Question

Why do alkali metals act as strong reducing agents?

Answer 1

Hint- In order to solve this problem, we will briefly understand the process of reduction. Then we will check for the chemical properties required for the elements to be a reducing agent and finally we will check for the properties of alkali metals due to which it is a reducing agent.

Complete answer:
Reduction is the process of gaining of electrons. A substance which donates or gives electrons is a good reducing agent.
If an element has 1, 2 or 3 electrons in its outer shell then it has a tendency to donate electrons so that it can expose the completely filled inner shell and thus achieve a stable octet configuration. Such elements are called metals.
Alkali metals are very electropositive. With one electron in the outer shell, they have a high potential to donate this electron to another element, and become an ion with a very stable electron configuration like the neighboring (on the periodic table) inert or “noble” gas.
That places them near or at the top of the “electromotive series”, and they are more active than common metals. In the right environment,
An alkali metal, such as sodium or potassium, will donate an electron to a copper ion, or a zinc ion, etc., reducing it to the free state, and in the process the alkali metal is oxidized and enters the solution.

Hence, due to these reasons alkali metals act as strong reducing agents.

Note- Reducing agent is an element or compound that loses an electron to an electron recipient in a redox chemical reaction. Therefore a reduction agent is oxidized as electrons are lost in the redox reaction. Reducing agents "reduce" oxidizing agents. Oxidizers "oxidize" reducers. Lithium metal is the strongest Reducing agent amongst all the metals because of the lowest standard reduction potential of the lithium metal. And fluorine is the strongest oxidizing agent amongst all.