CHEM 532 Physical Chemistry II (Quantum Chemistry) Fall 2013
... the variation method, time independent perturbation theory, degenerate perturbation theory, the anharmonic oscillator VIII. The Helium atom electron spin, ground state of He, excited electronic states of He, spin eigenfunctions of He IX. Many-electron wavefunctions indistinguishable particles, the P ...
... the variation method, time independent perturbation theory, degenerate perturbation theory, the anharmonic oscillator VIII. The Helium atom electron spin, ground state of He, excited electronic states of He, spin eigenfunctions of He IX. Many-electron wavefunctions indistinguishable particles, the P ...
The Relativistic Quantum World
... Use h= 6.62 × 10-34 Js to calculate: • Wavelength electron with v = 0.1 c: 0.024 nm • Wavelength of a fly (m = 0.01 gram, v = 10 m/s): 0.0000000000000000000062 nm ...
... Use h= 6.62 × 10-34 Js to calculate: • Wavelength electron with v = 0.1 c: 0.024 nm • Wavelength of a fly (m = 0.01 gram, v = 10 m/s): 0.0000000000000000000062 nm ...
chapter 2
... 13. What two things are classified as pure substances?___ compounds _____ and ____ elements ______ 14. What is the difference between a homogeneous and heterogeneous mixture? _____________________ __ HO – looks uniform in composition; HE – you can see different parts ____________ 15. Describe each o ...
... 13. What two things are classified as pure substances?___ compounds _____ and ____ elements ______ 14. What is the difference between a homogeneous and heterogeneous mixture? _____________________ __ HO – looks uniform in composition; HE – you can see different parts ____________ 15. Describe each o ...
27-3 A Photoelectric Effect Example
... (b) As we discussed in Exploration 27.2, the maximum kinetic energy of the emitted electrons is related to the minimum voltage across the two plates needed to stop the electrons from reaching the second plate (this is known as the stopping potential). In this case, the stopping potential is 1.40 V, ...
... (b) As we discussed in Exploration 27.2, the maximum kinetic energy of the emitted electrons is related to the minimum voltage across the two plates needed to stop the electrons from reaching the second plate (this is known as the stopping potential). In this case, the stopping potential is 1.40 V, ...
Document
... • Energy is quantized. It comes in chunks. • A quanta is the amount of energy needed to move from one energy level to another. • Since the energy of an atom is never “in between” there must be a quantum leap in energy. • Schrödinger derived an equation that described the energy and position of the e ...
... • Energy is quantized. It comes in chunks. • A quanta is the amount of energy needed to move from one energy level to another. • Since the energy of an atom is never “in between” there must be a quantum leap in energy. • Schrödinger derived an equation that described the energy and position of the e ...
Liad Elmelech 7.1-7.3 The Nature of Light, Atomic Spectroscopy
... • Light has properties of both waves and particles • Light is electromagnetic radiation • Energy of fluctuating electric and magnetic fields • Magnetic field - area were magnetic particles experience a force • Electric field – are regions were electrically charged particles experience a force • Trav ...
... • Light has properties of both waves and particles • Light is electromagnetic radiation • Energy of fluctuating electric and magnetic fields • Magnetic field - area were magnetic particles experience a force • Electric field – are regions were electrically charged particles experience a force • Trav ...
HOMEWORK ASSIGNMENT 12
... 3. [20 pts] Numerically compute the matrix elements of the z-component of the orbital electric and magnetic dipole moments for the |200i → |100i, |210i → |100i, and |211i → |100i transitions in hydrogen. Be sure to show your work. For the electric dipole moments, we need to compute ehi|Z|f i = ehi| ...
... 3. [20 pts] Numerically compute the matrix elements of the z-component of the orbital electric and magnetic dipole moments for the |200i → |100i, |210i → |100i, and |211i → |100i transitions in hydrogen. Be sure to show your work. For the electric dipole moments, we need to compute ehi|Z|f i = ehi| ...
INTRODUCTION TO QUANTUM MECHANICS I I mention in class
... two-dimensional space. When the electron is bound to one proton it has an energy E0 < 0. But there is always a small probability for it to tunnel through the other proton (with a probability amplitude T ) so the full hamiltonian (well, the crude approximation to it in the two-dimensional Hilbert spa ...
... two-dimensional space. When the electron is bound to one proton it has an energy E0 < 0. But there is always a small probability for it to tunnel through the other proton (with a probability amplitude T ) so the full hamiltonian (well, the crude approximation to it in the two-dimensional Hilbert spa ...
Chapter 4 Study Guide-Atomic Structure Define the following terms
... Periodic Table-arrangement of elements in which the elements are separated into groups based on a set of repeating properties Proton-positively charged subatomic particle that lives in the nucleus Plum Pudding Model-electrons stuck in positive lump (JJ Thomson) ...
... Periodic Table-arrangement of elements in which the elements are separated into groups based on a set of repeating properties Proton-positively charged subatomic particle that lives in the nucleus Plum Pudding Model-electrons stuck in positive lump (JJ Thomson) ...
Detailed Notes CH. 6
... • It cannot explain the spectra of atoms other than hydrogen. • Electrons do not move about the nucleus in circular orbits. However, the model introduces two important ideas: • The energy of an electron is quantized: electrons exist only in certain energy levels described by quantum numbers. • En ...
