π What are Single Bonds?
A single bond is a chemical bond where one pair of electrons is shared between two atoms. Think of it like holding hands β each person contributes one hand to form the connection.
π What are Double Bonds?
A double bond is a chemical bond where two pairs of electrons are shared between two atoms. It's like holding hands *and* linking arms - a stronger connection! These are common in organic molecules.
π What are Triple Bonds?
A triple bond is a chemical bond where three pairs of electrons are shared between two atoms. Imagine holding hands, linking arms, *and* putting your arms around each other's backs! This is an even stronger and shorter bond compared to single and double bonds. These are less common but very important.
π§ͺ Single vs. Double vs. Triple Bonds: A Side-by-Side Comparison
| Feature |
Single Bond |
Double Bond |
Triple Bond |
| Number of Electron Pairs Shared |
1 |
2 |
3 |
| Bond Strength |
Weakest |
Intermediate |
Strongest |
| Bond Length |
Longest |
Intermediate |
Shortest |
| Bond Energy |
Lowest |
Intermediate |
Highest |
| Rotation |
Free Rotation |
Restricted Rotation |
Restricted Rotation |
| Example |
Ethane ($C_2H_6$) |
Ethene ($C_2H_4$) |
Ethyne ($C_2H_2$) |
π‘ Key Takeaways
- 𧬠Strength: Triple bonds are the strongest, followed by double bonds, and then single bonds.
- π Length: Triple bonds are the shortest, followed by double bonds, and then single bonds.
- π Rotation: Single bonds allow free rotation, while double and triple bonds restrict rotation.
- π§ͺ Reactivity: Molecules with double and triple bonds are generally more reactive than those with only single bonds because of the higher electron density.