Question

Alkaline earth metals are denser than alkali metals because metallic bonding is
A. Stronger
B. Weaker
C. Not present
D. Volatile

Answer 1

Hint: A bond that functions in holding together many atoms of metals in a metallic substance is termed a metallic bond. The electrons responsible to form a metallic bond are valence electrons.

Complete Step by Step Answer:
Let's first understand alkali metals. In the periodic table, these types of metal occupy the position in group 1 . Their valence shell electronic configuration is \[n{s^1}\]. Some examples of alkali metals are Sodium, Lithium, etc.

Now, we will discuss alkaline earth metals. In the periodic table, these types of metals occupy the position in group 2 Their outermost shell configuration is \[n{s^2}\]. Some examples are magnesium, berrylium etc.

Now, we will discuss the formation of metallic bonds in detail. The outermost electrons are detached from the metal atom and overlap with the metal's neighboring atoms. Therefore, the electrons that form metallic bonds have the nature of non-localized and they can move freely in the crystal.

And as we know, alkaline earth metals possess one more valence electron than alkali metals. Therefore, the metallic bonding is stronger in the alkali earth metals than in alkali metals. So, the density of the former is more than the latter.
Hence, option A is right.

Note: There are many factors that affect the strength of a metallic bond. They are the number of electrons that undergo delocalization from the metal, the charge, and the size of a metallic atom. The metallic bonding is very strong in nature.