Formal Charge and Lewis Structures

The video tutorial explains how to draw the Lewis structure for the iodite ion (IO2-). It begins by counting the valence electrons and placing iodine in the center with oxygen atoms on either side. The initial structure is drawn, but it is not optimal due to formal charges. The video then demonstrates how to adjust the structure by forming a double bond to achieve the best configuration with minimized formal charges, resulting in a more stable ion representation.

What is the total number of valence electrons in the iodite ion (IO2-)?

• 22

• 20

• 18

• 24

Which element is placed at the center of the Lewis structure for IO2-?

• Oxygen

• Iodine

• Hydrogen

• Nitrogen

How many valence electrons are initially used to form chemical bonds in the IO2- structure?

• 16

• 4

• 8

• 12

What is the formal charge on the iodine atom in the initial Lewis structure of IO2-?

• -1

• 0

• +2

• +1

Why is the initial Lewis structure of IO2- not considered the best?

• It has too many electrons.

• Iodine is not in the center.

• It lacks a double bond.

• The formal charges are not minimized.

What change is made to the IO2- structure to achieve the best configuration?

• Changing the central atom

• Adding more electrons

• Forming a double bond

• Removing an oxygen atom

After optimization, what is the formal charge on the oxygen atom with a double bond in IO2-?

• +2

• +1

• 0

• -1

What is the overall charge of the iodite ion (IO2-)?

• -2

• -1

• +1

• 0

Which of the following best describes the final Lewis structure of IO2-?

• No bonds with iodine

• Two double bonds with iodine

• One double bond and one single bond with iodine

• Two single bonds with iodine

What is the purpose of placing brackets around the Lewis structure of IO2-?

• To denote resonance

• To indicate it is a molecule

• To show it is an ion

• To highlight the central atom