Shapes of Molecules Mark as Favorite (22 Favorites)
LAB in Covalent Bonding, VSEPR Theory, Molecular Geometry, Resonance. Last updated June 05, 2017.
Summary
In this lab, students will investigate the VSEPR geometry of covalent compounds. They will draw Lewis structures, use molecular models, and determine the geometry of covalent compounds. There is a lot of repetition so students gain a lot of practice.
Grade Level
High school
Objectives
By the end of this lesson, students should be able to
- Recognize from a Lewis structure the molecular geometry of a compound.
- Understand VSEPR theory.
Chemistry Topics
This lesson supports students’ understanding of
- VSEPR theory
- Molecular geometry
- Resonance
- Covalent bonding
Time
Teacher Preparation: 10 minutes
Lesson: 1 class period and complete for homework
Materials
For each group:
- A set of molecular models
Safety
No safety considerations need to be observed for this investigation.
Teacher Notes
- It’s helpful to have samples of each geometry at the front of the class so students can familiarize themselves with how to assemble molecular models.
- Tetrahedral (four atoms around one central atom)
- Trigonal pyramidal (three atoms, one unbonded pair of electrons around one central atom)
- Trigonal planar (three atoms and no unbonded electrons around one central atom)
- Bent (two atoms and two pairs of unbonded electrons around one central atom)
- Linear (two atoms and no unbonded electrons around one central atom)
- This investigation only covers compounds that satisfy the octet rule. A possible extension could be to add more complicated molecules that extend past the octet rule.
For the Student
Lesson
Background
The valence shell electron pair repulsion (VSEPR) theory is how the geometry of a molecule is determined. It’s called “vesper” theory for short. The shapes that are possible are tetrahedral, trigonal planar, trigonal pyramidal, bent, and linear. To determine the shape of a molecule, you must look at the central atom. Unbonded electrons around the central are not accounted for in the geometry, however they are important because they determine the geometry. Unbonded electrons around atoms that are not the central atom have little effect on the geometry.
In this experiment, you will draw Lewis structures for a number of compounds and use them to determine how the molecular models need to be assembled. From the models, you will determine the geometry of the compounds. After completing a few examples, you should start to see how the two dimensional drawings really exist in three dimensions.
Procedure
Complete each column in order. Compare your model to the samples at the front of the room if you are confused about which geometry your model makes.
|
Molecule (write the chemical formula) |
Total valence e- |
Lewis structure (check the box if a resonance structure is possible) |
Lewis structure with proper geometry (use the models to help here) |
VSEPR geometry (the name of the shape) |
|---|---|---|---|---|
|
Water |
||||
|
Nitrogen |
||||
|
Carbonate |
||||
|
Sulfite |
||||
|
Carbon tetrachloride |
||||
|
Ammonium |
||||
|
Bromine |
||||
|
Carbon monoxide |
||||
|
Dinitrogen monoxide |
||||
|
Ozone |
||||
|
Nitrate |
||||
|
Nitrite |
||||
|
Bromate |
||||
|
Chlorite |
||||
|
Phosphate |
||||
|
Acetic Acid (try your best! Both carbons are in the middle.) |
Analysis
Without using models, determine the geometry of these compounds (you can draw Lewis structures to help you):
NF3 H2S OCl2
HCN F2 SO2
SO42- ClO3- SO3 (not sulfite!)
Conclusion
All of the compounds in this exercise are what kind of compound? Explain why this is important.