How things work college course/Quantum mechanics timeline

• This timeline serves to guide student in understanding this Quiz, which has been placed on the openStax College list of quizzes.

What is Quantum Mechanics and what is Old Quantum Mechanics?

The 1927 Solvay Conference in Brussels.

Quantum mechanics (QM – also known as quantum physics, or quantum theory) is a branch of physics which deals with physical phenomena at microscopic scales. It departs from classical mechanics primarily at the quantum realm of atomic and subatomic length scales. Quantum mechanics provides a mathematical description of much of the dual particle-like and wave-like behavior and interactions of energy and matter. In most contexts, the term 'Quantum Mechanics' does not refer to theories that incorporate Einstein's theories of Relativity.

Old quantum theory is a collection of results from the years 1900–1925 which predate modern quantum mechanics. Although the theory was never complete or self-consistent, it yielded enough successes to establish that the classical Newtonian view of particle motion was insufficient. In 1926 Erwin Schrödinger found a completely quantum mechanical wave-equation, which reproduced all the successes of the old quantum theory without ambiguities and inconsistencies. At approximately the same time a matrix version of the theory was developed, and eventually the two versions merged to become equivalent. This essay focuses on the more accessible wave version.

When is a system in the quantum realm?

The Planck constant (denoted $h$) is a physical constant that appears throughout the theory of quantum mechanics, but that has no basis in the classical physics of Isaac Newton. A particle is likely to be in the quantum realm if either the mass, speed, or length is small:

• Electrons have less mass than protons or neutrons. For this reason, the electrons in an atom must be modeled by a quantum theory, but we have the option of treating the heavy nucleus as a stationary and classical object at the center.

• Atoms move very slowly when they are very cold. Quantum effects can occur at very low temperatures.

Timeline

↓   Click the year and link down in this page to a fuller explanation

• 1900 –– Max Planck vaguely and reluctantly introduces what we now call the photon to accurately model the experimentally observed spectrum of blackbody radiation.
• 1905 –– Albert Einstein uses Plank's hypotheses explains the photoelectric effect.
• 1909 –– Geoffrey Ingram Taylor shows that photons interfere with themselves even if only one photon is near the slits at any given time.
• 1913 –– Bohr used the Rydberg's (1888) formula to hypothesize the "Rutherford-Bohr atom".
• 1923 –– Arthurd Compton showed that X-rays bounce off and eject electrons in much the same way that billiard balls collide.
• 1924 –– Louis De Broglie extends wave-particle duality to particles (using relativistic arguments).
• 1926 –– Erwin Schrödinger proposes his Schrödinger equation wave equation but does not at first understand exactly what is waving.
• 1927 –– Davisson and Germer diffract electrons off a nickel crystal.
• 1927 –– Werner Heisenberg formulates the quantum uncertainty principle at about the same year that the Copenhagen interpretation is established.
• 1935 –– Schrödinger introduces Schrödinger's cat in response to the Copenhagen interpretation.

Black-body radiation 1900

A black body.

Old quantum theory came into existence in 1900 with a calculation by Plank that precisely matched the observed patterns of black-body radiation. He used the hypothesis that energy is radiated and absorbed in discrete "quanta" (or "energy elements"). In Plank's theory, the constant emerged as a relation between the energy ($E$) and the frequency ($f$) associated with the the interaction of light with the walls of the black body. This relation is called the Planck relation:

$E=hf\,.$

(Eq. 1)

Planck (cautiously) insisted that this was simply an aspect of the processes of absorption and emission of radiation and had nothing to do with the physical reality of the radiation itself. In fact, he considered his quantum hypothesis a mathematical trick to get the right answer rather than a sizeable discovery.

This equation predicts that photon energy is directly proportional to frequency; if you double f then E doubles. Frequency is inversely proportional to wavelength (since the speed of light is $c=f\lambda$ where λ (lambda) is the length of a wave.

How Plank constructed his model and performed his calculation is beyond the scope of this essay.

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Photoelectric Effect 1905

This depiction of photons (red) striking a metal plate and emitting photoelectrons serves to illustrate what cannot be seen.

In 1905 Albert Einstein published a paper that explained experimental data from the photoelectric effect that occurs when light strikes a metal surface. The photoelectric effect is the emission of an electron from a substance when light is absorbed. electrons are emitted from solids, liquids or gases when they absorb energy from light. Electrons emitted in this manner may be called photoelectrons. His hypothesis was that the photon's energy frequency obeyed $E=hf$ (i.e. Eq. (1) ). Each photon was assumed to give all of its energy to a single electron, and the energy of this electron could be measured by measuring the voltage required to keep the electron from escaping from the metal.

