IBrCl- Molecular Geometry and Structure

The video tutorial explains how to draw the Lewis structure for IBrCl⁻. It begins by counting the valence electrons of the halogens involved, noting that they belong to group 17. The tutorial then places electrons to form chemical bonds and complete the octet for each atom. It discusses the concept of formal charges, highlighting that bromine can have an expanded octet. The video concludes with an explanation of the molecular geometry using AXE notation, resulting in a linear shape with specific bond angles.

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

• 22

• 23

• 20

• 21

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

• Chlorine

• Bromine

• Iodine

• Fluorine

What is the initial step in forming the chemical bonds in the IBrCl- structure?

• Removing electrons from bromine

• Adding extra electrons to chlorine

• Placing a pair of electrons between each atom

• Placing lone pairs on iodine

How many electrons are left after completing the octet for iodine and chlorine?

• 6

• 4

• 0

• 2

What is the formal charge on bromine in the IBrCl- structure?

• 0

• -1

• -2

• +1

Why is bromine placed in the center of the IBrCl- structure?

• It is the most electronegative

• It is the least electronegative

• It has the highest atomic number

• It can have an expanded octet

What notation is used to determine the molecular geometry of IBrCl-?

• Molecular Orbital

• VSEPR

• AXE

• Lewis

What is the molecular geometry of the IBrCl- ion?

• Bent

• Trigonal Planar

• Linear

• Tetrahedral

How many lone pairs are present on the central atom in the IBrCl- structure?

• 1

• 2

• 3

• 4

What are the bond angles around the equatorial plane in the IBrCl- structure?

• 180°

• 120°

• 90°

• 109.5°