dumbgeek
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I got the answer of the Electron Config of the ion Mn2+ as

1s22s22p63s23p64s23d3

however the book says its

1s22s22p63s23p63d5, doesn't 4s come before 3d? confused also

electron config shorthand for Cl I got

[Ne] 3p5
book says its [Ne] 3s23p5 why is the bit in bold there?
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Andylol
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(Original post by dumbgeek)
I got the answer of the Electron Config of the ion Mn2+ as

1s22s22p63s23p64s23d3

however the book says its

1s22s22p63s23p63d5, doesn't 4s come before 3d? confused also

electron config shorthand for Cl I got

[Ne] 3p5
book says its [Ne] 3s23p5 why is the bit in bold there?
Transition metals are most stable when their d orbitals have either 5 or 10 electrons, so Mn loses the 4s electrons first to form mn2+

and for Cl, it's [Ne] 3s2 3p5 because... well.. basically, there's a 3s orbital before 3p orbital???

[Ne] = 1s2 2s2 2p6
Cl = 1s2 2s2 2p6 3s2 3p5
or.. [Ne] 3s2 3p5
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Heartdina
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the 4s orbital is lower in energy than the 3d orbital for main group elements. however for transition metals, the 3d orbital is lower than the 4s, thus 4s electrons will be lost first. hence Mn2 has a E.C of [Ar] 3d5 4s0
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MexicanKeith
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(Original post by dumbgeek)
I got the answer of the Electron Config of the ion Mn2+ as

1s22s22p63s23p64s23d3

however the book says its

1s22s22p63s23p63d5, doesn't 4s come before 3d? confused also

electron config shorthand for Cl I got

[Ne] 3p5
book says its [Ne] 3s23p5 why is the bit in bold there?
The full explanation as to the ordering of orbitals in this region of the periodic table is quite complicated and not something you need to worry about unless you’re doing a degree in chemistry, for a level a simple rule is that you fill the 4s before the 3d and empty the 4s before the 3d. This rule usually gives the correct configuration, but it’s not what is actually happening
Last edited by MexicanKeith; 1 week ago
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Marriyaa
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The 4s subshell in transition metals is still at a lower energy level than the 3d subshell, and more stable as well. This is why the electrons fill the 4s subshell in a transition metal first(because they have lower energy) However, when they are losing electrons, the 3d subshells, being closer to the nucleus, they repel the 4s electrons to a higher energy level. since the 4s subshells are at a higher energy level than the 3s subshells, the electrons are lost first from the 4s subshell.
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Hassan nazir
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Half filled orbitals are highly stable and the electrons will be withdrawn from 4s
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Akshat kumar
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Half and completely filled orbitals are more stable than partially filled ones so the configuration given in the book is correct. Electronic configuration of Mn2 is 1s2 2s2 2p6 3s2 3p6 4s0 3d5
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Soumyajeet
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During filling of the electron 4s come before 3d but during losing of electron, it happens from the last shell containing electron i.e., 4th shell or 4s.
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Harshdeep Singh
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Your book is correct because the atom will loose electron from its valence shell first. Here in case of mn,4 shell is valence shell so it will lost electron first from 4s then from 3d
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rbrooks26
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(Original post by dumbgeek)
I got the answer of the Electron Config of the ion Mn2+ as

1s22s22p63s23p64s23d3

however the book says its

1s22s22p63s23p63d5, doesn't 4s come before 3d? confused also

electron config shorthand for Cl I got

[Ne] 3p5
book says its [Ne] 3s23p5 why is the bit in bold there?
for Mn2+ i would say 1s2 2s2 2p6 3s2 3p6 4s0 3d5 because the electrons are always removed from the 4s orbital first. its V confusing i know but just remember that 4s is filled before and has electrons removed before 3d.
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Samvid Pundir
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Exactly the same q. was in my book and it says Configuration of Mn2 is 2,8,13 .It should be 2,8,11,2 .Even I am confused
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