... • It cannot explain the spectra of atoms other than hydrogen. • Electrons do not move about the nucleus in circular orbits. However, the model introduces two important ideas: • The energy of an electron is quantized: electrons exist only in certain energy levels described by quantum numbers. • En ...
LEWIS DOT STRUCTURES , MOLECULAR SHAPES, AND
... negative; subtract from the total number of electrons if the ion is positive. Example: if an ion has a –3 charge, add 3 more electrons to the total of valence electrons. 3. Total the number of valence electrons in the atoms to be combined 4. Arrange the atoms to form a skeletal structure for the mol ...
... negative; subtract from the total number of electrons if the ion is positive. Example: if an ion has a –3 charge, add 3 more electrons to the total of valence electrons. 3. Total the number of valence electrons in the atoms to be combined 4. Arrange the atoms to form a skeletal structure for the mol ...
Exam I
... Washing Machine Design Company. After you’ve been on the job for a few weeks, you attend a meeting where some of the engineers are fretting about static electric charges building up on the inside of the new model of washing machines. The big boss Bob is in the meeting and he says, “Where did you boz ...
... Washing Machine Design Company. After you’ve been on the job for a few weeks, you attend a meeting where some of the engineers are fretting about static electric charges building up on the inside of the new model of washing machines. The big boss Bob is in the meeting and he says, “Where did you boz ...
electrons - Portal UniMAP
... space because the volume of the nucleus and the electrons outside the nucleus are extremely small compared to the overall volume of the atom. ...
... space because the volume of the nucleus and the electrons outside the nucleus are extremely small compared to the overall volume of the atom. ...
Department of Physics and Physical Oceanography Sigma Pi Sigma INDUCTION
... Department of Physics, Yeshiva University ...
... Department of Physics, Yeshiva University ...
SPECIAL
... repeating this experiment [that of Hertz] I at first got the same result, but subsequentexperimentsshowedthat the absenceof deflexion is due to the conductivity conferred on the rarefied gas by the cathoderays."3 Thomsonthen performed the experiment at lower pressure and, indeed, observedthe deflect ...
... repeating this experiment [that of Hertz] I at first got the same result, but subsequentexperimentsshowedthat the absenceof deflexion is due to the conductivity conferred on the rarefied gas by the cathoderays."3 Thomsonthen performed the experiment at lower pressure and, indeed, observedthe deflect ...
Unit 2 Review for Test
... 5. Define: compound. 6. Over 96% of all living matter is made up of which elements? 7. Describe this formula: CO2. 8. Are elements made up of 1 or more atoms? 9. Draw a Bohr model and label the subatomic particles . 10. Define: isotope. 11. If an electron is lost during a reaction, would the charge ...
... 5. Define: compound. 6. Over 96% of all living matter is made up of which elements? 7. Describe this formula: CO2. 8. Are elements made up of 1 or more atoms? 9. Draw a Bohr model and label the subatomic particles . 10. Define: isotope. 11. If an electron is lost during a reaction, would the charge ...
QM lecture - The Evergreen State College
... Recall solution to Schrödinger eqn in spherical coordinates with Coulomb potential (H atom) Work on HW help sheet (linked to Help page) – Probs.1 and 10. Angular Momentum - Minilecture by Don Verbeke (Do Prob 4.18, and 4.20 p.150 as you did Prob.1 above) ...
... Recall solution to Schrödinger eqn in spherical coordinates with Coulomb potential (H atom) Work on HW help sheet (linked to Help page) – Probs.1 and 10. Angular Momentum - Minilecture by Don Verbeke (Do Prob 4.18, and 4.20 p.150 as you did Prob.1 above) ...
Bohr model
In atomic physics, the Rutherford–Bohr model or Bohr model, introduced by Niels Bohr in 1913, depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus—similar in structure to the solar system, but with attraction provided by electrostatic forces rather than gravity. After the cubic model (1902), the plum-pudding model (1904), the Saturnian model (1904), and the Rutherford model (1911) came the Rutherford–Bohr model or just Bohr model for short (1913). The improvement to the Rutherford model is mostly a quantum physical interpretation of it. The Bohr model has been superseded, but the quantum theory remains sound.The model's key success lay in explaining the Rydberg formula for the spectral emission lines of atomic hydrogen. While the Rydberg formula had been known experimentally, it did not gain a theoretical underpinning until the Bohr model was introduced. Not only did the Bohr model explain the reason for the structure of the Rydberg formula, it also provided a justification for its empirical results in terms of fundamental physical constants.The Bohr model is a relatively primitive model of the hydrogen atom, compared to the valence shell atom. As a theory, it can be derived as a first-order approximation of the hydrogen atom using the broader and much more accurate quantum mechanics and thus may be considered to be an obsolete scientific theory. However, because of its simplicity, and its correct results for selected systems (see below for application), the Bohr model is still commonly taught to introduce students to quantum mechanics or energy level diagrams before moving on to the more accurate, but more complex, valence shell atom. A related model was originally proposed by Arthur Erich Haas in 1910, but was rejected. The quantum theory of the period between Planck's discovery of the quantum (1900) and the advent of a full-blown quantum mechanics (1925) is often referred to as the old quantum theory.