Final answer:
Elements that seek to get rid of valence electrons are typically metals, especially those in groups 1 and 2 of the periodic table, such as alkali and alkaline earth metals. These elements tend to lose electrons to form cations and achieve a stable electron configuration similar to that of the noble gases.
Step-by-step explanation:
The type of elements that seek to get rid of valence electrons are generally the metals, particularly the alkali metals and alkaline earth metals found in groups 1 and 2 of the periodic table. These elements have 1-3 electrons in their valence shell and will tend to donate their electrons to other atoms until they attain a full outer shell, which results in the formation of positively charged ions, or cations. This behavior is due to the fact that valence electrons in these elements are easier to remove as they are shielded more and are farthest from the nucleus, possessing the highest energies. Ionization energies tend to increase across the periodic table from left to right, with lower values on the left side indicating that it is easier for these elements to lose electrons, a trend that is crucial in the formation of chemical compounds.
For example, sodium (Na), an alkali metal, readily loses one electron to become Na+, thus achieving the electron configuration of the nearest noble gas, neon. The transition metals follow a different rule, where they lose the ns electrons before losing the (n-1)d electrons, despite the order prescribed by the Aufbau principle. Understanding the periodic trend of valence electrons offers insight into the reactive behavior of the elements and their common oxidation states.