List I (Spectral Lines of Hydrogen for transitions from) |
List II (Wavelength (nm)) |
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\(\mathrm{A.}\) | \(n_2=3\) 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 \(n_1=2\) | \(\mathrm{IV.}\) | \(486.1\) |
Statement I: | Atoms are electrically neutral as they contain equal number of positive and negative charges. |
Statement II: | Atoms of each element are stable and emit their characteristic spectrum. |
1. | Both Statement I and Statement II are incorrect. |
2. | Statement I is correct but Statement II is incorrect. |
3. | Statement I is incorrect but Statement II is correct. |
4. | Both Statement I and Statement II are correct. |
List-I (Series) |
List-II (Wave number in cm-1) |
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A. | Balmer series | I. | \( R\left(\frac{1}{1^2}-\frac{1}{n^2}\right) \) |
B. | Lyman series | II. | \( R\left(\frac{1}{4^2}-\frac{1}{n^2}\right) \) |
C. | Brackett series | III. | \( R\left(\frac{1}{5^2}-\frac{1}{n^2}\right) \) |
D. | Pfund series | IV. | \( R\left(\frac{1}{2^2}-\frac{1}{n^2}\right)\) |
1. | visible region |
2. | far infrared region |
3. | ultraviolet region |
4. | infrared region |
1. | \(4.77~ \mathring{A}\) | 2. | \(0.53~ \mathring{A}\) |
3. | \(1.06~ \mathring{A}\) | 4. | \(1.59~ \mathring{A}\) |
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. \(2:3\)