What is the electron configuration of an isolated Fe atom (no ligands bound to it)?
(Use notation like [Ne]3s^23p^6 for your answer)
B. What is the electron configuration of an isolated Fe3+ cation?
(Use notation like [Ne]3s^23p^6 for your answer)
[Ar]3d^8 and [Ar]3d^5
To determine the electron configuration of an isolated Fe atom, we need to look at the periodic table.
A. Electron Configuration of an Isolated Fe Atom:
1. Locate Fe (Iron) on the periodic table. It is in the 26th position.
2. Starting from hydrogen (H) and moving across the periodic table, we find that the electron configuration of Fe is [Ar]4s^23d^6.
- The [Ar] represents the electron configuration of the noble gas Argon (Ar), which has the electron configuration 1s^22s^22p^63s^23p^6.
- After [Ar], we have 4s^23d^6.
So, the electron configuration of an isolated Fe atom is [Ar]4s^23d^6.
Moving on to the next question,
B. Electron Configuration of an Isolated Fe3+ Cation:
When Fe loses 3 electrons to form Fe3+ cation, the electron configuration changes.
1. Write out the electron configuration of an isolated Fe atom ([Ar]4s^23d^6).
2. Remove three electrons from the highest energy level (valence shell), in this case, the 4s orbital.
- Since the 4s orbital can hold a maximum of 2 electrons, we remove both electrons from the 4s orbital.
- So, we are left with [Ar]3d^6.
Thus, the electron configuration of an isolated Fe3+ cation is [Ar]3d^6.