Electron Configuration of Mn +4: Explained and Simplified

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In summary, the confusion about the electron configuration of ions is due to the crystal field splitting of the d orbitals when transition metals bind with ligands. This causes the 3d levels to become lower in energy than the 4s level, leading to a more stable configuration. This concept is covered in Chapter 24 of the book "Chemistry: The Central Science" and is typically studied in second year university inorganic chemistry.
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MichaelXY
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Homework Statement



I am a little unclear on the electron configuration of ions. For example; Mn +4 would seem to be 4s2 3d1, but instead it is 3d3. Ok, I get that an atom is stable at half full, or full, but it is not clear to me why 3d3 is anymore stable than 4s2 3d1.
Could someone help me here?

Thanks
 
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  • #2
I'm not sure if you have come across this yet, but that configuration is due to the crystal field splitting of the d orbitals when transition metals bind with ligands (molecule or ion that binds to a metal ion to form a complex). The 4s and 3d levels are not much different in energy and when a metal ion has ligands bound to it, the 3d levels can become lower than the 4s one due to a gain in stabilization energy. So the 4s electrons move over to the 3d orbitals.

Then all the d orbitals are no longer all the same energy with 3 of them lower and 2 higher or vice versa or other configuration (it depends on the molecular structure) And anytime a chemical species can find itself in a lower energy state, it will do that.

see these for more info
http://en.wikipedia.org/wiki/Crystal_field_theory
http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch12/crystal.php
 
  • #3
Thanks for the response. To be honest I had to look up ligands in my book. It is covered in Chap 24 of my book, I am on chap 6-7 (Electron Configurations). So what you said went way over my head.
BTW the book I am using is Chemistry The central science by Brown lemay Burstein.
Thanks for the help though.
 
  • #4
Yes, good book see pg 1034-1039. And its a subject covered in maybe 2nd year univ inorganic chemistry. So I didn't think it would make much sense at this point.
 

1. What is the electron configuration of Mn+4?

The electron configuration of Mn+4 is [Ar] 3d3 4s2.

2. Why does Mn+4 have this electron configuration?

Mn+4 has this electron configuration because it has lost four electrons, leaving it with a +4 charge. This results in the outermost energy level being filled with 18 electrons, following the stability rule known as the octet rule.

3. How is the electron configuration of Mn+4 determined?

The electron configuration of Mn+4 can be determined by using the Aufbau principle, which states that electrons fill orbitals in order of increasing energy. The 4s orbital is filled before the 3d orbital, resulting in the electron configuration [Ar] 3d3 4s2.

4. What is the shorthand notation for the electron configuration of Mn+4?

The shorthand notation for the electron configuration of Mn+4 is [Ar] 3d3 4s2, as the noble gas argon serves as the "core" electrons for Mn+4, while the valence electrons in the 3d and 4s orbitals are represented outside the brackets.

5. How does the electron configuration of Mn+4 affect its chemical properties?

The electron configuration of Mn+4 affects its chemical properties by making it a highly reactive element. With 18 electrons in its outermost energy level, Mn+4 is able to gain or lose electrons to form various compounds and exhibit a wide range of oxidation states.

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