1. Which is a pure substance? A) table salt B) bronze C) air D) soil 2. A tentative explanation of certain facts that provides the basis for further experimentation is a(n) A) observation B) hypothesis C) theory D) law 3. A well established hypothesis is often called a(n) A) observation B) fact C) theory D) law 4. When expressed in proper scientific notation the number 0.000034 is A. 3.4 X 10 4 B. 3.4 X 10-4 C. 3.4 X 10 3 D. 3.4 X 10-5 5. The density of copper is 8.96g/mL. The mass of 7.00 ml of copper is A. 62.7g B. 1.28g C. 0.781g D. 1.96g 6. Perform the following set of operations and choose the alternative that expresses the result to the proper number of significant figures. 65.43-43.2 A. 1.80 x 10 4 B. 1.804 x 10 4 C. 1.80 x 10 4 D. 1.8 x 10 4 1.232 x 10-3 7. Convert 12.5 m 3 to cm 3. A. 1.25 x 10 3 cm 3 B. 1.25 x 10 7 cm 3 C. 1.25 x 10 5 cm 3 D. 1.25 x 10 3 cm 3 8. At room temperature the majority of metals exist as A. vapors. B. solids. C. gases. D. liquids. 9. The halogens are in group A. 1 B. 2 C. 13 D. 17 10. What is the symbol of the element that is classified as an alkali metal and is in period 4? A. Ca B. K C. Br D. Na 11. Which is not a physical property of water? A. Water is colorless. B. The freezing point of water is 0 º Celsius. C. Water reacts with sodium metal to produce sodium hydroxide and hydrogen. D. The density of water at 4 º C is 1.00g/mL. 12. How many joules of energy are released when 45.0 g of water cools from 18.0 º C to 7.0 º C? A. 495 J B. 791 J C. 2860 J D. 2070 J
13. The specific heat of iron is 0.473 J/g º C and the specific heat of lead is 0.128 J/g º C. In order to raise the temperature of one gram of those metals by one degree Celsius, A. both metals require the same amount of energy. B. the iron requires more energy than the lead. C. the lead requires more energy than the iron. D. no correct answer is given. 14. The specific heat of aluminum is 0.900 J/g º C. A 300.0g sample of aluminum at 300.0 º C is dropped into 200.0g of water at 20.0 º C. Assume no heat is lost to the environment. Remember QlostAl=QgainedH2O; -mcδtal=mcδth2o A. What will be the final temperature of the water? B. What will be the final temperature of the aluminum? 15. The electrical charge of a nucleus is A. positive. B. negative. C. the nucleus has no charge, it is neutral. 16. Atoms of isotopes of an element contain the same number of A. protons. B. neutrons. C. alpha particles. 17. Ions can be formed from atoms by losing or gaining electrons. Select the alternative that states the correct number of protons, neutrons, and electrons in 63 2 29 Cu. A. 29 protons, 34 neutrons, 31 electrons B. 29 protons, 34 neutrons, 27 electrons C. 27 protons, 29 neutrons, 29 electrons D. 29 protons, 63 neutrons, 29 electrons 18. What is the formula of copper(ii) oxide? A. CuO B. Cu2O C. CuO2 D. CuO3 19. Which is ammonia? (Table L) A. NH2 B. NH3 C. NH4 + D. Am 20. Na2SO3 is A. sodium sulfide. B. sodium sulfate. C. sodium sulfite. D. sodium(ii) sulfur. 21. Which of the following alternatives represents an incorrect name-formula match? A. calcium chlorate = Ca(ClO4)2 B. tin(ii) nitrate = Sn(NO3)2 C. sodium carbonate = Na2CO3 D. silver sulfate = Ag2SO4 22. What is the mass of 0.118 moles of AgNO3? A. 0.118 g B. 0.710g C. 7.10 10 23 g. D. 20.0g
23. How many molecules are present in 0.340g of HCl? A. 1.78 10-22 B. 6.46 10 25 C. 5.61 10 21 D. 2.06 10-23 24. What is the mass of 3.01 10 24 molecules of Cl2? A. 137g B. 14.2g C. 213g D. 355g D. 2 29. The formula of the salt produced from the double-displacement reaction between HNO3 and Ba(OH)2 is: A. H2O B. NO3OH C. Ba(NO3)2 D. Ba(OH)2 30. Change these word equations into balanced chemical equations. A. Carbon plus oxygen yields carbon monoxide. 25. What is the percent by mass of hydrogen in H2SO4? A. 1.04% B. 2.06% C. 4.03% D. 5.93% 26. What is the empirical formula of a compound that consists of 39.99% carbon, 6.73% hydrogen, and 53.28% oxygen? A. CHO B. C2HO C. CH2O D. CHO2 27. What is the molecular formula of a compound with the empirical formula C13H19O2 and molar mass of 414.64g? A. CHO B. C13H19O2 C. C26H38O4 D. C39H57O6 28. Balance the following chemical equation using the smallest set of integers. The coefficient on NO2 is: HNO3 + S NO2 + H2SO4 + H2O A. 4 B. 6 C. 1 B. Sodium chlorate decomposes to form sodium chloride and oxygen. C. Fluorine and potassium bromide yields potassium fluoride and bromine. 31. Complete and balance the equation for each example in which a double replacement reaction will occur. A. AlBr3 + AgNO3 B. ZnBr2 + Na2S 32. What type of reaction does the following equation represent? Mg + CuCl2 MgCl2 + Cu A. synthesis C. decomposition
