What is the correct electron configuration for Iron (Fe)?A[Ar] 4s23d3B1s22s22p3C[Ar] 4s23d6D1s22s22p2

Break Down the Problem

1. Identify the atomic number of Iron (Fe).
2. Determine the electron configuration based on the atomic number.
3. Evaluate the provided options to find the correct configuration.

Relevant Concepts

• The atomic number of Iron (Fe) is 26, indicating that it has 26 electrons.
• Electron configurations are built by filling orbitals in the order defined by the Aufbau principle, Hund's rule, and the Pauli exclusion principle.

Analysis and Detail

1. The electron configuration can be constructed by filling the orbitals in the following order:
   • 1s, 2s, 2p, 3s, 3p, 4s, 3d.
2. Filling the orbitals for 26 electrons:
   • 1s² → 2 electrons
   • 2s² → 2 electrons
   • 2p⁶ → 6 electrons
   • 3s² → 2 electrons
   • 3p⁶ → 6 electrons
   • 4s² → 2 electrons
   • 3d⁶ → 6 electrons
3. Therefore, the complete configuration for Iron is: $1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^6$ which can be abbreviated using noble gas notation as: $[Ar] \, 4s^2 \, 3d^6$

Verify and Summarize

• The option that represents the correct electron configuration for Iron based on the analysis is C: $[Ar] \, 4s^2 \, 3d^6$.

Final Answer

The correct electron configuration for Iron (Fe) is C: [Ar] 4s² 3d⁶.