2.  Objectives  Today I will be able to: ▪ Determine the oxidation number of an element in a compound ▪ Apply rules to naming organic compounds  Informal assessment – monitoring student interactions as they complete the practice problems  Formal assessment – analyzing student responses to the practice problems and exit ticket  Common Core Connection  Build strong content knowledge  Make sense of problems and persevere in solving them  Reason abstractly and quantitatively

3.  Evaluate: Warm Up  Explain: Oxidation Number Notes  Elaborate: Oxidation Number Practice  Elaborate/ Evaluate: Organic Nomenclature Review  Evaluate: Exit Ticket

4.  Write the formula for the gas laws below  Boyle’s Law  Ideal Gas Law  Name the acids listed then identify the acid as a strong or weak acid  HBr  HC 2 H 3 O 2  H 2 SO 4  HClO 3  HClO 2

5.  Today I will be able to:  Determine the oxidation number of an element in a compound  Apply rules to naming organic compounds

6.  Signed Syllabus and Safety Contract due Friday, August 29  Cation/Anion Quiz sometime the week of September 2-5  Solubility Rule Quiz sometime the week of September 8-11  Summer Assignment due September 2  Summer Assignment Exam September 2

7.  Warm Up  Oxidation Number Notes  Oxidation Number Practice  Organic Nomenclature Review  Exit Ticket

9.  Are used to keep track of electrons being gained and lost

10.  Monatomic ions  oxidation number is the same as its charge  Examples: What are the oxidation numbers when the elements below form ions? ▪ Li ▪ Mg ▪ Al ▪ O

11.  Neutral molecules and polyatomic ions  Each atom is assigned a hypothetical charge  Charge is assigned by dividing up the electrons and through a specific set of rules

12. 1. For an atom in its elemental form, the oxidation number is always zero 2. For any monatomic ion the oxidation number equals the ionic charge 3. Nonmetals usually have negative oxidation numbers, although sometimes they can be positive  The oxidation number of oxygen is usually -2 in both ionic or molecular compounds. Exception: Peroxides with the O 2 2- ion giving oxygen an oxidation number of -1.  Oxidation number of hydrogen is usually +1 when bonded to nonmetals and -1 when bonded to metals (example: NaH)  Oxidation number of fluorine is -1 in all compounds. Other halogens have an oxidation number of -1 in most binary compounds. However, when combined with oxygen in oxyanions, they have positive oxidation states 4. The sum of the oxidation numbers in all atoms of a neutral compound is zero. The sum of the oxidation number in a polyatomic ion equals the charge of the ion

15.  What are the oxidation numbers for sulfur in the following compounds.  H2S  S8  SCl2  Na2SO3  SO42-