Understanding the Lewis Structure of SO2

The video tutorial explains how to draw the Lewis structure of sulfur dioxide (SO2) by counting valence electrons and arranging them to minimize formal charge. It covers the concept of expanded octets, resonance forms, and the importance of minimizing formal charge for stability. The tutorial also discusses the molecular geometry, hybridization, and bond angles of SO2, concluding with an explanation of its polarity due to dipole moments and vector components.

How many valence electrons are present in a sulfur dioxide (SO2) molecule?

• 22

• 18

• 20

• 16

What is the highest multiple of eight that is less than the total valence electrons in SO2?

• 32

• 24

• 16

• 8

What is the significance of the highest multiple of eight in drawing the Lewis structure?

• It helps in identifying lone pairs.

• It helps in minimizing formal charge.

• It determines the number of bonds.

• It indicates the number of resonance forms.

Which element can have an expanded octet?

• Carbon

• Sulfur

• Oxygen

• Nitrogen

What is the formal charge on sulfur in the most stable Lewis structure of SO2?

• +2

• +1

• 0

• -1

How many bonds does sulfur form in the most stable Lewis structure of SO2?

• 5

• 4

• 3

• 2

What is the molecular geometry of SO2?

• Tetrahedral

• Trigonal planar

• Bent

• Linear

What is the hybridization of the central sulfur atom in SO2?

• sp2

• sp3d

• sp3

• sp

What is the approximate bond angle in the SO2 molecule?

• 120°

• 104.5°

• 90°

• 180°

Why is the SO2 molecule considered polar?

• There is a separation of charge.

• It has no lone pairs.

• The dipole moments cancel out.

• It has a symmetrical shape.