27/04/2025
Transition from Classical Physics to Quantum Mechanics:
At the end of the nineteeth century, classical physics had progressed to such a level that many scientists thought all problems in physical science had been solved or were about to be solved. After all, classical Newtonian mechanics was able to predict the motions of celestial bodies, electromagnetism was described by Maxwell's equations, the formulation of the principles of thermodynamics had led to the understanding of the interconversion of heat and work and the limitations of this interconversion, and classical optics allowed the design and construction of scientific instruments such as the telescope and the microscope, both of which had advanced the understanding of the physical world around us. In chemistry, an experimentally derived classification of elements had been achieved (the rudimentary periodic table), although the nature of atoms and molecules and the concept of the electron's involvement in chemical reactions had not been realized. The experiments by Rutherford demonstrated that the atom consisted of very small, positively charged, and heavy nuclei that identify each element and electrons orbiting the nuclei that provided the negative charge to produce electrically neutral atoms. At this point, the question naturally rose: Why don't the electrons fall into the nucleus, given the fact that opposite electric charges do attaract? A planetary-like situation where the electrons are held in orbits by centrifugal forces was not plausible because of the (radiative) energy loss an orbiting electron would exeperience. This dilemma was one of the causes for the development of quantum mechanics. In addition, there were other experimental results that could not be explained by classical physics and needed the development of new theoretial concepts, e.g. the inability of classical models to reproduce the blackbody emission curve, the photoelectric effect.