Modern Atomic Theory (aka the electron chapter!)
... We need a new theory — now called QUANTUM or WAVE MECHANICS. e- can only exist in certain discrete orbits e- is restricted to QUANTIZED energy state (quanta = bundles of energy) ...
... We need a new theory — now called QUANTUM or WAVE MECHANICS. e- can only exist in certain discrete orbits e- is restricted to QUANTIZED energy state (quanta = bundles of energy) ...
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... Dark fringe: (x,y,z,t)2 small , possibility small 。 (x,y,z,t)2 is proportion to possibility density in this point. ...
... Dark fringe: (x,y,z,t)2 small , possibility small 。 (x,y,z,t)2 is proportion to possibility density in this point. ...
Worksheet 4 - Periodic Trends A number of physical and chemical
... When an electron is removed from an atom the repulsion between the remaining electrons decreases. The nuclear charge remains constant, so more energy is required to remove another electron from the positively charged ion. This means that, I1 < I2 < I3 < ..., for any given atom. Going down a group t ...
... When an electron is removed from an atom the repulsion between the remaining electrons decreases. The nuclear charge remains constant, so more energy is required to remove another electron from the positively charged ion. This means that, I1 < I2 < I3 < ..., for any given atom. Going down a group t ...
Handout 1: A More Detailed Look at Electronic Structure.
... Spin and orbital angular momenta can interact (couple) with one another and states which have different values for the combined angular momentum will differ in energy. Ligand electrical fields can restrict the motion of electrons about the nucleus thus quenching the orbital angular momentum and grea ...
... Spin and orbital angular momenta can interact (couple) with one another and states which have different values for the combined angular momentum will differ in energy. Ligand electrical fields can restrict the motion of electrons about the nucleus thus quenching the orbital angular momentum and grea ...
Lectures 7-9 - U of L Class Index
... The orbital angular momentum of electrons in an atom is quantized (i.e. has a fixed set of allowed values). Only orbitals whose angular momentum is an integer multiple of h/2p are “allowed”. These orbitals are called stationary states. The emission or absorption of light occurs when electrons ‘jump’ ...
... The orbital angular momentum of electrons in an atom is quantized (i.e. has a fixed set of allowed values). Only orbitals whose angular momentum is an integer multiple of h/2p are “allowed”. These orbitals are called stationary states. The emission or absorption of light occurs when electrons ‘jump’ ...
Planck`s quantum theory
... Where (Ze) is the charge of the nucleus and (e) is the charge on the electron. The distance between the mucleus and the electron is r. You can see that this potential depends on only the distance between the nucleus and the electron and not the coordinates (x,y,z). Such a “central potential” suggest ...
... Where (Ze) is the charge of the nucleus and (e) is the charge on the electron. The distance between the mucleus and the electron is r. You can see that this potential depends on only the distance between the nucleus and the electron and not the coordinates (x,y,z). Such a “central potential” suggest ...
Lectures 7-9
... The orbital angular momentum of electrons in an atom is quantized (i.e. has a fixed set of allowed values). Only orbitals whose angular momentum is an integer multiple of h/2p are “allowed”. These orbitals are called stationary states. The emission or absorption of light occurs when electrons ‘jump’ ...
... The orbital angular momentum of electrons in an atom is quantized (i.e. has a fixed set of allowed values). Only orbitals whose angular momentum is an integer multiple of h/2p are “allowed”. These orbitals are called stationary states. The emission or absorption of light occurs when electrons ‘jump’ ...
Unit 4 Notes
... F. Why does it matter that an electron behaves as both particle and wave? 1) The fact that electrons behave as waves leads to some odd observations, like: 2) Heisenberg’s uncertainty principle- it is impossible to know exactly both the of a particle at the same time. a. This limitation is critical i ...
... F. Why does it matter that an electron behaves as both particle and wave? 1) The fact that electrons behave as waves leads to some odd observations, like: 2) Heisenberg’s uncertainty principle- it is impossible to know exactly both the of a particle at the same time. a. This limitation is critical i ...
Ch. 2 Chemistry
... Consists of a certain kind of atom that is different from those of other elements ...
... Consists of a certain kind of atom that is different from those of other elements ...
Chapter1011
... • Polar or Non-Polar? – In very symmetrical structures (e.g. CO2 or CF4), the individual bond dipoles effectively cancel each other and the molecule is ...
... • Polar or Non-Polar? – In very symmetrical structures (e.g. CO2 or CF4), the individual bond dipoles effectively cancel each other and the molecule is ...
Document
... ''Lowest excited levels". It remains in that state for an average time of 1.610-8 s before it makes a transition back to a ground state, emitting a photon with wavelength 589.0 nm and energy 2.105 eV. What is the uncertainty in energy of that excited state? What is the wavelength spread of the corr ...
... ''Lowest excited levels". It remains in that state for an average time of 1.610-8 s before it makes a transition back to a ground state, emitting a photon with wavelength 589.0 nm and energy 2.105 eV. What is the uncertainty in energy of that excited state? What is the wavelength spread of the corr ...
Chapter 2: The Chemical Context of Life
... Electrons are not always symmetrically distributed in such a molecule and may accumulate by chance in one part of the molecule, resulting in regions of positive and negative charges. These ever-changing regions of positive and negative charge enable all atoms and molecules to stick to one another. T ...
... Electrons are not always symmetrically distributed in such a molecule and may accumulate by chance in one part of the molecule, resulting in regions of positive and negative charges. These ever-changing regions of positive and negative charge enable all atoms and molecules to stick to one another. T ...
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.