Advertisements
Advertisements
Question
Fluorine is a stronger oxidising agent than chlorine. Why?
Advertisements
Solution
The oxidising power of halogens decreases as we go down the group. The electrode potential of F2 is +2.87 V, while that of Cl2 is +1.36 V. This means that fluorine can be reduced more easily than chlorine. Therefore, fluorine is the strongest oxidising agent.
APPEARS IN
RELATED QUESTIONS
Draw structure of Chlorine pentafluoride
Account for the following: Fluorine does not exhibit positive oxidation state.
Why are halogens coloured?
With what neutral molecule is ClO− isoelectronic? Is that molecule a Lewis base?
The set with the correct order of acidity is:
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 |
Give reason to explain why ClF3 exists but FCl3 does not exist.
Iodine has lowest oxidiation state in ______.
Arrange the following in the increasing order of the property mentioned:
MF, MCl, MBr, MI (ionic character)
