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Practice MSL Multiple Choice 1. Compared to the charge and mass of a proton, an electron has a. b. c. d. the same charge and a smaller mass the same charge and the same mass an opposite charge and a smaller mass an opposite charge and the same mass 2. When alpha particles are used to bombard gold foil, most of the alpha particles pass through undeflected. This result indicates that most of the volume of a gold atom consists of ____. a. b. c. d. deuterons neutrons protons unoccupied space 3. A proton has approximately the same mass as a. b. c. d. a neutron an alpha particle a beta particle an electron 4. When electrons in an atom in an excited state fall to lower energy levels, energy is a. b. c. d. absorbed, only released, only neither released nor absorbed both released and absorbed 5. A neutron has approximately the same mass as a. b. c. d. an alpha particle a beta particle an electron a proton 6. Which symbols represent atoms that are isotopes? a. b. c. d. C-14 and N-14 O-16 and O-18 I-131 and I-131 Rn-222 and Ra-222 7. Which element's ionic radius is smaller than its atomic radius? a. b. c. d. neon nitrogen sodium sulfur 8. Which atom contains exactly 15 protons? a. b. c. d. P-32 S-32 O-15 N-15 9. An ion with 5 protons, 6 neutrons, and a charge of 3+ has an atomic number of a. b. c. d. 5 6 8 11 10. What is the mass number of an atom which contains 28 protons, 28 electrons, and 34 neutrons? a. b. c. d. 28 56 62 90 11. Which three groups of the Periodic Table contain the most elements classified as metalloids (semimetals)? a. b. c. d. 1, 2, and 13 2, 13, and 14 14, 15, and 16 16, 17, and 18 12. Which element has the highest first ionization energy? a. b. c. d. sodium aluminum calcium phosphorus 13. Which compound forms a colored aqueous solution? a. b. c. d. CaCl22 CrCl3 NaOH KBr 14. When a metal atom combines with a nonmetal atom, the nonmetal atom will a. b. c. d. lose electrons and decrease in size lose electrons and increase in size gain electrons and decrease in size gain electrons and increase in size 15. Which of the following elements has the smallest atomic radius? a. b. c. d. nickel cobalt calcium potassium 16. Which element in Group 15 has the strongest metallic character? a. b. c. d. Bi As P N 17. Which halogens are gases at STP? a. b. c. d. chlorine and fluorine chlorine and bromine iodine and fluorine iodine and bromine 18. When combining with nonmetallic atoms, metallic atoms generally will a. b. c. d. lose electrons and form negative ions lose electrons and form positive ions gain electrons and from negative ions gain electrons and form positive ions 19. Which set of elements contains a metalloid? a. b. c. d. K, Mn, As, Ar Li, Mg, Ca, Kr Ba, Ag, Sn, Xe Fr, F, O, Rn 20. Atoms of elements in a group on the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms' a. b. c. d. number of principal energy levels number of valence electrons atomic numbers atomic masses 21. As atoms of elements in Group 16 are considered in order from top to bottom, the electronegativity of each successive element a. decreases b. increases c. remains the same 22. What is the concentration of hydroxide ions if the pH is 3.75? a. b. c. d. 5.6 x 10-11 M 1.78 x 10-4 M 10.25 M 3.9 M 23. An atom of which of the following elements has the greatest ability to attract electrons? a. b. c. d. silicon sulfur nitrogen chlorine 24. At STP, which substance is the best conductor of electricity? a. b. c. d. nitrogen neon sulfur silver 25. Which metal is obtained commercially by the electrolysis of salt? a. b. c. d. Zn K Fe Ag 26. Which element can be found in nature in the free (uncombined) state? a. b. c. d. Ca Ba Au Al 27. Which of the following is a binary compound? a. b. c. d. hydrogen sulfide hydrogen sulfate ammonium sulfide ammonium sulfate 28. What is the formula for sodium oxalate? a. b. c. d. NaClO Na2ClO Na2C2O4 NaC2H3O2 29. Given the unbalanced equation: Al + O2 Al2O3 When this equation is completely balanced using the smallest whole numbers, what is the sum of the coefficients? a. b. c. d. 9 7 5 4 30. What is the empirical formula of the compound whose molecular formula is P4O10? a. b. c. d. PO PO2 P2O5 P8O20V 31. Which of the following is a binary compound? a. b. c. d. potassium chloride ammonium chloride potassium chlorate ammonium chlorate 32. Which is the correct formula for nitrogen monoxide? a. b. c. d. NO N2O NO2 N2O3 33. What is the total number of atoms represented in the formula CuSO4 . 