1. Compounds

2. Why are noble gases stable? How can other elements accomplish this?

3. What are Those? Compound – Chemically bonded atoms – Take on new properties/state – Sharing/lending of electrons – Chemical name: identifies elements of compound – Chemical formula: how many of each element in compound Ionic compounds Molecular compounds

4. Ions Uneven number of protons and electrons Positively/negatively charged atom – Give away electron: positive charge – Take electron: negative charge Represented using square brackets with charge on top right corner

5. Ionic Compounds Usually one metal and one non-metal High melting point Crystal lattice Soluble in water Solids at room temperature Conductors of electricity

6. Forming Ionic Compounds Atoms become an ion when combining – Lose/gain an electron Atoms come together by “giving” or “taking” an electron – Ionic bond

7. Draw CaCl 2

8. Naming Salts Name the metal ion first. The name of the metal ion is the same as the element name. If the element can form an ion in more than one way (multivalent elements), include a Roman numeral in brackets after the element to indicate the charge Name the non-metal ion second. The non- metal changes the ending to “ide” Combine the names of the metal and non- metal together

9. Name the following MgO BaF 2 NaF KI MgCl 2 CuS FeP FeBr 2

10. Chemical Formula of Salts Identify the ions and their charges Determine the number of each ion needed to balance the charges Note the ratio of positive to negative charges and write the formula

11. Write the Chemical Formula Potassium iodide Magnesium chloride Calcium oxide Calcium bromide Iron (II) chloride Copper (II) bromide Sodium sulfide Lithium bromide

12. Polyatomic Ions Group of atoms of different elements act as a single ion Do not need to change the ending of the polyatomic ion Be able to recognize them! – NaOH: sodium oxide hydrogen or sodium hydroxide?

13. Homework Page 213 # 1-5 Page 222 # 1-5 (practice problems) Page 225 # 1-5 (practice problems)