Number of Electrons in Chromium's L=2 Orbital

The electron configuration of an atom describes the distribution of electrons in its atomic orbitals. To determine the number of electrons present in the L=2 orbital of chromium (Cr), we need to understand its electron configuration.

1. Electron Configuration of Chromium (Cr)

The atomic number of chromium is 24, which means it has 24 electrons. The electron configuration of chromium can be determined by following the Aufbau principle, Hund's rule, and the Pauli exclusion principle.

The Aufbau principle states that electrons fill the lowest energy levels first before moving to higher ones. Hund's rule states that electrons fill degenerate orbitals (orbitals with the same energy) singly before pairing up. The Pauli exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers.

The electron configuration of chromium is as follows:

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵

2. Orbital Filling Order

To determine the number of electrons in the L=2 orbital, we need to understand the orbital filling order. The L=2 orbital corresponds to the d orbital.

The orbital filling order is as follows:

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p

3. Filling of the d Orbitals

The d orbitals can hold a maximum of 10 electrons. According to the electron configuration of chromium, its 3d subshell is partially filled with 5 electrons.

4. Number of Electrons in the L=2 Orbital of Chromium

Since the 3d subshell corresponds to the L=2 orbital, we can conclude that chromium has 5 electrons in its L=2 orbital.

Conclusion

In conclusion, the number of electrons present in the L=2 orbital of chromium is 5. This can be determined by understanding the electron configuration of chromium and the filling order of the d orbitals.

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