The electron configuration of chromium is unique because of:

The electron configuration of chromium is unique because of:

• A. Extra electrons in the s subshell
• B. Half-filled d subshell stability
• C. Full p subshell occupation
• D. Greater nuclear charge

Answer: (B)

The unique electron configuration of chromium can be attributed to the stability that arises from a half-filled d subshell. Specifically, chromium has the atomic number 24, and its electron configuration is typically expected to be [Ar] 4s² 3d⁴. However, in practice, it is more stable to have the configuration [Ar] 4s¹ 3d⁵. This arrangement leads to a half-filled d subshell (3d⁵), which is associated with enhanced stability due to exchange energy and symmetry, making it energetically favorable. Half-filled and fully filled subshells exhibit greater stability compared to other configurations, which is why chromium adopts this particular arrangement. This phenomenon is common in transition metals, where d-orbital filling often does not follow the expected pattern strictly based on the Aufbau principle. In terms of the other options, the presence of extra electrons in the s subshell or a full p subshell does not contribute to the unique characteristics of chromium’s electron configuration. Similarly, while a greater nuclear charge does influence overall energy levels and electron interactions, it does not specifically account for the unique stability associated with chromium’s half-filled d subshell.

The unique electron configuration of chromium can be attributed to the stability that arises from a half-filled d subshell. Specifically, chromium has the atomic number 24, and its electron configuration is typically expected to be [Ar] 4s² 3d⁴. However, in practice, it is more stable to have the configuration [Ar] 4s¹ 3d⁵.

This arrangement leads to a half-filled d subshell (3d⁵), which is associated with enhanced stability due to exchange energy and symmetry, making it energetically favorable. Half-filled and fully filled subshells exhibit greater stability compared to other configurations, which is why chromium adopts this particular arrangement. This phenomenon is common in transition metals, where d-orbital filling often does not follow the expected pattern strictly based on the Aufbau principle.

In terms of the other options, the presence of extra electrons in the s subshell or a full p subshell does not contribute to the unique characteristics of chromium’s electron configuration. Similarly, while a greater nuclear charge does influence overall energy levels and electron interactions, it does not specifically account for the unique stability associated with chromium’s half-filled d subshell.