Question

written response
elements in different groups of the periodic table tend to form predictable ions. compare and contrast how metals and non - metals typically form ions. explain the relationship between an elements group number and the charge of its ion, providing specific examples to support your explanation.

Explanation:

Metals lose electrons to form cations (e.g., sodium \(Na\) loses one electron to form \(Na^+\)). Non - metals gain electrons to form anions (e.g., chlorine \(Cl\) gains one electron to form \(Cl^-\)). The number of electrons lost or gained is related to the element's valence electron configuration. For metals in Group 1 (like \(Na\) with one valence electron), they lose one electron. For non - metals in Group 17 (like \(Cl\) with seven valence electrons), they gain one electron to achieve a stable electron configuration (usually a full outer shell).

Answer:

Metals form cations by losing electrons (e.g., \(Na
ightarrow Na^+\)), non - metals form anions by gaining electrons (e.g., \(Cl
ightarrow Cl^-\)). The number of electrons lost/gained is based on valence electrons to achieve stability.