Valence Electrons in IBr2- Structure

The video tutorial explains how to draw the Lewis structure for the IBr2- ion. It begins by calculating the total number of valence electrons, considering iodine and bromine atoms, and the extra electron due to the negative charge. Iodine, being the least electronegative, is placed at the center, with bromine atoms on the outside. The tutorial demonstrates forming chemical bonds and distributing the remaining valence electrons to satisfy the octet rule for bromine and the expanded octet for iodine. Finally, it shows how to indicate the ion with brackets and a negative charge.

How many total valence electrons are present in the IBr2- ion?

• 20

• 21

• 22

• 23

Which element is placed at the center of the IBr2- Lewis structure?

• Fluorine

• Chlorine

• Iodine

• Bromine

How many valence electrons are used to form chemical bonds between the atoms in IBr2-?

• 4

• 6

• 2

• 8

What is the total number of valence electrons around each bromine atom in the IBr2- structure?

• 9

• 8

• 7

• 6

Why can iodine hold more than eight valence electrons in the IBr2- structure?

• It is in period 6

• It is in period 3

• It is in period 4

• It is in period 5

What notation is used to indicate that IBr2- is an ion?

• Parentheses

• Brackets

• Curly braces

• Angle brackets