Final answer:
Group 2 elements become stable by losing their two valence electrons, thereby achieving the stable electron configuration of the nearest noble gas and forming divalent cations with a +2 charge.
Step-by-step explanation:
The question pertains to the behavior of Group 2 elements, which have two valence electrons. To achieve a full valence shell and become more stable (or 'happier'), these elements tend to lose their two valence electrons to form divalent cations (+2 charge). The loss of electrons leads to a stable electron configuration, resembling the nearest noble gas with an octet of electrons in the outermost shell. This is because Group 2 elements have s2 as their outer electron configuration, and by losing two electrons, they attain a noble gas electron configuration.
For example, magnesium (Mg), which is a Group 2 element, will lose two electrons to become Mg2+, achieving the same electron configuration as neon (Ne), the nearest noble gas. Although Group 2 elements require more energy for electron removal compared to Group 1 elements due to the need to remove two electrons instead of one, they are still reactive enough that they do not exist in their elemental form in nature, but instead are found as compounds.