1. Rewind your mind Naming/formulas  Naming Ionic compounds  These have a metal and nonmetal  Metals (groups 1-12) nonmetals (14-17)  Noble gases don’t bond….  Name the metal 1 st  Don’t change anything about the name  Name the nonmetal  Change the end to ide  Al2O3 Aluminum oxide

2. Ionic compounds  K2O  LiBr  Sr3N2  CaCl2  Potassium oxide  Lithium bromide  Strontium nitride  Calcium chloride  Be sure to swap and drop charges…use the periodic table

3. Ionic compounds with poly’s  Same rules, just name the poly from the reference tables  Then swap and drop  KNO3 Potassium Nitrate  NaOH sodium hydroxide

4. Covalent  These are nonmetals bonded to nonmetals  We need a way to tell how many are bonded together so we use prefixes  Name the 1 st element, if there is a subscript put that prefix on it  Name the 2 nd element and add ide  CO2  Carbon dioxide  Mono=1  Di=2  Tri=3  Tetra=4  Penta=5  Hexa=6  Septa=7  Octa=8  Nona=9

5. covalent  Si 6 O4  OF2  S 2 Cl5  Hexasilicon tetroxide  Oxygen diflouride  Disulfur pentachloride

6. Homework  Your homework tonight is to name or write the formulas for the compounds on the page  Use notebook paper so I can read it please….  Remember to swap and drop, use ide

7. 1/8 Today you will need…  The new Unit Plan. This will go in your binder behind the DBA.  The paper from the side table  This is your warm-up. You have TEN minutes to complete this assignment

9. Signs of a Chemical Reaction  Evolution of heat and light  Formation of a gas  Formation of a precipitate  Color change

10. Characteristics of Chemical Equations 1. The equation must represent known facts. 2. The equation must contain the correct formulas for the reactants and products. 1. You must remember & be able to apply the knowledge regarding writing names & formulas for ionic & covalent compounds. 3. The Law of Conservation of Mass must be satisfied.

11. Law of Conservation of Mass  Mass is neither created nor destroyed in a chemical reaction  Total mass stays the same  Atoms can only rearrange 4 H 2 O 4 H 2 O 4 g32 g 36 g

12. Chemical Equations A+B  C+D REACTANTS PRODUCTS

13. Chemical Equations

14. Celebrity Edition

15. 5 types of reactions  Synthesis  Decomposition  Single replacement  Double replacement  Combustion

16. Synthesis  When two or more reactants form one product.  8 Fe + S 8 ---> 8 FeS

17. Jay-Z Beyonce

18. Jay-Z and Beyonce

19. Decomposition  When one reactant breaks apart into two or more products.  2 H 2 O ---> 2 H 2 + O 2

20. Chris Brown and Rihanna

21. Chris Brown Rihanna

22. Single Replacement  When one element replaces another in a compound  Zn + 2 HCl --> ZnCl 2 + H 2

23. Justin & Cameron Jessica

24. Justin & Jessica Cameron

25. Double Replacement  Two compounds switch places and form two different compounds  NaCl + AgNO 3 --> NaNO 3 + AgCl

26. Brad & Jen Gerard & Angie

27. Brad & Angie Gerard & Jen

28. Combustion Reaction  An exothermic chemical rxn that combines C x H x (An Alkane) and oxygen O 2 to form a product of CO 2, H 2 O, and heat (the word heat want necessarily be written in the rxn).  CH 4 (g) + 2O 2 (g)  CO 2 (g) + 2H 2 O (g) + heat

29. Synthesis  AKA composition reaction  the combination of 2 or more substances to form a compound  only one product A + B  AB

30. Synthesis H 2(g) + Cl 2(g)  2HCl (g)

31. Decomposition  a compound breaks down into 2 or more simpler substances  only one reactant AB  A + B

32. Decomposition 2H 2 O (l)  2H 2(g) + O 2(g)

33. Decomposition of Binary Compounds  Binary compounds will decompose into their component elements.  2H 2 O(l)  2H 2 (g) + O 2 (g)

34. Single Replacement  one element replaces another in a compound  metal replaces metal (+)  nonmetal replaces nonmetal (-) A + BC  B + AC

35. Single Replacement Cu (s) + 2AgNO 3(aq)  Cu(NO 3 ) 2(aq) + 2Ag (s)

36. AB + CD  AD + CB Double Replacement  ions in two compounds “change partners”  cation of one compound combines with anion of the other

37. Double Replacement Pb(NO 3 ) 2(aq) + K 2 CrO 4(aq)  PbCrO 4(s) + 2KNO 3(aq)

38. Combustion CH 4(g) + 2O 2(g)  CO 2(g) + 2H 2 O (g)  the burning of any substance in O 2 to produce heat A + O 2  B

39. Na (s) + O 2(g)  Na (s) + O 2(g)  C 3 H 8(g) + O 2(g)  C 3 H 8(g) + O 2(g)  5 3 4 5 3 4 Combustion  Predicting Products:  contain oxygen  hydrocarbons form CO 2 + H 2 O CO 2(g) + H 2 O (g) CO 2(g) + H 2 O (g) Na 2 O (s) Na 2 O (s) 4 2 4 2