Minimum uncertainty in electron position

In summary: What is the actual minimum possible Δx for an isolated electron?There is no theoretical upper limit to how small ##\Delta x## can be; the size of the nucleus in which an electron must be located to be scattered off quarks is about ##10^{-15}## meters, but this is not a hard limit, since it can be decreased by increasing the energy of the electron.
  • #1
FrederikPhysics
9
0
I am wondering about the minimum possible uncertainty (standard deviation) in an electron's position (Δx). How precise can one know the electron's whereabouts without creating other sorts of particles and phenomenons.
I know of the localization energy interpretation of the energy uncertainty (ΔE). Using a Heisenberg relation we estimate Δx as
ΔEΔx≈ħc/2 ⇒ Δx≈ħ/2mc,​
since E=mc2 for an isolated electron (m is the rest mass). If Δx is smaller than this, extra localization energy manifests itself through other particles.

Now the questions are simple. Is this interpretation valid? What is the actual minimum possible Δx for an isolated electron? Have this been measured?
 
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  • #2
Wasn't it ##\Delta p\Delta x \ge \displaystyle {\hbar\over 2}## ?
 
  • #3
FrederikPhysics said:
How precise can one know the electron's whereabouts without creating other sorts of particles and phenomenons.

This is much too vague. What "other sorts of particles and phenomenons" are you thinking of?

FrederikPhysics said:
What is the actual minimum possible Δx for an isolated electron?

Theoretically, there is none; you can make ##\Delta x## as small as you like (as long as it's not zero), at the cost of making ##\Delta p## larger.

I'm not sure what the smallest ##\Delta x## is that has been achieved experimentally, but I think it's somewhere around the size of an atomic nucleus, about ##10^{-15}## meters. I'm basing that on the deep inelastic scattering experiments that first provided evidence for quarks; in these experiments, high energy electrons were fired into nuclei and scattered off quarks inside the nuclei, meaning that the electrons' positions had to be within the size of the nucleus, roughly, for the scattering to occur.
 
  • #4
Just as a side remark to post # 3: in whatever deep inelastic scattering of (fundamental or not) particles which are highly accelerated (energies of many GeV), there's no practical/theoretical way to test if the (non-relativistic) HUP is valid or not, for you can never measure the position of a particle in a scattering event, nor can you calculate its exact state vector. Remember that ##\Delta x## (the standard deviation from the mean) is theoretically computed as the statistical spread of the expectation values of x and x2 in the scattering state call it ##\psi(t)##. You cannot determine the state, because, due to the interaction term, the SE is not solvable, therefore you cannot calculate any expectation value.
 

FAQ: Minimum uncertainty in electron position

1. What is the uncertainty principle?

The uncertainty principle is a fundamental concept in quantum mechanics that states that it is impossible to know the exact position and momentum of a particle simultaneously. This means that there is always a degree of uncertainty in the measurement of these properties.

2. How does the uncertainty principle apply to electrons?

The uncertainty principle applies to all particles, including electrons. It means that it is impossible to know the exact position and momentum of an electron at the same time. This is due to the wave-like nature of electrons and the fact that their position and momentum are interrelated.

3. What is minimum uncertainty in electron position?

The minimum uncertainty in electron position refers to the smallest possible degree of uncertainty in the measurement of an electron's position. This is determined by the Heisenberg uncertainty principle and is equal to Planck's constant divided by the electron's momentum.

4. Why is there minimum uncertainty in electron position?

The minimum uncertainty in electron position is a consequence of the uncertainty principle and the wave-like nature of electrons. As electrons are described by a wave function, their position can only be determined within a certain range of probabilities, leading to a minimum uncertainty in their position measurement.

5. How does the uncertainty in electron position affect scientific research?

The uncertainty in electron position has significant implications for scientific research, particularly in the field of quantum mechanics. It means that we can never have complete knowledge of the behavior of subatomic particles and must rely on statistical probabilities. This has led to the development of new theories and technologies to better understand and manipulate particles with minimum uncertainty in their position.

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