Fall Semester Review

Fall Semester Review Chapter.1: Match the Lab equipment below to the proper letter.

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1. What are 2 qualitative and 2 quantitative characteristics about you?

Scientific Method and Variables Slimotosis Sponge Bob notices that his pal Gary is suffering from slimotosis, which occurs when the shell develops a nasty slime and gives off a horrible odor. His friend Patrick tells him that rubbing seaweed on the shell is the perfect cure, while Sandy says that drinking Dr. Kelp will be a better cure. Sponge Bob decides to test this cure by rubbing Gary with seaweed for 1 week and having him drink Dr. Kelp. After a week of treatment, the slime is gone and Gary’s shell smells better.

2. What was the initial observation? 3. What is the independent variable?

Fall Review 2009 CHEM 4. What is the dependent variable? 5. What should Sponge Bob’s conclusion be? ======

Chapter 2 6. A piece of metal with a mass of 147 g is placed in a 50-mL graduated cylinder. The water level rises from 20 mL to 41 mL. What is the density of the metal?

Metric Chart Prefix Abbreviation Definition Tera T 1012 or 1,000,000,000,000 Giga G 109 or 1,000,000,000 Mega M 106 or 1,000,000 Kilo k 103 or 1,000 BASE L, m, or g 100 or 1 Deci d 10-1 or 0.1 Centi c 10-2 or 0.01 Milli m 10-3 or 0.001 µ (Greek letter Micro 10-6 or 0.000001 mu) Nano n 10-9 or 0.000000001

7. How does adding the prefix, “mega” to a unit affect the quantity?

8. Which is the larger unit a. nm or mm? b. kL or L? c. Gg or ng? d. g or dg?

9. How many… a. Megameters in 1 meter? ______b. dg in 1 cg? ______c. mm in 1 m? ______d. kL in 1 cL? ______

Metric conversions: Perform the following SI prefix conversions: 10. 25 kg = g 11. 9.3 mL = L 12. 0.36 mm = m 13. 24 cm = km

14. How many kilometers are there in 3.4 miles?

Fall Review 2009 CHEM Scientific Notation:

Part I. Change the following numbers to proper scientific notation 15) 65.7 16) 0.00545 17) 22 450 000 Part II. Change the following numbers to standard notation 18) 8.85 x 104 19) 1.847 x 102 20) 3.400 x 10-3

Significant Figures

Identify the number of significant digits show in each of the following examples.

21) 400 22) 200.0 23) 0.0001 24) 218

T-chart problems: 25. How many seconds are there in 24 hours?

26. A paper clip is 3.2 cm long. What is its length in millimeters?

27. A quart is approximately equal to 946 mL. How many liters are in 1 quart?

28. . Accuracy and Precision

Density: 29. . You have a 23-g sample of ethanol with a density of 0.7893 g/mL. What volume of ethanol do you have?

Chapter 3:

CLASSIFICATION OF MATTER Classify the following as element (E), compound (C), heterogeneous mixture (H), or solution (S). 30. hydrogen gas 31. orange juice 32. clean air

33. carbon dioxide (CO2)

Classify the following as chemical changes (C) or physical changes (P).

Fall Review 2009 CHEM 34. grapes fermenting 35. copper melting 36. recycling aluminum 37. gasoline exploding

Chapter 4

Complete the following chart and answer the questions below.

Element Atomic Number of Number of Mass Number Name Number Protons Neutrons

Carbon 12

Hydrogen 1

Hydrogen 2

Nitrogen 14

38. Hydrogen appears twice on the table above. These two types of hydrogen are called ______. 39. The Scientist who proposed the plum pudding model of the atom? ______40. The scientist who discovered the nucleus is ______

Fall Review 2009 CHEM 41. Draw a picture of what each scientist thought the atom looked like

Define: 42. physical property and give an example______43. physical change and give an example______44. chemical property and give an example______45 chemical change and give an example______

46. The shape of an apple is a ______. a. chemical change b. chemical property c. physical change d. physical property

47. Define: mixture and give an example______Define pure substance and give an example______

48. A student took a beaker containing a colorless liquid and evaporated the liquid. After the liquid had evaporated, she observed a white, crystalline solid in the beaker. From these observations, she would conclude that the original liquid was ______. a. A mixture b. A metal c. An element d. A compound

49. A beaker contains a mixture of salt and sand. How can the mixture be separated? a. Use a magnet. b. Pick the sand out of the salt with forceps. c. Dissolve in water, filter, and collect salt on filter paper. d. Dissolve in water, filter, and collect sand on filter paper, evaporate water with Bunsen burner

Use the following diagram to answer questions 4 & 5.

