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Honors Chemistry Exam Review Questions Chapter 1 1. Which of the substances listed could be considered inorganic? A methane, CH4 B rubbing alcohol, C3H7OH C D ammonia, NH3 candle wax, C25H52 2. A hypothesis is: A B C D an observation recorded from an experiment a proposed explanation for what is observed. a concise statement that summarizes the results of a broad variety of experiments. a thoroughly tested model. 3. Which of the following is not a part of the scientific method? A experimenting B observing C D proving hypothesizing 4. What does a red 4 mean on a chemical bottle? A extreme health hazard B not a health hazard C D extreme fire hazard not a fire hazard 5. Which piece of laboratory equipment would be best to use if you wanted to measure exactly 8.0 mL of water? A 100 mL beaker B 100 mL graduated cylinder C D 10 mL graduated cylinder 125 mL Erlenmeyer flask 6. If you spill an acid on the lab counter, what should you do first? A Clean it up with a paper towel B Tell your teacher immediately C D Pour water on it Scream at the top of your lungs 7. Identify the false statement: A A scientific law fully explains a natural phenomenon. B The scientific method is a logical, systematic approach to the solution of a problem. C For the results of an experiment to be accepted, the experiment must produce the same results no matter how many times it is repeated. D The scientific process is repeated until a hypothesis either fits all the observed experimental facts or is discarded. 8. What is the volume of the diagram to the right? A 25.2 mL B 25.24 mL C D 25.3 mL 25.28 mL 9. Which of these components of scientific research involves stating a relationship but not proposing an explanation of the relationship? A observation B scientific law C D theory hypothesis Chapter 2 10. How many of the zeros in the measurement 0.000040200 m are significant? A 2 B 3 C D 7 8 C D 2.5 x 10-4 mg 2.5 x 106 mg 11. How many milligrams are in 2.5 kg? A 2.5 x 10-6 mg B 25 mg 12. What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL? A 86 mL B 0.012 mL C D 0.025 mL 42 mL 13. The temperature reading of -14oC corresponds to a Kelvin reading of : A 297.6 K B -287 K C D 287 K 259 K 14. Concentrated hydrochloric acid has a density of 1.19 g/mL. What is the mass, in grams, of 2.00 liters of this acid? A 2.38 x 103 g B 2.38 g C D 4.20 x 104 g 4.20 x 10-4 g 15. A student measures a volume as 25 mL, whereas the correct volume is 23 mL. What is the percent error? A 0.087% B 8.7% C D 0.92% 8.0% 16. Which of the following is the correct scientific notation for 0.00000862? A 86.2 x 107 km B 8.62 x 106 km C D 86.2 x 10-7 km 8.62 x 10-6 km 17. How many significant figures are in the measurement 603.040? A 3 B 4 C D 5 6 18. Which of these equalities is correct? A 1 g = 1000 kg B 1 cm = 100 m C D 1 L = 1000 mL 1 mm = 10 cm 19. Four kilometers are equal to how many centimeters? A 4.0 x 10-3 cm B 4.0 x 105 cm C D 4.0 x 10-5 cm 1.0 x 103 cm 20. A conversion factor: A B C D is equal to 1 is a ratio of equivalent measurements does not change the value of a measurement all of the above 21. Among the measurements given, which is the smallest? A 470 mm B 5.1 x 10-4 km C D 3.2 m 52 cm 22. The mass of an apple is approximately 125 grams. What conversion factor would you use to express its mass in kilograms? A 100 kg/1 g B 1000 g/1 kg C D 1 kg/1000 g 1 g/100 kg 23. How many feet per second are there in 85 miles per hour? A 120 ft/sec B 58 ft/sec C D 140 ft/sec 7500 ft/sec 24. How many cubic micrometers are there in 3.25 x 10-7 L? A B 25. How many cubic centimeters are contained in a volume of 4.25 L? A 4.25 x 102 cm3 B 4.25 x 10-3 cm3 C D 4.25 x 103 cm3 4.25 x 10-2 cm3 Chapter 3 26. All of the following are physical properties of a substance in the liquid state except: A definite volume B able to flow C D not easily compressed definite shape 27. Homogeneous mixtures: A