Formal Charges and Valence Electrons in HNO2

The video tutorial explains how to calculate the formal charges for each element in HNO2 using its Lewis structure. It covers the formal charge calculations for two oxygen atoms, nitrogen, and hydrogen, demonstrating that all formal charges are zero, indicating the most stable Lewis structure for nitrous acid.

What is the primary method used to determine formal charges in HNO2?

• Using atomic mass

• Using empirical formulas

• Using the Lewis structure

• Using molecular geometry

How many valence electrons does the first oxygen atom in HNO2 have?

• Five

• Seven

• Four

• Six

What is the formal charge of the first oxygen atom in HNO2?

• +2

• 0

• -1

• +1

How many unbonded valence electrons does the nitrogen atom in HNO2 have?

• Four

• Three

• Two

• One

What is the formal charge of the nitrogen atom in HNO2?

• 0

• +2

• -1

• +1

How does the bonding of the second oxygen atom differ from the first in HNO2?

• It forms a double bond

• It has no bonds

• It is bonded to hydrogen

• It forms a triple bond

What is the formal charge of the second oxygen atom bonded to hydrogen in HNO2?

• +1

• -1

• 0

• +2

How many valence electrons does hydrogen have in HNO2?

• One

• Two

• Three

• Four

What is the formal charge of the hydrogen atom in HNO2?

• +1

• 0

• -1

• +2

Why is the Lewis structure with all zero formal charges considered the best for HNO2?

• It maximizes energy

• It is the simplest

• It is the most complex

• It minimizes energy