Quantum Mechanics: Heisenberg's uncertainty principle.

Quantum Mechanics: Heisenberg's uncertainty principle.

STATEMENT OF THE HEISENBERG'S UNCERTAINTY PRINCIPLE  

Heisenberg's uncertainty principle states that quantum mechanics does not simultaneously permit the determination of the position and momentum of a particle accurately. Any attempt made to make the measurement of the position of the particle, such as an electron, very accurately, results in the large uncertainty in the measurement of the momentum and vice-a-versa.

MATHEMATICAL EXPRESSION: 

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PHYSICAL SIGNIFICANCE:

• The Heisenberg uncertainty principle is a physical law that forms part of quantum mechanics. It says that the more precisely you measure the position of a particle, the less precisely you can know it's motion (momentum or velocity).
• We should not think of the exact position or an accurate value for the momentum of a particle. Instead, we should think of the probability of finding the particle at a certain position or the probable value for the momentum of the particle. 
• The estimation of such probabilities is made using the probability density functions in quantum mechanics.  
• Many relations are corresponding to Heisenberg's uncertainty principle.

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• Derived in terms of energy.

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The Heisenberg uncertainty principle based on quantum physics explains several facts that could not be explained by classical physics.

NON-EXISTENCE OF ELECTRON IN NUCLEUS

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• This is practically not possible as the atom will become unstable with this value of K.E. hence electron cannot pre-exist in the free state of the nucleus.

Heisenberg's uncertainty is a very fascinating topic and its beauty cannot be expressed at this basic level. 

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Thank you.

~Amol Pandit.