Modern physics
... • Stefan-Boltzmann blackbody had UV catastrophe • Planck quantized light, and solved blackbody problem • Einstein used Planck’s quanta to explain photoelectric effect • Compton effect demonstrated quantization of light • Corrollary: deBroglie’s matter waves, discovered by Davisson & Germer ...
... • Stefan-Boltzmann blackbody had UV catastrophe • Planck quantized light, and solved blackbody problem • Einstein used Planck’s quanta to explain photoelectric effect • Compton effect demonstrated quantization of light • Corrollary: deBroglie’s matter waves, discovered by Davisson & Germer ...
Atomic Structure
... Identify Group, Period, block, total # eWrite orbital notation/orbital diagrams to see specific quantum numbers for atoms/electrons lines/boxes with arrows (2 opposite arrows on each line) ...
... Identify Group, Period, block, total # eWrite orbital notation/orbital diagrams to see specific quantum numbers for atoms/electrons lines/boxes with arrows (2 opposite arrows on each line) ...
Quantum Theory of Atoms
... • n is the principal quantum number and is associated with the distance r of an electron from the nucleus • l is the orbital quantum number and the angular momentum of the electron is given by L=[l(l+1)]1/2 ħ • m is the magnetic quantum number and the component of the angular momentum along the z-ax ...
... • n is the principal quantum number and is associated with the distance r of an electron from the nucleus • l is the orbital quantum number and the angular momentum of the electron is given by L=[l(l+1)]1/2 ħ • m is the magnetic quantum number and the component of the angular momentum along the z-ax ...
notes on Bohr and the hydrogen spectrum
... answer. But for an electron, the observation is analogous: either we interact with it or we don't. Now for the bad news. de Broglie's wave hypothesis is a good one. The electrical potential for the hydrogen nucleus is correct. But a lot of the story that we have just seen, all the analysis based on ...
... answer. But for an electron, the observation is analogous: either we interact with it or we don't. Now for the bad news. de Broglie's wave hypothesis is a good one. The electrical potential for the hydrogen nucleus is correct. But a lot of the story that we have just seen, all the analysis based on ...
Atomic Structure 1. Historical perspective of the model of the atom a
... a.) In 1803, John Dalton proposed the atomic theory which stated that all matter is made of atoms, atoms of the same type of element have the same chemical properties, compounds are formed by two or more different types of atoms, and that a chemical reaction involves either, joining, separating, or ...
... a.) In 1803, John Dalton proposed the atomic theory which stated that all matter is made of atoms, atoms of the same type of element have the same chemical properties, compounds are formed by two or more different types of atoms, and that a chemical reaction involves either, joining, separating, or ...
Quantum Mechanics and the Bohr Model - slater science
... •Explain how the frequencies of emitted light are related to changes in electron energies. •Distinguish between quantum mechanics and classical mechanics. ...
... •Explain how the frequencies of emitted light are related to changes in electron energies. •Distinguish between quantum mechanics and classical mechanics. ...
Chapter 6 review
... moving… • Then a particle moving at a velocity v has a wavelength using the equation m=h/v • Solve for and =h/mv • This is de Broglie’s equation. ...
... moving… • Then a particle moving at a velocity v has a wavelength using the equation m=h/v • Solve for and =h/mv • This is de Broglie’s equation. ...
Exam sample
... 7. “No two electrons in the same atom may have the same values for all four quantum numbers” is a statement of: a. Hund’s Rule. b. deBroglie’s Hypothesis. c. the Pauli Exclusion Principle. d. the Heisenberg Uncertainty Principle. 8. All s orbitals are: a. shaped like four-leaf clovers. b. dumbbell- ...
... 7. “No two electrons in the same atom may have the same values for all four quantum numbers” is a statement of: a. Hund’s Rule. b. deBroglie’s Hypothesis. c. the Pauli Exclusion Principle. d. the Heisenberg Uncertainty Principle. 8. All s orbitals are: a. shaped like four-leaf clovers. b. dumbbell- ...
Document
... the order of ave in an atomic scattering experiment: R ~ 0.1 nm (a typical atomic radius), N ~ 104 (no. of collisions in the target metal foil), kinetic energy of the alpha particle, mv2 ~ 10 MeV, z = 2 (charge of alpha particle); Z ~ 79 for gold. Putting in all figures, one expects that alpha par ...
... the order of ave in an atomic scattering experiment: R ~ 0.1 nm (a typical atomic radius), N ~ 104 (no. of collisions in the target metal foil), kinetic energy of the alpha particle, mv2 ~ 10 MeV, z = 2 (charge of alpha particle); Z ~ 79 for gold. Putting in all figures, one expects that alpha par ...
Bohr Model and Quantum Model
... understanding the behavior of light Light is composed of Electromagnetic (EM) waves EM spectrum shows all forms of radiation ...
... understanding the behavior of light Light is composed of Electromagnetic (EM) waves EM spectrum shows all forms of radiation ...
CHEMISTRY CHAPTER 4 – QUANTUM MECHANICS
... 7. Explain how the Heisenberg uncertainty principle and the Schrödinger wave equation led to the idea of atomic orbitals. 8. List the four quantum numbers and describe their significance. 9. Relate the number of sublevels corresponding to each of an atom’s main energy levels, the number of orbitals ...
... 7. Explain how the Heisenberg uncertainty principle and the Schrödinger wave equation led to the idea of atomic orbitals. 8. List the four quantum numbers and describe their significance. 9. Relate the number of sublevels corresponding to each of an atom’s main energy levels, the number of orbitals ...
Problem set #1 - U.C.C. Physics Department
... wave along the x-direction, the y-direction, and its direction of motion. 2) Bohr’s atomic model Recall that Bohr derived Rydberg’s constant by assuming (1) that the electrons move around the nucleus in discrete orbits; and (2) that the angular momentum is quantized. Here, I ask you to repeat Bohr’s ...
... wave along the x-direction, the y-direction, and its direction of motion. 2) Bohr’s atomic model Recall that Bohr derived Rydberg’s constant by assuming (1) that the electrons move around the nucleus in discrete orbits; and (2) that the angular momentum is quantized. Here, I ask you to repeat Bohr’s ...
Quantum Mechanical Model - Elmwood Park Memorial Middle School
... • These slides are on the webpage if you would like them. ...
... • These slides are on the webpage if you would like them. ...
DEVELOPMENT OF THE ATOMIC THEORY PROJECT due Friday
... In succeeding layers, you will add detail to your atom and name the scientist who developed this part of the atomic theory. You will also include a picture or a brief description of the method the scientist used. You must include development of the quantum model in your depiction of the electron clo ...
... In succeeding layers, you will add detail to your atom and name the scientist who developed this part of the atomic theory. You will also include a picture or a brief description of the method the scientist used. You must include development of the quantum model in your depiction of the electron clo ...
Introduction Slides
... It appears to predict the atom would radiate all the time from the orbiting electron The atom does not “look” like this it is not a small “point” electron in a classical orbit ...
... It appears to predict the atom would radiate all the time from the orbiting electron The atom does not “look” like this it is not a small “point” electron in a classical orbit ...
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.