- University of Massachusetts, Amherst
- Chemistry 102
Last Modified: 2011-06-25
- Lone e- pairs take up more space than bonding e- pairs
- Treat multiple bonds as single e- pair
- Lone e- pairs prefer equatorial postion
- No distinction between equatorial and axial positions
- Aka VSEPR
- Model expressing basic idea that bonding e- pairs and lone e- pairs in valence shell of atom repel each other and seek out to be as far as possible from one another in molecule
- Distance between nuclei of two bonded atoms
- Smaller atom = shorter bond length
- A bond order goes up, bond length goes down
- Energy (enthalpy) required to break bond
- ΔHr = energy required
- Shorter bonds = higher energy
- Bigger atoms = lower energy
- Predicts energy given off during given reaction
- ΔHrxn = Σ Δhbroken - Σ Δhformed
- Polar bond? (No = non-polar)
- If yes, lone pair on central atom? (Yes = polar)
- If no, attached atoms all same?
- If yes, non-polar. If no, polar
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