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प्रश्न
Arrange the following in the decreasing order of their reducing character :
HF, HCl, HBr, HI
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
Fluorine is a stronger oxidising agent than chlorine. Why?
F2 has lower bond dissociation enthalpy than Cl2. Why?
Give two examples to show the anomalous behaviour of fluorine.
Write the reactions of F2 and Cl2 with water.
Arrange the following in the order of property indicated for each set:
HF, HCl, HBr, HI - increasing acid strength.
Complete the following equations:
KMnO4 
Which one has the lowest boiling point?
Which is the strongest acid in the following:
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.
Arrange the following in the increasing order of the property mentioned:
\[\ce{MF}\], \[\ce{MCl}\], \[\ce{MBr}\], \[\ce{MI}\] (ionic character)
