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Atomic Physics.

Published by Laura Heath Modified over 9 years ago

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Presentation on theme: "Atomic Physics."— Presentation transcript:

History of the Atom.

Atomic Theory.

Models of the Atom a Historical Perspective

Atomic Theories Democritus (300 B. C.)

THE ROAD TO THE ATOM.

Dual Nature of Light. Light Quanta. Photoelectric Effect.

Atomic Theory and the Atom

The Structure of the Atom And Electrons in Atoms

Atomic Structure Objectives: History of an Atom Atomic Models

Chemistry Sheds Light on Our Lives Unit 4 Atoms and Light

SCH4U watch?v=-d23GS56HjQ G de 12 Cmistr Ra He Y Y.

Structure of Matter Structure of Matter Structure of Matter History of the Atom.

Atomic Theory and Structure Chapters 4-5 Atomic Theories Democritus ~ 400 BC believed that atoms were indivisible and indestructible Dalton ~ 1800’s.

Atomic Structure. Way Early Theories Democritus ( BC) –First person to propose that matter is not infinitely divisible –Atomos –Matter is empty.

Development of Atomic Theory 400 B.C. -Democritus was first to use the word : atom atomos meaning “indivisible” Aristotle (famous philosopher) disputed.

Matter Unit Learning Goal #2: Summarize the major experimental evidence that led to the development of various models, both historic and current.

II. History of atomic structure A. Democritus – 500 BCE Theorized that matter is composed of small, indivisible particles = ATOMOS (Greek for indivisible)

HISTORY OF THE ATOM. Aristotle 400 BC 400 BC - Claimed that there was no smallest part of matter - Claimed that there was no smallest part of matter -

Lecture 23 Models of the Atom Chapter 28.1  28.4 Outline The Thomson and Rutherford Models Atomic Spectra The Bohr Model.

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Atomic Structure PowerPoint Templates & Google Slides Themes

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This slide mentions key advantages obtained by using atomic swap technique to achieve blockchain interoperability. It includes decentralized nature, enhanced security, interoperability, reduced counterparty risk and privacy. Slidegeeks has constructed Understanding Various Blockchain Key Benefits Of Atomic Swap Technology BCT SS V after conducting extensive research and examination. These presentation templates are constantly being generated and modified based on user preferences and critiques from editors. Here, you will find the most attractive templates for a range of purposes while taking into account ratings and remarks from users regarding the content. This is an excellent jumping-off point to explore our content and will give new users an insight into our top-notch PowerPoint Templates.

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Atom Shapes for PowerPoint

Atom Shapes for PowerPoint – Atoms are the smallest unit particles of matter. The name is derived from the Greek word “atomos” meaning uncuttable. John Dalton initially discovered the particle concept that is present within chemicals. Create amazing and comprehensive atomic structure presentations using Atom Shapes for PowerPoint.

The PowerPoint template is ideal with atomic research and science reporting projects. The slide designs can supplement broader presentations. They are perfect for chemistry and physics subject matters. Some specific topics that can find Atom Shapes for PowerPoint useful are electromagnetic force, elements, chemical bonding, nuclear fission and fusion, matter and quantum physics.

In the first slide, the user can see the atomic model with the axis of all its parts. There are 4 spheres orbiting the larger sphere in the center. The sphere in the center can represent the nucleus which is actually composed of the proton and neutron. The outer spheres can refer to electrons. In the second slide, the same model is shown together with corresponding text placeholders. The presenter can provide a brief description for every part. The 3rd slide features Neils Bohr’s model of an atom where the axes are displayed in flat circles. The fourth and fifth slides illustrate pictures that highlight each atomic part through color filter. The remaining slides are replicas of the 2nd-4th slides, exhibited in black background.

An atom is the base of quantum physics where its behaviour and detailed accounts of its existence are developed. The parts of an atom are the neutrons, protons and electrons. The neutrons (no charge) and protons (positively charged) are attached together, forming a nucleus or a center. The electrons (negatively charged) are found around the nucleus in an orbiting manner.

Catchy and professional, Atom Shapes for PowerPoint can capture global audiences. 3 D Core Diagram for PowerPoint  is a further molecular and atomic model downloadable from the SlideModel gallery.

