Introducing Quantum Theory
Quantum theory confronts us with bizarre paradoxes which upset the logical edifice of classical physics. At the sub-atomic level, one particle seems to know what the others are doing (so-called non-locality), and according to Heisenberg's uncertainty principle, there is a limit on how accurately nature can be observed. And yet the theory is amazingly accurate and widely applied, explaining all of chemistry and most of physics. Introducing Quantum Theory takes us on a step-by-step tour with the key figures, including Planck, Einstein, Bohr, Heisenberg and Schrodinger. Each contributed at least one crucial concept to the theory. The puzzle of the wave-particle duality is here, along with descriptions of the two questions raised against Bohr's Copenhagen Interpretation - the famous dead and alive cat and the EPR paradox. Both remain unresolved at the beginning of the 21st century."
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19th century alpha ANCP angular momentum atomic structure Balmer Formula Black-Body Radiation Bohr's Boltzmann's Bright Line Broglie Broglie's calculate called Cambridge classical physicists classical physics concept Copenhagen dark lines discovery double-slit experiment Einstein electron orbits emitted energy entropy EPR paradox Exclusion Principle experimental explained frequencies fundamental gases gave heat Heinrich Rubens Heisenberg ideas interference interpretation kinetic laboratory Light Spectra linear lntroducing mathematical matrix mechanics Max Born Maxwell Maxwell's measurements metal microscopic molecules motion Niels Bohr non-locality nucleus Paul Dirac periodic table Photoelectric Effect photons postulate predicted PROBABLE TATE problem properties quantized quantum mechanics quantum physics RACPIATION Rutherford's Schrödinger shell Solvay Conference Sommerfeld spectral lines spectrum spin statistical temperature theoretical Thermodynamics THI4 three quantum numbers ultraviolet uncertainty principle University values velocity vibrating visualize voltage WAé WAVE AND PARTICLE wave equation wave function wavelength WHI£H whole number Wolfgang Pauli WOULDP Zeeman Effect