CameraIcon

SearchIcon

MyQuestionIcon

2

You visited us 2 times! Enjoying our articles? Unlock Full Access!

Hydrogen Peroxide

Explain: H3PO...

Question

Explain: H3PO2 shows reducing properties but H3PO4 does not.

Open in App

Solution

In H3PO2 and H3PO3 oxidation state of P is +1 and +3 respectively, which

can further be oxidized to a higher oxidation state. Hence they can act as

reducing agents. In H3PO4 oxidation state of P is +5, which is highest for P.

Hence H3PO4 cannot serve as a reducing agent

Suggest Corrections

thumbs-up

4

Similar questions

Q. How many species out of the following have reducing properties?

N H_{3}, P H_{3}, H_{3} P O_{2}, H_{3} P O_{3}, H_{3} P O_{4}, L i A l H_{4}, B H_{3}

Q. Assign reason for the following:
(i)

H_{3} P O_{2}

is a stronger reducing agent than

H_{3} P O_{4}

.
(ii) Sulphur shows more tendency for catenation than Oxygen.
(iii) Reducing character increases from

H F

H I

Q. The correct order for reducing nature of

H_{3} P O_{4}, H_{3} P O_{3}

H_{3} P O_{2}

Q. The order of the oxidation state of the phosphorous atom in

H_{3} P O_{2}, H_{3} P O_{4}, H_{3} P O_{3}

H_{4} P_{2} O_{6}

Q. Explain the following:
(i) Gallium has higher ionization enthalpy than aluminum.
(ii) Boron does not exist as

B^{3 +}

ion.
(iii) Aluminum forms

[A l F_{6}]^{3 -}

ion but boron does not form

[B F_{6}]^{3 -}

P b X_{2}

is more stable than

P b X_{4}

P b^{4 +}

acts as an oxidizing agent, but

S n^{2 +}

acts as a reducing agent.
(vi) Electron gain enthalpy of chlorine is more negative as compared to fluorine.
(vii)

T I (N O_{3})_{3}

acts as an oxidizing agent.
(viii) Carbon shows catenation property but lead does not.
(ix)

B F_{3}

does not hydrolyze.
(x) Why does the element silicon, not form a graphite-like structure whereas carbon does?

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Hydrogen Peroxide

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Hydrogen Peroxide

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon