1. By: Racquel Cantu & Nicole Keeler(:

2. Formation of Ions *An atom that has a net positive or negative electric charge is called an ion. *An ion with a negative charge is anion. A cation is a positively charged ion.

3. Formation of Ionic Bonds *A chemical bond is the force that holds atoms or ions together as a unit. *An ionic bond is the force that holds cations and anions together.

4. Ionization Energy *The amount of energy used to remove an electron is called ionization energy. *The lower the ionization energy, the easier it is to remove an electron from an atom.

5. *A sodium atom has one more electron than a neon atom. If a sodium atom was to lose its electron, its highest occupied energy level would have eight electrons. Transfer Of Electrons

6. Example If sodium and chlorine were to combine, the sodium atoms each lose an electron, which forms cations. The chlorine atoms would all gain electrons, making anions. The ions are attracted to each other, thus forming sodium chloride. Na + Cl → Na + + Cl − → NaCl

7. Ionic Compounds * A chemical formula is a notation that shows what elements a compound contains and the ratio of the atoms or ions of the elements in the compound. * Formula of sodium chloride is NaCl.

8. Crystal Lattices *Solids whose particles are arranged in a lattice structure are called crystals. * Crystals are classified into groups based on the shape of their crystals.

9. Polar Covalent Bonds Bonds that have partly ionic, and partly covalent parts are called POLAR COVALENT BONDS.

10. Ionic compounds usually have a high melting point and they are soluble in water. Soluble means something is able to be dissolved in water.

11. Difference Between Ionic Bonds and Covalent Bonds Covalent bonds are bound because they SHARE electrons, which forms stability. Whereas Ionic bonds are bound because of the opposite attraction of the ions. Opposites attract.

12. Properties of Ionic Compounds * Properties of sodium chloride are typical of an ionic compound. *In its solid state, sodium chloride is a poor conductor of electric current. * The properties of an ionic compound can be explained by the strong attractions among ions within a crystals lattice.

13. Conductivity When molten or dissolved, ionic compounds are able to conduct electricity because of their ability to move around and carry electrons. It is not the same when they are in solid form, the electrons are packed too tightly to move around.

14. Quiz 1. Define ion: 2. What’s the difference between a cation and an anion? 3. A _______ ________ is the force that holds atoms or ions together in a unit. 4. What makes it easier to remove an electron from an atom? 5. When sodium and chlorine combine, what ionic compound do they create? 6. What is the formula for that ionic compound? 7. Define a crystal lattice: 8. What are polar covalent bonds? 9. Describe the difference between Ionic bonds and Covalent bonds: 10. What causes ionic compounds to be good conductors of electricity?

15. Answer Key 1. An atom that has a net positive or negative electric charge. 2. An anion has a negative charge, and a cation has a positive charge. 3. chemical bond 4. A lower ionization energy. 5. Sodium Chloride 6. NaCl 7. A solid whose particles are arranged in a lattice structure. 8. Bonds that have partly ionic, and partly covalent parts. 9. Covalent bonds share electrons, while Ionic bonds are attracting opposites. 10. When they become molten or dissolved.

16. Bibliography. "Ionic bond." Wikipedia. Wikipedia, 15 2012. Web. 19 Nov 2012..