Advertisements
Advertisements
प्रश्न
Arrange the following in the order of property indicated for the given set:
HF, HCl, HBr, HI - increasing acid strength.
Arrange the following according to the property mentioned against the given:
HF, HCI, HI, HBr in the order of increasing acid strength.
Advertisements
उत्तर १
HF < HCl < HBr < HI
The bond dissociation energy of the H-X molecules, where X=F, Cl, Br, and I, decreases with an increase in the atomic size. Since the H-I bond is the weakest, HI is the strongest acid.
उत्तर २
The acid strength of HF, HCl, HBr and HI depends upon their bond dissociation enthalpies. Since the bond dissociation enthalpy of the H-X bond decreases from H-F to H-I as the size of the atom increases from F to I.
Thus, the acid strength order is HF < HCl < HBr < HI
The weak acidic strength of HF is also due to H-bonding, due to which the release of H+ becomes difficult.
संबंधित प्रश्न
Iodine exists as
- polar molecular solid
- ionic solid
- nonpolar molecular solid
- hydrogen bonded molecular solid
Draw structure of Chlorine pentafluoride
F2 has lower bond dissociation enthalpy than Cl2. Why?
Which halogen compound in each of the following pairs will react faster in SN2 reaction
(CH3)3 C – Cl or CH3 – Cl
Why are halogens coloured?
Complete chemical reactions are:Cl2 + H2O →
Complete the following equations:
KMnO4 
Arrange the following in the decreasing order of their reducing character :
HF, HCl, HBr, HI
Cl2 acts as a bleaching agent.
Tincture of iodine is ____________.
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:
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 |
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.
Give a reason for the following:
Mn+2 compounds are more stable than Fe+2 compounds.
Arrange the following in the increasing order of the property mentioned:
MF, MCl, MBr, MI (ionic character)
