A student analyzes the ground-state electron configuration of a neutral transition metal atom in Period 4. Magnetic susceptibility measurements demonstrate that this neutral atom possesses exactly six unpaired electrons in its ground state. Based on quantum mechanical principles and orbital stability, which electron configuration correctly represents this ground state, and what accounts for this arrangement?

A) [Ar] 4s² 3d⁴, because the 4s orbital is lower in energy and must remain completely filled before any electrons enter the 3d subshell.

B) [Ar] 3d⁶, because the 4s subshell is evacuated in transition elements to lower the principal quantum number of valence electrons.

C) [Ar] 4s¹ 3d⁵, because having half-filled 4s and 3d subshells provides enhanced stability through maximized exchange energy.

D) [Ar] 4s² 3d² 4p², because Hund's rule requires valence electrons to populate degenerate 4p orbitals before pairing in the 3d subshell.

Electron configurations Transitional Reasoning Practice

Chemistry · Atomic Structure · Chemistry · Electrons in Atoms

1 Chemistry practice questions on Electron configurations. Questions that build towards applied reasoning.

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Atomic Structure · Chemistry

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