Draw the Lewis Symbol for the Most Common Ion That Can Be Formed from Each of the Following Atoms: Na, Mg, Al, Si, P, S, Cl, Ar

To draw the Lewis symbols for the most common ions formed from the elements listed, we first need to identify the charge of the ions each element typically forms.

• Na (Sodium): Sodium is an alkali metal that loses one electron to form a Na⁺ ion. The Lewis symbol is Na with no dots around it, indicating it has lost its one valence electron.
• Mg (Magnesium): Magnesium, an alkaline earth metal, tends to lose two electrons to form a Mg²⁺ ion. The Lewis symbol for magnesium has no dots, showing both valence electrons have been removed.
• Al (Aluminum): Aluminum typically loses three electrons, resulting in an Al³⁺ ion. Like sodium and magnesium, its Lewis symbol shows no dots, indicating the loss of all three valence electrons.
• Si (Silicon): Silicon usually forms a negative ion (Si^4-) by gaining four electrons. Its Lewis symbol displays four dots around Si, representing these valence electrons.
• P (Phosphorus): Phosphorus commonly gains three electrons to become a P^3- ion. Its Lewis symbol has three dots, showing the three additional electrons gained.
• S (Sulfur): Sulfur can gain two electrons to form S^2-. The Lewis symbol shows six dots, representing its six valence electrons before gaining two more.
• Cl (Chlorine): Chlorine typically gains one electron to form a Cl^– ion. Its Lewis symbol has seven dots surrounding Cl, indicating the gain of one additional electron.
• Ar (Argon): Argon is a noble gas and does not typically form ions. Its Lewis symbol shows full valence shells with eight dots grouping around it, indicating stability.

In summary, the Lewis symbols effectively illustrate the ion formation and electron transfer of each element in relation to its common ionic state.