What does the uncertainty principle state regarding the existence of a definite path or trajectory of an electron?
(N/A) According to the Heisenberg uncertainty principle,it is impossible to determine the definite path or trajectory of an electron because it is impossible to simultaneously determine both the exact position and the exact momentum (or velocity) of an electron with absolute precision.
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Similar Questions
The uncertainty in the position of an electron (mass = $9.1 \times 10^{-31} \, kg$) moving with a velocity of $300 \, ms^{-1}$ with an accuracy of $0.001 \%$ is ...... $(h = 6.63 \times 10^{-34} \, Js)$
Medium
View SolutionAn electron moves with a speed of $300 \ ms^{-1}$ with an uncertainty of $0.01\%$. Find the uncertainty in its position.
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View Solution$A$ microscope using appropriate photons is engaged to track an electron in an atom within a distance of $0.001 \ nm$. What will be the uncertainty involved in measuring its velocity?
Which of the following statements does not form part of Bohr's model of the hydrogen atom?
MediumAIPMT 1989
View SolutionThe uncertainty in position and velocity of a particle in motion are $1 \times 10^{-8} \ m$ and $6.627 \times 10^{-20} \ m/s$, respectively. The mass of the particle is $(h = 6.627 \times 10^{-34} \ J \cdot s)$
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