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Arrange the following compounds in decreasing order of their boiling points
(i) CH3Br (ii) CH3CH2Br (iii) CH3CH2CH2Br (iv) BrC6H4Br
(i) CH3Br (ii) CH3CH2Br (iii) CH3CH2CH2Br (iv) BrC6H4Br
- a)(i) > (ii) > (iii) > (iv)
- b)(iv) > (iii) > (ii) > (i)
- c)(i) > (iii) > (ii) > (iv)
- d)(iii) > (iv) > (i) > (ii)
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
Arrange the following compounds in decreasing order of their boiling p...
Boiling point is directly proportional to molecular masses.
Most Upvoted Answer
Arrange the following compounds in decreasing order of their boiling p...
Explanation:
There are several factors that influence the boiling points of organic compounds, including molecular size, shape, and polarity. In this case, we are comparing the boiling points of four different alkyl bromides.
Size of alkyl group:
- The size of the alkyl group attached to the bromine atom affects the boiling point. Generally, larger alkyl groups experience stronger London dispersion forces, leading to higher boiling points.
Branching of alkyl group:
- Branching decreases the surface area of the molecule, reducing the strength of intermolecular forces and lowering the boiling point.
Analysis of compounds:
- CH3Br: This compound is the smallest and simplest alkyl bromide. It has the lowest boiling point among the given compounds.
- CH3CH2Br: The addition of an ethyl group increases the size of the molecule, resulting in a higher boiling point compared to CH3Br.
- CH3CH2CH2Br: The presence of a propyl group further increases the size of the molecule, leading to a higher boiling point compared to CH3CH2Br.
- BrC6H4Br: This compound has the largest and most complex structure among the given compounds. It experiences stronger London dispersion forces due to its larger size, resulting in the highest boiling point.
Therefore, the correct order of boiling points is:
(iv) > (iii) > (ii) > (i)
There are several factors that influence the boiling points of organic compounds, including molecular size, shape, and polarity. In this case, we are comparing the boiling points of four different alkyl bromides.
Size of alkyl group:
- The size of the alkyl group attached to the bromine atom affects the boiling point. Generally, larger alkyl groups experience stronger London dispersion forces, leading to higher boiling points.
Branching of alkyl group:
- Branching decreases the surface area of the molecule, reducing the strength of intermolecular forces and lowering the boiling point.
Analysis of compounds:
- CH3Br: This compound is the smallest and simplest alkyl bromide. It has the lowest boiling point among the given compounds.
- CH3CH2Br: The addition of an ethyl group increases the size of the molecule, resulting in a higher boiling point compared to CH3Br.
- CH3CH2CH2Br: The presence of a propyl group further increases the size of the molecule, leading to a higher boiling point compared to CH3CH2Br.
- BrC6H4Br: This compound has the largest and most complex structure among the given compounds. It experiences stronger London dispersion forces due to its larger size, resulting in the highest boiling point.
Therefore, the correct order of boiling points is:
(iv) > (iii) > (ii) > (i)
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Arrange the following compounds in decreasing order of their boiling points (i) CH3Br (ii) CH3CH2Br (iii) CH3CH2CH2Br (iv) BrC6H4Bra)(i) > (ii) > (iii) > (iv)b)(iv) > (iii) > (ii) > (i)c)(i) > (iii) > (ii) > (iv) d)(iii) > (iv) > (i) > (ii)Correct answer is option 'B'. Can you explain this answer?
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