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Lesson: VSEPR Theory

In this lesson, we will learn how to predict molecular geometries from the numbers of lone and bonding electron pairs and how to explain variations in bond angle.

Worksheet • 5 Questions

Q1:

Which of the following species has the smallest bond angle?

  • A O H 2
  • B N H 3
  • C B e H 2
  • D C H 4
  • E B H 3

Q2:

Why is the bond angle of water ( 1 0 4 . 5 ∘ ) less than the bond angle for methane ( 1 0 9 . 5 ∘ )?

  • AThe repulsion between a lone pair and a bonding pair is greater than the repulsion between two bonding pairs. Oxygen in water has two lone pairs and two bonding pairs, while the carbon in methane has four bonding pairs.
  • BMethane contains more bonds, so the bonds are forced further apart.
  • CThe O atom in water is surrounded by more electron pairs than the C atom in methane.
  • DThe bonding electron pairs in water repel each other more strongly than those in methane.
  • EThe O atom in water is sp2 hybridized.

Q3:

In which of the following species is the angle between the S O bonds the smallest?

  • A S O 3 2 –
  • B S O 2 3 2 –
  • C S O 2
  • D S O 4 2 –
  • E S O 3

Q4:

The A X E 3 structure notation best describes which molecule?

  • A N H 3
  • B H O 2
  • C X e F 4
  • D S F 4

Q5:

Which of the following species has the smallest bond angle?

  • A N O 2 –
  • B N O 2
  • C N O 2
  • D N 3 –
  • E N O 3 –
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