Introduction To Quantum Mechanics

In this episode of the I Can't Sleep Podcast, fall asleep learning about the Introduction to Quantum Mechanics. The original article on this subject is a little more technical, although you may still find some of these concepts a little dense. It should be just written for those looking for a little shut-eye tonight.

Happy sleeping!

Transcript

Welcome to the I Can't Sleep podcast, Where I read random articles from across the web to bore you to sleep with my soothing voice. I'm your host Benjamin Boster. Today's episode is from a Wikipedia article titled, Introduction to Quantum Mechanics. Quantum mechanics is the study of matter and its interactions with energy on the scale of atomic and subatomic particles. By contrast, Classical physics explains matter and energy only on a scale familiar to human experience, Including the behavior of astronomical bodies such as the moon. Classical physics is still used in much of modern science and technology. However, Towards the end of the 19th century, Scientists discovered phenomena in both the large macro and the small micro worlds that classical physics could not explain. The desire to resolve inconsistencies between observed phenomena and classical theory led to a revolution in physics, A shift in the original scientific paradigm, The development of quantum mechanics. Many aspects of quantum mechanics are counterintuitive and can seem paradoxical, Because they describe behavior quite different from that seen at larger scales. In the words of quantum physicist Richard Feynman, Quantum mechanics deals with nature as she is, Absurd. Features of quantum mechanics often defy simple explanations in everyday language. One example of this is the uncertainty principle. Precise measurements of position cannot be combined with precise measurements of velocity. Another example is entanglement. In certain circumstances, Two particles with a shared history may become mutually entangled, In which case a measurement made on one particle, Such as an electron that is measured to have spin up, Will be statistically correlated with the outcome of an equivalent measurement on the other particle, That the other will more likely be found to have spin down. This applies even though the particles may be so far apart that it is impossible for the result of the first measurement to have been transmitted to the second particle before the second measurement takes place. Quantum mechanics helps us understand chemistry because it explains how atoms interact with each other and form molecules. Many remarkable phenomena can be explained using quantum mechanics, Like superfluidity. Liquid helium in a container cooled to a temperature near absolute zero spontaneously flows up and over the rim of its container, An effect which cannot be explained by classical physics. Maxwell's unification of electricity, Magnetism, And light in the 1880s led to experiments on the interaction of light and matter. Some of these experiments had aspects which could not be explained. Quantum mechanics emerged in the early part of the 20th century from efforts to explain these results. The seeds of the quantum revolution appear in the discovery by J. J. Thompson in 1897, That cathode rays were not continuous but corpuscles, Now called electrons. Electrons had been named just six years earlier as part of the emerging theory of atoms. In 1900, Max Planck, A conservative physicist unconvinced by the atomic theory, Discovered that he needed discrete entities like atoms or electrons to explain black-body radiation. Hot objects radiate heat. Very hot objects, Red-hot, White-hot objects, All look similar when heated to the same temperature. This temperature-dependent look results from a common curve of light intensity at different frequencies or colors. The common curve is called black-body radiation. The lowest frequencies are invisible heat rays, Infrared light. White-hot objects have intensity across many colors in the visible range. Continuous wave theories of light and matter cannot explain the black-body radiation curve. Planck spread the heat energy among individual oscillators of an undefined character but with discrete energy capacity. The black-body radiation behavior was then predicted by this model. At the time, Electrons, Atoms, And discrete oscillators were all exotic ideas to explain exotic phenomena. But in 1905, Albert Einstein proposed that light was also corpuscular, Consisting of energy quanta, Seemingly in contradiction to the established science of light as a continuous wave, Stretching back a hundred years to Thomas Young's work on diffraction. His revolutionary proposals started by reanalyzing Planck black-body theory, Arriving at the same conclusions by using the new energy quanta. Einstein then showed how energy quanta connected to J. J. Thomson's electron. In 1902, Philip Leonard directed light from an arc lamp onto freshly cleaned metal plates housed in an evacuated glass tube. He measured the electric current coming off the metal plate for higher and lower intensity of light and for different metals. This is the photoelectric effect. Leonard showed that amount of current, The number of electrons, Depended on the intensity of the light, But that the velocity of these electrons did not depend on intensity. The continuous wave theories of the time would predict that more light intensity would accelerate the same amount of current to higher velocity, Contrary to experiment. Einstein's energy quanta explained the volume increase. One electron is ejected for each quantum. More quanta mean more electrons. Einstein then predicted that the electron velocity would increase in direct proportion to the light frequency above a fixed value that depended upon the metal. Here the idea is that energy in energy quanta depends upon the light frequency. The energy transferred to the electron comes in proportion to the