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Question

Which of the following options does not give to the correct trends indicated against it?
(I) F2>Cl2>Br2>I2 : Bond dissociation energy
(II) F2>Cl2>Br2>I2: Oxidizing nature
(III) Cl>F>Br>I : Electron gain enthalpy
(IV) F>Cl>Br>I : Electronegativity


Correct Answer
A
I only
Your Answer
B
II and III
Your Answer
C
III and IV
Your Answer
D
II, III and IV

Solution

The correct option is A I only
(I) Because of small size of fluorine atom  there is a high inter electronic repulsion between two fluorine atoms.
The correct decreasing order is: Cl2>Br2>F2>I2
(II) Oxidation ability decreases on moving down the group because of electronegativity  and hydration energy decreases.
The correct decreasing order is F2>Cl2>Br2>I2
(III) Electron gain enthalpy becomes less negative on moving down a group due to an increase in the atomic size. However, the electron gain enthalpy of F is less negative than that of Cl due to electron-electron repulsion in the small-sized F atom. Thus, the correct order is F<Cl>Br>I.
(IV) Electronegativity decreases as we move doen the group, so the correct order is F>Cl>Br>I

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