Lecture 2 - Tufts University
... dimension except that crests and troughs aren't points, but form lines (2D) or planes (3-D) perpendicular to the direction of wave propagation. The Figure shows a plane sine wave in two dimensions. The large arrow is a vector called the wave vector, which defines (1) the direction of wave propagatio ...
... dimension except that crests and troughs aren't points, but form lines (2D) or planes (3-D) perpendicular to the direction of wave propagation. The Figure shows a plane sine wave in two dimensions. The large arrow is a vector called the wave vector, which defines (1) the direction of wave propagatio ...
Chapter 1 Learning Objective Summary
... Chemical reactions involve the gain, loss, or sharing of the outer electrons, whereas nuclear reactions involve changes to the composition of the nucleus. This means that alchemy is possible (though not economical!), because transmutation of one element into another can be accomplished via radioacti ...
... Chemical reactions involve the gain, loss, or sharing of the outer electrons, whereas nuclear reactions involve changes to the composition of the nucleus. This means that alchemy is possible (though not economical!), because transmutation of one element into another can be accomplished via radioacti ...
The principles of transmission electron microscopy image formation
... To understood theory of image formation in TEM, it is necessary to introduce some elements of quantum mechanics. The first element is an electron wave function (EWF), which gives amplitude and phase of an electron wave in given point and time. The square of EWF represents the intensity of electron b ...
... To understood theory of image formation in TEM, it is necessary to introduce some elements of quantum mechanics. The first element is an electron wave function (EWF), which gives amplitude and phase of an electron wave in given point and time. The square of EWF represents the intensity of electron b ...
tutorial 12 - UBC Physics
... is just a símple oscillation, but once we add up these waves in a general wavefunction, we get wavepackets (or more general shapes) that propagate, disperse, etc... . Any superposition of the oscillating pure as ...
... is just a símple oscillation, but once we add up these waves in a general wavefunction, we get wavepackets (or more general shapes) that propagate, disperse, etc... . Any superposition of the oscillating pure as ...
Models of the Hydrogen Atom
... Push the red “O” button on the gun and write down your observations of what happens as the photons pass through the box. Be specific, covering everything you observe. Do your observations match your prediction? ...
... Push the red “O” button on the gun and write down your observations of what happens as the photons pass through the box. Be specific, covering everything you observe. Do your observations match your prediction? ...
Modern Atomic Structure
... Further they fall, more energy, higher frequency. This is simplified the orbitals also have different energies inside energy levels All the electrons can move around. ...
... Further they fall, more energy, higher frequency. This is simplified the orbitals also have different energies inside energy levels All the electrons can move around. ...
COMPCHEM1_2011
... – the lowest energy path between reactants and products is called the intrinsic reaction path ...
... – the lowest energy path between reactants and products is called the intrinsic reaction path ...
Lectures 10-11: Multi-electron atoms System of non
... The + sign in the symmetry column applies if the wave function is symmetric with respect to particle exchange, while the - sign indicates that the wave function is anti-symmetric. The Sz value is indicated by the quantum number for ms, which is obtained by adding the ms values of the two electrons t ...
... The + sign in the symmetry column applies if the wave function is symmetric with respect to particle exchange, while the - sign indicates that the wave function is anti-symmetric. The Sz value is indicated by the quantum number for ms, which is obtained by adding the ms values of the two electrons t ...
File
... • Negatively charged particles located in orbitals • Neutral atoms have same number of electrons and protons • Ions are charged particles – unbalanced – Cation – more protons than electrons = net positive charge – Anion – fewer protons than electrons = net negative charge ...
... • Negatively charged particles located in orbitals • Neutral atoms have same number of electrons and protons • Ions are charged particles – unbalanced – Cation – more protons than electrons = net positive charge – Anion – fewer protons than electrons = net negative charge ...
Atomic Structure Tick Sheet
... I know that PROTONS have a MASS of 1 unit and a charge of +1. I know that NEUTRONS have a MASS of 1 unit and 0 charge. I know that the nucleus is surrounded by very small negative particles called ELECTRONS. I know that ELECTRONS have NEGLIGIBLE MASS and a charge of -1. I know that all ATOMS are ELE ...
... I know that PROTONS have a MASS of 1 unit and a charge of +1. I know that NEUTRONS have a MASS of 1 unit and 0 charge. I know that the nucleus is surrounded by very small negative particles called ELECTRONS. I know that ELECTRONS have NEGLIGIBLE MASS and a charge of -1. I know that all ATOMS are ELE ...