50. The diagram above shows the same substance in different states of matter (A, B, C,). Which of the following statements is a true interpretation of the diagram? a. The particles in “A” exhibit absolutely no motion. b. The particles in “B” occupy the entire volume of the container c. The particles in “C” represent the gaseous state. d. The particles in “B” represent the condensed state of the particles in “A”.

Fall Review 2009 CHEM 51. Which statement correctly describes the compressibility of solids, liquids, and gases? a. Solids, liquids, and gases cannot be compressed. b. Solids, liquids, and gases can all be greatly compressed. c. Solids and gases can all be greatly compressed; liquids cannot be greatly compressed. d. Solids and liquids cannot be greatly compressed; gases can be greatly compressed.

The following is a list of observations from the lab activity.

“Observing a Chemical Reaction”

Step 1: The crystals are small in size. The crystals are dark blue-green in color.

Step II: The crystals on the bottom of the beaker are green. The solution above the crystals becomes pale blue. After a few minutes, the solution just above the crystals becomes dark green.

Step III: The crystals dissolve readily to give a blue-green solution. The foil disintegrates in acid solution rapidly. A gas is given off. A red-brown precipitate drops to the bottom of the beaker. The final temperature is 83.5◦ C.

52. Which step(s) of the lab involve(s) a chemical change? a. steps I and II b. step II c. step III d. steps I, II, and III

53. Write the equation for density______

54. Rearrange the density equation to solve for mass______

Rearrange the density equation to solve for volume______

55. An irregularly shaped solid object made of copper is placed into a graduated cylinder containing water. The density of copper is 8.96 g/ml. The volume of the irregularly shaped object would be______.

56. The volume of another copper object is found to be 13.0 ml. (density = 8.96 g/ml). The mass of this object, calculated to the correct number of significant digits, would be______. 57.

Fall Review 2009 CHEM A group of students collected samples of equal volume of several different liquids, such as dish detergent, vinegar, molasses, and shampoo. They placed the liquids in identical graduated cylinders and measured the amount of time it took for a marble to drop from the top of the liquid to the bottom. What are the students measuring? ______

58. How many electrons does an atom of element atomic number 97 contain? ______

59. The nucleus of an atom has a______charge?

60. All atoms of the same element have the same ______.

61. An isotope of bromine (Br) has 40 neutrons. What is the mass number for this isotope?______

62. To determine the mass of an element, you must consider the______of every isotope of that element. atomic mass atomic number isotopic mass electron charge

63. Define: isotope______

64. The isotope Carbon – 14 is also written as ______

64. 14 Using 6 C , how many protons______, neutrons______, and electrons______are in this isotope?

65. Which notations represent an isotope of the element Chlorine? ______35 35 37 17 I. 17 Cl II. 18 Cl III. 17 Cl IV. 35Cl

66. If the mass of KClO3 is 245.2 grams and the mass of Oxygen formed is 96 grams. What mass of KCl is produced?_____

Use the diagram below to answer questions

Fall Review 2009 CHEM 67. In the beaker below, what evidence is there of a change? It is a chemical or physical change?

Conservation of Mass problems:

68. Household ammonia is made from nitrogen and hydrogen. If 55 grams of ammonia is formed, how many grams of reactant are needed?

69. In a galaxy far, far away, compounds are made from only two elements: lint and spit. If 2 grams of lint form 8 grams of the compound lint-spit, how many grams of spit were needed?

70. When hydrogen peroxide decomposes, it gives off oxygen and hydrogen gas. When 101 grams is decomposed in a beaker, 0 grams of hydrogen peroxide are left behind. Does this violate the law of conservation of mass? Where did all the hydrogen peroxide go?

71. Element B combines with element A to form the compound AB. If 18 grams of AB are formed, and 9 grams of B was used, how much A is needed?

72. When baking soda reacts with vinegar, gas is formed. If 10 g of baking soda is reacted with 5 grams of vinegar, and the product only weighs 12 grams, does the reaction violate the law of conservation of mass? Why or why not?

Fall Review 2009 CHEM