Hybridization and Molecular Geometry
Definition
Hybridization
Hybridization is the process of combining atomic orbitals (such as s and p orbitals) to create new hybrid orbitals that are better suited for bonding.
These hybrid orbitals have specific shapes and energy levels that enable atoms to form stable bonds and geometries.
Key Features of Hybridization:
- Number of Hybrid Orbitals: The number of hybrid orbitals equals the number of atomic orbitals combined.
- Energy and Shape: Hybrid orbitals have identical energy and specific geometries that minimize electron repulsion.
- Electron Domains and Hybridization: The type of hybridization corresponds to the number of electron domains (bonding and lone pairs) around the central atom.
Tip
Remember, hybridization depends on the number ofelectron domainsaround the central atom, not just the number of bonds.
Types of Hybridization: sp, sp², and sp³
sp Hybridization
- What Happens? One s orbital and one p orbital mix to form two sp hybrid orbitals. The remaining two p orbitals remain unhybridized.
- Geometry: Linear, with bond angles of 180°.
Example
- In ethyne (C₂H₂), each carbon has two electron domains (a triple bond and a single bond).
- This corresponds to sp hybridization, resulting in a linear geometry.
2. sp² Hybridization
- What Happens? One s orbital and two p orbitals mix to form three sp² hybrid orbitals. One p orbital remains unhybridized.
- Geometry: Trigonal planar, with bond angles of approximately 120°.
Example
- In ethene (C₂H₄), each carbon has three electron domains (two single bonds and one double bond).
- This corresponds to sp² hybridization, leading to a trigonal planar geometry.
Tip
In molecules with double bonds, one of the bonds is always a sigma bond, while the other is a pi bond formed by unhybridized p orbitals.
3. sp³ Hybridization
- What Happens? One s orbital and three p orbitals mix to form four sp³ hybrid orbitals.
- Geometry: Tetrahedral, with bond angles of approximately 109.5°.
Example
- In methane (CH₄), carbon has four electron domains (four single bonds).
- This corresponds to sp³ hybridization, resulting in a tetrahedral geometry.
Linking Hybridization to Molecular Geometry
The type of hybridization directly determines the molecular geometry. Here’s a summary:
| Hybridization | Nuumber of electron domains | Electron domain geometry | Molecular geometry |
|---|---|---|---|
| $sp$ | 2 | Linear | Linear |
| $sp^2$ | 3 | Trigonal planar | Trigonal planar |
| $sp^3$ | 4 | Tetrahedral | Tetrahedral |
Organic and Inorganic Examples of Hybridization
Organic Example: Ethyne (C₂H₂)
- Each carbon atom is sp hybridized, forming a linear molecule.
- The triple bond consists of one sigma bond (sp–sp overlap) and two pi bonds (p–p overlap).
Inorganic Example: Carbon Dioxide (CO₂)
- The central carbon atom is sp hybridized, with two double bonds to oxygen atoms.
- The molecule is linear, with a bond angle of 180°.
Predicting Hybridization and Geometry
From Hybridization to Geometry
- Determine the type of hybridization based on the number of electron domains.
- Use the hybridization to predict the molecular geometry.
From Geometry to Hybridization
- Determine the molecular geometry using VSEPR theory.
- Use the geometry to deduce the hybridization of the central atom.
Example
To predict the hybridization and geometry of ammonia (NH₃):
- Step 1: Count the electron domains around nitrogen (three bonds and one lone pair = 4 domains).
- Step 2: Four domains correspond to sp³ hybridization.
- Step 3: The molecular geometry is trigonal pyramidal.
Self review
Why does methane have a bond angle of 109.5°, while ethene has a bond angle of 120°?
