1. Chemical Reactions & Acids, bases, and solutions
Chapter 6 and 7

2. Explain balancing equations using Cornell Notes and Vocab Maps.
Today we will
Explain balancing equations using Cornell Notes and Vocab Maps.

3. 1. Describing chemical equations
2. Chemical equations – what are they? 3. Short, easy way to show a chemical reaction, using symbols instead of words 3. Reactant + reactant product + product

4. 2. Conservation of matter
3. During a chemical reaction, matter is neither created nor destroyed. 3. The mass of the reactants must equal the mass of the products 3. The number of atoms stays the same no matter how they are arranged.

5. 2. Open and closed systems
3. Open system – matter can enter from or escape the surroundings 4. ex: Fire place
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6. 3. Closed system – Matter not allowed to leave or enter. 4
3. Closed system – Matter not allowed to leave or enter. 4. Pumpkin decaying in a bag.
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7. 2. Balancing equations
3. A chemical equation must show the SAME number of each type of atom on both sides of the equations

8. 3. Steps to balancing equations
Step 1: write the equation Step 2: Count the atoms Step 3: Use Coefficients to balance atoms Step 4: Look back and count 3. Coefficient – what are they? 4. Number placed in front of a chemical formula

10. Today we will…
Classify chemical reactions using Cornell Notes, our brains, and concept maps.

11. 1. Describing Chemical reactions

12. 2. Classifying chemical reactions
3. Synthesis 4. Put things together 4. Two or more elements or compounds combine to make a more complex substance 4. Ex: 2H + O = Water

14. 3. Decomposition
4. Compounds break down into simpler products 4. Ex: Hydrogen peroxide breaks down into water and oxygen 2H202 2H20 + O2

15. 3. Replacement
4. When one element replaces another in a compound 4. When two elements in different compounds trade place 2Cu2O + C 4Cu + CO2

16. Questions
How could you determine ….? What would happen if….? How would you categorize….?

17. Concept maps: Synthesis Decomposition Replacement
Homework
Concept maps: Synthesis Decomposition Replacement

18. Today we will….
Analyze solutions, concentrations and solubility using Cornell Notes and task cards.

19. 1. Solutions – what are they?
2. A uniform mixture that contains a solvent and at least one solute 2. Solvent – what is it? 3. A Part of the solution present in the largest amount 2. Solute – dissolved by the solvent and cannot be seen in the solution

20. 2. Example Water + Sugar = Sugar water Water = Solvent Sugar = Solute Sugar water = solution

21. 2. Colloids – what are they?
3. Mixture that contains small, undissolved particles that do not settle out. 3. The particles are too small to be seen, but large enough to scatter a light beam 3. Examples: 4. Fats and proteins in milk 4. Fog 4. Jell-O 4. Shaving cream

22. 2. Suspension – what is it?
3. A mixture in which particles can be seen and easily separated by settling or filtration. 3. Heterogeneous mixture 3. Examples : 4. Snow globe

23. 2. Concentrated Solution
3. A lot of solute dissolved in a certain amount of liquid 3. Examples 4. Frozen fruit juices 4. 3 cups of sugar in lemonade

24. 2. Measuring concentration
3. The amount of solute is compared to the amount of solution and measured by %
4. Solute/solution * 100 = % concentration

25. Practice problem
A solution contains 12 grams of solute dissolved in 36 grams of solution. What is the concentration of the solution?

26. Practice problems
Page 267 Numbers 4 and 5

27. 2. Dilute solution – what is it?
3. Has a little solute dissolved in a certain amount of solvent. 3. Example 4. 1 Cup of sugar dissolved in 8 cups of lemonade 4. Frozen fruit juice with 8 cups of water added.

28. 2. Solubility – what is it?
3. Measure of how much solute can dissolve in a solvent at a given temperature 3. Unsaturated solution 4. You can add more to the solution 3. Saturated solution 4. You cannot add more to the solution 3. Supersaturated solution 4. Has more solute than the solution can hold and usually it settles out.

29. 3. Temperature
4. As temperature increases, solubility increases 5. the solution can hold more solute 4. To dissolve more sugar, heat the water 4. Gases tend to become more soluble in cold temperatures 5. Hot soda tastes “flat”

30. Practice time 
Page 266 numbers 1-4 on the graph.

31. Describe acids and bases using Cornell notes and litmus paper.
Today we will…
Describe acids and bases using Cornell notes and litmus paper.

32. 1. Acids and Bases
2. Acids – what are they? 3. A substance that tastes sour, and reacts with metals and carbonates on the pH scale 3. Can be corrosive 3. Turns blue litmus paper red 3. Produce a hydrogen ion H+ in water

33. 3. Examples of Acids 4.
4. Oranges
4. Tomatoes
4. Spinach

34. 2. Uses of Acids 3. Vitamin C 3. Various vitamins and minerals 3
2. Uses of Acids 3. Vitamin C 3. Various vitamins and minerals 3. Used to clean bricks and metals 3. Found in fertilizer 3. Batteries

35. 2. Bases – what are they?
3. A substance that tastes bitter and feels slippery on the pH scale 3. Produces hydroxide ions OH- in water 3. Turns litmus red litmus paper blue

36. 3. Examples 4. Ammonia 4. Glass cleaner 4. Baking Soda 4
3. Examples 4. Ammonia 4. Glass cleaner 4. Baking Soda 4. Calcium Oxide and calcium hydroxide make mortar and cement

37. 2. Uses of bases 3. Cleaning agent 3. Creates mortar and cement 3
2. Uses of bases 3. Cleaning agent 3. Creates mortar and cement 3. Used in baking that make baked goods fluffy.

