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The S-Block Elements

Question
CBSEENCH11007141
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How will you explain the reducing character of alkaline earth metals?

Solution

Except beryllium, the alkaline earth metals have a fairly strong tendency to lose two electrons to form dipositive ions because of their low ionisation enthalpies and high negative value of standard electrode potentials. Therefore, they act as reducing agents.
The reducing character of alkaline earth metals increases as we move down the group from Be to Ba because the ionisation enthalpies increase and electrode potentials become more and more negative with increasing atomic number from Be to Ba. 

Some More Questions From The s-Block Elements Chapter

Why are alkali metals not found in nature?

Lithium shows similarities to magnesium in the chemical behaviour. What is the cause of this similarity?

What is the nature of lithium compounds?

Group 1 elements are called alkali metals. Why?

Why caesium can be used in photoelectric cell while lithium can not be?

In aqueous solution, Li+ ion has lowest mobility. Why?

Lithium has highest ionisation energy in group 1 elements, yet it is strongest reducing agent. Comment.

The softness of group 1 elements increases down the group with increasing atomic number. Give reason. 

Which is the most reactive alkali metal and why?

Why alkali metals do not form M2+ ions?

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