Explain Heisenberg's uncertainty principle .

Mathematically, Heisenberg's uncertainty principle can best be explained by

The formula for Heisenberg's uncertainty principle is

State the expression for Heisenberg.s uncertainty principle.

State Heisenberg's uncertainty principle. If the uncertainties in the measurement of position and momentum of an electron are equal calculate the uncertainty in measuring the velocity.

Why electron cannot exist inside the nucleus according to Heisenberg's uncertainty principle?

According to Heisenberg's uncertainty principle, on increasing the wavelength of light used to locate a microscopic particle, uncertainly in measurement of position of particle :

It is impossible to determine simultaneously the position of velocity of small microscopic particle such as electron , proton or neutron with accuracy .This is called Heisenberg's uncertainty principle. Mathematically, it is represented as Delta x. Delta p ge (h)/(4pi) , Delta x is uncertainty in position Delta p is uncertainty in momentum.

Using Heisenberg's uncertainty principle, calculate the uncertainty in velocity of an electron if uncertainty in its position is 10^(-11)m Given, h =6.6 xx 10^(-14)kg m^2s^(-1), m=9.1 xx 10^(-31)kg

Which of the following is the most correct expression for Heisenberg's uncerainty principle?

It is not possible to determine precisely both the position and momentum (or velocity) of a small moving particle such as electron, proton etc. This is known as Heisenberg uncertainty principle. The mathematical form of this principle is : Delta x.Delta p ge (h)/(4pi) (constant) However this principle is irrelevant in case of bigger particles such as a cup, ball, car etc., that we come across in our daily life. In case of small microscopic particles, Heisenberg's uncertainty principle rules out simultaneous exact determination of their