A mathematical representation is given below:
`DeltaX xx Deltap_(x) ge h/(4pi)`
b) If the position of the electron is measured within an accuracy of `+-0.002` nm. Calculate the uncertainty in the momentum of the electron.

A mathematical representation is given below: DeltaX xx Deltap_(x) ge h/(4pi) a) Which principle is illustrated by this equation?

A microscope with suitable photons is employed to locate an electron in an atom within a distance of 0.4A. What is the uncertainty involved in the measurement of its velocity?

A microscope with suitable photons is employed to locate an electron in an atom within a distance of 0.4A. What is the uncertainty involved in the measurement of its velocity?

Werner Heisenberg considered the limits of how precisely we can measure the properties of an electron or other microscopic particle. He determined that there is a fundamental limit to how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse is also true. This is summed up in what we now call the Heisenberg uncertainty principle. The equation is Delta x Delta (mv) ge (h)/(4 pi) The uncertainty in the position or in the momentum of a macroscopic object like a baseball is too small to observe. However, the mass of microscopic object such as an electron is small enough for the uncertainty to be relatively large and significant. If the uncertainties in position and momentum are equal, the uncertainty in the velocity is:

Werner Heisenberg considered the limits of how precisely we can measure the properties of an electron or other microscopic particle. He determined that there is a fundamental limit to how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse is also true. This is summed up in what we now call the Heisenberg uncertainty principle. The equation is Delta x Delta (mv) ge (h)/(4 pi) The uncertainty in the position or in the momentum of a macroscopic object like a baseball is too small to observe. However, the mass of microscopic object such as an electron is small enough for the uncertainty to be relatively large and significant. If the uncertainty in velocity and position is same, then the uncertainty in momentum will be:

An electron is moving with a velocity of 2.5 xx 10^(6) ms^(-1) . If the uncertainty in its velocity is 0.1% , calculate the uncertainty in its position. (Plank's constant, h = 6.626 xx 10^(-34) Js),( Mass of the electron = 9.1 xx 10^(-31) kg.)

For one-electron species, the wave number of radiation emitted during the transition of electron from a higher energy state (n_(2)) to a lower energy state (n_(1)) is given by: bar v =(1)/(lamda)=R_(H) xx Z^() ((1)/(n_(1)^(2)) (1)/(n_(2)^(2))) where R_(H)=(2 pi m_(s) k^(2) c^(4))/(h^(3) c) is Rydberg constant for hydrogen atom. Now, considering nuclear motion, the accurate measurement would be obtained by replacing mass of electron (m_(e)) by the reduced mass (mu) in the above expression, defined as mu =(m_(n)xx m_(e))/(m_(n) +m_(e)) where m_(n) = mass of nucleus. For Lyman series, n_(t) =1 (fixed for all the lines) while n_(2) = 2, 3, 4 .... For Balmer series: n_(1) = 2 (fixed for all the lines) while n_(2) = 3,4,5 .... If proton in hydrogen nucleus is replaced by a positron having the same mass as that of an electron but same charge as that of proton, then considering the nuclear motion, the wavenumber of the lowest energy transition of He+ ion in Lyman series will be equal to