Higher -o-o-o- Past Paper questions o-o-o- 3.4 Spectra
|
|
|
- Randall Cox
- 5 years ago
- Views:
Transcription
1 Higher -o-o-o- Past Paper questions o-o-o- 3.4 Spectra
2
3 1992 Q37 The diagram below shows the energy levels for the hydrogen atom. (a) Between which two energy levels would an electron transition lead to the emission of radiation of highest frequency? (b) Calculate the frequency of the radiation in part (a). [Data:- Planck s constant = 6.63x10-34 Js] 1996 Q36 A particular atom has energy levels as shown below. Transitions are possible between all these levels to produce emission lines in the spectrum. (a) How many lines are in the spectrum of this atom? (b) Between which two energy levels would an electron transition lead to the emission of radiation of the lowest frequency? (c) Explain why some lines in the spectrum are more intense than others.
4 1993 Q9 (a) Laser light is monochromatic and coherent. Briefly explain the meaning of the terms monochromatic and coherent. (b) A laser radiates energy when electrons are stimulated to fall from energy level E 2 to energy level E 1 as shown in the diagram. (i) What are the frequency and wavelength of the radiation emitted? (ii) Name the section of the electromagnetic spectrum in which the radiation occurs. (c) The beam of light from a laser is very intense. Give two reasons for this.
5 1994 Q10 (a) A sodium vapour lamp emits bright yellow light when electrons make transitions from one energy level to another within the sodium atoms. (i) State whether electrons are moving to higher or lower energy levels when the light is emitted. (ii) Using information provided in the data sheet, calculate the energy difference between these two electron energy levels in the sodium atom. [Data:- Planck s constant = 6.63x10-34 Js ] (b) A Bunsen flame containing vaporised sodium is placed between a sodium vapour lamp and a screen as shown. (i) Explain why a dark shadow of the flame is seen on the screen. (ii) The sodium vapour lamp is replaced with a cadmium vapour lamp. Explain why there is now no dark shadow of the flame on the screen.
6 1998 Q9 The line emission spectrum of hydrogen has four lines in the visible spectrum as shown in the following diagram. These four lines are caused by electron transitions in a hydrogen atom from high energy levels to a low energy level E 2 as shown below. (a) From the information above, state which spectral line W, X, Y or Z is produced by an electron transition from E 3 to E 2. (b) Explain why lines Y and Z in the line emission spectrum are brighter than the other two lines. (c) Infrared radiation of frequency 7.48x10 13 Hz is emitted from a hydrogen atom. (i) Calculate the energy of one photon of this radiation. (ii) Show by calculation which electron transition produces this radiation.
7 2001 Q11 The diagram shows some of the energy levels in an atom. (a) For the energy levels shown, how many different wavelengths of radiation can be emitted? (b) Which transition between the energy levels in the above diagram produces radiation with the shortest wavelength? You must justify your answer. Numerical calculation is not required. (c) An electron makes the transition from energy level E 3 to energy level E 2. (i) Calculate the energy of the photon emitted. (ii) Calculate the Wavelength of the photon emitted. (iii) Using the data sheet, identify the element in which this transition occurs.
8 2003 Q27 (a) (a) Electrons which orbit the nucleus of an atom can be considered as occupying discrete energy levels. The following diagram shows some of the energy levels for a particular atom. (i) The transition between which two of these energy levels produces radiation with the longest wavelength? You must justify your answer. (ii) Calculate the frequency of the photon produced when an electron falls from E 3 to E Q28. (a) Electrons which orbit the nucleus of an atom can be considered as occupying discrete energy levels. The following diagram shows some of the energy levels for a particular atom. (i) Radiation is produced when electrons make transitions from a higher to a lower energy level. Which transition, between these energy levels, produces radiation with the shortest wavelength? Justify your answer. (ii) An electron is excited from energy level E 2 to E 3 by absorbing light energy. What frequency of light is used to excite this electron?
Higher Physics. Particles and Waves
Perth Academy Physics Department Higher Physics Particles and Waves Particles and Waves Homework Standard Model 1 Electric Fields and Potential Difference 2 Radioactivity 3 Fusion & Fission 4 The Photoelectric
Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.
