In which group can you find elements that form compounds with a tendency to lose electrons?

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The correct answer is metals because these elements are characterized by their tendency to lose electrons during chemical reactions, which allows them to form positive ions or cations. This behavior is primarily attributed to their low electronegativity and the fewer electrons in their outermost shell, making it energetically favorable for them to lose electrons and achieve a noble gas electron configuration.

Metals are located on the left side and in the center of the periodic table and include groups such as alkali metals and alkaline earth metals, both of which readily lose their outer electrons. Examples include sodium, which loses one electron to form Na⁺, and magnesium, which loses two electrons to form Mg²⁺.

The other groups mentioned, such as nonmetals, metalloids, and inner transition metals, do not typically exhibit the same strong tendency to lose electrons as metals do. Nonmetals, for instance, are more likely to gain or share electrons to achieve stability, while metalloids have properties that are intermediate between metals and nonmetals. Inner transition metals, while they can lose electrons, are more complex in their behavior and generally do not exhibit the straightforward electron loss characteristic of metals.

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