The Question is from neet-chemistry chemical-thermodynamics inter-molecular-forces, and it was created by the author Mr. S M HUSSAIN

Question

Arrange the following compounds in order of increasing boiling point: $CH_3CH_2OH$, $CH_3OCH_3$, $CH_3CH_2CH_3$, $CH_3COOH$.

Mr. S M HUSSAIN · Accepted Answer

## CORE INFORMATION
✓ **Answer**: A
## CONCEPT FRAMEWORK
 **Primary Concept**: Intermolecular forces and boiling point
 **Related Topics**: Hydrogen bonding, dipole-dipole interactions, London dispersion forces
 **Prerequisites**: Understanding of intermolecular forces and their effect on boiling point.
## SOLUTION PATHWAY
**Given Information**:
  Four compounds: $CH_3CH_2OH$ (ethanol), $CH_3OCH_3$ (dimethyl ether), $CH_3CH_2CH_3$ (propane), $CH_3COOH$ (acetic acid).
  We need to arrange them in increasing order of boiling point.
**Method & Steps**:
 1. Identify the types of intermolecular forces present in each compound.
  Reasoning: Boiling point is directly related to the strength of intermolecular forces. Stronger intermolecular forces lead to higher boiling points.
  
 2. Compare the strengths of the intermolecular forces.
  Working:
  * $CH_3CH_2CH_3$ (propane): Only London dispersion forces (weakest).
  * $CH_3OCH_3$ (dimethyl ether): Dipole-dipole interactions (stronger than London dispersion forces, but weaker than hydrogen bonding).
  * $CH_3CH_2OH$ (ethanol): Hydrogen bonding (strongest among these compounds).
  * $CH_3COOH$ (acetic acid): Hydrogen bonding (stronger than ethanol due to dimerization through two hydrogen bonds).
  Key Point: Hydrogen bonding is significantly stronger than dipole-dipole interactions and London dispersion forces.
 3. Arrange the compounds in order of increasing boiling point.
  Result: $CH_3CH_2CH_3 < CH_3OCH_3 < CH_3CH_2OH < CH_3COOH$
  Verification: The order reflects the increasing strength of intermolecular forces.
 ## OPTION ANALYSIS
A ✓: $CH_3CH_2CH_3 < CH_3OCH_3 < CH_3CH_2OH < CH_3COOH$ - Correctly arranges the compounds based on increasing strength of intermolecular forces.
B :x: Incorrect order, placing dimethyl ether before propane.
C :x: Incorrect order, placing acetic acid before ethanol.
D :x: Incorrect order, completely reversed.
 ## LEARNING AIDS
 **Common Mistakes**:
  1.Ignoring the strength differences between hydrogen bonding, dipole-dipole, and London dispersion forces: Leads to incorrect ordering.
  How to avoid: Carefully analyze the molecular structure to identify all types of intermolecular forces.
  2.Overlooking the effect of molecular size on London dispersion forces: Larger molecules have stronger London dispersion forces.
  How to avoid: Consider the size and shape of the molecules when comparing London dispersion forces.
 **Quick Tips**:
  1.Prioritize hydrogen bonding as the strongest intermolecular force among these compounds.
  2.Remember that dipole-dipole interactions are stronger than London dispersion forces.

Mr. S M HUSSAIN · Answer

The correct Option is "$CH_3CH_2CH_3 < CH_3OCH_3 < CH_3CH_2OH < CH_3COOH$"

Mr. S M HUSSAIN · Answer

$CH_3OCH_3 < CH_3CH_2CH_3 < CH_3CH_2OH < CH_3COOH$

Mr. S M HUSSAIN · Answer

$CH_3CH_2CH_3 < CH_3COOH < CH_3CH_2OH < CH_3OCH_3$

Mr. S M HUSSAIN · Answer

$CH_3COOH < CH_3CH_2OH < CH_3OCH_3 < CH_3CH_2CH_3$

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