   # Quantum Numbers to Periodic Tables: The Electronic Structure of Atoms

A Google image search on the term "atom" will produce two general types of picture: Unfortunately, both of these conventional representations are incorrect (in several ways), and the electronic structure of atoms needs to be understood in terms of the Schrödinger wave equation.

## Atoms

In stars atomic nuclei are born naked, but their net positive charge – their atomic number Z – attracts the comparatively mass-less electrons to produce neutral atoms.

• The nucleus of a gold atom has an atomic of atomic number, Z = 79, so the Au79+ ion attracts 79 negatively charged electrons to give a neutral atom of gold, Au.

The first problem with the conventional images shown above is that the atomic nucleus is absolutly tiny compared with the size of the overall atom! Compared with the size of the gold nucleus, a gold atom is huge... comparable with the relative size of the Sun and solar system: The above diagram is developed from one on the HyperPhysics website but converted to metric units.

## The Electronic Structure of The Atom

The second problem with the conventional images above is that the negatively charged electrons "associate" with the positively charged nucleus as three dimensional resonant standing waves:

The electrons move about the point positive charge
in a beautiful & subtle quantum mechanical dance

The modes of resonance for single electron systems such as the hydrogen atom are described by the Schrödinger wave equation. Very briefly Schrödinger:

• Knew of de Broglie's proposal that a moving particle has wavelength, l, proportional to Planck's constant, h, and momentum p so that l = h/p, a property we now known as wave-particle duality.
• So constructed a differential equation for a wave-like electron resonating in three dimensions about a point positive charge, the time-independent Schrödinger wave eqn. (Wikipedia): • Solutions to the Schrödinger wave equation correspond to modes of electron resonance and are formally called wavefunctions.
• The quantised wavefunctions and the corresponding energy levels correspond to the energy levels in one electron atoms & ions: H, He+, Li2+, Be3+, etc. The energy difference between these energy levels result in the spectral lines of these species*.
• Although not exactly the same, chemists tend to call wavefunctions "orbitals".

* Thanks to Mark Kubinec Director, Digital Chemistry Project, UC Berkeley for a suggested rewording of this bullet point. Marks suggests that some of the videos from UC Berkeley may be of interest readers.

## 1-Dimensional resonant standing waves: the vibrating string: ## 2-Dimensional resonant standing wave, a vibrating drum skin (see QuickTime movies here and here): ## 3-Dimensional resonant standing waves: So, what does an atom look like?

There is no good/ideal representation (yet), but the one that comes closest – in this author's humble opinion – is the old Windows 97 'flowerbox' screensaver:

## Quantum Numbers to Orbitals

Chemists recognise s, p, d and f-orbitals. The topologies of these orbitals: the shape, phase & electron occupancy are described by four quantum numbers:

 n The principal quantum number l The subsidiary or azimuthal or angular momentum or orbital shape quantum number ml The magnetic quantum number ms The electron spin quantum number

From Wikipedia: These quantum numbers conspire to give spherical s-orbitals, dumbbell shaped p-orbitals that come in sets of three, double dumbbell d-orbitals that come in sets of five, etc.

Electrons enter and fill orbitals according to four rules:

 Pauli Exclusion Principle Orbitals can contain a maximum of two electrons which must be of opposite spin. Aufbau or Build-up Principle Electrons enter and fill lower energy orbitals before higher energy orbitals. Hund's Rule When there there are degenerate (equal energy) orbitals available, electrons will enter the orbitals one-at-a-time to maximise degeneracy, and only when all the orbitals are half filled will pairing-up occur. This is the rule of maximum multiplicity. Madelung's Rule Orbitals fill with electrons as n + l, where n is the principal quantum number and l is the subsidiary quantum number. This rule 'explains' why the 4s orbital has a lower energy than the 3d orbital, and it gives the periodic table its characteristic appearance.

Certain 'magic' numbers of electrons of electrons exhibit energetic stability: 2, 10, 18, 36, 54, 86 and, one assumes, 118, are associated with the Group 18 inert or noble gases: He, Ne, Ar, Kr, Xe, Rn & Uuo.

• The 'magic' numbers inevitably arise from the underlying quantum mechanics, but as Richard Feynman told us (here): "I think I can safely say that nobody understands quantum mechanics."

We can predict quantum mechanical patterns, but we don't know why we can predict the patterns. We do not understand QM in terms of a deeper theory.

Now available on the web are Richard Feynman's "Messenger Lectures" where he looks at the nature of physical theory and its relationship with mathematics. Highly recommended!

## Quantum Patterns

The pattern of orbital structure is very rich and can be mapped onto the two dimensions of paper in many different ways.

Some mappings emphasize how the orbitals are ordered and filled with electrons, others stress how the chemical elements and their orbitals are ordered with respect to atomic number Z. Each tells us something different about atomic orbital structure and/or elemental periodicity.

## Orbital Filling

Madelung's Rule says the orbitals fill in the order n + l (lowest n first). This gives the sequence:

• (n = 1) + (l = 0) = 1    1s
• (n = 2) + (l = 0) = 2    2s
• (n = 2) + (l = 1) = 3    2p
• (n = 3) + (l = 0) = 3    3s
• (n = 3) + (l = 1) = 4    3p
• (n = 4) + (l = 0) = 4    4s
• (n = 3) + (l = 2) = 5    3d
• (n = 4) + (l = 1) = 5    4p
• (n = 5) + (l = 0) = 5    5s
• and so on... A nice electron shell representation from the Encyclopedia Britannica:

Thus, the orbital filling sequence is, from the bottom of this diagram, upwards because the lowest energies fill first: ## Electron Shells

As electrons are added, the quantum numbers build up the orbitals. Read this diagram, from the top downwards: Fuzzy Atoms

One of several animations and explanations/realisations of quantum physics from Data-Burger, scientific advisor: J. Bobroff:

What is particularly nice about this video is that it shows the quantum fuzziness of the atoms. This explains/shows how and why induced-dipole/induced-dipole (London force) interactions occur, an important class of van der Waals intermolecular interaction.

