1. Chemical Reactions and Properties of Matter

2. Matter is neither created nor destroyed
In a chemical reaction, the same number and types of atoms occur in the products as in the original reactants
The mass of the products always equals the mass of the reactants
The law of conservation of mass

3. Balancing Equations
Demonstrates the law of conservation of matter/mass
In chemical equations, the coefficients in front of the chemical formulas represent the number of molecules of reactants or products

4. Use this chemical equation to answer the question:
What coefficients of Fe, O2 and Fe2O3 will show that matter is conserved in this chemical reaction?
2, 1, 2
2, 3, 2
4, 1, 2
4, 3, 2

5. Types of chemical reactions
Synthesis reaction – two or more substances combine to form a compound

6. Balancing a synthesis reaction

7. Types of chemical reactions cont.
A decomposition reaction is the opposite of a synthesis reaction
A compound breaks down into more simple substances

8. Balancing a decomposition reaction

9. Types of chemical reactions cont.
A single replacement reaction involves a single element replacing another element in a compound, forming a different compound.

10. Balancing a single replacement reaction

11. Types of chemical reactions cont.
In a double replacement reaction, two elements in two different compounds replace each other, forming two different compounds

12. Balancing a double replacement reaction

13. Gas Laws
Pressure (P), volume (V), and absolute temperature (T) are used to describe the condition of a gas

14. States of Matter
Solid – rigid structure, atoms vibrate in place, definite volume and shape
Liquid – atoms held loosely together but not rigid, free to move to a degree, definite volume, no definite shape
Gas – atoms experience greatest freedom, very little attractive forces between atoms/molecules, move freely, no definite shape or volume
Plasma – high energy, atoms stripped of some or all electrons ex: lightning, solar flares

15. Properties of Matter
Physical properties are measurable and can be observed or measured without changing the identity of the substance.
Color, hardness, area, length, strength, density*, temperature, melting point, boiling point, solubility, electrical conductivity, and state of matter
d = m/v

16. Properties of matter cont.
Chemical properties can be measured only by chemically changing an object
Flammability, oxidation, toxicity, heat of combustion

17. Classification of Matter
Matter can be classified as a pure substance or a mixture
A pure substances is anything that when broken down into its smallest component, all those components are the SAME (ex: elements and compounds)
A mixture is a material that is made up of two or more different substances

18. Mixtures
The substances in a heterogeneous mixtures can be seen and relatively easily separated (ex: sand, trail mix, Cheerios in milk…)
A homogeneous mixture has a uniform composition – the individual substances can not be detected visually, but it can be separated by physical means (ex. Air, milk, salt water, iced tea…)

19. Solutions A solution is type of homogeneous mixture
A solution consists of a solute (the substance being dissolved or broken down) and a solvent (the substance doing the dissolving)
Solubility is the ability of a substance to dissolve in a solvent. When the maximum amount of solute that can be dissolved is added to the solvent, the solution becomes saturated.

20. Solutions cont.
Concentration describes how much solute has been dissolved in solution
Concentration is represented as a ratio or percent
Solubility rate is affected by several factors (stirring/agitation, surface area, temperature
Raising temperature in a gas would decrease its ability to dissolve a solute

21. Solubility curves Unsaturated, supersaturated
If 110 grams of solute is dissolved in 100 grams of water at 70oC, at what point will the solute begin to precipitate?

22. Conductivity
In aqueous solutions, dissolved ionic compounds yield solutions with high conductivity (electrolyte)
Strong acids and bases are also strong electrolytes

23. Acids and Bases

24. pH scale – measures the acidity or basicity of a solution
pH scale – measures the acidity or basicity of a solution. >7 base, <7 acid
Compounds that give off hydrogen ions in solution are acids (hydronium)
Compounds that accept the hydrogen ions to form a salt are bases (hydroxide)
Acid + Base is a neutralization reaction resulting in the formation of a salt and water
Ex:

28. The density of aluminum is 2. 70 g/cm3
The density of aluminum is 2.70 g/cm3. A piece of aluminum foil has a volume of 54.0 cm3. What is the mass of this piece of aluminum foil? a. 146 g b g c g d g

29. The density of aluminum is 2. 70 g/cm3
The density of aluminum is 2.70 g/cm3. A piece of aluminum foil has a volume of 54.0 cm3. What is the mass of this piece of aluminum foil? a. 146 g b g c g d g

30. Which of the following is an example of a physical change. a
Which of the following is an example of a physical change? a. burning of methane gas produces water and carbon dioxide b. vinegar and baking soda combining to form a salt and water c. condensation of water vapor on the outside of a cold can of soda d. formation of silver sulfide when silver reacts with sulfur in the air

