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प्रश्न
Explain in brief, the significance of the azimuthal quantum number.
उत्तर
- Azimuthal quantum number is also known as the subsidiary quantum number and is represented by the letter l.
- It represents the subshell to which the electron belongs. It also defines the shape of the orbital that is occupied by the electron.
- Its value depends upon the value of principal quantum number ‘n’. It can have only positive values between 0 and (n − 1).
- Atomic orbitals with the same value of ‘n’ but different values of ‘l’ constitute a subshell belonging to the shell for the given ‘n’. The azimuthal quantum number gives the number of subshells in a principal shell. The subshells have l to be 0, 1, 2, 3 … which are represented by symbols s, p, d, f, … respectively.
Principal shell Value of n Permissible value of l Possible subshell Number of subshells in shell K 1 0 s 1 L 2 0, 1 s, p 2 M 3 0, 1, 2 s, p, d 3 N 4 0, 1, 2, 3 s, p, d, f 4
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| `n` | `l` | `m_l` | |
| (i) | 1 | 1 | +2 |
| (ii) | 2 | 1 | +1 |
| (iii) | 3 | 2 | –2 |
| (iv) | 3 | 4 | –2 |
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| (i) \[\ce{Cu}\] | (a) 1s2 2s2 2p6 3s2 3p6 3d10 |
| (ii) \[\ce{Cu^{2+}}\] | (b) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 |
| (iii) \[\ce{Zn^{2+}}\] | (c) 1s2 2s2 2p6 3s2 3p6 3d10 4s1 |
| (iv) \[\ce{Cr^{3+}}\] | (d) 1s2 2s2 2p6 3s2 3p6 3d9 |
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| Quantum number | Information provided |
| (i) Principal quantum number | (a) orientation of the orbital |
| (ii) Azimuthal quantum number | (b) energy and size of orbital |
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| Column I | Column II |
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| (iii) \[\ce{Ni^{2+}}\] | (c) [Ar]3d64s0 |
| (iv) \[\ce{Cu}\] | (d) [Ar] 3d54s1 |
| (e) [Ar]3d64s2 |
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