What is the Difference Between Ethane and Ethene?
🆚 Go to Comparative Table 🆚Ethane and ethene are both hydrocarbons, but they have different structures and properties. The main differences between ethane and ethene are:
- Structure: Ethane has single bonds only, whereas ethene has a double bond between the two carbon atoms. Ethane is considered a saturated hydrocarbon, while ethene is considered an unsaturated hydrocarbon.
- Molecular Formula: The molecular formula for ethane is C2H6, and for ethene, it is C2H4.
- Hybridization: The carbon atoms in ethane are sp3 hybridized, while the carbon atoms in ethene are sp2 hybridized.
- Reactivity: Ethene has a double bond, which is electron-rich, making it easier to attract an electrophile and break the double bond to form multiple single bonds. Ethane is more stable and less reactive due to its saturated structure.
- Boiling Point: Ethane has stronger intermolecular attractions (van der Waals forces) than ethene, which results in a higher boiling point for ethane.
- Polymerization: Ethene can undergo polymerization reactions, but ethane cannot.
- Bromine Test: Ethene and ethane can be differentiated using the bromine test. Ethene is an unsaturated compound and will decolorize bromine water, while ethane is a saturated compound and will not decolorize bromine water.
Comparative Table: Ethane vs Ethene
Here is a table comparing the differences between ethane and ethene:
Property | Ethane | Ethene |
---|---|---|
Chemical Formula | C2H6 | C2H4 |
Molecular Structure | Each carbon atom is bonded to four hydrogen atoms (tetrahedral structure). | Each carbon atom is bonded to three hydrogen atoms and has a double bond with the other carbon atom (trigonal planar structure with each bond angle approximately 120 degrees). |
Bonding | Each carbon requires a full octet and forms four sigma bonds with hydrogen atoms and one sigma bond between the carbons (forming a total of 7 sigma bonds). | Each carbon atom forms three sigma bonds with hydrogen atoms and a pi bond with the other carbon atom (forming a total of 6 sigma bonds and 1 pi bond). |
Stability | Ethane has stronger intermolecular attractions (van der Waals forces) than ethene, making it more stable. | Ethene has a double bond, which is electron-rich, making it easier to attract an electrophile and break the double bond to form multiple single bonds. A pi bond is easier to break than a sigma bond, making ethene more reactive than ethane. |
Boiling Point | Ethane has a higher boiling point than ethene due to its stronger intermolecular attractions. | Ethene has a lower boiling point than ethane because of its weaker intermolecular attractions. |
In summary, ethane has a more stable structure with tetrahedral geometry and a higher boiling point, while ethene has a trigonal planar geometry with a double bond between the carbons, making it more reactive and with a lower boiling point.
Read more:
- Ethane Ethene vs Ethyne
- Methane vs Ethane
- Ethane vs Ethanol
- Acetylene vs Ethylene
- Ethylene vs Ethylidene
- Ethyl Nitrite vs Nitroethane
- Alkenes vs Alkynes
- Butane vs Butene
- Cyclohexane vs Cyclohexene
- Chloroethane vs Chlorobenzene
- Ethyl vs Methyl
- Ethanol vs Methanol
- Ethyl Alcohol vs Ethanol
- Ether vs Ketone
- Ether vs Petroleum Ether
- Ethyl Chloride vs Chlorobenzene
- Alkanes vs Alkenes
- Ethanol vs Ethanoic Acid
- Ethanal vs Propanal