SO FAR: We Solved some of the Problems with Classical Physics
|
|
- Laurence Harmon
- 5 years ago
- Views:
Transcription
1 SO FAR: We Solved some of the Problems with Classical Physics Blackbody Radiation? Plank Quantized Energy of Atoms: En nhf Photoelectric Effect? Einstein Quantized energy states of light photons: E hf Compton Effect? Light is a particle with momentum! h Matter Waves? debroglie waves! e p Discrete Spectra? Atoms?
2
3 Continuous vs Discrete This is a continuous spectrum of colors: all colors are present. This is a discrete spectrum of colors: only a few are present. Copyright 2008 Pearson Education, Inc., publishing as Pearson Addison-Wesley.
4 Continuous Discrete
5 Review: Dispersion: Diffraction Gratings How does dispersion with a grating compare with a prism? Longer wavelength light is bent more with a grating. Shorter wavelength light is bent more with a prism. d sin m Copyright 2008 Pearson Education, Inc., publishing as Pearson Addison-Wesley.
6 Incandescent Light Bulb Copyright 2008 Pearson Education, Inc., publishing as Pearson Addison-Wesley.
7 Hydrogen Spectra Copyright 2008 Pearson Education, Inc., publishing as Pearson Addison-Wesley.
8 Helium Spectra Copyright 2008 Pearson Education, Inc., publishing as Pearson Addison-Wesley.
9 Mercury Spectra Copyright 2008 Pearson Education, Inc., publishing as Pearson Addison-Wesley.
10 Neon Spectrum Copyright 2008 Pearson Education, Inc., publishing as Pearson Addison-Wesley.
11 The Evidence.
12 Kirkoff s Rules for Spectra: 1859 German physicist who developed the spectroscope and the science of emission spectroscopy with Bunsen. Kirkoff Bunsen * Rule 1 : A hot and opaque solid, liquid or highly compressed gas emits a continuous spectrum. * Rule 2 : A hot, transparent gas produces an emission spectrum with bright lines. * Rule 3 : If a continuous spectrum passes through a gas at a lower temperature, the transparent cooler gas generates dark absorption lines. Copyright 2008 Pearson Education, Inc., publishing as Pearson Addison-Wesley.
13 Compare absorption lines in a source with emission lines found in the laboratory! Kirchhoff deduced that elements were present in the atmosphere of the Sun and were absorbing their characteristic wavelengths, producing the absorption lines in the solar spectrum. He published in 1861 the first atlas of the solar spectrum, obtained with a prism ; however, these wavelengths were not very precise : the dispersion of the prism was not linear at all. Copyright 2008 Pearson Education, Inc., publishing as Pearson Addison-Wesley.
14 Kirkoff s Rules Copyright 2008 Pearson Education, Inc., publishing as Pearson Addison-Wesley.
15 Anders Jonas Ångström 1869 Ångström measured the wavelengths on the four visible lines of the hydrogen spectrum, obtained with a diffraction grating, whose dispersion is linear, and replaced Kirchhoff's arbitrary scale by the wavelengths, expressed in the metric system, using a small unit (10-10 m) with which his name was to be associated. Line color red blue-green violet violet Wavelength Å Å Å Å
16 Balmer Series: 1885 Johann Balmer found an empirical equation that correctly predicted the four visible emission lines of hydrogen Johannes Robert Rydberg generalized it in 1888 for all transitions: 1 R 1 1 λ 2 n H 2 2 R H is the Rydberg constant R H = x 10 7 m -1 n is an integer, n = 3, 4, 5, The spectral lines correspond to different values of n H α is red, λ = nm H β is green, λ = nm H γ is blue, λ = nm H δ is violet, λ = nm
17 Theories.
18
19 Let no one unversed in geometry enter here. The Universe is made of pure mathematical ideas the Platonic Solids. Plato believed that the stars, planets, Sun and Moon move round the Earth in crystalline spheres.
20 Earth and the universe were seen as constructed out of five basic elements: earth, water, air, fire, and ether. The natural place of the motionless Earth was at the centre of that universe. The stars in the heavens were made up of an indestructible substance called ether (aether) and were considered as eternal and unchanging.
21 Joseph John Thomson Plum Pudding Model 1904 Received Nobel Prize in 1906 Usually considered the discoverer of the electron Worked with the deflection of cathode rays in an electric field His model of the atom A volume of positive charge Electrons embedded throughout the volume
22 1911: Rutherford s Planetary Model of the Atom A beam of positively charged alpha particles hit and are scattered from a thin foil target. Large deflections could not be explained by Thomson s pudding model. (Couldn t explain the stability or spectra of atoms.)
23 1911: Rutherford s Planetary Model of the Atom A beam of positively charged alpha particles hit and are scattered from a thin foil target. Large deflections could not be explained by Thomson s model. (Couldn t explain the stability or spectra of atoms.)
24 Classical Physics at the Limit WHY IS MATTER (ATOMS) STABLE?
25 Electrons exist in quantized orbitals with energies given by multiples of Planck s constant. Light is emitted or absorbed when an electron makes a transition between energy levels. The energy of the photon is equal to the difference in the energy levels: E nhf, n= 0,1,2,3, h 6.626x10 Js E E E hf i f
26 Light Absorption & Emission E E E hf i f
27 Bohr s Model Electrons in an atom can occupy only certain discrete quantized states or orbits. E nhf, n= 0,1,2,3, Electrons are in stationary states: they don t accelerate and they don t radiate. 3. Electrons radiate only when making a transition from one orbital to another, either emitting or absorbing a photon. Postulate: E E E hf i f The angular momentum of an electron is always quantized and cannot be zero: h L n ( n 1,2,3,...) 2
28 Bohr s Derivation of the Energy for Hydrogen: Conservation of E: E K U F is centripetal: Sub back into E: From Angular Momentum: (2) h From : L n = mvr ( n 1,2,3,...) 2 (1) Sub r back into (1): Sub into (2): v kq 2 q q e e e nh 4 0hn 2 0hn Why is it negative?
29 Bohr Orbital Binding Energy for The Hydrogen Atom En eV n 2 Ground State: n = 1 First Excited: n = 2 2 nd Excited: n = eV is the energy of the H ground state. 2. Negative because it is the Binding Energy and work must be done on the atom (by a photon) to ionize it. 3. A 13.6eV photon must be absorbed to ionize the ground state 4. Bohr model only works for single electron atoms since it doesn t take into account electron-electron interaction forces.