5H2O? a. b. c. d. 8 13 21 27 34. What is the gram formula mass of K2CO3? a. b. c. d. 138 g 106 g 99 g 67 g 35. What is the total number of atoms contained in 2.00 moles of nickel? a. b. c. d. 58.9 118 6.02 x 1023 1.2 x 1024 a. b. c. d. 36. What is the percent by mass of oxygen in magnesium oxide, MgO? a. b. c. d. 20% 40% 50% 60% 1.5 moles 2.00 moles 6.02 moles 9.03 moles a. b. c. d. CH CH2 CH3 CH4 a. b. c. d. 40. What is the mass in grams of 3.0 x 10 molecules of CO2? a. b. c. d. 22 g 44 g 66 g 88 g 23 113 g 121 g 149 g 404 g 45. What is the empirical formula of a compound that contains 85% Ag and 15% F by mass? a. b. c. d. 2.5 5.0 10 20 1.00 M 2.00 M 3.00 M 4.00 M 44. What is the gram formula mass of (NH4)3PO4? a. b. c. d. 39. What is the total number of moles of H2SO4 needed to prepare 5.0 liters of a 2.0 M solution of H2SO4? 22.4 L Ar 28.0 L of N2 32. 0 L of H2 44.8 L of He 43. What is the molarity of a KF (aq) solution containing 116 grams of KF in 1.00 liter of solution? a. b. c. d. 38. A compound is 86% carbon and 14% hydrogen by mass. What is the empirical formula for this compound? 6.89% 14.5% 26.1% 62.9% 42. At STP, 32.0 liters of O2 contain the same number of molecules as a. b. c. d. 37. What is the total number of moles of hydrogen gas contained in 9.03 x 1023 molecules? a. b. c. d. 41. What is the percent by mass of water in the hydrate Na2CO3 * 10H2O (formula mass = 286)? AgF Ag2F AgF2 Ag2F2 46. Given the reaction CH4 + 202 --> C02 + 2H20, What amount of oxygen is needed to completely react with 1 mole of CH4? a. b. c. d. 2 moles 2 atoms 2 grams 2 molecules 47. Which formula represents a molecular substance? a. b. c. d. CaO CO Li2O Al2O3 53. Which gas is monatomic at STP? a. b. c. d. chlorine fluorine neon nitrogen 54. What Kelvin temperature is equal to 25°C? 48. Which sequence of Group 18 elements demonstrates a gradual decrease in the strength of the Van der Waals forces? All the choices are elements in the liquid state. a. b. c. d. Ar, Kr, Ne, Xe Kr, Xe, Ar, Ne Ne, Ar, Kr, Xe Xe, Kr, Ar, Ne 49. Which substance is an example of a network solid? a. b. c. d. nitrogen dioxide sulfur dioxide carbon dioxide silicon dioxide 50. Which combination of atoms can form a polar covalent bond? a. b. c. d. H and H H and Br N and N Na and Br 51. A strontium atom differs from a strontium ion in that the atom has a greater a. b. c. d. number of electrons number of protons atomic number mass number 52. Which bond has the greatest ionic character? a. b. c. d. H---Cl H---F H---O H---N a. b. c. d. 248 K 298 K 100 K 200 K 55. When the external pressure is 101.3 kPa, water will boil at what temperature? a. b. c. d. 12.8°C 14.5°C 100°C 18°C 56. As ice cools from 273 K to 263 K, the average kinetic energy of its molecules will a. decrease b. increase c. remain the same 57. The phase change represented by the equation I2 (s) ----> I2 (g) is called a. b. c. d. sublimation condensation melting boiling 58. The heat of fusion is defined as the energy required at constant temperature to change 1 unit mass of a a. b. c. d. gas to a liquid gas to a solid solid to a gas solid to a liquid 59. As the pressure of a gas at 2 atm is changed to 1 atm at constant temperature, the volume of the gas a. decreases b. increases c. remains the same 60. What is the total number of joules of heat energy absorbed by 15 grams of water when it is heated from 30°C to 40°C? a. b. c. d. 10 63 150 630 61. A compound differs from a mixture in that a compound always has a a. b. c. d. homogeneous composition maximum of two components minimum of three components heterogeneous composition 62. Which substance cannot be decomposed into simpler substances? a. b. c. d. ammonia aluminum methane methanol 63. How many joules are equivalent to 35 kilojoules? a. b. c. d. 0.035 joules 0.35 joules 3,500 joules 35,000 joules 64. Which statement describes a chemical property? a. b. c. d. Its crystals are a metallic gray. It dissolves in alcohol. It forms a violet-colored gas. It reacts with hydrogen to form a gas. 65. A solution in which the crystallizing rate of the solute