The Bohr Atom Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. What is the energy of the emitted photon when an electron drops from the third
Do 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
The Structure of the Atom
CHAPTER 5 The Structure of the Atom 5.4 Light and Spectroscopy 460 370 BC 1808 1870 1897 1910 1925 Today Democritus Atomism Dalton Modern atomic theory Crookes Cathode rays Thomson Discovery of the electron
Bohr. Electronic Structure. Spectroscope. Spectroscope
Bohr Electronic Structure Bohr proposed that the atom has only certain allowable energy states. Spectroscope Using a device called a it was found that gaseous elements emitted electromagnetic radiation
Atomic Spectra for Atoms and Ions. Light is made up of different wavelengths
Atomic Spectra for Atoms and Ions What will you be doing in lab next week? Recording the line spectra of several different substances in discharge tubes. Recording the line spectra of several ions from
The 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
1) Introduction 2) Photo electric effect 3) Dual nature of matter 4) Bohr s atom model 5) LASERS
1) Introduction 2) Photo electric effect 3) Dual nature of matter 4) Bohr s atom model 5) LASERS 1. Introduction Types of electron emission, Dunnington s method, different types of spectra, Fraunhoffer
Ex: N has 5 valence electrons, so it s Lewis structure would look like: N
Chemistry Ms. Ye Review: Bohr Model of the Atom Name Date Block Electrons are shown in concentric shells or energy levels around the nucleus o The first shell can hold up to o The second shell can hold
Light, Waves, and Electrons
Light, Waves, and Electrons Light: Travels 1. 2. Light Waves Wavelength Frequency Electromagnetic Spectrum Speed of light The product of frequency of a wave and wavelength = the speed of light Calculate
Chapter 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
Light Emission.
Light Emission www.physics.sfasu.edu/friedfeld/ch29lec.ppt Radio waves are produced by electrons moving up and down an antenna. Visible light is produced by electrons changing energy states in an atom.
c = 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
Particle nature of light & Quantization
Particle nature of light & Quantization A quantity is quantized if its possible values are limited to a discrete set. An example from classical physics is the allowed frequencies of standing waves on a
Bohr Diagram, Lewis Structures, Valence Electrons Review 1. What is the maximum number of electrons you can fit in each energy level or shell?
AP Chemistry Ms. Ye Name Date Block Bohr Diagram, Lewis Structures, Valence Electrons Review 1. What is the maximum number of electrons you can fit in each energy level or shell? 1 st shell 2 nd shell
Chapter 28 Assignment Solutions
Chapter 28 Assignment Solutions Page 770 #23-26, 29-30, 43-48, 55 23) Complete the following concept map using these terms: energy levels, fixed electron radii, Bohr model, photon emission and absorption,
The relationship between these aspects is described by the following equation: E = hν =
1 Learning Outcomes EXPERIMENT A10: LINE SPECTRUM Upon completion of this lab, the student will be able to: 1) Examine the line spectrum of the hydrogen atom. 2) Calculate the frequency and energy of the
Types of Spectra. How do spectrum lines form? 3/30/09. Electron cloud. Atom. Nucleus
The electron should be thought of as a distribution or cloud of probability around the nucleus that on average behave like a point particle on a fixed circular path Types of Spectra How do spectrum lines
Line Spectra. 6 The line spectrum of hydrogen includes no X-ray frequencies because
TOPI 27 Line Spectra 1 The table below gives the energies of the six lowest levels of the hydrogen atom: Leveln 2 3 nergy/j -2.2 x 10-'8-5.3 X 10-'9-2.4 X 10-'9 Level 11 4 5 6 nergy/j -1.3 x JO-'9-8.0
Higher Physics Particles and Waves 2 Notes
Higher Physics Particles and Waves 2 Notes Teachers Booklet Learning Outcomes Interference and diffraction This builds on information from N5 Waves and Radiation H Particles and Waves book 1 At the end
Unit 1. Electronic Structure page 1
Unit 1 Electronic Structure Section 1. Learning Outcomes Practice Questions Answers Electronic Structure Electromagnetic spectrum / calculations Electron configuration / Periodic Table Electronic Structure
Bright line spectrum questions
Base your answers to questions 1 and 2 on the information below and on your knowledge of chemistry. The bright-line spectra for four elements and a mixture of elements are shown in the diagram below. 1.
