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प्रश्न
How many radial nodes for 2s, 4p, 5d and 4f orbitals exhibit? How many angular nodes?
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उत्तर
| Orbital | n | l | Radial node n − l − 1 |
Angular node l |
| 2s | 2 | 0 | 1 | 0 |
| 4p | 4 | 1 | 2 | 1 |
| 5d | 5 | 2 | 2 | 2 |
| 4f | 4 | 3 | 0 | 3 |
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संबंधित प्रश्न
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Reason: Number of radial and angular nodes depends only on principal quantum number.
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n = 3, l = 1 and m = –1
The total number of orbitals associated with the principal quantum number n = 3 is
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| n | l | m | s | |
| (i) | 3 | 0 | 0 | `+1/2` |
| (ii) | 2 | 2 | 1 | `-1/2` |
| (iii) | 4 | 3 | –2 | `+1/2` |
| (iv) | 1 | 0 | –1 | `+1/2` |
| (v) | 3 | 4 | 3 | `-1/2` |
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