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प्रश्न
Arrange the following in the order of property indicated for each set:
HF, HCl, HBr, HI - increasing acid strength.
उत्तर १
HF < HCl < HBr < HI
The bond dissociation energy of H-X molecules where X = F, Cl, Br, I, decreases with an increase in the atomic size. Since H-I bond is the weakest, HI is the strongest acid.
उत्तर २
Acid strength of HF, HCI, HBr and HI depends upon their bond dissociation enthalpies. Since the bond dissociation enthalpy of H – X bond decreases from H – F to H-l as the size of atom increases from F to I.
Thus, the acid strength order is HF < HCI < HBr < HI
The weak acidic strength of HF is also due to H-bonding due to which release of H+ becomes difficult.
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संबंधित प्रश्न
Iodine exists as
- polar molecular solid
- ionic solid
- nonpolar molecular solid
- hydrogen bonded molecular solid
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.
Write two uses of ClO2.
Write the reactions of F2 and Cl2 with water.
With what neutral molecule is ClO− isoelectronic? Is that molecule a Lewis base?
Complete the following equations:
KMnO4 
Arrange the following in the decreasing order of their reducing character :
HF, HCl, HBr, HI
The set with the correct order of acidity is:
Which is the strongest acid in the following:
Which of the following pairs of ions are isoelectronic and isostructural?
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 |
In solid state \[\ce{PCl5}\] is a ______.
The reaction \[\ce{3ClO- (aq) -> ClO3- (aq) + 2Cl- (aq) + 2Cl- (aq)}\] is an example of
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 light of the above statements, choose the correct answer from the options given below.
Give a reason for the following:
Mn+2 compounds are more stable than Fe+2 compounds.