light frequency. The type of metal gives a barrier, The fixed value, That the electrons must climb over to exit their atoms to be emitted from the metal surface and be measured. Ten years elapsed before Millikan's definitive experiment verified Einstein's prediction. During that time many scientists rejected the revolutionary idea of quanta, But Planck's and Einstein's concept was in the air and soon affected other theories. Experiments with light and matter in the late 1800s uncovered a reproducible but puzzling regularity. When light was shown through purified gases, Certain frequencies or colors did not pass. These dark absorption lines followed a distinctive pattern. The gaps between the lines decreased steadily. By 1889 the Rydberg formula predicted the lines for hydrogen gas using only a constant number and the integers to index the lines. The origin of this regularity was unknown. Solving this mystery would become the first major step toward quantum mechanics. Throughout the 19th century evidence grew for the atomic nature of matter. With J. J. Thomson's discovery of the electron in 1897, Scientists began the search for a model of the interior of the atom. Thomson proposed negative electrons swimming in a pool of positive charge. Between 1908 and 1911, Rutherford showed that the positive part was only one three-thousandth of the diameter of the atom. Models of planetary electrons orbiting a nuclear Sun were proposed. It cannot explain why the electron does not simply fall into the positive charge. In 1913 Niels Bohr and Ernest Rutherford connected the new atom models to the mystery of the Rydberg formula. The orbital radius of the electrons were constrained and the resulting energy differences matched the energy differences in the absorption lines. This meant that absorption and emissions of light from atoms was energy quantized. Only specific energies that matched the difference in orbital energy would be emitted or absorbed. Trading one mystery, The regular pattern of the Rydberg formula, For another mystery, Constraints on electron orbits, Might not seem like a big advance. But the new atom model summarized many other experimental findings. The quantization of the photoelectric effect and now the quantization of the electron orbits set the stage for the final revolution. In 1922 Otto Stern and Walter Gerlach demonstrated that the magnetic properties of silver atoms defy classical explanation. They fired a beam of silver atoms through a magnetic field. According to classical physics the atoms should have emerged in a spray with a continuous range of directions. Instead the beam separated into two and only two diverging streams of atoms. Unlike the other quantum effects known at the time, This striking result involves the state of a single atom. In 1927 T. E. Phipps and J. P. Taylor obtained a similar but less pronounced effect using hydrogen atoms in their ground state, Thereby eliminating any doubts that they may have been caused by the use of silver atoms. In 1924 Wolfgang Pauli called it two-valuedness not describable classically and associated it with electrons in the outermost shell. The experiments led to the formulation of its theory described to arise from spin of the electron in 1925 by Samuel Goudsmit and George Uhlenbeck under the advice of Paul Ehrenfest. In 1924 Louis de Broglie proposed that electrons in an atom are constrained not in orbits but as standing waves. In detail his solution did not work but his hypothesis that the electron corpuscle moves in the atom as a wave spurred Erwin Schrodinger to develop a wave equation for electrons. When applied to hydrogen the Rydberg formula was accurately reproduced. Max Born's 1924 paper zur Quantenmechanik was the first use of the word quantum mechanics in print. His later work included developing quantum collision models. In a footnote to a 1926 paper he proposed the Born rule connecting theoretical models to experiment. In 1927 at Bell Labs Clinton Davison and Lester Germer fired slow-moving electrons at a crystalline nickel target which showed a diffraction pattern indicating wave nature of electron whose theory was fully explained by Hans Bethe. A similar experiment by George Padgett Thompson and Alexander Reed firing electrons at thin celluloid foils and later metal films observing rings independently discovered the matter wave nature of electrons. In 1928 Paul Dirac published his relativistic wave equation simultaneously incorporating relativity predicting antimatter and providing a complete theory for the Stern-Gerlach result. These successes launched a new fundamental understanding of our world at small-scale quantum mechanics. Planck and Einstein started the revolution with quanta that broke down the continuous models of matter and light. 20 years later core puzzles like electrons came to be modeled as continuous waves. This result came to be called wave-particle duality. One iconic idea along with the uncertainty principle that sets quantum mechanics apart from older models of physics. In 1923 Compton demonstrated that the Planck-Einstein energy quanta from light also had momentum. Three years later the energy quanta got a new name photon. Despite its role in almost all stages of the quantum revolution no explicit model for light quanta existed until 1927 when Paul Dirac began work on a quantum theory of radiation that became quantum electrodynamics. Over the following decades this work evolved into quantum field theory the basis for modern quantum optics and particle physics. Throughout the first and the modern era of quantum mechanics the concept that classical mechanics must be valid macroscopically constrained possible quantum models. This concept was formalized by Bohr in 1923 as the correspondence principle. It requires quantum theory to converge to classical limits. One principle paradox is the apparent inconsistency between Newton's laws and quantum