A golf ball has a mass of 40g and a speed of 45m/s. If the speed can be measured within accuracy of 2%, calculate the uncertainty in the position.
If the position of the electron is measured within an accuracy of calculate the uncertainty in the momentum of the electron. Suppose the momentum of the electron is is there any problem in defining this value?
In view of Heisenberg’s uncertainty principle, Bohr’s model of the atom in which electrons are treated as particles revolving in definite orbits is meaningless. Thus, its trajectory can not be described as was done by Bohr.
Since in view of Heisenberg’s uncertainty principle, the exact position and momentum of a small moving panicle- like electron can not be determined simultaneously. so the best way is to speak of the probability of finding an electron in a certain region of space around the nucleus rather than describing its specific position. Thus, Heisenberg’s uncertainty principle introduces the concept of probability.