• At any moment, the electron distribution is not perfectly spherical, which means that there is an instantaneous dipole on the atom.
• This instantaneous dipole is able to induce a dipole on an adjacent atom, with the effect that the two atoms are attracted when they touch.
• The overall effect is as if atoms are sticky, a bit like Velcro.
• This effect explains why the Group 18 noble gas elements are able to form liquids and solids [not He] at low temperatures, and why non-polar molecules, such as Cl2, Br2, I2, P4, S8 & hydrocarbons are able to condense.

## Elements by Orbital, And Some Subtleties...

The electronic structure can be illustrated adding electrons to boxes (to represent orbitals). This representation shows the Pauli exclusion principle, the aufbau principle and Hund's rule in action.

There are some subtle effects with the d block elements chromium, Cr, and copper, Cu. Hund's rule of maximum multiplicity lowers the energy of the 3d orbital below that of the the 4s orbital, due to the stabilisation achieved with a complete and spherically symmetric set of five 3d orbitals containing five or ten electrons. Thus,

• Chromium has the formulation: [Ar] 3d5 4s1 and not: [Ar] 3d4 4s2
• Copper has the formulation: [Ar] 3d10 4s1 and not: [Ar] 3d9 4s2 ## The Periodic Table

A periodic table – of sorts – can be constructed by listing the elements by n and l quantum number: The problem with this mapping is that the generated sequence is not contiguous with respect to atomic number atomic number, Z, and so is NOT a periodic table. Try counting the numbers past the red lines | on this representation: Named after a French chemist who first published in the formulation in 1929, the Janet or Left-Step Periodic Table uses a slightly different mapping that is contiguous with atomic number: While the Janet periodic table is very logical and clear, it does not separate metals from non-metals as well as the Mendeleev version, and helium is problem chemically.

However, it is a simple 'mapping' to go from the Janet or Left-Step periodic table to a modern formulation of Mendeleev's periodic table. There are a couple of steps: Including the movement of He to Group 18: Drop the f-block down, and move the s-block and d and p-blocks into the space produced, and this gives the commonly used medium form periodic table: Note, this is the 'correct' medium form, with Group 3 as: Sc, Y, Lu & Lr and with the f-block as La-Yb and Ac-No.

Many medium form PTs incorrectly leave a gap where Lu and Lr are situated, and then add these two elements to the end of the f-block: ### The Devil In The Detail

Matters are considerably more involved than implied above.

Wavefunctions are called orbitals by chemists, but this ignores the existence of real and imaginary portions of the complex wave function – where the term 'complex' is being used in the mathematical sense.

Orbitals should not be considered as being physically real, and in principle no experimental technique can directly observe orbitals.

• The wavefunction is Ψ, and the normalised wavefunction is |Ψ|.
• Electron density is |Ψ|2, and this is a measurable quantity.
• However, the orbital is the square root of the electron density, and on taking the root all phase information is lost, for the same reason the square root of minus 1 cannot be known.

Solutions for the isolated hydrogen atom must be physically spherically symmetric (because the isolated hydrogen atom force field is spherically symmetric) and this gives rise to the 1s, 2s, 3s.. 'shells'. But mathematically one also gets 2p, 3p... solutions (lobes) that are not spherically symmetric because theta and phi are defined. These angles presuppose x, y, z axes that exist mathematically and allow non-symmetrical solutions. Physically these lobes don't exist for any isolated atom, but chemists talk about them when atoms are closely interacting, i.e. they exist in non-uniform fields, where axes and lobes can make physical sense.

The Schrödinger wave equation can only be solved analytically for one electron systems. For multi-electron systems it is necessary to use approximations, and the more electrons are involved, the more severe are the approximations. That said, mathematically manipulated orbitals are the foundation of much computational quantum chemistry software.

We chemists can fool ourselves into thinking that we understand s and p-orbitals, because they can be superimposed upon (mapped to) the easily understandable three dimensional x, y, z Cartesian coordinate system. But d-orbitals project into 5-dimensional space, and f-orbitals into 7-dimensional space. d-Orbitals can be mapped to the 3-dimensional Cartesian coordinate system, but a mathematical artifact is the 'strange looking' dz2 orbital.

Real, physical chemical structure and reactivity systems also exist in three dimensional Cartesian coordinate space. Mother Nature must also solve the 5-dimensional to Cartesian dimensional reduction when forming transition metal complexes, such as [Cu(H2O)6]2+, that use d-orbitals. Understanding comes from crystal field theory that is able to predict what happens when a Cartesian array of charges interacts with d-orbitals that are degenerate in 5-dimensional space. The geometry causes the 5 d-orbitals to split in energy to give three lower energy orbitals and two higher energy orbitals.

Thanks to DD, an ex-physicist/philosopher of science, for his input into this section.

Quantum Physics of Atoms, Molecules, Solids, Nuclei, and Particles (2nd Ed.) by Robert Eisberg & Robert Resnick, 1985 (John Wiley & Sons, NY. pp. 252)   Segré Chart The Periodic Table: What Is It Showing?

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