Name: Class: Date: Chemistry I - 2017 Spring - Pre-Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. According to the figure below, what is the most volatile substance shown? a. benzene c. toluene b. water d. aniline 2. In a chemical reaction a. the mass of the reactants equals the mass of the products. b. the mass of the products is greater than the mass of reactants. c. the number of atoms in the reactants and products must change. d. energy as heat must be added to the reactants. 3. The nucleus of an atom has all of the following characteristics except that it a. is positively charged. b. is very dense. c. contains nearly all of the atom's mass. d. contains nearly all of the atom's volume. 4. Which equation is not balanced? a. 2H 2 + O 2 2H 2 O b. 4H 2 + 2O 2 4H 2 O c. H 2 + H 2 + O 2 H 2 O + H 2 O d. 2H 2 + O 2 H 2 O 5. Each carbon atom in a molecule forms four single covalent bonds with other atoms in a(n) a. aromatic hydrocarbon. c. structural isomer. b. saturated hydrocarbon. d. geometric isomer. 1
Name: 6. Isotopes are atoms of the same element that have different a. principal chemical properties. c. numbers of protons. b. masses. d. numbers of electrons. 7. The atomic number of oxygen, 8, indicates that there are eight a. protons in the nucleus of an oxygen atom. b. oxygen nuclides. c. neutrons outside the oxygen atom's nucleus. d. energy levels in the oxygen atom's nucleus. 8. For an electron in an atom to change from the ground state to an excited state, a. energy must be released. b. energy must be absorbed. c. radiation must be emitted. d. the electron must make a transition from a higher to a lower energy level. 9. The density of a substance undergoes the greatest change when the substance changes from a a. liquid to a gas. c. solid to a liquid. b. liquid to a solid. d. a molecular solid to an ionic solid. 10. Which of the following is not an example of a molecular formula? a. H 2 O c. NH 3 b. B d. O 2 11. Which of the following are the small units joined to each other by organic reactions in a polymer? a. monomers c. copolymers b. micropolymers d. linear polymers 12. The reason the boiling point of water (H 2 O) is higher than the boiling point of hydrogen sulfide (H 2 S) is partially explained by a. London forces. c. ionic bonding. b. covalent bonding. d. hydrogen bonding. 13. Balance the following equation: 239 93 Np + 0 1 e a. 239 Th c. 90 94 239 Pu b. 239 U d. 92 94 238 Pu 14. What is the formula for the compound formed by lead(ii) ions and chromate ions? a. PbCrO 4 c. Pb 2 (CrO 4 ) 3 b. Pb 2 CrO 4 d. Pb(CrO 4 ) 2 15. A substance that ionizes nearly completely in aqueous solutions and produces H 3 O + is a a. weak base. c. weak acid. b. strong base. d. strong acid. 16. Which of the following is an extensive property of matter? a. melting point c. volume b. boiling point d. density 2
Name: 17. Plasma is the fourth state of matter. In the plasma state a. atoms gain electrons. b. atoms lose electrons. c. atoms form molecules. d. atomic nuclei break down. 18. According to Bohr, electrons cannot reside at in the figure below. a. point A c. point C b. point B d. point D 19. How many moles of ions are produced by the dissociation of 1 mol of Al 2 (CO 3 ) 3? a. 2 mol c. 5 mol b. 4 mol d. 11 mol 20. Which of the following is not a chemical change? a. rusting c. melting b. igniting d. burning 21. Bases react with a. acids to produce salts and water. c. water to produce acids and salts. b. salts to produce acids and water. d. neither acids, salts, nor water. 22. Which of the following does not increase the rate of dissolving a solid in water? a. raising the temperature of the water b. stirring the solution c. using larger pieces of solid d. crushing the solid 23. The electrons involved in the formation of a chemical bond are called a. dipoles. c. Lewis electrons. b. s electrons. d. valence electrons. 24. A measure of the quantity of matter is a. density. c. volume. b. weight. d. mass. 25. As atoms bond with each other, they a. increase their potential energy, thus creating less-stable arrangements of matter. b. decrease their potential energy, thus creating less-stable arrangements of matter. c. increase their potential energy, thus creating more-stable arrangements of matter. d. decrease their potential energy, thus creating more-stable arrangements of matter. 3
