Questions: Write the ground-state electron configuration for a neutral atom of each element: manganese iron

Write the ground-state electron configuration for a neutral atom of each element: manganese iron
Transcript text: Write the ground-state electron configuration for a neutral atom of each element: \begin{tabular}{|c|c|} \hline manganese & $\square$ \\ \hline iron & $\square$ \\ \hline \end{tabular}
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Solution

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Solution Steps

Step 1: Identify the Elements and Their Atomic Numbers

The elements in question are manganese and iron. Manganese has an atomic number of 25, and iron has an atomic number of 26. This means manganese has 25 electrons and iron has 26 electrons in their neutral states.

Step 2: Understand the Electron Configuration Order

The electron configuration follows the order of filling orbitals based on the Aufbau principle, which is generally: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, etc.

Step 3: Write the Electron Configuration for Manganese

For manganese (Mn), with 25 electrons, the electron configuration is:

  • 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵
Step 4: Write the Electron Configuration for Iron

For iron (Fe), with 26 electrons, the electron configuration is:

  • 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶

Final Answer

  • Manganese: \(\boxed{1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^5}\)
  • Iron: \(\boxed{1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^6}\)
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