Elements on the far left of the periodic table tend to form cations while elements on the far right tend to form anions Explain why this trend occurs?

Answer 1

Elements on the far left of the Periodic Table need to lose electrons when they ionize, giving them a positive net charge. Conversely, elements on the far right usually gain electrons with the negative charge acquired making them anions.

Answer 2

Because those elements on the left, metals, have weak electronegativity and donate their valance electrons to the elements on the right, nonmetals, which accept the electrons into their valance shells.

Answer 3

On the far left of the periodic table, the elements have one or two electrons more than the stable noble gas configuration, so it is energetically more favorable to lose electrons and hence become cations.

On the far right, the elements have one or two electrons less than the stable noble gas, so it is energetically more favorable to gain electrons and hence become anions.

Answer 4

Elements on the far left of the periodic table have fewer electrons in their outermost shell, so they tend to lose these electrons to achieve a more stable electron configuration, forming cations. In contrast, elements on the far right of the periodic table have more electrons in their outermost shell, making it easier for them to gain electrons to achieve a full outer shell, forming anions. This trend is based on the tendency of atoms to attain a stable electron configuration similar to that of noble gases.