Name: 26. In an equation, the symbol for a substance in water solution is followed by a. (1). c. (aq). b. (g). d. (s). 27. Which coefficients correctly balance the formula NH 4 NO 2 N 2 + H 2 O? a. 1,2,2 c. 2,1,1 b. 1,1,2 d. 2,2,2 28. According to VSEPR theory, the structure of the ammonia molecule, NH 3, is a. trigonal-planar. c. trigonal-pyramidal. b. bent. d. tetrahedral. 29. Name the compound CF 4. a. calcium fluoride c. carbon tetrafluoride b. carbon fluoride d. monocalcium quadrafluoride 30. Under ordinary conditions of temperature and pressure, the particles in a gas are a. closely packed. b. very far from one another. c. held in fixed positions. d. unevenly distributed. 31. Carbon dioxide dissolved in water is an example of which solute-solvent combination? a. gas-liquid c. liquid-liquid b. liquid-gas d. cannot be determined Use the table below to answer the following questions. General Solubility Guidelines 1. Most sodium, potassium, and ammonium compounds are soluble in water. 2. Most nitrates, acetates, and chlorates are soluble. 3. Most chlorides are soluble, except those of silver, mercury(i), and lead. Lead(II) chloride is soluble in hot water. 4. Most sulfates are soluble, except those of barium, strontium, and lead. 5. Most carbonates, phosphates, and silicates are insoluble, except those of sodium, potassium, and ammonium. 6. Most sulfides are insoluble, except those of calcium, strontium, sodium, potassium, and ammonium. 32. Which of the following pairs of solutions produces a precipitate when combined? a. Cu(NO 3 ) 2 and NaCl c. Cu(NO 3 ) 2 and K 2 CO 3 b. Fe(NO 3 ) 3 and MgCl 2 d. CaCl 2 and NaNO 3 33. Particles within a solid a. do not move. c. move about freely. b. vibrate about fixed positions. d. exchange positions easily. 4
Name: 34. Which part of the illustration below shows the particles in a heterogeneous mixture? a. a c. c b. b d. d 35. Which of these can happen due to decreasing the average energy of a liquid's particles? a. vaporization c. a random arrangement b. evaporation d. freezing 36. What is the pressure exerted by 1.2 mol of a gas with a temperature of 20. C and a volume of 9.5 L? a. 0.030 atm c. 3.0 atm b. 1.0 atm d. 30. atm 37. The volume of a gas is 5.0 L when the temperature is 5.0 C. If the temperature is increased to 10.0 C without changing the pressure, what is the new volume? a. 2.5 L c. 5.1 L b. 4.8 L d. 10.0 L 38. According to the table below, if a rock contains 25% as much uranium-235 as rocks being formed today, how old is the rock? Nuclide Half-Life (years) carbon-14 5.71 10 3 potassium-40 1.26 10 9 radium-226 1.60 10 3 thorium-230 7.54 10 4 uranium-235 7.04 10 8 a. 7.04 10 8 years c. 2.84 10 9 years b. 3.55 10 8 years d. 1.41 10 9 years 5
Name: 39. Name the compound Al 2 S 3. a. aluminum sulfate c. aluminum(ii) sulfate b. aluminum sulfur d. aluminum sulfide 40. What is the net ionic equation for the precipitation reaction between BaCl 2 and Na 2 SO 4? a. BaCl 2 (aq) + Na 2 SO 4 (aq)? BaSO 4 (s) + 2NaCl(aq) b. Na + (aq) + Cl - (aq)? NaCl(s) c. Ba 2+ (aq) + SO 2-4 (aq)? BaSO 4 (s) d. Ba 2+ (aq) + 2Cl - (aq) + 2 Na + (aq) + SO 2-4 (aq)? BaSO 4 (s) + 2Cl - (aq) + 2Na + (aq) 41. All of the following equations are statements of the ideal gas law except P a. P = nrtv. c. n = RT V. PV PV b. = nr. d. R = T nt. 42. The molar mass of LiF is 25.94 g/mol. How many moles of LiF are present in 10.37 g? a. 0.3998 mol c. 2.500 mol b. 1.333 mol d. 36.32 mol 43. In nature, the alkali metals occur as a. elements. c. complex ions. b. compounds. d. gases. 44. A molecular compound has the empirical formula XY 3. Which of the following is a possible molecular formula? a. X 2 Y 3 c. X 2 Y 5 b. XY 4 d. X 2 Y 6 45. What is removed when the ionization energy is supplied to an atom of an element? a. the electron cloud c. an electron b. the nucleus d. an ion 46. The element that has the greatest electronegativity is a. oxygen. c. chlorine. b. sodium. d. fluorine. 47. A mixture of four gases exerts a total pressure of 860 mm Hg. Gases A and B each exert 220 mm Hg. Gas C exerts 110 mm Hg. What pressure is exerted by gas D? a. 165 mm Hg c. 860 mm Hg b. 310 mm Hg d. 220 mm Hg 48. Isomers are compounds that have a. the same molecular formula but different structures. b. the same molecular formula and the same structure. c. different molecular formulas and different structures. d. different molecular formulas but the same structure. 6
