Why do lanthanides have +3 oxidation state(most stable).

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SUMMARY

Lanthanides predominantly exhibit a +3 oxidation state due to their electronic configuration, specifically 4f0-145d0-16s2. This configuration indicates three valence electrons when the 4f and 5d subshells are considered. Although there are instances where lanthanides can show +2 or +4 states, the +3 state remains the most stable due to the stability provided by the filled 5s and partially filled 5d orbitals. The discussion highlights the complexity of oxidation states in lanthanides and the importance of electronic configuration in determining stability.

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Raghav Gupta
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Lanthanides can exhibit 2,4 states also but why 3 is most stable one?
 
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Have you checked their electronic configuration?
 
Borek said:
Have you checked their electronic configuration?
Yes, 4f0-145d0-16s2.
So when d has 1 electron then we can say that there are 3 valence electrons but in case there are 0 electrons in d then it should be 2 , the most stable but that is not so.
What to do?
 
Borek said:
Have you checked their electronic configuration?
You may think that I have understood or answered on my own in above post.
But carefully looking that is not so.
I mean when the elec. con. Is 4f0-145d16s2 the oxidation number is 3 which is okay but how when
elec. con. Is 4f0-145d06s2 the oxidation number could be 3?
Shouldn't that be 2?
 

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