Question
Question: Tendency to lose electrons shows the reducing property of the element. Which of the following orders...
Tendency to lose electrons shows the reducing property of the element. Which of the following orders is/are correct in terms of reducing property of the element?
This question has multiple correct options.
A.Na<K<Rb
B.Na>Mg>Al
C.F−<Cl−<Br−<I−
D.Mg<Ca<Sr
Solution
We have that when an molecule, an ion (or) an atom loses electrons, then such a reaction is known as oxidation reaction and when an atom, an ion, (or) a molecule gains electrons, then we call such a reaction as reduction reaction. The other name of oxidation reaction is de-electronation and the other name of reduction reaction is electronation.
Complete answer:
We can say that when a substance forces another substance to gain electrons, it undergoes oxidation by donating electrons, and the substance which donates electrons is known as a reducing agent. It is a donor of electrons.
We can say that when a substance forces another substance to lose electrons, it undergoes reduction by gaining electrons, and the substance which gains electrons is known as oxidizing agent. It is an acceptor of electrons.
The ability of an element to donate electrons is known as reducing property and by this property, the substance goes through the oxidation process. The ability of an element to gain electrons is known as oxidizing property and by this property, the substance goes through a reduction process.
For Na<K<Rb, when we move down the group, there is an increase in electropositive character and increase in reducing character. So, Option (A) is correct.
For Na>Mg>Al, when we move from left to right across a period, there is a decrease in electropositive character and decrease in reducing property. So, Option (B) is correct.
For F−<Cl−<Br−<I−, when there is an increase in halide ion size, there is an increase in electropositive character and increase in reducing character. So, Option (C) is correct.
For Mg<Ca<Sr, when we move down the group, there is an increase in electropositive character and increase in reducing character. So, Option (B) is correct.
All the options are correct.
Note:
We have to know that some of the factors that affect the oxidizing and reducing properties are ionization potential, atomic size, metallic and non-metallic nature, the number of outermost electrons, electropositivity (or) electronegativity.