Question

How do the hydrides of s-block elements act as powerful reducing agents?

Answer 1

s-block elements:

Element of s-block of the periodic table belongs to groups 1 and 2. Group 1 elements are referred to as Alkali metals ($\mathrm{Li},\mathrm{Na},\mathrm{K},\mathrm{Rb},\mathrm{Cs}\mathrm{and}\mathrm{Fr}$), while group 2 elements are Alkaline earth metals (Be, Mg, Ca, Sr, Ba, and Ra).

• Group 1 and 2 metals are electropositive and it forces the hydrogen atom to accept an electron and form ionic hydrides.
• Reducing agents are those elements that can easily release electrons.
• Elements of s-block have low values of ionization energies and are hence highly electropositive.
• Alkali metals have 1 valence electrons while alkaline earth metals have 2 valence electrons. That's the reason they have low ionization potential.
• Hence due to easy release of electrons, they are a strong reducing agent.