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Great and Glorious Test Day

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1 Great and Glorious Test Day
Starter S-105 Test Day Great and Glorious Test Day Yahoo Yipee Yah

2 Starter S-101 What is the chemical formula for Hydrochloric Acid
Nitrogen Dioxide Iron (II) Phosphate

3 Chapter 11 Chemical Reactions

4 11.1 Describing Chemical Reactions
Chapter 11 11.1 Describing Chemical Reactions

5 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

6 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

7 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

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

9 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

10 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

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

12 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

13 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

14 11.1 Describing Chemical Reactions
methane gas + oxygen  carbon dioxide + water CH4 + O2  CO2 + H2O

15 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) Solid (s) Liquid (l) Gas (g) Aqueous (aq)

16 Starter S-102 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

17 Starter S-106 A chunk of iron is placed in a solution of hydrochloric acid. A gas bubbles out of the solution that is tested and found to be hydrogen. The solution left in the test tube is iron (III) chloride.

18 Starter S-107 Water is placed in a test tube and zapped with electricity. Two gases are produced. One makes a glowing wooden split light up, so it is oxygen. The other causes a small explosion when a burning wooden splint is placed in it, so it is hydrogen.

19 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

20 11.1 Describing Chemical Reactions
Example Al + O2  Al2O3 1. Write elements on each side and how many of each are present

21 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

22 11.1 Describing Chemical Reactions
Al + O2  Al2O3 Al – 2 Al – 2 O – 2 O – 3

23 11.1 Describing Chemical Reactions
Al O2 Al + O2  Al2O3 Al – 2 Al – 2 O – 4 O – 3

24 11.1 Describing Chemical Reactions
Al O2 Al2O3 Al + O2  Al2O3 Al – 2 Al – 4 O – 4 O – 6

25 11.1 Describing Chemical Reactions
Al,Al,Al O2 Al2O3 Al + O2  Al2O3 Al – 4 Al – 4 O – 4 O – 6

26 11.1 Describing Chemical Reactions
Al,Al,Al O2,O2 Al2O3 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

27 11.1 Describing Chemical Reactions
4Al + 3O2  2Al2O3

28 11.1 Describing Chemical Reactions
Balance the following equations Cu + AgNO3  Cu(NO3)2 + Ag

29 11.1 Describing Chemical Reactions
Balance the following equations Cu + 2AgNO3  Cu(NO3)2 + 2Ag FeCl3 + NaOH  Fe(OH)3 + NaCl

30 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

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 AgNO3 + H2S  Ag2S + HNO3

32 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

33 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

34 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

35 Starter S-107 Balance C6H6 + O2  CO2 + H2O CH3CH2OH + O2  CO2 + H2O

36 11.2 Types of Chemical Reactions
Chapter 11 11.2 Types of Chemical Reactions

37 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

38 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions 2. Decomposition Form Example Decomposition

39 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

40 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions 4. Double Replacement Reaction Form Example Double

41 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions 5. Combustion Reaction Form Example Combustion

42 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

43 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions Reactions are predicted based on recognizing forms.

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

45 Objective I can perceive and predict products for at least six different types of chemical reactions.

46 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions Reaction AgNO3 + NaCl  Type: Double Replacement Products: AgNO3 + NaCl  AgCl + NaNO3 Balanced:

47 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

48 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

49 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

50 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

51 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions Reaction NH3  Type: Decomposition Products: NH3  N2 + H2 Balanced: 2NH3  N2 + 3H2

52 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

53 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions Reaction Ca + F2  Type: Synthesis Products: Ca + F2  CaF2 Balanced:

54 Starter S-112 What type of reaction is C2H5OH + O2 
Write and balance the reaction

55 11.3 Reactions in Aqueous Solutions
Chapter 11 11.3 Reactions in Aqueous Solutions

56 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution Many reactions take place in water – aqueous For example, the reaction of Silver Nitrate and Sodium Chloride But in a solution, most ionic compounds have dissociated to form ions

57 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution That is they are really in this form This is called the Complete Ionic Equation Notice – the solid is not broken into ions, only what is in solution

58 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution Look carefully at the equation There are Na+ and NO3- ions that stay the same These are called Spectator Ions A Net Ionic Equation shows only ions that actually do something in a reaction

59 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution Net Ionic Equation Try this one

60 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution Practice Equation Compete Ionic Equations Net Ionic Equation

61 Starter S-113 Write the complete ionic and net ionic equations for
Fe(NO3)3(aq) + 3NaOH(aq)  Fe(OH)3(s) + 3NaNO3(aq) Complete Ionic Fe+3(aq)+3NO3-(aq) + 3Na+(aq)+3OH-(aq) Fe(OH)3(s)+ 3Na+(aq)+3NO3-(aq) Net Ionic Fe+3(aq)+3OH-(aq) Fe(OH)3(s)

62 Starter S-115 A. Write the complete ionic and net ionic equations for
Cu(s) + AgNO3(aq)  Ag(s) + Cu(NO3)2(aq) random squirrel with light saber

63 Practice

64 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution Precipitate – separates from a solution as a solid Predicted using a solubility chart In the reaction Is either product a solid? Chart

65 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution AgCl – insoluble NaNO3

66 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution AgCl – insoluble - solid NaNO3

67 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution AgCl – insoluble - solid NaNO3 – soluble

68 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution AgCl – insoluble - solid NaNO3 – soluble - aqueous

69 Starter S-115 A. Write the complete ionic and net ionic equations for
Cu(s) + AgNO3(aq)  Ag(s) + Cu(NO3)2(aq) B. Which of the following are soluble Cu(OH)2 Mg(NO3)2 AgCl random squirrel with light saber

70 Starter S-117 Predict the products of the following reaction. Determine the correct states for the products AgNO3(aq) + NaCl(aq) 

71 Starter S-117 Test

72 Starter S-119 Predict the products of the following reaction. Determine the correct states for the products KOH + Mg(NO3)2 

73 Starter S-120 Predict the products of the following reaction. Determine the correct states for the products Cu(NO3)2 + Fe(OH)3 

74 Starter S-122 How would you identify the following aqueous solutions? Name a simple test. AgNO3 H2SO4 KOH Cu(NO3)2 CoCl2

75 Starter S-122 If 12.0 g of AgCl react What is the molar mass of AgCl?
How many moles of AgCl are present as a reactant? Silver chloride precipitate


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