Structure of At...

The number of revolutions per second made by an electron in the first Bohr's orbit of hydrogen atom is(Given, $$r=0.53\overset{o}{A}$$).

The highest energy in Balmer series, in the emission spectra of hydrogen is represented by:
$$\left({R}_{H}=109737 {cm}^{-1}\right)$$

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

Which of the following orbitals has the highest energy?

The spectral lines corresponding to the radiation emitted by an electron jumping from higher orbits to first orbit belong to:

If the shortest wavelength of the spectral line of $${ He }^{ + }$$ in Lyman series is $$x$$, then longest wavelength of the line in Balmer series of $${ Li }^{ 2+ }$$ is:

The fast emission line on hydrogen atomic spectrum in the Balmer series appears at:

The magnitude of potential energy of an electron in the second Bohr orbit of a hydrogen atom is:

The minimum wavelength absorbed by electron initially present in $$(n_1+1)$$ shell of $$Li^{+2}$$ ion:(during its excitation)

Calculate the wavelength of the first line of $$He^{+}$$ ion spectral series whose interval with extreme lines is:
$$\dfrac{1}{\lambda_{1}} - \dfrac{1}{\lambda_{2}} = 2.7541 \times 10^{4} cm^{-1}$$