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Why the oxidising power of HClO4,HCl03,HCl02,HClO are in the order of HCl0>HCl02>HCl03>HCl04.

Why the oxidising power of HClO4,HCl03,HCl02,HClO are in the order of HCl0>HCl02>HCl03>HCl04.


13 Answers

Vaibhav Jindal (Meet the Champ)
53 Points
10 years ago

Dear sunindra Kanghujan

The oxiding power of HClO4, HClO3, HCLO2, HClO are in the order 

 HClO >HCLO2 >HClO3>HClO4 because the oxidising states of chlorine in HClO4, HClO3, HCLO2, HClO are 7,5,3,1 respectively so HClO with lowest oxidation state of chlorine have greatest tendency to get oxidised and increase its oxidation state.

Hope this has helped you Smile

19 Points
10 years ago

 higher the oxidation no. higher is the oxidizing power. 

for e.g.

in hclo o.n is -1

in hclo2 o.n is -3.

Sajid Zaman
14 Points
7 years ago
because of HClO4 is more stable than other oxyacids of chlorine so its oxidizing power is low.
Sajid Zaman
14 Points
7 years ago
The oxiding power of HClO4, HClO3, HCLO2, HClO are in the following order: HClO >HCLO2 >HClO3>HClO4 because the oxidizing power of oxyacids of chlorine is inversely related to the thermal stability of these acids i.e. higher the thermal stability, lower will be oxidizing power of the oxyacid and vice versa. For example the HClO4 is most stable so it has lowest oxidizing power amongst the oxyacids of chlorine. The order of thermal stability of oxyacids of chlorine is HClO4>HClO3>HClO2>HClO.
11 Points
4 years ago
Actually with increase in oxidation state of the central atom, the X-O bond acquires more amount of covalent character due to polarisation, hence the electron deficiency gets somehow compensated. Thus the oxidizing power decreases. Moreover the X-O bond acquires partial double bond character in the compounds of higher oxidation state. Hence in order to get reduced, X-O bond has to be broken which requires more energy.
19 Points
4 years ago
Bcoz here oxidising power is asked which refers​to loose of electrons so the one having lowest oxidation state will have highest oxidising power as it has electrons so it can easily loose them
13 Points
4 years ago
The partial double bond character in HClO4 is the highest as there are 3 Cl=O bonds and also the highest when compared to the rest so it is thermally the most stable. Now coming to the oxidizing power, it basically means the ability to Gain Electrons, remember that pal, to gain electrons and Oxidize Others. Oxidizing power concerns itself to oxidize others. So HClO4 being the most stable does not gain electrons and the Enthalpy of its gaining electron is very low (assuming the magnitude of enthalpy not its sign). And hence the reaction of HClO gaining electrons is more feasible and hence the best oxidizing agent.
11 Points
4 years ago
Just see their structures hclo4 is resonance stablised so has least probability of accepting an electron , so among them hclo will accept electron more easily due to no resonance
Sanjit Barueal
16 Points
2 years ago
The oxidising power of oxy acids depends on its oxidation state.I.e. higher the oxidation state of chlorine stronger will be the oxidising power.Hence oxidising strength of oxyacids are in the following order:
HClO>HClO2>HClO3>HClO4 and so on.
Cool Tight Killa
13 Points
2 years ago
All of the above answers are wrong. Higher the oxidation state, higher the tendency to get reduced meaning higher the oxidising power. This should imply that HClO4(Cl at +7 oxidation number) should oxidise more than HOCl(Cl at +1 oxidation number) right? The actual explanation for why HClO4 is less oxidising than HOCl is that HOCl performs what is referred as bleaching. In this process, actual Oxygen is released which is a better oxidising agent than most other compounds irrespective of oxidation state similar to how KMnO4(with Mn at +7) is a worse oxidising agent than K2Cr2O7(Cr at +6) , due to Standard Oxidation and Reduction Potential values.
Please do not approve scientifically wrong answers that appear logically correct.
13 Points
2 years ago
in acidic conditions Mn(+7)changes to Mn(+2) which is more stable than Cr(+3).So permanganate is a better oxidising agent than dichromate.But this cannot be applied here is the problem.
Kushagra Madhukar
askIITians Faculty 629 Points
one year ago
Hi Student
The reason behind this trend lies in the resonance stabilisation of oxoanions of chlorine of the compounds mentioned.
ClO4- has four resonance structures
ClO3has 3 resonance structures
ClO2has 2 resonance structures
ClO- has no stabilising resonance structure
Hence based on their resonance stabilisation, we can arrange them in the order of stability as follows
ClO4- > ClO3- > ClO2- > ClO-
Hence the order of acidic nature of these compounds follows the order-
HClO4 > HClO3 > HClO2 > HClO   
( as more the stability of anion, more will be the tendency of the acid to lose H+ and achieve that stable form)
Now, we know that acids are reducing agents and more the acidic nature, the more will be the reducing nature and thus lesser will be oxidising nature of the compound.
In short, oxidising nature is inversely proportional to the acidic nature.
Therefore, we conclude the order of oxidising power is
HClO4 3 
Hope it helps.
13 Points
5 months ago
Bruh if you don't know don't mislead others. 
This is the actual reason,
Oxidation state of Cl can vary from - 1 to +7. If we calculate the oxidation number of HClO we get a Oxidation number of +1. But as mentioned earlier Cl can have a variety of higher oxidation states hence has a very chance of getting oxidised. But if we see HClO4 the Oxidation number of Cl has obtained a maximum(+7) therefore it won't get oxised further. Keeping the minimum tendacy of oxidation to be HClO4 and the maximum tenancy as HClO, arrange the rest of the oxoacids of chlorine:)) 

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