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प्रश्न
Number of angular nodes for 4d orbital is ______.
पर्याय
4
3
2
1
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उत्तर
Number of angular nodes for 4d orbital is 2.
Explanation:
The number of angular nodes is given by n – l
Where n is principal quantum number, l is azimuthal quantum number
For 4d orbital, n = 4 and l = 2
Thus, the number of angular nodes = n – l = 4 – 2 = 2
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संबंधित प्रश्न
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| (i) | (a) `n = 3, l = 2, m_l = -2, m_s = - 1/2` |
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| (b) `n = 3, l = 2, m_l = 1, m_s = + 1/2` | |
| (iv) | (a) `n = 3, l = 2, m_l = +2, m_s = - 1/2` |
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(i) Angular quantum number determines the three dimensional shape of the orbital.
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| Quantum number | Information provided |
| (i) Principal quantum number | (a) orientation of the orbital |
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| (iii) Magnetic quantum number | (c) spin of electron |
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| (i) Photon | (a) Value is 4 for N shell |
| (ii) Electron | (b) Probability density |
| (iii) ψ2 | (c) Always positive value |
| (iv) Principal quantum number n | (d) Exhibits both momentum and wavelength |
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