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Atomic Physics - PowerPoint PPT Presentation

Atomic Physics

Atomic physics quantization of energy atomic models quantum mechanics matter waves frequency of matter waves can be found with planck s equation evidence for matter ... – powerpoint ppt presentation.

• Quantization of Energy
• Atomic Models
• Quantum Mechanics
• A changing magnetic field can induce a current in a circuit (Faradays Law of Induction)
• A magnetic field is created around a current-carrying wire (Amperes Law)
• Electric field lines start on positive charges and end at negative charges (Coulombs Law / Gausss Law)
• Magnetic field lines always form closed loops with no beginning and no end (Gausss Law for magnetism)
• These unrelated observations, experiments and equations were all known by the mid-1800s, but nothing linked them together.
• James Clerk Maxwell (1831-1879)
• Scottish theoretical physicist mathematician
• Maxwells Equations
• Set of differential equations that describe the relationship between electric and magnetic field
• Summarized all previous work of Coulomb, Ampere, Gauss, Faraday others
• a changing magnetic field would create a changing electric field, which would, in turn, create a changing magnetic field, and so on
• existence of electromagnetic waves that move through space at the speed of light
• light is an electromagnetic wave
• Heinrich Hertz in 1887
• generated and detected the first E/M waves
• Oscillating electric and magnetic fields
• E-field and B-field are at right angles to each other
• Propagates at a right angle to both fields (transverse wave)
• EM waves can be produced most easily by an oscillating charged particle
• Frequency of oscillation determines frequency of the EM wave
• Wavelength related to frequency by
• Energy is the ability to do work
• E-fields B-fields store energy because they exert a force (do work) on charged particles
• Electromagnetic Radiation
• transfer of energy associated with electric and magnetic fields
• can be transferred to objects in the EM waves path
• can be converted to other forms, such as heat
• Continuous distribution of wavelengths on the electromagnetic spectrum.
• All objects emit electromagnetic radiation
• Continuous distribution of wavelengths from the infrared, visible, and UV portions of the EM spectrum
• Intensity distribution of different wavelengths varies with temperature
• At low temps mostly infrared (invisible)
• Temp increases distribution shifts to visible UV
• Metals glow red gt yellow gt white gt blue
• Most objects absorb some incoming radiation and reflect the rest
• Ideal system that absorbs all incoming radiation
• Hollow object with a small opening
• Perfect absorber and perfect radiator
• Emits radiation based only on its temperature
• In 1900, Max Planck (1858-1947), proposed that the walls of a blackbody contained billions of submicroscopic electric oscillators, which he called resonators. These resonators, produced the blackbody radiation.
• Planck found that the total energy of a resonator is an integer multiple of the frequency
• Because the energy of each resonator comes in discrete units, it is said to be quantized.
• Allowed energy states are called quantum states or energy levels.
• Einstein applied the concept of quantized energy to light.
• Photon quantized unit of light energy
• Photons are absorbed or given off by electrons jumping from one quantum state to another.
• Classical physics predicts
• Light waves of any frequency should have enough energy to eject electrons if the intensity is high enough
• At low intensities, electrons should be ejected if light shines on the metal for a long enough period of time
• Increasing the intensity of the light waves should increase the kinetic energy of the photoelectrons.
• Maximum kinetic energy of a photoelectron should be determined by the lights intensity
• Experimental evidence shows that
• No photoelectrons emitted if the light frequency falls below a certain threshold frequency, even if the intensity is very high
• Threshold frequency, ft, depends on material
• If light frequency exceeds ft
• of photoelectrons emitted is proportional to light intensity
• Maximum kinetic energy of photoelectrons is proportional to the frequency and is independent of the intensity
• Electrons are emitted instantaneously, even at low intensities
• Classical physics could not explain the photoelectric effect but Einstein could!
• EM waves are quantized
• Think of light as a stream of particles, called photons
• Photon energy given by Plancks equation
• When photons collide with electrons in metal, they transfer energy to electrons
• If photon energy is greater than work function of the metal, photoelectrons are ejected
• If photon has more energy than the work function, the difference is the kinetic energy of the photoelectrons ejected from the surface
• American physicist Arthur Compton (1892-1962) proposed that momentum energy should be conserved in a collision between photons electrons
• After a collision, scattered photon should have a lower energy, therefore a lower frequency (longer wavelength)
• In 1923, conducted experiments with X rays to demonstrate this change in wavelength, known as Compton shift.
• Thomson Model / Plum Pudding Model
• Discovery of electron in 1897
• Negative electrons in sphere of positive charge
• Rutherford Model / Planetary Model
• 1911 experiment by Geiger Marsden demonstrated that practically all of atoms mass and all positive charge must be centrally located in atom (nucleus)
• Electrons orbit nucleus like planets around Sun
• Electrons orbiting the nucleus would undergo centripetal acceleration
• Accelerating electrons would radiate EM waves
• Electrons radiating EM waves would lose energy
