The question asks why sodium metal is oxidized in the given reaction. Oxidation is defined as the loss of electrons, an increase in oxidation state, or the gain of oxygen. In this specific reaction, we need to analyze the electron transfer for sodium.
Correct Option: D) Loses one electron to form Na+
The question asks to identify why chlorine atoms are reduced in the given reaction. Reduction is defined as the gain of electrons, a decrease in oxidation state, or the gain of hydrogen. In this specific reaction, we need to analyze the electron transfer for chlorine.
A) Gains one electron to form Cl- — This is correct because reduction is the gain of electrons, and in the reaction, each chlorine atom goes from an oxidation state of 0 to -1, indicating it has gained one electron to become a chloride ion (\(\text{Cl}^-\)).
The question asks to identify the two half-reactions that constitute a redox reaction. A redox reaction involves the transfer of electrons, which means one species loses electrons and another gains them. We need to recall the definitions of these processes.
Correct Option: D) Oxidation half-reaction and reduction half-reaction
Redox reactions involve the transfer of electrons. Oxidation is defined as the loss of electrons, and reduction is defined as the gain of electrons. The fundamental principle of conservation of charge dictates the relationship between these two processes.
Correct Option: A) Exactly equal to the total number of electrons gained during reduction. This is a fundamental principle of redox chemistry and the conservation of charge. Electrons are transferred, not created or destroyed.
The question asks to identify the role of Zn(s) in the given half-reaction. This requires understanding the definitions of oxidation, reduction, oxidizing agents, and reducing agents in terms of electron transfer.
B) Reducing agent, since it loses electrons and is itself oxidised. This statement correctly identifies Zn(s) as a reducing agent because it loses electrons (undergoes oxidation) in the given half-reaction.
This question tests the understanding of fundamental concepts in redox reactions: oxidation, reduction, oxidising agents, and reducing agents. We need to define each term and relate it to the species involved in electron transfer.
Correct Option: A) Oxidising agent (oxidant)
The definition provided in the question perfectly matches that of an oxidising agent. An oxidising agent facilitates the oxidation of another species by accepting electrons from it, and in doing so, the oxidising agent itself gets reduced (gains electrons).