Carbon and Acetate Ion Properties

The video tutorial explains how to calculate the formal charges for each element in the acetate ion (CH3COO-). It uses Lewis structures to demonstrate the process, starting with hydrogen, then moving to the two carbon atoms, and finally the two oxygen atoms. The tutorial highlights that the overall charge of the acetate ion is -1, with the negative charge residing on the single-bonded oxygen. The video concludes with a summary of the formal charges for each element.

What is the purpose of using a Lewis structure when determining formal charges?

• To represent valence electrons and bonds

• To identify the number of protons

• To calculate the molecular weight

• To visualize the molecular geometry

How many valence electrons does hydrogen have in the acetate ion?

• Two

• Four

• One

• Three

What is the formal charge of each hydrogen atom in the acetate ion?

• +2

• 0

• -1

• +1

Which group on the periodic table does carbon belong to?

• Group 18

• Group 14

• Group 16

• Group 1

What is the formal charge of the first carbon atom in the acetate ion?

• -1

• 0

• +1

• +2

How many valence electrons are involved in bonds for the second carbon atom?

• Two

• Eight

• Six

• Four

What is the formal charge of the oxygen atom with a double bond?

• +2

• 0

• +1

• -1

How many unbonded electrons does the single-bonded oxygen have?

• Two

• Four

• Six

• Eight

What is the formal charge of the oxygen atom with a single bond?

• -1

• 0

• +1

• +2

Why is it not surprising that the single-bonded oxygen has a negative charge?

• Because it is bonded to hydrogen

• Because it is more electronegative

• Because the overall acetate ion has a negative charge

• Because it has more protons