B. double replacement D. single replacement 33. How many grams of molecular chlorine will be required to completely react with 0.0223 moles of sodium iodide according to the following reaction? 2NaI + Cl2 2NaCl + I2 A. 1.57 10-4 grams B. 3.16 grams C. 0.0112 grams D. 0.791 grams 34. Calculate the number of moles of Br2 needed to completely react with 50.0 g of KI: 2KI + Br2 2KBr + I2 37. What mass of NH3 is produced when 1.20 moles of H2 react completely in the following equation? A. 34.1g B. 20.4g C. 13.6g D. 30.7g N2 + 3H2 2NH3 38. Which principal energy level will contain electrons with the lowest energy? A. First B. Second C. Third D. Fourth A. 5.44 moles B. 0.151 moles C. 0.0117 moles D. 0.162 moles 35. Based on the following chemical equation 4HCN(g) + 5O2(g) 2N2(g) + 4CO2(g) + 2H2O(g) Calculate how many liters of N2 that can be produced at STP when 105 g of HCN reacts. A. 43.6 L of N2 are produced B. 35.0 L of N2 are produced C. 51.8 L of N2 are produced D. 24.6 L of N2 are produced 36. How many units of K2SO4 are produced when 0.250 moles of K react completely in the following equation? 2K + MgSO4 K2SO4 + Mg A. 7.53 10 22 B. 3.01 10 23 C. 6.02 10 23 D. 1.51 10 23 39. What is a possible exited state electron configuration for the element beryllium? A. 2-2 B. 2-8-1 C. 2-8-8 D. 2-1-1 40. What is the maximum number of electrons that can occupy the third principal energy level? A. 2 B. 6 C. 8 D. 18 41. On the periodic table, elements in the same group contain the same number of A. protons. B. electrons. C. principal energy levels in their ground state. D. valence electrons in their ground state. 42. The electron configuration, 2-8-8-1, is the ground state electron configuration of A. potassium. B. phosphorous. C. fluorine. D. sodium.
43. Which element has four electrons in its valence shell? A. P B. Mg C. Cl D. Si 44. Which of the following statements is true for most atoms? A. In general, as the atomic radius increases, the first ionization energy increases. B. In general, as the atomic radius increases, the first ionization energy decreases. C. In general, as the first ionization energy decreases, the electronegativity increases. D. No correct answer is given. 45. Which element forms an ion that is larger than its atom? A. Lithium B. Calcium C. Chromium D. Chlorine 46. Which element forms an ion that is smaller than its atom? A. Strontium B. Sulfur C. Oxygen D. Fluorine 47. A bond that is principally covalent will form between A. potassium and oxygen. B. fluorine and oxygen. C. sodium and chlorine. D. aluminum and fluorine. 49. Which of the following does not have a noble gas electron configuration? A. S -2 B. Al +3 C. Sb D. Ar 50. Which structure represents the best Lewis structure for O2? A. B. C. D. 51. A sample of an unknown gas was isolated in a glass bulb. The volume of the bulb was 1.425 L. The temperature was 25.4 º C, and the pressure was 0.767 atm. What volume would this gas sample occupy at STP? A. 1.00 L B. 1.20 L C. 1.70 L D. 2.03 L 52. A sample of a gas occupies a volume of 185.5 ml at STP. What pressure would it exert if it is transferred to a gas bulb with a volume of 255.5 ml in which the temperature is maintained at 34.5 º C? A. 0.724 atm B. 0.818 atm C. 0.615 atm D. 1.40 atm 48. What is the number of valence electrons in an aluminum atom in the ground state? A. 1 C.3 B. 2 D. 4
53. Which of the following is a condition that must be met for a gas to be considered as ideal? A. The gas must contain carbon. B. The gas molecules must have no attractive forces. C. The gas sample must not contain water vapor. D. The gas sample must be enclosed in a large container. 54. The conversion of mass to energy is measureable only in A. chemiluminescent transformations. B. exothermic reactions. C. explosive chemical reactions. D. nuclear reactions. 55. What is the mass number of an alpha particle? A. 0 B. 2 C. 4 D. 1 57. Identify the missing species in the nuclear equation: Ir + e? A. B. C. D. 193 Ir 76 193 Ir 77 192 Os 76 193 Os 76 193 0 77-1 58. Ytterbium-175 is a -emitter with a half-life of 101 hours. How long would it take for a sample of this isotope to decay to exactly 1/8 th of its original value? A. 303 hours B. 225 hours C. 356 hours D. 202 hours 56. The nuclear radiation with the least penetrating ability is: A. alpha radiation. C. gamma radiation B. beta radiation. D. neutrons
Answers: 1. A 43. D 2. B 44. B 3. C 45. D 4. D 46. A 5. A 47. B 6. C 48. C 7. B 49. C 8. B 50. A 9. D 51. A 10. B 52. B 11. C 53. B 12. D 54. D 13. B 55. C 14. A. 88.3 º C; B. 88.3 º C 56. A 15. A 57. D 16. A 58. A 17. B 18. A 19. B 20. C 21. A 22. D 23. C 24. D 25. B 26. C 27. C 28. B 29. C 30. A. 2C + O2 2CO; B. 2NaClO3 2NaCl + 3O2; C. F2 + 2KBr 2KF + Br2 31. A. AlBr3 + 3AgNO3 Al(NO3)3 + 3AgBr; B. ZnBr2 + Na2S 2NaBr + ZnS 32. D 33. D 34. B 35. A 36. A 37. C 38. A 39. D 40. D 41. D 42. A