For more on the Photoelectric effect see PhET's http://phet.colorado.edu/en/simulation/photoelectric Photoelectric Lab] and Wikiverty's Photoelectric Effect

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Taylor makes things spooky with very dim light in 1909

We know light is a wave because it interferes with itself when passing through two slits.

Young's original drawing was used to make specfic predictions of the diffraction pattern for a given wavelength.

Interference occurs even when particles pass one at a time (animation).

While studying medicine at Göttingen in the 1790s, Thomas Young wrote a thesis on the physical and mathematical properties of sound and in 1799, he presented a paper to the Royal Society where he argued that light was also a wave. His idea was furiously opposed because it contradicted Newton, whose views were considered sacred. Nonetheless, he continued to develop his ideas. In 1801, he presented a famous paper to the Royal Society entitled "On the Theory of Light and Colours" which described various interference phenomena, and in 1803 he performed his famous double-slit experiment (strictly speaking, a double hole experiment).

Diffraction occurs also with water and sound. Diffraction allows one to measure wavelength, and the same value of wavelength occurs for diffraction through single slits, double slits, and N-slits, as well through a circular hole.

This experiment was repeated 100 years later by G. I. Taylor in light so dim that only one photon at a time was likely to be involved with the interference. Amazingly, one photon can interfere with itself. The experiment has been repeated in recent years with electrons, atoms, and even molecules containing over 800 atoms.

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Bohr-Rutherford Model 1913

Here, E = E₂-E₁, is the energy lost by the electron as it "falls" from high to low energy.

The Bohr model, introduced by Niels Bohr in 1913, depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus—similar in structure to the solar system, but with attraction provided by electrostatic forces rather than gravity. The Bohr model is a primitive model of the hydrogen atom that has been surpassed by the more sophisticated Schrodinger's equation. Nevertheless, Bohr's calculation should be viewed as more than a lucky guess. A guess based on dimensional analysis using a new and controversial fundamental constant is also an educated guess. The Bohr model assumes circular orbits of radius, $v$, and follows Newton's laws of physics, but with the following two embellishments to Newton's theory:

$n\lambda =2\pi r\,\,\,(n=1,2,3,\cdots )$

(Eq. 2)

$\lambda =h/p,$

(Eq. 3)

and $p=mv$ is momentum. Lambda, or $\lambda$, is now known as the De Broglie wavelength (although Bohr did not use the De Broglie wavelength to construct this model.) For an electron of mass ,$m$ and velocity $v$, $p=mv$.

Only the orbit on the left satisfies Bohr's conditions for an "allowed" orbit.

These standing waves somewhat resemble electrons in the Bohr model. The momentum, and hence the speed and energy of each "orbit" can be calculated from the wavelength.

The meaning of allowed orbits can be discerned from the pair of figures situated to the left. The wavelength must be such that the number that fit into a full circumference (2пr) must equal one, or two, or 3, or 4 (and so forth). In one case, the wave fits perfectly in the circles (with exactly four wavelengths). This corresponds to an electron in the third excited state, or n =4. The other wave does not fit into its allowed radius because it doubles over itself. This energy level does not exist for this atom.

Plank's relation (i.e. Eq.(1)) holds for the photons that are emitted from the hydrogen atom, with the photon energy, $E$, being equal to the difference in energy between the two electron orbitals. This can be expressed as an energy conservation law:

$E_{2}-E_{1}=hf$ ,

where $E_{2}$ is the higher energy and is $E_{2}$ the lower energy of the atom. These energies were calculated using Newton's laws of physics, just as one would calculate the energy of a satellite orbiting the Earth. The frequency of the light, $f$, could be measured by passing light the very hot gas (glowing) through a prism and measuring the wavelength.

While equations(1), (2), and (3) seem to embody all the calculations of Old Quantum Mechanics, they oversimplify the lines of reasoning actually used. Bohr, for example, did not use equation (3). And he wrote (2) not as a statement about "allowed" wavelengths, but about the quantization of angular momentum (L = mvr= nh/(2π)). In fact, the wave behavior of matter particles such as the electron (i.e., matter waves) was not suspected in 1913, and at that time Bohr did not believe in the existence of photons.

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Compton Effect 1923

Compton scattering is like this, but in two dimensions and relativistic.

In physics, a theory is judged primarily by its ability to match experimental observations. Click here to see a closeup and note how Total is approximately the sum of Compton and Photoelectric, and Pair, but not quite. Resolving the discrepancy requires a more complicated model that involves quantum energy levels.

More evidence that Eq.(3) also holds for the momentum of an individual photon was provided by Arthur Holly Compton in 1923. Since the photon is generally understood to be massless, the momentum, $p$, of the photon is not equal to $mv$, but equal to $hf/c$, where $c$ is the speed of light. The calculation of Compton scattering is a bit more difficult than those collisions usually studied in an undergraduate physics course because it is necessary to perform a relativistic calculation. Nevertheless, the calculation can be performed and predictions were confirmed by experimental observation.