• Loss of energy would cause electrons orbital radius to drop
• Frequency of emitted radiation would increase
• Electrons would rapidly collapse into nucleus
• Need a better model!
• 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 of only certain wavelengths
• Emission Spectrum diagram or graph that indicates the wavelengths of radiant energy that a substance emits (bright lines)
• Absorption Spectrum same thing, just for light absorbed by a substance (dark lines)
• What does this have to do with atomic models?
• Similar to Rutherfords model, but only allows certain, discrete orbits
• Electrons are never found between orbits, but can jump from one orbit to another
• Electrons only emit radiation when they jump from an outer orbit to an inner one
• Energy of emitted photon is equal to energy decrease of electron. This determines frequency of emitted radiation.
• Energy of emitted photon is quantized only certain quantities are allowed. Hence, electrons undergo quantum leaps. (Obligatory pop culture reference)
• Lowest energy state ground state
• Radius of this state Bohr radius
• Electrons usually here at ordinary temps
• How do electrons jump between states?
• Absorb photon with energy (hf) exactly equal to energy difference between ground state excited state
• Absorbed photons account for dark lines in absorption spectrum
• Spontaneous emission
• Electron in excited state jumps back to a lower energy level by emitting a photon
• Does NOT need to jump all the way back to the ground state
• Emitted photon has energy equal to energy difference between levels
• Accounts for bright lines on emission spectrum
• Jumps between different energy levels correspond to various spectral lines
• Account for wavelengths of all spectral lines of hydrogen
• Provides explanation for auroras
• Gave expression for radius of hydrogen atom
• Predicted energy levels of hydrogen
• Also successful when applied to hydrogen-like atoms (only one electron)
• Unsuccessful when applied to multi-electron atoms
• Did not explain why electrons do not radiate energy when in a stable orbit
• Did not explain why other orbits do not occur
• Combined classical and non-classical physics
• Is light a particle or a wave?
• Particle blackbody radiation, photoelectric effect
• Wave interference, diffraction
• Which model is correct?
• Both are correct, but depends on the situation
• Each phenomenon exhibits only one or the other natures of light
• True nature of light is not describable in terms of a single classical idea
• Low Frequency Light
• (Wave Nature)
• High Frequency Light
• (Photon Nature)
• Very low energy
• Difficult to detect a single photon
• Photon nature of light not evident
• Long wavelength
• Wave effects, like diffraction and interference are easy to observe
• Very high energy
• Easy to detect single photons
• Photon nature of light is evident
• Short wavelength
• Wave effects, like diffraction and interference are more difficult to observe
• Since light can be described as either a particle or a wave, can we do the same for all objects, like atoms and people and cars?
• Louis de Broglie thought so!
• In 1924, proposed that all matter may have wave properties and particle properties
• Matter has a dual nature, just like light!
• Proposed idea of matter waves
• The larger the momentum of an object, the smaller its wavelength
• Frequency of matter waves can be found with Plancks equation
• 1927 Davisson Germer, showed that electrons can be diffracted by a single crystal of nickel
• Electron diffraction is possible because the de Broglie wavelength of an electron is approx. equal to distance between atoms (the size of the diffraction grating)
• Large-scale objects dont demonstrate this well because large momentum generates wavelengths much smaller than any possible aperture through which the object could pass (wont be diffracted)
• De Broglie hypothesized that only certain electron orbits are stable
• Circumference of orbit must contain an integral multiple of electron wavelengths
• Similar to standing waves on a string
• Wave nature of particles restricts the precision of our measurements
• Werner Heisenberg (1927)
• It is fundamentally impossible to make simultaneous measurements of a particles position and momentum with infinite accuracy
• The more we learn about a particles momentum, the less we know of its position, and vice versa.
• Imagine trying to measure an electrons position and momentum with a powerful microscope
• In order to see the electron, thereby determining its location, at least one photon of light must bounce off the electron and pass through the microscope to your eye
• When the photon strikes the electron, it transfers some energy momentum to the electron. So we are less sure of the electrons momentum.
• Erwin Schrodinger (1926) proposed a wave equation for de Broglies matter waves
• Each particle can be represented by a wave function , ?, dependent on the position of the particle and time
• Max Born (1926) interpreted Schrodingers wave function to show probability of finding an electron at certain locations
• ?2 is proportional to probability of finding the electron at a certain position
• Peak probability for an electron in the ground state corresponds to Bohr radius
• Electrons are not confined to particular orbital distances as assumed in Bohr model
• Electron cloud a probability cloud
• Density at each location related to probability of finding electron at that location
• Wave function predicts geometry for energy levels (some spherical, others more complex)
• Most probable location still corresponds to Bohr radii, but impossible to determine actual location
• Mathematical picture of the atom that explains certain aspects of atomic structure that Bohr model cannot explain

