Question

Combination of phosphorus and oxygen is an example of
A) Oxidation.
B) Reduction.
C) Rancidity.
D) None of these.

Answer 1

Hint: We know that the oxidation is defined as a loss of electrons and increase in oxidation number. When all is said in done the oxidation of natural mixes is viewed as the response where oxygen is added to the atom or hydrogen is eliminated from the particle.

Complete step by step solution:
The reaction between phosphorus and oxygen is a case of oxidation reactions.
We have to know that the oxidation reactions are extraordinary kinds of reactions where one reactant is being oxidized by another reactant similarly, in the reactions of phosphorus and oxygen, the phosphorus is oxidized by the oxygen and produces a vaporous substance which is phosphorus pentoxide.
Compound reactions:
\[P + {O_2} \to {P_2}{O_5}\]
Therefore, the option A is correct.
As we know that the reduction is an opposite process of oxidation. If the electrons are accepted by a molecule, atom or ion then it is called reduction it occurs when the oxidation state of the species is decreased.
Therefore, option B is incorrect.
We have to remember that rancidity is an extremely broad term and in its most broad significance, it alludes to the waste of a food so that it gets unfortunate (and generally risky) for utilization. At the point when individuals state that a food has "turned sour," what they're generally discussing is rancidity.
Therefore, the option C is incorrect.
Hence, option (A) is our final answer.

Note: If an element or a compound loses an electron to an electron recipient in a redox chemical reaction it is called a reducing agent. Thus, the reducing agent is the one which oxidized in a reaction. Reducing agent reduces the oxidizing agent.
Consider the reaction,
$Pb\left( s \right) + Pb{O_2}\left( s \right) + 2{H_2}S{O_4}\left( {aq} \right) \to 2PbS{O_4}\left( s \right) + 2{H_2}O\left( l \right)$
In the above reaction, the oxidation state of lead$\left( {Pb} \right)$ is zero and the oxidation state of lead in $\left( {Pb{O_2}} \right)$ is $ + 4$ and the oxidation state of lead in $\left( {PbS{O_4}} \right)$is$ + 2$. Therefore, lead is the oxidized species and lead oxide is the reduced species.