The kinetic energy of an electron in the ground state of a $Be^{3+}$ ion is given by:

According to the Bohr model for the hydrogen atom,the radius of stationary orbits is proportional to which of the following?

For any given series of spectral lines of atomic hydrogen,let $\Delta \bar{\nu} = \Delta \bar{\nu}_{\max} - \Delta \bar{\nu}_{\min}$ be the difference in maximum and minimum wavenumbers in $cm^{-1}$. The ratio $\Delta \bar{\nu}_{\text{Lyman}} / \Delta \bar{\nu}_{\text{Balmer}}$ is

The radii of the first Bohr orbit of $H$ $(r_{H})$,$He^{+}$ $(r_{He^{+}})$ and $Li^{2+}$ $(r_{Li^{2+}})$ are in the order

When electronic transition occurs from a higher energy state to a lower energy state with an energy difference equal to $\Delta E$ electron volts,the wavelength of the emitted line is approximately equal to

Choose the correct option regarding: Assertion: Energy of the orbital decreases with increase of $n$.
Reason: Energy is required in shifting away the negatively charged electron from the positively charged nucleus.