The Heisenberg uncertainty principle is a way of expressing the qualitative properties of quantum mechanics in an easy to visualize way.
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Figure 3.3 is a combination plot of the position
of a
particle and the corresponding linear momentum
,
the mass and
the velocity in the
-
The right of the figure shows what happens if you squeeze down on the
particle to try to restrict it to one position
:
Heisenberg showed that according to quantum mechanics, the area of the “blob” cannot be contracted to a point. When you try to narrow down the position of a particle, you get into trouble with momentum. Conversely, if you try to pin down a precise momentum, you lose all hold on the position.
The area of the blob has a minimum value below which you cannot go.
This minimum area is comparable in size to the so-called
“Planck constant,” roughly ![]()
/s
Key Points
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- The Heisenberg uncertainty principle says that there is always a minimum combined uncertainty in position and linear momentum.
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- It implies that a particle cannot have a mathematically precise position, because that would require an infinite uncertainty in linear momentum.
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- It also implies that a particle cannot have a mathematically precise linear momentum (velocity), since that would imply an infinite uncertainty in position.