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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: ParaChase on February 24, 2013, 10:07:29 PM

Title: Sn3+?
Post by: ParaChase on February 24, 2013, 10:07:29 PM

Can anyone tell me why there is no Tin(III), but there is Tin(IV) and Tin(II)? I can't seem to find it online... Thanks!

Title: Re: Sn3+?
Post by: Stovn0611 on February 24, 2013, 11:02:48 PM

Tin(II) would have the electron configuration [Kr]5s²4d¹⁰
Tin(IV) would have the electron configuration [Kr]4d¹⁰

Tin(III) would have an electron remaining in the 5s orbital which would be unstable, but losing 2 or 4 electrons allows all of its orbitals to be full which makes it more stable

Title: Re: Sn3+?
Post by: ParaChase on February 25, 2013, 01:48:25 AM

Ah, ok. I forgot about electron configurations there. Thanks