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Physical Review

Pictorial Representations of the Dirac Electron Cloud for Hydrogen-Like Atoms

Harvey E. White

Published Aug 1, 1931• 34 citations
Publisher

Abstract

Previous attempts to represent graphically the Schrodinger electron cloud for hydrogen-like atoms have been so successful that similar graphical representations have been looked for on the Dirac theory. With a single electron specified on Dirac's theory by a set of four wave functions instead of one, the probability density $\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}={\ensuremath{\psi}}_{I}{{\ensuremath{\psi}}_{I}}^{*}+{\ensuremath{\psi}}_{2}{{\ensuremath{\psi}}_{2}}^{*}+{\ensuremath{\psi}}_{3}{{\ensuremath{\psi}}_{3}}^{*}+{\ensuremath{\psi}}_{4}{{\ensuremath{\psi}}_{4}}^{*}$ is treated by considering, as on the Schrodinger theory, the independent angular and radial factors separately. Tables and graphs are given for $\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}$ as a function of $\ensuremath{\theta}$ alone. The graphs are compared with and shown to correspond closely to the space quantization of the classical electron orbits. Graphs representative of $\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}$ as a function of $r$ alone are given and compared with the electronnucleus distances of the corresponding electron orbits. The radial and angular factors are brought together by means of a mechanical device described previously, which when photographed represents closely the electron-cloud $\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}$. Photographs are given for the states $1^{2}S_{\frac{1}{2}}$, $2^{2}P_{\frac{1}{2}, \frac{3}{2}}$, $3^{2}D_{\frac{3}{2}, \frac{5}{2}}$ $4^{2}F_{\frac{5}{2}, \frac{7}{2}}$, and $5^{2}G_{\frac{7}{2}}$, with $m=\ifmmode\pm\else\textpm\fi{}\frac{1}{2},\ifmmode\pm\else\textpm\fi{}\frac{3}{2},\ensuremath{\cdots}\ifmmode\pm\else\textpm\fi{}j$

DOI
10.1103/physrev.38.513

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Pictorial Representations of the Electron Cloud for Hydrogen-Like Atoms

Harvey E. White

It is well known that the solutions of the wave-equation for hydrogen-like atoms may be represented graphically by interpreting $\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}$ as a probability density. The probability density factors ${\ensuremath{\Phi}}_{m}{{\ensuremath{\Phi}}_{m}}^{*}\ifmmode\cdot\else\textperiodcentered\fi{}{[{\ensuremath{\Theta}}_{m,l}]}^{2}\ifmmode\cdot\else\textperiodcentered\fi{}{[{R}_{n,l}]}^{2}=\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}$ are represented graphically and briefly discussed and compared with the electron orbits of four classical models. Graphs for $s$, $p$, $d$, $f$, $g$, and $h$ electrons are given. An attempt to combine the probability density factors and form some graphical representation of $\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}$ has resulted in the construction of a mechanical device or model, see Fig. 5, which when photographed, gives very closely the desired result. Photographs for the magnetic states $m=0,\ifmmode\pm\else\textpm\fi{}1,\ifmmode\pm\else\textpm\fi{}2,\ifmmode\pm\else\textpm\fi{}3,\ensuremath{\cdots}$ are given for $1s$, $2p$, $3d$, $4f$, $2s$, $3p$, $4d$, $5f$, $3s$, $4p$, and $5d$ electrons, see Fig. 6.

Physical Review•Jun 1, 1931•54 citations

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The mere existence of stable atoms, and their arrangement into many-atom nanoscale structures, can only be explained by the laws of quantum mechanics. Indeed, the accumulated evidence regarding the internal structure of atoms motivated the formulation of quantum mechanics at the early twentieth century. Here we focus on single-electron (hydrogen-like) atoms. The dominance of the Coulomb central potential between the electron and nucleus, translates into a simple Schrödinger equation for their relative position distribution. Solving rigorously this equation reveals quantized energy levels, which explains the emission spectra of hydrogen-like atoms (Rydberg formula). The corresponding stationary probability density distributions for the electron around the nucleus are reminiscent of the Bohr model, where classical trajectories (orbits) are replaced by single-electron wave functions (orbitals). The degeneracies of different orbitals, associated with three quantum numbers, will later turn out to be critical for understanding many-electron atoms and the periodic table of the elements.

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Abstract This chapter reiterates the quantum numbers for atomic orbitals, known from general chemistry, and places them into the context developed so far. It is sketched how the Schrodinger equation (SE) for the hydrogen atom hydrogen-like systems (one electron plus a nucleus of charge Z) is set up. When the nucleus is treated as a fixed point charge, the SE is only for the electron. The solutions of the SE can be obtained by switching to spherical polar coordinates, such that the variables are separable in terms of the electron distance from the nucleus, r, and two angles. The kinetic energy of the electron then has a radial component, and an angular component. The latter is associated with the angular momentum quantum number, which is codified by the letters s, p, d, f, and so forth. A step by step solution of the SE is provided later, in chapter 19.

