1. Hydrates

2.  Chemical compounds that have water molecules sticking to them  Water molecules form part of the chemical compound’s crystal structure  Water of hydration—water within the crystal structure  # of water molecules fixe, does NOT change  Chemical compounds that have water molecules sticking to them  Water molecules form part of the chemical compound’s crystal structure  Water of hydration—water within the crystal structure  # of water molecules fixe, does NOT change

3. Hydrate Nomenclature Formula = XY  H 2 O  Chemical compound + # of water molecules  Separated by a “dot”  Ratio of water to chemical compound—represented by the prefixes  The name and formula indicate how many water molecules are within the chemical structure Formula = XY  H 2 O  Chemical compound + # of water molecules  Separated by a “dot”  Ratio of water to chemical compound—represented by the prefixes  The name and formula indicate how many water molecules are within the chemical structure

4. Example 1: CaSO 4  2H 2 O

5. Example 2: Calcium chloride dihydrate

6. Practice !  1) sodium sulfate decahydrate  2) FeSO 4  7H 2 O  3) CoCl 2  6H 2 O  4) magnesium sulfate heptahydrate  5) tin (IV) chloride pentahydrate  1) sodium sulfate decahydrate  2) FeSO 4  7H 2 O  3) CoCl 2  6H 2 O  4) magnesium sulfate heptahydrate  5) tin (IV) chloride pentahydrate

7. Acid/Base Nomenclature

8. Acids  Formulas usually begin with an “H” 1)Binary  Hydrogen joined to a nonmetal, 2 elements  Shorten “hydrogen” to “HYDRO”  Drop “ide” ending, add “-IC ACID” 2)Polyatomic  More than 2 elements  Many are oxoacids (H, O, nonmetal)—name based on # of oxygens.  Formulas usually begin with an “H” 1)Binary  Hydrogen joined to a nonmetal, 2 elements  Shorten “hydrogen” to “HYDRO”  Drop “ide” ending, add “-IC ACID” 2)Polyatomic  More than 2 elements  Many are oxoacids (H, O, nonmetal)—name based on # of oxygens.

9. Acids (cont.) 2 ) Polyatomic ions (cont.)  “-ate” ending, add “-IC ACID” (original)  “-ite” ending, add “-OUS ACID” (one less O than original)  Prefix with hydro and “-ite ending:” add “HYDRO” and “-OUS acid” (2 less O than original)  One additional oxygen than original, add “HYPER/PER” prefix and “IC ACID” 2 ) Polyatomic ions (cont.)  “-ate” ending, add “-IC ACID” (original)  “-ite” ending, add “-OUS ACID” (one less O than original)  Prefix with hydro and “-ite ending:” add “HYDRO” and “-OUS acid” (2 less O than original)  One additional oxygen than original, add “HYPER/PER” prefix and “IC ACID”

10. Acid Practice 1)HClO 3 2)Sulfuric acid 3)HNO 2 4)Hydrobromic acid 1)HClO 3 2)Sulfuric acid 3)HNO 2 4)Hydrobromic acid

11. Bases  Groups IA and IIA form main bases 1)Name the cation 2)Add “hydroxide” to end  Groups IA and IIA form main bases 1)Name the cation 2)Add “hydroxide” to end

12. Base Practice 1)NH 4 OH 2)Strontium hydroxide 3)Ca(OH) 2 1)NH 4 OH 2)Strontium hydroxide 3)Ca(OH) 2

13. Classwork  Finish Nomenclature Worksheet

14. Homework  Inquiry #1 Lab Report—Beer’s Law  Read over Percent Water Lab procedure  Inquiry #1 Lab Report—Beer’s Law  Read over Percent Water Lab procedure