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प्रश्न
Account for the following: Fluorine does not exhibit positive oxidation state.
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उत्तर
Fluorine being the most electronegative atom does not exhibit positive oxidation state because the electrons in fluorine are strongly attracted by the nuclear charge because of small size of fluorine atom and therefore, removal of an electron is not possible.
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संबंधित प्रश्न
Which halogen compound in each of the following pairs will react faster in SN2 reaction
(CH3)3 C – Cl or CH3 – Cl
Write the reactions of F2 with water.
Complete the following equations:
KMnO4 
Arrange the following in the decreasing order of their reducing character :
HF, HCl, HBr, HI
Fluorine differs from the rest of the halogens in some of its properties. This is due to ____________.
Bond dissociation enthalpy of E–H (E = element) bonds is given below. Which of the compounds will act as the strongest reducing agent?
| Compound | \[\ce{NH3}\] | \[\ce{PH3}\] | \[\ce{AsH3}\] | \[\ce{SbH3}\] |
| Δdiss (E – H)/kJ mol–1 | 389 | 322 | 297 | 255 |
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 the 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:
MF, MCl, MBr, MI (ionic character)
