Lewis Structures and Formal Charges

The video tutorial explains the process of drawing the Lewis structure for the iodate ion (IO3-). It begins by identifying the total number of valence electrons and placing iodine at the center with oxygen atoms around it. The tutorial covers forming chemical bonds, satisfying octets, and understanding iodine's ability to have an expanded octet. It then calculates formal charges for iodine and oxygen, and adjusts them by forming double bonds. The final structure is confirmed with correct formal charges and brackets to indicate the negative ion.

What is the total number of valence electrons in the IO3- ion?

• 28

• 30

• 26

• 24

Which element is placed at the center of the IO3- Lewis structure?

• Hydrogen

• Iodine

• Nitrogen

• Oxygen

How many valence electrons are used to form chemical bonds initially in the IO3- structure?

• 8

• 2

• 4

• 6

Why can iodine have more than 8 valence electrons in its Lewis structure?

• It is in period 2 of the periodic table

• It is below period 2 on the periodic table

• It can form multiple bonds

• It is highly electronegative

What is the formal charge of iodine before adjusting the bonds?

• -1

• 0

• +1

• +2

What is the formal charge of each oxygen atom before any double bonds are formed?

• 0

• -1

• +1

• -2

How can the formal charge on iodine be reduced to zero?

• By adding more electrons

• By forming double bonds with oxygen

• By forming a triple bond

• By removing electrons

What is the formal charge of the entire IO3- structure after adjustments?

• 0

• -1

• -2

• +1

Why is it important to put brackets and a negative sign around the IO3- Lewis structure?

• To indicate it is a positive ion

• To show it is a neutral molecule

• To indicate it is a negative ion

• To highlight the central atom

What makes the final Lewis structure of IO3- more likely?

• The formal charges are close to zero

• The structure uses fewer electrons

• The structure has more bonds

• The structure is symmetrical