B C D consist only of liquids consist of two or more phases have a varying composition are known as solutions 28. A compound A B C D is a pure substance has a variable composition can be physically separated into its elements has properties similar to those of its elements 29. Physical properties of a substance include: A color and solubility B melting and boiling points C D density and odor all of the above 30. Which term does not fit with the others listed? A ice B steam C D salt water 31. Which of the following is an example of a physical change? A bread molding B burning a hamburger C D digesting a banana melting butter 32. An example of a heterogeneous mixture would be: A sugar B salt water C D tap water vegetable soup 33. A method of separating a mixture based on the difference in particle size is called A chromatography B filtration C D distillation magnetism C D oxygen water 34. Which of the following is a compound? A carbon B hydrogen 35. Which of the following can best distinguish a physical change from a chemical change? A energy is absorbed or released B a color change occurs C D a gas is produced mass is conserved 36. Which of the following changes of state are endothermic? A gas liquid B liquid gas C D gas solid liquid solid 37. Which of the following is an example of a chemical change? A rotting meat B slicing cheese C D dissolving sugar in iced tea freezing water 38. How much heat is absorbed when 20.0 grams of water is heated from 25.0oC to 39.0oC? A 380. J B 1590 J C D 1170 J 2090 J 39. What is the specific heat of a 35.0 gram sample of a metal that gives off 825 J of energy when the cools from 95oC to 25oC. A 0.589 J/goC B 0.403 J/goC C D 0.672 J/goC 0.337 J/goC Chapter 4 40. Which of the following is not a part of Dalton’s atomic theory? A B C D all elements are composed of atoms atoms of the same element are alike atoms are always in motion atoms that combine do so in simple whole-number ratios 41. The nucleus of an atom is: A B C D negatively charged and has a low density negatively charged and has a high density positively charged and has a low density positively charged and has a high density 42. Dalton theorized that atoms are indivisible and that all atoms of an element are identical. Scientists now know that: A B C D Dalton’s theories are completely correct. atoms of an element can have different numbers of protons. atoms are all divisible all atoms of an element are not identical but they all have the same mass 43. The number of neutrons in the nucleus of an atom can be calculated by A adding together the numbers of electrons and protons. B subtracting the number of protons from the number of electrons. C subtracting the number of protons from the mass number D adding the mass number to the number of protons 44. The sum of the protons and neutrons in an atom equals the: A atomic number B number of electrons C D atomic mass mass number 45. All atoms of the same element have the same: A number of protons B number of neutrons C D mass number mass 46. An atom of an element with atomic number 48 and mass number 120 contains: A B C D 48 protons, 48 electrons, and 72 neutrons 72 protons, 48 electrons, and 48 neutrons 120 protons, 48 electrons, and 72 neutrons 72 protons, 72 electrons, and 48 neutrons 47. Which of the following statements is not consistent with the results obtained in Rutherford’s gold foil experiment? A B C D the nucleus of an atom is positively charged the nucleus of an atom contains mostly all the mass of the atom atoms are composed mainly of empty space electrons are contained in the nucleus of an atom 48. The identity of an element can be determined on the basis of which of the following? A B C D the number of protons in an atom of the element the number of neutrons in an atom of the element the mass number of the element the atomic mass of the element 49. Isotopes of the same element have: A B C D the same number of protons but