1. Introduction Chemical Bonding Ms. Armesto & Ms. Hickey

2. Class Agenda Discussion Item One – An Unlikely Combination Observing what occurs what happens when water is combined with vegetable oil Discussion Item Two – Chemical Bonding Video Discovery Education gives us insight into ionic and covalent bonding Discussion Item Three – Intro To Chemical Bonding Lecture on the vocabulary that goes with this lesson Discussion Item Four – Chemical Bonding Review Questions Working together to analyze & explain our lesson on ionic & covalent bonds 20 mins 3 mins 40 mins 30 mins

3. Introduction to Bonding Bell Ringer Your mission: Look at your glass beaker and see how many total mL this can hold. Divide that number in half and place that quantity of water and vegetable oil inside. Record the amount of mL of water & vegetable oil Write down what occurs. Be specific Brainstorm & explain WHY you think this occurred.

4. Chemical Bonding Vocabulary Start making flashcards! Chemical Bond Stability Ion Metallic Bond Covalent Bond Molecule Polar Bond Chemical Formula

5. Molecules, crystals, & gases are held together by chemical bonds An attraction of between atoms that forms compounds What’s a chemical bond? Electromagnetic force Based on the electronegativity of the element Closest to Fluorine, electronegativity increases Farthest away from Fluorine, decreases

6. Stability When an element is stable this means that is does not easily or quickly change from one state to another. Example: Platinum is an element used to make expensive jewelry. It is expensive because it stable and lasts a long time.

7. Is an atom or group of atoms that has an electric charge. Loses a valence electron, loses a negative charge. (positive ion) *Metals* Gains an electron, it gains a negative charge. (negative ion) *Nonmetals* Ions

8. When atoms that easily lose electrons react with atoms that easily gain electrons. For example: Sodium has 1 v.e. Chlorine has 7 v.e. They share their electrons so that they have 8 valence electrons and can be stable together. Ionic Bonds

9. Most metals are crystalline solids. A metal crystal is composed of closely, packed positively charged metal ions. Properties: Luster Malleability Ductility Thermal Conductivity Electrical Conductivity Able to make alloys Metallic Bonds

10. Sharing of electrons when 2 nonmetal atoms bond together to get the 8 valence electrons. Fun Fact: Covalent Bonds & Music Due to poor conductivity, your headphones are lined with plastics or rubber that prevent the electrical charge from shocking you while listening to music! Covalent Bonds

11. Is a compound like water, oxygen, and sucrose (sugar) that are considered to be molecular compounds because they are made up of covalent bonds. Ions CANNOT form molecular compounds! Molecules

12. Geckos can climb glass because of spatulae that make up the bottoms of their feet. Due to the polar bond called van der Waals forces that forms because the negative atom is attracted to the positive one. Just like Oxygen is attracted to Hydrogen to form water. Polar Bonds

13. Is a group of symbols that show the ratio of elements in a compound. Magnesium Chloride’s chemical formula is MgCl2 1 magnesium ion for every 2 ions of chloride Fun Fact: Coral reefs make calcium carbonate, which helps protect them. When the coral dies, its calcium carbonate shell remains and adds structure to the reef. Chemical Formulas

14. Chemical Bonding Review Questions 1.An atom or group of atoms that has an electric charge is called 2. How does the gaining and losing of electrons affect the atom differently? 3. What are the 3 properties of ionic compounds? 4. What 3 dimensional arrangement do ionic bonds result in? 5. How are electrons shared in a nonpolar covalent bond? 6. How can a molecule be nonpolar overall & still contain polar bonds? 7. When you laundry what causes nonpolar oil or greasy dirt to mix with the polar water?