High energy X-rays bounce off electrons in much the same way billiard balls collide on a pool table (except for relativistic effects).

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de Broglie Waves 1924

When I conceived the first basic ideas of wave mechanics in 1923–24, I was guided by the aim to perform a real physical synthesis, valid for all particles, of the coexistence of the wave and of the corpuscular aspects that Einstein had introduced for photons in his theory of light quanta in 1905. — Louis de Broglie

Equations (1) and (3) above are known as the de Broglie relations because de Broglie argued that if they are true in one reference frame, they would be true in all reference frames. In other words, if a stationary observer concluded that wavelength, frequency, energy, and momentum are related by these equations, then all observers would also measure these relations to hold. Consequently, if there is a simple relationship between momentum, energy, frequency, and wavelength, it must be these equations.

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Schrödinger Wave Equation 1926

This illustration illustrates how a simple wavepacket moves through space.

Schrödinger put forth a wave equation that gave the correct energy levels of the hydrogen atom in 1926. At last we have an equation from which a fundamental wave theory of quantum mechanics might be constructed.

$i\hbar {\frac {\partial }{\partial t}}\Psi (\mathbf {r} ,t)=\left[{\frac {-\hbar ^{2}}{2m}}\nabla ^{2}+V(\mathbf {r} ,t)\right]\Psi (\mathbf {r} ,t)$

(Eq. 4)

Although Heisenberg, Born, and Jordan had already developed a parallel effort using matrices that would prove to be a mathematically equivalent theory), we shall take this as the starting point in our quest for a fully developed theory. While this equation looks intimidating to a novice, it is a standard wave equation that is in many respects simpler than Maxwell's Equations. It is completely deterministic, meaning that it allows one to predict how a wave will evolve (given initial conditions). In other words, like Newton's $F=ma$, equation (4) predicts the future of the wave amplitude (We shall soon discover that predicting future values of ψ is not necessarily the same as predicting the future behavior of the particle.)

The electron probability density for the first few hydrogen atom electron orbitals shown as cross-sections. These orbitals form an orthonormal basis for the wave function of the electron. Different orbitals are depicted with different scale.

Quantum mass on spring. Waves G and H are almost particle-like

Computer generated solutions Schrödinger's equations for a (very tiny) mass attached to a spring are shown to the left. The symbol, ψ, is spelled psi, but often pronounced "sigh", with a hint of "p" at the beginning. It can also be pronounced "psee". It is called the "wavefunction", and is essentially the "amplitude", analogous to the "height" of the wave. The wavefunctions C through F represent states of known energy not unlike the "allowed" orbits of the Bohr atom. Wavefunctions G and H are more complicated and have no counterpart in Bohr's model of "allowed" states. They are known as "mixed energy" states.

What is waving?

The Schrödinger equation details the behavior of ψ but says nothing of its nature. Schrödinger unsuccessfully tried to interpret it as a charge density. More specifically it seemed plausible to interpret the square of the amplitude, |ψ|², as a charge density, since the total charge can be shown to remain constant if ψ obeys Schrödinger's equation. Schrödinger always opposed a statistical or probabilistic approach, with its associated discontinuities—much like Einstein, who believed that quantum mechanics was a statistical approximation to an underlying deterministic theory— and never reconciled with the Copenhagen interpretation. In 1926, Max Born successfully interpreted ψ as the probability amplitude, whose absolute square,|ψ|², is equal to probability density. Like charge, probability also obeys a conservation law, namely that the sum of all probabilities always adds to 1 (i.e., 100%)

Even though Schrödinger is (correctly) credited with inventing this wave equation, a connection between waves and particle motion was understood as early as 1834 when Hamilton wrote equations that describe the path taken by light in the approximation that the wavelength is very small (see The Eikonal Approximation and Classical Particle Motion for a discussion at the intermediate level).

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Davisson–Germer's accidental diffraction of electrons 1927

Davisson (left) and Germer (right)

While attempting to clean an oxide film off of nickel surface, Davisson and Germer heated the specimin to high temperature, not knowing that this would create large single crystal big enough to caused diffraction of their electron beam.

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Heisenberg's uncertainty principle 1927

Have you ever noticed that you can't ask a person what they are thinking without changing what they are thinking about? Here is what one of the founders of Quantum Mechanics had to say:

"If a person tries to observe what he is thinking about at the very moment that he is reflecting on a particular subject, it is generally agreed that he introduces unpredictable and uncontrollable changes in the his thoughts proceed thereafter. Why this happens is not definitely known at the present, but some plausible explanations will be suggested later."— David Bohm

Heisenberg came up with more convincing understanding that learning about something changes it in an unpredictable way. His argument imagined a powerful but hypothetical microscope that could see the electron as it orbited around the nucleus. Combining his knowledge of optics with the Compton Effect, Heisenberg concluded that the light required to see the electron would drastically change its orbit. And if the light were gentle, with low-energy photons, the microscope would yield an image so blurred that it would be impossible to track the electron's path.

