heisenberg uncertainty principle can't be applied to stationary electron.why?
If you know the speed you don't know the position. If you know the position, you can't know the speed. So if you know the velocity is zero (stationary), you can't know where it is.
The Heisenberg uncertainty principle states that it is impossible to simultaneously know the exact position and momentum of a particle with absolute certainty. However, this principle is not applicable to stationary electrons.
To understand why, let's first define what it means for an electron to be "stationary." In quantum mechanics, stationary states are energy eigenstates, which means that the electron is in a stable energy level where its position and momentum do not change over time. In other words, the electron is in a confined region of space and has a well-defined momentum.
Since a stationary electron is in a well-defined position and has a deterministic momentum, the uncertainty principle does not come into play. This is because the uncertainty principle arises from the wave-particle duality of quantum objects. For a stationary electron, its wavefunction is in a precise state, which means its position and momentum are well-defined.
On the other hand, if the electron is in a state of motion, such as an excited state or a free electron, then the uncertainty principle becomes relevant. In these cases, the electron's position and momentum can only be known within certain ranges due to the wave-like nature of particles.
In summary, the Heisenberg uncertainty principle does not apply to stationary electrons because they are in well-defined energy levels, resulting in precise position and momentum values.