Issaga B.

asked • 04/21/20

Chemical bonding

Draw the Lewis structure for the acetate ion,

CH3CO2, including any important resonance structures. Label each atom with its formal charge.

J.R. S.

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I tried to answer this question with a video recording and also in the answer section below but apparently it didn't work. The only way I can describe the Lewis dot with resonance and format charge is to tell you what it looks like. It will have a C atom with 3 H atoms attached and another C atom attached. This 2nd C has a double bonded O and a single boned O. The double bonded O has 2 lone pairs; the single bonded O has 3 lone pairs. All atoms have a formal charge of zero except the single bonded O which has a formal charge of -1. The resonance structure is the same except you change the position of the double bonded O. Hope this makes sense and helps.
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04/21/20

1 Expert Answer

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Helen B. answered • 06/03/20

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Helen B.

Total Valence electrons of CH3COO- =(2*4)+(2*6)+(3*1) =23 and 1 electron for the minus charge =24 electrons Each single bond =2e- and and each dot represent an e-. 7bonds =14e- and 10 dots =10e- which makes a total of 24 electrons. Arrange the elements such a way the least electronegative atom goes to the center(H is an exception) and distribute the electrons such a way each atom gets an octet number of electrons. H is an exception gets duet number of electrons.
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06/03/20

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