Formal Charges in ClO3-

The video tutorial explains the Lewis structure of the chlorate ion (ClO3-) and its exception to the octet rule. It demonstrates how to calculate formal charges for each atom in the ion, focusing on oxygen and chlorine. The tutorial concludes by confirming the overall formal charge of the ion, aligning with its negative charge.

What is the main exception to the octet rule observed in the ClO3- ion?

• Oxygen has less than eight valence electrons.

• Chlorine has more than eight valence electrons.

• Oxygen has more than eight valence electrons.

• Chlorine has exactly eight valence electrons.

How many non-bonding valence electrons are present on the first oxygen atom in ClO3-?

• Eight

• Two

• Four

• Six

What is the formal charge of the first oxygen atom in ClO3-?

• +1

• -1

• -2

• 0

What is the formal charge of the second oxygen atom in ClO3-?

• -1

• 0

• +1

• -2

Why is it unnecessary to recalculate the formal charge for the third oxygen atom?

• It is not bonded to chlorine.

• It has the same orientation as the second oxygen.

• It has no valence electrons.

• It has a different orientation.

How many non-bonding valence electrons does the chlorine atom have in ClO3-?

• Eight

• Four

• Six

• Two

What is the formal charge of the chlorine atom in ClO3-?

• -1

• -2

• 0

• +1

What is the overall formal charge of the ClO3- ion?

• -1

• 0

• -2

• +1

Why does the overall formal charge of ClO3- make sense?

• Because the ion is neutral.

• Because the ion has a negative charge.

• Because the ion has no charge.

• Because the ion has a positive charge.

What is the significance of calculating formal charges in a Lewis structure?

• To determine the molecular geometry.

• To find the most stable structure.

• To identify the type of bonds present.

• To calculate the molecular weight.