This intrinsic angular momentum is called spin angular momentum, or simply spin, since it is possible to picture it as being due to the electron spinning around its own axis. The spin angular momentum of the electron is fixed and a magnitude of ℏ√3 / 4, corresponding to a half-integer quantum number, s = 1 / 2. Angular Momentum States. P.5.July 27, 1999 measuarble values of the spin on the z axis will bear a simple relationship to the quantum number MS. According to the laws of quantum mechanics spin angular momentum is. The magnitude of spin angular momentum of an electron is given by s (s + 1) 2 π h For a single electron s = ± 2 1 but for calculating spin angular momentum of an electron on positive value of s is taken. Addition of angular momentum April 21, 2015 Often we need to combine different sources of angular momentum to characterize the total angular momentum of a system, or to divide the total angular momentum into parts to evaluate the effect of a.
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Spin Angular Momentum Formula
- Survey of optical spectroscopy
- General principles
- Practical considerations
- Types of electromagnetic-radiation sources
- Methods of dispersing spectra
- Foundations of atomic spectra
- Hydrogen atom states
- The periodic table
- Molecular spectroscopy
- Theory of molecular spectra
- Fields of molecular spectroscopy
- Microwave spectroscopy
- Infrared spectroscopy
- Visible and ultraviolet spectroscopy
- Fluorescence and phosphorescence
- Laser spectroscopy
- X-ray and radio-frequency spectroscopy
- X-ray spectroscopy
- Production methods
- Radio-frequency spectroscopy
- X-ray spectroscopy
- Resonance-ionization spectroscopy
- Ionization processes
- Resonance-ionization mass spectrometry
- RIS atomization methods
- Additional applications of RIS
For atoms in the first three rows and those in the first two columns of the periodic table, the atom can be described in terms of quantum numbers giving the total orbital angular momentum and total spin angular momentum of a given state. The total orbital angular momentum is the sum of the orbital angular momenta from each of the electrons; it has magnitude Square root of√L(L + 1) (ℏ), in which L is an integer. The possible values of L depend on the individual l values and the orientations of their orbits for all the electrons composing the atom. The total spin momentum has magnitude Square root of√S(S + 1) (ℏ), in which S is an integer or half an odd integer, depending on whether the number of electrons is even or odd. The possible value of the total spin angular momentum can be found from all the possible orientations of electrons within the atom. In summing the L and S values, only the electrons in unfilled shells (typically the outermost, or valence, shell) need be considered: in a closed subshell, there are as many electrons with spins oriented in one direction as there are with spins in the opposite direction, with the result that their orbital and spin momenta add up to zero. Thus, only electrons in unfilled shells contribute angular momentum to the whole atom. For light atoms and heavier atoms with just a few electrons outside the inner closed shells, the total angular momentum is approximately given by the vector sum of the total of orbital angular momentum and the total spin angular momentum. The total angular momentum has the magnitude Square root of√J(J + 1) (ℏ), in which J can take any positive value from L + S to |L − S| in integer steps; i.e., if L = 1 and S = 3/2, J can be 5/2, 3/2, or 1/2. The remaining quantum number, mJ, specifies the orientation of the atom as a whole; mJ can take any value from +J to −J in integer steps. A term is the set of all states with a given configuration: L, S, and J.
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If the total angular momentum can be expressed approximately as the vector sum of the total orbital and spin angular momenta, the assignment is called the L-S coupling, or Russell-Saunders coupling (after the astronomer Henry Norris Russell and the physicist Frederick A. Saunders, both of the United States).
For heavier atoms, magnetic interactions among the electrons often contrive to make L and S poorly defined. The total angular momentum quantum numbers J and mJ remain constant quantities for a given state of an atom, but their values can no longer be generated by the addition of the L and S values. A coupling scheme known as jj coupling is sometimes applicable. In this scheme, each electronn is assigned an angular momentum j composed of its orbital angular momentum l and its spin s. The total angular momentum J is then the vector addition of j1 + j2 + j3 +…, where each jn is due to a single electron.
Atomic transitions
An isolated atom or ion in some excited state spontaneously relaxes to a lower state with the emission of one or more photons, thus ultimately returning to its ground state. In an atomic spectrum, each transition corresponding to absorption or emission of energy will account for the presence of a spectral line. Quantum mechanics prescribes a means of calculating the probability of making these transitions. The lifetimes of the excited states depend on specific transitions of the particular atom, and the calculation of the spontaneous transition between two states of an atom requires that the wave functions of both states be known.
