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Name: Class: _ Date: _ EOC review questions I Matching Match each item with the correct statement below. a. mixture d. reactant b. product e. heterogeneous mixture c. phase f. vapor 1. gaseous state of substance that is a liquid or solid at room temperature 2. a physical blend of two or more components 3. part of a sample having uniform composition and properties 4. not uniform in composition 5. a substance formed in a chemical reaction 6. starting substance in a chemical reaction Match each item with the correct statement below. a. distillation d. compound b. mass e. element c. chemical reaction f. homogeneous 7. amount of matter an object contains 8. describes mixture with a uniform composition 9. a process in which a liquid is boiled to produce a vapor that is condensed again into a liquid 10. substance that cannot be changed into simpler substances by chemical means 11. composed of two or more substances chemically combined in a fixed proportion 12. process in which substances are changed into different substances Match each item with the correct statement below. a. proton d. electron b. nucleus e. neutron c. atom 13. the smallest particle of an element that retains the properties of that element 14. a positively charged subatomic particle 15. a negatively charged subatomic particle 16. a subatomic particle with no charge 17. the central part of an atom, containing protons and neutrons 1

Name: Multiple Choice Identify the choice that best completes the statement or answers the question. 18. A horizontal row of the periodic table is usually referred to as a a. family. b. period. c. group. d. property. 19. Which of the following is a physical property? a. explosive b. combustible c. melting point d. ability to rust 20. Which state of matter has a definite volume and takes the shape of its container? a. solid b. liquid only c. gas only d. both b and c 21. Which state of matter expands when heated and is easy to compress? a. gas b. liquid only c. solid only d. both b and c 22. Which of the following is a physical change? a. corrosion b. explosion c. evaporation d. rotting of food 23. Which of the following can be classified as a mixture? a. pure water b. pure air c. pure nitrogen d. pure gold 24. Which of the following is a heterogeneous mixture? a. air b. salt water c. steel d. soil 25. A substance that can be separated into two or more substances only by a chemical change is a(n). a. solution b. element c. mixture d. compound 2

Name: 26. The chemical symbol for iron is _. a. fe b. FE c. Fe d. Ir 27. Which of the following is a chemical change? a. grating cheese b. melting cheese c. fermenting of cheese d. mixing two cheeses in a bowl 28. What must be done to be certain that a chemical change has taken place? a. Check for the production of bubbles before and after the change. b. Demonstrate that a release of energy occurred after the change. c. Check the composition of the sample before and after the change. d. Demonstrate that energy was absorbed by the reactants after the change. 29. What happens to matter during a chemical reaction? a. Matter is neither destroyed or created. b. Some matter is destroyed. c. Some matter is created. d. Some matter is destroyed and some is created. 30. The diameter of a carbon atom is 0.000 000 000 154 m. What is this number expressed in scientific notation? a. 1.54 10 12 m b. 1.54 10 12 m c. 1.54 10 10 m d. 1.54 10 10 m 31. The expression of 5008 km in scientific notation is. a. 5.008 10 3 km b. 50.08 10 4 km c. 5.008 10 3 km d. 5.008 10 4 km 32. The closeness of a measurement to its true value is a measure of its. a. precision b. accuracy c. reproducibility d. usefulness 3

Name: 33. Which of the following measurements contains two significant figures? a. 0.004 00 L b. 0.004 04 L c. 0.000 44 L d. 0.004 40 L 34. In the measurement 0.503 L, which digit is the estimated digit? a. 5 b. the 0 immediately to the left of the 3 c. 3 d. the 0 to the left of the decimal point 35. How many significant figures are in the measurement 0.003 4 kg? a. two b. four c. five d. This cannot be determined. 36. How many significant figures are in the measurement 811.40 grams? a. two b. three c. four d. five 37. What is the measurement 111.009 mm rounded off to four significant digits? a. 111 mm b. 111.0 mm c. 111.01 mm d. 110 mm 38. A conversion factor that shows the relationship between grams and kilograms is a. b. 1000 c. 1000 d. 39. What quantity is represented by the metric system prefix deci-? a. 1000 b. 100 c. 0.1 d. 0.01 40. What is the temperature 34 C expressed in kelvins? a. 139 K b. 207 K c. 239 K d. 339 K 4

