Lecture 1 (Bohr model of the atom)
... • In this theory electrons are considered to be point objects in orbit around the nucleus • It gives a 1st order explanation of the spectral lines, & remains a useful treatment of electron behaviour • Next year you will gain enough QM knowledge to see how the true quantum description of such systems ...
... • In this theory electrons are considered to be point objects in orbit around the nucleus • It gives a 1st order explanation of the spectral lines, & remains a useful treatment of electron behaviour • Next year you will gain enough QM knowledge to see how the true quantum description of such systems ...
Unit 4: Atoms and Nuclei
... • In this theory electrons are considered to be point objects in orbit around the nucleus • It gives a 1st order explanation of the spectral lines, & remains a useful treatment of electron behaviour • Next year you will gain enough QM knowledge to see how the true quantum description of such syst ...
... • In this theory electrons are considered to be point objects in orbit around the nucleus • It gives a 1st order explanation of the spectral lines, & remains a useful treatment of electron behaviour • Next year you will gain enough QM knowledge to see how the true quantum description of such syst ...
Atomic
... Early ideas about the existence of atoms are usually attributed to the philosophers of Ancient Greece. The hard core of this model contains two ideas: i. matter is composed of very small indivisible corpuscles - probably first called ‘atoms’ by Leukippos. ii. atoms are infinitely hard and differ in ...
... Early ideas about the existence of atoms are usually attributed to the philosophers of Ancient Greece. The hard core of this model contains two ideas: i. matter is composed of very small indivisible corpuscles - probably first called ‘atoms’ by Leukippos. ii. atoms are infinitely hard and differ in ...
Atomic Physics
... choosing n = 1 for the orbit where the kinetic energy of the electron is zero. adding a constant 13.6 eV to the potential energy for all values of n. adding a constant 27.2 eV to the potential energy for all values of n. subtracting a constant 13.6 eV from the potential energy for all values of n. s ...
... choosing n = 1 for the orbit where the kinetic energy of the electron is zero. adding a constant 13.6 eV to the potential energy for all values of n. adding a constant 27.2 eV to the potential energy for all values of n. subtracting a constant 13.6 eV from the potential energy for all values of n. s ...
Slide 1 - Southwest High School
... This work is protected by United States copyright laws and is provided solely for the use of instructors in teaching their courses and assessing student learning. Dissemination or sale of any part of this work (including on the World Wide Web) will destroy the integrity of the work and is not permit ...
... This work is protected by United States copyright laws and is provided solely for the use of instructors in teaching their courses and assessing student learning. Dissemination or sale of any part of this work (including on the World Wide Web) will destroy the integrity of the work and is not permit ...
atomic physics
... and energy loss as required by classical electromagnetics. The Bohr model of an atom was based upon Planck's quantum theory of radiation. 3. Electrons can only gain and lose energy by jumping from one allowed orbit to another, absorbing or emitting electromagnetic radiation with a frequency ν determ ...
... and energy loss as required by classical electromagnetics. The Bohr model of an atom was based upon Planck's quantum theory of radiation. 3. Electrons can only gain and lose energy by jumping from one allowed orbit to another, absorbing or emitting electromagnetic radiation with a frequency ν determ ...
Document
... Atomic Transitions – Stimulated Emission An atom is in an excited stated and a photon is incident on it The incoming photon increases the probability that the excited atom will return to the ground state There are two emitted photons, the incident one and the emitted one ...
... Atomic Transitions – Stimulated Emission An atom is in an excited stated and a photon is incident on it The incoming photon increases the probability that the excited atom will return to the ground state There are two emitted photons, the incident one and the emitted one ...
2_Lecture BOHR.pptx
... Be able to use the Bohr Model to solve problems describing electronic transitions in the Hydrogen atom. If ni = 2 and nf = 1, is energy emitted or absorbed? 1 . emitted 2 . absorbed ...
... Be able to use the Bohr Model to solve problems describing electronic transitions in the Hydrogen atom. If ni = 2 and nf = 1, is energy emitted or absorbed? 1 . emitted 2 . absorbed ...
Models of an atom and old quantum theory
... system which carries oscillatory motion can be described by a set of appropriate canonical coordinates qi which are periodic functions of time. There is a canonical momentum pi associated with each canonical coordinate qi . Canonical coordinates and momenta are a convenient way to generalize the for ...
