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प्रश्न
Draw structure of Chlorine pentafluoride
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उत्तर
Structure of Chlorine pentafluoride
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संबंधित प्रश्न
Iodine exists as
- polar molecular solid
- ionic solid
- nonpolar molecular solid
- hydrogen bonded molecular solid
Fluorine is a stronger oxidising agent than chlorine. Why?
Compare the oxidizing action of F2 and Cl2 by considering parameters such as bond dissociation enthalpy, electron gain enthalpy and hydration enthalpy.
Account for the following :
Acidic character increases from HF to HI.
F2 has lower bond dissociation enthalpy than Cl2. Why?
Which halogen compound in the following pair will react faster in SN2 reaction CH3Br or CH3I.
Give two examples to show the anomalous behaviour of fluorine.
Write two uses of ClO2.
Why are halogens coloured?
Arrange the following in the order of property indicated for the given set:
HF, HCl, HBr, HI - increasing acid strength.
Complete chemical reactions are:Cl2 + H2O →
Arrange the following in the decreasing order of their reducing character :
HF, HCl, HBr, HI
Select the correct alternative from the choices given :
The correct order of increasing acidic strength of the oxoacids of chlorine is:
Cl2 acts as a bleaching agent.
Which one has the lowest boiling point?
Fluorine differs from the rest of the halogens in some of its properties. This is due to ____________.
The set with the correct order of acidity is:
Which is the strongest acid in the following:
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 |
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.
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.
Write the name and formula of oxoacid of fluorine.
Arrange the following in the increasing order of the property mentioned:
MF, MCl, MBr, MI (ionic character)