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FURTHER STUDY ON THE SOLUTION OF SCHRÖDINGER EQUATION OF HYDROGEN-LIKE ATOM

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In this work the Schrödinger equation of the hydrogen-like atom is analytically solved. Three sets of analytical solution are obtained if the factor r−l is not neglected. The first solution is the same as the traditional radial wave function; another one diverges; the last one is far different from the traditional solution. On the consideration of the finite size of the nucleus, the third wave function does not diverge while r approaches to zero. Its radial wave function has below characteristics: (1) the angular-momentum quantum number l must be greater than the principal quantum number n; (2) l must not be 0 or 1; (3) the electron-cloud distribution differs from the traditional one; (4) the electron is closer to the nucleus by comparison with that in traditional results. On the other hand, the validity of solutions needs to be verified experimentally. 1.

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This chapter begins with the simple solution of the Schrödinger equation for hydrogen atom for which the energy value has been derived. The Bohr radius of H atom has also been computed. After this, this chapter provides the generalised solution of the Schrödinger equation for H atom/hydrogen-like species in which F equation, R equation, and T equations have been derived in a simple and lucid way. This chapter also deals with the Laguerre differential equation, Laguerre polynomials, Rodrigues formula for the Laguerre polynomials, Laguerre associated equation and its solution, associated Laguerre polynomials, Rodrigues formula for the associated Laguerre polynomials, and solution of the radial equation. It also provides normalisation of the radial wave function and complete wave function; for the hydrogen atom, hydrogenic atomic orbital; electron density of 1 s electron; mathematical background of shape of orbitals; the most probable distance of electron from nucleus of hydrogen atom, and average distance of electron from the nucleus of hydrogen atom. The end of this chapter describes the references and adequate computational problems (solved problems and question on concepts).

