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 ...
Recitation 3
... Problem 20. In 1911, Ernest Rutherford and his assistants Hans Geiger and Ernest Mardsen conducted an experiment in which they scattered alpha particles from thin sheets of gold. An alpha particle, having a charge of qα = +2e and a mass of m = 6.64 · 10−27 kg is a product of certain radioactive deca ...
... Problem 20. In 1911, Ernest Rutherford and his assistants Hans Geiger and Ernest Mardsen conducted an experiment in which they scattered alpha particles from thin sheets of gold. An alpha particle, having a charge of qα = +2e and a mass of m = 6.64 · 10−27 kg is a product of certain radioactive deca ...
2015-2016 AP CHEMISTRY MIDTERM EXAM Review
... 4. Answer all three portions in this part. Give the formulas to show the reactants and the products for the three following chemical reactions. Each reaction occurs in aqueous solution unless otherwise indicated. Represent the substances in solution as ions if the substance is extensively ionized. ...
... 4. Answer all three portions in this part. Give the formulas to show the reactants and the products for the three following chemical reactions. Each reaction occurs in aqueous solution unless otherwise indicated. Represent the substances in solution as ions if the substance is extensively ionized. ...
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... Note for He2 (4 electrons), Pauli principle means two e’s in antibonding state as well as bonding state so no overall energy saving (inert gases – no bond - no He2) Mid-periodic table elements (half-filled orbitals) tend to have strongest bonds (e.g. melting points. etc.) ...
... Note for He2 (4 electrons), Pauli principle means two e’s in antibonding state as well as bonding state so no overall energy saving (inert gases – no bond - no He2) Mid-periodic table elements (half-filled orbitals) tend to have strongest bonds (e.g. melting points. etc.) ...
Introduction to Quantum Mechanics II Quiz 14
... Introduction to Quantum Mechanics II Quiz 14 Name: December 7, 2012 The Zeeman effect is due to the interaction of the magnetic dipole moment of the atom with an external magnetic field, ∆E = −µ · B. For the orbital motion of the electron, µ= ...
... Introduction to Quantum Mechanics II Quiz 14 Name: December 7, 2012 The Zeeman effect is due to the interaction of the magnetic dipole moment of the atom with an external magnetic field, ∆E = −µ · B. For the orbital motion of the electron, µ= ...
Chapter 7: Electrons in Atoms Electromagnetic Radiation
... But, for circular orbits, electrons would possess angular momentum (acceleration) and therefore radiate energy! So, using Planck’s quantum hypothesis, 1) Electrons move in fixed orbits around the nucleus 2) Fixed orbits (stationary states) mean properties of individual electrons will have unique v ...
... But, for circular orbits, electrons would possess angular momentum (acceleration) and therefore radiate energy! So, using Planck’s quantum hypothesis, 1) Electrons move in fixed orbits around the nucleus 2) Fixed orbits (stationary states) mean properties of individual electrons will have unique v ...
File first semester final study guide key
... Their presence is what allows us to calculate the ___average atomic mass____ which is our final number on the periodic table. Short Answer: Using a brief statement, answer each of the following questions about atomic structure. 1. John Dalton’s atomic theory states that, “atoms of a given element ar ...
... Their presence is what allows us to calculate the ___average atomic mass____ which is our final number on the periodic table. Short Answer: Using a brief statement, answer each of the following questions about atomic structure. 1. John Dalton’s atomic theory states that, “atoms of a given element ar ...
2·QUIZLET VOCABULARY: Quantum Numbers Study online at
... 3. electron configuration: the arrangement of electrons around nucleus in an atom 4. Hunds rule: orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin 5. Magnetic (orbital) ...
... 3. electron configuration: the arrangement of electrons around nucleus in an atom 4. Hunds rule: orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin 5. Magnetic (orbital) ...
TEST on Atomic Structure
... _____ 26) Which of the following is true about subatomic particles? a. Electrons have no charge and have almost no mass. b. Protons are negatively charged and the lightest subatomic particle. c. Neutrons have a negative charge and are the lightest subatomic particle. d. Electrons have almost no mass ...
... _____ 26) Which of the following is true about subatomic particles? a. Electrons have no charge and have almost no mass. b. Protons are negatively charged and the lightest subatomic particle. c. Neutrons have a negative charge and are the lightest subatomic particle. d. Electrons have almost no mass ...
Final Exam 2004
... two atoms. For large R, the dipole-dipole interaction can be considered as a small perturbation. Show that the energy of the dipole-dipole interaction of the two atoms in their ground states is zero in the first order of the perturbation theory. [Hint: Since the ground state is nondegenerate, you ca ...
