Question

Magnesium is more metallic in nature than sodium.
A. True
B. False

Answer 1

Hint:We know that the metallic character is the level of reactivity of that element as a metal. The metallic property of a metal is determined by its tendency to lose electrons. To solve this we have to determine which metal has the tendency to lose electrons easily.

Complete answer:
We know that the atomic number of Sodium is 11. Thus, the electronic configuration of sodium is as follows: $1{s^2}2{s^2}2{p^6}3{s^1}$
We know that the atomic number of Magnesium is 12. Thus, the electronic configuration of sodium is as follows: $1{s^2}2{s^2}2{p^6}3{s^2}$
From the electronic configurations of sodium and magnesium, we can see that sodium loses one electron and gains an octet configuration. And magnesium needs to lose two electrons to gain an octet configuration. Thus, the tendency to lose electrons is higher in case of sodium than that of in magnesium.
We know that the metallic property of a metal is determined by its tendency to lose electrons. The metallic property depends on the ease of removal of electrons. Thus, as sodium has a higher tendency to lose electrons, it is more metallic in nature than magnesium.
Thus, the statement ‘magnesium is more metallic in nature than sodium’ is false.

Thus, the correct option is (B) false.

Note:
We can also solve this by using the trend in reactivity of metals. The trend in reactivity of metals is that, as we go from left to right in the periodic table, the reactivity of metals decreases. We know that magnesium lies to the right side of sodium. Thus, magnesium is less metallic in nature than sodium.