Name: 41. Chlorine boils at 239 K. What is the boiling point of chlorine expressed in degrees Celsius? a. 93 C b. 34 C c. 61 C d. 34 C 42. What is the volume of 45.6 g of silver if the density of silver is 10.5 g/ml? a. 0.23 ml b. 4.34 ml c. 479 ml d. none of the above 43. Dalton's atomic theory included which idea? a. All atoms of all elements are the same size. b. Atoms of different elements always combine in one-to-one ratios. c. Atoms of the same element are always identical. d. Individual atoms can be seen with a microscope. 44. Which discovery did J. J. Thomson make that improved upon Dalton's atomic theory? a. Atoms contain tiny, negatively charged electrons. b. Atoms are always in motion. c. Atoms contain a tiny, positively charged nucleus. d. Atoms that combine do so in simple whole-number ratios. 45. All atoms are a. positively charged, with the number of protons exceeding the number of electrons. b. negatively charged, with the number of electrons exceeding the number of protons. c. neutral, with the number of protons equaling the number of electrons. d. neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons. 46. The particles that are found in the nucleus of an atom are. a. neutrons and electrons b. electrons only c. protons and neutrons d. protons and electrons 47. Which model of the atom is thought to be true? a. Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom. b. The nucleus is made of protons, electrons, and neutrons. c. Electrons are distributed around the nucleus and occupy almost all the volume of the atom. d. The nucleus is made of electrons and protons. 48. The atomic number of an element is the total number of which particles in the nucleus? a. neutrons b. protons c. electrons d. protons and electrons 5

Name: 49. The sum of the protons and neutrons in an atom equals the. a. atomic number b. nucleus number c. atomic mass d. mass number 50. What does the number 84 in the name krypton-84 represent? a. the atomic number b. the mass number c. the sum of the protons and electrons d. twice the number of protons 51. All atoms of the same element have the same. a. number of neutrons b. number of protons c. mass numbers d. mass 52. Isotopes of the same element have different a. numbers of neutrons. b. numbers of protons. c. numbers of electrons. d. atomic numbers. 53. In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly? a. In, 49 protons, 49 electrons b. Zn, 30 protons, 60 electrons c. Cs, 55 protons, 132.9 electrons d. F, 19 protons, 19 electrons 54. Using the periodic table, determine the number of neutrons in 16 O. a. 4 b. 8 c. 16 d. 24 55. How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125 contain? a. 50 protons, 50 electrons, 75 neutrons b. 75 electrons, 50 protons, 50 neutrons c. 120 neutrons, 50 protons, 75 electrons d. 70 neutrons, 75 protons, 50 electrons 6

Name: 56. Which of the following sets of symbols represents isotopes of the same element? a. 91 J 92 J 93 J 42 42 40 b. 50 L 50 L 50 L 19 20 21 c. 84 M 86 38 38 M 87 38 M d. 138 Q 133 59 55 Q 133 Q 54 57. How is the number of neutrons in the nucleus of an atom calculated? a. Add the number of electrons and protons together. b. Subtract the number of electrons from the number of protons. c. Subtract the number of protons from the mass number. d. Add the mass number to the number of electrons. 58. What unit is used to measure weighted average atomic mass? a. amu b. gram c. angstrom d. nanogram 59. The atomic mass of an element is the. a. total number of subatomic particles in its nucleus b. weighted average of the masses of the isotopes of the element c. total mass of the isotopes of the element d. average of the mass number and the atomic number for the element Short Answer 60. The following length measurements were taken by students using several different measuring devices. Find the average of the measurements. Make sure that your answer has the correct number of significant figures. 10.05 cm, 10.1 cm, 9.741 cm, 10.6 cm, 10.5 cm 61. Round off the measurement 0.003 095 5 m to three significant figures. 7

