why alkaline earth metals have electropositive character than alkali metals?
Answers
Reason: Due to smaller size of the cation and greater number of valence electrons, the metallic bonding in alkaline earth metal is stronger as compared to alkali metal. Because of this reason ,these metals are less soft then alkali metals.
Answer:
Question
why alkaline earth metals have electropositive character than alkali metals?
Answer
Group 1 and 2 elements (the so-called alkali and alkaline earth metals, indeed) used to be termed as electropositive because of their outer electron structure.
These elements have either one (alkali) or two (alkaline earth) electrons in their outermost shells, respectively; this means that they can be easily lost to an oxidiser, thus forming stable ionic compounds in which these metals are actually present as +1 (alkali) and +2 (alkaline earth) cations.
Group 1 metal cations: Li⁺, Na⁺, K⁺, Rb⁺, Cs⁺.
Group 2 metal cations: Be²⁺, Mg²⁺, Ca²⁺, Sr²⁺, Ba²⁺.
The term electropositive (not so used anymore, as a matter of fact), refers to their willingness to lose the aforementioned electrons: the easier it is, the more electropositive a metal is.
From this point of view, the electropositivity of both groups increases on descending either group: in other words, their reactivity increases on passing from top to bottom. This happens because the principal quantum number increases from top to bottom and so does the average distance of the outermost electrons from the nucleus.
In other words, although the outermost electrons of, say, magnesium and barium are both loosely attracted to their nuclei, the latter ones feel even less attraction to the nucleus, thus rendering barium very reactive and a good reducing agent.
Explanation:
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