Unit 2 - Particles and Waves - Part 2
WAVE-PARTICLE DUALITY Unit - Particles and Waves - Part 8. The photoelectric effect and wave particle duality Photoelectric effect as evidence for the particulate nature of light. Photons of sufficient
Arrangement of Electrons in the Atom
Arrangement of Electrons in the Atom Bohr s Study of Atomic Spectra When white light is passed through a prism, the white light is broken up into an array of colours. This spread of colours is called a
Chapter 7 QUANTUM THEORY & ATOMIC STRUCTURE Brooks/Cole - Thomson
Chapter 7 QUANTUM THEORY & ATOMIC STRUCTURE 1 7.1 The Nature of Light 2 Most subatomic particles behave as PARTICLES and obey the physics of waves. Light is a type of electromagnetic radiation Light consists
Chemistry 212 ATOMIC SPECTROSCOPY
Chemistry 212 ATOMIC SPECTROSCOPY The emission and absorption of light energy of particular wavelengths by atoms and molecules is a common phenomenon. The emissions/absorptions are characteristic for each
PHYS General Physics II Lab The Balmer Series for Hydrogen Source. c = speed of light = 3 x 10 8 m/s
PHYS 1040 - General Physics II Lab The Balmer Series for Hydrogen Source Purpose: The purpose of this experiment is to analyze the emission of light from a hydrogen source and measure and the wavelengths
1 Electrons are emitted from a metal surface when it is illuminated with suitable electromagnetic radiation. ...[1]
![1 Electrons are emitted from a metal surface when it is illuminated with suitable electromagnetic radiation. ...[1]](/thumbs/81/83978040.jpg "1 Electrons are emitted from a metal surface when it is illuminated with suitable electromagnetic radiation. ...[1]")
1 Electrons are emitted from a metal surface when it is illuminated with suitable electromagnetic radiation. 1 (a) (b) Name the effect described above....[1] The variation with frequency f of the maximum
Chapter 5 Electrons In Atoms
Chapter 5 Electrons In Atoms 5.1 Revising the Atomic Model 5.2 Electron Arrangement in Atoms 5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 Copyright Pearson Education, Inc., or its affiliates.
Lab: Excited Electrons
Part A: EMISSION SPECTROSCOPY Lab: Excited Electrons According to the Bohr atomic model, electrons orbit the nucleus within specific energy levels. These levels are defined by unique amounts of energy.
WEEK 2: 4 SEP THRU 10 SEP; LECTURES 4-6
Learning Objectives Energy: Light as energy Describe the wave nature of light, wavelength, and frequency using the equation c = λν What is meant by the particle nature of light? Calculate the energy of
Unit 2 Particles and Waves
North Berwick High School Higher Physics Department of Physics Unit 2 Particles and Waves Section 7 Spectra Section 7 Spectra Note Making Make a dictionary with the meanings of any new words. Irradiance
I understand the relationship between energy and a quanta I understand the difference between an electron s ground state and an electron s excited
NCCS 1.1.2 & 1.1.3 I understand the relationship between energy and a quanta I understand the difference between an electron s ground state and an electron s excited state I will describe how an electron
The 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
hf = E 1 - E 2 hc = E 1 - E 2 λ FXA 2008 Candidates should be able to : EMISSION LINE SPECTRA
1 Candidates should be able to : EMISSION LINE SPECTRA Explain how spectral lines are evidence for the existence of discrete energy levels in isolated atoms (i.e. in a gas discharge lamp). Describe the
Wavelength (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
AST 102 chapter 5. Radiation and Spectra. Radiation and Spectra. Radiation and Spectra. What is light? What is radiation?
5 Radiation and Spectra 1 Radiation and Spectra What is light? According to Webster: a.something that makes vision possible b.the sensation aroused by stimulation of the visual receptors c.electromagnetic
Quick Review. 1. Kinetic Molecular Theory. 2. Average kinetic energy and average velocity. 3. Graham s Law of Effusion. 4. Real Gas Behavior.