Measuring a fly's location with a fly-swatter that has a hole in the center

Here the slit width equals the wavelength

A larger slit width 5 times larger than the wavelength results in 5 times less diffraction. By making Δx larger we allow Δp to be smaller. Here, x is the vertical direction.

Suppose you are in large dark room with small particle that is known to be at rest. You want to measure its location. The room must be dark because light would interact with the particle and induce motion. So you put a small hole in a large flat sheet and wave the sheet past where you think the particle is (there is of course no air in the room.) If the sheet strikes the particle, your measurement was a failure. But if you repeat the experiment often enough, you will eventually succeed and have knowledge about where the particle is located. Since your sheet never touched the particle, it is still at rest, right? Wrong!--No force ever acted on the particle; but nevertheless the particle has now been set in motion! Moreover, you don't know exactly how it is moving.

To understand why, put yourself reference frame of your flat sheet. The sheet is now at rest and the particle is moving towards it. By the de Broglie hypothesis, this particle will have wavelength (given by Eq. (3) to be h/mv). But if the particle acts as a wave, it will undergo single slit diffraction as shown in the figures to the left and right. Notice how decreasing the diameter of the hole increases the motion the spreading of the wave. The more you know about the position, the less you know about the motion, and vice versa. With a bit of basic algebra, the well-known equation for single slit diffraction can be shown to be consistent with the following inequality:

$\sigma _{x}\sigma _{p}\geq {\frac {\hbar }{2}}$

(Eq. 5)

where $\sigma _{x}$, is the uncertainty in position, and $\sigma _{p}$ is the uncertainty in momentum, $p=mv$. (The symbol $\sigma$ is called "sigma"). Equation (5) is known as Heisenberg's uncertainty principle, and renowned theoretical physicists have spent hours attempting to violate it. Under the Copenhagen interpretation of quantum mechanics, it can be proven as a mathematical theorem.

Copenhagen interpretation

The image to the left illustrates a simple argument for a probabilistic interpretation. What attribute of a particle can be in two places at the same time? Probability! To create this situation in a classroom, tape a wooden block to a stretched snaky spring and strike it, as shown in the other figure to the left.

Heisenberg also devised an argument based on what would happen if one attempted to use a microscope to violate the uncertainty principle. Since it was necessary to imagine a microscope that performed far beyond what was feasible at time, the figure to the right is known as Heisenberg's microscope. In this hypothetical microscope, the electron is illuminated from below by light depicted as both photons and waves, with wavefronts shown as blue lines. Photons that enter the microscope deviate from the vertical by an angle less than ε/2, and impart momentum to the electron as they scatter off it. The depiction of the wavefronts inside the microscope is unphysical due to diffraction effects that produce a blurred image and hence uncertainty in position.

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Schrodinger's cat 1935

A cat, a flask of poison, and a radioactive source are placed in a sealed box. If an internal monitor detects a single atom decaying, the flask is shattered, releasing the poison that kills the cat. The Copenhagen interpretation implies that after a while, the cat is simultaneously alive and dead.

The idea that an object can be in two places at the same time is unsettling, although there seems to be little evidence that this philosophical mystery has interfered with the pursuit of experimental or even theoretical physics. Three ideas have been put forth that have become cultural icons of Quantum Mechanics. They are the EPR Paradox, Schrodingers Cat, and Bell's Theorem (which has been justifiably called “the most profound discovery of science”.) Of these three cultural icons, Schrodinger's cat is easiest to grasp. Schrödinger wrote:

"One can even set up quite ridiculous cases. A cat is penned up in a steel chamber, along with the following device (which must be secured against direct interference by the cat): in a Geiger counter, there is a tiny bit of radioactive substance, so small, that perhaps in the course of the hour one of the atoms decays, but also, with equal probability, perhaps none; if it happens, the counter tube discharges and through a relay releases a hammer that shatters a small flask of hydrocyanic acid. If one has left this entire system to itself for an hour, one would say that the cat still lives if meanwhile no atom has decayed. The psi-function of the entire system would express this by having in it the living and dead cat (pardon the expression) mixed or smeared out in equal parts"—Erwin Schrödinger

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Recent Developments

• 1964 – John Stewart Bell puts forth Bell's theorem
• 1982 - The violation of Bell's theorem was experimentally verified by Alain Aspect
• 2010 - Cleland puts an object visible to the naked eye (but smaller than a cat) into a mixed energy state.

References and Endnotes

• Most of material was lifted out of Wikipedia