Formal Charge and Molecular Structure

The video tutorial explains how to calculate the formal charge for each element in chloric acid (HCl3). It begins with an introduction to the concept of formal charge and its importance in determining the best Lewis structure. The tutorial then calculates the formal charge for hydrogen, chlorine, and oxygen atoms in HCl3, demonstrating that all atoms have a formal charge of zero. This indicates that the given Lewis structure is the most favorable for chloric acid.

What is the purpose of calculating the formal charge in a molecule?

• To identify the color of the compound

• To calculate the boiling point

• To find the most stable Lewis structure

• To determine the molecular weight

Why does hydrogen in HCl3 have a formal charge of zero?

• It is in group 17

• It forms a single bond

• It forms a double bond

• It has no electrons

Which group does chlorine belong to on the periodic table?

• Group 18

• Group 16

• Group 15

• Group 17

What is the significance of chlorine having an expanded octet?

• It is less reactive

• It cannot form any bonds

• It has fewer electrons

• It can form more than four bonds

How many unbonded electrons does each double-bonded oxygen have?

• Six

• Two

• Four

• Eight

What is the formal charge of each double-bonded oxygen in HCl3?

• +2

• +1

• -1

• 0

How many unbonded electrons are present in the single-bonded oxygen?

• Eight

• Four

• Two

• Six

What is the formal charge of the single-bonded oxygen in HCl3?

• +1

• -1

• 0

• +2

What does a formal charge of zero on all atoms in HCl3 indicate?

• The molecule is unstable

• The Lewis structure is incorrect

• The molecule is highly reactive

• The Lewis structure is most favorable

What is the chemical name for HCl3?

• Perchloric acid

• Chloric acid

• Hypochlorous acid

• Hydrochloric acid