mechanics which can be explained using Ehrenfest's theorem which shows that the average values obtained from quantum mechanics e. G. Position and momentum obey classical laws. However Ehrenfest's theorem is far from capable of explaining all the counterintuitive phenomena quantum weirdness that have been observed but rather is a mathematical expression of the correspondence principle. The concept of wave-particle duality says that neither the classical concept of particle nor of wave can fully describe the behavior of quantum scale objects either photons or matter. Wave-particle duality is an example of the principle of complementarity in quantum physics. An elegant example of wave-particle duality is the double-slit experiment and the double-slit experiment as originally performed by Thomas Young in 1803 and then Augustine Fresnel a decade later. A beam of light is directed through two narrow closely spaced slits producing an interference pattern of light and dark bands on a screen. If one of the slits is covered up one might naively expect that the intensity of the fringes due to interference would be halved everywhere. In fact a much simpler pattern is seen, A diffraction pattern diametrically opposite the open slit. The same behavior can be demonstrated in water waves and so the double-slit experiment was seen as a demonstration of the wave nature of light. Variations of the double-slit experiment have been performed using electrons atoms and even large molecules and the same type of interference pattern is seen. Thus it has been demonstrated that all matter possesses both particle and wave characteristics. Even if the source intensity is turned down so that only one particle e. G. Photon or electron is passing through the apparatus at a time, The same interference pattern develops over time. The quantum particle acts as a wave when passing through the double slits but as a particle when it is detected. This is a typical feature of quantum complementarity. A quantum particle acts as a wave in an experiment to measure its wave-like properties and like a particle in an experiment to measure its particle-like properties. The point on the detector screen where an individual particle shows up is the result of a random process. However the distribution pattern of many individual particles mimics the diffraction pattern produced by waves. Suppose it is desired to measure the position and speed of an object, For example a car going through a radar speed trap. It can be assumed that the car has a definite position and speed at a particular moment in time. How accurately these values can be measured depends on the quality of the measuring equipment. If the precision of the measuring equipment is improved, It provides a result closer to the true value. It might be assumed that the speed of the car and its position could be operationally defined and measured simultaneously, As precisely as might be desired. In 1927 Heisenberg proved that this last assumption is not correct. Quantum mechanics shows that certain pairs of physical properties, For example position and speed, Cannot be simultaneously measured or defined in operational terms to arbitrary precision. The more precisely one property is measured or defined in operational terms, The less precisely can the other. This statement is known as the uncertainty principle. The uncertainty principle is not only a statement about the accuracy of our measuring equipment, But more deeply is about the conceptual nature of the measured quantities. The assumption that the car had simultaneously defined position and speed does not work in quantum mechanics. On a scale of cars and people, These uncertainties are negligible, But when dealing with atoms and electrons they become critical. Heisenberg gave as an illustration the measurement of the position and momentum of an electron using a photon of light. In measuring the electron's position, The higher the frequency of the photon, The more accurate is the measurement of the position of the impact of the photon with the electron, But the greater is the disturbance of the electron. This is because from the impact with the photon, The electron absorbs a random amount of energy, Rendering the measurement obtained of its momentum increasingly uncertain, For one is necessarily measuring its post-impact disturbed momentum from the collision products and not its original momentum, Momentum which should be simultaneously measured with position. With a photon of lower frequency, The disturbance and hence uncertainty in the momentum is less, But so is the accuracy of the measurement of the position of the impact. At the heart of the uncertainty principle is a fact that for any mathematical analysis in the position and velocity domains, Achieving a sharper more precise curve in the position domain can only be done at the expense of a more gradual less precise curve in the speed domain and vice versa. More sharpness in the position domain requires contributions from more frequencies in the speed domain to create the narrow curve and vice versa. It is a fundamental trade-off inherent in any such related or complementary measurements, But is only really noticeable at the smallest Planck scale near the size of elementary particles. The uncertainty principle shows mathematically that the product of the uncertainty in the position and momentum of a particle, Momentum is velocity multiplied by mass, Could never be less than a certain value and that this value is related to Planck's constant. Wave-function collapse means that a measurement is forced or converted a quantum probabilistic or potential state into a definite measured value. This phenomenon is only seen in quantum mechanics rather than classical mechanics. For example, Before a photon actually shows up on a detection screen, It can be described only with a set of probabilities for where it might show up. When it does appear, For