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प्रश्न
Explain why the stability of oxoacids of chlorine increases in the order given below:
\[\ce{HClO < HClO2 < HClO3 < HClO4}\]
उत्तर
Oxygen is more electronegative than chlorine, therefore dispersal of negative charge present on chlorine increases from \[\ce{ClO^{-}}\] to \[\ce{ClO^{-}_{4}}\] ion because number of oxygen atoms attached to chlorine is increasing. Therefore, stability of ions will increase in the order given below:
\[\ce{ClO < ClO2 < ClO3 < ClO5}\]
Thus due to increase instability of conjugate base, acidic strength of corresponding acid increases in the following order
\[\ce{HClO < HClO2 < HClO5 < HClO4}\]
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संबंधित प्रश्न
Write chemical formula of the following oxoacids of chlorine:
a. Hypochlorous acid
b. Chlorous acid
c. Chloric acid
d. Perchloric acid
Account for the following :
Fluorine forms only one oxoacid HOF
Draw the structures of the following:
(1) HClO4
(2) H3PO3
Draw the structures of the HClO3.
Arrange the following oxyacids of chlorine in decreasing order of their thermal stability. Give reason.
HOClO, HOCl, HClO4, HOClO2
The increasing order of reducing power of the halogen acids is:
A black compound of manganese reacts with a halogen acid to give greenish-yellow gas. When excess of this gas reacts with \[\ce{NH3}\] an unstable trihalide is formed. In this process the oxidation state of nitrogen changes from ______.
Assertion: \[\ce{HI}\] cannot be prepared by the reaction of KI with concentrated \[\ce{H2SO4}\]
Reason: \[\ce{HI}\] has lowest \[\ce{H - X}\] bond strength among halogen acids.
Which halogen forms an oxyacid that contains the halogen atom in tripositive oxidation state?
Which among the following factors is the most important in making fluorine, the strongest oxidizing halogen?
