Valence Electrons and Formal Charge

The video tutorial explains the process of drawing the Lewis structure for the IF4- ion. It begins by counting the total valence electrons, placing Iodine at the center, and arranging Fluorine atoms around it. Bonds are formed, and the octets for Fluorine are filled. The remaining electrons are placed on Iodine, which can hold more than eight electrons. Formal charges are checked to ensure the structure is correct, with Fluorine having a charge of zero and Iodine having a charge of negative one. Finally, brackets are added to indicate the ion's negative charge.

What is the total number of valence electrons in the IF4- ion?

• 32

• 34

• 36

• 38

Which element is placed at the center of the IF4- Lewis structure?

• Nitrogen

• Oxygen

• Iodine

• Fluorine

How many valence electrons are used to form bonds between Iodine and Fluorines in IF4-?

• 12

• 14

• 10

• 8

What is the formal charge on each Fluorine atom in the IF4- structure?

• -2

• -1

• 0

• +1

Why is it acceptable for Iodine to have more than eight valence electrons in IF4-?

• Iodine is highly electronegative

• Iodine is a metal

• Iodine is in period 5

• Iodine is in period 3

What is the formal charge on the Iodine atom in the IF4- structure?

• +1

• 0

• -1

• -2

What is the purpose of adding brackets around the IF4- Lewis structure?

• To indicate it is a molecule

• To emphasize the octet rule

• To highlight the central atom

• To show it is an ion with a negative charge