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Atomic Physics and Lasers

Mar 16, 2019

4.34k likes | 4.68k Views

Atomic Physics and Lasers. The idea of a photon Black body radiation Photoelectric Effect The structure of the atom How does a Laser work? Interaction of lasers with matter Laser safety Applications Spectroscopy, detection of art forgery, flow cytometry, eye surgery.

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Presentation Transcript

Atomic Physics and Lasers • The idea of a photon • Black body radiation • Photoelectric Effect • The structure of the atom • How does a Laser work? Interaction of lasers with matter • Laser safety • Applications • Spectroscopy, detection of art forgery, flow cytometry, eye surgery.

The idea of a photon • What is light? • A wave? • Well yes, but…. • The wave picture failed to explain physical phenomena including : • the spectrum of a blackbody • the photoelectric effect • line spectra emitted by atoms

Light from a hot object... Vibrational motion of particles produces light(we call the light “Thermal Radiation”)

The first clue that something was very, very wrong…Blackbody radiation • What is a blackbody? • An object which emits or absorbs all the radiation incident on it. • Typical black bodies • A light globe • A box with a small hole in it.

Example of a Blackbody A BLACKBODY

Example of a Blackbody We measure radiation as a function of frequency (wavelength)

A Thermal Spectrum How does a thermal spectrum change when you change T?

Thermal Radiation T= Temp. in Kelvin Total energy emitted by an object (or Luminosity W/m2) Wavelength where flux is a maximum s = 5.7 x 10-8 W/(m2.K4) k = 2.898 x 10-3 m.K Stefan’s Law Wien’s Law

Matter at some temperature T Oscillators Light and matter interact • The spectra we have looked at are for ideal objects that are perfect absorbers and emitters of light Light is later emitted Light is perfectly absorbed A BLACKBODY

Not so good here F l u x Okay here l F l u x Problems with wave theory of light • Take a Blackbody witha temperature, T • Calculate how the spectrum would look if light behaved like a wave (Lord Rayleigh) • Compare with what isactually observed

Max Plank Solved the problem in 1900 • Oscillators cannot have any energy! They can be in states with fixed amounts of energy. • The oscillators change state by emitting/absorbingpackets with a fixed amounts of energy Max Plank

Atomic Physics/Blackbody • Max Planck (1858-1947) was impressed by the fact • spectrum of a black body was a universal property. E =nhf • To get agreement between the experiment and the theory, Planck proposed a radical idea: Light comes in packets of energy called photons, and the energy is given by E= nhf The birth of the quantum theory = Planck’s hypothesis

The birth of the Photon • In 1906, Einstein proved that Planck’s radiation law could be derived only if the energy of each oscillator is quantized. En = nhf ; n = 0, 1, 2, 3, 4,... h=Planck’s constant= 6.626x10 -34 J.s f=frequency in Hz; E=energy in Joules (J). • Einstein introduced the idea that radiation • equals a collection of discrete energy quanta. • G.N. Lewis in 1926 named quanta “Photons”.

