Question

Why electrons don't exist in nucleus using uncertainty principle?

Answer 1

the nucleus contains protons and neutrons and is a positively charged body. the electrons are negatively charged bodies which move in their elliptical orbits around the nucleus. if the electrons would fall into the nucleus the atom would collapse.
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Answer 2

The non existence of electron inside the nucleus can be explained by using the concept of Heisenberg’s uncertainty principle.

The basic funda behind this principle is that the position and momentum of a particle cannot be simultaneously measured with arbitrarily high precision. There is a minimum for the product of the uncertainties of these two measurements.

This throws light upon the fact that the measurement of these two parameters is always accompanied by a certain amount of uncertainty. And this even holds good for energy and time as such.

So next if we jump on to the actual question asked it is highly impossible to accommodate electrons inside a nucleus.And this can be theoretically proved using Heisenberg's uncertainty principle.

The atomic radius of any nucleus considered is (10^-15) for an electron to be inside a nucleus it is supposed to have a maximum uncertainty of (10^-15) metre in position.

We know that the mass of an electron is 9.1*10^(-31) Kg.Now if we further move on by substituting all the known parameter and end up finding the velocity , we get a value equal to 5.77*10^(10) m/s which is higher than the usual velocity of light (3*10^8 m/s).

Therefore it is highly impossible for an electron to exist inside a nucleus.

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