Quick Review 1. Kinetic Molecular Theory. 2. Average kinetic energy and average velocity. 3. Graham s Law of Effusion. 4. Real Gas Behavior. Emission spectra Every element has a unique emission spectrum
PhysicsAndMathsTutor.com 1
Q1. When a clean metal surface in a vacuum is irradiated with ultraviolet radiation of a certain frequency, electrons are emitted from the metal. (a) Explain why the kinetic energy of the emitted electrons
The 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
where n = (an integer) =
5.111 Lecture Summary #5 Readings for today: Section 1.3 (1.6 in 3 rd ed) Atomic Spectra, Section 1.7 up to equation 9b (1.5 up to eq. 8b in 3 rd ed) Wavefunctions and Energy Levels, Section 1.8 (1.7 in
The 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)
Modern Atomic Theory and Electron Configurations
Chem 101 Modern Atomic Theory and Electron Configurations Lectures 8 and 9 Types of Electromagnetic Radiation Electromagnetic radiation is given off by atoms when they have been excited by any form of
What are the energies (J) and wavelengths (in nm) for these colors? Color Energy wavelength. Rev. F11 Page 1 of 5
Exp. 8 Pre Lab ASSIGNMENT Name: Lab Section Score: / 10 (1) Use the equations [see the discussion on the next page] to calculate the energies of the 6 lowest states for the hydrogen atom, and enter your
Chapter 6: The Electronic Structure of the Atom Electromagnetic Spectrum. All EM radiation travels at the speed of light, c = 3 x 10 8 m/s
Chapter 6: The Electronic Structure of the Atom Electromagnetic Spectrum V I B G Y O R All EM radiation travels at the speed of light, c = 3 x 10 8 m/s Electromagnetic radiation is a wave with a wavelength
HOMEWORK - Chapter 4 Spectroscopy
Astronomy 10 HOMEWORK - Chapter 4 Spectroscopy Use a calculator whenever necessary. For full credit, always show your work and explain how you got your answer in full, complete sentences on a separate
Electromagnetic spectrum Electromagnetic radiation
Chapter 4 Section 1 Electromagnetic spectrum includes all the different wave lengths of radiation. Electromagnetic radiation is a form of energy that exhibits wave like behavior as it travels through space.
A fluorescent tube is filled with mercury vapour at low pressure. After mercury atoms have been excited they emit photons.
Q1.(a) A fluorescent tube is filled with mercury vapour at low pressure. After mercury atoms have been excited they emit photons. In which part of the electromagnetic spectrum are these photons? What is
2) 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,
Chapter 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
Light Emission. Today s Topics. Excitation/De-Excitation 10/26/2008. Excitation Emission Spectra Incandescence
Light Emission Excitation Emission Spectra Incandescence Absorption Spectra Today s Topics Excitation/De-Excitation Electron raised to higher energy level Electron emits photon when it drops back down
Atomic Physics Worksheet. between 4000 and 5000 Angstroms ( nanometers): between 6500 and 7500 Angstroms ( nanometers):
Atomic Physics Worksheet 1. Which of the gas samples shows an emission line with a wavelength between 4000 and 5000 Angstroms (400-500 nanometers): between 6500 and 7500 Angstroms (650-750 nanometers):
Experiment 3 Electromagnetic Radiation and Atom Interaction
Experiment 3 Electromagnetic Radiation and Atom Interaction B OBJECTIVES To be familiar with the relationship between emission line spectra and the energy levels of electrons in various atoms. B INTRODUCTION
Electrons, 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.
Chapter 5 Electrons In Atoms
Chapter 5 Electrons In Atoms 5.1 Revising the Atomic Model 5.2 Electron Arrangement in Atoms 5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 Copyright Pearson Education, Inc., or its affiliates.
5.3. 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
Chapter 5 Light and Matter: Reading Messages from the Cosmos. What is light? Properties of Waves. Waves. The Electromagnetic Spectrum
Chapter 5 Light and Matter: Reading Messages from the Cosmos What is light? Light is a form of radiant energy Light can act either like a wave or like a particle (photon) Spectrum of the Sun 1 2 Waves
WAVES AND PARTICLES. (c)
WAVES AND PARTICLES 1. An electron and a proton are accelerated through the same potential difference. The ration of their De Broglie wave length will be -- (a) (b) (c) (d) 1 2. What potential must be
NOTES: 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
Chapter 4. Spectroscopy. Dr. Tariq Al-Abdullah
Chapter 4 Spectroscopy Dr. Tariq Al-Abdullah Learning Goals: 4.1 Spectral Lines 4.2 Atoms and Radiation 4.3 Formation of the Spectral Lines 4.4 Molecules 4.5 Spectral Line Analysis 2 DR. T. AL-ABDULLAH
Chapter 4 Spectroscopy
Chapter 4 Spectroscopy The beautiful visible spectrum of the star Procyon is shown here from red to blue, interrupted by hundreds of dark lines caused by the absorption of light in the hot star s cooler
Electrons, Energy, & the Electromagnetic Spectrum Notes
Electrons, Energy, & the Electromagnetic Spectrum Notes Bohr Model Diagram Interpretation What form of EM radiation is released when an electron in a hydrogen atom falls from the 5 th energy level to the
CSUS Department of Chemistry Experiment 9 Chem. 1A
CSUS Department of Chemistry xperiment 9 Chem. 1A xp. 9 PR-Lab ASSIGNMNT Name: Lab Section (1) Use equation (2) [see the discussion on the next page] to calculate the energies of the ten lowest states
LIGHT. Question. Until very recently, the study of ALL astronomical objects, outside of the Solar System, has been with telescopes observing light.
