What is the correct order of metallic character of the following metals?

Correct option is D

The correct answer is (d) Mg < Na < Ba < Cs.

Explanation:

The metallic character of an element refers to its ability to lose electrons and form positive ions (cations). It depends on the atomic structure and position in the periodic table. The metallic character increases:

• Down a group: As you move down a group in the periodic table, the number of shells increases, making the outer electrons farther from the nucleus. This results in weaker nuclear attraction, making it easier for the element to lose electrons.
• From right to left across a period: As you move from right to left across a period, the nuclear charge decreases, and the ability to lose electrons increases.

Analysis of elements:

• Cesium (Cs): It belongs to Group 1 (alkali metals) and is located at the bottom of the group. It has the highest metallic character among the given elements.
• Barium (Ba): It belongs to Group 2 (alkaline earth metals) and is below magnesium in the periodic table, giving it higher metallic character than Mg but lower than Cs.
• Sodium (Na): It is also in Group 1, but above cesium, meaning it has a lower metallic character than Cs but higher than Mg.
• Magnesium (Mg): It belongs to Group 2 and is above barium, meaning it has the lowest metallic character among the given elements.

Thus, the correct order of metallic character is Mg < Na < Ba < Cs.