Formal Charge and Valence Electrons in CO2

The video tutorial explains how to determine the formal charges for each atom in CO2 using a Lewis structure. It begins by calculating the formal charge for carbon, which is found to be zero, and then proceeds to calculate the formal charge for oxygen, which is also zero. The tutorial concludes that the best Lewis structure for CO2 is one where all atoms have a formal charge of zero, aligning with the molecule's neutral charge.

What is the first step in determining the formal charges for each atom in CO2?

• Calculate the molecular weight.

• Determine the oxidation states.

• Draw a Lewis structure.

• Identify the molecular geometry.

How many valence electrons does carbon have in CO2?

• Two

• Four

• Six

• Eight

What is the formal charge on carbon in CO2?

• +2

• +1

• 0

• -1

In which group is oxygen found on the periodic table?

• Group 4

• Group 10

• Group 6

• Group 8

How many non-bonding valence electrons does oxygen have in CO2?

• Four

• Two

• Eight

• Six

What is the formal charge on each oxygen atom in CO2?

• +1

• -1

• 0

• +2

Why do the formal charges in CO2 add up to zero?

• Because CO2 has a positive charge.

• Because CO2 has a negative charge.

• Because CO2 is an ion.

• Because CO2 is a neutral molecule.

What does a formal charge of zero on all atoms in CO2 indicate?

• The molecule is an ion.

• The Lewis structure is incorrect.

• The Lewis structure is optimal.

• The molecule is unstable.