30 The frequency of the photon emitted when the electron makes a transition from an outer orbit to an inner orbit is E E k e i f e ƒ 2 2 h 2aoh nf ni It is convenient to look at the wavelength instead The wavelengths are found by 2 1 ƒ kee R 2 2 H 2 2 λ c 2a ohc n f n i n f n i
31 Bohr Line Spectra of Hydrogen Bohr s Theory derived the spectra equations that Balmer, Lyman and Paschen had previously found experimentally! ( ) 2 RZ n 2 2 f n i 7 1 R x10 m Balmer: Visible Lyman: UV Paschen: IR
32 Bohr: Allowed Orbital Radii r n 2 2 n m k e e e n 1, 2, 3, 2 r (5.9x10 m) n n 11 2 rn a n 0 2 n = 1, 2, 3 Bohr Radius (ground state): ao = 5.9x10-11 m
33 Problem A hydrogen atom is in the third (n = 4) excited state. It can make a jump to a different state by transition A, B, or C as shown, and a photon is either emitted or absorbed. a) Which transition, A, B, or C, emits a photon with the greatest energy? Calculate the wavelength in m and the energy in ev. b) What is the energy of a photon needed to ionize the atom when the electron is initially in the third excited state? Calculate in ev. c) What is the orbital radius of the n=4 state? ( ) 2 RZ n 2 2 f n i m (1.097 x10 m )1 ( ) x10 8 m E 13.6eV Z eV eV 2 r n a n 0 ao = 5.9x10-11 m
34 Spontaneous Emission: Random Transition Probabilities Fermi s Golden Rule Transition probabilities correspond to the intensity of light emission.
35 IMPORTANT NOTE!! Free electrons have continuous energy states! Only bound electrons have quantized energy states! This is because they are not forced to fit in a confined space like a wave in a box!!! Continuous or Discrete? Bound-Bound Transitions: Atoms, boxes D Bound-Free Transitions: Ionization C Free-Bound Transitions: Ion captures an electron C Free-Free Transitions: Collisions, electron absorption C
36 1. Bohr model does not explain angular momentum postulate. 2. Bohr model does not explain splitting of spectral lines. 3. Bohr model does not explain multi-electron atoms. 4. Bohr model does not explain ionization energies of elements. E Z ev
37 1. Bohr model does not explain angular momentum postulate: The angular momentum of an electron is always quantized and cannot be zero*: h L n = nh 2 ( n 1,2,3,...) *If L=0 then the electron travels linearly and does not orbit. But if it is orbiting then it should radiate and the atom would be unstable eek gads! WHAT A MESS!
38 If photons can be particles, then why can t electrons be waves? p E hf h c c debroglie Wavelength: e h p Electrons are STANDING WAVES in atomic orbitals. 34 h 6.626x10 J s
39 2 r n n 1924: de Broglie Waves Explains Bohr s postulate of angular h p momentum quantization: 2 r n n h h 2 r n n n p e m v m vr e n h n 2 L m vr nh e n ( n 1,2,3,...)
40 1926:Schrodinger s Equation Rewrite the SE in spherical coordinates. Solutions to it give the possible states of the electron. Solution is sepearable:
41 Quantum Numbers and their quantization are derived purely from Mathematical Solutions of Schrodinger s Equation (boundary conditions) However, they have a phenomenological basis!! To be discussed later Solution:
42 Wave Functions given by Quantum Numbers!! The probability of finding an electron within a shell of radius r and thickness δr around a proton is where the first three radial wave functions of the electron in a neutral hydrogen atom are
43 Quantum H Atom 1s Wave Function: Radial Probability Density: 1 1 s () r e a 3 0 r/ a P(r) = 4πr 2 ψ 2 0 Most Probable value: solve dp 0 dr Average value: rave r rp() r dr 0 Probability in (0-r): P r P() r dr 0
44 Stationary States of Hydrogen Solutions to the Schrödinger equation for the hydrogen atom potential energy exist only if three conditions are satisfied: 1. The atom s energy must be one of the values where a B is the Bohr radius. The integer n is called the principal quantum number. These energies are the same as those in the Bohr hydrogen atom.
45 Stationary States of Hydrogen 2. The angular momentum L of the electron s orbit must be one of the values The integer l is called the orbital quantum number. 3. The z-component of the angular momentum must be one of the values The integer m is called the magnetic quantum number. Each stationary state of the hydrogen atom is identified by a triplet of quantum numbers (n, l, m).
46 Interpretation: Orbital Angular Momentum & its Z-component are Quantized Angular momentum magnitude is quantized: L l( l 1) h ( l 0,1,2,... n 1) Angular momentum direction is quantized: L m h ( m l,.. 1,0,1,2,... l) Z l l For each l, there are (2l+1) possible m l states. cos L z L Note: for n = 1, l = 0. This means that the ground state angular momentum in hydrogen is zero, not h/2, as Bohr assumed. What does it mean for L = 0 in this model?? Standing Wave
47 Zeeman Effect Explained The Zeeman Effect is the splitting of spectral lines when a magnetic field is applied. This is due to the interaction between the external field and the B field produced by the orbital motion of the electron. Only certain angles are allowed between the orbital angular momentum and the external magnetic field resulting in the quantization of space! L m ( m l,.. 1,0,1,2,... l) h L l( l 1) h ( l 0,1,2,... n 1) Z l l
48 Stern-Gerlach 1921 A beam of silver atoms sent through a non-uniform magnetic field was split into two discrete components. Classically, it should be spread out because the magnetic moment of the atom can have any orientation. QM says if it is due to orbital angular momentum, there should be an odd number of components, (2l+1), but only two components are ever seen. This required an overhaul of QM to include Special Relativity. Then the electron magnetic spin falls out naturally from the mathematics. The spin magnetic moment of the electron with two spin magnetic quantum number values: ms 1 2
49
50 Intrinsic Spin is Quantized Fine Line Splitting: B field due to intrinsic spin interacts with B field due to orbital motion and produces additional energy states. Spin magnitude is quantized and fixed: S h 3 h s( s 1) Spin direction is quantized: h 1 1 S m ( m, ) Z s 2 s 2 2 spin e m S
51 Spin is the Spin Quantum Entanglement Quantum Computing The Qubit At the heart of the realm of quantum computation is the qubit. The quantum bit, by analogy with the binary digit, the bit, used by everyday computers, the qubit is the quantum computer's unit of currency. Instead of being in a 1 or zero state, a qubit can be in a superposition of both states.