31. Which of the following is an example of a physical change. a
Which of the following is an example of a physical change? a. burning of methane gas produces water and carbon dioxide b. vinegar and baking soda combining to form a salt and water c. condensation of water vapor on the outside of a cold can of soda d. formation of silver sulfide when silver reacts with sulfur in the air

32. When copper reacts with oxygen in the air, a color change takes place, and the metal changes color from reddish brown to green. This green color is called a patina, and it has a different chemical composition from copper. What type of change occurs to produce a patina? a. dissolving b. conductivity c. physical change d. chemical change

33. When copper reacts with oxygen in the air, a color change takes place, and the metal changes color from reddish brown to green. This green color is called a patina, and it has a different chemical composition from copper. What type of change occurs to produce a patina? a. dissolving b. conductivity c. physical change d. chemical change

34. Examine the diagram. Which substance is the densest. a. lamp oil b
Examine the diagram. Which substance is the densest? a. lamp oil b. vegetable oil c. water d. honey

35. Examine the diagram. Which substance is the densest. a. lamp oil b
Examine the diagram. Which substance is the densest? a. lamp oil b. vegetable oil c. water d. honey

36. Which chemical equation is properly balanced. a. 4Ba(s) + S8(s)
Which chemical equation is properly balanced? a. 4Ba(s) + S8(s) 4BaS(s) b. 4HgO(s) 4Hg(l) + O2 c. 2FeO(s) + 4C(s) Fe(l) + S8CO2(g) d. SiI4(s) + 2Mg(s) Si(s) + 2MgI2(s)

37. Which chemical equation is properly balanced. a. 4Ba(s) + S8(s)
Which chemical equation is properly balanced? a. 4Ba(s) + S8(s) 4BaS(s) b. 4HgO(s) 4Hg(l) + O2 c. 2FeO(s) + 4C(s) Fe(l) + S8CO2(g) d. SiI4(s) + 2Mg(s) Si(s) + 2MgI2(s)

38. Which chemical equation represents a decomposition reaction. a
Which chemical equation represents a decomposition reaction? a. 8Bs(s) + S8(s) 8BaS(s) b. 6HgO(s) 6Hg(l) + 3O2(g) c. 2FeO(s) + C(s) 2Fe(s) + CO2(g) d. SiI4(s) + 2Mg(s) Si(s) + 2MgI2(s)

39. Which chemical equation represents a decomposition reaction. a
Which chemical equation represents a decomposition reaction? a. 8Bs(s) + S8(s) 8BaS(s) b. 6HgO(s) 6Hg(l) + 3O2(g) c. 2FeO(s) + C(s) 2Fe(s) + CO2(g) d. SiI4(s) + 2Mg(s) Si(s) + 2MgI2(s)

40. What is the coefficient on Al2O3 when the equation describing the following synthesis reaction is balanced? Al + O2 __Al2O3 a. 1 b. 2 c. 3 d. 6

41. What is the coefficient on Al2O3 when the equation describing the following synthesis reaction is balanced? Al + O2 __Al2O3 a. 1 b. 2 c. 3 d. 6

42. What is true in every balanced chemical equation. a
What is true in every balanced chemical equation? a. mass has to be conserved b. the reaction does not give off any energy c. all coefficients have to be an even number d. atoms are created when products are formed

43. What is true in every balanced chemical equation. a
What is true in every balanced chemical equation? a. mass has to be conserved b. the reaction does not give off any energy c. all coefficients have to be an even number d. atoms are created when products are formed

44. What type of arrangement and motion do particles in a liquid have. a
What type of arrangement and motion do particles in a liquid have? a. particles in liquid are closely packed together and vibrating b. particles in liquid are not in contact with each other and are moving very quickly c. particles in liquid are in contact with each other, but they are able to slip past one another d. particles in liquid are not in contact with one another and are moving at extreme speeds

45. What type of arrangement and motion do particles in a liquid have. a
What type of arrangement and motion do particles in a liquid have? a. particles in liquid are closely packed together and vibrating b. particles in liquid are not in contact with each other and are moving very quickly c. particles in liquid are in contact with each other, but they are able to slip past one another d. particles in liquid are not in contact with one another and are moving at extreme speeds

46. What phase change occurs when a solid changes directly into a gas. a
What phase change occurs when a solid changes directly into a gas? a. freezing b. melting c. evaporation d. sublimation

47. What phase change occurs when a solid changes directly into a gas. a
What phase change occurs when a solid changes directly into a gas? a. freezing b. melting c. evaporation d. sublimation

48. Which state of matter is characterized by neutral particles that have no definite volume and take the shape of the container in which they are placed? a. solid b. liquid c. gas d. plasma

49. Which state of matter is characterized by neutral particles that have no definite volume and take the shape of the container in which they are placed? a. solid b. liquid c. gas d. plasma

50. During the process of melting, what happens to the temperature of the substance? a. it stays constant b. it increases c. it decreases d. it increases and then decreases

