Answer
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Hint: To answer this question, you should recall the concept of oxoacids of phosphorus. Phosphorus belongs to group 15 of the periodic table and forms various oxoacids: hypo phosphorous acid\[\left( {{H_3}P{O_2}} \right)\], Phosphorous acid\[\left( {{H_3}P{O_3}} \right)\], Hypo phosphoric acid\[\left( {{H_3}P{O_4}} \right)\], pyro phosphoric acid \[\left( {{H_4}{P_2}{O_7}} \right)\]and poly metaphosphoric acid\[{\left( {HP{O_3}} \right)_n}\].
Complete Step by step solution:
Oxoacids of phosphorus which contain phosphorus-oxygen linkages are the most dominated subset in Phosphorus Chemistry.
Pyro phosphoric acid is a tetrabasic acid and prepared by heating orthophosphoric acid at about \[{250^o}{\text{C}}\] : \[2{H_3}P{O_4} \to {H_4}{P_2}{O_7} + {H_2}O\] The structure of Pyro phosphoric acid can be represented as:
The chemical formula of pyrophosphoric acid is \[{H_4}{P_2}{O_5}\]. The structure can be represented as:
The formula for Poly metaphosphoric acid is \[{(HP{O_3})_n}\]. It has a linear polymer structure where the oxidation state of phosphorus is +5. The structure can be represented as:
Cyclo trimetaphosphoric acid is a tribasic acid of phosphorus which has a formula \[{(HP{O_3})_3}\]. The three metaphosphoric acid molecules form a ring structure. Phosphorus is in the $ + 5$ oxidation state. In this structure, there are three \[P - OH\] bonds, three \[P = O\] bonds, and three \[P - O - P\] bonds:
Note: Important acidic nature of oxoacids of phosphorus: You are already aware of the term acids. These acids show varied physical and chemical properties of acids. Some simple ones are – they need a pH below 7, they turn blue paper red, they need a sour taste and that they react with alkalis to make salts. There is little difference of acidic strength among \[{{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_{\text{4}}}{\text{, }}{{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_{{\text{3}}}}{\text{ and }}{{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_{\text{2}}}\] because the hydrogen in these acids aren't all bonded to oxygen, and phosphorus isn't a highly electronegative element i.e. its oxides are less basic and electronegativities of ${\text{P}}$ and ${\text{H}}$ are almost the same. Hence, they all have almost similar acidic strength.
Complete Step by step solution:
Oxoacids of phosphorus which contain phosphorus-oxygen linkages are the most dominated subset in Phosphorus Chemistry.
Pyro phosphoric acid is a tetrabasic acid and prepared by heating orthophosphoric acid at about \[{250^o}{\text{C}}\] : \[2{H_3}P{O_4} \to {H_4}{P_2}{O_7} + {H_2}O\] The structure of Pyro phosphoric acid can be represented as:
![seo images](https://www.vedantu.com/question-sets/5580aeac-4bb4-40a3-af05-fafcace569a38488914411806007702.png)
The chemical formula of pyrophosphoric acid is \[{H_4}{P_2}{O_5}\]. The structure can be represented as:
![seo images](https://www.vedantu.com/question-sets/63e44eb9-a913-4b45-a6de-667b6d4d6b86313850814907133435.png)
The formula for Poly metaphosphoric acid is \[{(HP{O_3})_n}\]. It has a linear polymer structure where the oxidation state of phosphorus is +5. The structure can be represented as:
![seo images](https://www.vedantu.com/question-sets/05ca3e53-8c42-4ef8-8d7f-0ba37b8dd0e59154193986796931801.png)
Cyclo trimetaphosphoric acid is a tribasic acid of phosphorus which has a formula \[{(HP{O_3})_3}\]. The three metaphosphoric acid molecules form a ring structure. Phosphorus is in the $ + 5$ oxidation state. In this structure, there are three \[P - OH\] bonds, three \[P = O\] bonds, and three \[P - O - P\] bonds:
![seo images](https://www.vedantu.com/question-sets/84143fbe-94cb-4c85-bd8f-a9477fd326295561879524900893785.png)
Note: Important acidic nature of oxoacids of phosphorus: You are already aware of the term acids. These acids show varied physical and chemical properties of acids. Some simple ones are – they need a pH below 7, they turn blue paper red, they need a sour taste and that they react with alkalis to make salts. There is little difference of acidic strength among \[{{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_{\text{4}}}{\text{, }}{{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_{{\text{3}}}}{\text{ and }}{{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_{\text{2}}}\] because the hydrogen in these acids aren't all bonded to oxygen, and phosphorus isn't a highly electronegative element i.e. its oxides are less basic and electronegativities of ${\text{P}}$ and ${\text{H}}$ are almost the same. Hence, they all have almost similar acidic strength.
![seo images](https://www.vedantu.com/question-sets/87bf527e-6f23-4b0a-92f1-74fe5b9a23571299295902390772292.png)
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