52
53 Quantum Numbers Once the principal quantum number is known, the values of the other quantum numbers can be found. The possible states of a system are given by combinations of quantum numbers! Quantum Rules n 1,2,3,4... l 0,1,2... n 1 m l, l 1,...,0,1,... l 1, l m l s 1/ 2, 1/ 2
54 Shells and Subshells Shells are determined by the principle quantum number, n. Subshells are named after the type of line they produce in the emission spectrum and are determined by the l quantum number. s: Sharp line (l = 0) p: Very bright principle line( l = 1) d: Diffuse line (l = 2) f: Fundamental (hydrogen like) ( l =3) 1s 2s 2p
55 Wave Functions given by Quantum Numbers!! The probability of finding an electron within a shell of radius r and thickness δr around a proton is where the first three radial wave functions of the electron in a neutral hydrogen atom are
56 Wave Functions for Hydrogen The simplest wave function for hydrogen is the one that describes the 1s (ground) state and is designated ψ 1s (r) 1 rao ψ1 s() r e 3 πa As ψ 1s (r) approaches zero, r approaches and is normalized as presented ψ 1s (r) is also spherically symmetric This symmetry exists for all s states o
57 Radial Probability Density The radial probability density function P(r) is the probability per unit radial length of finding the electron in a spherical shell of radius r and thickness dr 1 A spherical shell of radius r and thickness dr has a volume of 4πr 2 dr The radial probability density function is P(r) = 4πr 2 ψ 2 rao ψ1 s() r e πa 3 o where ψ 1 o 2 2ra 1s e 3 πao P r 4r e 2 2rao 1s () 3 ao
58 P(r) for 1s State of Hydrogen The radial probability density function for the hydrogen atom in its ground state is P r 4r e 2 2rao 1s () 3 ao The peak indicates the most probable location, the Bohr radius. The average value of r for the ground state of hydrogen is 3/2 a o The graph shows asymmetry, with much more area to the right of the peak
59 Electron Clouds The charge of the electron is extended throughout a diffuse region of space, commonly called an electron cloud This shows the probability density as a function of position in the xy plane The darkest area, r = a o, corresponds to the most probable region
60
61
62 Hydrogen 1s Radial Probability
63 Sample Problem
64 Sample Problem
65 Wave Function of the 2s state The next-simplest wave function for the hydrogen atom is for the 2s state n = 2; l = 0 The wave function is 3 2 r r 2a o 1 1 ψ2s( r ) 2 e 4 2π ao ao ψ 2s depends only on r and is spherically symmetric
66 Hydrogen 2s Radial Probability The next-simplest wave function for the hydrogen atom is for the 2s state: n = 2; l = r r 2a o 1 1 ψ2s( r ) 2 e 4 2π ao ao
67 Comparison of 1s and 2s States The plot of the radial probability density for the 2s state has two peaks The highest value of P corresponds to the most probable value In this case, r 5a o
68 Hydrogen 1s Radial Probability
69 Hydrogen 2s Radial Probability
70 Hydrogen 2p Radial Probability
71 Hydrogen 3s Radial Probability
72 Hydrogen 3p Radial Probability
73 Hydrogen 3d Radial Probability
74
75
76 1926:Schrodinger s Equation Rewrite the SE in spherical coordinates. Solutions to it give the possible states of the electron. Solution is sepearable:
77 Quantum Numbers and their quantization are derived purely from Mathematical Solutions of Schrodinger s Equation (boundary conditions) However, they have a phenomenological basis!! To be discussed later Solution:
78 Wave Functions given by Quantum Numbers!! The probability of finding an electron within a shell of radius r and thickness δr around a proton is where the first three radial wave functions of the electron in a neutral hydrogen atom are
79
80 Stationary States of Hydrogen Solutions to the Schrödinger equation for the hydrogen atom potential energy exist only if three conditions are satisfied: 1. The atom s energy must be one of the values where a B is the Bohr radius. The integer n is called the principal quantum number. These energies are the same as those in the Bohr hydrogen atom.
81 Stationary States of Hydrogen 2. The angular momentum L of the electron s orbit must be one of the values The integer l is called the orbital quantum number. 3. The z-component of the angular momentum must be one of the values The integer m is called the magnetic quantum number. Each stationary state of the hydrogen atom is identified by a triplet of quantum numbers (n, l, m).
82 Interpretation: Orbital Angular Momentum & its Z-component are Quantized Angular momentum magnitude is quantized: L l( l 1) h ( l 0,1,2,... n 1) Angular momentum direction is quantized: L m h ( m l,.. 1,0,1,2,... l) Z l l For each l, there are (2l+1) possible m l states. cos L z L Note: for n = 1, l = 0. This means that the ground state angular momentum in hydrogen is zero, not h/2, as Bohr assumed. What does it mean for L = 0 in this model?? Standing Wave
83 Intrinsic Spin is Quantized Fine Line Splitting: B field due to intrinsic spin interacts with B field due to orbital motion and produces additional energy states. Spin magnitude is quantized and fixed: S h 3 h s( s 1) Spin direction is quantized: h 1 1 S m ( m, ) Z s 2 s 2 2 spin e m S
84 Spin is the Spin Quantum Entanglement Quantum Computing The Qubit At the heart of the realm of quantum computation is the qubit. The quantum bit, by analogy with the binary digit, the bit, used by everyday computers, the qubit is the quantum computer's unit of currency. Instead of being in a 1 or zero state, a qubit can be in a superposition of both states.
