The ratio of kinetic energy to the total energy of an electron in a Bohr orbit of the hydrogen atom is:

1. 1 : 1

2. 1 : -1

3. 2 : -1

4. 1 : -2

The ratio of wavelengths of the last line of Balmer series and the last line of Lyman series is:
1. \(1\)
2. \(4\)
3. \(0.5\)
4. \(2\)

If an electron in a hydrogen atom jumps from the 3rd orbit to the 2nd orbit, it emits a photon of wavelength $\lambda$. When it jumps from the 4th orbit to the 3rd orbit, the corresponding wavelength of the photon will be:

1.  $\frac{16}{25}\mathrm{\lambda }$

2.  $\frac{9}{16}\mathrm{\lambda }$

3.  $\frac{20}{7}\mathrm{\lambda }$

4.  $\frac{20}{13}\mathrm{\lambda }$

Given that the value of the Rydberg constant is 10⁷ m^-1, what will be the wave number of the last line of the Balmer series in the hydrogen spectrum?
1. \(0.5 \times 10^{7} ~m^{-1}\)
2. \(0.25 \times 10^{7} \mathrm{~m}^{-1}\)
3. \(2.5 \times 10^{7} \mathrm{~m}^{-1}\)
4. \(0.025 \times 10^{4} ~m^{-1}\)