In the Periodic Table, why does Group 2 and 17 bond together so easily?
~thanks
Group 2 elements want to lose electrons. Group 17 elements want to gain electrons. Voila! A perfect match.
Group 2 elements in the Periodic Table, also known as the alkaline earth metals, and Group 17 elements, known as the halogens, tend to bond together easily due to their specific electronic configurations.
To understand why they readily bond, you need to look at their electron configurations. Group 2 elements have two valence electrons in their outermost energy level, while Group 17 elements have seven valence electrons in their outermost energy level.
The electronic configurations of these groups provide them with a strong driving force to bond together and form compounds. Group 2 elements want to lose their two outermost electrons to achieve a stable, full electron configuration. By doing so, they will have the same electronic configuration as a noble gas, which is highly stable.
On the other hand, Group 17 elements want to gain one electron to complete their outermost energy level and achieve a stable configuration. By gaining one electron, they will also have the same electronic configuration as a noble gas.
Thus, when a Group 2 element reacts with a Group 17 element, the Group 2 element donates its two valence electrons to the Group 17 element, resulting in both achieving a stable electron configuration. This type of bond formation is known as an ionic bond, where one element gives electrons (becomes a cation) and the other element accepts electrons (becomes an anion).
Overall, the strong drive of Group 2 elements to donate their two valence electrons and the strong drive of Group 17 elements to gain one electron make them highly reactive and allow them to bond together easily.