ICl3 Molecular Structure and Bonding

The video tutorial explains the Lewis structure of ICl3. It begins with calculating the total valence electrons for Iodine and Chlorine, followed by placing Iodine at the center due to its lower electronegativity. Chlorines are placed around Iodine, and electrons are distributed to form chemical bonds. The tutorial highlights that Iodine can violate the octet rule due to its position in period 4, allowing it to have more than eight valence electrons. The structure is finalized with all valence electrons used, ensuring Chlorines have octets and Iodine has an expanded octet.

How many total valence electrons are present in ICl3?

• 28

• 14

• 35

• 21

Which atom is placed at the center of the ICl3 molecule?

• Hydrogen

• Oxygen

• Iodine

• Chlorine

How many electrons are used to form chemical bonds between the atoms in ICl3?

• 10

• 8

• 4

• 6

Why is it acceptable for iodine in ICl3 to have more than eight valence electrons?

• Iodine is in period 3

• Iodine is in period 4

• Iodine is in period 5

• Iodine is in period 6

What is the final electron configuration around the chlorine atoms in ICl3?

• Each chlorine has 7 electrons

• Each chlorine has 9 electrons

• Each chlorine has 6 electrons

• Each chlorine has 8 electrons