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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
Draw structure of Chlorine pentafluoride
Give two examples to show the anomalous behaviour of fluorine.
Why are halogens coloured?
With what neutral molecule is ClO− isoelectronic? Is that molecule a Lewis base?
Arrange the following in the decreasing order of their reducing character :
HF, HCl, HBr, HI
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
The reaction \[\ce{3ClO- (aq) -> ClO3- (aq) + 2Cl- (aq) + 2Cl- (aq)}\] is an example of
Arrange the following in the increasing order of the property mentioned:
MF, MCl, MBr, MI (ionic character)
