Statement I : Acid strength increases in the order given as $H F << H C l << H B r << H I .$
Statement II : As the size of the elements $F, C l, B r, I$ increases down the group, the bond strength of $H F, H C l, H B r a n d H I$ decreases and so the acid strength increases. In the light of the above statements, choose the correct answer from the options given below

Statement I is incorrect but Statement II is true

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Both statement I and Statement II are true

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Both Statement I and Statement II are false

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Statement I is correct but statement II is false

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Solution

The correct option is B Both statement I and Statement II are true
In the modern periodic table, moving down the group as the size of halogen atom increases, the H – X bond length also increases as a result the bond enthalpy decreases. Hence, The acidic strength also increases.
So, the correct order of acidic strength is
$H I > H B r > H C l > H F$

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Similar questions

H F << H C l << H B r << H I .

Statement II : As the size of the elements

F, C l, B r, I

H F, H C l, H B r a n d H I

H F << H C l << H B r << H I

F, C l, B r, I

H F, H C l, H B r, and H I

Arrange the following in the order of property indicated for each set:

(i) F₂, Cl₂, Br₂, I₂ - increasing bond dissociation enthalpy.

(ii) HF, HCl, HBr, HI - increasing acid strength.

(iii) NH₃, PH₃, AsH₃, SbH₃, BiH₃ − increasing base strength.

H F, H C l, H B r, H I

Arrange the following in the order of property indicated for each set:

$F_{2}, C l_{2}, B r_{2}, I_{2}$ - increasing bond dissociation enthalpy.

HF,HCl, HBr, HI- Increasing acid strength.

$N H_{3}, P H_{3}, A s H_{3}, S b H_{3}, B i H_{3}$ - increasing base strength.

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