Atomic Physics/Photon • The energy of each photon: E = hf h=Planck’s constant f=frequency Ex. 1. Yellow light has a frequency of 6.0 x 1014 Hz. Determine the energy carried by a quantum of this light. If the energy flux of sunlight reaching the earth’s surface is 1000 Watts per square meter, find the number of photons in sunlight that reach the earth’s surface per square meter per second. Ans. 2.5 eV and 2.5 x 10 21 photons / m 2 /s

Shining light onto metals Light in Nothing happens METAL

Different Energy Light in electrons come out Shining light onto metals METAL

The Photoelectric Effect • When light is incident on certain metallic surfaces, electrons are emitted = the Photoelectric Effect(Serway and Jewett 28.2) • Einstein: A single photon gives up all its energy to a single electron EPhoton =EFree + EKinetic Need at least this much energy to free the electron Whatever is left makes it move

Kinetic Energy of electron Different metals Frequency of Light fo Threshold frequency The Photoelectric Effect

Metal plate Application of Photoelectric Effect Soundtrack on Celluloid film To speaker

Another Blow for classical physics: Line Spectra • The emission spectrum from a rarefied gas through which an electrical discharge passes consists of sharp spectral lines. • Each atom has its own characteristic spectrum. • Hydrogen has four spectral lines in the visible region and many UV and IR lines not visible to the human eye. • The wave picture failed to explain these lines.

Atomic Physics/Line spectra 400 500 600 (nm) H Emission spectrum for hydrogen The absorption spectrum for hydrogen; dark absorption lines occur at the same wavelengths as emission lines.

-0.85 n=4 -1.51 n=3 Paschen IR n=2 -3.39 Balmer Visible R =Rydberg Constant = 1.09737x10 7m-1 -13.6 1 1 1 R ( nm2 n=1 Lyman UV ) Atomic Physics/Line Spectra

So what is light? • Both a wave and a particle. It can be both, but in any experiment only its wave or its particle nature is manifested. (Go figure!)

Two revolutions: The Nature of light and the nature of matter • Light has both a particle and wave nature: • Wave nature: • Diffraction, interference • Particle nature • Black body radiation, photoelectric effect, line spectra • Need to revise the nature of matter (it turns out that matter also has both a particle and wave nature

The spectrum from a blackbody • Empirically: • (max)T = constant, • Hotter = whiter • The wave picture (Rayleigh-Jeans) failed to explain the distribution of the energy versus wavelength. UV Catastrophe!!!! 6000K Rayleigh- Jeans Relative Intensity Observed 5000K 0 2 4 6 8 10  (10 -7 m)

Photoelectric Effect Light in e Electron out METAL

The Photoelectric Effect • Photoelectric effect=When light is incident on certain metallic surfaces, photoelectrons are emitted. • Einstein applied the idea of light quanta: In a photoemission process, a single photon gives up all its energy to a single electron. Energy of photon Energy to free electron = + KE of emitted electron

Atomic Physics/Photoelectric Effect =work function; minimum energy needed to extract an electron. hf = KE +  KE x fo = threshold freq below which no photoemission occurs. x x x f0 f, Hz

Atomic Physics/The Photoelectric Effect-Application The sound on a movie film Sound Track Phototube Light Source speaker

The photoelectric effect • Photoelectric effect=When light is incident on certain metallic surfaces, photoelectrons are emitted. • Einstein applied the idea of light quanta: In a photoemission process, a single photon gives up all its energy to a single electron. Energy to free electron Energy of photon KE of emitted electron = +

The Photoelectric Effect experiment Metal surfaces in a vacuum eject electrons when irradiated by UV light.

