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प्रश्न
Arrange the following in the decreasing order of their reducing character :
HF, HCl, HBr, HI
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उत्तर
The bond length of the given molecules increases down the group. Therefore, the tendency to lose H+ increases down the group. Hence, the decreasing order of reducing character is HI>HBr>HCl>HF.
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संबंधित प्रश्न
Account for the following: Fluorine does not exhibit positive oxidation state.
Fluorine is a stronger oxidising agent than chlorine. Why?
Account for the following :
Acidic character increases from HF to HI.
Why are halogens coloured?
Arrange the following in the order of property indicated for the given set:
HF, HCl, HBr, HI - increasing acid strength.
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:
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 |
Which of the following statements are true?
(i) Only type of interactions between particles of noble gases are due to weak dispersion forces.
(ii) Ionisation enthalpy of molecular oxygen is very close to that of xenon.
(iii) Hydrolysis of XeF6 is a redox reaction.
(iv) Xenon fluorides are not reactive.
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.
