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Standard XI
Chemistry
Hydrogen Bonding
Question

When we move from HF to HCl, the boiling point drops sharply but on moving further to HBr and HI the boiling point increases. Why ? or Out of HCl, HBr, and HI which has lowest boiling point and why ?

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Solution
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In $$H - F$$ there is H-bonding. Hence the boiling point is high. There is no H-bonding in $$HCl.$$ So the boiling point is less. On moving further to $$HBr$$ and $$HI,$$ the size of the molecules increases and so the van der Waal's forces increase and so does the boiling point. Hence $$HCl$$ has the lowest boiling point.

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Similar Questions
Q1
When we move from HF to HCl, the boiling point drops sharply but on moving further to HBr and HI the boiling point increases. Why ? or Out of HCl, HBr, and HI which has lowest boiling point and why ?
View Solution
Q2
The boiling points of HF,HCl,HBr and HI follows the order:
View Solution
Q3
Use the information and data given below to answer the questions (a) to (c):

$$\bullet$$ Stronger intermolecular forces result in a higher boiling point.
$$\bullet$$ Strength of London forces increases with the number of electrons in the molecule.
$$\bullet$$ Boiling point of $$HF,HCl,HBr$$ and $$HI$$ are $$293K,189K,206K$$ and $$238K$$ respectively.

(a) Which type of intermolecular forces are present in the molecules $$HF, HCl, HBr,$$ and $$HI$$?
(b) Looking at the trend of boiling points of $$HCl,HBr$$ and $$HI$$, explain out of dipole-dipole interaction and London interaction, which one is predominant here?
(c) Why is the boiling point of $$HF$$ highest while that of hydrogen chloride lowest?
View Solution
Q4
A Which type of intermolecular forces are present in the molecules HF,HCl,HBr and HI?

B Looking at the trend of boiling points of HCl,HBr and HI, explain out of dipole-dipole interactions and London interaction, which one is predominant here.

C Why is the boiling point of hydrogen fluoride highest while that of hydrogen chloride lowest?
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Q5

Use the information and date given below to answer the question (a) to (c),

Stronger intermolecular forces result in higher boiling point.

Strength of London forces increases with the number of electrons in the molecule.

Boiling point of HF,HCl, HBr and Hi are 293 k, 189 k, 206 k and 238 k respectively.

(a) Which type of intermolecular forces are present in the molecules HF, HCl, HBr an HI?

(b) Looking at the trend of boiling points of HCl, HBr and HI, explain out of dipole-dipole interaction and London interaction, which one is predominant here.

(c) Why is boiling point of hydrogen fluoride highest while that of hydrogen chloride lowest?

View Solution