Question

below is the electron configuration of iron. label the parts of the electron configuration

green numbers:

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶

last part:

red letters:

yellow numbers:

location of valence electrons # electron shell or energy level

number of electrons in subshell # subshell

Explanation:

• Green Numbers: In electron configuration, the numbers before the letter (e.g., 1 in 1s, 2 in 2s etc.) represent the electron shell or energy level.
• Yellow Numbers: The superscript numbers (e.g., 2 in \(1s^{2}\), 2 in \(2s^{2}\) etc.) indicate the number of electrons in the sub - shell.
• Red Letters: The letters (s, p, d) represent the sub - shell.
• Last part (\(3d^{6}\)): The \(4s\) orbital is filled before the \(3d\) orbital. But in terms of valence electrons for transition metals like iron, the \(3d\) electrons can also be considered as valence - like in some chemical reactions. However, strictly based on the electron configuration notation rules:
• The general form of electron configuration is \(n\ell^{m}\) where \(n\) (green number) is the principal quantum number (electron shell/energy level), \(\ell\) (red letter) is the sub - shell (s, p, d, f), and \(m\) (yellow number) is the number of electrons in the sub - shell.

Answer:

• Green Numbers: Electron Shell or energy level
• Yellow Numbers: Number of electrons in subshell
• Red Letters: Subshell
• Last part (\(3d^{6}\)): Location of Valence Electrons (for transition metals, \(3d\) electrons can be involved in bonding similar to valence electrons in main - group elements)