state heisenberg's uncertainity principle and explain it mathematically
Answers
Explanation:
According to the Heisenberg’s uncertainty rule, it is not possible to know exactly both the position and the momentum of an electron. Thus, the certainty of determination of one property leads to uncertainty of determination of the other. The uncertainty in the measurement of position, ∆x, and uncertainty of determination of momentum, ∆p are related by Heisenberg’s relationship as-
(∆x) X (∆p) ≥ h/4π
Where h is Planck’s constant.
If ∆x is very small, i.e., the position of the electron is known more or less exactly, ∆p would be large, i.e. uncertainty of momentum will be large or vice- versa.
On the basis of the concept of probability, it is possible to state or predict the probability or relative chance of finding an electron of a particular energy in a given region of space at a given time. The volume in space around the nucleus of the atom, in which there is the maximum probability of finding an electron, is called an orbital. The charge on the electron is diffused just like a cloud. The regions in space where the density of charge cloud is highest are called as atomic orbitals. Most of the time, the possibility of finding an electron in these orbitals is very large