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प्रश्न
F2 has lower bond dissociation enthalpy than Cl2. Why?
उत्तर
The size of a fluorine atom is very small as compared to a chlorine atom. Therefore, the repulsion between electrons in the outer most shell of the two atoms in a fluorine molecule is much greater than that in a chlorine molecule. Hence, it requires less energy to break up the fluorine molecule, making its bond dissociation energy lesser than that of chlorine molecule.
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संबंधित प्रश्न
Iodine exists as
- polar molecular solid
- ionic solid
- nonpolar molecular solid
- hydrogen bonded molecular solid
Write the reactions of F2 and Cl2 with water.
Arrange the following in the order of property indicated for each set:
HF, HCl, HBr, HI - increasing acid strength.
Arrange the following in the decreasing order of their reducing character :
HF, HCl, HBr, HI
Cl2 acts as a bleaching agent.
Fluorine differs from the rest of the halogens in some of its properties. This is due to ____________.
Reduction potentials of some ions are given below. Arrange them in decreasing order of oxidising power.
| Ion | \[\ce{CIO^{-}_{4}}\] | \[\ce{IO^{-}_{4}}\] | \[\ce{BrO^{-}_{4}}\] |
| Reduction potential EΘ/V |
EΘ = 1.19 V | EΘ = 1.65V | EΘ = 1.74 V |
Solubility of iodine in water may be increase by adding
Statement I: Acid strength increases in the order given as HF << HCl << HBr << HI.
Statement II: As the size of the elements F, Cl, Br, and I increase down the group, the bond strength of HF, HCl, HBr and HI decreases and so the acid strength increases.
In light of the above statements, choose the correct answer from the options given below.
Arrange the following in the increasing order of the property mentioned:
\[\ce{MF}\], \[\ce{MCl}\], \[\ce{MBr}\], \[\ce{MI}\] (ionic character)
