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 is the main idea behind the Aufbau principle?

• Electrons fill orbitals in decreasing order of energy.

• Electrons fill orbitals based on atomic mass.

• Electrons fill orbitals in increasing order of energy.

• Electrons fill orbitals randomly.

According to the n plus l rule, which orbital is filled first?

• The orbital with the highest n value.

• The orbital with the lowest n plus l value.

• The orbital with the highest n plus l value.

• The orbital with the lowest l value.

What happens when two orbitals have the same n plus l value?

• The orbital with the lower n value is filled first.

• The orbital with the higher n value is filled first.

• Both orbitals are filled simultaneously.

• Neither orbital is filled.

What does the Pauli exclusion principle state about electrons in an atom?

• Electrons must have different principal quantum numbers.

• Electrons must have the same azimuthal quantum number.

• Electrons can have the same set of four quantum numbers.

• No two electrons can have the same set of four quantum numbers.

Why is the electronic configuration of chromium considered stable?

• Because it has a completely empty p orbital.

• Because it has a half-filled and fully filled orbital configuration.

• Because it has a half-filled s orbital.

• Because it has a fully filled d orbital.