equals the dissolving rate of the solute must be a. b. c. d. saturated unsaturated concentrated dilute 66. A sample of unknown gas at STP has a density of 0.630 g per liter. What is the gram molecular mass of this gas? a. b. c. d. 2.81 g 14.1 g 22.4 g 63 g 67. The heat of fusion of a compound is 30 joules per gram. What is the total number of joules of heat that must be absorbed by a 15.0 gram sample to change the compound from a solid to a liquid at its melting point? a. b. c. d. 15 cal 45 cal 150 cal 450 cal 68. How many joules of heat are absorbed when 70.0 grams of water is completely vaporized at its boiling point? a. b. c. d. 23, 352 7, 000 15, 813 158, 130 69. Under which conditions are gases most soluble in water? a. b. c. d. high pressure and high temperature high pressure and low temperature low pressure and high temperature low pressure and low temperature d. potential energy of the products 70. A student investigated the physical and chemical properties of a sample of unknown gas and then investigated the gas. Which statement represents a conclusion rather than an experimental observation? a. The gas is colorless. b. The gas is carbon dioxide. c. When the gas is bubbled in limewater, the liquid becomes cloudy. d. When placed in the gas, a flaming splint stops burning. 71. A student determined the heat of fusion of water to be 366.9 J/g. If the accepted value is 333.3J/g, what is the student's percent error? a. b. c. d. 8.0% 10.0% 15% 30.0% 72. What occurs as potassium nitrate is dissolved in a beaker of water, indicating that the process is endothermic? a. b. c. d. The temperature of the solution decreases. The temperature of the solution increases. The solution changes color. The solution gives off a gas. 73. To determine the density of an irregularly shaped object, a student immersed the object in 21.2 milliliters of H2O in a graduated cylinder, causing the level of the H2O to rise to 27.8 milliliters. If the object had a mass of 22.4 grams, what was the density of the object. a. b. c. d. 27.8 g / mL 6.6 g / mL 3.0 g / mL 3.4 g/ mL 74. When a catalyst is added to a system at equilibrium, a decrease occurs in the a. activation energy b. heat of reaction c. potential energy of the reactants 75. In a chemical reaction, a catalyst changes the a. b. c. d. potential energy of the products potential energy of the reactants heat of reaction activation energy 76. Which element is present in all organic compounds? a. b. c. d. carbon nitrogen oxygen phosphorous 77. In which pair of hydrocarbons does each compound contain only one double bond per molecule? a. b. c. d. C2H2 and C2H6 C2H2 and C3H6 C4H8 and C2H4 C6H6 andC7H8 78. What is the maximum number of covalent bonds that an atom of carbon can form? a. b. c. d. 1 2 3 4 79. What is the net ionic equation for the following: 2Na3PO4 (aq) + 3 CaCl2 (aq) 6 NaCl (aq) + Ca3(PO4)2 (s) a. b. c. d. 6Na+(aq) + 6Cl-(aq) NaCl (aq) 2PO43-(aq) + 3Ca+2(aq) Ca3(PO4)2(s) 6Na+(aq) + 2PO43-(aq) Ca3(PO4)2(s) 6Cl-(aq) + 3Ca+2NaCl(aq) 80. Which substance functions as the electrolyte in an automobile battery? a. b. c. d. PbO2 PbSO4 H2SO4 H2O 81. Consider the equation, 2H2 + O2 ↔ 2H2O. If hydrogen was added, in which direction would we see a shift? a. b. c. d. toward left toward right toward left and right no shift 82. What are the spectator ions in the following equation: AgNO3(aq) + LiBr(aq) ↔ AgBr(aq) + LiNO3(s) a. b. c. d. Ag+(aq) and Br-(aq) Li+(aq) and NO3-(aq) Ag+(aq) and NO3-(aq) Li+(aq) and Br-(aq) 83. If a flask contains 5.90 mL of NH3 at 100 C, what would the new temperature be if the volume was changed to 13.7 mL? a. b. c. d. 0.00115C 0.217C 593C 866C 84. Given the reaction: 2Li(s) + Cl2(g) -> 2LiCl(s) As the reaction takes place, the Cl2(g) will a. b. c. d. gain electrons lose electrons gain protons lose protons. 