Chlorine and Iodine Compounds

The video tutorial explains how to write the Lewis structure for chlorine tri-iodide (ClI3). It begins by clarifying the symbols for chlorine and iodine, then calculates the total valence electrons. The tutorial places chlorine in the center with iodines around it, forms chemical bonds, and completes the octets. It discusses the expanded octet for chlorine and calculates formal charges, concluding that the structure is optimal with zero formal charges.

What is the total number of valence electrons in ClI3?

• 14

• 21

• 35

• 28

Which atom is placed at the center in the Lewis structure of ClI3?

• Oxygen

• Iodine

• Chlorine

• Hydrogen

How many iodine atoms are bonded to the central chlorine atom in ClI3?

• Three

• Two

• Four

• One

What is the purpose of placing a pair of electrons between elements in ClI3?

• To change the element

• To reduce atomic size

• To increase electronegativity

• To form chemical bonds

How many valence electrons are used after completing the octets for iodine atoms in ClI3?

• 32

• 20

• 28

• 24

What allows chlorine to have more than 8 electrons in its valence shell?

• Its position in the periodic table

• Its small size

• Its ability to have an expanded octet

• Its high electronegativity

How many total valence electrons are used in the final Lewis structure of ClI3?

• 24

• 26

• 28

• 30

What is the formal charge on each atom in the best Lewis structure of ClI3?

• +2

• -1

• +1

• 0

Why is the Lewis structure with zero formal charges considered favorable for ClI3?

• It increases reactivity

• It decreases stability

• It maximizes energy

• It minimizes energy