85
86 Quantum Numbers Once the principal quantum number is known, the values of the other quantum numbers can be found. The possible states of a system are given by combinations of quantum numbers! Quantum Rules n 1,2,3,4... l 0,1,2... n 1 m l, l 1,...,0,1,... l 1, l m l s 1/ 2, 1/ 2
87 Shells and Subshells Shells are determined by the principle quantum number, n. Subshells are named after the type of line they produce in the emission spectrum and are determined by the l quantum number. s: Sharp line (l = 0) p: Very bright principle line( l = 1) d: Diffuse line (l = 2) f: Fundamental (hydrogen like) ( l =3) 1s 2s 2p
88
89
90 Pauli Exclusion Principle No two electrons can have the same set of quantum numbers. That is, no two electrons can be in the same quantum state. From the exclusion principle, it can be seen that only two electrons can be present in any orbital: One electron will have spin up and one spin down. Maximum number of electrons in a shell is: # = 2n 2 Maximum number of electrons in a subshell is: # = 2(2l+1) You must obey Pauli to figure out how to fill orbitals, shells and subshells. (This is not true of photons or other force carrying particles such as gravitons or gluons (bosons))
91 Hund s Rule Hund s Rule states that when an atom has orbitals of equal energy, the order in which they are filled by electrons is such that a maximum number of electrons have unpaired spins Some exceptions to the rule occur in elements having subshells that are close to being filled or half-filled
92 Hund s Rule Hund s Rule states that when an atom has orbitals of equal energy, the order in which they are filled by electrons is such that a maximum number of electrons have unpaired spins Some exceptions to the rule occur in elements having subshells that are close to being filled or half-filled The filling of electronic states must obey both the Pauli Exclusion Principle and Hund s Rule.
93
94 How many electrons in n=3 Shell? n 3 l 0,1,2 m m l s Quantum Rules n 1,2,3,4... l 0,1,2... n 1 m l, l 1,...,0,1,... l 1, l m l s 1/ 2, 1/ 2 2, 1,0,1,2 1/ 2, 1/ 2 2(2l 1) 2e 6e 10e =18e = 2n 2
95 Bohr model does not explain ionization energies of elements but QM does. How?
96 Spontaneous Emission: Random Transition Probabilities Fermi s Golden Rule Transition probabilities correspond to the intensity of light emission.
97 Excited States and Spectra An atom can jump from one stationary state, of energy E 1, to a higher-energy state E 2 by absorbing a photon of frequency In terms of the wavelength: Note that a transition from a state in which the valence electron has orbital quantum number l 1 to another with orbital quantum number l 2 is allowed only if
98 Hydrogen Energy Level Diagram Selection Rules The selection rules for allowed transitions are Δl = ±1 Δm l = 0, ±1 Transitions in which l does not change are very unlikely to occur and are called forbidden transitions Such transitions actually can occur, but their probability is very low compared to allowed transitions
99 X-Ray Production The discrete lines are called characteristic x-rays. These are created when A bombarding electron collides with a target atom The electron removes an inner-shell electron from orbit An electron from a higher orbit drops down to fill the vacancy Typically, the energy is greater than 1000 ev The continuous spectrum is called bremsstrahlung, the German word for braking radiation
100 Synchrotron Radiation X-Ray and Radio
101
102 X Ray Imaging when X-ray light shines on us, it goes through our skin, but allows shadows of our bones to be projected onto and captured by film. When X-ray light shines on us, it goes through our skin, but allows shadows of our bones to be projected onto and captured by film.
103 Lasers Light Amplification by Stimulated Emission of Radiation "A splendid light has dawned on me about the absorption and emission of radiation..." Albert Einstein, 1916
104 Stimulated Emission 1 photon in, 2 out "When you come right down to it, there is really no such thing as truly spontaneous emission; its all stimulated emission. The only distinction to be made is whether the field that does the stimulating is one that you put there or one that God put there..." David Griffths, Introduction to Quantum Mechanics
105
106
107 Stimulated Emission
108 Sample Problem What average wavelength of visible light can pump neodymium into levels above its metastable state? From the figure it takes 2.1eV to pump neodymium into levels above its metastable state. Thus, hc E ev m 2.10 ev m 590 nm
109 Laser Applications
110 Phaser?
111 UV in, vibrant color out. Fluorescence
112 Phosphorescence Time Delayed Fluorescence Glow in the Dark: Day Glow
113 BTW: Iridescence: Diffraction
We now realize that the phenomena of chemical interactions, and, ultimately life itself, are to be understood in terms of electromagnetism".
We now realize that the phenomena of chemical interactions, and, ultimately life itself, are to be understood in terms of electromagnetism". -Richard Feynman Quantum H Atom Review Radia Wave Function (1s):
More informationChapter 28. Atomic Physics
Chapter 28 Atomic Physics Quantum Numbers and Atomic Structure The characteristic wavelengths emitted by a hot gas can be understood using quantum numbers. No two electrons can have the same set of quantum
More informationChapter 29 Atomic Physics. Looking Ahead. Slide 29-1
Chapter 29 Atomic Physics Looking Ahead Slide 29-1 Atomic Spectra and the Bohr Model In the mid 1800s it became apparent that the spectra of atomic gases is comprised of individual emission lines. Slide
More informationChapter 28. Atomic Physics
Chapter 28 Atomic Physics Sir Joseph John Thomson J. J. Thomson 1856-1940 Discovered the electron Did extensive work with cathode ray deflections 1906 Nobel Prize for discovery of electron Early Models
More informationChapter 31 Atomic Physics
100 92 86 100 92 84 100 92 84 98 92 83 97 92 82 96 91 80 96 91 76 95 91 74 95 90 68 95 89 67 95 89 66 94 87 93 86 No. of Students in Range Exam 3 Score Distribution 25 22 20 15 10 10 5 3 2 0 0 0 0 0 0
More informationPhysics 1C Lecture 29B
Physics 1C Lecture 29B Emission Spectra! The easiest gas to analyze is hydrogen gas.! Four prominent visible lines were observed, as well as several ultraviolet lines.! In 1885, Johann Balmer, found a
More informationPhysics 1C Lecture 29A. Finish off Ch. 28 Start Ch. 29
Physics 1C Lecture 29A Finish off Ch. 28 Start Ch. 29 Particle in a Box Let s consider a particle confined to a one-dimensional region in space. Following the quantum mechanics approach, we need to find
More informationParticle Wave Duality. What is a particle? What is a wave?