LIGHT Question Until very recently, the study of ALL astronomical objects, outside of the Solar System, has been with telescopes observing light. What kind of information can we get from light? 1 Light
Dept. of Physics, MIT Manipal 1
Chapter 1: Optics 1. In the phenomenon of interference, there is A Annihilation of light energy B Addition of energy C Redistribution energy D Creation of energy 2. Interference fringes are obtained using
Electromagnetic Radiation. is a form of energy that exhibits wavelike behavior as it travels through space.
Electromagnetic Radiation is a form of energy that exhibits wavelike behavior as it travels through space. What are the 7 forms of electromagnetic radiation, in order of INCREASING wavelength? gamma rays
RED. BLUE Light. Light-Matter
1 Light-Matter This experiment demonstrated that light behaves as a wave. Essentially Thomas Young passed a light of a single frequency ( colour) through a pair of closely spaced narrow slits and on the
Chapter 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
Pre-Lab Exercises Lab 2: Spectroscopy
Pre-Lab Exercises Lab 2: Spectroscopy 1. Which color of visible light has the longest wavelength? Name Date Section 2. List the colors of visible light from highest frequency to lowest frequency. 3. Does
Introduction to light Light is a form of energy called electromagnetic radiation. A chart of the electromagnetic spectrum is shown below.
Experiment: Spectroscopy Introduction to light Light is a form of energy called electromagnetic radiation. A chart of the electromagnetic spectrum is shown below. Radiowave Microwave Infrared Visible Ultraviolet
Electron Energy and Light
Why? Electron Energy and Light How does light reveal the behavior of electrons in an atom? From fireworks to stars, the color of light is useful in finding out what s in matter. The emission of light by
General Chemistry by Ebbing and Gammon, 8th Edition
Chem 1045 General Chemistry by Ebbing and Gammon, 8th Edition George W.J. Kenney, Jr Last Update: 26-Mar-2009 Chapter 7: Quantum Theory of the Atom These Notes are to SUPPLIMENT the Text, They do NOT Replace
Conceptual Physics Fundamentals
Conceptual Physics Fundamentals Chapter 15: QUANTUM THEORY This lecture will help you understand: The Photoelectric Effect Absorption Spectra Fluorescence Incandescence Lasers Wave-Particle Duality Particles
Electrons in Atoms. Section 5.1 Light and Quantized Energy
Name Date Class 5 Electrons in Atoms Section 5.1 Light and Quantized Energy In your textbook, read about the wave nature of light. Use each of the terms below just once to complete the passage. amplitude
Write 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
Physics 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
Experiment #9. Atomic Emission Spectroscopy
Introduction Experiment #9. Atomic Emission Spectroscopy Spectroscopy is the study of the interaction of light with matter. This interaction can be in the form of the absorption or the emission of electromagnetic
Information in Radio Waves
Summative Assessment: Natural Sources of Radio Performance expectation: Develop and use a model of two objects interacting through electric or magnetic fields to illustrate the forces between objects and
ATOMIC STRUCTURE ELECTRON CONFIGURATION 10/13/15 PROJECT DATE. Tuesday, October 13, 15
PROJECT DATE ATOMIC STRUCTURE ELECTRON CONFIGURATION 10/13/15 Agenda Begin Topic 2.2 Electron Configuration Homework: Energy of waves calculations Due tomorrow! Yes - tomorrow Atomic Structure The nuclear
Atomic Theory: Spectroscopy and Flame Tests
Atomic Theory: Spectroscopy and Flame Tests Introduction Light energy is also known as electromagnetic (EM) radiation. The light that we observe with our eyes, visible light, is just a small portion of
Democritus & Leucippus (~400 BC) Greek philosophers: first to propose that matter is made up of particles called atomos, the Greek word for atoms
Chemistry Ms. Ye Name Date Block The Evolution of the Atomic Model Since atoms are too small to see even with a very powerful microscope, scientists rely upon indirect evidence and models to help them
Atomic Theory: Spectroscopy and Flame Tests
Atomic Theory: Spectroscopy and Flame Tests Introduction Light energy is also known as electromagnetic (EM) radiation. The light that we observe with our eyes, visible light, is just a small portion of
The Bohr Model Bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.
