Question:
P\(_4\) \(\rightarrow\) PH\(_3\) + H\(_2\)PO\(_2\)
Oxidation state of phosphorus change from -------- to -------- respectively.
P\(_4\) \(\rightarrow\) PH\(_3\) + H\(_2\)PO\(_2\)
Oxidation state of phosphorus change from -------- to -------- respectively.
Oxidation state of phosphorus change from -------- to -------- respectively.
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In redox reactions, the oxidation state of elements changes. Remember that a decrease in oxidation state indicates reduction, while an increase indicates oxidation.
Updated On: Apr 18, 2026
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Solution and Explanation
Step 1: Determine the oxidation state of phosphorus in P\(_4\).
In P\(_4\), phosphorus is in its elemental form, and thus its oxidation state is 0.
Step 2: Determine the oxidation state of phosphorus in PH\(_3\).
In PH\(_3\), hydrogen has an oxidation state of +1, so for the molecule to be neutral, phosphorus must have an oxidation state of -3.
Step 3: Determine the oxidation state of phosphorus in H\(_2\)PO\(_2\).
In H\(_2\)PO\(_2\), hydrogen has an oxidation state of +1, and oxygen has an oxidation state of -2. For the molecule to be neutral, phosphorus must have an oxidation state of +1.
Step 4: Conclusion.
Therefore, the oxidation state of phosphorus changes from 0 in P\(_4\) to -3 in PH\(_3\), and then from -3 to +1 in H\(_2\)PO\(_2\).
In P\(_4\), phosphorus is in its elemental form, and thus its oxidation state is 0.
Step 2: Determine the oxidation state of phosphorus in PH\(_3\).
In PH\(_3\), hydrogen has an oxidation state of +1, so for the molecule to be neutral, phosphorus must have an oxidation state of -3.
Step 3: Determine the oxidation state of phosphorus in H\(_2\)PO\(_2\).
In H\(_2\)PO\(_2\), hydrogen has an oxidation state of +1, and oxygen has an oxidation state of -2. For the molecule to be neutral, phosphorus must have an oxidation state of +1.
Step 4: Conclusion.
Therefore, the oxidation state of phosphorus changes from 0 in P\(_4\) to -3 in PH\(_3\), and then from -3 to +1 in H\(_2\)PO\(_2\).
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