Understanding SbCl5 Geometry and Valence Electrons

The video tutorial explains how to draw the Lewis structure for antimony pentachloride (SbCl5). It begins by counting the valence electrons, placing antimony in the center, and arranging five chlorine atoms around it. The tutorial highlights that antimony can have an expanded octet. It then describes the molecular geometry of SbCl5 as trigonal bipyramidal, using AXE notation to confirm the geometry. The video concludes with a summary of the Lewis structure and molecular geometry.

How many valence electrons are there in total for SbCl5?

• 40

• 45

• 35

• 30

Which element is placed at the center of the SbCl5 Lewis structure?

• Antimony

• Hydrogen

• Chlorine

• Oxygen

Why can antimony have more than eight valence electrons in its Lewis structure?

• It forms ionic bonds

• It is highly electronegative

• It is a metal

• It can have an expanded octet

What is the total number of valence electrons used in the SbCl5 Lewis structure?

• 30

• 35

• 40

• 45

What is the molecular geometry of SbCl5 when all chlorine atoms are added?

• Linear

• Trigonal Planar

• Trigonal Bipyramidal

• Tetrahedral

What are the bond angles along the equator in the trigonal bipyramidal geometry of SbCl5?

• 180°

• 120°

• 90°

• 60°

What is the electron geometry of SbCl5?

• Trigonal Bipyramidal

• Trigonal Planar

• Linear

• Tetrahedral

Using AXE notation, what does the 'X' represent in the geometry of SbCl5?

• Total valence electrons

• Number of lone pairs

• Number of atoms attached

• Central atom

How many chlorine atoms are attached to the central antimony atom in SbCl5?

• 6

• 5

• 4

• 3

What is the correct AXE notation for SbCl5?

• AX3

• AX4

• AX5

• AX6