Filling of Orbital in Atoms

The video tutorial covers the Aufbau principle, which explains the order of filling orbitals with electrons based on increasing energy levels. It highlights exceptions to this principle, such as the filling of 4f and 5d orbitals. The n+l rule is introduced to determine the energy order of orbitals. The Pauli exclusion principle is explained, emphasizing that no two electrons can have the same set of quantum numbers. The video also discusses the electronic configuration of chromium, noting its stability due to half-filled and fully filled orbitals.

What does the Aufbau principle state about the filling of orbitals with electrons?

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Explain how to draw the Aufbau diagram.

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What are the exceptions to the Aufbau principle regarding the filling of 4f and 5d orbitals?

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Describe the n plus l rule and its significance in determining the order of orbital filling.

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How does the Pauli exclusion principle relate to the electronic configuration of atoms?

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