85. Given the reaction: __Mg + __Cr3+ -> __Mg2+ + __Cr When the equation is correctly balanced using smallest whole numbers, the sum of the coefficients will be a. b. c. d. 10 7 5 4 86. How many grams of KCl are needed at STP if volume is 152mL? a. b. c. d. 0.00678 g 0.506 g 6.78 g 506 g 87. Which formula represents a salt? a. b. c. d. KOH KCl CH3OH CH3COOH 88. Which substance can be classified as an Arrhenius acid? a. b. c. d. HCl NaCl LiOH KOH 89. Which solution will change red litmus to blue? a. b. c. d. HCl(aq) NaCl(aq) CH3OH(aq) NaOH(aq) 90. An acidic solution could have a pH of a. b. c. d. 7 10 3 14 91. What is the pH of a 0.00001 molar HCl solution? a. b. c. d. 1 9 5 4 92. What is the pH of a solution with a hydronium ion concentration of 0.01 mole per liter? a. b. c. d. 1 2 10 14 93. There are alternate acid base theories that define an acid as any species that can a. b. c. d. donate a proton donate an electron accept a proton accept an electron 94. Which 0.1 M solution will turn phenolphthalein pink? a. b. c. d. HBr(aq) CO2(aq) LiOH(aq) CH3OH(aq) 95. As the hydrogen ion concentration of an aqueous solution increases, the hydroxide ion concentration of this solution will a. decrease b. increase c. remain the same 96. Which radioactive emanations have a charge of -1? a. b. c. d. neutrons gamma rays alpha particles beta particles 97. As the temperature of a sample of a radioactive element decreases, the half-life will a. decrease b. increase c. remain the same 98. What kind of radiation will travel through an electric field on a pathway that remains unaffected by the field? a. b. c. d. a proton a gamma ray an electron an alpha particle 99. Which particle cannot be accelerated in a magnetic field? a. b. c. d. alpha particle beta particle neutron proton 100. In the reaction 4Be9 + X -> 6C12 + 0n1, the X represents a. b. c. d. an alpha particle a beta particle an electron a proton 101. Which substance has chemical properties similar to those of radioactive 235U? a. b. c. d. 235 Pa Pa 233 U 206 Pb 233 102. Which reaction illustrates fusion? a. b. c. d. 2 2 4 1H + 1H -> 2He 1 27 24 4 0n + 13Al - > 11Na + 2He 27 4 30 1 13Al + 2He -> 15P + 0n 14 4 1 17 7N + 2He -> 1H + 8O 103. Which statement describes characteristics of an endothermic reaction? a. b. c. d. The sign of H is positive, and the products have less potential energy than the reactants. The sign of H is positive, and the products have more potential energy than the reactants. The sign of H is negative, and the products have less potential energy than the reactants. The sign of H is negative, and the products have more potential energy than the reactants. 104. Which statement explains why the speed of some chemical reactions is increased when the surface area of the reactant is increased? a. b. c. d. This change increases the density of the reactant particles. This change increases the concentration of the reactant. This change exposes more reactant particles to a possible collision. This change alters the electrical conductivity of the reactant particles. 105. Which conditions will increase the rate of chemical reaction? a. b. c. d. decreased temperature and decreased concentration of reactants? decreased temperature and increased concentration of reactants? increased temperature and decreased concentration of reactants? increased temperature and increased concentration of reactants? 106. Which procedure will increases the solubility of KCl in water? a. b. c. d. stirring the solute and solvent mixture increasing the surface area of the solute raising the temperature of the solvent increasing the pressure on the surface of the solvent 107. Given the reaction: Mg(C2H3O2)2 (aq) + K2CO3(aq) MgCO3 (s) + 2KC2H3O2 (aq) What is the net ionic equation? a. b. c. d. Mg+2(aq) + 2C2H3O2-(aq) MgCO3(s) 2C2H3O2-(aq) + 2K+(aq) MgCO3(s) 2C2H3O2-(aq) + CO3-2(aq) MgCO3(s) Mg+2(aq) + CO3-2(aq) MgCO3(s) 108. The following data were collected at the endpoint of a titration performed to find the molarity of an HCl solution. Volume of acid (HCl) used = 14.4 mL Volume of base (NaOH) used = 22.4 mL Molarity of standard base (NaOH) = 0.20 M What is the molarity of the acid solution? a. b. c. d. 1.6 M 0.64 M 0.31M 0.13M 109. In a fusion reaction, reacting nuclei must collide. Collisions between two nuclei are difficult to achieve because the nuclei are a. b. c. d. both negatively charged and repel each other both positively charged and repel each other oppositely charged and attract each other oppositely charged and repel each other 110. A particle accelerator can increase the kinetic energy of a. b. c. d. an alpha particle and a beta particle an alpha particle and a neutron a gamma ray and a beta particle a neutron and a gamma ray 111. Which solution is the most concentrated? a. b. c. d. 1 mole of solute dissolved in 1 liter of solution? 