Quantum-Mechanical Model of the Atom
... things at the atomic/molecular level! • We shall see that, in fact, we can visualize things as standing waves. ...
... things at the atomic/molecular level! • We shall see that, in fact, we can visualize things as standing waves. ...
2s - Chemistry
... orbitals that can be produced by the overlap of atomic orbitals. Head-on overlap of atomic orbitals produces (sigma) orbitals. Side-on overlap of atomic orbitals produces (pi) orbitals. Two 1s atomic orbitals that overlap produce two molecular orbitals designated as: 1s or bonding molecular orb ...
... orbitals that can be produced by the overlap of atomic orbitals. Head-on overlap of atomic orbitals produces (sigma) orbitals. Side-on overlap of atomic orbitals produces (pi) orbitals. Two 1s atomic orbitals that overlap produce two molecular orbitals designated as: 1s or bonding molecular orb ...
South Pasadena · Chemistry
... 4. There are five 4d orbitals. List the quantum numbers for each orbital. n l ml ...
... 4. There are five 4d orbitals. List the quantum numbers for each orbital. n l ml ...
Quantum Theory of Atoms and Molecules
... properties of elementary particles (electrons etc.), atoms and molecules, to describe some of the important physical and chemical applications of this theory, and to provide an elementary understanding of atomic and molecular spectroscopy. The lectures also cover essential material on electrostatics ...
... properties of elementary particles (electrons etc.), atoms and molecules, to describe some of the important physical and chemical applications of this theory, and to provide an elementary understanding of atomic and molecular spectroscopy. The lectures also cover essential material on electrostatics ...
Electron Configurations
... So you learned about the Bohr model of an atom as well the electronic configuration of that atom. If you have taken or are taking any sort of an advanced chemistry class, then you probably didn’t have much trouble with these concepts. Otherwise, you may want some extra information on the subject. Mo ...
... So you learned about the Bohr model of an atom as well the electronic configuration of that atom. If you have taken or are taking any sort of an advanced chemistry class, then you probably didn’t have much trouble with these concepts. Otherwise, you may want some extra information on the subject. Mo ...
Chapter 6 review
... higher energy levels are acting more like standing waves than like particles. • Schrödinger looked at the wave function of the electron. This wave function describes the electron’s orbital. ...
... higher energy levels are acting more like standing waves than like particles. • Schrödinger looked at the wave function of the electron. This wave function describes the electron’s orbital. ...
energy levels.
... P Orbitals There are 3 sub orbitals Each contains 2 electrons totals electrons = 6 groups 13-18 on the periodic table are p orbitals ...
... P Orbitals There are 3 sub orbitals Each contains 2 electrons totals electrons = 6 groups 13-18 on the periodic table are p orbitals ...
Electronic Structure of Atoms (i.e., Quantum Mechanics)
... This image shows a ring of 76 iron atoms on a copper (111) surface. Electrons on this surface form a two-dimensional electron gas and scatter from the iron atoms but are confined by boundary or "corral." The wave pattern in the interior is due to the density distribution of the trapped electrons.The ...
... This image shows a ring of 76 iron atoms on a copper (111) surface. Electrons on this surface form a two-dimensional electron gas and scatter from the iron atoms but are confined by boundary or "corral." The wave pattern in the interior is due to the density distribution of the trapped electrons.The ...
Chapter 9 – Many Electron Atoms
... In practice one uses a basis set. The accuracy of a HF calculation is limited by the size of the basis set. Hartree-‐Fock results can be qualitatively wrong when you expect degeneracies between gr ...
... In practice one uses a basis set. The accuracy of a HF calculation is limited by the size of the basis set. Hartree-‐Fock results can be qualitatively wrong when you expect degeneracies between gr ...
course materials
... surfaces and of molecule-surface interactions. For molecules a much-used approximation is molecular orbital (MO) theory, similarly, for crystalline solids and surfaces a widely used approximation is band theory. For molecules point group symmetry can be used to make the computations easier and also ...
