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Pairing of electron in the orbitals belo...

Pairing of electron in the orbitals belonging to the same sub-shell (p,d or f) does not take place until each orbital belonging to that sub-shell has got one electron each, i.e. it is singly occupied. This is called

A

Hund's rule of maximum multiplisity

B

Paul's exclusion principle

C

Aufbau principle

D

None of the above

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To solve the question regarding the pairing of electrons in orbitals belonging to the same sub-shell, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding Electron Configuration**: - Electrons are arranged in orbitals around the nucleus of an atom. Each orbital can hold a maximum of two electrons with opposite spins. 2. **Identifying Sub-shells**: - Sub-shells are designated as s, p, d, and f. Each sub-shell consists of one or more orbitals. For example, the p sub-shell has three orbitals (px, py, pz), the d sub-shell has five orbitals, and the f sub-shell has seven orbitals. 3. **Filling Electrons in Orbitals**: - When filling electrons into these orbitals, there is a specific order that must be followed to minimize electron-electron repulsion and maximize stability. 4. **Applying Hund's Rule**: - According to Hund's Rule of Maximum Multiplicity, electrons will first fill each orbital in a sub-shell singly before any orbital gets a second electron (pairing occurs). This means that for a given sub-shell, each orbital must have one electron before any of them can have two. 5. **Conclusion**: - The rule that states that pairing of electrons in the orbitals belonging to the same sub-shell does not take place until each orbital has one electron is known as **Hund's Rule of Maximum Multiplicity**. ### Final Answer: The pairing of electrons in the orbitals belonging to the same sub-shell does not take place until each orbital has one electron each, which is called **Hund's Rule of Maximum Multiplicity**. ---
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