## uncertainty principle
h/2π, where h is Planck's
constant. The uncertainty principle was arrived at from considerations of the dualistic nature of the electron. The very definition of a particle implies that at any instant it has a definite momentum and occupies a definite position in space. Unless we can simultaneously determine both the momentum and the position in space we can't actually say that a "particle" in the accepted sense has been observed. Since an electron is somewhere within the wave packet, moving with group velocity, uncertainty about the defined particle velocity arises, because the group is not infinitely narrow and has a velocity spread. It is impossible to know where, within the group, the electron actually is and what is its exact velocity. For a long wave packet, with many crests, the position of the electron is very uncertain but the velocity spread is very small so that the particle velocity is fairly accurately known. In a short packet the position of the particle is more or less fixed, but as the velocity spread of such a packet can be shown to be large, the particle velocity is indeterminate. Either the position or the velocity can be known accurately, but not both, and one has a doubtful value. It can be proved that it's impossible to determine simultaneously both the momentum and the position of a particle with accuracy. This is shown by the following treatment. A wave packet representing a particle has a finite length Δ x
and the extreme ends have a wave number difference Δν. It can be
shown from general wave theory Δx ~ 1/Δν, the length
of the wave packet being inversely proportional to the difference in wave
numbers of the two ends of the packet. Thus Δx.Δ&nu
~ 1. Since we have also λ = h/mv = h/p
where the momentum mv is written as p, then
Differentiating gives Δwhence, by substitution, we get ΔIt is clear that Δ x represents the uncertainty in determining
the exact location of the particle within the packet, and as there is a
range of wave numbers Δν in the packet Δp is the
uncertainty in evaluating the momentum. This then is Heisenberg's uncertainty
relationship which states that the product of the uncertainties in determining
position and momentum is approximately equal to Planck's constant h.
The more exactly we define the position, i.e., the smaller we make Δ x,
the larger becomes Δp and vice versa. The relationship shows
that it is impossible to measure both the position and the momentum accurately
simultaneously. Clearly this is fundamental since it sets a limit to the
possible accuracy of observation. The uncertainty arises from the smeared-out
properties of wave packets compared with finite points representing the
centers of the particles. No matter what method is tried it is impossible to avoid the consequences of the uncertainty relationship. ## Related category• PARTICLE PHYSICS | |||||||

Home • About • Copyright © The Worlds of David Darling • Encyclopedia of Alternative Energy • Contact |