... two atoms. For large R, the dipole-dipole interaction can be considered as a small perturbation. Show that the energy of the dipole-dipole interaction of the two atoms in their ground states is zero in the first order of the perturbation theory. [Hint: Since the ground state is nondegenerate, you ca ...
Lecture 13 (Slides) September 26
... • Coulomb’s Law → to pull the proton and electron apart we must do work/supply energy. Conversely, energy must be released if the proton and electron come closer to each other. The closer the e- comes to the nucleus the greater the amount of energy released. The application of Coulomb’s Law to atom ...
... • Coulomb’s Law → to pull the proton and electron apart we must do work/supply energy. Conversely, energy must be released if the proton and electron come closer to each other. The closer the e- comes to the nucleus the greater the amount of energy released. The application of Coulomb’s Law to atom ...
Matter – Properties and Changes
... • Substance: a form of matter that has a uniform and unchanging composition; also known as a pure substance. • Mixture: a physical blend of 2 or more pure substances in any proportion in which each substance retains its individual properties; can be separated by physical means • Chemical property: t ...
... • Substance: a form of matter that has a uniform and unchanging composition; also known as a pure substance. • Mixture: a physical blend of 2 or more pure substances in any proportion in which each substance retains its individual properties; can be separated by physical means • Chemical property: t ...
Document
... from Niels Bohr who explained experimentally observed discrete nature of atomic spectrum of Hydrogen. In spite of its immediate success in providing theoretical account of the spectrum and other nature of Hydrogen atom, a complete understanding of Bohr’s atom came only after de Broglie’s conjecture ...
... from Niels Bohr who explained experimentally observed discrete nature of atomic spectrum of Hydrogen. In spite of its immediate success in providing theoretical account of the spectrum and other nature of Hydrogen atom, a complete understanding of Bohr’s atom came only after de Broglie’s conjecture ...
LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034 /1.00-4.00
... 11. Discuss the failures of classical mechanics and the success of quantum theory in the explanation of black body radiation. . 12. What are quantum mechanical postulates? Explain briefly any two of the postulates. 13. The work function for Cesium is 2.14 eV. What is the kinetic energy and the speed ...
... 11. Discuss the failures of classical mechanics and the success of quantum theory in the explanation of black body radiation. . 12. What are quantum mechanical postulates? Explain briefly any two of the postulates. 13. The work function for Cesium is 2.14 eV. What is the kinetic energy and the speed ...
Chapter 9 - Fayetteville State University
... 7) Periodic Law: States that elements arranged in order of the atomic number share similar chemical and physical properties. These arrangement are called groups, examples are the alkali metals (Li, Na, K, Rb, Cs), the halogens (F, Cl, Br, I). 8) Groups: A sequence of elements of increasing atomic nu ...
... 7) Periodic Law: States that elements arranged in order of the atomic number share similar chemical and physical properties. These arrangement are called groups, examples are the alkali metals (Li, Na, K, Rb, Cs), the halogens (F, Cl, Br, I). 8) Groups: A sequence of elements of increasing atomic nu ...
Document
... 43) In a chemical reaction, the name(s) of the material(s) that you start with are called the reactants and appear on the left side of the arrow, 44) In a chemical reaction, the name(s) of the material(s) that you end with are called the products and appear on the right side of the arrow. 45) In a c ...
... 43) In a chemical reaction, the name(s) of the material(s) that you start with are called the reactants and appear on the left side of the arrow, 44) In a chemical reaction, the name(s) of the material(s) that you end with are called the products and appear on the right side of the arrow. 45) In a c ...
Atomic theory
In chemistry and physics, atomic theory is a scientific theory of the nature of matter, which states that matter is composed of discrete units called atoms. It began as a philosophical concept in ancient Greece and entered the scientific mainstream in the early 19th century when discoveries in the field of chemistry showed that matter did indeed behave as if it were made up of atoms.The word atom comes from the Ancient Greek adjective atomos, meaning ""uncuttable"". 19th century chemists began using the term in connection with the growing number of irreducible chemical elements. While seemingly apropos, around the turn of the 20th century, through various experiments with electromagnetism and radioactivity, physicists discovered that the so-called ""uncuttable atom"" was actually a conglomerate of various subatomic particles (chiefly, electrons, protons and neutrons) which can exist separately from each other. In fact, in certain extreme environments, such as neutron stars, extreme temperature and pressure prevents atoms from existing at all. Since atoms were found to be divisible, physicists later invented the term ""elementary particles"" to describe the ""uncuttable"", though not indestructible, parts of an atom. The field of science which studies subatomic particles is particle physics, and it is in this field that physicists hope to discover the true fundamental nature of matter.