Heisenberg’s Uncertainty Principle is applicable for the microscopic particles only. Let’s discuss about the Uncertainty Principle in detail.
What is Heisenberg’s Uncertainty Principle
It is impossible to measure simultaneously the position and momentum of a small microscopic particle with absolute accuracy.
if one of them is measured with absolute accuracy, the other becomes less accurate.
Suppose, we attempt to measure both the position and momentum of an electron. To find out the position of electron, use light to strike the electron. As a result, position and velocity of the electron are disturbed.
Significance of Uncertainty Principle
It applies to all objects but Uncertainty Principle is significant for microscopic objects only. The energy of photon is insufficient to change the position and the momentum of the big objects on colliding them. For example, light falling from the torch can’t change the position and momentum of the rat in the dark room.
If uncertainty in position is small then, uncertainty in velocity becomes significant. Therefore, concept of probability replaces Bohr’s concept of definite position and momentum.
Why electron does not exist in nucleus
The diameter of the nucleus is of the order of 10^-15m . If electron to exist in nucleus, the maximum uncertainty in its position can be 10^-15m. The mass of the electron is 9.1 X 10^-31Kg, the minimum uncertainty in velocity will be 5.77 X 10^10 m/s which is very large. The value is higher even than the velocity of light is 3 X 10^8 m which is not possible.
FAQ’s related to Heisenberg’s Uncertainty Principle
- Is Heisenberg’s Uncertainty Principle principle valid for moving electrons ?
Answer : It is not applicable to big moving objects or stationary objects. But is valid for moving electrons.
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