Particle Wave Duality What is a particle? What is a wave? Problems with Classical Physics Nature of Light? Discrete Spectra? Blackbody Radiation? Photoelectric Effect? Compton Effect? Model of Atom? Thomas
More informationParticle 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
More informationNicholas J. Giordano. Chapter 29. Atomic Theory. Marilyn Akins, PhD Broome Community College
Nicholas J. Giordano www.cengage.com/physics/giordano Chapter 29 Atomic Theory Marilyn Akins, PhD Broome Community College Atomic Theory Matter is composed of atoms Atoms are assembled from electrons,
More informationModern Physics for Scientists and Engineers International Edition, 4th Edition
Modern Physics for Scientists and Engineers International Edition, 4th Edition http://optics.hanyang.ac.kr/~shsong Review: 1. THE BIRTH OF MODERN PHYSICS 2. SPECIAL THEORY OF RELATIVITY 3. THE EXPERIMENTAL
More informationAtom Physics. Chapter 30. DR JJ UiTM-Cutnell & Johnson 7th ed. 1. Model of an atom-the recent model. Nuclear radius r m
Chapter 30 Atom Physics DR JJ UiTM-Cutnell & Johnson 7th ed. 1 30.1 Rutherford Scattering and the Nuclear Atom Model of an atom-the recent model Nuclear radius r 10-15 m Electron s position radius r 10-10
More informationFinal Exam Tuesday, May 8, 2012 Starting at 8:30 a.m., Hoyt Hall Duration: 2h 30m
Final Exam Tuesday, May 8, 2012 Starting at 8:30 a.m., Hoyt Hall. ------------------- Duration: 2h 30m Chapter 39 Quantum Mechanics of Atoms Units of Chapter 39 39-1 Quantum-Mechanical View of Atoms 39-2
More informationElectronic structure of atoms
Chapter 1 Electronic structure of atoms light photons spectra Heisenberg s uncertainty principle atomic orbitals electron configurations the periodic table 1.1 The wave nature of light Much of our understanding
More informationTHE 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
More informationChapter 27 Early Quantum Theory and Models of the Atom Discovery and Properties of the electron
Chapter 27 Early Quantum Theory and Models of the Atom 27-1 Discovery and Properties of the electron Measure charge to mass ratio e/m (J. J. Thomson, 1897) When apply magnetic field only, the rays are
More informationChapter 7: The Quantum-Mechanical Model of the Atom
C h e m i s t r y 1 A : C h a p t e r 7 P a g e 1 Chapter 7: The Quantum-Mechanical Model of the Atom Homework: Read Chapter 7. Work out sample/practice exercises Check for the MasteringChemistry.com assignment
More informationLIGHT. 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
More informationCHAPTER 27 Quantum Physics
CHAPTER 27 Quantum Physics Units Discovery and Properties of the Electron Planck s Quantum Hypothesis; Blackbody Radiation Photon Theory of Light and the Photoelectric Effect Energy, Mass, and Momentum
More informationPhysics: Quanta to Quarks Option (99.95 ATAR)
HSC Physics Year 2016 Mark 95.00 Pages 22 Published Jan 15, 2017 Physics: Quanta to Quarks Option (99.95 ATAR) By Edward (99.95 ATAR) Powered by TCPDF (www.tcpdf.org) Your notes author, Edward. Edward
More informationAtomic Structure. Standing Waves x10 8 m/s. (or Hz or 1/s) λ Node
Atomic Structure Topics: 7.1 Electromagnetic Radiation 7.2 Planck, Einstein, Energy, and Photons 7.3 Atomic Line Spectra and Niels Bohr 7.4 The Wave Properties of the Electron 7.5 Quantum Mechanical View
More informationModels 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
More informationChapters 31 Atomic Physics
Chapters 31 Atomic Physics 1 Overview of Chapter 31 Early Models of the Atom The Spectrum of Atomic Hydrogen Bohr s Model of the Hydrogen Atom de Broglie Waves and the Bohr Model The Quantum Mechanical
More informationChapter 39. Particles Behaving as Waves
Chapter 39 Particles Behaving as Waves 39.1 Electron Waves Light has a dual nature. Light exhibits both wave and particle characteristics. Louis de Broglie postulated in 1924 that if nature is symmetric,
More informationAtomic Structure 11/21/2011
Atomic Structure Topics: 7.1 Electromagnetic Radiation 7.2 Planck, Einstein, Energy, and Photons 7.3 Atomic Line Spectra and Niels Bohr 7.4 The Wave Properties of the Electron 7.5 Quantum Mechanical View
More informationLECTURE 23 SPECTROSCOPY AND ATOMIC MODELS. Instructor: Kazumi Tolich
LECTURE 23 SPECTROSCOPY AND ATOMIC MODELS Instructor: Kazumi Tolich Lecture 23 2 29.1 Spectroscopy 29.2 Atoms The first nuclear physics experiment Using the nuclear model 29.3 Bohr s model of atomic quantization
More informationChapter 37 Early Quantum Theory and Models of the Atom. Copyright 2009 Pearson Education, Inc.
