Understanding the Compound
The compound in question is Ba(H2PO2)2, which consists of barium (Ba) and the hypophosphite ion (H2PO2-). It’s essential to determine the oxidation state of phosphorus (P) in this context.
Analyzing Barium
- Barium is an alkaline earth metal and typically has an oxidation state of +2 in its compounds.
- Therefore, in Ba(H2PO2)2, the contribution of two barium ions is +4.
Considering the Hypophosphite Ion
- The hypophosphite ion (H2PO2-) consists of two hydrogen atoms, one phosphorus atom, and two oxygen atoms.
- The overall charge of this ion is -1.
Calculating the Oxidation State of P
1. Assign Known Oxidation States:
- Hydrogen (H) generally has an oxidation state of +1.
- Oxygen (O) typically has an oxidation state of -2.
2. Sum of Oxidation States in H2PO2-:
- For 2 H: 2 x (+1) = +2
- For 2 O: 2 x (-2) = -4
3. Setting Up the Equation:
- Let the oxidation state of phosphorus be x.
- The equation becomes: x + 2 - 4 = -1.
4. Solving for x:
- Rearranging gives: x - 2 = -1
- Thus, x = +1.
Conclusion
- The oxidation state of phosphorus (P) in Ba(H2PO2)2 is +1.
- This conclusion is consistent with the ion's overall charge and the known oxidation states of the other elements involved.