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For each element, tell how it will fill its outer shell and become stable in an ionic bond. (Remember: Metals will lose all their valence electrons to have the next available outermost energy level full. Nonmetals will gain valence electrons to fill the outermost energy level with 8 valence electrons)


Sulfur (S) a nonmetal in Group 6A ________.


Potassium (K) a metal in Group 1A _________.

Chlorine (Cl) a nonmetal in Group 7A ___________.

Phosphorus (P) a nonmetal in Group 5A ____________.


Aluminum (Al) a metal in Group 3A ______________.

Magnesium (Mg) a metal in Group 2A ____________.

Choices:

It will gain 3 electrons to fill its outer shell.

It will gain 1 electron to fill its outer shell.

It will lose 1 valence electron.

It will lose 2 valence electrons.

It will gain 2 electrons to fill its outer shell.

It will lose 3 valence electrons.

choose the correct answers

1 answer

Here's how each element will fill its outer shell and become stable in an ionic bond:

  1. Sulfur (S) a nonmetal in Group 6A: It will gain 2 electrons to fill its outer shell.

  2. Potassium (K) a metal in Group 1A: It will lose 1 valence electron.

  3. Chlorine (Cl) a nonmetal in Group 7A: It will gain 1 electron to fill its outer shell.

  4. Phosphorus (P) a nonmetal in Group 5A: It will gain 3 electrons to fill its outer shell.

  5. Aluminum (Al) a metal in Group 3A: It will lose 3 valence electrons.

  6. Magnesium (Mg) a metal in Group 2A: It will lose 2 valence electrons.

These choices accurately represent the behavior of each element to achieve a stable electron configuration through ionic bonding.