Elements that are most likely to give up electrons rather than share them are those located on the left side of the periodic table, specifically in Groups 1 and 2, also known as the alkali metals and alkaline earth metals, respectively.

Here's why:

* Low electronegativity: These elements have low electronegativity, meaning they have a weak attraction for electrons. This makes them willing to lose electrons to achieve a stable electron configuration.

* One or two valence electrons: They have only one or two valence electrons in their outermost shell. Losing these electrons allows them to achieve a stable, noble gas configuration.

Example:

* Sodium (Na) has one valence electron. It readily loses this electron to form a +1 ion (Na+), achieving the stable electron configuration of neon (Ne).

While sharing electrons is a common way for elements to achieve stability, elements in Groups 1 and 2 are more inclined to lose electrons to form cations rather than share electrons to form covalent bonds.