PE effect:5 Experimental observations • If V is kept constant, the photoelectric current ip increases with increasing UV intensity. • Photoelectrons are emitted less than 1 nS after surface illumination • For a given surface material, electrons are emitted only if the incident radiation is at or above a certain frequency, independent of intensity. • The maximum kinetic energy, Kmax, of thephotoelectrons is independent of the light intensity I. • The maximum kinetic energy, Kmax of the photoelectrons depends on the frequency of the incident radiation.

Failure of Classcial Theory Observation 1: is in perfect agreement with classical expectations Observation 2: Cannot explain this. Very weak intensity should take longer to accumulate energy to eject electrons Observation 3: Cannot explain this either. Classically no relation between frequency and energy. Observations 4 and 5: Cannot be explained at all by classical E/M waves. . Bottom line: Classical explanation fails badly.

Quantum Explanation. • Einstein expanded Planck’s hypothesis and applied it directly to EM radiation • EM radiation consists of bundles of energy (photons) • These photons have energy E = hf • If an electron absorbs a photon of energy E = hf in order to escape the surface it uses up energy φ,called the work function of the metal • φis the binding energy of the electron to the surface • This satisfies all 5 experimental observations .

Photoelectric effect • hf = KE + φ • ( φ=work function; minimum energy needed to extract an electron.) • fo = threshold freq, below which no photoemission occurs KE x . x x x f0 f (Hz)

Application: Film soundtracks Sound Track Phototube Light Source speaker

5m Example: A GaN based UV detector This is a photoconductor

Response Function of UV detector

Choose the material for the photon energy required. • Band-Gap adjustable by adding Al from 3.4 to 6.2 eV • Band gap is direct (= efficient) • Material is robust

The structure of a LED/Photodiode

Characterization of Detectors • NEP= noise equivalent power = noise current (A/Hz)/Radiant sensitivity (A/W) • D = detectivity = area/NEP • IR cut-off • maximum current • maximum reverse voltage • Field of view • Junction capacitance

Photomultipliers e e e e hf e e PE effect Secondary electron emission Electron multiplication

hf e Anode Dynode -V Photomultiplier tube • Combines PE effect with electron multiplication to provide very high detection sensitivity • Can detect single photons.

Microchannel plates • The principle of the photomultiplier tube can be extended to an array of photomultipliers • This way one can obtain spatial resolution • Biggest application is in night vision goggles for military and civilian use

Microchannel plates • MCPs consist of arrays of tiny tubes • Each tube is coated with a photomultiplying film • The tubes are about 10 microns wide http://hea-www.harvard.edu/HRC/mcp/mcp.html

MCP array structure http://hea-www.harvard.edu/HRC/mcp/mcp.html

MCP fabrication http://hea-www.harvard.edu/HRC/mcp/mcp.html

Disadvantages of Photomultiplers as sensors • Need expensive and fiddly high vacuum equipment • Expensive • Fragile • Bulky

Photoconductors • As well as liberating electrons from the surface of materials, we can excite mobile electrons inside materials • The most useful class of materials to do this are semiconductors • The mobile electrons can be measured as a current proportional to the intensity of the incident radiation • Need to understand semiconductors….

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Chapter 9. Atomic Physics. Atomic Physics. Classical physics (Newtonian physics) – development of physics prior to around 1900 Classical physics was generally concerned with macrocosm – the description & explanation of large-scale phenomena

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Atomic Physics. Atoms with dipoles – surface effects. Any sort of collision…. 1. Ion Velocity: E/mc 2 = E(MeV)/0.5(MeV) = ½ M N v 2 / mc 2 Therefore v/c = √ [ 4E(MeV) (m/M N )] = ( 2/√1840 ) √[(E (MeV)/A( amu )] Giving v = 13.9 mm/ns √[(E (MeV)/A( amu )]

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Atomic and Nuclear Physics

Atomic and Nuclear Physics. Topic 7. Atomic models. Videos :D. Properties of protons, neutrons and electrons. 1. + 1. nucleus. 1. 0. nucleus. outside nucleus. 0.0005. - 1. Nuclear notation. Nucleon number = mass number A = Z + N. Atomic number = number of protons. Terms .

