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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.
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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
Fluorine is a stronger oxidising agent than chlorine. Why?
Account for the following :
Acidic character increases from HF to HI.
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
Give two examples to show the anomalous behaviour of fluorine.
Write the reactions of F2 with water.
With what neutral molecule is ClO− isoelectronic? Is that molecule a Lewis base?
Complete chemical reactions are:Cl2 + H2O →
Select the correct alternative from the choices given :
The correct order of increasing acidic strength of the oxoacids of chlorine is:
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 ____________.
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 ______.
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.
Iodine has lowest oxidiation state in ______.
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.