instance in the CCD of an electronic camera, The time and space where it interacted with the device are known within very tight limits. However, The photon has disappeared in the process of being captured, Measured, And its quantum wave function has disappeared with it. In its place, Some macroscopic physical change in the detection screen has appeared, E. G. An exposed spot in a sheet of photographic film, Or a change in electric potential in some cell of a CCD. Because of the uncertainty principle, Statements about the position and momentum of particles can assign only a probability that the position or momentum has some numerical value. Therefore, It is necessary to formulate clearly the difference between the state of something indeterminate, Such as an electron in a probability cloud, And the state of something having a definite value. When an object can definitely be pinned down in some respect, It is said to possess an eigenstate. In the Stern-Gerlach experiment discussed above, The spin of the atom about the vertical axis has two eigenstates, Up and down. Before measuring it, We can only say that an individual atom has an equal probability of being found to have spin up or spin down. The measurement process causes the wave function to collapse into one of the two states. The eigenstates of spin about the vertical axis are not simultaneously eigenstates of spin about the horizontal axis. So this atom has an equal probability of being found to have either value of spin about the horizontal axis. Measuring the spin about the horizontal axis can allow an atom that was spun up to spin down. Measuring its spin about the horizontal axis collapses its wave function into one of the eigenstates of this measurement, Which means it is no longer an eigenstate of spin about the vertical axis, So can take either value. In 1924, Wolfgang Pauli proposed a new quantum degree of freedom, Or quantum number, With two possible values, To resolve inconsistencies between observed molecular spectra and the predictions of quantum mechanics. In particular, The spectrum of atom hydrogen had a doublet, Or a pair of lines differing by a small amount, Where only one line was expected. Pauli formulated his exclusion principle, Stating, There cannot exist an atom in such a quantum state that two electrons within it have the same set of quantum numbers. A year later, Uhlembeck and Goudsmit identified Pauli's new degree of freedom with the property called spin, Whose effects were observed in the Stern-Gerlach experiment. In 1928, Paul Dirac extended the Pauli equation, Which describes spinning electrons, To account for special relativity. The result was a theory that dealt properly with events, Such as the speed at which an electron orbits the nucleus, Occurring at a substantial fraction of the speed of light. By using the simplest electromagnetic interaction, Dirac was able to predict the value of the magnetic momentum associated with the electron spin, And found the experimentally observed value, Which was too large to be that of a spinning charged sphere governed by classical physics. He was able to solve for the spectral lines of the hydrogen atom, And to reproduce from physical first principles, Sommerfeld's successful formula for the fine structure of the hydrogen spectrum. Dirac's equation sometimes yielded a negative value for energy, For which he proposed a novel solution. He posited the existence of an anti-electron in a dynamical vacuum. This led to the many-particle quantum field theory. The Pauli exclusion principle says that two electrons in one system cannot be in the same state. Nature leaves open the possibility, However, That two electrons can have both states superimposed over each of them. Recall that the wave functions that emerge simultaneously from the double slits arrive at the detection screen in a state of superposition. Nothing is certain until the superimposed waveforms collapse. At that instant, An electron shows up somewhere in accordance with the probability that is a square of the absolute value of the sum of the complex valued amplitudes of the two superimposed waveforms. The situation there is already very abstract. A concrete way of thinking about entangled photons, Photons in which two contrary states are superimposed on each of them in the same event, Is as follows. Imagine that we have two color-coded states of photons, One state labeled blue and another state labeled red. Let the superposition of the red and the blue state appear in imagination as a purple state. We consider a case in which two photons are produced as the result of one single atomic event. Perhaps they are produced by the excitation of a crystal that characteristically absorbs a photon of a certain frequency and emits two photons of half the original frequency. In this case, The photons are interconnected by their shared origin in a single atomic event. This setup results in superimposed states of the photons. So the two photons come out purple. If the experimenter now performs some experiment that determines whether one of the photons is either blue or red, Then that experiment changes the photon involved from one having a superposition of blue and red characteristics to a photon that has only one of those characteristics. The problem that Einstein had with such an imagined situation was that if one of these photons had been kept bouncing between mirrors in a laboratory on earth, And the other one had traveled halfway to the nearest star when its twin was made to reveal itself as either blue or red, That meant that the distant photon now had to lose its purple status too. So whenever it might be investigated after its twin had been measured, It would necessarily show up in the opposite state to whatever its twin had revealed. In trying to show that quantum mechanics was not a complete theory, Einstein started with the theory's prediction that two or more