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Electron orbital

Once the 2s and 2p orbitals are filled the next level is the 3s followed by the 3p 3py and 3p orbitals Electrons in these orbitals are farther from the nucleus than those in the 2s and 2p orbitals and are of higher energy... [Pg.10]

The molecular orbital approach to chemical bonding rests on the notion that as elec trons m atoms occupy atomic orbitals electrons m molecules occupy molecular orbitals Just as our first task m writing the electron configuration of an atom is to identify the atomic orbitals that are available to it so too must we first describe the orbitals avail able to a molecule In the molecular orbital method this is done by representing molec ular orbitals as combinations of atomic orbitals the linear combination of atomic orbitals molecular orbital (LCAO MO) method... [Pg.61]

Its powerful oxidizing properties result from the tight binding of its valence sheU 7-orbital electrons. No commercial source is available. [Pg.235]

The emission of y rays follows, in the majority of cases, what is known as P decay. In the P-decay process, a radionuclide undergoes transmutation and ejects an electron from inside the nucleus (i.e., not an orbital electron). For the purpose of simplicity, positron and electron capture modes are neglected. The resulting transmutated nucleus ends up in an excited nuclear state, which prompdy relaxes by giving offy rays. This is illustrated in Figure 2. [Pg.673]

Bahn, /. way, road, track path orbit trajectory railway breadth (of cloth), bahnbrechend, p.a. pioneer, epoch-making. Bahn-brecher, m. pioneer, -durchmesser, m. orbital diameter, -ebene, /. orbital plane, -elektron, n. orbital electron, bahnen, v.t. beat, smooth, clear (a way). Bahn-hof, m. (railway) station, -impuls, m. linear momentum orbital moment, -sdileife, -schlinge, /., orbital loop, -spur, /, track, -tibergang, m. orbital transition, -zug, m. railway train. [Pg.55]

Volume around nucleus occupied by orbiting electrons... [Pg.4]

There are three common ways by which nuclei can approach the region of stability (1) loss of alpha particles (a-decay) (2) loss of beta particles (/3-decay) (3) capture of an orbital electron. We have already encountered the first type of radioactivity, a-decay, in equation (/0). Emission of a helium nucleus, or alpha particle, is a common form of radioactivity among nuclei with charge greater than 82, since it provides a mechanism by which these nuclei can be converted to new nuclei of lower charge and mass which lie in the belt of stability. The actinides, in particular, are very likely to decay in this way. [Pg.417]

Figure 5. Niels Bohr came up with the idea that the energy of orbiting electrons would be in discrete amounts, or quanta. This enabled him to successfully describe the hydrogen atom, with its single electron, In developing the remainder of his first table of electron configurations, however, Bohr clearly relied on chemical properties, rather than quantum theory, to assign electrons to shells. In this segment of his configuration table, one can see that Bohr adjusted the number of electrons in nitrogen s inner shell in order to make the outer shell, or the reactive shell, reflect the element s known trivalency. Figure 5. Niels Bohr came up with the idea that the energy of orbiting electrons would be in discrete amounts, or quanta. This enabled him to successfully describe the hydrogen atom, with its single electron, In developing the remainder of his first table of electron configurations, however, Bohr clearly relied on chemical properties, rather than quantum theory, to assign electrons to shells. In this segment of his configuration table, one can see that Bohr adjusted the number of electrons in nitrogen s inner shell in order to make the outer shell, or the reactive shell, reflect the element s known trivalency.
For 7-ray energies below 1 MeV (the range of interest) there are two principal modes of interaction with matter — Compton scattering and photoelectron absorption. Compton scattering is the elastic scattering of the 7 photon by an orbital electron in which part of the incident 7-energy is imparted to the recoiling electron. [Pg.380]

Unsaturated organic molecules, such as ethylene, can be chemisorbed on transition metal surfaces in two ways, namely in -coordination or di-o coordination. As shown in Fig. 2.24, the n type of bonding of ethylene involves donation of electron density from the doubly occupied n orbital (which is o-symmetric with respect to the normal to the surface) to the metal ds-hybrid orbitals. Electron density is also backdonated from the px and dM metal orbitals into the lowest unoccupied molecular orbital (LUMO) of the ethylene molecule, which is the empty asymmetric 71 orbital. The corresponding overall interaction is relatively weak, thus the sp2 hybridization of the carbon atoms involved in the ethylene double bond is retained. [Pg.52]

