Define electropositivity?

Electropositivity is the tendency of an atom to lose electrons and form a positive ion.

An electropositive element gives up electrons easily during chemical reactions. When an atom loses electrons, it becomes a cation. Metals are usually electropositive, which is why metals form ionic compounds with nonmetals.

Trends in the periodic table

• Down a group: Electropositivity increases. Atomic size grows, the outer electron is farther from the nucleus, and shielding increases. Loss of electrons becomes easier.
• Across a period (left to right): Electropositivity decreases. Nuclear charge increases and holds electrons more strongly, so atoms prefer to gain or share rather than lose.
• Most electropositive: Alkali metals and alkaline earth metals. Francium and cesium are at the top in reactivity, but francium is rare and radioactive.

How it shows up in reactions

• Ionic bonding: Highly electropositive metals like Na, K, Ca transfer electrons to electronegative elements like Cl, O, S.
• Reducing nature: Electropositive elements are strong reducing agents, as they donate electrons.
• Oxides and hydroxides: Electropositive metals form basic oxides and hydroxides (e.g., Na₂O, Ca(OH)₂).

Comparison with electronegativity