EOC review questions I Answer Section MATCHING 1. ANS: F PTS: 1 DIF: L1 REF: p. 37 OBJ: 2.1.3 Classify physical changes. 2. ANS: A PTS: 1 DIF: L1 REF: p. 38 OBJ: 2.2.1 Explain how mixtures are classified. 3. ANS: C PTS: 1 DIF: L1 REF: p. 39 OBJ: 2.2.1 Explain how mixtures are classified. 4. ANS: E PTS: 1 DIF: L1 REF: p. 39 OBJ: 2.2.1 Explain how mixtures are classified. 5. ANS: B PTS: 1 DIF: L1 REF: p. 48 OBJ: 2.4.1 Describe what happens during a chemical change. 6. ANS: D PTS: 1 DIF: L1 REF: p. 48 OBJ: 2.4.1 Describe what happens during a chemical change. 7. ANS: B PTS: 1 DIF: L1 REF: p. 34 OBJ: 2.1.1 Explain why all samples of a substance have the same intensive properties. 8. ANS: F PTS: 1 DIF: L1 REF: p. 39 OBJ: 2.2.1 Explain how mixtures are classified. 9. ANS: A PTS: 1 DIF: L1 REF: p. 40 OBJ: 2.2.2 Explain how mixtures can be separated. 10. ANS: E PTS: 1 DIF: L1 REF: p. 42 OBJ: 2.3.1 Explain the difference between an element and a compound. 11. ANS: D PTS: 1 DIF: L1 REF: p. 42 OBJ: 2.3.1 Explain the difference between an element and a compound. 12. ANS: C PTS: 1 DIF: L1 REF: p. 48 OBJ: 2.4.1 Describe what happens during a chemical change. 13. ANS: C PTS: 1 DIF: L1 REF: p. 102 OBJ: 4.1.1 Explain how Democritus and John Dalton described atoms. 14. ANS: A PTS: 1 DIF: L1 REF: p. 107 OBJ: 4.2.1 Identify three types of subatomic particles. 15. ANS: D PTS: 1 DIF: L1 REF: p. 105 OBJ: 4.2.1 Identify three types of subatomic particles. 16. ANS: E PTS: 1 DIF: L1 REF: p. 107 OBJ: 4.2.1 Identify three types of subatomic particles. 1

17. ANS: B PTS: 1 DIF: L1 REF: p. 108 OBJ: 4.2.2 Describe the structure of atoms according to the Rutherford model. MULTIPLE CHOICE 18. ANS: B PTS: 1 DIF: L1 REF: p. 46 OBJ: 2.3.4 Explain how a periodic table is useful. 19. ANS: C PTS: 1 DIF: L2 REF: p. 35 OBJ: 2.1.1 Explain why all samples of a substance have the same intensive properties. 20. ANS: B PTS: 1 DIF: L2 REF: p. 36 OBJ: 2.1.2 Identify the three states of matter. 21. ANS: A PTS: 1 DIF: L2 REF: p. 36 OBJ: 2.1.2 Identify the three states of matter. 22. ANS: C PTS: 1 DIF: L2 REF: p. 37 OBJ: 2.1.3 Classify physical changes. 23. ANS: B PTS: 1 DIF: L2 REF: p. 36 p. 44 OBJ: 2.3.1 Explain the difference between an element and a compound. 2.3.2 Distinguish between a substance and a mixture. 24. ANS: D PTS: 1 DIF: L2 REF: p. 39 OBJ: 2.2.1 Explain how mixtures are classified. 25. ANS: D PTS: 1 DIF: L2 REF: p. 42 OBJ: 2.3.1 Explain the difference between an element and a compound. 26. ANS: C PTS: 1 DIF: L2 REF: p. 46 OBJ: 2.3.3 Describe what chemists use to represent elements and compounds. 27. ANS: C PTS: 1 DIF: L2 REF: p. 48 OBJ: 2.4.1 Describe what happens during a chemical change. 28. ANS: C PTS: 1 DIF: L2 REF: p. 48 OBJ: 2.4.1 Describe what happens during a chemical change. 29. ANS: A PTS: 1 DIF: L1 REF: p. 50 OBJ: 2.4.3 Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 30. ANS: D PTS: 1 DIF: L2 REF: p. 62 OBJ: 3.1.1 Write numbers in scientific notation. 31. ANS: A PTS: 1 DIF: L2 REF: p. 62 OBJ: 3.1.1 Write numbers in scientific notation. 32. ANS: B PTS: 1 DIF: L1 REF: p. 64 OBJ: 3.1.2 Evaluate accuracy and precision. 33. ANS: C PTS: 1 DIF: L2 REF: p. 62 OBJ: 3.1.1 Write numbers in scientific notation. 2

