Formal Charges and Nitrogen in NO3-

The video tutorial explains how to calculate the formal charges for the nitrate ion (NO3 minus) by examining each atom's valence electrons, non-bonding electrons, and bonding electrons. The tutorial covers the formal charge calculations for oxygen atoms, including those with single and double bonds, and the nitrogen atom. It emphasizes the importance of formal charges being as close to zero as possible and highlights the significance of electronegativity in determining charge distribution. The overall formal charge for NO3 minus is confirmed to be negative one.

What is the primary focus when calculating formal charges for NO3- in this tutorial?

• Determining molecular geometry

• Calculating formal charges without resonance

• Considering resonance structures

• Identifying hybridization states

How many non-bonding electrons are present on the left oxygen atom in NO3-?

• Six

• Four

• Two

• Eight

What is the formal charge of the oxygen atom with a double bond in NO3-?

• +2

• -1

• 0

• +1

How many valence electrons does nitrogen have in NO3-?

• Three

• Eight

• Five

• Seven

What is the formal charge of the nitrogen atom in NO3-?

• +2

• -1

• 0

• +1

What is the overall net formal charge of NO3-?

• -2

• -1

• 0

• +1

Why is it logical for the negative formal charges to be on the oxygen atoms in NO3-?

• Oxygen is less electronegative

• Oxygen has more protons

• Oxygen is more electronegative

• Oxygen has fewer electrons

What rule cannot be violated by nitrogen in NO3-?

• Triple bond rule

• Resonance rule

• Duet rule

• Octet rule

What is the significance of having formal charges close to zero?

• It suggests a high boiling point

• It means the molecule is polar

• It shows a high reactivity

• It indicates a stable structure

Who is the presenter of this tutorial?

• Dr. A

• Dr. B

• Dr. D

• Dr. C