* Electron Configuration: Alkali metals have one valence electron in their outermost shell, making them eager to lose that electron to achieve a stable noble gas configuration. Alkaline earth metals have two valence electrons.
* Ionization Energy: Alkali metals have lower ionization energies than alkaline earth metals. This means it takes less energy to remove an electron from an alkali metal atom, making them more likely to participate in reactions.
* Electropositivity: Alkali metals are more electropositive (meaning they tend to lose electrons) than alkaline earth metals.
In summary: Alkali metals are more reactive because they are easier to ionize and readily lose their single valence electron to form stable cations.
Example:
Sodium (Na), an alkali metal, reacts vigorously with water, producing hydrogen gas and sodium hydroxide. Calcium (Ca), an alkaline earth metal, reacts with water but at a slower rate.
