If nitrogen atom has an electronic configuration of $1{\mathrm{s}}^7$, it would have energy lower than that of the normal ground state configuration, $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^3$, because the electrons would be closer to the nucleus, yet $1{\mathrm{s}}^7$ is not observed because it violates

According to Bohr's theory, the energy required for an electron in ${\mathrm{Li}}^{2+}$ ion to be emitted from $\mathrm{n}=2$ state is:

(Given that the ground state ionization energy of hydrogen atom is $13.6 \mathrm{eV})$

The energy of second Bohr orbit of the hydrogen atom is $-328 \mathrm{kJ} {\mathrm{mol}}^{-1}$, hence, the energy of the fourth Bohr orbit would be

What would be the wavelength of the radiation emitted when in a hydrogen atom, an electron falls from infinity to the stationary state $1$? (Rydberg's constant $=1.097\times {10}^7 {\mathrm{m}}^{-1})$

The ratio of the slopes of ${\mathrm{K}}_{\max }$ vs $\mathrm{\nu }$ and ${\mathrm{V}}_0$ vs $\mathrm{\nu }$ curves in the photoelectric effects gives

($\mathrm{\nu }=$ frequency, ${\mathrm{K}}_{\max }=$ maximum kinetic energy, ${\mathrm{V}}_0=$ stopping potential)

For Balmer series in the spectrum of atomic hydrogen, the wave number of each line is given by: $\overline{\mathrm{v}}={\mathrm{R}}_{\mathrm{H}}\left(\frac{1}{{\mathrm{n}}_1^2}-\frac{1}{{\mathrm{n}}_2^2}\right)$, where, ${\mathrm{R}}_{\mathrm{H}}$ is Rydberg constant and ${\mathrm{n}}_1$ and ${\mathrm{n}}_2$ are integers. Which of the following statement(s) is(are) correct?

I. As wavelength decreases, the lines in the series converge.

II. The integer, ${\mathrm{n}}_1$ is equal to $2.$

III. The ionization energy of hydrogen can be calculated from the wave number of these lines.

IV. The line of the longest wavelength corresponds to ${\mathrm{n}}_2=3.$

The energy of an electron in the first Bohr orbit of $\mathrm{H}$ atom is $-13.6 \mathrm{eV}.$ The possible energy value(s) of the excited state (s) for electrons in Bohr orbits of hydrogen is

The ratio of the radius of the first Bohr orbit for the electron orbiting the hydrogen nucleus to that of the electron orbiting the deuterium nucleus (mass nearly twice that of the hydrogen nucleus) is approximately