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Define hesienburg Uncertainity principle?

Asked by Hoozan07 30th April 2015, 11:31 AM
Answered by Expert

Dear Hoozan,

  • Heisenberg’s uncertainty principle: It states that it is impossible to simultaneously determine, the exact position and momentum (or velocity) of an electron.


∆x—Uncertainty in position

∆vx—Uncertainty in velocity

∆px—Uncertainty in momentum


This means that if the position of electron is known, the velocity of electrons will be uncertain. On the other hand, if the velocity of electron is precisely known, the position of electrons will be uncertain.

  • Heisenberg’s uncertainty principle rules out the existence of definite paths or trajectories of electrons and other similar particles.
Answered by Expert 4th May 2015, 6:07 PM
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