Solid-state quantum computing using spectral holes M. S. Shahriar, P. R. Hemmer,
... single-particle Raman transitions. Consider a situation where each atom has a ⌳-type transition, with two nondegenerate spin states coupled to a single optically excited state, as shown in Fig. 1. For two atoms separated by a frequency matching the energy difference between the low-lying states, cho ...
... single-particle Raman transitions. Consider a situation where each atom has a ⌳-type transition, with two nondegenerate spin states coupled to a single optically excited state, as shown in Fig. 1. For two atoms separated by a frequency matching the energy difference between the low-lying states, cho ...
Book-Abstracts - The Fritz Haber Center for Molecular dynamics
... Ab initio calculations of high dimensional potential energy surfaces (PES) for ground and excited states of the CO/Cr2O3(0001) will be presented. The surface model consists of a small cluster embedded in a semiinfinite array of point charges to simulate the electrostatic field above the surface. Bas ...
... Ab initio calculations of high dimensional potential energy surfaces (PES) for ground and excited states of the CO/Cr2O3(0001) will be presented. The surface model consists of a small cluster embedded in a semiinfinite array of point charges to simulate the electrostatic field above the surface. Bas ...
BSPH 111 - Refresher Chemistry
... An atom consists of a nucleus of protons and neutrons, surrounded by electrons. Each of the elements in the periodic table is classified according to its atomic number, which is the number of protons in that element's nucleus. Protons have a charge of +1, electrons have a charge of -1, and neutrons ...
... An atom consists of a nucleus of protons and neutrons, surrounded by electrons. Each of the elements in the periodic table is classified according to its atomic number, which is the number of protons in that element's nucleus. Protons have a charge of +1, electrons have a charge of -1, and neutrons ...
Atomic structure and periodic table
... A periodic table is a horizontal and vertical arrangement of elements according to their atomic numbers. This table was successfully arranged in 1913 by the British scientist Henry Moseley from the previous work of the Russian Scientist Dmitri Mendeleev. The horizontal arrangement forms period. Atom ...
... A periodic table is a horizontal and vertical arrangement of elements according to their atomic numbers. This table was successfully arranged in 1913 by the British scientist Henry Moseley from the previous work of the Russian Scientist Dmitri Mendeleev. The horizontal arrangement forms period. Atom ...
W(CO)
... were also varied. According to the thermodynamic data from NIST,[10] ΔHf(CO) = −110.53 kJ/mole, ΔH(W) = 851.03 kJ/mole, and ΔHf[W(CO)6] = −882.9 kJ/mole, which gives a thermodynamic mean BDE(W–CO) value of 1.85 eV3 that is consistent with the value calculated here for t1 = 0 (1.84 eV). All the other ...
... were also varied. According to the thermodynamic data from NIST,[10] ΔHf(CO) = −110.53 kJ/mole, ΔH(W) = 851.03 kJ/mole, and ΔHf[W(CO)6] = −882.9 kJ/mole, which gives a thermodynamic mean BDE(W–CO) value of 1.85 eV3 that is consistent with the value calculated here for t1 = 0 (1.84 eV). All the other ...
Transitions between highly excited states of an atom when a neutral
... whelming majority of the recent theoretical and experimental studies of l-mixing (see Refs. 14-23 and the review'). The analysis presented here leads to the following basic conclusion: for transitions with change n-tn' of the principal quantum number there can occur a situation which is the inverse ...
... whelming majority of the recent theoretical and experimental studies of l-mixing (see Refs. 14-23 and the review'). The analysis presented here leads to the following basic conclusion: for transitions with change n-tn' of the principal quantum number there can occur a situation which is the inverse ...
e - Physlab
... 9. An electron is held in orbit about a proton by electrostatic attraction. (a) Assume that an “orbiting electron wave” has the same energy an orbiting particle would have if at radius r and of momentum mv. Write an expression for this energy. (b) If the electron behaves as a classical particle, it ...
... 9. An electron is held in orbit about a proton by electrostatic attraction. (a) Assume that an “orbiting electron wave” has the same energy an orbiting particle would have if at radius r and of momentum mv. Write an expression for this energy. (b) If the electron behaves as a classical particle, it ...
Peeking and poking at atoms with laser light
... characterisation from people like Fraunhofer, Kirchoff, Bunsen, Balmer, and Zeeman followed, but it was not until 1913, with the introduction of the Rutherford-Bohr atomic model, that a cornerstone was laid for what would become a quantum mechanical description of the atom. ...
... characterisation from people like Fraunhofer, Kirchoff, Bunsen, Balmer, and Zeeman followed, but it was not until 1913, with the introduction of the Rutherford-Bohr atomic model, that a cornerstone was laid for what would become a quantum mechanical description of the atom. ...
`Bound` states of an electron in the far
... is undoubtedly the most celebrated problem in atomic physics (the hydrogen atom), but the motion of an electron in the field of an electric dipole does not seem to have been studied at all. There is indeed good reason for this: no nucleus has a measurable electric dipole moment. Nuclei do have magne ...
... is undoubtedly the most celebrated problem in atomic physics (the hydrogen atom), but the motion of an electron in the field of an electric dipole does not seem to have been studied at all. There is indeed good reason for this: no nucleus has a measurable electric dipole moment. Nuclei do have magne ...
Luminescence spectroscopy
... choices including emission of a photon to give fluorescence, radiationless deactivation to ground state, or intersystem crossing (ISC). The process of intersystem crossing involves transfer of the electron from an excited singlet to a triplet state. This process can actually take place since the vib ...
... choices including emission of a photon to give fluorescence, radiationless deactivation to ground state, or intersystem crossing (ISC). The process of intersystem crossing involves transfer of the electron from an excited singlet to a triplet state. This process can actually take place since the vib ...
Oxidation numbers
... metals. They are also oxidized by nonmetals, losing their electrons to the nonmetal and forming ionic compounds. However, many Transition metals exhibit multiple oxidation states, forming cations with different positive charges. This is due to the fact that many Transition Metals are characterized b ...
... metals. They are also oxidized by nonmetals, losing their electrons to the nonmetal and forming ionic compounds. However, many Transition metals exhibit multiple oxidation states, forming cations with different positive charges. This is due to the fact that many Transition Metals are characterized b ...
Feasible Nanometric Magnetoresistance Devices
... approximation, the molecular orbital energy (at B ) 0) is given by an effective mass model Em ≈ h2m2/2µ*L2, m ) 0, (1, ..., where µ* is the effective mass. Thus, by changing the gate potential Vg we select a molecular orbital with an approximate momentum hm/L through which conductance takes place. I ...
... approximation, the molecular orbital energy (at B ) 0) is given by an effective mass model Em ≈ h2m2/2µ*L2, m ) 0, (1, ..., where µ* is the effective mass. Thus, by changing the gate potential Vg we select a molecular orbital with an approximate momentum hm/L through which conductance takes place. I ...
Final Exam Practice Problems: R = 0.0821 Latm/molK NA = 6.022
... 2. A substance that can't be chemically broken down into simpler substances is considered to be A) a homogeneous mixture. B) an element. C) a heterogeneous mixture. D) a compound. E) an electron. 3. Which of the following are examples of a chemical change? A) coffee brewing B) water boiling C) leave ...
... 2. A substance that can't be chemically broken down into simpler substances is considered to be A) a homogeneous mixture. B) an element. C) a heterogeneous mixture. D) a compound. E) an electron. 3. Which of the following are examples of a chemical change? A) coffee brewing B) water boiling C) leave ...
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.