Chapter 37 Early Quantum Theory and Models of the Atom Planck s Quantum Hypothesis; Blackbody Radiation Photon Theory of Light and the Photoelectric Effect Energy, Mass, and Momentum of a Photon Compton
More informationTHE NATURE OF THE ATOM. alpha particle source
chapter THE NATURE OF THE ATOM www.tutor-homework.com (for tutoring, homework help, or help with online classes) Section 30.1 Rutherford Scattering and the Nuclear Atom 1. Which model of atomic structure
More information3. Particle nature of matter
3. Particle nature of matter 3.1 atomic nature of matter Democrit(us) 470-380 B.C.: there is only atoms and empty space, everything else is mere opinion (atoms are indivisible) Dalton (chemist) 180: chemical
More informationPreview. Atomic Physics Section 1. Section 1 Quantization of Energy. Section 2 Models of the Atom. Section 3 Quantum Mechanics
Atomic Physics Section 1 Preview Section 1 Quantization of Energy Section 2 Models of the Atom Section 3 Quantum Mechanics Atomic Physics Section 1 TEKS The student is expected to: 8A describe the photoelectric
More informationLECTURE # 19 Dennis Papadopoulos End of Classical Physics Quantization Bohr Atom Chapters 38 39
PHYS 270-SPRING 2011 LECTURE # 19 Dennis Papadopoulos End of Classical Physics Quantization Bohr Atom Chapters 38 39 April 14, 2011 1 HOW TO MEASURE SPECTRA Spectroscopy: Unlocking the Structure of Atoms
More informationEarly Quantum Theory and Models of the Atom
Early Quantum Theory and Models of the Atom Electron Discharge tube (circa 1900 s) There is something ( cathode rays ) which is emitted by the cathode and causes glowing Unlike light, these rays are deflected
More informationAtomic Structure and Atomic Spectra
Atomic Structure and Atomic Spectra Atomic Structure: Hydrogenic Atom Reading: Atkins, Ch. 10 (7 판 Ch. 13) The principles of quantum mechanics internal structure of atoms 1. Hydrogenic atom: one electron
More informationGeneral Physics (PHY 2140)
General Physics (PHY 140) Lecture 33 Modern Physics Atomic Physics Atomic spectra Bohr s theory of hydrogen http://www.physics.wayne.edu/~apetrov/phy140/ Chapter 8 1 Lightning Review Last lecture: 1. Atomic
More informationChapter 37 Early Quantum Theory and Models of the Atom
Chapter 37 Early Quantum Theory and Models of the Atom Units of Chapter 37 37-7 Wave Nature of Matter 37-8 Electron Microscopes 37-9 Early Models of the Atom 37-10 Atomic Spectra: Key to the Structure
More informationQuantum and Atomic Physics - Multiple Choice
PSI AP Physics 2 Name 1. The Cathode Ray Tube experiment is associated with: (A) J. J. Thomson (B) J. S. Townsend (C) M. Plank (D) A. H. Compton 2. The electron charge was measured the first time in: (A)
More informationProfessor K. Atomic structure
Professor K Atomic structure Review Reaction- the formation and breaking of chemical bonds Bond- a transfer or sharing of electrons Electrons Abbreviated e - What are they? How were they discovered? Early
More informationHistorical Background of Quantum Mechanics
Historical Background of Quantum Mechanics The Nature of Light The Structure of Matter Dr. Sabry El-Taher 1 The Nature of Light Dr. Sabry El-Taher 2 In 1801 Thomas Young: gave experimental evidence for
More informationEinstein. Quantum Physics at a glance. Planck s Hypothesis (blackbody radiation) (ultraviolet catastrophe) Quantized Energy
Quantum Physics at a glance Quantum Physics deals with the study of light and particles at atomic and smaller levels. Planck s Hypothesis (blackbody radiation) (ultraviolet catastrophe) Quantized Energy
More informationChapter 9: Electrons and the Periodic Table
C h e m i s t r y 1 2 C h 9 : E l e c t r o n s a n d P e r i o d i c T a b l e P a g e 1 Chapter 9: Electrons and the Periodic Table Work on MasteringChemistry assignments What we have learned: Dalton
More informationChapter 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
More informationThe Hydrogen Atom. Dr. Sabry El-Taher 1. e 4. U U r
The Hydrogen Atom Atom is a 3D object, and the electron motion is three-dimensional. We ll start with the simplest case - The hydrogen atom. An electron and a proton (nucleus) are bound by the central-symmetric
More informationComplete nomenclature for electron orbitals
Complete nomenclature for electron orbitals Bohr s model worked but it lacked a satisfactory reason why. De Broglie suggested that all particles have a wave nature. u l=h/p Enter de Broglie again It was
More informationStellar Astrophysics: The Interaction of Light and Matter
Stellar Astrophysics: The Interaction of Light and Matter The Photoelectric Effect Methods of electron emission Thermionic emission: Application of heat allows electrons to gain enough energy to escape
More informationThe Photoelectric Effect
The Photoelectric Effect Light can strike the surface of some metals causing an electron to be ejected No matter how brightly the light shines, electrons are ejected only if the light has sufficient energy
More informationChapter 5 Light and Matter
Chapter 5 Light and Matter Stars and galaxies are too far for us to send a spacecraft or to visit (in our lifetimes). All we can receive from them is light But there is much we can learn (composition,
More informationChapter 6 - Electronic Structure of Atoms
Chapter 6 - Electronic Structure of Atoms 6.1 The Wave Nature of Light To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation Visible light is an example
More informationThe Hydrogen Atom According to Bohr
The Hydrogen Atom According to Bohr The atom We ve already talked about how tiny systems behave in strange ways. Now let s s talk about how a more complicated system behaves. The atom! Physics 9 4 Early
More informationSpectroscopy. Hot self-luminous objects light the Sun or a light bulb emit a continuous spectrum of wavelengths.
Hot self-luminous objects light the Sun or a light bulb emit a continuous spectrum of wavelengths. In contract, light emitted in low=pressure gas discharge contains only discrete individual wavelengths,
More informationis the minimum stopping potential for which the current between the plates reduces to zero.
Module 1 :Quantum Mechanics Chapter 2 : Introduction to Quantum ideas Introduction to Quantum ideas We will now consider some experiments and their implications, which introduce us to quantum ideas. The
More informationChapter 6 Electronic structure of atoms
Chapter 6 Electronic structure of atoms light photons spectra Heisenberg s uncertainty principle atomic orbitals electron configurations the periodic table 6.1 The wave nature of light Visible light is
More informationChapter 6 Electronic Structure of Atoms. 許富銀 ( Hsu Fu-Yin)
Chapter 6 Electronic Structure of Atoms 許富銀 ( Hsu Fu-Yin) 1 The Wave Nature of Light The light we see with our eyes, visible light, is one type of electromagnetic radiation. electromagnetic radiation carries
More informationPlanck s Quantum Hypothesis Blackbody Radiation
Planck s Quantum Hypothesis Blackbody Radiation The spectrum of blackbody radiation has been measured(next slide); it is found that the frequency of peak intensity increases linearly with temperature.
More informationAtomic Structure and the Periodic Table
Atomic Structure and the Periodic Table The electronic structure of an atom determines its characteristics Studying atoms by analyzing light emissions/absorptions Spectroscopy: analysis of light emitted
More informationChapter 27 Lecture Notes
Chapter 27 Lecture Notes Physics 2424 - Strauss Formulas: λ P T = 2.80 10-3 m K E = nhf = nhc/λ fλ = c hf = K max + W 0 λ = h/p λ - λ = (h/mc)(1 - cosθ) 1/λ = R(1/n 2 f - 1/n 2 i ) Lyman Series n f = 1,
More informationATOMIC MODELS. Models are formulated to fit the available data. Atom was known to have certain size. Atom was known to be neutral.
