Formal Charge and Valence Electrons

The video tutorial explains how to calculate the formal charges for carbon monoxide (CO). It begins with the carbon atom, detailing the subtraction of unbonded and bonded electrons to find its formal charge. The same process is applied to the oxygen atom. The tutorial concludes by discussing the best Lewis structure for CO, emphasizing the importance of using all valence electrons and completing octets.

What is the first step in calculating the formal charge for an atom?

• Multiply the valence electrons by two

• Add the unbonded electrons

• Count the valence electrons

• Subtract the bonded electrons

How many valence electrons does carbon have in group 14?

• Eight

• Two

• Six

• Four

What is the formal charge on carbon in carbon monoxide?

• Negative two

• Positive one

• Negative one

• Zero

How many unbonded electrons are subtracted from oxygen's valence electrons?

• Four

• Three

• Two

• One

What is the formal charge on oxygen in carbon monoxide?

• Zero

• Negative two

• Positive one

• Negative one

Why can't the formal charges in CO be reduced to zero?

• The molecule is unstable

• The Lewis structure is incorrect

• The octets cannot be completed

• There are not enough valence electrons

What is the total number of valence electrons used in the CO molecule?

• Ten

• Eight

• Twelve

• Fourteen

What is the significance of completing the octets in the Lewis structure?

• It decreases the charge

• It increases the charge

• It makes the molecule reactive

• It stabilizes the molecule