Which electron configuration is correct for Sn4+?
A. [Kr]4d10
B. [Kr]5s2 4d8
C. [Kr]5s2 5d8
I know that the answer is A, but can someone explain why it doesn't go in the order of [Kr] 5s2 then 4d10 ?? (Therefore being answer B) The quantum numbers for 3 and 4 go in the order 3s2 3p6 4s2 then 3d10 Why wouldn't this be the case for this problem? Please help!
Sn atomic number is 50 no of electrons are 50 and electron
configuration => [Kr] 5s2 4d10
5p2
when it forms the Sn4+ by loosing the 4 electrons and gets the electron configuration is as follows [Kr] 5s0 4d10 5p0 (or) [Kr] 4d10
because the electrons are removed from the outer most energy orbital i.e from the 5S and 5P orbitals and achieves the [Kr] 5s0 4d10 5p0 by loosing the electrons from the 5S and 5P orbitals it shows the a pseudo-noble gas configuration by the empty orbitals of higher energy levels i.e 5S and 5P orbitals and fullfilled d-subshell i.e 4d shell and this shows the stability to the atom
answer=> due to the pseudo-noble gas configuration and stability attained by the electron configuration of an atom
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