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In the acidic medium, hydrogen peroxide changes Cr2O72- to CrO5, which has two (-O-O-) bonds. The oxidation state of Cr in CrO5 is
- a)+1
- b)+3
- c)+6
- d)-5
Correct answer is option 'C'. Can you explain this answer?
Most Upvoted Answer
In the acidic medium, hydrogen peroxide changes Cr2O72-to CrO5, which ...
This option is correct because CrO5 has a butterfly structure having two peroxo bonds as shown below:
In the peroxo bonds, the oxidation state of each oxygen is -1. Now, let the oxidation state of Cr in CrO5 be x.
Therefore, x + 4(-1) + 1(-2) = 0
x = +6
In the peroxo bonds, the oxidation state of each oxygen is -1. Now, let the oxidation state of Cr in CrO5 be x.
Therefore, x + 4(-1) + 1(-2) = 0
x = +6
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Community Answer
In the acidic medium, hydrogen peroxide changes Cr2O72-to CrO5, which ...
Explanation:
The given reaction is:
Cr2O72- + H2O2 → CrO5 + H2O
In this reaction, hydrogen peroxide acts as an oxidizing agent and converts dichromate ion to chromium trioxide.
Step 1: Oxidation of Cr2O72- to CrO42-
Cr2O72- + H2O2 → 2CrO42- + 2H+ + O2
In this step, hydrogen peroxide oxidizes the dichromate ion to chromate ion by adding two oxygen atoms.
Step 2: Formation of CrO5
2CrO42- + 2H+ → Cr2O72- + H2O
In this step, the chromate ions formed in step 1 react with hydrogen ions to form dichromate ions.
Cr2O72- → CrO5 + H2O
In this step, the dichromate ion loses one oxygen atom to form chromium trioxide (CrO5).
The oxidation state of chromium in CrO5 can be calculated as follows:
Let x be the oxidation state of chromium in CrO5.
The total oxidation state of oxygen atoms in CrO5 is -10 (since there are two (-O-O-) bonds).
Therefore, the total oxidation state of chromium and oxygen in CrO5 is:
x + (-10) = 0
x = +10
Hence, the oxidation state of chromium in CrO5 is +6.
Therefore, option (c) is the correct answer.
The given reaction is:
Cr2O72- + H2O2 → CrO5 + H2O
In this reaction, hydrogen peroxide acts as an oxidizing agent and converts dichromate ion to chromium trioxide.
Step 1: Oxidation of Cr2O72- to CrO42-
Cr2O72- + H2O2 → 2CrO42- + 2H+ + O2
In this step, hydrogen peroxide oxidizes the dichromate ion to chromate ion by adding two oxygen atoms.
Step 2: Formation of CrO5
2CrO42- + 2H+ → Cr2O72- + H2O
In this step, the chromate ions formed in step 1 react with hydrogen ions to form dichromate ions.
Cr2O72- → CrO5 + H2O
In this step, the dichromate ion loses one oxygen atom to form chromium trioxide (CrO5).
The oxidation state of chromium in CrO5 can be calculated as follows:
Let x be the oxidation state of chromium in CrO5.
The total oxidation state of oxygen atoms in CrO5 is -10 (since there are two (-O-O-) bonds).
Therefore, the total oxidation state of chromium and oxygen in CrO5 is:
x + (-10) = 0
x = +10
Hence, the oxidation state of chromium in CrO5 is +6.
Therefore, option (c) is the correct answer.
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In the acidic medium, hydrogen peroxide changes Cr2O72-to CrO5, which has two (-O-O-) bonds. The oxidation state of Cr in CrO5isa)+1b)+3c)+6d)-5Correct answer is option 'C'. Can you explain this answer?
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