What are the 4 VSEPR shapes?
What are the 4 VSEPR shapes?
Now, we will discuss each shape in detail:
- Linear Shape of Molecule:
- Trigonal Planar Shape of Molecule:
- Tetrahedral Shape of Molecule:
- Trigonal Bipyramid Shape of Molecule:
- How can the VSEPR Theory be used to Predict the Shapes of Molecules?
What are the 5 possible VSEPR shapes?
VSEPR Chart Downloads
| Molecular Shape Image Downloads | |
|---|---|
| Linear (CN 4) | Bisphenoidal (seesaw) |
| Linear (CN 5) | T-shaped |
| Trigonal planar | Octahedral |
| Angled (CN 3) | Square pyramidal |
What are the VSEPR types?
The VSEPR theory describes five main shapes of simple molecules: linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral.
How do you determine a VSEPR shape?
- VSEPR Rules:
- Identify the central atom.
- Count its valence electrons.
- Add one electron for each bonding atom.
- Add or subtract electrons for charge (see Top Tip)
- Divide the total of these by 2 to find the total.
- number of electron pairs.
- Use this number to predict the shape.
What are the rules of VSEPR?
VSEPR Rules. Draw the Lewis structure for the molecule or ion. Count the total number of regions of high electron density (bonding and unshared electron pairs) around the central atom. Double and triple bonds count as ONE REGION OF HIGH ELECTRON DENSITY.
Is seesaw planar?
The name “seesaw” comes from the observation that it looks like a playground seesaw. Most commonly, four bonds to a central atom result in tetrahedral or, less commonly, square planar geometry….
| Seesaw molecular geometry | |
|---|---|
| μ (Polarity) | >0 |
What are the rules of VSEPR theory?
How does VSEPR affect the shape of molecules?
Using the VSEPR theory, the electron bond pairs and lone pairs on the center atom will help us predict the shape of a molecule. The shape of a molecule is determined by the location of the nuclei and its electrons. The electrons and the nuclei settle into positions that minimize repulsion and maximize attraction.