CRC Press eBooks•Jan 15, 2021•0 citations
Previous attempts to represent graphically the Schrodinger electron cloud for hydrogen-like atoms have been so successful that similar graphical representations have been looked for on the Dirac theory. With a single electron specified on Dirac's theory by a set of four wave functions instead of one, the probability density \ensuremathΨ\ensuremathΨ∗=\ensuremathψI\ensuremathψI∗+\ensuremathψ2\ensuremathψ2∗+\ensuremathψ3\ensuremathψ3∗+\ensuremathψ4\ensuremathψ4∗\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}={\ensuremath{\psi}}_{I}{{\ensuremath{\psi}}_{I}}^{*}+{\ensuremath{\psi}}_{2}{{\ensuremath{\psi}}_{2}}^{*}+{\ensuremath{\psi}}_{3}{{\ensuremath{\psi}}_{3}}^{*}+{\ensuremath{\psi}}_{4}{{\ensuremath{\psi}}_{4}}^{*}\ensuremathΨ\ensuremathΨ∗=\ensuremathψI​\ensuremathψI​∗+\ensuremathψ2​\ensuremathψ2​∗+\ensuremathψ3​\ensuremathψ3​∗+\ensuremathψ4​\ensuremathψ4​∗ is treated by considering, as on the Schrodinger theory, the independent angular and radial factors separately. Tables and graphs are given for \ensuremathΨ\ensuremathΨ∗\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}\ensuremathΨ\ensuremathΨ∗ as a function of \ensuremathθ\ensuremath{\theta}\ensuremathθ alone. The graphs are compared with and shown to correspond closely to the space quantization of the classical electron orbits. Graphs representative of \ensuremathΨ\ensuremathΨ∗\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}\ensuremathΨ\ensuremathΨ∗ as a function of rrr alone are given and compared with the electronnucleus distances of the corresponding electron orbits. The radial and angular factors are brought together by means of a mechanical device described previously, which when photographed represents closely the electron-cloud \ensuremathΨ\ensuremathΨ∗\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}\ensuremathΨ\ensuremathΨ∗. Photographs are given for the states 12S121^{2}S_{\frac{1}{2}}12S21​​, 22P12,322^{2}P_{\frac{1}{2}, \frac{3}{2}}22P21​,23​​, 32D32,523^{2}D_{\frac{3}{2}, \frac{5}{2}}32D23​,25​​ 42F52,724^{2}F_{\frac{5}{2}, \frac{7}{2}}42F25​,27​​, and 52G725^{2}G_{\frac{7}{2}}52G27​​, with m=\ifmmode±\else\textpm\fi12,\ifmmode±\else\textpm\fi32,\ensuremath⋯\ifmmode±\else\textpm\fijm=\ifmmode\pm\else\textpm\fi{}\frac{1}{2},\ifmmode\pm\else\textpm\fi{}\frac{3}{2},\ensuremath{\cdots}\ifmmode\pm\else\textpm\fi{}jm=\ifmmode±\else\textpm\fi21​,\ifmmode±\else\textpm\fi23​,\ensuremath⋯\ifmmode±\else\textpm\fij
It is well known that the solutions of the wave-equation for hydrogen-like atoms may be represented graphically by interpreting $\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}$ as a probability density. The probability density factors ${\ensuremath{\Phi}}_{m}{{\ensuremath{\Phi}}_{m}}^{*}\ifmmode\cdot\else\textperiodcentered\fi{}{[{\ensuremath{\Theta}}_{m,l}]}^{2}\ifmmode\cdot\else\textperiodcentered\fi{}{[{R}_{n,l}]}^{2}=\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}$ are represented graphically and briefly discussed and compared with the electron orbits of four classical models. Graphs for sss, ppp, ddd, fff, ggg, and hhh electrons are given. An attempt to combine the probability density factors and form some graphical representation of $\ensuremath{\Psi}{\ensuremath{\Psi}}^{*}$ has resulted in the construction of a mechanical device or model, see Fig. 5, which when photographed, gives very closely the desired result. Photographs for the magnetic states $m=0,\ifmmode\pm\else\textpm\fi{}1,\ifmmode\pm\else\textpm\fi{}2,\ifmmode\pm\else\textpm\fi{}3,\ensuremath{\cdots}$ are given for 1s1s1s, 2p2p2p, 3d3d3d, 4f4f4f, 2s2s2s, 3p3p3p, 4d4d4d, 5f5f5f, 3s3s3s, 4p4p4p, and 5d5d5d electrons, see Fig. 6.
The mere existence of stable atoms, and their arrangement into many-atom nanoscale structures, can only be explained by the laws of quantum mechanics. Indeed, the accumulated evidence regarding the internal structure of atoms motivated the formulation of quantum mechanics at the early twentieth century. Here we focus on single-electron (hydrogen-like) atoms. The dominance of the Coulomb central potential between the electron and nucleus, translates into a simple Schrödinger equation for their relative position distribution. Solving rigorously this equation reveals quantized energy levels, which explains the emission spectra of hydrogen-like atoms (Rydberg formula). The corresponding stationary probability density distributions for the electron around the nucleus are reminiscent of the Bohr model, where classical trajectories (orbits) are replaced by single-electron wave functions (orbitals). The degeneracies of different orbitals, associated with three quantum numbers, will later turn out to be critical for understanding many-electron atoms and the periodic table of the elements.
Abstract This chapter reiterates the quantum numbers for atomic orbitals, known from general chemistry, and places them into the context developed so far. It is sketched how the Schrodinger equation (SE) for the hydrogen atom hydrogen-like systems (one electron plus a nucleus of charge Z) is set up. When the nucleus is treated as a fixed point charge, the SE is only for the electron. The solutions of the SE can be obtained by switching to spherical polar coordinates, such that the variables are separable in terms of the electron distance from the nucleus, r, and two angles. The kinetic energy of the electron then has a radial component, and an angular component. The latter is associated with the angular momentum quantum number, which is codified by the letters s, p, d, f, and so forth. A step by step solution of the SE is provided later, in chapter 19.
In this work the Schrödinger equation of the hydrogen-like atom is analytically solved. Three sets of analytical solution are obtained if the factor r−l is not neglected. The first solution is the same as the traditional radial wave function; another one diverges; the last one is far different from the traditional solution. On the consideration of the finite size of the nucleus, the third wave function does not diverge while r approaches to zero. Its radial wave function has below characteristics: (1) the angular-momentum quantum number l must be greater than the principal quantum number n; (2) l must not be 0 or 1; (3) the electron-cloud distribution differs from the traditional one; (4) the electron is closer to the nucleus by comparison with that in traditional results. On the other hand, the validity of solutions needs to be verified experimentally. 1.
This chapter begins with the simple solution of the Schrödinger equation for hydrogen atom for which the energy value has been derived. The Bohr radius of H atom has also been computed. After this, this chapter provides the generalised solution of the Schrödinger equation for H atom/hydrogen-like species in which F equation, R equation, and T equations have been derived in a simple and lucid way. This chapter also deals with the Laguerre differential equation, Laguerre polynomials, Rodrigues formula for the Laguerre polynomials, Laguerre associated equation and its solution, associated Laguerre polynomials, Rodrigues formula for the associated Laguerre polynomials, and solution of the radial equation. It also provides normalisation of the radial wave function and complete wave function; for the hydrogen atom, hydrogenic atomic orbital; electron density of 1 s electron; mathematical background of shape of orbitals; the most probable distance of electron from nucleus of hydrogen atom, and average distance of electron from the nucleus of hydrogen atom. The end of this chapter describes the references and adequate computational problems (solved problems and question on concepts).