Posters

1. Posters • Signs of a chemical reaction • Chemical vs. Physical reaction • Symbols used in chemical reactions • Synthesis • Decomposition • Single diplacement • Double displacement • Combustion

2. Journal Entry • How were these rocks formed?

3. Signs of a chemical reaction • Production of…. • Heat • Light • Gas • Precipitate (solid formed from two liquids) • Color change

4. The 5 Types of Reactions We classify reactions into 5 categories so that we may more easily predict the products. NEXT

5. Synthesis Definition Synthesis reaction – 2 substances are combined to form a single product • Combination reactions may also be called composition or synthesis reactions. A + B  AB  + MENU

6. Synthesis Examples 2Mg + O2 2MgO Magnesium and oxygen combine to form magnesium oxide. 2H2 + O2  2H2O Hydrogen and oxygen combine to form dihydrogen monoxide (water) MENU

7. Synthesis Demonstration Zinc + Sulfur  Zinc Sulfide Zn + S  ZnS Observations:

8. Decomposition Definition Decomposition reaction – A single compound is broken down into 2 or more products. AB  A + B +  MENU

9. Decomposition Examples 2NaCl(s)  2Na(s) + Cl2(g) Sodium chloride (table salt) decomposes into sodium and chlorine gas. CaCO3  CaO + CO2 Limestone (CaCO3 ) decomposes into lime (CaO) and carbon dioxide. MENU

10. Decomposition 2 H2O  2H2 + O2 Water decomposing into hydrogen gas and oxygen gas. Decomposition of H2O2 MENU

12. Decomposition Demonstration C12H22O11 + H2SO4 → C + H2O + SO2 (balance this!) Sugar + Sulfuric acid  Pure carbon + Water + Sulfur dioxide Observations:

13. Decomposition Demonstration • 2 NaHCO3 --> Na2CO3 + H2O + CO2 Observations: Massinitial Massfinal

14. Combustion Definition Combustion reaction – Hydrogen or a hydrocarbon (H and C) burn in oxygen to produce water and carbon dioxide. Heat is given off as energy. CxHx + O2 XH2O + XCO2 MENU

15. Combustion Examples CH4 + 2O2  2H2O + CO2 Methane burns in oxygen to produce water and carbon dioxide. C12H22O11 + 12O2  11H2O + 12CO2 A sugar molecule burns in oxygen to produce water and carbon dioxide. MENU

16. Combustion demonstration • Ethanol + Oxygen yields Water + Carbon dioxide C6H12O6 + O2 H2O + CO2

18. Single Replacement Definition Single Replacement reaction – A single element takes the place of an element in a compound. A + BC  B + AC + +  MENU

20. Single Replacement Examples Mg + BeO  Be + MgO Magnesium replaces beryllium in beryllium oxide to form magnesium oxide and beryllium. 2Na + 2HCl  H2 + 2NaCl Sodium replaces hydrogen in hydrochloric acid to yield hydrogen and sodium chloride. MENU

21. Single Replacement Demo. A single replacement of Zinc metal for hydrogen in hydrochloric acid. Zn + 2HCl  H2 + ZnCl2

22. Double Replacement Definition Double Replacement reaction – Elements in 2 compounds switch places to form 2 new compounds. AB + CD  AD + CB + +  MENU

24. Double Replacement Examples MgO + BeS  MgS + BeO Oxygen and sulfur switch places to form magnesium sulfide and beryllium oxide. Na2S + Zn(NO3)2  2Na(NO3) + ZnS Sulfur and nitrate switch places to form sodium nitrate and zinc sulfide.

25. Make a Venn diagram comparing…. • Synthesis vs. Decomposition • Single replacement vs. double replacement

26. What type of reaction? • 2 H2 + O2 -- 2H20

27. What type of reaction? • A + BX  AX + B

28. What type of reaction? AgNO3 + CuSO4 AgSO4 + CuNO3

29. What type of reaction is this? • 2 HCl (aq) + Zn (s) --> ZnCl2 (aq) + H2 (g)

30. What type of reaction?

31. Counting atoms • How many Carbons are in each of the following compounds: • CO2 • C2H6 • Na(CO3)2 • Mg(C2O)4

32. Warm-up • Around the room there are _7__ pictures representing types of reactions. YOUR pictures. • Make a list in your notebook, 1- _7__. Try to determine what type of reaction is being represented by the drawing.

33. Definitions • Co-efficient: The number before an element/compound (allowed to change when balancing) • Ex: 2 H2 • Subscript: The small number after an element/compound (NEVER allowed to change when balancing • Ex: 2 H2

34. Sacrificial Gummy Bear • Demonstrates: • Two types of chemical reactions • HIGHLY Exothermic energy change • Chemical energy converted into thermal, radiant and sound energy

35. Chemicals used • KClO3 - Potassium chlorate • C12H22O11 - Sucrose

36. First reaction KClO3 (s)  KCl (l) + O2 What type of reaction is this?

37. First reaction KClO3 (s)  KCl (l) + O2 Is this reaction balanced? (Make an RT table)

38. First reaction KClO3 (s)  KCl (l) + O2 Balance it!

39. First reaction 2 KClO3 (s)  2 KCl (l) + 3 O2 (g)

40. First reaction 2 KClO3 (s)  2 KCl (l) + 3 O2 (g)

41. Second reaction C12H22O11 + O2 (g)  C (s) + CO2 (g) + H2O (g) What type of reaction is this?

42. Second reaction C12H22O11 + O2 (g)  C (s) + CO2 (g) + H2O (g) Is it balanced? (Make an R/P table) If not, balance it! (1 min. early release if done correctly!)

43. Second reaction C12H22O11 + 3 O2 9 C + 3 CO2 + 11 H2O Balanced equation

44. Exothermic • Reactions which release energy ∆H = 5635 kJ

46. How to balance equations • 1.) Create a “R/P” table • (Reactants vs. Products) • 2.) Add coefficients to create equal numbers • 3.) update the R/P table • 4.) Change co-efficients until R = P

48. Pre-lab/practice • Purpose: To generate hydrogen gas • To set norms of behavior when dealing with acid

49. Norms:

50. Locations • Ring stands are on top of fume hood • Clamps are in 4A • All other materials are on counter by sink 1