Q. No.| 1. | \(h\) | 2. | \(\dfrac{h}{2}\) |
| 3. | \(\dfrac{h}{2 \pi}\) | 4. | \(\dfrac{h}{\lambda}\) |
1. \( 4.2 \times 10^6 ~\text{m/s} \)
2. \( 8.4 \times 10^6 ~\text{m/s} \)
3. \( 2.1 \times 10^6~\text{m/s} \)
4. \( 3.6 \times 10^6 ~\text{m/s} \)
Which of the following statements correctly describes Bohr's model of the atom?
| 1. | It incorporates Einstein’s photoelectric equation. |
| 2. | It predicts a continuous emission spectrum for atoms. |
| 3. | The quantization of angular momentum is a key postulate of Bohr's model. |
| 4. | It predicts identical emission spectra for all types of atoms. |
| 1. | \(\mu_n\propto n\) |
| 2. | \(\mu_n\propto n^2\) |
| 3. | \(\mu_n\propto {\Large\frac{1}{n}}\) |
| 4. | \(\mu_n\propto {\Large\frac{1}{n^2}}\) |
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| 1. | \(11.3\times 10^{-11}\) m | 2. | \(12.9\times 10^{-11}\) m |
| 3. | \(15.9\times 10^{-11}\) m | 4. | \(47.7\times 10^{-11}\) m |
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. \(E_n = -{13.6}\times{n^2}~\text{eV}\)
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The speed of the electron in a hydrogen atom in the \({n=1}\) level is:
1. \(1.1 \times10^{6} ~\text{m/s}\)
2. \(2.18 \times10^{6} ~\text{m/s}\)
3. \(1.08\times10^{6} ~\text{m/s}\)
4. \(3.07 \times10^{6} ~\text{m/s}\)
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The angular momentum of the particle in its orbit is:
| 1. | \(\Large\frac{h}{2\pi}\) | 2. | \(\Large\frac{h}{\pi}\) |
| 3. | \(\Large\frac{3h}{2\pi}\) | 4. | \(\Large\frac{2h}{\pi}\) |
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| 1. | zero; \(13.6\) eV |
| 2. | \(-6.8\) eV; \(-6.8\) eV |
| 3. | \(13.6\) eV; \(-27.2\) eV |
| 4. | \(-13.6\) eV; zero |
The Bohr's model of the atom:-
1. Assumes that the angular momentum of electrons is quantized.
2. Uses Einstein's photo-electric equation.
3. Predicts continuous emission spectra for atoms.
4. Predicts the same emission spectra for all types of atoms.
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