Question

Using Heisenberg's uncertainty principle, can you prove that electrons can never exist in a nucleus?

Answer 1

Hint: Heisenberg’s uncertainty principle states that it is impossible to determine both the position and momentum of the electron in an orbit. This principle can be useful to calculate these two terms only. Nucleus consists of only protons and neutrons as it is a positively charged sphere.

Complete answer:
Atoms are the basis for the combination of atoms that leads to the formation of molecules. Every atom is neutral as it has an equal number of protons, and equal number of electrons. An atom has a positively charged sphere at the center of a nucleus which can be called a nucleus. Nucleus consists of protons and neutrons.
Heisenberg’s uncertainty principle was stated by German physicist Werner Heisenberg’s. It gives the relationship between momentum and position of an electron. It states that finding the position and momentum of an electron is not possible simultaneously.
Heisenberg’s uncertainty principle is given as $ \Delta x \times \Delta p \geqslant \dfrac{h}{{4\pi }} $
 $ \Delta x $ is uncertainty in position
 $ \Delta p $ is uncertainty in velocity
 $ h $ is Planck’s constant and has the value of $ 6.6 \times {10^{ - 34}}J\sec $
Thus, when uncertainty in velocity is given, uncertainty in position can be determined and vice versa. Thus, this principle cannot explain anything about the existence of an electron in the nucleus.

Note:
Neutrons are charged less subatomic particles, whereas protons are positively charged subatomic particles. These both subatomic particles give the nucleus positively charged. But electrons are negatively charged which are present outside the nucleus. These two oppositely charged forces balance the atom.