Let \(L_1\) and \(L_2\) be the orbital angular momentum of an electron in the first and second excited states of the hydrogen atom, respectively. According to Bohr's model, the ratio \(L_1:L_2\) is:
1. \(1:2\)
2. \(2:1\)
3. \(3:2\)
4. \(2:3\)
1. | \(4.77~ \mathring{A}\) | 2. | \(0.53~ \mathring{A}\) |
3. | \(1.06~ \mathring{A}\) | 4. | \(1.59~ \mathring{A}\) |
1. | visible region |
2. | far infrared region |
3. | ultraviolet region |
4. | infrared region |
The total energy of an electron in the \(n^{th}\) stationary orbit of the hydrogen atom can be obtained by:
1. \(E_n = \frac{13.6}{n^2}~\text{eV}\)
2. \(E_n = -\frac{13.6}{n^2}~\text{eV}\)
3. \(E_n = \frac{1.36}{n^2}~\text{eV}\)
4. \(E_n = -{13.6}\times{n^2}~\text{eV}\)
List I (Spectral Lines of Hydrogen for transitions from) |
List II (Wavelength (nm)) |
||
\(\mathrm{A.}\) | \(n_2=3\) to \(n_1=2\) | \(\mathrm{I.}\) | \(410.2\) |
\(\mathrm{B.}\) | \(n_2=4\) to \(n_1=2\) | \(\mathrm{II.}\) | \(434.1\) |
\(\mathrm{C.}\) | \(n_2=5\) to \(n_1=2\) | \(\mathrm{III.}\) | \(656.3\) |
\(\mathrm{D.}\) | \(n_2=6\) to \(n_1=2\) | \(\mathrm{IV.}\) | \(486.1\) |