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What is the correct configuration for Zn2+?
Why is the answer [Ar]4s0 3d10 and not [Ar]4s2 3d8
Why is the answer [Ar]4s0 3d10 and not [Ar]4s2 3d8
Only the outermost electrons are extracted. So 4s.n2o* said:What is the correct configuration for Zn2+?
Why is the answer [Ar]4s0 3d10 and not [Ar]4s2 3d8
Richnator said:Only the outermost electrons are extracted. So 4s.
You look at the primary quantum number for outermost, so 4 .n2o* said:doesn't 4s fill before 3d? so wouldn't 3d be the outermost? Or are you just looking at n=4 vs. n=3?
n2o* said:doesn't 4s fill before 3d? so wouldn't 3d be the outermost? Or are you just looking at n=4 vs. n=3?
714guy said:The 4s shell does normally fill up first, but for some transitional metals 1/2 or completely filled D subshells for are more stable. So in the case of Zn2+ it donates the 2 e- from the 4s to 3d to completely fill it making it most stable.
n2o* said:are u saying that if we were not dealing with a transition metal, the answer would be different?
n2o* said:What is the correct configuration for Zn2+?
Why is the answer [Ar]4s0 3d10 and not [Ar]4s2 3d8
Sweeti8286 said:You always take from s shell first then d (b/c 4s has a higher energy than 3d....and things like to have lowest energy to be more stable) Also, having a half filled or full electron shell is the more stable and preferred) For example, copper..Cu....the electron config is [Ar]4s1 3d10 not [Ar]4s2 3d9
n2o* said:3d is a higher energy than 4s. n+l for 3d is 3+2, while 4s is 4+0. I do kind of understand the explanations that were given, tho.