The ground term of the cP configuration is F. That of is also F. Those of and d are " F. We shall discuss these patterns in Section 3.10. For the moment, we only note the common occurrence of F terms and ask how they split in an octahedral crystal field. As for the case of the D term above, which splits like the d orbitals because the angular parts of their electron distributions are related, an F term splits up like a set of / orbital electron densities. A set of real / orbitals is shown in Fig. 3-13. Note how they comprise three subsets. One set of three orbitals has major lobes directed along the cartesian x or y or z axes. Another set comprises three orbitals, each formed by a pair of clover-leaf shapes, concentrated about two of the three cartesian planes. The third set comprises just one member, with lobes directed equally to all eight corners of an inscribing cube. In the free ion, of course, all seven / orbitals are degenerate. In an octahedral crystal field, however, the... [Pg.46]

Electron propagator theory generates a one-electron picture of electronic structure that includes electron correlation. One-electron energies may be obtained reliably for closed-shell molecules with the P3 method and more complex correlation effects can be treated with renormalized reference states and orbitals. To each electron binding energy, there corresponds a Dyson orbital that is a correlated generalization of a canonical molecular orbital. Electron propagator theory enables interpretation of precise ab initio calculations in terms of one-electron concepts. [Pg.49]

The n orbital amplitudes of ethene are identical on both carbons. Unsymmetrical substitutions polarize the n orbital. Electron acceptors or electrophiles attack the carbon with the larger r amplitude. The polarization of frontier orbitals is important for regioselectivities of reactions. Here, mechanism of the n orbital polarization of ethene by methyl substitution [4] is described (Scheme 5). [Pg.60]

C22-0011. Identify the nuclides that decay in the following manner (a) A nuclide undergoes 3 and y decay to give Z = 58 and A = 140 (b) A nuclide undergoes a decay to give polonium-218 and (c) A nuclide captures an orbital electron to give tellurium with 73 neutrons. [Pg.1573]


See other pages where Electron orbital is mentioned: [Pg.2023]    [Pg.10]    [Pg.156]    [Pg.275]    [Pg.410]    [Pg.9]    [Pg.10]    [Pg.156]    [Pg.30]    [Pg.21]    [Pg.293]    [Pg.501]    [Pg.117]    [Pg.381]    [Pg.499]    [Pg.1036]    [Pg.71]    [Pg.286]    [Pg.986]    [Pg.419]    [Pg.427]    [Pg.651]    [Pg.693]    [Pg.19]    [Pg.21]    [Pg.37]    [Pg.381]    [Pg.735]    [Pg.271]    [Pg.563]    [Pg.854]    [Pg.692]    [Pg.21]    [Pg.22]   
See also in sourсe #XX -- [ Pg.305 ]

See also in sourсe #XX -- [ Pg.2 , Pg.10 ]




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Active sites electron orbitals