The possible radiative transitions are classified as either allowed or forbidden, depending on the probability of their occurrence. In some instances, as, for example, when both the initial and final states have a total angular momentum equal to zero, there can be no single photon transition between states of any kind. The allowed transitions obey certain restrictions, known as selection rules: the J value of the atom can change by unity or zero, and if L and S are well defined within the atom, the change in L is also restricted to 0 or ±1 while S cannot change at all. The time required for an allowed transition varies as the cube of the wavelength of the photon; for a transition in which a photon of visible light (wavelength of approximately 500 nanometres) is emitted, a characteristic emission time is 1–10 nanoseconds (10−9 second).
Forbidden transitions proceed slowly compared to the allowed transitions, and the resulting spectral emission lines are relatively weak. For atoms in about the first third of the periodic table, the L and S selection rules provide useful criteria for the classification of unknown spectral lines. In heavier atoms, greater magnetic interactions among electrons cause L and S to be poorly defined, and these selection rules are less applicable. Occasionally, excited states are found that have lifetimes much longer than the average because all the possible transitions to lower energy states are forbidden transitions. Such states are called metastable and can have lifetimes in excess of minutes.
Perturbations of levels
This intrinsic angular momentum is called spin angular momentum, or simply spin, since it is possible to picture it as being due to the electron spinning around its own axis. The spin angular momentum of the electron is fixed and a magnitude of ℏ√3 / 4, corresponding to a half-integer quantum number, s = 1 / 2. Angular Momentum States. P.5.July 27, 1999 measuarble values of the spin on the z axis will bear a simple relationship to the quantum number MS. According to the laws of quantum mechanics spin angular momentum is. The magnitude of spin angular momentum of an electron is given by s (s + 1) 2 π h For a single electron s = ± 2 1 but for calculating spin angular momentum of an electron on positive value of s is taken. Addition of angular momentum April 21, 2015 Often we need to combine different sources of angular momentum to characterize the total angular momentum of a system, or to divide the total angular momentum into parts to evaluate the effect of a.
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Spin Angular Momentum Formula
- Survey of optical spectroscopy
- General principles
- Practical considerations
- Types of electromagnetic-radiation sources
- Methods of dispersing spectra
- Foundations of atomic spectra
- Hydrogen atom states
- The periodic table
- Molecular spectroscopy
- Theory of molecular spectra
- Fields of molecular spectroscopy
- Microwave spectroscopy
- Infrared spectroscopy
- Visible and ultraviolet spectroscopy
- Fluorescence and phosphorescence
- Laser spectroscopy
- X-ray and radio-frequency spectroscopy
- X-ray spectroscopy
- Production methods
- Radio-frequency spectroscopy
- X-ray spectroscopy
- Resonance-ionization spectroscopy
- Ionization processes
- Resonance-ionization mass spectrometry
- RIS atomization methods
- Additional applications of RIS
For atoms in the first three rows and those in the first two columns of the periodic table, the atom can be described in terms of quantum numbers giving the total orbital angular momentum and total spin angular momentum of a given state. The total orbital angular momentum is the sum of the orbital angular momenta from each of the electrons; it has magnitude Square root of√L(L + 1) (ℏ), in which L is an integer. The possible values of L depend on the individual l values and the orientations of their orbits for all the electrons composing the atom. The total spin momentum has magnitude Square root of√S(S + 1) (ℏ), in which S is an integer or half an odd integer, depending on whether the number of electrons is even or odd. The possible value of the total spin angular momentum can be found from all the possible orientations of electrons within the atom. In summing the L and S values, only the electrons in unfilled shells (typically the outermost, or valence, shell) need be considered: in a closed subshell, there are as many electrons with spins oriented in one direction as there are with spins in the opposite direction, with the result that their orbital and spin momenta add up to zero. Thus, only electrons in unfilled shells contribute angular momentum to the whole atom. For light atoms and heavier atoms with just a few electrons outside the inner closed shells, the total angular momentum is approximately given by the vector sum of the total of orbital angular momentum and the total spin angular momentum. The total angular momentum has the magnitude Square root of√J(J + 1) (ℏ), in which J can take any positive value from L + S to |L − S| in integer steps; i.e., if L = 1 and S = 3/2, J can be 5/2, 3/2, or 1/2. The remaining quantum number, mJ, specifies the orientation of the atom as a whole; mJ can take any value from +J to −J in integer steps. A term is the set of all states with a given configuration: L, S, and J.
