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प्रश्न
Calculate the total number of angular nodes and radial nodes present in 3p orbital.
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उत्तर
The number of radial nodes is given by n – l – 1, where n is the principal quantum number, l is the azimuthal quantum number.
The number of angular nodes is given by n – l, where n is the principal quantum number, l is the azimuthal quantum number.
Here n = 3 and l = 1
Thus, angular nodes = 3 – 1 = 2 and radial node = 3 – 1 – 1 = 1.
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संबंधित प्रश्न
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| (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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| (i) \[\ce{Cr}\] | (a) [Ar]3d84s0 |
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