Valence Electrons and Iodine Compounds

The video tutorial explains how to draw the Lewis structure for IBr4-. It begins by counting the total valence electrons, considering iodine and bromine's group numbers and the negative charge. The iodine atom is placed at the center with bromine atoms around it, forming bonds. The octets of bromine are completed, and the remaining electrons are placed on iodine, which can have an expanded octet. The final structure shows iodine with 12 valence electrons, demonstrating the concept of expanded octets.

How many total valence electrons are there in the IBr4- ion?

• 32

• 34

• 36

• 38

Which element is placed at the center of the IBr4- Lewis structure?

• Fluorine

• Chlorine

• Iodine

• Bromine

How many bromine atoms are bonded to the central iodine in IBr4-?

• 2

• 3

• 5

• 4

What is the total number of valence electrons used after completing the octets for bromine atoms?

• 30

• 34

• 28

• 32

How many additional electrons need to be placed after completing the bromine octets?

• 2

• 5

• 3

• 4

What is the maximum number of valence electrons iodine can have in an expanded octet?

• 14

• 10

• 8

• 12

In the final Lewis structure of IBr4-, how many valence electrons does the central iodine have?

• 14

• 12

• 10

• 8

Why is it acceptable for iodine to have more than 8 valence electrons in IBr4-?

• Iodine is a metal.

• Iodine can form double bonds.

• Iodine is a noble gas.

• Iodine can have an expanded octet.

What is the charge on the IBr4- ion?

• -1

• 0

• +1

• -2