Question

What is the importance of the Heisenberg Uncertainty Principle?

Answer 1

Hint:In this question, students mainly have to think about the momentum, velocity and the position of the particle. This topic is related to quantum physics and the great German physicist named Werner Karl Heisenberg gave this Heisenberg Uncertainty Principle in 1927. This principle was given after Bohr’s theory failed.

Complete answer:
Bohr's hypothesis thinks about an electron as a material molecule. Its position and momentum can be resolved with exactness. However, when an electron is considered as a wave as proposed by de-Broglie, it is absurd to expect to simultaneously learn the specific position and speed of the electron with full accuracy at a given moment since the wave is stretching out all through a region of space. In 1927, Werner Heisenberg introduced a standard known as Heisenberg Uncertainty rule which states as: "It is difficult to quantify at the same time the specific position and accurate momentum of a body as small as an electron."The mathematical expression of the principle is given as:
$\Delta x \times \Delta y \geqslant \dfrac{h}{{4\Pi }}$
Where $\Delta x$ is the change in the position of the particle, $\Delta y$ is the change in the momentum of the particle and h is called Planck’s constant. Value of Planck’s constant, h = 6.626×10−34 joule-sec

Additional information:Werner Karl Heisenberg was a German theoretical physicist and one of the great scientists of quantum mechanics.

Note:Heisenberg’s uncertainty principle is only valid in the macroscopic world (the uncertainties in the position and velocity of objects with large masses are almost null), it holds significant value in the quantum world. As atoms and subatomic particles have very small masses, a small increase in the accuracy of their positions will be accompanied by an increase in the uncertainty related to their velocities.