Phosphorus can have several different oxidation numbers ranging in value from -3 to +5. (a) When phosphorus burns in air or oxygen, it yields either tetraphosphorus hexoxide or tetraphosphorus decoxide. Write the formula and give the oxidation number for each compound.

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Identify the chemical formulas for tetraphosphorus hexoxide and tetraphosphorus decoxide.

For tetraphosphorus hexoxide, the formula is \( \text{P}_4\text{O}_6 \).

For tetraphosphorus decoxide, the formula is \( \text{P}_4\text{O}_{10} \).

Calculate the oxidation number of phosphorus in \( \text{P}_4\text{O}_6 \) by setting up the equation: \( 4x + 6(-2) = 0 \), where \( x \) is the oxidation number of phosphorus.

Calculate the oxidation number of phosphorus in \( \text{P}_4\text{O}_{10} \) by setting up the equation: \( 4x + 10(-2) = 0 \), where \( x \) is the oxidation number of phosphorus.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Oxidation Numbers

Oxidation numbers are a way to keep track of electrons in chemical compounds. They indicate the degree of oxidation of an atom in a molecule, helping to determine how many electrons are lost or gained during a reaction. For phosphorus, common oxidation states include -3, 0, +3, and +5, which reflect its ability to either gain or lose electrons.

Phosphorus Oxides

Phosphorus can form several oxides, with tetraphosphorus hexoxide (P4O6) and tetraphosphorus decoxide (P4O10) being two notable examples. The former contains phosphorus in the +3 oxidation state, while the latter has phosphorus in the +5 oxidation state. Understanding these compounds is essential for recognizing how phosphorus interacts with oxygen.

Combustion Reactions

Combustion reactions involve the reaction of a substance with oxygen, typically producing heat and light. In the case of phosphorus, burning in air or oxygen leads to the formation of phosphorus oxides. Recognizing the products of combustion and their corresponding oxidation states is crucial for predicting the outcomes of such reactions.

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