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Atomic Physics. Hyperfine structure Part 3 Higher order multipole moment effects A general theory Some experiments. Elaborating our topic – hyperfine structure…. Higher order multipole moment hyperfine effects.

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Nuclear and Atomic Physics

Nuclear and Atomic Physics. Intro: Atomic Structure and a little history.  Print off the topic outline for this unit by tomorrow!. Early atomic structure…. JJ Thomson: “Plum pudding” model An atom is a mixture of positive and negative charges.

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Atomic Physics. Core. (d) Half-life -use the term half-life in simple calculations which might involve information in tables or decay curves (e) Safety precautions -describe how radioactive materials are handled , used and stored in a safe way. Half life.

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Spin and Atomic Physics

Spin and Atomic Physics. Today. HW 8, problem 7.38 Quiz 11.6 Topics in this chapter: The spin and the Stern-Gerlach experiment. Fermion, Boson and the Pauli exclusion principle. Multi-electron atoms and the Periodic Table. Characteristic X-rays. HW problem 7.38.

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Atomic and Nuclear Physics. The Atom Light Spectrum for Hydrogen Modern Model The Photon. The Atom. Matter is made of particles called atoms.

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Atomic Physics. Chapter 28. Atomic Models. Introduction. How do neon signs work?. Our main focus will be on the hydrogen atom. It is the simplest atomic system. Why is it important to study the hydrogen atom?

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Atomic Physics. Chapter 29. Lecture 24. All nature, then, as self-sustained, consists Of twain of things: of bodies and of void In which they're set, and where they're moved around. …. This ultimate stock we have devised to name Procreant atoms, matter, seeds of things,

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Atomic and Nuclear Physics. Atomic Physics. The last 150 years have actually been a time of great advancement for physics. Several important theories and ideas were postulated this time – ideas that you accept as commonplace.

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Atomic Physics. Micro-world Macro-world Lecture 15. Dimitri Mendeleev. Periodic table of elements. Elements in vertical rows have similar chemical properties. Inert gases. Schroedinger’s Equation for multi-electron Atoms. -. -. -. +. -. -.

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Quantum Physics 2002. Atomic Physics. Recommended Reading: Harris Chapter 7. L. Current. r. m. v. . Angular Momentum and Magnetic Dipole Moment.

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Chapter 29. Atomic Physics. Early Models of the Atom – Rutherford. Rutherford Planetary model Based on results of thin foil experiments Positive charge is concentrated in the center of the atom, called the nucleus Electrons orbit the nucleus like planets orbit the sun.

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Atomic Physics. “Driving Doppler Down” Doppler-free methods Laser cooling, trapping, quantum computing. COOLING – FUN demos…. Motion of an atom affects the absorption frequency, and its emission frequency. A reminder:. Question: Estimate the halfwidth at room temperature

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Atomic Physics. The Dirac equation for a one-electron atom Part 1. Controlling the Quantum World: http://www.nap.edu/catalog.php?record_id=11705.

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ATOMIC PHYSICS

ATOMIC PHYSICS. Dr. Anilkumar R. Kopplkar Associate Professor S.S. Margol College, SHAHABAD Gulbarga,Karnatka- India. Atomic Physics: Vector Atom model. Space quantization Electron spin Quantum numbers Pauli`s Exclusion principle Stern Gerlach Experiment

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Atomic Physics. Question 1. Calculate the Kinetic Energy gained by an electron when it is accelerated through a P.D. of 50kV in an X-ray tube. Firstly we know that KE is measured in Joules. JDeV….. eV = ½mv 2 (KE) eV = ( 1.6 X 10 -19 )(50000) = 8 X 10 -15 Joules = KE.

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Atomic Physics. K K Dey Assistant Professor in Physics B B College, Asansol. hydrogen atom It is the simplest atomic system. Why is it important to study the hydrogen atom? The hydrogen atom is an ideal system for relating theory to experimentation.

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Emission and absorption spectrum. Atomic Physics. Atoms emit and absorb light of specific wavelengths. Atoms from different elements have different wavelengths of emitted and absorbed light. These specific wave- lengths are the same for both emitted and absorbed light.

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