What will be the order of decreasing nature for the given metals?
A. \[Zn > Na > Fe > Mg > Cu > Ag\]
B. \[Cu > Fe > Mg > Zn > Na > Ag\]
C. \[Ag > Cu > Fe > Zn > Mg > Na\]
D. \[Na > Mg > Zn > Fe > Cu > Ag\]

Hint: Reducing nature can be explained easily when we are familiar with the terms oxidation and reduction, the oxidation is directly referred with the loss of electron and reduction is directly referred to the gain of electrons by an atom, here reducing nature refers to the tendency of the metal to reduce another atom rather than reducing itself.

Complete step by step solution:
Now as we are familiar with the terms let’s try to solve the question, there is one more term one needs to know and that is the electrochemical series which is a series which tell us the reducing nature of any metal and based on the electrochemical series, the elements can be arranged in order of increasing as well as decreasing reducing nature for the given metals. So as a conclusion, Thus, metals with the lowest capacity to accept electrons are the one which have the most reduction in nature. And the trend states that the alkali metals are most electropositive as they have a tendency of losing one electron to attain noble gas configuration followed by alkaline earth metals, thus have most negative reduction potential and the least capacity to accept electrons or highest reducing nature.
Thus, \[Na > Mg > Zn > Fe > Cu > Ag\] is the trend where reduction potential of $C{u^{2 + }}$, $A{g^ + }$ is positive and others having a negative value of ${E_o}$.
So, the correct answer is Option D.

Note: The student can be confused about the fact that the one that reduces another atom itself undergoes oxidation and such species are referred to as reducing agent, based on the function they exhibits, and the one which oxidises another atom undergoes reduction itself and are known as oxidising agent.