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What is the formula of the ion formed when the tin achieves a stable electron configuration?

Updated: 10/11/2021

Wiki User

∙ 6y ago

Best Answer

It could be either Sn2+ ion (stannous ion) or Sn4+ ion (stannic ion)

Barrett Kunze ∙

Lvl 10

∙ 2y ago

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Wiki User

∙ 14y ago

A tin atom has an electron configuration with the first 3 shells full. Then 5s2 4d10 5p 2. However the most common stable ion of Tin has a charge of +4, as in SnCl4. Now the electron configuration is 4s2 3d10 4p6 5s0 4d10 5p 0 . $ electrons have been taken by the 4 Chloride's.

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