ATOMIC MODELS Models are formulated to fit the available data. 1900 Atom was known to have certain size. Atom was known to be neutral. Atom was known to give off electrons. THOMPSON MODEL To satisfy the
More informationThe Nature of Light. Chapter Five
The Nature of Light Chapter Five Guiding Questions 1. How fast does light travel? How can this speed be measured? 2. Why do we think light is a wave? What kind of wave is it? 3. How is the light from an
More informationCHAPTER 5 ATOMIC STRUCTURE SHORT QUESTIONS AND ANSWERS Q.1 Why it is necessary to decrease the pressure in the discharge tube to get the cathode rays? The current does not flow through the gas at ordinary
More informationPhysics 116. Nov 22, Session 32 Models of atoms. R. J. Wilkes
Physics 116 Session 32 Models of atoms Nov 22, 2011 Thomson Rutherford R. J. Wilkes Email: ph116@u.washington.edu Announcements Exam 3 next week (Tuesday, 11/29) Usual format and procedures I ll post example
More informationAtomic Structure Discovered. Dalton s Atomic Theory. Discovery of the Electron 10/30/2012
Atomic Structure Discovered Ancient Greeks Democritus (460-362 BC) - indivisible particles called atoms Prevailing argument (Plato and Aristotle) - matter is continuously and infinitely divisible John
More informationUNIT : QUANTUM THEORY AND THE ATOM
Name St.No. Date(YY/MM/DD) / / Section UNIT 102-10: QUANTUM THEORY AND THE ATOM OBJECTIVES Atomic Spectra for Hydrogen, Mercury and Neon. 1. To observe various atomic spectra with a diffraction grating
More informationPhysics 1C. Lecture 28D
Physics 1C Lecture 28D "I ask you to look both ways. For the road to a knowledge of the stars leads through the atom; and important knowledge of the atom has been reached through the stars." --Sir Arthur
More informationFinal Exam: Thursday 05/02 7:00 9:00 pm in STEW 183
Final Exam: Thursday 05/02 7:00 9:00 pm in STEW 183 Covers all readings, lectures, homework from Chapters 17 through 30 Be sure to bring your student ID card, calculator, pencil, and up to three onepage
More informationCHEMISTRY Topic #1: Atomic Structure and Nuclear Chemistry Fall 2017 Dr. Susan Findlay See Exercises 3.1 to 3.3
CHEMISTRY 1000 Topic #1: Atomic Structure and Nuclear Chemistry Fall 2017 Dr. Susan Findlay See Exercises 3.1 to 3.3 Light: Wave? Particle? Both! Modern models of the atom were derived by studying the
More informationAtomic Spectra. What does this have to do with atomic models?
Atomic Physics -2 Atomic Spectra Fill a glass tube with pure atomic gas Apply a high voltage between electrodes Current flows through gas & tube glows Color depends on type of gas Light emitted is composed
More informationThe Atom. Result for Hydrogen. For example: the emission spectrum of Hydrogen: Screen. light. Hydrogen gas. Diffraction grating (or prism)
The Atom What was know about the atom in 1900? First, the existence of atoms was not universally accepted at this time, but for those who did think atoms existed, they knew: 1. Atoms are small, but they
More informationSECTION A Quantum Physics and Atom Models
AP Physics Multiple Choice Practice Modern Physics SECTION A Quantum Physics and Atom Models 1. Light of a single frequency falls on a photoelectric material but no electrons are emitted. Electrons may
More informationLecture PowerPoints. Chapter 27 Physics: Principles with Applications, 7th edition Giancoli
Lecture PowerPoints Chapter 27 Physics: Principles with Applications, 7th edition Giancoli This work is protected by United States copyright laws and is provided solely for the use of instructors in teaching
More informationParticle and Nuclear Physics. Outline. Structure of the Atom. History of Atomic Structure. 1 Structure of the Atom
Outline of 1 of Atomic Spectra of Helium Classical Atom of Existence of spectral lines required new model of atom, so that only certain amounts of energy could be emitted or absorbed. By about 1890, most
More informationAP Chemistry. Chapter 6 Electronic Structure of Atoms
AP Chemistry Chapter 6 Electronic Structure of Atoms Section 6.1 Wave Nature of Light When we say "light," we generally are referring to visible light a type of electromagnetic radiation But actually Visible
More informationChapter 1. From Classical to Quantum Mechanics
Chapter 1. From Classical to Quantum Mechanics Classical Mechanics (Newton): It describes the motion of a classical particle (discrete object). dp F ma, p = m = dt dx m dt F: force (N) a: acceleration
More information1 The Cathode Rays experiment is associated. with: Millikan A B. Thomson. Townsend. Plank Compton
1 The Cathode Rays experiment is associated with: A B C D E Millikan Thomson Townsend Plank Compton 1 2 The electron charge was measured the first time in: A B C D E Cathode ray experiment Photoelectric
More informationAtomic Structure and Periodicity
p. 99 p. 98 p. 98 Electromagnetic Spectrum Image Atomic Structure and Periodicity Chemistry Zumdahl Chapter 7 Properties of Light Electromagnetic Radiation: a form of energy that exhibits wavelike behavior
More informationPHY293 Lecture #15. November 27, Quantum Mechanics and the Atom
PHY293 Lecture #15 November 27, 2017 1. Quantum Mechanics and the Atom The Thompson/Plum Pudding Model Thompson discovered the electron in 1894 (Nobel Prize in 1906) Heating materials (metals) causes corpuscles
More informationReview Models of the Atom
Review Models of the Atom Copyright 2007 Pearson Benjamin Cummings. All rights reserved. Dalton proposes the indivisible unit of an element is the atom. Thomson discovers electrons, believed to reside
More informationLIGHT AND THE QUANTUM MODEL
LIGHT AND THE QUANTUM MODEL WAVES Wavelength ( ) - length of one complete wave Frequency ( ) - # of waves that pass a point during a certain time period hertz (Hz) = 1/s Amplitude (A) - distance from the
More informationChapter 6 Electronic Structure of Atoms
Chapter 6 Electronic Structure of Atoms What is the origin of color in matter? Demo: flame tests What does this have to do with the atom? Why are atomic properties periodic? 6.1 The Wave Nature of Light
More informationChemistry 111 Dr. Kevin Moore
Chemistry 111 Dr. Kevin Moore Black Body Radiation Heated objects emit radiation based on its temperature Higher temperatures produce higher frequencies PhotoElectric Effect Light on a clean metal surface
More informationChapter 5. The Electromagnetic Spectrum. What is visible light? What is visible light? Which of the following would you consider dangerous?
