Strong reducing agent in `IA` and `IIA` group elements in aqueous solutions are
`Li & Be`
`Cs and Be`
`Li & Ba`
`Cs & Ba`

Strong reductant in IIA and IA group is-

Consider the following points : (a) Cs is the strongest reducing agent is IA group element (B)" "Be(OH)_(2) is amphoteric (c ) The density of potassium is less than sodium (d) In alkali metals Li,Na,K and Rb , lithium has the minimum value of M.P. Correct statements are :

Why s-block elements act as strong reducing agents ?

How do you account for the strong reducing power of lithium in aqueous solution?

Statement-1: Lithium is the strongest reducing agent is aqueous solution. Statement-2: Lithium cannot be obtained by chemical reduction of its ore.

Alkali &alkaline earth metals have low ionisation enthalpies and hence exhibit characteristic flame colouration. They have high negative electrode potentials & hence are strong reducing agents. It dissolve in liquid ammonia to give a solution which conducts electricity and act as strong reducing agent. being stronger reducing agent than hydrogen, they are usually prepared by the electrolysis of their fused chlorides. Their oxides are basic and the basic strength increases down the group. The solubility of carbonates and sulphates of alkali and alkaline earth metals show opposite trends. only the carbonates of Li and alkaline earth metals decompose on heating. The bicarbonates of both alkali & alkaline earth metals on heating give carbonates. Which of the following process is used in the extractive metallurgy of sodium?

Why Sm^(2+) , Eu^(2+) and Yb^(2+) ions are good reducing agents , but and aqueous solution of Ce^(4+) is good oxidsing (Z=64) and Lutetium (Z= 7) are especially, stable . Why ?

The 2^(nd) group element the least density is: (A) Be (B) Mg (C) Ca (D) Ba

Account for the following statements : (i) Co (ii) is stable in aqueous solution but in the presence of strong ligands and air it can get oxidised to Co (III) (at. No Co=27) (ii) of the d^4 species Cr (II) is strongly reducing but Mn (III) is strongly oxidising (at. no Cr= 24 , Mn = 25, Co = 27)

Why Eu^(2+) and Yb^(2+) ions in solutions are good reducing agents but an aqueous solution of Ce^(4+) is a good oxidising agent?