2 moles of solute dissolved in 3 liters of solution? 6 moles of solute dissolved in 4 liters of solution? 4 moles of solute dissolved in 8 liters of solution? 112. Under the same conditions of temperature and pressure, a liquid differs from a gas because the particles of the liquid a. b. c. d. are in constant straight-line motion take the shape of the container they occupy have no regular arrangement have stronger forces of attraction between them 113. The volume of a given mass of an ideal gas at constant pressure is a. b. c. d. directly proportional to the Kelvin temperature. directly proportional to the Celsius temperature. inversely proportional to the Kelvin temperature. inversely proportional to the Celsius temperature. 114. How are the boiling and freezing points of a sample of water affected when salt is dissolved in the water? a. b. c. d. The boiling point decreases and the freezing point decreases. The boiling point decreases and the freezing point increases. The boiling point increases and the freezing point decreases. The boiling point increases and the freezing point increases. 115. A solid is dissolved in a beaker of water. Which observation suggests that the process is endothermic? a. b. c. d. The solution gives off a gas. The solution changes color. The temperature of the solution decreases. The temperature of the solution increases. 116. Salt A and salt B were dissolved separately in 100 mL beakers of water. The water temperatures were measured and recorded as shown in the table below: Salt A: initial water temp. 25.1°C final water temp. 30.2°C Salt B: initial water temp. 25.1°C final water temp. 20.0°C Which statement is a correct interpretation of these data? a. b. c. d. The dissolving of only salt A was endothermic. The dissolving of only salt B was exothermic The dissolving of both salt A and salt B was endothermic. The dissolving of salt A was exothermic and the dissolving of salt B was endothermic. 117. Which statement explains why the element carbon forms so many compounds? a. b. c. d. Carbon atoms combine readily with oxygen. Carbon atoms have very high electronegativity. Carbon readily forms ionic bonds with other carbon atoms. Carbon readily forms covalent bonds with other carbon atoms. 118. When HCl(aq) is exactly neutralized by NaOH(aq), the hydrogen ion concentration in the resulting mixture is a. b. c. d. always less than the concentration of the hydroxide ions always greater than the concentration of the hydroxide ions always equal than the concentration of the hydroxide ions sometimes greater and sometimes less than the concentration of the hydroxide ions 119. A student wishes to prepare approximately 100 milliliters of an aqueous solution of 6M HCl using 12 M HCl. Which procedure is correct? a. b. c. d. adding 50 mL of 12 M HCl to 50 mL of water while stirring the mixture steadily. adding 50 mL of 12 M HCl to 50 mL of water and then stirring the mixture steadily. adding 50 mL of water to 50 mL of 12 M HCl while stirring the mixture steadily. adding 50 mL of water to 50 mL of 12 M HCl and then stirring the mixture steadily. Answer Sheet: Practice MSL 1.______ 25._____ 49._____ 73._____ 2.______ 26._____ 50._____ 74._____ 3.______ 27._____ 51._____ 75._____ 4.______ 28._____ 52._____ 5.______ 29._____ 53._____ 6.______ 30._____ 54._____ 97._____ 98._____ 99._____ 7.______ 8.______ 9.______ 31._____ 32._____ 33._____ 11._____ 35._____ 59._____ 12._____ 36._____ 60._____ 13._____ 37._____ 61._____ 14._____ 38._____ 62._____ 15._____ 39._____ 63._____ 16._____ 40._____ 64._____ 19._____ 42._____ 43._____ 101.____ 78._____ 102.____ 79._____ 103.____ 80._____ 104.____ 81._____ 105.____ 82._____ 106.____ 83._____ 107.____ 84._____ 108.____ 85._____ 109.____ 86._____ 110.____ 87._____ 111.____ 88._____ 112.____ 89._____ 113.____ 90._____ 114.____ 91._____ 115.____ 92._____ 116.____ 93._____ 117.____ 94._____ 118.____ 95._____ 119.____ 96._____ 120.____ 57._____ 58._____ 18._____ 77._____ 56._____ 34._____ 41._____ 100.____ 55._____ 10._____ 17._____ 76._____ 65._____ 66._____ 67._____ 20._____ 44._____ 68._____ 21._____ 45._____ 69._____ 22._____ 46._____ 70._____ 23._____ 47._____ 71._____ 24._____ 48._____ 72._____ 121.____