOLECULAR SPECTROSCOPY
Determination of Molecular Structure by MOLEULAR SPETROSOPY hemistry 3 B.Z. Shakhashiri Fall 29 Much of what we know about molecular structure has been learned by observing and analyzing how electromagnetic
More informationTime dependence in quantum mechanics Notes on Quantum Mechanics
Time dependence in quantum mechanics Notes on Quantum Mechanics http://quantum.bu.edu/notes/quantummechanics/timedependence.pdf Last updated Thursday, November 20, 2003 13:22:37-05:00 Copyright 2003 Dan
More informationKEY. Honors Chemistry Assignment Sheet- Unit 3
KEY Honors Chemistry Assignment Sheet- Unit 3 Extra Learning Objectives (beyond regular chem.): 1. Related to electron configurations: a. Be able to write orbital notations for s, p, & d block elements.
More informationCHAPTER 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 informationChapter 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 informationQuantum 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 information3) 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 informationChapter 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 informationUse the following image to answer the next question. 1. Which of the following rows identifies the electrical charge on A and B shown above?
Old Science 30 Physics Practice Test A on Fields and EMR Test Solutions on the Portal Site Use the following image to answer the next question 1. Which of the following rows identifies the electrical charge
More informationExperiment #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 informationCalculating 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 informationModels of the Atom and periodic Trends Exam Study Guide
Name 1. What is the term for the weighted average mass of all the naturally occurring isotopes of an element? ans: atomic mass 2. Which is exactly equal to 1/12 the mass of a carbon -12 atom? ans: atomic
More informationP. Table & E Configuration Practice TEST
P. Table & E Configuration Practice TEST Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A line spectrum is produced when an electron moves from one energy
More informationFluorescence for high school students
Fluorescence for high school students Niek G Schultheiss 1,2 and Tom W Kool 3 1 Nikhef, Amsterdam, the Netherlands 2 Zaanlands Lyceum, Zaandam, the Netherlands 3 Van t Hoff Institute for Molecular Sciences,
More informationCHAPTER 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 informationPreview of Period 3: Electromagnetic Waves Radiant Energy II
Preview of Period 3: Electromagnetic Waves Radiant Energy II 3.1 Radiant Energy from the Sun How is light reflected and transmitted? What is polarized light? 3.2 Energy Transfer with Radiant Energy How
More informationExperiment IV: Atomic Spectra and the Bohr model
P19: INTRODUCTORY PHYSICS III Experiment IV: Atomic Spectra and the Bohr model Department of Physics and Astronomy Dartmouth College 6127 Wilder Laboratory Hanover, NH 03755 USA Overview In this lab, we
More information