QQuestionChemistry
QuestionChemistry
Draw two Lewis structures for a compound with the formula C^2H^6O and compare the boiling points of the two molecules.
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Identify Possible Structural Isomers
There are two possible structural isomers for $$\mathrm{C}_{2}\mathrm{H}_{6}\mathrm{O}$$:
Step 3:
Ethanol ($$\mathrm{CH}_{3}\mathrm{CH}_{2}\mathrm{OH}$$)
Step 4:
Dimethyl ether ($$\mathrm{CH}_{3}\mathrm{OCH}_{3}$$)
Step 5:: Draw Lewis Structure for Ethanol
- Contains an $$\mathrm{OH}$$ hydroxyl group
\text{H} \ \text{|} \ \mathrm{H}-\mathrm{C}-\mathrm{C}-\mathrm{O}-\mathrm{H} \ \text{|} \quad \text{|} \ \text{H} \quad \text{H} \end{array} Key features: - Polar molecule due to hydrogen bonding - Capable of intermolecular hydrogen bonding
Step 6:: Draw Lewis Structure for Dimethyl Ether
- Contains an $$\mathrm{O}$$ atom connecting two methyl groups
\text{H} \quad \text{H} \ \text{|} \quad \text{|} \ \mathrm{H}-\mathrm{C}-\mathrm{O}-\mathrm{C}-\mathrm{H} \ \text{|} \quad \text{|} \ \text{H} \quad \text{H} \end{array} Key features: - Less polar - Cannot form hydrogen bonds as effectively
Step 7:: Compare Boiling Points
Ethanol boiling point: $$78.4 \mathrm{~°C}
Dimethyl ether boiling point: - 24.9 \mathrm{~°C} Explanation of Boiling Point Difference: - Ethanol has strong hydrogen bonding between molecules - Hydrogen bonds require more energy to break - Results in significantly higher boiling point - Dimethyl ether has weak intermolecular forces (van der Waals) - Requires less energy to separate molecules
Final Answer
The two \mathrm{C}_{2}\mathrm{H}_{6}\mathrm{O} isomers are ethanol and dimethyl ether. Ethanol has a much higher boiling point (78.4 \mathrm{~°C}) compared to dimethyl ether (- 24.9 \mathrm{~°C}) due to stronger intermolecular hydrogen bonding.
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