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If the total angular momentum can be expressed approximately as the vector sum of the total orbital and spin angular momenta, the assignment is called the L-S coupling, or Russell-Saunders coupling (after the astronomer Henry Norris Russell and the physicist Frederick A. Saunders, both of the United States).
For heavier atoms, magnetic interactions among the electrons often contrive to make L and S poorly defined. The total angular momentum quantum numbers J and mJ remain constant quantities for a given state of an atom, but their values can no longer be generated by the addition of the L and S values. A coupling scheme known as jj coupling is sometimes applicable. In this scheme, each electronn is assigned an angular momentum j composed of its orbital angular momentum l and its spin s. The total angular momentum J is then the vector addition of j1 + j2 + j3 +…, where each jn is due to a single electron.
Atomic transitions
An isolated atom or ion in some excited state spontaneously relaxes to a lower state with the emission of one or more photons, thus ultimately returning to its ground state. In an atomic spectrum, each transition corresponding to absorption or emission of energy will account for the presence of a spectral line. Quantum mechanics prescribes a means of calculating the probability of making these transitions. The lifetimes of the excited states depend on specific transitions of the particular atom, and the calculation of the spontaneous transition between two states of an atom requires that the wave functions of both states be known.
The possible radiative transitions are classified as either allowed or forbidden, depending on the probability of their occurrence. In some instances, as, for example, when both the initial and final states have a total angular momentum equal to zero, there can be no single photon transition between states of any kind. The allowed transitions obey certain restrictions, known as selection rules: the J value of the atom can change by unity or zero, and if L and S are well defined within the atom, the change in L is also restricted to 0 or ±1 while S cannot change at all. The time required for an allowed transition varies as the cube of the wavelength of the photon; for a transition in which a photon of visible light (wavelength of approximately 500 nanometres) is emitted, a characteristic emission time is 1–10 nanoseconds (10−9 second).
Forbidden transitions proceed slowly compared to the allowed transitions, and the resulting spectral emission lines are relatively weak. For atoms in about the first third of the periodic table, the L and S selection rules provide useful criteria for the classification of unknown spectral lines. In heavier atoms, greater magnetic interactions among electrons cause L and S to be poorly defined, and these selection rules are less applicable. Occasionally, excited states are found that have lifetimes much longer than the average because all the possible transitions to lower energy states are forbidden transitions. Such states are called metastable and can have lifetimes in excess of minutes.
Perturbations of levels
The energies of atomic levels are affected by external magnetic and electric fields in which atoms may be situated. A magnetic field causes an atomic level to split into its states of different mJ, each with slightly different energy; this effect is known as the Zeeman effect (after Pieter Zeeman, a Dutch physicist). The result is that each spectral line separates into several closely spaced lines. The number and spacing of such lines depend on the J values for the levels involved; hence, the Zeeman effect is often used to identify the J values of levels in complex spectra. The corresponding effect of line splitting caused by the application of a strong electric field is known as the Stark effect.
Small modifications to electronic energy levels arise because of the finite mass, nonzero volume of the atomic nucleus and the distribution of charges and currents within the nucleus. The resulting small energy changes, called hyperfine structure, are used to obtain information about the properties of nuclei and the distribution of the electron clouds near nuclei. Systematic changes in level positions are seen as the number of neutrons in a nucleus is increased. These effects are known as isotope shifts and form the basis for laserisotope separation. For light atoms, the isotope shift is primarily due to differences in the finite mass of the nucleus. For heavier atoms, the main contribution comes from the fact that the volume of the nucleus increases as the number of neutrons increases. The nucleus may behave as a small magnet because of internal circulating currents; the magnetic fields produced in this way may affect the levels slightly. If the electric field outside the nucleus differs from that which would exist if the nucleus were concentrated at a point, this difference also can affect the energy levels of the surrounding electrons (see belowRadio-frequency spectroscopy).
Spin Angular Momentum Wiki
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