particles that have interacted in the past can appear strongly correlated when their various properties are later measured. He sought to explain this seeming interaction classically, Through their common past, And preferably not by some spooky action at a distance. The argument is worked out in a famous paper, Einstein, Podolsky, And Rosen setting out what is now called the EPR paradox. Assuming what is now usually called local realism, EPR attempted to show from quantum theory that a particle has both position and momentum simultaneously, While according to the Copenhagen interpretation, Only one of those two properties actually exists, And only at the moment that it's being measured. EPR concluded that quantum theory is incomplete in that it refuses to consider physical properties that objectively exist in nature. Einstein, Podolsky, And Rosen, 1935, Is currently Einstein's most cited publication in physics journals. In the same year, Erwin Schrödinger used the word entanglement and declared, I would not call that one, But rather the characteristic trait of quantum mechanics. The Irish physicist John Stuart Bell carried the analysis of quantum entanglement much further. He deduced that if measurements are performed independently on the two separated particles of an entangled pair, Then the assumption that the outcomes depend upon hidden variables within each half implies a mathematical constraint on how the outcomes on the two measurements are correlated. This constraint would later be named the Bell inequality. Bell then showed that quantum physics predicts correlations that violate this inequality. Consequently, The only way that hidden variables could explain the predictions of quantum physics is if they are non-local, Which is to say that somehow the two particles are able to interact instantaneously no matter how widely they ever become separated. Performing experiments like those that Bell suggested, Physicists have found that nature obeys quantum mechanics and violates Bell inequalities. In other words, The results of these experiments are incompatible with any local hidden variable theory. The idea of quantum field theory began in the late 1920s with the British physicist Paul Dirac when he attempted to quantize the energy of the electromagnetic field. Just like in quantum mechanics, The energy of an electron in the hydrogen atom was quantized. Quantization is a procedure for constructing a quantum theory starting from a classical theory. Merriam Webster defines a field in physics as a region or space in which a given effect such as magnetism exists. Other effects that manifest themselves as fields are gravitation and static electricity. In 2008, Physicist Richard Hammond wrote, Sometimes we distinguish between quantum mechanics, QM, And quantum field theory, QFT. QM refers to a system in which the number of particles is fixed, And the fields, Such as the electromechanical field, Are continuous classical entities. QFT goes a step further and allows for the creation and annihilation of particles. He added, However, That quantum mechanics is often used to refer to the entire notion of quantum view. In 1931, Dirac proposed the existence of particles that later became known as antimatter. Dirac shared the Nobel Prize in physics for 1933 with Schrödinger for the discovery of new productive forms of atomic theory. Quantum electrodynamics, QED, Is the name of the quantum theory of the electromagnetic force. Understanding QED begins with understanding electromagnetism. Electromagnetism can be called electrodynamics because it is a dynamic interaction between electrical and magnetic forces. Electromagnetism begins with the electric charge. Electric charges are the sources of and create electric fields. An electric field is a field that exerts a force on any particles that carry electric charges at any point in space. This includes the electron, Proton, And even quarks, Among others. As a force is exerted, Electric charges move, A current flows, And a magnetic field is produced. The changing magnetic field, In turn, Causes electric current, Often moving electrons. The physical description of interacting charged particles, Electrical currents, Electrical fields, And magnetic fields, Is called electromagnetism. In 1928, Paul Dirac produced a relativistic quantum theory of electromagnetism. This was the progenitor to modern quantum electrodynamics, And that it had essential ingredients of the modern theory. However, The problem of unsolvable infinities developed in this relativistic quantum theory. Years later, Renormalization largely solved this problem. Initially viewed as a provisional suspect procedure by some of its originators, Renormalization eventually was embraced as an important and self-consistent tool in QED and other fields of physics. Also, In the late 1940s, Feynman diagrams provided a way to make predictions with QED by finding a probability amplitude for each possible way that an interaction could occur. The diagram showed, In particular, That the electromagnetic force is the exchange of photons between interacting particles. The Lamb shift is an example of a quantum electrodynamics prediction that has been experimentally verified. It is an effect whereby the quantum nature of the electromagnetic field makes the energy levels in an atom or ion deviate slightly from what they would otherwise be. As a result, Spectral lines may shift or split. Similarly, Within a free propagating electromagnetic wave, The current can also be just an abstract displacement current, Instead of involving charge carriers. In QED, Its full description makes essential use of short-lived virtual particles. There, QED again validates an earlier, Rather mysterious concept.

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When I saw the title, it sounded like it had success written all over it. I was right. 😉😴Thank you for another great track, Benjamin 🥰