QQuestionChemistry
QuestionChemistry
Draw the Lewis structure for the acetate ion, CH^3CO2^-, including any important resonance structures. label each atom with its formal charge. thank you in advance!
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Answer
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Step 1:: Determine the total number of valence electrons in the acetate ion
The acetate ion, CH^3CO^2 -, is formed by removing one hydrogen atom from acetic acid. Therefore, the acetate ion has one less proton and one less electron than acetic acid. Acetic acid has 6 carbon valence electrons, 8 hydrogen valence electrons, and 4 oxygen valence electrons, for a total of 18 valence electrons. Since the acetate ion has one less electron than acetic acid, the acetate ion has 17 valence electrons.
Step 2:: Draw the skeletal structure of the acetate ion
The acetate ion has a total of 17 valence electrons. Place one electron between each pair of bonded atoms to form single bonds. This uses up 8 electrons, leaving 9 electrons for the remaining atoms. Place one electron around the oxygen atom to form a negative charge, indicating that it has one more electron than it needs for a full octet. This uses up 2 electrons, leaving 7 electrons for the remaining atoms.
Step 3:: Distribute the remaining electrons to achieve an octet for each atom
Place two electrons around the carbon atom to form a double bond with the oxygen atom. This uses up 2 electrons, leaving 5 electrons for the remaining atoms. Place two electrons around the oxygen atom to form a double bond with the carbon atom. This uses up 2 electrons, leaving 3 electrons for the remaining atoms. Place the remaining 3 electrons around the oxygen atom to form a negative charge, giving it a full octet.
Step 4:: Calculate the formal charge on each atom
The formal charge on an atom is calculated as: For the carbon atom: * Valence Electrons = 4 * Nonbonding Electrons = 0 * Bonding Electrons = 8 (4 single bonds) Therefore, the formal charge on the carbon atom is: For the oxygen atom in the single bond: * Valence Electrons = 6 * Nonbonding Electrons = 2 * Bonding Electrons = 4 (2 single bonds) Therefore, the formal charge on the oxygen atom in the single bond is: For the oxygen atom in the double bond: * Valence Electrons = 6 * Nonbonding Electrons = 4 * Bonding Electrons = 6 (3 double bonds) Therefore, the formal charge on the oxygen atom in the double bond is:
Step 5:: Draw the resonance structures
The acetate ion has two resonance structures, which are shown below: Resonance structure 1: * The carbon atom has a formal charge of 0. * The oxygen atom in the single bond has a formal charge of + 2. * The oxygen atom in the double bond has a formal charge of 0. Resonance structure 2: * The carbon atom has a formal charge of 0. * The oxygen atom in the single bond has a formal charge of 0. * The oxygen atom in the double bond has a formal charge of - 1.
Step 6:: Draw the Lewis structure for the acetate ion
The Lewis structure for the acetate ion is a hybrid of the two resonance structures, with the formal charges distributed evenly between the two oxygen atoms. The final Lewis structure is shown below: * The carbon atom has a formal charge of 0. * The oxygen atom in the single bond has a formal charge of + 1. * The oxygen atom in the double bond has a formal charge of - 1.
Final Answer
The Lewis structure for the acetate ion, CH^3CO^2 -, is shown above, including the formal charges on each atom. The acetate ion has two resonance structures, which are also shown above.
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