different numbers of neutrons the same number of protons but different numbers of electrons the same number of neutrons but different numbers of protons the same number of neutrons but different numbers of electrons 50. In general, metals are: A ductile B malleable C D good electrical conductors all of these C D oxygen copper 51. Which of the following is a nonmetal? A iron B silver 52. Three isotopes of oxygen occur in nature: oxygen-16, oxygen-17, and oxygen-18. If the atomic mass of oxygen is 15.994, which of the three isotopes, if any, is the most abundant? A oxygen-16 B oxygen-17 C D oxygen-18 all are equally abundant Chapter 28 53. Which of the following is not true concerning an alpha particle? A It has a mass of 4 amu B It has a +1 charge C D It is a helium nucleus It contains two neutrons 54. A piece of wood found in an ancient burial mound contains one-fourth as much carbon-14 as a piece of wood cut from a living tree growing nearby. If the half-life of carbon-14 is 5730 years, what is the approximate age of the ancient wood? A 1432.5 years B 2865 years C D 5730 years 11460 years 55. If an isotope undergoes beta emission: A B C D the mass number changes the atomic number changes the atomic number remains the same the number of neutrons remains the same 56. Which of the following particles is needed to complete this nuclear equation? 54 2 1 25Mn + 1H _____ + 0n A B 56 27Co 57 26Fe C D 55 26Fe 58 24Cr 57. In nuclear fission: A B C D certain atoms break into fragments when struck by neutrons a chain reaction cannot occur energy is absorbed all of these 58. Nuclear fusion: A B C D occurs when large nuclei fuse together takes place in the sun generally produces hydrogen nuclei all of these 59. What particle is needed to complete this equation? 14 14 1 7 N + _____ 6C + 1H 1 4 A 0n C 2He 0 0 C -1e D +1e 60. Which of the following is always true about radioisotopes? A B C D They have unstable nuclei Their neutron-to-proton ratio is 1:1. Their decay products are stable isotopes all of these 61. Which of the following types of radiation has no mass and no charge? A alpha B beta C D gamma positron 62. When U-238 undergoes radioactive decay by losing an alpha particle, the other product is: A U-234 B Th-234 C D Pu-234 U-242 Chapter 5 63. What is the ionic charge on the chromium ion in the ionic compound that has the formula Cr2O3? A +3 B -2 C D -5 +5 64. Which element when combined with chlorine would most likely form an ionic compound? A lithium B carbon C D phosphorus bromine 65. Choose the correct formula for calcium hydrogen phosphate? A CaHPO4 B Ca2HPO4 C D Ca(H2PO4)2 Ca(HPO4)2 66. Compounds that are composed of ions: A B C D are molecular compounds are generally crystalline solids at room temperature are for the most part composed of two or more metallic elements all of the above 67. The cation Fe+3 is formed when: A B C D an atom of iron loses two electrons an atom of iron gains two electrons an atom of iron loses three electrons an atom of iron gains three electrons 68. What is the total number of atoms in one molecule of C6H12O6? A 3 B 12 C D 18 24 69. Name the following compound: Fe2(CO3)3 A Iron (III) carbonate B Diiron (III) tricarbonate C D Iron (II) carbonate Diron (II) tricarbonate 70. What is the formula for trinitrogen heptachloride? A N2Cl7 B N4Cl6 C D N3Cl6 N3Cl7 71. The name of Copper (II) nitrate A Cu(NO3)2 B CuNO3 C D Cu(NO3)2 CuNO3 72. Among the following, which combination would be most likely to form an ionic compound? A H and O C S and Cl C D Na and I Si and O 73. The nonmetals in Groups 15,16, and 17: A B C D lose electrons when they form ions form positively charged ions form ions with charges -3, -2, and -1, respectively form ions with a numerical charge equal to their group number 74. Among the following, which atom is most likely to form an ion with a charge of +2? A O B Na C D Al Ca 75. What is the name of the following compound: (NH4)2S2O3? A Ammonium sulfate B Ammonium thiosulfate C D Nitrogen hydrogen thiosulfate Ammonium disulfate C D H2C2O4 H2CO3 76. What is the formula for Oxalic acid? A HC2O4 B H2CO3 77. Name the following compound: Fe3(PO4)2 A Iron (III) phosphate tetrahydrate B Iron (II) phosphite tetrahydrate C D . 