... system which carries oscillatory motion can be described by a set of appropriate canonical coordinates qi which are periodic functions of time. There is a canonical momentum pi associated with each canonical coordinate qi . Canonical coordinates and momenta are a convenient way to generalize the for ...
Lyman alpha forest
... Convolution of a Gaussian and a Lorentzian The core part is approximately Gaussian whereas the wing part is Lorentzian. Resonance line shape is approximately Lorentzian in the near wing part. Far wing part, deviation from a Lorentzian is observed depending on the atomic wavefunction. ...
... Convolution of a Gaussian and a Lorentzian The core part is approximately Gaussian whereas the wing part is Lorentzian. Resonance line shape is approximately Lorentzian in the near wing part. Far wing part, deviation from a Lorentzian is observed depending on the atomic wavefunction. ...
5. Atomic models
... since the electrons now have enough energy to reach the plate. Eventually another sharp drop (at 9.8 V) in the current occurs because, again, the electron has collected just the same energy to excite the same energy level in the other atoms. The higher ...
... since the electrons now have enough energy to reach the plate. Eventually another sharp drop (at 9.8 V) in the current occurs because, again, the electron has collected just the same energy to excite the same energy level in the other atoms. The higher ...
Chemistry Chapter 5 Test Multiple Choice (1.5% each) Identify the
... b. Compare the results to the grades of students who did not participate in the study program. c. Compare the history grades of students who participated in the program to their science grades. 11. The lowest possible energy state the electrons in an atom can have. a. Ground State c. Quantum Mechani ...
... b. Compare the results to the grades of students who did not participate in the study program. c. Compare the history grades of students who participated in the program to their science grades. 11. The lowest possible energy state the electrons in an atom can have. a. Ground State c. Quantum Mechani ...
class slides for Chapter 39
... measure of the magnitude of the angular momentum associated with the quantum state. The orbital magnetic quantum number ml is related to the orientation in space of this angular momentum vector. ...
... measure of the magnitude of the angular momentum associated with the quantum state. The orbital magnetic quantum number ml is related to the orientation in space of this angular momentum vector. ...
Study On the Capacitance Between Orbitals and Atoms Modeling
... Figure 1 illustrates the proposed model for the Hydrogen atom (It looks like tunnel junctions turnstile). The capacitances between energy levels can be computed by substituting the first values of the line spectrum series, stated in Table 1 for Hydrogen atom, in equation (5). The capacitances C 12 t ...
... Figure 1 illustrates the proposed model for the Hydrogen atom (It looks like tunnel junctions turnstile). The capacitances between energy levels can be computed by substituting the first values of the line spectrum series, stated in Table 1 for Hydrogen atom, in equation (5). The capacitances C 12 t ...
Worksheet
... 1) Summarize the contributions of each of the following individuals to our understanding of the atom and atomic structure (you may have to look back into CH 4 for the first 3…or the summary on page 133). Include a sketch of what the atom would look like according to their explanations. • Dalton: ...
... 1) Summarize the contributions of each of the following individuals to our understanding of the atom and atomic structure (you may have to look back into CH 4 for the first 3…or the summary on page 133). Include a sketch of what the atom would look like according to their explanations. • Dalton: ...
1 slide per page() - Wayne State University Physics and Astronomy
... 9Atomic Physics 9Early models of the atom 9Atomic spectra 9Bohr’s theory of hydrogen 9De Broglie wavelength in the atom 9Quantum mechanics and Spin Chapter 28 ...
... 9Atomic Physics 9Early models of the atom 9Atomic spectra 9Bohr’s theory of hydrogen 9De Broglie wavelength in the atom 9Quantum mechanics and Spin Chapter 28 ...
Bohr vs. Correct Model of Atom
... Summary • Bohr’s Model gives accurate values for electron energy levels... • But Quantum Mechanics is needed to describe electrons in atom. • Electrons jump between states by emitting or absorbing photons of the appropriate energy. • Each state has specific energy and is labeled by 4 quantum number ...
... Summary • Bohr’s Model gives accurate values for electron energy levels... • But Quantum Mechanics is needed to describe electrons in atom. • Electrons jump between states by emitting or absorbing photons of the appropriate energy. • Each state has specific energy and is labeled by 4 quantum number ...
