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 ${\mathrm{n}}_2=3.$

In Bohr series of lines of hydrogen spectrum, the third line from the red-end corresponds to which one of the following inter-orbit jumps of the electron for Bohr orbits in an atom of hydrogen?

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