38. Homework
Memory map: Acid, Base

39. Warm-up
On the left side of your notes complete the following: Create a Venn Diagram to compare and contrast ACIDS vs Bases. You have 5 minutes!

40. Today we will…
Describe acids and bases in Solutions using Cornell Notes and a foldable.

41. 1. Acids and Bases in solutions
2. Acids in solutions 3. H+ are present 3. HCl -> H+ + Cl- in water 3. In water the H breaks the bonds with the compound and forms H+

42. 2. Bases in solutions
3. OH- (hydroxide ion) when bases dissolve in water 3. Not all bases contain OH- 4. ammonia NH3 3. Produces OH- ions in water

43. 2. Strength of acids and bases
3. pH scale ranges from Describes the concentration of ions acidic 4. lemon 3. 7 neutral 4. water – 14 basic 4. Drain cleaner 3. 0 = Strong acid while 6 is a weak acid 3. 8 = weak base while 14 is a strong base

44. 2. Acid-base reactions
3. Neutralization 4. reaction between an acid and a base causing it to become neutral

45. Antacid Pre-Lab
Question: Which antacid works the best? Hypothesis: Materials Procedure

46. Antacid Table Substance pH before pH with Antacid A pH with Antacid B
pH with Antacid C

47. Chemistry is
A characteristic of a substance that can be observed without changing the substance into another substance
The study of matter and how matter changes
Anything that has mass and takes up space
A rapid reaction between oxygen and a substance called fuel.

48. Anything that has mass and takes up space is considered
Matter
Energy
Chemistry
Endothermic

49. What happens when chemical bonds break and new bonds form?
A physical change
A chemical reaction
Matter is destroyed
Surface area increases

50. The only sure evidence for a chemical reaction is
The formation of a gas
A color change
The production of one or more new substances
Changes in properties

51. Endothermic Exothermic Combustion Unbalanced
A chemical reaction that absorbs energy in the form of heat is described as
Endothermic
Exothermic
Combustion
Unbalanced

52. CaCO3 represents a chemical
Symbol
Formula
Subscript
Reaction

53. Chemical equation Chemical formula Symbol Subscript
A shorter, easier way to show chemical reactions, using symbols instead of words, is called a
Chemical equation
Chemical formula
Symbol
Subscript

54. The substances listed on the left side of a chemical equation are the
Products
Coefficients
Precipitates
Reactants

55. In a(n) ____ change, elements and/or compounds rearrange to form new substances.

56. A material used to decrease the rate of a reaction is called a _____.

57. The process of solid ice changing into liquid water is a(n) ____ change.

58. A precipitate is a(n) ____ that forms from solution during a chemical reaction.

59. The ____ is the amount of one material present in a given volume of another material.

60. In a chemical equation, the substances written on the right side of the arrow are called?

61. A chemical reaction that releases energy in the form of heat is a(n) _______ reaction.

62. Every chemical reaction involves a change in
Energy
Concentration
State
Mass

63. Subscript Coefficient Reactant Product
The number placed below an element’s symbol in a chemical formula is called a
Subscript
Coefficient
Reactant
Product

64. Chemical energy Activation energy Endothermic energy Exothermic energy
The minimum amount of energy that has to be added to start a reaction is the
Chemical energy
Activation energy
Endothermic energy
Exothermic energy

65. What is the purpose of a coefficient?

66. Chemistry is? The study of matter and how matter changes
Anything that has mass and takes up space
A rapid reaction between oxygen and a substance
The study of physics

67. Enzymes Fuels Inhibitors Reactants
Chemicals that act as biological catalysts by speeding up reactions in living things are
Enzymes
Fuels
Inhibitors
Reactants

68. List three examples of a chemical change

69. Define Synthesis and decomposition.

70. Discuss with your group the following questions.
Why is learning exothermic and endothermic reactions important to your life?
Based on what you know, how would you explain chemical reactions?

71. Today we will…
Analyze how to control chemical reactions using Cornell Notes and a word map.

72. 1. Controlling Chemical Reactions
2. Activation energy 3. A reaction cannot happen unless it has enough energy 3. All chemical reactions require a certain amount of activation energy to get started 3. EX: Spark, lightning

73. 2. Exothermic and Endothermic reactions
3. Exothermic – heat energy is released 3. Endothermic – heat energy is absorbed

74. 2. Rates of chemical reactions
3. To make reactions happen faster, add more energy 3. Factors that affect rates of reaction includes surface area, temperature, concentration, and the presence of catalysts or inhibitors

75. 3. Surface area
4. Smaller surface area can cause a faster reaction 4. Chewing food into smaller pieces causes the body to digest the food faster

76. 3. Temperature
4. When an object is heated, the particles move faster and increase the rate of reaction 4. Faster moving molecules have more energy

77. 3. Concentration
4. The amount of a substance in a given volume 4. More particles = more particles to react

78. 3. Catalysts
4. A material that increases the rate of reaction by lowering the activation energy 4. Enzymes – biological catalysts

79. 3. Inhibitors
4. A material used to decrease the rate of reaction 4. Some reactions work better when they do not react as fast. 4. EX: Food preservatives