ICl4- Structure and Valence Electrons

The video tutorial explains how to draw the Lewis structure for ICl4-. It begins by calculating the total valence electrons, placing iodine at the center, and surrounding it with chlorine atoms. The tutorial then forms bonds and completes the octets for chlorine, using up the valence electrons. It discusses iodine's ability to hold more than eight electrons and places the remaining electrons on iodine. The video checks formal charges, ensuring iodine has a charge of negative one and chlorines have zero. Finally, it emphasizes the importance of brackets to indicate the ion's negative charge.

How many valence electrons does iodine have in the ICl4- structure?

• 7

• 6

• 8

• 5

What is the total number of valence electrons used in the ICl4- structure?

• 32

• 34

• 36

• 38

Which atom is placed at the center of the ICl4- structure?

• Chlorine

• Iodine

• Hydrogen

• Oxygen

How many valence electrons are initially used to form bonds between iodine and chlorine?

• 4

• 8

• 6

• 10

Why can iodine hold more than eight valence electrons in the ICl4- structure?

• It is in period 3 of the periodic table.

• It is a noble gas.

• It has a high electronegativity.

• It is in period 5 of the periodic table.

What is the formal charge on the iodine atom in the ICl4- structure?

• +1

• -2

• -1

• 0

Why are brackets used around the ICl4- Lewis structure?

• To indicate it is a molecule.

• To show it is an ion with a negative charge.

• To separate it from other structures.

• To highlight the central atom.