51. During the process of melting, what happens to the temperature of the substance? a. it stays constant b. it increases c. it decreases d. it increases and then decreases

52. What law relates the temperature and volume of a gas at a constant pressure? A. Boyle’s law b. Charles’s law c. Gay-Lussac’s law d. Newton’s law

53. What law relates the temperature and volume of a gas at a constant pressure? A. Boyle’s law b. Charles’s law c. Gay-Lussac’s law d. Newton’s law

54. Xavier filled up a balloon to its maximum capacity inside his air-conditioned home. He walked outside into the intense summer heat. According to Charles’s Law, what could happen to his balloon? a. it could pop because the increase in temperature would cause an increase in volume b. it could pop because the increase in temperature would cause a decrease in pressure c. it could get smaller because the increase in temperature would cause a decrease in pressure d. it could get smaller because the increase in temperature would cause a decrease in volume

55. Xavier filled up a balloon to its maximum capacity inside his air-conditioned home. He walked outside into the intense summer heat. According to Charles’s Law, what could happen to his balloon? a. it could pop because the increase in temperature would cause an increase in volume b. it could pop because the increase in temperature would cause a decrease in pressure c. it could get smaller because the increase in temperature would cause a decrease in pressure d. it could get smaller because the increase in temperature would cause a decrease in volume

56. What law does the graph illustrate?
a. Boyle’s law b. Charles’s law c. Gay-Lussac’s law d. Newton’s law

57. What law does the graph illustrate?
a. Boyle’s law b. Charles’s law c. Gay-Lussac’s law d. Newton’s law

58. Which of the following graphs BEST illustrates Boyle’s law?

59. An unknown solution is tested using blue litmus paper
An unknown solution is tested using blue litmus paper. The blue litmus paper remains blue. What can be determined about the pH using this test? a. the pH is greater than 7 b. the pH is less than 7 c. the pH is 7 d. the pH cannot be determined

60. An unknown solution is tested using blue litmus paper
An unknown solution is tested using blue litmus paper. The blue litmus paper remains blue. What can be determined about the pH using this test? a. the pH is greater than 7 b. the pH is less than 7 c. the pH is 7 d. the pH cannot be determined

61. Four solutions are prepared in beakers
Four solutions are prepared in beakers. In all solution, 20g of sugar are added to 100ml of water. Beaker A is placed on the lab table at room temp (25oC). Beaker B is placed in the refrigerator. Beaker C is placed on a hot plate set at 40oC. In what order would the beakers be arranged to show the dissolving of sugar from fastest to slowest? a. A, B, C b. C, B, A c. C, A, B d. B, A, C

62. Four solutions are prepared in beakers
Four solutions are prepared in beakers. In all solution, 20g of sugar are added to 100ml of water. Beaker A is placed on the lab table at room temp (25oC). Beaker B is placed in the refrigerator. Beaker C is placed on a hot plate set at 40oC. In what order would the beakers be arranged to show the dissolving of sugar from fastest to slowest? a. A, B, C b. C, B, A c. C, A, B d. B, A, C

63. An unknown substance is dissolved in water
An unknown substance is dissolved in water. The solution is corrosive, conducts electricity, and has a higher concentration of H+ ions than OH- ions. What kind of solution does this unknown substance form? a. an acidic solution b. a basic solution c. a neutral solution d. a non-electrolyte solution

64. An unknown substance is dissolved in water
An unknown substance is dissolved in water. The solution is corrosive, conducts electricity, and has a higher concentration of H+ ions than OH- ions. What kind of solution does this unknown substance form? a. an acidic solution b. a basic solution c. a neutral solution d. a non-electrolyte solution

65. What happens to the solubility of a typical solid solute as temperature increases? a. the solubility decreases b. the solubility increases c. the solubility remains the same d. there is no way to know without knowing which exact solute

66. What happens to the solubility of a typical solid solute as temperature increases? a. the solubility decreases b. the solubility increases c. the solubility remains the same d. there is no way to know without knowing which exact solute

67. How does a phase diagram indicate when a substance is changing phase? a. the temperature rises during a phase change b. the temperature is constant during a phase change c. the temperature falls during a phase change d. the temperature changes 20 decreases Celsius during a phase change

68. How does a phase diagram indicate when a substance is changing phase? a. the temperature rises during a phase change b. the temperature is constant during a phase change c. the temperature falls during a phase change d. the temperature changes 20 decreases Celsius during a phase change

69. In which phase do the particles of a substance have the greatest freedom of motion? a. all phases have the same freedom of motion b. the gas phase c. the solid phase d. the liquid phase

70. In which phase do the particles of a substance have the greatest freedom of motion? a. all phases have the same freedom of motion b. the gas phase c. the solid phase d. the liquid phase