Molecular Shapes and Bond Angles

The video tutorial covers predicting the shapes and bond angles of simple Lewis structures using VSEPR theory. It starts with methane, explaining its tetrahedral shape and bond angle. The tutorial then explores ammonia and water, highlighting the effects of lone pairs on bond angles. It discusses structures with three charge centers, like boron trihydride and sulfur dioxide, and two charge centers, such as carbon dioxide. The video concludes with a creative visualization of molecular shapes.

What is the shape of methane (CH4) according to VSEPR theory?

• Bent

• Trigonal Planar

• Linear

• Tetrahedral

How does the presence of a lone pair affect the bond angle in ammonia (NH3)?

• Makes the molecule linear

• Has no effect

• Decreases the bond angle

• Increases the bond angle

What is the bond angle in a water molecule (H2O)?

• 105°

• 107°

• 120°

• 109.5°

Which of the following molecules has a bent shape due to lone pairs?

• Methane (CH4)

• Boron trihydride (BH3)

• Ammonia (NH3)

• Water (H2O)

Which molecule has a trigonal planar shape?

• Water (H2O)

• Boron trihydride (BH3)

• Ammonia (NH3)

• Methane (CH4)

What is the bond angle in sulfur dioxide (SO2)?

• 180°

• 120°

• 109.5°

• Less than 120°

Which molecule is stable with only six electrons around the central atom?

• Ammonia (NH3)

• Methane (CH4)

• Boron trihydride (BH3)

• Water (H2O)

What is the shape of carbon dioxide (CO2)?

• Tetrahedral

• Bent

• Trigonal Planar

• Linear

What is the bond angle in a linear molecule like carbon dioxide (CO2)?

• 120°

• 109.5°

• 180°

• 90°

What is the effect of lone pairs on the bond angles in a molecule?

• They decrease the bond angles

• They make the molecule linear

• They increase the bond angles

• They have no effect