... surfaces and of molecule-surface interactions. For molecules a much-used approximation is molecular orbital (MO) theory, similarly, for crystalline solids and surfaces a widely used approximation is band theory. For molecules point group symmetry can be used to make the computations easier and also ...
Modern Model of the Atom
... aufbau principle: electrons fill the lowest energy orbitals first Pauli exclusion principle: no two electrons in an atom can have the same four quantum numbers Hund’s rule: every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons ...
... aufbau principle: electrons fill the lowest energy orbitals first Pauli exclusion principle: no two electrons in an atom can have the same four quantum numbers Hund’s rule: every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons ...
Lecture 5 Molecular Orbital Theory Part 1 Molecular Orbital Theory
... • When the constituent AOs are in phase the result is a bonding orbital • This MO can accommodate two electrons (usually one from each atom). • The energy of the MO is lower than the energy of the two constituent AOs, so placing two electrons in such an orbital results in a net stabilisation of the ...
... • When the constituent AOs are in phase the result is a bonding orbital • This MO can accommodate two electrons (usually one from each atom). • The energy of the MO is lower than the energy of the two constituent AOs, so placing two electrons in such an orbital results in a net stabilisation of the ...
Population Analysis
... and basis function n on center l is 2 Pµ k ;ν l ∆ µ k ;ν l where the factor of two obtains because P and D are symmetric. Example An SCF calculation (using GAUSSIAN98) on CH2O using a 6-31g* basis set (at the optimal SCF geometry) results in the following N(m,n) array. Condensed to atoms (all electr ...
... and basis function n on center l is 2 Pµ k ;ν l ∆ µ k ;ν l where the factor of two obtains because P and D are symmetric. Example An SCF calculation (using GAUSSIAN98) on CH2O using a 6-31g* basis set (at the optimal SCF geometry) results in the following N(m,n) array. Condensed to atoms (all electr ...
Test 4
... Chapter 8 1) Define, identify and/or give examples of: electron configuration, Aufbau Principle, Hund’s Rule, Pauli Exclusion Principle, ground state, excited state, degenerate orbital, shielding, effective nuclear charge, valence electrons, valence shell, s, p, d, & f block, atomic radius, periodic ...
... Chapter 8 1) Define, identify and/or give examples of: electron configuration, Aufbau Principle, Hund’s Rule, Pauli Exclusion Principle, ground state, excited state, degenerate orbital, shielding, effective nuclear charge, valence electrons, valence shell, s, p, d, & f block, atomic radius, periodic ...
Chapter 6.8 - Periodic Trends
... a. increasing when progressing across a row from left to right b. decreasing when progressing across a row from left to right c. increasing when progressing down a column from top to bottom d. decreasing when progressing down a column from top to bottom ...
... a. increasing when progressing across a row from left to right b. decreasing when progressing across a row from left to right c. increasing when progressing down a column from top to bottom d. decreasing when progressing down a column from top to bottom ...
Slide 1
... overlap with each other. • Consider methane, CH4. The sp3 hybrid orbitals of carbon each point to a 1s orbital of hydrogen and, therefore, we add and subtract these atomic orbitals to create molecular orbitals. • As with H2, one resulting MO is lower in energy than the separated atomic orbitals, and ...
... overlap with each other. • Consider methane, CH4. The sp3 hybrid orbitals of carbon each point to a 1s orbital of hydrogen and, therefore, we add and subtract these atomic orbitals to create molecular orbitals. • As with H2, one resulting MO is lower in energy than the separated atomic orbitals, and ...
Molecular orbital
In chemistry, a molecular orbital (or MO) is a mathematical function describing the wave-like behavior of an electron in a molecule. This function can be used to calculate chemical and physical properties such as the probability of finding an electron in any specific region. The term orbital was introduced by Robert S. Mulliken in 1932 as an abbreviation for one-electron orbital wave function. At an elementary level, it is used to describe the region of space in which the function has a significant amplitude. Molecular orbitals are usually constructed by combining atomic orbitals or hybrid orbitals from each atom of the molecule, or other molecular orbitals from groups of atoms. They can be quantitatively calculated using the Hartree–Fock or self-consistent field (SCF) methods.