Ethane Structure and Lewis Formula with Diagrams
Ethane is essential in chemistry and helps students understand various practical and theoretical applications related to this topic. This simple hydrocarbon is the foundation for learning about alkanes, bonding, and how natural gas fuels modern life. Let's explore everything about ethane below!
What is Ethane in Chemistry?
A hydrocarbon, ethane is an alkane with the formula C2H6. It consists of two carbon atoms and six hydrogen atoms joined by single bonds. This concept appears in chapters related to alkane structure, hydrocarbons, and organic compounds, making it a foundational part of your chemistry syllabus.
Molecular Formula and Composition
The molecular formula of ethane is C2H6. It consists of a single carbon–carbon bond, with three hydrogen atoms attached to each carbon. Ethane belongs to the alkane family, which are all saturated hydrocarbons containing only single bonds.
Preparation and Synthesis Methods
Industrially, ethane is separated from natural gas using a process called cryogenic distillation. In the laboratory, ethane can be prepared by the Wurtz reaction, where ethyl halides are reacted with sodium metal in dry ether:
C2H5Br + 2Na + BrC2H5 → C2H6 + 2NaBr
Another method involves the hydrogenation of ethylene (ethene) using a catalyst.
Physical Properties of Ethane
Ethane is a colorless, odorless, and flammable gas at room temperature. Here is a compact summary of its main physical properties:
| Property | Value |
|---|---|
| Chemical Formula | C2H6 |
| Molar Mass | 30.07 g/mol |
| Boiling Point | -88.5 °C |
| Melting Point | -182.8 °C |
| Solubility | Very slightly soluble in water |
| State at Room Temperature | Gas |
Chemical Properties and Reactions
Ethane is a stable alkane, so it is not very reactive. However, it undergoes certain important reactions:
1. Combustion: Burns in oxygen to form carbon dioxide and water.
C2H6 + 3.5 O2 → 2CO2 + 3H2O
2. Halogenation: Reacts with chlorine or bromine under UV light to produce haloalkanes.
3. Cracking: Can be thermally cracked to form ethylene (ethylene is vital for manufacturing plastics).
Frequent Related Errors
- Confusing ethane with ethene (C2H4), which is an alkene with a double bond.
- Assuming ethane is an unsaturated hydrocarbon (it is saturated and contains only single bonds).
- Mistaking ethane for being toxic or poisonous (at normal exposure levels, it is not toxic).
- Incorrectly drawing the Lewis structure (forgetting the complete eight electrons on both carbons).
Uses of Ethane in Real Life
Ethane is widely used in the petrochemical industry. Key uses include:
- As a feedstock for producing ethylene (used to make plastics like polyethylene).
- Limited use as a fuel, mostly where natural gas is processed.
- Used in laboratories and refrigeration systems in liquid form.
- Helps make acetic acid, ethanol, and other chemicals via chemical conversion.
Relation with Other Chemistry Concepts
Ethane connects with several important chemistry topics. For example, its simple bonding and structure are the basis for learning about alkanes and organic compounds.
The way ethane burns links to combustion reactions and energy cycles. Compared to methane and ethene, it helps students see differences between saturated and unsaturated hydrocarbons.
Step-by-Step Reaction Example
1. Combustion of ethane:C2H6 + O2 → CO2 + H2O
2. Balance carbon first:
C2H6 + O2 → 2CO2 + H2O
3. Balance hydrogen next (6 H = 3 H2O):
C2H6 + O2 → 2CO2 + 3H2O
4. Balance oxygen (2x2 = 4, 3x1 = 3; total 7 O on right):
Use 3.5 O2 on left.
5. Final Balanced Equation:
C2H6 + 3.5 O2 → 2CO2 + 3H2O
Lab or Experimental Tips
Remember ethane as the "two-carbon, single-bond" alkane! A simple way to draw ethane is to write two “CH3” groups connected by a single line (CH3–CH3). Vedantu educators often use this tip in live sessions to help students quickly visualize ethane's structure for exam diagrams.
Try This Yourself
- Write the IUPAC name of C2H6.
- Draw the full Lewis structure for ethane with all bonds shown.
- Compare ethane and ethene—what is the main difference in bonding?
- List two uses of ethane in the petrochemical industry.
Final Wrap-Up
We explored ethane—its structure, properties, reactions, and real-life importance. Understanding ethane forms the base for concepts like alkanes, hydrocarbons, and chemical reactions. For more in-depth explanations and exam-prep tips, explore live classes and notes on Vedantu.
Related Reading: Alkanes, Hydrocarbons, Organic Compounds, Methane
FAQs on Ethane – Structure, Formula, Properties and Uses
1. What is the chemical formula of ethane?
Ethane has the chemical formula C2H6. This means each molecule contains two carbon atoms and six hydrogen atoms, forming a saturated hydrocarbon (alkane).
2. What is ethane used for?
Ethane is primarily used as a raw material in chemical industries. Main uses include:
- Production of ethylene (for making plastics and polymers)
- As a petrochemical feedstock
- Limited use as a gaseous fuel
3. Is ethane toxic to humans?
Ethane is generally non-toxic at low concentrations. However, in enclosed spaces, it may displace oxygen and cause suffocation. It is flammable but considered less hazardous than some other hydrocarbons.
4. Why is ethane not commonly used as a fuel?
Ethane is less commonly used as a fuel because:
- Methane is more abundant and easier to handle
- Ethane is mainly reserved for industrial chemical production
- Storage and transport are more challenging than for methane
5. What is the molar mass of ethane?
The molar mass of ethane (C2H6) is 30.07 grams per mole (g/mol). This is calculated as:
- 2 × 12.01 (C) = 24.02
- 6 × 1.008 (H) = 6.048
- Total = 30.07 g/mol
6. What is the structure of ethane?
Ethane has a single covalent bond between two carbon atoms, with each carbon atom bonded to three hydrogen atoms. The structural formula is written as CH3–CH3, and the molecule is tetrahedral around each carbon atom.
7. What are the physical properties of ethane?
Ethane is a colorless, odorless, flammable gas under standard conditions. Key properties include:
- Boiling point: –88.6 °C
- Melting point: –182.8 °C
- Slightly soluble in water
- Density: 1.356 kg/m3 (at 0°C)
8. How is ethane's structure different from ethene?
Ethane (C2H6) contains a single bond between the two carbon atoms (alkane), while ethene (C2H4) contains a double bond (alkene). Ethane is saturated; ethene is unsaturated.
9. Can ethane form isomers?
No, ethane cannot form structural isomers. Its carbon chain is too short for rearrangement, so only one structural form exists for C2H6.
10. What is the hybridization of carbon atoms in ethane?
Both carbon atoms in ethane are sp3 hybridized, resulting in a tetrahedral geometry around each carbon atom. This allows for single (sigma) bonds only.
11. How is ethane obtained in industry?
Industry obtains ethane mainly by:
- Fractional distillation of natural gas
- Cryogenic separation from natural gas streams
12. How does ethane impact the environment?
Ethane is a volatile organic compound that can participate in atmospheric reactions leading to ozone formation. However, its direct greenhouse gas effect is much lower than methane.
