1. CHEMICAL REACTIONS! BUBBLES PRECIPITATE COLOR CHANGES EVOLUTION OF HEAT & LIGHT (FIRE!)

2. Chemical Equations The “sentence” that describes the reaction. The “sentence” that describes the reaction. Reactants – parts before the reaction Reactants – parts before the reaction Yield sign – arrow representing the actual reaction. Yield sign – arrow representing the actual reaction. Products – parts remaining after the reaction has occurred. Products – parts remaining after the reaction has occurred.

3. Chemical Equations MUST INCLUDE ALL REACTANTS & PRODUCTS MUST INCLUDE ALL REACTANTS & PRODUCTS COMPOUNDS MUST BE WRITTEN WITH CORRECT FORMULAS ACCORDING TO OXIDATION NUMBERS COMPOUNDS MUST BE WRITTEN WITH CORRECT FORMULAS ACCORDING TO OXIDATION NUMBERS MUST SATISFY THE LAW OF CONSERVATION OF MATTER MUST SATISFY THE LAW OF CONSERVATION OF MATTER

4. 7 DIATOMIC ELEMENTS HYDROGEN NITROGEN OXYGEN FLUORINE CHLORINE BROMINE IODINE Mr & Mrs BrINClHOF

5. Organic Nomenclature (organic means carbon based) Alkane – carbon chain held together with single bonds. General formula – C n H 2n+2 Cyclic alkanes - C n H 2n

6. TYPES of CHEMICAL REACTIONS 1. Combustion – an organic molecule (carbon based) burns with oxygen and always produces CO 2 and H 2 O. Alkanes C n H 2n+2 1. methane6. hexane 2. ethane7. heptane 3. propane8. octane 4. butane9. nonane 5. pentane10.decane

7. Continued… 2. Synthesis – Two or more reactants combine to form one product. A + B  AB Examples sodium + sulfur hydrogen + oxygen

8. TYPES of CHEMICAL REACTIONS 3. Decomposition – One reactant breaks apart to form two or more products. AB  A + B

9. Types of Decomposition Reaction binary compounds  metal carbonate  metal hydroxide  metal chlorate  acids 

10. Continued… 4. Single Replacement – a single element replaces the similar element within a compound.  Cation exchange – positive ion is replaced  Anion exchange – negative ion is replaced

11. Activity Series A list of elements organized according to the ease with which they undergo reactions. Established with single- replacement reactions - most active on top, least active on bottom.

12. Activity Series… Elements on the activity series chart can replace any element below it on the activity series. Examples-  sodium + zinc chloride   sodium + barium chloride   chlorine + potassium iodide   chlorine + potassium fluoride 

13. Last but not least… 5. Double Replacement reactions – (aka- metathesis) reaction between two compounds where similar ions exchange places.

14. Reactions in Aqueous Solutions Aqueous Solutions? Net ionic equations Spectator ions

15. Types of D.R. Reactions Precipitate – reaction between solutions of soluble compounds that yield an insoluble product. Example – K 2 SO 4 + Ba(NO 3 ) 2 

16. Molecular – ionic reactions that yield a covalent product. (i.e. – water) Example – NaOH + HCl 

17. Gas – reactions that produce some type of gas that bubbles away. Example – HCl (aq) + FeS (s) 

18. Gases to Look For as Products H 2 S NH 4 OH  NH 3 + H 2 O H 2 CO 3  H 2 O + CO 2

19. Examples HBr + LiOH  CaCO 3 (s) + HCl (aq)  (NH 4 ) 2 S (aq) + LiOH (aq)  K 2 CrO 4 (aq) + AgNO 3 (aq)  Ca(NO 3 ) 2 (aq) + RbCl (aq) 