Algebraic solutions electronic orbital

An orbital explanation of electron-counting rules

Angular momentum electron orbital

Angular momentum electronic orbital, conservation

Antibonding electron orbital

Appendix —Four Electrons Three Orbitals VB Treatment

Approximate Molecular Orbital Theory for 4-Electron 3-Centre Bonding Units

Atom superposition, electron delocalization molecular orbital approach

Atom-superposition electron-delocalization molecular orbital

Atom-superposition electron-delocalization molecular orbital theory

Atomic Orbitals A Quantum Mechanical Description of Electrons Around the Nucleus

Atomic Orbitals, Electron Spin, Linear Combinations

Atomic orbitals allocating electrons

Atomic orbitals electron assignment

Atomic orbitals electron configuration and

Atomic orbitals electron density

Atomic orbitals electron density surfaces

Atomic orbitals electron probability curves

Atomic orbitals electron shells

Atomic orbitals electronic structure calculations

Atomic orbitals valence-shell electron-pair

Atomic orbitals, electron transfer

Atomic orbitals, electron transfer between

Atomic orbitals, electronic configurations and the Periodic Table

Atomic structure orbitals and electronic configurations

Atoms, Electrons, and Orbitals

Availability of electron orbitals in metals and metalloids

Bond Orbitals for Atoms Carrying Unshared Electron Pairs

Bonding molecular orbitals electronic transitions from

Centre Molecular Orbitals and Pauling 3-Electron Bonds

Classical electron orbit

Classifying molecular orbitals and electronic states

Combining the Localized Electron and Molecular Orbital Models

Complex-valued natural orbitals in electron wavepacket dynamics

Confined atoms, electronic structure orbital energies

Core electrons molecular orbital theory

D electron orbital populations

D orbitals electrons

D-orbital electronic configuration

Delocalized Electrons An Explanation Based on Molecular Orbital Theory

Delocalized Molecular Orbital Theory for 4-Electron 3-Centre Bonding Units

Delocalized electrons molecular orbital description

Delta-orbital electron, bonding

Delta-orbital electron, bonding bonds

Diatomic molecule, orbitals electron configuration

Double bond, electronic structure molecular orbitals

Dynamic electron correlation energy orbitals

Dyson orbitals electron propagator calculations

Dyson orbitals, momentum density, electron

Economical description of electron orbitals

Effective one-electron spin-orbit Hamiltonians

Electron Configurations How Electrons Occupy Orbitals

Electron Configurations of the Lanthanides and f Orbitals

Electron Densities and Frontier Orbital Energies

Electron Density Distributions and Molecular Orbitals

Electron Orbital Assignments for Some Transition Elements

Electron Repulsion and Bond Angles. Orbital Hybridization

Electron configuration and orbital hybridization

Electron configuration orbitals

Electron configurations orbital diagrams

Electron configurations orbital wave functions

Electron delocalization molecular orbital

Electron excitation probability atomic orbitals approximation

Electron orbit transition

Electron orbit-nuclear spin interaction

Electron orbital compatibility

Electron orbital dipole moment

Electron orbital levels

Electron orbital models

Electron orbital motions

Electron orbital specificity

Electron orbital transitions

Electron orbital, nuclear magnetic resonance

Electron orbitals

Electron orbitals

Electron orbitals for

Electron orbitals hybrid

Electron orbitals overlapping

Electron orbits occupied

Electron paramagnetic resonance spin-orbit coupling

Electron propagator theory corresponding orbitals

Electron repulsion orbitals, an approximation

Electron spin-orbit energy

Electron transfer orbital interaction

Electron transfer, long range and orbital

Electron transfer, long range and orbital interactions

Electron, orbiting

Electron, orbiting

Electronic Hamiltonian, conical intersections spin-orbit interaction

Electronic charge distribution molecular orbital theory

Electronic conductivity orbital ordering

Electronic configuration molecular orbitals

Electronic configuration orbitals

Electronic coupling frontier molecular orbital interactions

Electronic d orbitals

Electronic density orbital language

Electronic excitation between complementary orbitals

Electronic frontier molecular orbital energy

Electronic magnetic dipole orbital angular momentum

Electronic orbital

Electronic orbital control

Electronic orbits

Electronic structural model fragment orbital type

Electronic structure atomic orbitals

Electronic structure frontier orbitals

Electronic structure representation molecular orbitals

Electronic structure spin-orbit coupling

Electronic transitions between molecular orbitals

Electrons anti-bonding orbitals

Electrons atomic orbitals

Electrons in atomic orbitals

Electrons in d orbitals

Electrons in orbitals

Electrons molecular orbitals and

Electrons occupation of orbitals

Electrons occupy atomic orbitals

Electrons occupying orbitals

Electrons orbital approximation

Electrons orbital shapes

Electrons orbital velocities

Electrons orbits

Electrons relaxed orbitals)

Electrons, valence orbitals

Energies of Atomic Orbitals in Many-Electron Systems

Free, electron molecular orbital theory

Free, electron molecular orbital theory electrons

Free, electron molecular orbital theory energy

Free, electron molecular orbital theory radicals

Free, electron molecular orbital theory valence

Free-electron model highest occupied molecular orbital

Free-electron model lowest unoccupied molecular orbital

Free-electron molecular orbital method FEMO)