Name: 49. A species that remains when an acid has lost a proton is a a. conjugate base. c. strong base. b. conjugate acid. d. strong acid. 50. If electromagnetic radiation A has a lower frequency than electromagnetic radiation B, then compared to B, the wavelength of A is a. longer. c. equal. b. shorter. d. exactly half the length of B's wavelength. 51. Among atoms with low atomic numbers, what is the neutron-proton ratio of the most stable nuclei? a. 1:1 c. 1.51:1 b. 1.5:1 d. 1:2 52. Which of the following is a nonelectrolyte? a. sodium chloride c. sugar b. hydrogen chloride d. potassium chloride 53. The reaction represented by the equation Pb(NO 3 ) 2 (aq) + 2KI(aq) PbI 2 (s) + 2KNO 3 (aq) is a a. double-displacement reaction. c. decomposition reaction. b. synthesis reaction. d. combustion reaction. 54. In the equation 2KClO 3 2KCl + 3O 2, how many moles of oxygen are produced when 3.0 mol of KClO 3 decompose completely? a. 1.0 mol c. 3.0 mol b. 2.5 mol d. 4.5 mol 55. What is the formula for hydrochloric acid? a. HF c. HClO b. HCl d. H 2 CO 3 56. The nuclear binding energy is released when a nucleus a. is bombarded. c. is formed from its constituent particles. b. divides. d. decays. 57. Why could the pressure of a sample of gas at a constant volume fall 75 mm Hg? a. The container exploded. c. The temperature decreased. b. The temperature increased. d. The volume increased. 58. Visible light, X rays, infrared radiation, and radio waves all have the same a. energy. c. speed. b. wavelength. d. frequency. 59. Which of the following is a strong base? a. KOH c. NH 3 b. H 2 d. HCl 60. Which of the following is the correct relationship between mass and energy? a. E = mc 2 c. E 2 = mc b. E = mc d. E = m 2 c 7
Name: 61. What is the correct Lewis structure for hydrogen chloride, HCl? a. A c. C b. B d. D 62. A plausible explanation of a body of observed natural phenomena is a scientific a. control. c. law. b. experiment. d. theory. 63. Name the compound Fe(NO 3 ) 2. a. iron(ii) nitrate c. iron(iii) nitrate b. iron(ii) nitrite d. iron(iii) nitride 64. The number of electrons in the highest energy level of the argon atom (atomic number 18) is a. 10. c. 6. b. 2. d. 8. 65. According to the kinetic-molecular theory, gases condense into liquids because of a. gravity. c. forces between molecules. b. atmospheric pressure. d. elastic collisions. 66. The forces of attraction between molecules in a molecular compound are a. stronger than the forces among formula units in ionic bonding. b. weaker than the forces among formula units in ionic bonding. c. approximately equal to the forces among formula units in ionic bonding. d. zero. 67. What do all organic compounds contain? a. hydrogen c. oxygen b. water d. carbon 68. Dalton's atomic theory agrees with modern atomic theory except for the statement that a. all matter is made up of small particles. b. atoms are not divided in chemical reactions. c. atoms of the same element are chemically alike. d. all atoms of the same element have the same mass. 69. If repeated measurements agree closely but differ widely from the accepted value, these measurements are a. neither precise nor accurate. b. accurate, but not precise. c. both precise and accurate. d. precise, but not accurate. 70. What does the constant bombardment of gas molecules against the inside walls of a container produce? a. temperature c. pressure b. density d. diffusion 8
Name: 71. What is the electron configuration for nitrogen, atomic number 7? a. 1s 2 2s 2 2p 3 b. 1s 2 2s 3 2p 2 c. 1s 2 2s 3 2p 1 d. 1s 2 2s 2 2p 2 3s 1 72. The reaction represented by the equation 2HgO(s) 2Hg(l) + O 2 (g) is a(n) a. single-displacement reaction. c. combustion reaction. b. synthesis reaction. d. decomposition reaction. 73. What is the formula mass of (NH 4 ) 2 SO 4? a. 114.09 amu c. 128.06 amu b. 118.34 amu d. 132.16 amu 74. In oxides of nitrogen, such as N 2 O, NO, NO 2, and N 2 O 3, atoms combine in small whole-number ratios. This evidence supports the law of a. conservation of mass. c. definite composition. b. multiple proportions. d. mass action. 75. Malleability and ductility are characteristic of substances with a. covalent bonds. c. Lewis structures. b. ionic bonds. d. metallic bonds. 9