Molecular Geometry and Bond Angles

This video tutorial continues from a previous introduction to VSEPR theory, focusing on various molecular geometries. It covers the trigonal bipyramidal structure using phosphorus pentachloride as an example, explaining bond angles and electron arrangements. The seesaw geometry is illustrated with sulfur tetrafluoride, while the T-shaped structure is demonstrated with iodine trifluoride, including a method for determining Lewis structures. The octahedral geometry is explained with sulfur hexafluoride, and the differences between square pyramidal and square planar structures are discussed, using iodine pentafluoride and xenon tetrafluoride as examples.

What is the bond angle between the axial atoms in a trigonal bipyramidal structure?

• 60 degrees

• 180 degrees

• 120 degrees

• 90 degrees

Which molecule is an example of a trigonal bipyramidal structure?

• IF3

• PCl5

• XeF4

• SF4

In a seesaw molecular geometry, how many lone pairs are present on the central atom?

• Two

• None

• One

• Three

Which molecule is an example of a seesaw molecular geometry?

• XeF4

• SF4

• PCl5

• IF3

How many lone pairs are on the central atom in a T-shaped molecular geometry?

• Two

• One

• Three

• None

Which molecule is an example of a T-shaped molecular geometry?

• SF4

• PCl5

• XeF4

• IF3

What is the bond angle in an octahedral molecular geometry?

• 90 degrees

• 60 degrees

• 120 degrees

• 180 degrees

Which molecule is an example of an octahedral molecular geometry?

• XeF4

• SF6

• IF3

• PCl5

In a square pyramidal structure, how many atoms are attached to the central atom?

• Three

• Six

• Five

• Four

Which molecule is an example of a square planar molecular geometry?

• SF4

• PCl5

• IF3

• XeF4