QQuestionChemistry
QuestionChemistry
2. Complete the two Lewis structures of the acetate ion, $\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}{ }^{-}$, showing resonance.
| H | 0 | H | 0 |
| --- | --- | --- | --- |
| H - C-C | and | H-C-C | |
| H | 0 | H | 0 |
Draw acetic acid, $\mathrm{HC}*{2} \mathrm{H}*{3} \mathrm{O}*{2}$, which has the additional hydrogen attached to one of the oxygen atoms:
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Answer
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Step 1:: Draw the Lewis structure for acetic acid, which has the molecular formula HC^2H^3O^2.
Start by drawing the skeletal structure with carbon (C) atoms bonded to four other atoms, oxygen (O) atoms bonded to two other atoms, and hydrogen (H) atoms bonded to one other atom. There are two C atoms, two O atoms, and five H atoms in acetic acid. H - C - C - O - H | | H - C - O - H
Step 2:: Add enough electrons to complete the octets of all the atoms.
In this case, there are a total of 16 valence electrons (8 from the C atoms, 6 from the O atoms, and 2 from the H atoms) in acetic acid. Place these electrons around the skeletal structure as lone pairs and bond pairs. H - C - C - O:- H: | | H - C - O:-
Step 3:: To show resonance in the acetate ion (C^2H^3O^2 -), move one of the lone pairs of electrons on the negatively charged oxygen atom to form a double bond with the carbon atom it is bonded to.
This creates a second resonance structure. H - C - C - O:- H: | | H - C = O H - C - C - O: H: | | H - C - O:
Step 4:: The final Lewis structures of the acetate ion showing resonance are:
H - C - C - O:- H: | | H - C = O H - C - C - O: H: | | H - C - O:
Step 5:: To draw acetic acid, which has the additional hydrogen attached to one of the oxygen atoms, add an H atom to one of the oxygen atoms in the Lewis structure for acetic acid.
H - C - C - O:- H: | | H - C = O - H
Final Answer
H - C - C - O:- H: | | H - C = O H - C - C - O: H: | | H - C - O: And the Lewis structure of acetic acid is: H - C - C - O:- H: | | H - C = O - H
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