Advertisements
Advertisements
Question
Arrange the following in the decreasing order of their reducing character :
HF, HCl, HBr, HI
Advertisements
Solution
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.
APPEARS IN
RELATED QUESTIONS
Iodine exists as
- polar molecular solid
- ionic solid
- nonpolar molecular solid
- hydrogen bonded molecular solid
Account for the following :
Acidic character increases from HF to HI.
F2 has lower bond dissociation enthalpy than Cl2. Why?
Give two examples to show the anomalous behaviour of fluorine.
Complete chemical reactions are:Cl2 + H2O →
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 |
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)