Chapter 39
... measure of the magnitude of the angular momentum associated with the quantum state. The orbital magnetic quantum number ml is related to the orientation in space of this angular momentum vector. The restrictions on the values of the quantum numbers for the hydrogen atom, as listed in Table 39-2, are ...
... measure of the magnitude of the angular momentum associated with the quantum state. The orbital magnetic quantum number ml is related to the orientation in space of this angular momentum vector. The restrictions on the values of the quantum numbers for the hydrogen atom, as listed in Table 39-2, are ...
P. LeClair
... charge, they can’t be accelerated by electric potentials like electrons. The microscope simply won’t work like this, there is no resolution! Why not protons, though, since they can be accelerated by potentials? Electrons, we found, are bound to their atomic nuclei with energies on the order of a few ...
... charge, they can’t be accelerated by electric potentials like electrons. The microscope simply won’t work like this, there is no resolution! Why not protons, though, since they can be accelerated by potentials? Electrons, we found, are bound to their atomic nuclei with energies on the order of a few ...
AP Physics 2 Syllabus Student
... Big Idea 5 – Changes that occur as a result of interactions are constrained by conservation laws. Big Idea 6 – Waves can transfer energy and momentum from one location to another without the permanent transfer of mass and serve as a mathematical model for the description of other phenomena. Big Idea ...
... Big Idea 5 – Changes that occur as a result of interactions are constrained by conservation laws. Big Idea 6 – Waves can transfer energy and momentum from one location to another without the permanent transfer of mass and serve as a mathematical model for the description of other phenomena. Big Idea ...
Calculus with Analytic Geometry
... Mathematical Methods for Physicists, by Arfken or, Mathematical Methods of Physics by Mathews and Walker ...
... Mathematical Methods for Physicists, by Arfken or, Mathematical Methods of Physics by Mathews and Walker ...
Atomic Theory Review
... Both Rutherford’s and Bohr’s models of the atom have a nucleus, which is an extremely small, dense region in the center of the atom, that contains most of the atom’s mass and all of its positive charge. Both models have negatively charged electrons orbiting the nucleus. The difference is that Bohr’s ...
... Both Rutherford’s and Bohr’s models of the atom have a nucleus, which is an extremely small, dense region in the center of the atom, that contains most of the atom’s mass and all of its positive charge. Both models have negatively charged electrons orbiting the nucleus. The difference is that Bohr’s ...
James Franck
James Franck (26 August 1882 – 21 May 1964) was a German physicist who won the 1925 Nobel Prize for Physics with Gustav Hertz ""for their discovery of the laws governing the impact of an electron upon an atom"". He completed his doctorate in 1906 and his habilitation in 1911 at the Frederick William University in Berlin, where he lectured and taught until 1918, having reached the position of professor extraordinarius. He served as a volunteer in the German Army during World War I. He was seriously injured in 1917 in a gas attack and was awarded the Iron Cross 1st Class.Franck became the Head of the Physics Division of the Kaiser Wilhelm Gesellschaft for Physical Chemistry. In 1920, Franck became professor ordinarius of experimental physics and Director of the Second Institute for Experimental Physics at the University of Göttingen. While there he worked on quantum physics with Max Born, who was Director of the Institute of Theoretical Physics. His work included the Franck–Hertz experiment, an important confirmation of the Bohr model of the atom. He promoted the careers of women in physics, notably Lise Meitner, Hertha Sponer and Hilde Levi.After the NSDAP came to power in Germany in 1933, Franck resigned his post in protest against the dismissal of fellow academics. He assisted Frederick Lindemann in helping dismissed Jewish scientists find work overseas, before he left Germany in November 1933. After a year at the Niels Bohr Institute in Denmark, he moved to the United States, where he worked at Johns Hopkins University in Baltimore and then the University of Chicago. During this period he became interested in photosynthesis.Franck participated in the Manhattan Project during World War II as Director of the Chemistry Division of the Metallurgical Laboratory. He was also the chairman of the Committee on Political and Social Problems regarding the atomic bomb, which is best known for the compilation of the Franck Report, which recommended that the atomic bombs not be used on the Japanese cities without warning.