FirstSemesterReviewHonors
... You may use the study guide on the final exam. You must provide all formulas where needed, since formulas will not be provided for you on the final. You should take at least 1 week to complete the material within the study guide. Chapter 1 1. A characteristic of a scientific theory is that it can ne ...
... You may use the study guide on the final exam. You must provide all formulas where needed, since formulas will not be provided for you on the final. You should take at least 1 week to complete the material within the study guide. Chapter 1 1. A characteristic of a scientific theory is that it can ne ...
PPT
... The uncertainty principle explains why electrons in atoms don’t simply fall into the nucleus: If the electron were confined too close to the nucleus (small Dx), it would have a large Dp, and therefore a very large average kinetic energy ( (Dp)2/2m). The uncertainty principle does not say “everythin ...
... The uncertainty principle explains why electrons in atoms don’t simply fall into the nucleus: If the electron were confined too close to the nucleus (small Dx), it would have a large Dp, and therefore a very large average kinetic energy ( (Dp)2/2m). The uncertainty principle does not say “everythin ...
Chapter 5 Sec. 2 Sublevels and Orbitals NOTES
... At any given time, the electron in a hydrogen atom can occupy only one orbital. When the hydrogen atom is in the ground state, the electron occupies the 1s orbital. Depending on the ENERGY available the electron can move to the 2s orbital, to one of the three 2p orbitals, or to any other vacant orbi ...
... At any given time, the electron in a hydrogen atom can occupy only one orbital. When the hydrogen atom is in the ground state, the electron occupies the 1s orbital. Depending on the ENERGY available the electron can move to the 2s orbital, to one of the three 2p orbitals, or to any other vacant orbi ...
SAMPLE midterm with solutions
... The quantum Hall effect is robust because it exists so long as there are edge states at opposite sides of the sample, which carry current in one direction only and are in separate equilibrium. The states on a single edge are chiral, that is, they propagate only in one direction. Therefore even if an ...
... The quantum Hall effect is robust because it exists so long as there are edge states at opposite sides of the sample, which carry current in one direction only and are in separate equilibrium. The states on a single edge are chiral, that is, they propagate only in one direction. Therefore even if an ...
The Hydrogen Atom Revisited
... hydrogen cannot go below this ground state in isolation. However, there is no known composition of matter containing hydrogen in the ground state of 13.6 eV. It is a myth that hydrogen has a theoretical ground state based on first principles. Historically there were many directions in which to proce ...
... hydrogen cannot go below this ground state in isolation. However, there is no known composition of matter containing hydrogen in the ground state of 13.6 eV. It is a myth that hydrogen has a theoretical ground state based on first principles. Historically there were many directions in which to proce ...
18. The Light Quantum Hypothesis.
... "Indeed, it seems to me that the observations of 'black-body radiation', photoluminescence, production of cathode rays by ultraviolet light, and other related phenomena associated with the emission or transformation of light appear more readily understood if one assumes that the energy of light is d ...
... "Indeed, it seems to me that the observations of 'black-body radiation', photoluminescence, production of cathode rays by ultraviolet light, and other related phenomena associated with the emission or transformation of light appear more readily understood if one assumes that the energy of light is d ...
Chemistry Chapter 8 (HW Jan 28 Due Feb 5 Test Feb 6)
... a covalent bond in which the shared electron pair comes from only one of the atoms a type of bond that is very important in determining the properties of water and of important biological molecules such as proteins and DNA Match each item with the correct statement below. a. network solid e. tetrahe ...
... a covalent bond in which the shared electron pair comes from only one of the atoms a type of bond that is very important in determining the properties of water and of important biological molecules such as proteins and DNA Match each item with the correct statement below. a. network solid e. tetrahe ...
1 - Groupfusion.net
... The nucleus contains the protons and neutrons which make up most of the mass of the atom. The size of the nucleus is very small compared to the rest of the atom. ...
... The nucleus contains the protons and neutrons which make up most of the mass of the atom. The size of the nucleus is very small compared to the rest of the atom. ...
High School Curriculum Standards: Chemistry
... Chemistry is the study of matter—its properties and its changes. The idea that matter is made up of particles is over 2000 years old, but the idea of using properties of these particles to explain observable characteristics of matter has more recent origins. In ancient Greece, it was proposed that m ...
... Chemistry is the study of matter—its properties and its changes. The idea that matter is made up of particles is over 2000 years old, but the idea of using properties of these particles to explain observable characteristics of matter has more recent origins. In ancient Greece, it was proposed that m ...
Review # 3
... History of Atomic Theory: key milestones, persons, and experiments Atomic structure Nuclear notations Average atomic mass Nuclear stability Radioactive decay: , particles and ray; and decays Nuclear equations Half-life, radioactive dating ...
... History of Atomic Theory: key milestones, persons, and experiments Atomic structure Nuclear notations Average atomic mass Nuclear stability Radioactive decay: , particles and ray; and decays Nuclear equations Half-life, radioactive dating ...
Discrete-continuous and classical-quantum
... of Schrödinger (corresponding to a differential equation seating in a Hilbert space) is in fact a economical extension of the finite dimension matrices of Heisenberg. It might suffice to understand this to read the preface of the book (Halmos 1949) (1949) where Halmos explains how the link between ...
... of Schrödinger (corresponding to a differential equation seating in a Hilbert space) is in fact a economical extension of the finite dimension matrices of Heisenberg. It might suffice to understand this to read the preface of the book (Halmos 1949) (1949) where Halmos explains how the link between ...
electron spin - Project PHYSNET
... S1. Given the orbital and spin angular momentum for given atomic energy levels, label the levels with spectroscopic notation. S2. Given the spectroscopic notation of an atomic energy level, find the orbital and spin angular momentum quantum numbers. ...
... S1. Given the orbital and spin angular momentum for given atomic energy levels, label the levels with spectroscopic notation. S2. Given the spectroscopic notation of an atomic energy level, find the orbital and spin angular momentum quantum numbers. ...
Chapter 8 & 9 PowerPoint
... between metal atoms and the surrounding sea of electrons • Ionic bonding – results from the electrical attraction between positive and negative ions. • Covalent bonding – results from the sharing of electron pairs between two atoms ...
... between metal atoms and the surrounding sea of electrons • Ionic bonding – results from the electrical attraction between positive and negative ions. • Covalent bonding – results from the sharing of electron pairs between two atoms ...
Niels Bohr - Nobel Lecture
... year would be different from its present value. It is quite otherwise in the case of atoms. The definite and unchangeable properties of the elements demand that the state of an atom cannot undergo permanent changes due to external actions. As soon as the atom is left to itself again, its constituent ...
... year would be different from its present value. It is quite otherwise in the case of atoms. The definite and unchangeable properties of the elements demand that the state of an atom cannot undergo permanent changes due to external actions. As soon as the atom is left to itself again, its constituent ...
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.