Do your homework on a separate piece of paper, or
... 17. A photosensitive metal has a work function of 3.75 eV. Find the minimum frequency of light needed to free an electron from its surface. hf = = 3.75(1.610-19) = 610-19. 6.6310-34f = 610-19. f = 9.041014 Hz. 18. If a photon having a higher frequency than the one determined in the previous p ...
... 17. A photosensitive metal has a work function of 3.75 eV. Find the minimum frequency of light needed to free an electron from its surface. hf = = 3.75(1.610-19) = 610-19. 6.6310-34f = 610-19. f = 9.041014 Hz. 18. If a photon having a higher frequency than the one determined in the previous p ...
Nature of Atoms Atomic Structure
... • Atoms of a single element that possess different numbers of neutrons • Radioactive isotopes are unstable and emit radiation as the nucleus breaks up ...
... • Atoms of a single element that possess different numbers of neutrons • Radioactive isotopes are unstable and emit radiation as the nucleus breaks up ...
Notes on Atomic Structure atoms
... same proportions (by mass and by number) of its elements This means a given compound always has the same composition, regardless of where it came from. ...
... same proportions (by mass and by number) of its elements This means a given compound always has the same composition, regardless of where it came from. ...
Chemistry 1 Revision: Metals and their uses
... When e.......................... react, their atoms join with other atoms to form ...
... When e.......................... react, their atoms join with other atoms to form ...
inverse quantum states of hydrogen
... which produces an electron spin of [- ½] . To obtain the other spin, we employ the series ...
... which produces an electron spin of [- ½] . To obtain the other spin, we employ the series ...
Facilitator`s Guide PDF
... remain closer to the nucleus. So the 1s orbital fills first, then 2s, then 2p. (Note: This is another way of stating Hund’s rule.) Let’s see why that is. Show participants the visualization of atomic orbitals for hydrogen at http://www.falstad.com/qmatom/. Use the “real orbitals” and start at n=1, m ...
... remain closer to the nucleus. So the 1s orbital fills first, then 2s, then 2p. (Note: This is another way of stating Hund’s rule.) Let’s see why that is. Show participants the visualization of atomic orbitals for hydrogen at http://www.falstad.com/qmatom/. Use the “real orbitals” and start at n=1, m ...
Light, Energy, and More
... Proposed idea that accounted for the fixed energy levels in Bohr’s model ...
... Proposed idea that accounted for the fixed energy levels in Bohr’s model ...
Unit 3 Spiraling
... -Max Planck discovered that atoms in a flame could absorb or emit energy in discrete amounts. This ‘discrete’ amount of energy is called a quantum. An atom is said to be in the ground state when all of its electrons are in the lowest available energy levels. When an electron absorbs energy, it jumps ...
... -Max Planck discovered that atoms in a flame could absorb or emit energy in discrete amounts. This ‘discrete’ amount of energy is called a quantum. An atom is said to be in the ground state when all of its electrons are in the lowest available energy levels. When an electron absorbs energy, it jumps ...
Name - TeacherWeb
... Molecular Orbitals One model of molecular bonding pictures a molecular orbital that is a combination of individual atomic orbitals. A bonding orbital can be occupied by a pair of electrons. In a sigma (σ) bond, the molecular orbital is symmetrical around the axis connecting two atomic nuclei. In a p ...
... Molecular Orbitals One model of molecular bonding pictures a molecular orbital that is a combination of individual atomic orbitals. A bonding orbital can be occupied by a pair of electrons. In a sigma (σ) bond, the molecular orbital is symmetrical around the axis connecting two atomic nuclei. In a p ...
Physics116_L31
... E. Rutherford (1911) bounces “alpha rays” off gold atoms • We now know: α = nucleus of helium: 2 protons + 2 neutrons • “Scattering experiment” = model for modern particle physics – Size of atoms was approximately known from chemistry – He finds: scattering is off a much smaller very dense core (nuc ...
... E. Rutherford (1911) bounces “alpha rays” off gold atoms • We now know: α = nucleus of helium: 2 protons + 2 neutrons • “Scattering experiment” = model for modern particle physics – Size of atoms was approximately known from chemistry – He finds: scattering is off a much smaller very dense core (nuc ...
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.