1. Ionic Bonds and Compounds

2. The Octet Rule The Octet rule states that elements gain or lose electrons to attain an electron configuration of the nearest noble gas Noble gases are the most stable elements because they have a full valence electron shell ALL ELEMENTS WANT TO BE STABLE LIKE THE NOBLE GASES That is why there are ions, if an element gives up or gains electrons it has a better chance of being stable like a noble gas!

3. Ions Cations are positive ions formed by removal of electrons from metallic atoms – If an atom is metallic it means it is a metal Anions are negative ions formed by gaining of electrons by nonmetallic – If an atom is nonmetallic it means it is a nonmetal **remember** – metals are more willing to give up their electrons and non-metals are more willing to gain electrons

4. Ionic Bonds Atoms transfer their electrons to other atoms to become more stable, this type of bond is known as an Ionic bond An ionic bond is the attraction between two oppositely charged ions (cation and anion) When two ions come together, the opposite charges cancel out In Ionic bonds, Electrons tend to transfer from the cation to the anion

5. Ionic Bonds and Lewis Dot To show an ionic bond through Lewis Dot structures you need to follow these steps: let’s try it sodium and Chlorine! – 1) write the symbol for each element side by side Na Cl

6. Ionic Bonds and Lewis Dot To show an ionic bond through Lewis Dot structures you need to follow these steps: – 1) write the symbol for each element side by side – 2) draw the Lewis dot structure for each element Na Cl

7. Ionic Bonds and Lewis Dot To show an ionic bond through Lewis Dot structures you need to follow these steps: – 1) write the symbol for each element side by side – 2) draw the Lewis dot structure for each element – 3) draw an arrow showing the transfer of electrons from the cation to the anion Na Cl

8. Ionic Bonds and Lewis Dot To show an ionic bond through Lewis Dot structures you need to follow these steps: – 1) write the symbol for each element side by side – 2) draw the Lewis dot structure for each element – 3) draw an arrow showing the transfer of electrons from the cation to the anion Na Cl

9. Let’s practice! Magnesium and Oxygen

10. Let’s Practice! Lithium and Fluorine

11. Let’s practice! Calcium and Sulfur

12. Let’s practice! Potassium and Bromine

13. Let’s practice! Hydrogen and Fluorine

14. Let’s practice! Sodium and Iodine