What would the electron configuration of [Pt]2+ be? I can't figure it out, it keeps telling me I'm wrong (I had to do about 12, and this is the only one I couldn't figure out.)
Thanks.
2007-01-20 06:56:52 · 1 answers · asked by countrygurl587 3 in Science & Mathematics ➔ Chemistry
[Xe] 4f14 5d8 worked, thanks!!!
2007-01-20 07:43:04 · update #1
Analysis. From the periodic table Pt is a transition metal in 6th period. Also note the Pt already went thru the 57-72 "loop" that means it has to have not only 5d orbitals but also 4f orbitals.
Moreover, make the adjustment of deducting 2 electrons from metallic Pt- so you only have to account for 76 electrons not 78.
The electronic configuration of Pt is [Xe]4f14 5d9 6s1
then, the electronic configuration of Pt2+ is [Xe] 4f14 5d8, where all the d orbitals are paired.
If this will still give you an error message then use [Xe] 4f14 5d7 6s1, but I doubt it.
2007-01-20 07:25:39 · answer #1 · answered by Aldo 5 · 0⤊ 0⤋