Free-electron molecular orbital model

Free-electron molecular orbital model description

Free-electron molecular-orbital

Free-electron molecular-orbital method

Free-electron-nonbonding molecular orbital

Frontier orbital theory electron densities

Full One- and Two-Electron Spin-Orbit Operators

Gauge-including atomic orbital density functional theory, electron

General Form of One-Electron Orbitals in Periodic Potentials— Blochs Theorem

Ground state electron orbitals

Ground-state wave function electronic Hamiltonian, spin-orbit

Highest occupied molecular orbital electron injection

Highest occupied molecular orbital, unpaired electron

Highest occupied molecular orbitals HOMOs). electron promotion

Hiickel molecular orbitals electron configurations

How Are Electrons in Orbitals Represented

How to find electronic orbitals and configurations in NBO output

Hybrid orbitals electron-group geometry

Hybrid orbitals lone electron pairs

ISOTOPES, ELECTRON ORBITALS, AND THE PERIODIC TABLE

Independent-electron models orbital functional theory

K orbital electrons

Ligand orbitals, exchanged electron

Localized electron model hybrid orbitals

Localized electron orbital models

Localized electron orbitals

Localized molecular orbitals many electron correlation effects

Lone pair orbitals adjacent electron rich interactions

Lowest unoccupied molecular orbital electron injection

Lowest unoccupied molecular orbitals LUMOs), electron promotion

Magnetic field orbiting electrons

Many-electron molecular orbital

Many-electron molecular orbital wavefunctions

Many-electron wave functions atomic orbitals approximation

Matrix elements many-electron spin-orbit

Metal orbitals, exchanged electron

Modified free-electron molecular orbital

Molecular Orbital Theory Electron Delocalization

Molecular Orbital Treatment of Many-Electron Systems

Molecular geometry orbitals Valence-shell electron-pair

Molecular orbital A one-electron

Molecular orbital calculation-constrained electron diffraction

Molecular orbital calculations electronic structures

Molecular orbital calculations multiple electronic states

Molecular orbital electron counting rule

Molecular orbital methods electron correlation

Molecular orbital methods electron distribution from

Molecular orbital theory electron correlation

Molecular orbitals , nuclear magnetic density functional theory, electron

Molecular orbitals and electronic

Molecular orbitals and electronic states

Molecular orbitals and electronic transitions

Molecular orbitals electron clouds

Molecular orbitals electron model

Molecular orbitals electron spectra

Molecular orbitals valence shell electron-pair

Molecular-orbital electron configurations

Multi-Electronic Orbitals in the Crystal Field

Multi-electron atoms orbital energy

Numbers of Electrons and Orbitals

One-Electron Molecules and Orbitals

One-Electron, Two-Orbital Interaction

One-electron atoms Atomic orbitals

One-electron orbit

One-electron orbital energies

Orbital (MO) Theory and Electron Delocalization

Orbital Energies and Total Electronic Energy

Orbital Interaction Between a Nucleophilic Radical and an Electron-poor Alkene

Orbital angular momentum of electron

Orbital electron capture

Orbital electron configuration and

Orbital electronic configuration

Orbital energy electron repulsion and

Orbital energy of electrons

Orbital interactions and long-range electron

Orbital interactions four electron

Orbital interactions zero electron

Orbital momentum electron

Orbital ordering, electronic

Orbital properties 77 electron systems

Orbital quantum number multi-electron species

Orbital splitting and electron spin

Orbital total electron density

Orbital vs. Density Electronic Localization in Bonding

Orbitals and Electronic Structure

Orbitals and Hybridization in Electron-Sharing Bonds of Transition Metals

Orbitals and electron pairing in valence-bond theory

Orbitals electron shell

Orbitals electron spin

Orbitals electrons and

Orbitals localized electron model

Orbitals number of electrons

Orbitals of electrons

Orbitals, electronic

Orbitals, exchanged electrons

Outermost electrons orbital

Outermost electrons spherical orbital

P orbital electrons

Pyridine electron orbitals

Radiation, emitted from orbiting electrons

Rydberg electron high orbital angular momentum states

Scenario 2—There is a Single Unpaired Electron in One of the Orbitals

Scenario 6—There are Three Electrons in a Triply Degenerate Orbital

Singly occupied molecular orbital single electron transfer oxidation

Skill 1.3c-Predict molecular geometries using Lewis dot structures and hybridized atomic orbitals, e.g., valence shell electron pair repulsion model (VSEPR)

Spin-orbit coupling conduction electrons

Spin-orbit coupling electron delocalization

Spin-orbit coupling electronic Hamiltonian

Spin-orbit coupling transition metal electronic structure

Spin-orbit interaction electronic Hamiltonian

Spin-orbit interaction various electrons

Surface electron orbitals

The Free-Electron Molecular Orbital Method

The One-electron Bond and Non-paired Spatial Orbital Structures

The Wavefunctions of Many-Electron Atoms Can Be Described to a Good Approximation Using Atomic Orbitals

Three-Electron, Two-Orbital Interaction

Two-component all-electron methods for spin-orbit coupling

Two-electron orbit

Two-orbital-four-electron interaction

Two-step treatment of electron correlation and spin-orbit coupling

Valence bond theory 3 orbitals with 3 electrons

Valence bond theory 6 orbitals with 6 electrons, benzene

Valence electron orbital

Valence electrons molecular orbital mode)

Valence-shell electron-pair repulsion theory orbital hybridization

Virtual orbitals, electron correlation

Wave Properties of Electrons in Orbitals

Zero-Electron, Two-Orbital Interaction

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