How do you draw the lewis structure for polyatomic ions?

Question

How do you draw the lewis structure for polyatomic ions?

1 Answer

Impact of this question

7443 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2018-05-30T18:20:18

Well you use [VESPER....](https://socratic.org/questions/how-does-vsepr-theory-classify-molecules)

Explanation:

And $VSEPR \equiv Valence shell electron pair repulsion theory.$ $"VSEPR"-="Valence shell electron pair repulsion theory."$

And I will give ONE bond, the VESPER treatment of nitrate ion...we gots $N O_{3}^{-}$ $NO_3^(-)$ ...and there are ……

$3 \times 6_{oxygen valence electrons} + 5_{nitrogen valence electrons} + 1_{negative charge}$ $3xx6_"oxygen valence electrons"+5_"nitrogen valence electrons"+1_"negative charge"$ $= 24 electrons$ $="24 electrons"$ , i.e. TWELVE electron pairs to distribute over FOUR CENTRES....

And we get.... $O = + N {(- O^{-})}_{2}^{-}$ $O=stackrel(+)N(-O^(-))_2$ ...THREE of the four participating atoms have a formal charge...the leftmost oxygen is NEUTRAL (it has 8 electrons), the nitrogen has SIX electrons, and therefore has a FORMAL POSITIVE charge...and two of the oxygens bear 9 electrons, and thus have a FORMAL NEGATIVE charge... The overall charge is this $+ 1 - 1 - 1 = - 1$ $+1-1-1=-1$ .

Can you try for $S O_{4}^{2 -}$ $SO_4^(2-)$ ?

Science

Math

Humanities

... and beyond

How do you draw the lewis structure for polyatomic ions?

1 Answer

Explanation:

Related questions

Impact of this question