The Heisenberg uncertainty principle can be applied to :

The mass of an electron is $9.11 \times 10^{-31} \ kg$,and the Planck constant is $6.626 \times 10^{-34} \ J \ s$. The uncertainty involved in the measurement of velocity within a distance of $0.1 \ \mathring{A}$ is:

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

The mass of particle $A$ is $5$ times that of particle $B$. The uncertainty in their velocities are $0.05 \ ms^{-1}$ and $0.02 \ ms^{-1}$ respectively. What is the ratio of the uncertainties in their positions,i.e.,$\Delta x_A : \Delta x_B$?

For an electron,if the uncertainty in velocity is $\Delta \nu$,the uncertainty in its position $(\Delta x)$ is given by:

What is $\psi$ and what is $|\psi|^2$? What do they represent?