QQuestionAnatomy and Physiology
QuestionAnatomy and Physiology
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!
6 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
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.
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.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students