State Heisenberg's Uncertainty Principle. Show that electron doesn'texist in
the nucleus.Find the accuracy in the position of an electron moving with speed 350
m/sec with uncertainty of 0.01%.
Heisenberg'suncertainty principle states that one can not measure position and
moment of the moving particle exactly.Thus,the inaccuracies Δx and Δp in the
simultaneous determination of the position'x' and momentum 'p'respectively of a particle are related as
Where ħ=h/2π, h being Planck's constant.
Non existence of electron inside the nucleus.
If the electromagnetic is inside the nucleus of radius of the other of10-15m,the maximum
uncertainty in the position of electron will be of the order of its radius
From the limiting condition of Heisenberg's uncertainty principle,
As Δvmin<v v>1.159×1011 m/a>c
Therefore, the electron behaves as are lativistic particle.
The relativistic energy of the electronis
Since,the actual momentum of the electronp >>Δpmin,p2c2>>mo
mass energy of the electron the value of which is 0.511MeV.Hence,
Assuming p=Δpmin,the least energy that an electron should posses within a nucleus
is given by
Inreality, the only source of generation of electron within a nucleus is the process of
decay.The maximum kinetic energy possessed by the electrons during β-decay is about100 KeV.This shows that an electron can not exist within a nucleus
Numerical Solutlon :
Answer: Minimum uncertainty in position is 3.314×10-3m