1. Lesson 7

2. Lesson Outcome  B8: I am able to read and interpret chemical formulas for compounds of two elements, and give the IUPAC name and common names of compounds.  B9: I am able to distinguish between ionic and molecular compounds. I am able to identify examples of combining ratios/numbers of atoms per molecule found in some common materials, and use information on ion charges to predict combining ratios in ionic compounds or two elements. I am able to assemble and draw simple models of molecular and ionic compounds.

3. Compounds  Elements combine to forms compounds.  There are two types of compounds: Ionic Compounds Molecular Compounds

4. Ionic Compounds  Made up of a metal and non-metal An element from both sides of the staircase  These elements give and take electrons to become a compound.

5. Molecular Compounds  Made up of a non-metal and non-metal Both elements are found on the right side of the stair case.  The elements share electrons to form a compound.

6. Ionic or Molecular  NaCl  CO 2  MgO  NH 3  CH 4  FeCl 2  H 2 O  NaOH

7. Chemical Formulas  Uses symbols and numbers to represent the number and type of each atom found in the compound.  Ex: H 2 O

8. Practice Time!  What type and how many atoms?

9. Diatomic Compounds  Di = 2  These are compounds that have two of the same elements.  H O F Br I N Cl H 2 O 2 F 2 Br 2 I 2 N 2 Cl 2

10. Naming Molecular Compounds  1. Write the entire name of the first element.  2. Change the ending on the name of the second element to “ide”  3. Use a prefix to indicate the number of each type of atom in the formula 1 = mono 2= di 3 = tri 4= tetra Note: the prefix mono is only used with the second element

11. Practice  CO  CCl 4  SiO 2  SO 2  H 2 O  NH 3  CH 4

12. Practice  Phosphorous trihydride  Carbon tetrachloride  Nitrogen dioxide  Sulfur trioxide

13. Naming Ionic Compounds  1. Write the name of the metal in the compound first.  2. Write the non-metal element second and change the ending to “ide”  3. Subscripts indicate the ratio of ions in the compound: Ex: CaCl 2 = 1:2 ratio Note: we do not use prefixes for ionic compounds

14. Practice  NaCl  NaF  LiCl  ZnS  MgO  K 2 S  Na 2 O

15. Making Ionic Formulas from a Name  1. write the symbols for both elements.  2. swap and drop the charges  3. reduce

16. Trends  What charges to metals always have?  What charges do non-metals always have?

17. Practice  Sodium chloride  Potassium oxide  Magnesium nitride  Beryllium oxide  Cesium sulfide  Lithium bromide