principle

Heisenberg uncertainty principle

The Heisenberg uncertainty principle states that the position and momentum of a particle cannot both be precisely determined simultaneously.
11 related articles · 1 formulas · 3 who worked here

Description

In the quantum world, you cannot simultaneously know exactly where a particle is and how fast it is moving. If we try to measure the position more precisely, the speed becomes more and more blurred, and vice versa. It's like trying to photograph a hovering hummingbird: to freeze the motion, you need a short exposure, but then the image will be dark and fuzzy. Or conversely, you can take a bright image with a long exposure, but the wings will blur. Nature seems to play hide-and-seek with us: the more you learn about one, the less about the other.

History

Werner Heisenberg formulated the principle in 1927 while working in Copenhagen under the guidance of Niels Bohr. Initially, he reasoned in terms of a thought microscope, showing that measuring the position of an electron by scattering a gamma ray inevitably introduces uncertainty in momentum. Later, mathematical rigor was provided by Hermann Weyl and Earle Kennard, who derived the inequality from commutation relations. Bohr generalized the principle to the idea of complementarity. Over time, the inequality was generalized to other pairs of quantities, such as angular momentum projection and angle.

How it works

The principle always works, but it manifests significantly for microparticles, where Planck's constant is not negligible. In the macroworld, the product of uncertainties is usually tiny compared to the sizes of bodies and their momenta, so we do not notice the limitations. In quantum technologies, for example, in a scanning tunneling microscope, it determines resolution. The principle also limits the precision of simultaneous measurement of signal and phase in quantum optics. The energy-time relation explains the creation of virtual particles: they can exist by 'borrowing' energy from the vacuum for a time inversely proportional to that energy.

Fun fact

The uncertainty principle prevents electrons from falling onto the atomic nucleus! If an electron 'sat' on the nucleus, its position would become very precise, and its momentum would be huge, and it would instantly fly out. So atoms are stable precisely because of quantum uncertainty.

Concept graph →

Formulas

$$\Delta x \Delta p \geq \frac{\hbar}{2}$$
Minimum uncertainty in position and momentum.
What is in the formula
\Delta xvariableStandard deviation of position — position uncertainty metre
\Delta pvariableStandard deviation of momentum — momentum uncertainty kilogram metre per second
\hbarconstantReduced Planck constant — reduced planck constant = 1.054571817e-34 joule second
δxδp=\frac{1}{2} · 2505.00475v2
δxδp\geq\frac{ħ}{2} · 2602.16215
δxδp\geq\frac{ħ}{2} · 2607.06967
δxδp\ge\frac{h}{4π} · 2602.19671

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