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Classical mechanics would predict that an electron orbits a proton just as planets orbit the sun. Classical electromagnetism would predict that the orbiting electron would emit a time-varying electrical field just as a radio station does. But the electron would lose energy as it emits this radiation, and would orbit closer and closer to the proton, until it collapses into the proton! Such a model cannot be correct.
Classical mechanics would predict that an electron orbits a proton just as planets orbit the sun. Classical electromagnetism would predict that the orbiting electron would emit a time-varying electrical field just as a radio station does. But the electron would lose energy as it emits this radiation, and would orbit closer and closer to the proton, until it collapses into the proton! Such a model cannot be correct.
Quantum mechanics discovered that an electron behaves as both a wave and a particle. As a result of the wave nature of the electron, the position of the electron is never precisely known. When it is observed, however, knowledge of the electron's velocity is lost. Hence, there is an inherent uncertainty that prevents precisely measuring both the position and the momentum simultaneously. This is known as the [[Werner Heisenberg|Heisenberg]] uncertainty principle.
Quantum mechanics posits that an electron behaves as both a wave and a particle. As a result of the wave nature of the electron, the position of the electron is never precisely known. Whenever it is attempted to be measured, knowledge of the electron's velocity is lost. Hence, there is an inherent uncertainty that prevents precisely measuring both the position and the momentum simultaneously. This is known as the [[Werner Heisenberg|Heisenberg]] uncertainty principle.
Quantum mechanics forms the basis for our understanding of chemical reactions, as well as all computers and electronic devices today.
Quantum mechanics forms the basis for our understanding of chemical reactions, as well as all computers and electronic devices today.
An important aspect of Quantum Mechanics is the predictions it makes about the radioactive decay of isotopes. This decay is random, and the randomness is inherently a quantum mechanical effect. As a result, the decay follows "1st-order kinetics" - typically resulting in an exponential decrease in the amount of isotope present as a function of time. The characteristic time required for 1/2 of the original amount of isotope to decay is known as the "half-life" and can vary from billionths of a second to billions of years.
For an excellent discussion of quantum mechanics, see:
For an excellent discussion of quantum mechanics, see: