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Starter S-105

Learn how to calculate the grams of copper (II) chloride in a given number of formula units. Practice balancing chemical equations and writing word equations. Suitable for Chemistry students.

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Starter S-105

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  1. Starter S-105 • How many grams of copper (II) chloride are in 3.83 x 1021 formula units?

  2. Chemical Reactions Chapter 11

  3. 11.1 Describing Chemical Reactions Chapter 11

  4. 11.1 Describing Chemical Reactions Writing Chemical Reactions Word Equations – gives the names of compounds and elements in the equation reactants  products Reactants – compounds and elements before the reaction Products – compounds and elements after the reaction

  5. 11.1 Describing Chemical Reactions Different compounds, or elements are separated by a plus sign Copper + Oxygen  Copper (II) Oxide These are often converted from descriptions of the reaction

  6. 11.1 Describing Chemical Reactions When antiseptic hydrogen peroxide is put in an open cut bubbles of oxygen form rapidly. Water is also produced. Reaction – reactants hydrogen peroxide

  7. 11.1 Describing Chemical Reactions When antiseptic hydrogen peroxide in an open cut bubbles of oxygen from rapidly. Water is also produced. Reaction – products hydrogen peroxide

  8. 11.1 Describing Chemical Reactions When antiseptic hydrogen peroxide in an open cut bubbles of oxygen from rapidly. Water is also produced. Reaction – products hydrogen peroxide  oxygen + water

  9. 11.1 Describing Chemical Reactions When a stove burner is lit, methane gas reacts with oxygen to form carbon dioxide and water. Reaction – reactants methane gas + oxygen

  10. 11.1 Describing Chemical Reactions When a stove burner is lit, methane gas reacts with oxygen to carbon dioxide and water. Reaction – products methane gas + oxygen

  11. 11.1 Describing Chemical Reactions When a stove burner is lit, methane gas reacts with oxygen to carbon dioxide and water. Reaction – products methane gas + oxygen  carbon dioxide + water

  12. 11.1 Describing Chemical Reactions Chemical Equations – replace the names of compounds and elements with the chemical formula hydrogen peroxide  oxygen + water H2O2  O2 + H2O Remember diatomic elements

  13. 11.1 Describing Chemical Reactions methane gas + oxygen  carbon dioxide + water CH4 + O2  CO2 + H2O

  14. 11.1 Describing Chemical Reactions Usually the state of each compound or element is given beside the formula CH4(g)+ O2(g)  CO2(g) + H2O(g)

  15. Starter S-106 When solutions of potassium iodide and lead (II) nitrate are mixed in a beaker, a brilliant yellow solid is formed. This solid when analyzed turns out to be lead (II) iodide. Further analysis shows that potassium nitrate is now dissolved in the water. • Write the word equation. • Write the chemical equation

  16. 11.1 Describing Chemical Reactions Balancing Chemical Equations – both sides of a chemical equation have the same number of each atom Mass is conserved Balancing Demo

  17. 11.1 Describing Chemical Reactions Example Al + O2 Al2O3 1. Write elements on each side and how many of each are present

  18. 11.1 Describing Chemical Reactions Example Al + O2 Al2O3 Al – 1 Al – 2 O – 2 O – 3 2. Add one element at a time to the side that doesn’t have enough

  19. 11.1 Describing Chemical Reactions Al Al + O2 Al2O3 Al – 2 Al – 2 O – 2 O – 3

  20. 11.1 Describing Chemical Reactions Al O2 Al + O2 Al2O3 Al – 2 Al – 2 O – 4 O – 3

  21. 11.1 Describing Chemical Reactions Al O2 Al2O3 Al + O2 Al2O3 Al – 2 Al – 4 O – 4 O – 6

  22. 11.1 Describing Chemical Reactions Al,Al,Al O2 Al2O3 Al + O2 Al2O3 Al – 4 Al – 4 O – 4 O – 6

  23. 11.1 Describing Chemical Reactions Al,Al,Al O2,O2Al2O3 Al + O2 Al2O3 Al – 4 Al – 4 O – 6 O – 6 Balanced 3. Count the number of each compound or element – write a coefficient for each

  24. 11.1 Describing Chemical Reactions 4Al + 3O2 2Al2O3

  25. 11.1 Describing Chemical Reactions Balance the following equations • Cu + AgNO3  Cu(NO3)2 + Ag

  26. 11.1 Describing Chemical Reactions Balance the following equations • Cu + 2AgNO3  Cu(NO3)2 + 2Ag • FeCl3 + NaOH  Fe(OH)3 + NaCl

  27. 11.1 Describing Chemical Reactions Balance the following equations • Cu + 2AgNO3  Cu(NO3)2 + 2Ag • FeCl3 + 3NaOH  Fe(OH)3 + 3NaCl • CS2 + Cl2  CCl4 + S2Cl2

  28. 11.1 Describing Chemical Reactions Balance the following equations • Cu + 2AgNO3  Cu(NO3)2 + 2Ag • FeCl3 + 3NaOH  Fe(OH)3 + 3NaCl • CS2 + 3Cl2  CCl4 + S2Cl2 • AgNO3 + H2S  Ag2S + HNO3

  29. 11.1 Describing Chemical Reactions Balance the following equations • Cu + 2AgNO3  Cu(NO3)2 + 2Ag • FeCl3 + 3NaOH  Fe(OH)3 + 3NaCl • CS2 + 3Cl2  CCl4 + S2Cl2 • 2AgNO3 + H2S  Ag2S + 2HNO3 • Zn(OH)2 + H3PO4  Zn3(PO4)2 + H2O

  30. 11.1 Describing Chemical Reactions Balance the following equations • Cu + 2AgNO3  Cu(NO3)2 + 2Ag • FeCl3 + 3NaOH  Fe(OH)3 + 3NaCl • CS2 + 3Cl2  CCl4 + S2Cl2 • 2AgNO3 + H2S  Ag2S + 2HNO3 • 3Zn(OH)2 + 2H3PO4  Zn3(PO4)2 + 6H2O • Fe2O3 + H2  Fe + H2O

  31. 11.1 Describing Chemical Reactions Balance the following equations • Cu + 2AgNO3  Cu(NO3)2 + 2Ag • FeCl3 + 3NaOH  Fe(OH)3 + 3NaCl • CS2 + 3Cl2  CCl4 + S2Cl2 • 2AgNO3 + H2S  Ag2S + 2HNO3 • 3Zn(OH)2 + 2H3PO4  Zn3(PO4)2 + 6H2O • Fe2O3 + 3H2  2Fe + 3H2O

  32. Starter S-107 • Balance C6H6 + O2 CO2 + H2O CH3CH2OH + O2  CO2 + H2O

  33. 11.2 Types of Chemical Reactions Chapter 11

  34. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions You will need to know and predict the product for 6 types of chemical reactions • Synthesis Form Example Synthesis

  35. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions 2. Decomposition Form Example Decomposition

  36. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions 3. Single Replacement Reaction Form Example For metals, the reactions occurs if the metal is more reactive than the the one in the compound Single

  37. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions 4. Double Replacement Reaction Form Example Double

  38. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions 5. Combustion Reaction Form Example Combustion

  39. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions 6. Acid/Base Neutralization Reaction Form Example The substance AB is called a Chemical Salt Acid Base

  40. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reactions are predicted based on recognizing forms.

  41. Starter S-110 What type of reaction is this? CaCl2 + Pb(NO3)2 Write the complete balanced equation

  42. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction AgNO3 + NaCl  Type: Double Replacement Products: AgNO3 + NaCl  AgCl + NaNO3 Balanced: AgNO3 + NaCl  AgCl + NaNO3

  43. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction Pb + AgNO3 Type: Single Replacement Products: Pb + AgNO3 Ag + Pb(NO3)2 Balanced: Pb + 2AgNO3 2Ag + Pb(NO3)2

  44. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction FeCl3 + KOH  Type: Double Replacement Products: FeCl3 + KOH  Fe(OH)3 + KCl Balanced: FeCl3 + 3KOH  Fe(OH)3 + 3KCl

  45. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction NaOH + H2SO4 Type: Acid Base Neutralization Products: NaOH + H2SO4 Na2SO4 + H2O Balanced: 2NaOH + H2SO4 Na2SO4 + 2H2O

  46. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction C2H8 + O2 Type: Combustion Products: C2H8 + O2 CO2 + H2O Balanced: C2H8 + 4O2 2CO2 + 4H2O

  47. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction NH3 Type: Decomposition Products: NH3 N2 + H2 Balanced: 2NH3 N2 + 3H2

  48. 11.2 Type of Chemical Reactions 11.2 Types of Chemical Reactions Reaction Bi(NO3)3 + H2S  Type: Double Replacement Products: Bi(NO3)3 + H2S  Bi2S3 + HNO3 Balanced: 2Bi(NO3)3 + 3H2S  Bi2S3 + 6HNO3

  49. Starter S-111 What type of reaction is Fe + CuCl2 Write and balance the reaction

  50. 11.3 Reactions in Aqueous Solutions Chapter 11

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