![]() ![]() The situation is similar to measuring momentum. If someone asked you, "what is the position of a wave?" you would have difficulty answering – its position is spread out over a range of values. You can think of position as a particle-type property and momentum as a wave-type property (as waves are always traveling somewhere). ![]() Therefore an electron behaves like a particle and a wave. However, if you fire a load of electrons at two slits in a metal plate, you will get an interference pattern on the other side, as if the electrons were acting like waves. For example, we all think of an electron as a particle. It comes from the concept of wave-particle duality (see the De Broglie wavelength calculator) in quantum physics. This uncertainty doesn't come about due to any deficiency in the equipment used to make the measurements. The more accurately you set out to measure a particle's location, the more uncertain you are about its momentum (mass and velocity combined) and vice versa. The two most famous properties that follow Heisenberg's uncertainty principle are position and momentum (mass times speed). If your experiment sets out to measure one quantum property with high precision, then you will lose accuracy in the measurement of its other properties. ![]() His uncertainty principle states that you cannot measure all of the quantum properties of a particle with the same accuracy at the same time. In 1927, Werner Heisenberg proposed a principle that applies to measuring the properties of quantum-sized objects (e.g., atomic and sub-atomic particles). ![]()
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