Which of the following would you consider dangerous? X-rays Radio waves Gamma rays UV radiation Visible light Microwaves Infrared radiation Chapter 5 Periodicity and Atomic Structure 2 The Electromagnetic
More informationExplain the term subshell. 5. Explain de-broglie equation (relationship). 6. Discuss the dual nature of electrons
MODEL COLLEGE ASSIGNMENT SHEET FOR STRUCTURE OF ATOM. What are the main postulates of Bohr s theory of an atom?. Explain how the angular momentum of an electron in an atom is quantized? 3. What are the
More informationEnergy levels and atomic structures lectures chapter one
Structure of Atom An atom is the smallest constituent unit of ordinary matter that has the properties of a element. Every solid, liquid, gas, and plasma is composed of neutral or ionized atoms. Atoms are
More informationEarlier we learned that hot, opaque objects produce continuous spectra of radiation of different wavelengths.
Section7: The Bohr Atom Earlier we learned that hot, opaque objects produce continuous spectra of radiation of different wavelengths. Continuous Spectrum Everyone has seen the spectrum produced when white
More informationPHYS 3313 Section 001 Lecture #14
PHYS 3313 Section 001 Lecture #14 Monday, March 6, 2017 The Classic Atomic Model Bohr Radius Bohr s Hydrogen Model and Its Limitations Characteristic X-ray Spectra 1 Announcements Midterm Exam In class
More informationAtomic Structure. Chapter 8
Atomic Structure Chapter 8 Overview To understand atomic structure requires understanding a special aspect of the electron - spin and its related magnetism - and properties of a collection of identical
More informationATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY All matter is made of atoms. There are a limited number of types of atoms; these are the elements. (EU 1.A) Development of Atomic Theory Atoms are so small
More informationAstronomy The Nature of Light
Astronomy The Nature of Light A. Dayle Hancock adhancock@wm.edu Small 239 Office hours: MTWR 10-11am Measuring the speed of light Light is an electromagnetic wave The relationship between Light and temperature
More informationOutline Chapter 9 The Atom Photons Photons The Photoelectron Effect Photons Photons
Outline Chapter 9 The Atom 9-1. Photoelectric Effect 9-3. What Is Light? 9-4. X-rays 9-5. De Broglie Waves 9-6. Waves of What? 9-7. Uncertainty Principle 9-8. Atomic Spectra 9-9. The Bohr Model 9-10. Electron
More informationUNIT 4 Electrons in Atoms. Advanced Chemistry 235 Lanphier High School Mr. David Peeler
UNIT 4 Electrons in Atoms Advanced Chemistry 235 Lanphier High School Mr. David Peeler Section 4.1 Models of the Atom OBJECTIVES: Identify the inadequacies in the Rutherford atomic model. Section 4.1 Models
More informationTopics Covered in Chapter. Light and Other Electromagnetic Radiation. A Subatomic Interlude II. A Subatomic Interlude. A Subatomic Interlude III
Light and Other Electromagnetic Radiation Topics Covered in Chapter 1.Structure of Atoms 2.Origins of Electromagnetic Radiation 3.Objects with Different Temperature and their Electromagnetic Radiation
More informationLight and Other Electromagnetic Radiation
Light and Other Electromagnetic Radiation 1 Topics Covered in Chapter 1.Structure of Atoms 2.Origins of Electromagnetic Radiation 3.Objects with Different Temperature and their Electromagnetic Radiation
More informationProblems with the atomic model?
Modern Atomic Theory- Electronic Structure of Atoms DR HNIMIR-CH7 Where should (-) electrons be found? Problems with the atomic model? First, a Little About Electromagnetic Radiation- Waves Another Look
More informationFrom Last Time Pearson Education, Inc.
From Last Time Light: Absorption, Emission, Transmission, Reflection, and Scattering c=λ x f E=h x f Light (electromagnetic radiation) extends from gamma rays (high E, high f, small λ) to radio waves (small
More informationHistory of the Atomic Model
Chapter 5 Lecture Chapter 5 Electronic Structure and Periodic Trends 5.1 Electromagnetic Radiation Learning Goal Compare the wavelength, frequency, and energy of electromagnetic radiation. Fifth Edition
More informationThe Quantum Mechanical Atom
The Quantum Mechanical Atom CHAPTER 7 Chemistry: The Molecular Nature of Matter, 6 th edition By Jesperson, Brady, & Hyslop CHAPTER 8: Quantum Mechanical Atom Learning Objectives q Light as Waves, Wavelength
More informationAccounts for certain objects being colored. Used in medicine (examples?) Allows us to learn about structure of the atom
1.1 Interaction of Light and Matter Accounts for certain objects being colored Used in medicine (examples?) 1.2 Wavelike Properties of Light Wavelength, : peak to peak distance Amplitude: height of the
More informationAIIMS,CBSE,AIPMT, AFMC,Bio.Tech & PMT, Contact : , Mail at :- by AKB
1 Splitting of spectral lines when atoms are subjected to strong electric field is called (a) Zeeman effect (b) Stark effect (c) Photoelectric effect (d) Compton effect 2 The velocity of photon is (a)
More informationChapter 9. Blimps, Balloons, and Models for the Atom. Electrons in Atoms and the Periodic Table. Hindenburg. Properties of Elements Hydrogen Atoms
Chapter 9 Electrons in Atoms and the Periodic Table Blimps, Balloons, and Models for the Atom Hindenburg Blimps, Balloons, and Models for the Atom Properties of Elements Hydrogen Atoms Helium Atoms 1 Blimps,
More informationQuantum Mechanics & Atomic Structure (Chapter 11)
Quantum Mechanics & Atomic Structure (Chapter 11) Quantum mechanics: Microscopic theory of light & matter at molecular scale and smaller. Atoms and radiation (light) have both wave-like and particlelike
More informationQuantum theory and models of the atom
Guess now. It has been found experimentally that: (a) light behaves as a wave; (b) light behaves as a particle; (c) electrons behave as particles; (d) electrons behave as waves; (e) all of the above are
More informationDifferent energy levels
Different energy levels In the microscopic world energy is discrete www.cgrahamphysics.com Review Atomic electrons can only exist in certain discrete energy levels Light is made of photons When e s lose
More information