Probability density, electronic

Probability densities, electron densities and the shape of Is atomic orbitals... 

Here pyy r ) represents the probability density for finding the 1 electrons at r, and e / mutual Coulomb repulsion between electron density at r and r. ... 

The magnitude and shape of such a mean-field potential is shown below [21] in figure B3.1.4 for the two 1 s electrons of a beryllium atom. The Be nucleus is at the origin, and one electron is held fixed 0.13 A from the nucleus, the maximum of the Is orbital s radial probability density. The Coulomb potential experienced by the second electron is then a function of the second electron s position along the v-axis (coimecting the Be nucleus and the first electron) and its distance perpendicular to the v-axis. For simplicity, this second electron... 

By expressing the mean-field interaction of an electron at r with the N- 1 other electrons in temis of a probability density pyy r ) that is independent of the fact that another electron resides at r, the mean-field models ignore spatial correlations among the electrons. In reality, as shown in figure B3.T5 the conditional probability density for finding one ofA - 1 electrons at r, given that one electron is at r depends on r. The absence of a spatial correlation is a direct consequence of the spin-orbital product nature of the mean-field wavefiinctions... 

The principal diagonal of the HMO output matrix is the it electron probability density at atomy, where the summation is over all occupied orbitals. This... 

Basis sets can be further improved by adding new functions, provided that the new functions represent some element of the physics of the actual wave function. Chemical bonds are not centered exactly on nuclei, so polarized functions are added to the basis set leading to an improved basis denoted p, d, or f in such sets as 6-31G(d), etc. Electrons do not have a very high probability density far from the nuclei in a molecule, but the little probability that they do have is important in chemical bonding, hence dijfuse functions, denoted - - as in 6-311 - - G(d), are added in some very high-level basis sets. 

A functional is a function of a function. Electron probability density p is a function p(r) of a point in space located by radius vector r measured from an origin (possibly an atomic mi dens), and the energy E of an electron distribution is a function of its probability density. E /(p). Therefore E is a functional of r denoted E [pfr). ... 

The first approximation we ll consider comes from the interpretation of as a probability density for the electrons within the system. Molecular orbital theory decomposes t(/ into a combination of molecular orbitals <()j, (jij,. To fulfill some of the conditions on we discussed previously, we choose a normalized, orthogonal set of molecular orbitals ... 

This formulation is not just a mathematical trick to form an antisymmetric vravefunction. Quantum mechanics specifies that an electron s location is not deterministic but rather consists of a probability density in this sense, it can he anywhere. This determinant mixes all of the possible orbitals of all of the electrons in the molecular system to form the wavefunction. 

Finally, many of the common molecular electronic properties depend only on the chance of finding any electron in dx and this is obviously m times the above quantities. We focus attention on points in space (written r) and interest ourselves in the electron probability density... 

This vanishing of the probability density for rx — r2 and Ci == C2 means that it is unlikely for two electrons having parallel spins to be in the same place (rx = r2). The phenomenon is called the Fermi hole and we note that it is a direct consequence of the Pauli principle for electrons with the same spin. 

From Eq. 11.62 follows that the two-electron probability density does not show any "Coulomb hole" for pairs of either parallel or antiparallel spins, and this implies that the Hartree scheme is certainly affected by a large correlation error. 

All s-orbitals are independent of the angles 0 and c[>, so we say that they are spherically symmetrical (Fig. 1.31). The probability density of an electron at the point (r,0,ct>) when it is in a ls-orbital is found from the wavefunction for the ground state of the hydrogen atom. When we square the wavefunction (which was given earlier, but can also be constructed as RY from the entries for R and V in Tables 1.2a and 1.2b) we find that... 

FIGURE 1.32 The radial distribution function tells us the probability density for finding an electron at a given radius summed over all directions. The graph shows the radial distribution function for the 1s-, 2s-, and 3s-orbitals in hydrogen. Note how the most probable radius icorresponding to the greatest maximum) increases as n increases. 

FIGURE 1.34 The radial wavefunctions of the first three s-orbitals of a hydrogen atom. Note that the number of radial nodes increases (as n 1), as does the average distance of the electron from the nucleus (compare with Fig. 1.32). Because the probability density is given by ip3, all s-orbitals correspond to a nonzero probability density at the nucleus. 

Two electrons occupy the in-phase combined orbital. The probability density inaeases in the overlap region. Two more electrons occupy the out-of-phase combined orbital and reduce the density there. The decrease is greater than the increase. The electrons are expelled from the overlap region. 

The power dissipated at two different frequencies has been calculated for all reactions and compared with the energy loss to the walls. It is shown that at 65 MHz the fraction of power lost to the boundary decreases by a large amount compared to the situation at 13.56 MHz [224]. In contrast, the power dissipated by electron impact collision increases from nearly 47% to more than 71%, of which vibrational excitation increases by a factor of 2, dissociation increases by 45%, and ionization stays approximately the same, in agreement with the product of the ionization probability per electron, the electron density, and the ion flux, as shown before. The vibrational excitation energy thresholds (0.11 and 0.27 eV) are much smaller than the dissociation (8.3 eV) and ionization (13 eV) ones, and the vibrational excitation cross sections are large too. The reaction rate of processes with a low energy threshold therefore increases more than those with a high threshold. 

All the s orbitals have the spherical harmonic Too(0, q>) as a factor. This spherical harmonic is independent of the angles 0 and spherically symmetric about the origin. Likewise, the electronic probability density is spherically symmetric for s orbitals. 

The radial distribution function Dniir) is the probability density for the electron being in a spherical shell with inner radius r and outer radius r -h dr. For the Is, 2s, and 2p states, these functions are... 

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