Valence Shell Electron Pair Repulstion Theory

Multiple Choice

Which molecular geometry has a bond angle of 180° and no nonbonded electron pairs on the central atom?

• Linear

• Trigonal planar

• Tetrahedral

• Bent

Multiple Select

Select all the molecular geometries that have only bonded pairs and no nonbonded pairs on the central atom.

• Linear

• Trigonal planar

• Tetrahedral

• Bent

Multiple Choice

Which of the following molecules has a bond angle closest to 109.5°?

• CH4

• NH3

• H2O

• CO2

Multiple Choice

What is the bond angle between equatorial atoms in a trigonal bipyramidal geometry?

• 90°

• 120°

• 101.6°

• 154.5°

Multiple Select

Which of the following molecular geometries have a flat square arrangement of equatorial atoms?

• Octahedral

• Square planar

• Square pyramid

• Trigonal bipyramidal

Multiple Choice

Which molecular geometry has two lone pairs on the central atom and a bond angle of 90°?

• Square planar

• Octahedral

• Square pyramid

• Trigonal bipyramidal

Open Ended

Explain how the presence of lone pairs affects the bond angles in molecular geometries. Use examples from the images to support your answer.

Multiple Choice

Which molecule shown has a T-shaped molecular geometry?

• SF3

• H2O

• CCl4

• Br2

Open Ended

Compare the electron pair geometry and molecular geometry of H2O and SF3.

Multiple Select

Which of the following molecules are linear in shape?

• Br2

• HCl

• SF3

• H2O

Multiple Choice

Which of the following molecules has a bent molecular geometry?

• HCl

• H2O

• Br2

• CCl4

Multiple Select

Select all molecules from the images that have a linear molecular geometry.

• O2

• HF

• SCl2

• NF3

Multiple Choice

Which of the following molecules has a trigonal pyramidal molecular geometry?

• NH3

• O2

• HF

• SeH2

Multiple Choice

Lewis structures show a 2D picture of a molecule, but what is a major limitation of using Lewis structures to represent molecules?

• They do not show the 3D shape of molecules.

• They always show the correct number of electrons.

• They are only used for ionic compounds.

• They can represent all molecules accurately.