5.1 The Development of Atomic Models Rutherford s atomic model could not explain the chemical properties of elements. Rutherford s atomic model could not explain why objects change color when heated. The
Instructor Resources
SPECTROSCOPY Quantitative Analysis with Light Instructor Resources Learning Objectives The objectives of this experiment are to: identify band and line spectra, and relate the physical state of a light-emitting
An element Is a substance that cannot be split into simpler substance. It is composed of discrete particles called atoms.
digitalteachers.co.ug Atomic structure Inorganic chemistry deals with the physical and chemical properties of the elements of the the periodic table. An element Is a substance that cannot be split into
Properties 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
It s a wave. It s a particle It s an electron It s a photon. It s light!
It s a wave It s a particle It s an electron It s a photon It s light! What they expected Young s famous experiment using a beam of electrons instead of a light beam. And, what they saw Wave-Particle Duality
Models of the Atom. Spencer Clelland & Katelyn Mason
Models of the Atom Spencer Clelland & Katelyn Mason First Things First Electrons were accepted to be part of the atom structure by scientists in the1900 s. The first model of the atom was visualized as
THE UNIVERSITY OF QUEENSLAND DEPARTMENT OF PHYSICS PHYS2041 ATOMIC SPECTROSCOPY
THE UNIVERSITY OF QUEENSLAND DEPARTMENT OF PHYSICS PHYS2041 ATOMIC SPECTROSCOPY Warning: The mercury spectral lamps emit UV radiation. Do not stare into the lamp. Avoid exposure where possible. Introduction
Unit 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
Atomic Theory: Spectroscopy and Flame Tests
Atomic Theory: Spectroscopy and Flame Tests Introduction Light energy is also known as electromagnetic (EM) radiation. The light that we observe with our eyes, visible light, is just a small portion of
[2] (b) An electron is accelerated from rest through a potential difference of 300 V.
![[2] (b) An electron is accelerated from rest through a potential difference of 300 V.](/thumbs/89/98791036.jpg "[2] (b) An electron is accelerated from rest through a potential difference of 300 V.")
1 (a) In atomic physics electron energies are often stated in electronvolts (ev) Define the electronvolt. State its value in joule.. [2] (b) An electron is accelerated from rest through a potential difference
Atomic Theory C &03
Atomic Theory Part One: Flame Tests Part Two: Atomic Spectra Part Three: Applications of Spectra (optional) C12-2-02 &03 This activity will focus on the visible portion of the electromagnetic spectrum.
(i) Show that the energy of a single photon is about 3 x J.
1(a) A helium-neon laser emits red light of wavelength 6.3 x 10 7 m. (i) Show that the energy of a single photon is about 3 x 10 19 J. [2] The power of the laser beam is 1.0 mw. Show that about 3 x 10
Light. October 16, Chapter 5: Electrons in Atoms Honors Chemistry. Bohr Model
Chapter 5: Electrons in Atoms Honors Chemistry Bohr Model Niels Bohr, a young Danish physicist and a student of Rutherford improved Rutherford's model. Bohr proposed that an electron is found only in specific
CHM 111 Unit 7 Sample Questions
Name: Class: Date: As you work these problems, consider and explain: A. What type of question is it? B. How do you know what type of question it is? C. What information are you looking for? D. What information
ATOMIC WORLD P.1. ejected photoelectrons. current amplifier. photomultiplier tube (PMT)
ATOMIC WORLD P. HKAL PAPER I 0 8 The metal Caesium has a work function of.08 ev. Given: Planck constant h = 6.63 0 34 J s, charge of an electron e =.60 0 9 C (a) (i) Calculate the longest wavelength of
Light, Electrons, and Energy. Pre-AP
Light, Electrons, and Energy Pre-AP Light Waves! Electromagnetic Frequency Light Phenomenon Light can act as a wave or as a particle, but most light-electron interactions use wave physics. = greek letter
Electrons in Atoms. Section 5.1 Light and Quantized Energy Section 5.2 Quantum Theory and the Atom Section 5.3 Electron Configuration
Electrons in Atoms Section 5.1 Light and Quantized Energy Section 5.2 Quantum Theory and the Atom Section 5.3 Electron Configuration Click a hyperlink or folder tab to view the corresponding slides. Exit
Background: The Electromagnetic Spectrum
Background: The Electromagnetic Spectrum Wavelength (λ) in meters wavelength decreasing 10 4 10 2 10 0 10-2 10-4 10-6 10-8 10-10 10-12 10-14 microwaves ultraviolet Gamma rays Radio waves AM 10 4 Shortwave