Question
Describe the reducing nature of group $1$ and group $2$ elements.
✓
Answer
The reducing power of an element is measured in terms of standard electrode potential $(E^0)$ corresponding to the following transformation i.e, tendency to lose electron.
$M(s)⟶M+(aq)+e−$
$i.$ Reducing nature of group $1$ elements:
All the alkali metals have high negative values of $E^0$ which indicates that they have strong reducing nature and hence, they can be used as strong reducing agents.
Lithium is the most powerful and sodium is the least powerful reducing agent in the group.
$ii.$ Reducing nature of group $2$ elements:
All the alkaline earth metals have high negative values of stanard reduction potential $(E^0)$ and are strong reducing agents.
However, reducing power of alkaline earth metals is less than that of alkali metals.
$M(s)⟶M+(aq)+e−$
$i.$ Reducing nature of group $1$ elements:
All the alkali metals have high negative values of $E^0$ which indicates that they have strong reducing nature and hence, they can be used as strong reducing agents.
Lithium is the most powerful and sodium is the least powerful reducing agent in the group.
$ii.$ Reducing nature of group $2$ elements:
All the alkaline earth metals have high negative values of stanard reduction potential $(E^0)$ and are strong reducing agents.
However, reducing power of alkaline earth metals is less than that of alkali metals.
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