4 H2O Iron (II) phosphate tetrahydrate Iron (II) phosphate trihydrate 78. Among the following, which is a binary molecular compound? A CO2 B NaCl C D FeO MgS Chapter 8 79. The chemical formula of aspirin is C9H8O4. What is the mass of 0.200 mol of aspirin? A 22.5 g B 5.4 g C D 80 g 36.0 g 80. How many moles of SO3 are in 2.4 x 1024 molecules of SO3? A 0.25 B 3.4 x 1022 C D 4.0 2.9 x 10-23 81. The representative particle for nitrogen gas (N2) is: A an atom B a molecule C D a formula unit none of these C D 125.8 g/mol 76.4 g/mol 82. What is the molar mass of MgCl2? A 59.8 g/mol B 95.3 g/mol 83. How many atoms of aluminum are present in a 0.275 mole sample of Al2(CO3)3? A 1.66 x 1023 atoms B 4.38 x 1024 atoms C D 3.31 x 1023 atoms 2.19 x 1024 atoms 84. How many grams of Ba(IO3)2 are there in a 1.25 x 1022 formula unit sample of Ba(IO3)2? A 14.1 grams B 101 grams C D 6.48 grams 10.1 grams 85. Find the number of moles in 3.30 g of (NH4)2SO4? A 132.1 mol B 40.0 mol C D 0.0279 mol 0.0250 mol 86. What is the volume (in liters at STP) of 2.50 mol of carbon monoxide? A 0.112 L B 3.10 L C D 56.0 L 8.96 L 87. Which of the following is not an empirical formula? A Na2SO4 B C6H5Cl C D N2H4 Sn3(PO4)4 88. A compound has the empirical formula C2H3O and a molar mass of 172.0 g/mol. What is its molecular formula? A C6H9O3 B C8H12O4 C D C9H16O3 C7H8O5 89. Determine the number of moles in 625 L of H2 gas at STP? A 3.58 x 10-2 mol B 27.9 mol C D 1.40 x 104 mol 1250 mol 90. What is the percent of aluminum in Al2(SO4)3? A 28.1% B 54.0% C D 15.8% 56.7% 91. What is the empirical formula of a compound that is 3.05% carbon, 0.26% hydrogen, and 96.96% iodine? A C2HI7 B CH2I5 C D C3H2I11 CHI3 92. The following would be classified as which type of reaction? CH4 + 2 O2 CO2 + 2 H2O A B C D synthesis combustion single displacement double displacement 93. Which of the following describes the products of a double displacement reaction? A B C D carbon dioxide and water a single product an element and a compound two ionic compounds 94. When the following equation is balanced, what is the coefficient that goes with water? _____ Mn(OH)3 + _____ H2SO3 _____ Mn2(SO3)3 + _____ H2O A B C D 2 3 6 12 Midterm Exam Sample Free Response Questions For the following problems, SHOW ALL OF YOUR WORK! Include units in all of your answers, and round each answer off to the correct number of significant figures, where necessary. 1. Convert 84.3 gallons per square milligram to cubic nanometers per square pounds 2. How many formula units of Mn(NO3)2 are there in 28.9 grams of Mn(NO3)2? Show your set up for determining molar mass. How many moles of nitrogen are present? How many atoms of oxygen as present in the sample? 3. Fill in the following table Atomic # Mass # # protons #neutrons #electrons charge AZ ________ _________ ___54____ _____ __128__ ___52___ 4. Name the following compounds Cr(NO3) 3 ___________________________ NaHCO3 ___________________________ P4Cl7 ___________________________ H2SO4 ___________________________ Fe4C3 2 H2O__________________________ Xcharge __________ Write the formula for the following compounds Aluminium hydrogen sulfite ____________________________ Trinitrogen hexasulfide ____________________________ Copper (I) thiosulfate ____________________________ Perchloric acid ____________________________ Auric dichromate octahydrate ____________________________ 5. The specific heat of a metal is 0.486 J/goC. What is the mass of the metal when a sample of the metal absorbs 625 J of energy when it is heated from 25.0oC to 96.0oC? Assume that all of the energy lost by the metal is gained by the water. (Cp of water = 4.18 J/goC).