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प्रश्न
State Hund’s rule of maximum multiplicity with a suitable example.
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उत्तर
Hund’s rule of maximum multiplicity:
- Statement: “Pairing of electrons in the orbitals belonging to the same subshell does not occur unless each orbital belonging to that subshell has got one electron each.”
- For example, according to Hund’s rule, each of the three-degenerate p-orbitals must get one electron of parallel spin before anyone of them receives the second electron of opposite spin. Therefore, the configuration of four electrons occupying p-orbitals is represented as
and not as↑↓ ↑ ↑ ↑↓ ↑↓ - As a result of Hund’s rule, the atom with fully filled and half-filled set of degenerate orbitals has extra stability.
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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 |
| (e) 1s2 2s2 2p6 3s2 3p6 3d3 |
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| (i) Principal quantum number | (a) orientation of the orbital |
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| (iii) Magnetic quantum number | (c) spin of electron |
| (iv) Spin quantum number | (d) shape of the orbital |
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