An accelerated electron has a speed of $5 \times 10^{6} \ m \ s^{-1}$ with an uncertainty of $0.02 \ \%$. The uncertainty in finding its location while in motion is $x \times 10^{-9} \ m$. The value of $x$ is $......$ (Nearest integer)
[Use mass of electron $= 9.1 \times 10^{-31} \ kg, h = 6.63 \times 10^{-34} \ J \ s, \pi = 3.14]$

The simultaneous determination of the exact position and momentum of an electron is:

Given below are two statements:
Statement $I:$ According to Bohr's model of hydrogen atom,the angular momentum of an electron in a given stationary state is quantised.
Statement $II:$ The concept of electron in Bohr's orbit,violates the Heisenberg uncertainty principle.
In the light of the above statements,choose the most appropriate answer from the options given below:

If a proton is accelerated to a velocity of $3 \times 10^7 \text{ ms}^{-1}$ which is accurate up to $\pm 0.5 \%$,then the uncertainty in its position will be $\ldots \ldots \ldots$ [mass of proton $= 1.66 \times 10^{-27} \text{ kg}$,$h = 6.6 \times 10^{-34} \text{ Js}$]

What is the uncertainty product $\Delta v \cdot \Delta x$ for a particle of mass $1 \ mg$? What does this imply?

What is indicated by $\psi$ for atomic and molecular orbitals? How is the molecular orbital obtained by the Schrodinger wave equation?