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Honors Chemistry Midterm 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. 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 3. 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 4. 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 5. 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 C D 2.5 x 10-4 mg 2.5 x 106 mg Chapter 2 6. How many milligrams are in 2.5 kg? A 2.5 x 10-6 mg B 25 mg 7. The temperature reading of -14oC corresponds to a Kelvin reading of : A 297.6 K B -287 K C D 287 K 259 K 8. 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 9. 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% 10. How many significant figures are in the measurement 603.040? A 3 B 4 C D 5 6 11. 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 12. 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 13. 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 14. 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 15. 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 16. Physical properties of a substance include: A color and solubility B melting and boiling points C D density and odor all of the above 17. 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 18. An example of a heterogeneous mixture would be: A sugar B salt water C D tap water vegetable soup 19. A method of separating a mixture based on the difference in particle size is called A chromatography B filtration C D distillation magnetism 20. Which of the following changes of state are endothermic? A gas liquid B liquid gas C D gas solid liquid solid 21. 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 22. 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 23. 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 24. 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 25. 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 26. 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 27. 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 28. 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 29. 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 30. In general, metals are: A ductile B malleable C D good electrical conductors all of these C D oxygen copper 31. Which of the following is a nonmetal? A iron B silver 32. 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 18 33. 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 34. 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 35. Which of the following particles is needed to complete this nuclear equation? 54 25Mn A B 56 27Co 57 26Fe + 21H _____ + 10n C D 55 26Fe 58 24Cr 36. 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 37. Nuclear fusion: A B C D occurs when large nuclei fuse together takes place in the sun generally produces hydrogen nuclei all of these 38. What particle is needed to complete this equation? 14 7N A B 1 0n 0 -1e + _____ 146C + 11H C D 4 2He 0 +1e 39. 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 40. 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 41. Which element when combined with chlorine would most likely form an ionic compound? A lithium B carbon C D phosphorus bromine 42. Choose the correct formula for calcium hydrogen phosphate? A CaHPO4 B Ca2HPO4 C D Ca(H2PO4)2 Ca(HPO4)2 43. 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 44. What is the total number of atoms in one molecule of C6H12O6? A 3 B 12 C D 18 24 45. Name the following compound: Fe2(CO3)3 A Iron (III) carbonate B Diiron (III) tricarbonate C D Iron (II) carbonate Diron (II) tricarbonate 46. What is the formula for trinitrogen heptachloride? A N2Cl7 B N4Cl6 C D N3Cl6 N3Cl7 47. The formula of Copper (II) nitrate is: A Cu(NO3)2 B CuNO3 C D Cu(NO3)2 CuNO3 48. 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 49. 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 50. 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 51. 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 52. What is the formula for Oxalic acid? A HC2O4 B H2CO3 53. 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 54. Among the following, which is a binary molecular compound? A CO2 B NaCl C D FeO MgS Chapter 8 55. 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 56. What is the molar mass of MgCl2? A 59.8 g/mol B 95.3 g/mol 57. 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 58. 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 59. 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 60. 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 61. Which of the following is not an empirical formula? A Na2SO4 B C6H5Cl C D N2H4 Sn3(PO4)4 62. 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 63. 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 64. What is the percent of aluminum in Al2(SO4)3? A 28.1% B 54.0% C D 15.8% 56.7% 65. 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 Chapter 6 66. 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 67. 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 68. 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 Chapter 7 69. The reaction in question 70 is an example of a(n): A decomposition B synthesis C D single displacement combustion 70. In a double displacement reaction: A B C D one of the products is always a gas one of the products must be an element positive ions are exchanged between two compounds all of the above 71. Water is always a product in: A B combustion reactions decomposition reactions C D single-displacement reactions decomposition reactions 72. The following would be classified as which type of reaction? CH4 + 2 O2 CO2 + 2 H2O A B synthesis single displacement C D combustion double displacement 73. Which of the following describes the products of a synthesis reaction? A B carbon dioxide and water C an element and a compound D a single product two ionic compounds 74. O2, N2, Cl2, and I2 are examples of— A B diatomic molecules ionic compounds C D compounds atoms 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. A metal has a mass of 88.4 grams and an initial temperature of 106.2oC. The heated metal is then placed into 25.9 grams of water with an initial temperature of 23.4oC. The final temperature of the metal and the water is 26.7oC. What is the specific heat of the metal, assuming that all of the heat lost by the metal is gained by the water? 6. Predict the products of the following equations given their reactants along with the type of reaction for each equation. ___C2H5OH + ___ O2 ___ CO2 + ___ H2O Type: ___Pb(NO3)2 + ___K3PO4 ___Pb3(PO4)2 + ___KNO3 Type: ___Zn + ___HClO3 ___ H0 + Zn(ClO3)2 Type: ___Na + ___FeBr3 ___ NaBr + Fe Type: 7. Caffeine, a stimulant found in coffee, contains 49.5% C, 5.15% H, 28.9% N and 16.5% O. The molecular formula has a molar mass of 194.22 g/mol. Determine the empirical and molecular formulas for caffeine. 8. Fill in the blanks for the following nuclear decay: 115In 3protons 2 3 neutrons 3