why are most elements on the periodic table found as compound in nature?

Most elements on the periodic table are found as compounds in nature due to their reactivity and tendency to form chemical bonds with other elements. The formation of compounds is a result of the desire of atoms to achieve a stable and balanced electron configuration in their outermost energy level, also known as the valence shell.

The valence electrons are the outermost electrons of an atom, and they play a crucial role in determining the chemical properties of an element. Atoms with incomplete valence shells are generally more reactive, as they strive to either gain or lose electrons to achieve a stable electron configuration, similar to the noble gases.

Compounds are formed when two or more atoms chemically bond together by sharing or transferring electrons. This enables them to achieve a more stable electron configuration by either filling their valence shells or achieving a noble gas-like configuration.

Additionally, some elements are highly reactive due to their smaller atomic size or their electronegativity. For example, alkali metals like sodium and potassium are highly reactive and readily form compounds with other elements to achieve a stable electron configuration.

In nature, elements are often found in combination with other elements or compounds because the compounds formed are more stable and have lower energy states compared to isolated atoms. These compounds can range from simple molecules to complex structures, such as minerals and ores.

Therefore, the tendency of most elements to be found as compounds in nature is primarily driven by their desire to achieve a stable electron configuration, leading to chemical bonding with other elements.