Valence Electrons and Carbonate Ion

The video tutorial explains how to draw the Lewis structure for the carbonate ion (CO3 2-). It begins by calculating the total number of valence electrons using the periodic table. The least electronegative atom, carbon, is placed at the center, surrounded by oxygen atoms. Electrons are distributed to form bonds, and octets are completed. A double bond is formed to satisfy the octet rule for carbon. The video also covers calculating formal charges and discusses resonance, where the double bond is averaged across the three carbon-oxygen bonds.

Which group in the periodic table does carbon belong to?

• Group 14

• Group 16

• Group 4

• Group 6

How many valence electrons does a single oxygen atom have?

• 2

• 8

• 6

• 4

What is the total number of valence electrons in the carbonate ion?

• 20

• 26

• 18

• 24

Which atom is placed at the center of the carbonate ion's Lewis structure?

• Nitrogen

• Oxygen

• Carbon

• Hydrogen

What type of bond is formed between carbon and oxygen in the initial structure?

• Single bond

• Double bond

• Triple bond

• Ionic bond

How is the octet of carbon completed in the carbonate ion?

• By forming a triple bond

• By removing electrons

• By adding more electrons

• By forming a double bond with one oxygen

What is the formal charge on the carbon atom in the carbonate ion?

• 0

• -1

• -2

• +1

What is the formal charge on the oxygen atoms with single bonds in the carbonate ion?

• -2

• -1

• 0

• +1

What does the resonance in the carbonate ion indicate?

• The double bond is averaged across all oxygen atoms

• The ion is unstable

• The double bond is fixed in one position

• There are no double bonds

How is the charge of the carbonate ion represented in its Lewis structure?

• With a minus sign

• With brackets and a 2- charge

• With a 2+ charge

• With a plus sign