Question

Alkali metals have high oxidation potential and hence they behave as: (a) Electrolytes (b) Lewis bases (c) Oxidizing agents (d) Reducing agents

Short answer

Alkali metals behave as reducing agents.

Step-by-step solution

Understand Alkali Metals

Alkali metals are elements in Group 1 of the periodic table. They include lithium, sodium, potassium, etc. These metals are characterized by having a single electron in their outermost shell, which they can lose easily.

Define Oxidation Potential

Oxidation potential refers to the tendency of an element to lose electrons and undergo oxidation. Alkali metals have high oxidation potential, meaning they easily lose their outer shell electron.

Explore Behavior as Reducing Agents

A reducing agent is a substance that loses electrons and in doing so, reduces another substance. Since alkali metals easily lose their electrons due to their high oxidation potential, they act as reducing agents.

Evaluate Each Option

- (a) Electrolytes: Substances that conduct electricity when dissolved in water — not directly related to individual alkali metal capabilities. - (b) Lewis bases: Electron pair donors — not applicable for metals losing electrons. - (c) Oxidizing agents: Gain electrons — opposite of alkali metals' behavior. - (d) Reducing agents: Lose electrons — fits alkali metals' high oxidation potential.

Key concepts

Oxidation Potential

Oxidation potential is an important concept in understanding the chemical behavior of elements, particularly metals like those in the alkali group. This potential represents how easily an element can lose electrons, undergoing oxidation in the process. When a substance has a high oxidation potential, it readily gives up its electrons.
Alkali metals, such as lithium, sodium, and potassium, are known for their exceptionally high oxidation potential. They have a single electron in their outermost shell. This makes it energetically favorable for them to lose this electron.
Due to this feature, alkali metals are highly reactive, especially in the presence of non-metals like halogens. Their inclination to lose electrons determines much of their chemistry and their role in various chemical reactions.

Reducing Agents

Reducing agents are substances that lose electrons during a chemical reaction. By losing electrons, they facilitate the reduction of another substance by donating the electrons they lose.
Alkali metals are prime examples of strong reducing agents. This characteristic stems from their high oxidation potential, which allows them to easily shed electrons and transfer them to other atoms or molecules.
This electron donation is critical in many chemical processes, such as in batteries where alkali metals help in reactions that generate electricity.

• When an alkali metal acts as a reducing agent, it becomes oxidized.
• This electron loss results in the formation of positive ions, which is a key step in the reduction-oxidation (redox) process.

Periodic Table Group 1

Group 1 of the periodic table comprises the alkali metals, famously known for their distinct properties and reactivity.
This group includes the elements lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). These metals are all characterized by having a single electron in their outer shell.
Their placement in the periodic table is strategic, indicating their tendency to lose this lone outer electron easily. As a result, they form cations with a charge of +1 after shedding the electron.

• Alkali metals are soft and can often be cut with a knife.
• They have low melting points and are highly reactive, especially with water, often producing hydrogen gas upon reaction.

Their ability to easily lose their outer electron makes them integral in many everyday applications, including in the production of salts and various compounds.