Question

Review the concept of electronegativity in the textbook, and rank these elements from the weakest to strongest reducing agent: (a) nitrogen, N: (b) silicon, Si: (c)fluorine, F. Rank from weakest to strongest. To rank items as equivalent, overlap them.

Answer 1

Ranking these elements from the weakest to strongest reducing agent: (a) silicon, Si; (b) nitrogen, N; (c) fluorine, F.

Step-by-step explanation:

Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. In the context of redox reactions, reducing agents are substances that tend to lose electrons. Elements with lower electronegativity are generally better at losing electrons and are stronger reducing agents.

Silicon (Si) has a lower electronegativity compared to nitrogen (N) and fluorine (F). As we move from left to right across a period in the periodic table, electronegativity generally increases. Silicon, being a metalloid, is less electronegative than nitrogen and fluorine.

Nitrogen (N) has a higher electronegativity than silicon but lower than fluorine. Nitrogen is more likely to act as a reducing agent compared to fluorine.

Fluorine (F) has the highest electronegativity among the three elements. It strongly attracts electrons, making it a poor reducing agent. In fact, fluorine is more likely to gain electrons and act as an oxidizing agent in redox reactions.

Therefore, based on their electronegativities, silicon is the weakest reducing agent, followed by nitrogen, and fluorine is the strongest reducing agent among the given elements.