Lecture 18 (Slides) October 4
... Schrodinger equation, can be factored into an angular and a radial part if we employ spherical polar coordinates. The use of these coordinates makes it especially easy to locate nodes (regions of zero “electron density”) and to represent 3 dimensional probabilities (i.e. represent in 3 dimensions th ...
... Schrodinger equation, can be factored into an angular and a radial part if we employ spherical polar coordinates. The use of these coordinates makes it especially easy to locate nodes (regions of zero “electron density”) and to represent 3 dimensional probabilities (i.e. represent in 3 dimensions th ...
BASIC CHEMISTRY
... In our biosphere, everything is made of atoms Through the interaction of chemicals we can better understand our biosphere Give an example from what we have already done in Bio. ...
... In our biosphere, everything is made of atoms Through the interaction of chemicals we can better understand our biosphere Give an example from what we have already done in Bio. ...
H - unix.eng.ua.edu
... Eigenvalues of this equation = “electronic energy”. VN is constant for a set of fixed nuclear coordinates. SOLUTION: Wavefunctions invariant to constant terms in H, thus VN can be removed and the eigenvalue = “pure electronic energy” ...
... Eigenvalues of this equation = “electronic energy”. VN is constant for a set of fixed nuclear coordinates. SOLUTION: Wavefunctions invariant to constant terms in H, thus VN can be removed and the eigenvalue = “pure electronic energy” ...
Ch. 3
... going to give up electrons or take in electrons in order to become stable. Positive oxidation numbers mean the atom is going to give up electrons. ...
... going to give up electrons or take in electrons in order to become stable. Positive oxidation numbers mean the atom is going to give up electrons. ...
chem 1411- chapter 7
... get excited to higher energy levels by absorbing energy. This is the excited state of an atom, which is unstable. The electrons then start falling from higher levels to lower levels, releasing energy. This energy when resolved through a spectroscope, we get different lines of specific wavelengths. T ...
... get excited to higher energy levels by absorbing energy. This is the excited state of an atom, which is unstable. The electrons then start falling from higher levels to lower levels, releasing energy. This energy when resolved through a spectroscope, we get different lines of specific wavelengths. T ...
Jan. 23, 2006
... from excited-state atoms emitting a photon and falling down to a lower quantum-number ...
... from excited-state atoms emitting a photon and falling down to a lower quantum-number ...
Elec Structure of Atom
... high energy state to a low energy state; light can be absorbed to excite the electron from a low energy state to a high energy state. The frequency of light emitted or absorbed must be such that hv=the difference in energy between two allowed states of the atom. ...
... high energy state to a low energy state; light can be absorbed to excite the electron from a low energy state to a high energy state. The frequency of light emitted or absorbed must be such that hv=the difference in energy between two allowed states of the atom. ...
Shell model I - Evidence
... Atomic Shell Model By the end of the 1920s, the laws of quantum mechanics had been worked out. They had been applied to the hydrogen atom. They had also been extended to the MULTI-ELECTRON ATOM. This gave the first full understanding of the ...
... Atomic Shell Model By the end of the 1920s, the laws of quantum mechanics had been worked out. They had been applied to the hydrogen atom. They had also been extended to the MULTI-ELECTRON ATOM. This gave the first full understanding of the ...
Document
... •Predictions of wave equations for the position and momentum of electron are based only on probabilities. •The kinetic theory of gases is based on probabilities but this is different because gas molecules were assumed to move in a deterministic way but there were too many molecules to keep track of. ...
... •Predictions of wave equations for the position and momentum of electron are based only on probabilities. •The kinetic theory of gases is based on probabilities but this is different because gas molecules were assumed to move in a deterministic way but there were too many molecules to keep track of. ...
Notetakers
... Example: Calculate the energy required to excite the hydrogen electron from level n=1 to n=2. What wavelength of light and portion of the elecromagnetic spectrum is capable of supplying this amount of energy. ...
... Example: Calculate the energy required to excite the hydrogen electron from level n=1 to n=2. What wavelength of light and portion of the elecromagnetic spectrum is capable of supplying this amount of energy. ...
Lecture 1 Where it all Began
... Wave / particle duality de Broglie (1923) proposed that particles could have wave properties (wave/particle duality). Particles could have an associated wavelength (λ) ...
... Wave / particle duality de Broglie (1923) proposed that particles could have wave properties (wave/particle duality). Particles could have an associated wavelength (λ) ...
Quantum theory
... • Is the ratio between the number of times the e- is in that current position and the total number of times it is at all positions • The higher the probability, the more likely the e- will be found in a given position • The probability plots give a three dimensional shape to a region of space an eis ...
... • Is the ratio between the number of times the e- is in that current position and the total number of times it is at all positions • The higher the probability, the more likely the e- will be found in a given position • The probability plots give a three dimensional shape to a region of space an eis ...
Detailed Notes CH. 6
... Students confuse Bohr’s orbits with orbitals; most spellcheckers do not recognize the word “orbital.” Students mistakenly think that spectral lines represent energy levels; consequently . . . Students have difficulties associating a given line in an emission (or absorption) spectrum with a transitio ...
... Students confuse Bohr’s orbits with orbitals; most spellcheckers do not recognize the word “orbital.” Students mistakenly think that spectral lines represent energy levels; consequently . . . Students have difficulties associating a given line in an emission (or absorption) spectrum with a transitio ...
Recitation Activity 6 (Chem 121) Chapter 6
... Both atoms have 18 electrons with n=3 3. For each of the following “pictures” of an atomic orbital. (a) Give the common name of the orbital type (s, p, d, f, etc.), (b) identify the azimuthal quantum number, (c) Draw the nodal planes if any exist, (d) Give the possible values of the magnetic quantum ...
... Both atoms have 18 electrons with n=3 3. For each of the following “pictures” of an atomic orbital. (a) Give the common name of the orbital type (s, p, d, f, etc.), (b) identify the azimuthal quantum number, (c) Draw the nodal planes if any exist, (d) Give the possible values of the magnetic quantum ...
Atomic orbital
An atomic orbital is a mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom. This function can be used to calculate the probability of finding any electron of an atom in any specific region around the atom's nucleus. The term may also refer to the physical region or space where the electron can be calculated to be present, as defined by the particular mathematical form of the orbital.Each orbital in an atom is characterized by a unique set of values of the three quantum numbers n, ℓ, and m, which respectively correspond to the electron's energy, angular momentum, and an angular momentum vector component (the magnetic quantum number). Any orbital can be occupied by a maximum of two electrons, each with its own spin quantum number. The simple names s orbital, p orbital, d orbital and f orbital refer to orbitals with angular momentum quantum number ℓ = 0, 1, 2 and 3 respectively. These names, together with the value of n, are used to describe the electron configurations of atoms. They are derived from the description by early spectroscopists of certain series of alkali metal spectroscopic lines as sharp, principal, diffuse, and fundamental. Orbitals for ℓ > 3 continue alphabetically, omitting j (g, h, i, k, …).Atomic orbitals are the basic building blocks of the atomic orbital model (alternatively known as the electron cloud or wave mechanics model), a modern framework for visualizing the submicroscopic behavior of electrons in matter. In this model the electron cloud of a multi-electron atom may be seen as being built up (in approximation) in an electron configuration that is a product of simpler hydrogen-like atomic orbitals. The repeating periodicity of the blocks of 2, 6, 10, and 14 elements within sections of the periodic table arises naturally from the total number of electrons that occupy a complete set of s, p, d and f atomic orbitals, respectively.