34. ANS: C PTS: 1 DIF: L2 REF: p. 66 35. ANS: A PTS: 1 DIF: L2 REF: p. 67 36. ANS: D PTS: 1 DIF: L2 REF: p. 67 37. ANS: B PTS: 1 DIF: L2 REF: p. 68 p. 69 38. ANS: A PTS: 1 DIF: L2 REF: p. 85 OBJ: 3.3.1 Explain what happens when a measurement is multiplied by a conversion factor. 39. ANS: C PTS: 1 DIF: L2 REF: p. 75 OBJ: 3.2.1 Explain why metric units are easy to use. 40. ANS: C PTS: 1 DIF: L2 REF: p. 79 OBJ: 3.2.2 Identify the temperature units scientists commonly use. 41. ANS: D PTS: 1 DIF: L2 REF: p. 79 OBJ: 3.2.2 Identify the temperature units scientists commonly use. 42. ANS: B PTS: 1 DIF: L2 REF: p. 80 OBJ: 3.2.3 Calculate the density of a substance. 43. ANS: C PTS: 1 DIF: L2 REF: p. 102 OBJ: 4.1.1 Explain how Democritus and John Dalton described atoms. 44. ANS: A PTS: 1 DIF: L2 REF: p. 105 OBJ: 4.2.1 Identify three types of subatomic particles. 45. ANS: C PTS: 1 DIF: L3 REF: p. 107 OBJ: 4.2.1 Identify three types of subatomic particles. BLM: synthesis 46. ANS: C PTS: 1 DIF: L2 REF: p. 108 p. 109 OBJ: 4.2.2 Describe the structure of atoms according to the Rutherford model. 47. ANS: C PTS: 1 DIF: L2 REF: p. 109 OBJ: 4.2.2 Describe the structure of atoms according to the Rutherford model. 48. ANS: B PTS: 1 DIF: L1 REF: p. 112 49. ANS: D PTS: 1 DIF: L1 REF: p. 113 50. ANS: B PTS: 1 DIF: L2 REF: p. 115 OBJ: 4.3.2 Explain how isotopes of an element differ. 3

51. ANS: B PTS: 1 DIF: L2 REF: p. 112 52. ANS: A PTS: 1 DIF: L1 REF: p. 114 OBJ: 4.3.2 Explain how isotopes of an element differ. 53. ANS: A PTS: 1 DIF: L2 REF: p. 112 OBJ: 4.2.1 Identify three types of subatomic particles. 54. ANS: B PTS: 1 DIF: L2 REF: p. 113 55. ANS: A PTS: 1 DIF: L2 REF: p. 113 56. ANS: C PTS: 1 DIF: L2 REF: p. 115 OBJ: 4.3.2 Explain how isotopes of an element differ. 57. ANS: C PTS: 1 DIF: L2 REF: p. 113 58. ANS: A PTS: 1 DIF: L1 REF: p. 116 OBJ: 4.3.3 Calculate the atomic mass of an element. 59. ANS: B PTS: 1 DIF: L2 REF: p. 117 OBJ: 4.3.3 Calculate the atomic mass of an element. SHORT ANSWER 60. ANS: Average = (10.05 + 10.1 + 9.741 + 10.6 + 10.5) / 5 = 10.2 cm PTS: 1 DIF: L3 REF: p. 67 p. 70 p. 71 61. ANS: 0.003 10 m PTS: 1 DIF: L2 REF: p. 68 p. 69 4

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