Valence Electrons and Molecular Structure

The video tutorial explains the Lewis structure of IF3, detailing the valence electrons of iodine and fluorine. Iodine, being the least electronegative, is placed at the center with fluorines surrounding it. Initial bonds are formed, and octets are completed for fluorines. Iodine, in period 5, can hold more than eight electrons, allowing for an expanded octet. The structure is finalized with all formal charges at zero, ensuring all electrons are used correctly.

How many valence electrons does iodine have in the IF3 molecule?

• 5

• 8

• 6

• 7

What is the total number of valence electrons in the IF3 molecule?

• 42

• 35

• 28

• 21

Why is iodine placed at the center of the IF3 molecule?

• It has the lowest electronegativity.

• It has the most valence electrons.

• It has the highest electronegativity.

• It is the smallest atom.

How many valence electrons are used to form bonds between iodine and fluorine in IF3?

• 8

• 6

• 4

• 2

What is the significance of iodine being in period 5 for the IF3 structure?

• It can hold more than eight valence electrons.

• It has no significance.

• It can only hold eight valence electrons.

• It cannot form bonds with fluorine.

What is the formal charge on each atom in the IF3 molecule?

• Iodine has a formal charge of +1, and fluorines have 0.

• All atoms have a formal charge of 0.

• All atoms have a formal charge of -1.

• All atoms have a formal charge of +1.