Chemistry Final Exam Review Multiple Choice Practice Questions Work through the following problems. Do your work in a neat orderly fashion either on this page or on another sheet. 1. Which of the following is a chemical property of magnesium? A. is ductile B. oxidizes to produce a white powder C. melts at 650 C D. has a density of 1.74 g/ml 2. Which of the following is a physical change? A. an egg frying B. an apple being digested C. butter melting D. bread toasting 3. Two isotopes of an element have different A. number of electrons C. number of protons B. atomic numbers D. mass number 4. Rutherford s gold foil experiment demonstrated: A. electrons have a negative charge B. energy is given off in little packets C. x rays are characteristic of the metal used as the anode D. most of the atom is empty space 5. In the modern periodic table, the elements within a column A. similar atomic diameters B. similar atomic masses C. the same number of energy levels D. similar properties 6. A substance that conducts heat well, is hard and is malleable is best classified as A. nonmetal C. halogen B. metalloid D. metal 7. How many atoms of oxygen are in aluminum sulfate, Al 2 (SO 4 ) 3? A. 12 B. 7 C. 4 D. 1 8. The empirical formula for benzene (C 6 H 6 ) is A. C 3 H 3 B. C 6 H 6 C. CH D. C 2 H 2 9. How many atoms of sulfur dioxide (SO 2 ) are present in 1.60 moles of sulfur dioxide? A. 9.63 x 10 23 B. 102.1 x 10 1 C. 7.62 x 10 1 D.3.76 x 10 23 10. What is the empirical formula of a compound containing 25.9 % nitrogen and 74.1 % oxygen? A. NO B. N 2 O C. N 2 O 5 D. NO 2 1
11. Which of the following is the correct equation for the single displacement reaction between bromine and calcium iodide? A. Br + CaI 2 -------à Ca + BrI 2 B. Br 2 + CaI ------------à CaIBr 2 C. Br 2 + CaI 2 --------à CaBr 2 + I 2 D. Br 2 + CaI 2 --------à Ca + Br 2 + I 2 12. The coefficient that should be placed before manganese when the following equation is balanced is. Al + MnO à Al 2 O 3 + Mn A. 4 B. 1 C. 3 D. 2 13. Which of the following is a product resulting from a reaction between silver nitrate (AgNO 3 ) and sodium chloride (NaCl)? A. silver chloride C. silver metal B. sodium chlorate D. chlorine gas 14. 15. Which of the following is the largest atom? A. Al B. O C. Ar D. Kr E. Na The amount of energy required to remove the most loosely held electron from an atom is the: A. electronegativity C. bonding energy B. electron affinity D. first ionization energy 16. Which of the following occurs when an element in Group 2 attains a stable electron configuration? A. It gains 8 electrons B. It loses 2 electrons C. It gains 2 electrons D. It gains 6 electrons 17. Which of the following lists the elements in order of increasing electronegativity? A. Br, Cl, F C. Li, Na, K B. O, P, Ge D. Cl, S, P 18. The type of bond that is formed by the transfer of electrons is: A. metallic C. intermolecular B. ionic D. covalent 19. A bond in which one of the atoms attracts the shared pair of electrons more strongly than does the atom is a(n): A. metallic bond C. ionic bonds B. nonpolar covalent bond D. polar covalent bond 20. With pressure constant, the temperature of a gas is increased from 30 C to 90 C. The volume will: A. decrease B. increase C. remain the same 2
21. 300. ml of gas exerts a pressure of 75.0 kpa. If the gas is condensed to 100. ml, what will the pressure be if temperature remains constant? A. 25.0 kpa B. 225 kpa C. 113 kpa D. 75.0 kpa 22. Le Chatelier s principle states that if a system is in equilibrium and a condition is changed, the system will: A. shift to minimize the amount of products B. shift to restore equilibrium C. shift to minimize the amount of reactants D. remain unchanged 23. The mechanism for a reaction is four steps. The rate determining step is: A. slowest step B. first step C. last step D. fastest step 24. What is the hydronium ion concentration of a solution with a ph of 5.5? A. 5.5 x 10-1 M C. 3.2 x 10-6 M B. 0.5 x 10-5 M D. 1 x 10-5 M 25. Find the hydronium ion concentration of a solution if the hydroxide concentration is 1.0 x 10-3. A. 1.0 x 10-14 C. 1.0 x 10-11 B. 1.0 x 10-3 D. 1.0 x 10-8 26. Find the oxidation number of the underlined atom in : Na 2 S 2 O 3 A. 2 B. 3 C. 4 D. 1 27. 28. Substances that are conductors in water solution are known as: A. oxidizing agents B. catalyst C. complexing agents D. electrolytes The degree of disorder in a system is the: A. Entropy B. enthalpy C. internal energy D. free energy 29. Based on the solubility curve below what is the solubility of KNO 3 at 40 C? A. 70 g/100 g H 2 O B. 63g/100 g H 2 O C. 40 g/100g H 2 O 3
30. Using the same table, at approximately what temperature is the solubility of KNO 3 three times that of NaCl? A. 0 C B. 20 C C. 35 C D. 70 C 31. Which of the following is true? A. Heterogeneous matter is the same throughout B. Homogeneous matter is the same throughout C. Vegetable soup is homogeneous D. Homogeneous matter can be separated by physical means 32. Where are the metals found on the periodic table? A. Left of stair step B. right of the stair step C. on the stair step 33. What is the molar mass of sodium sulfate, Na 2 SO 4? A. 110 g B. 142 g C. 160 g D. 210 g 34. Using the phase diagram below predict the phase at the conditions of 60 C and 0.9 atm A. solid B. liquid C. gas D. can t predict 35. The production of hydronium and hydroxide in aqueous solutions is referred to as: A. auto-ionization B. self reduction C. catalyzation D. acidification 36. Performing a chemical experiment, you observe the formation of steam; you can conclude the reaction is: A. exothermic B. endothermic C. a neutralization D. a titration 37. What is the correct name for MnO 2? A. Magnesium oxide C. Manganese oxide B. Manganese (II) oxide D. Manganese (IV) oxide 38. 39. An insoluble solid formed from two solutions is: A. a precipitate B. a spectator ion C. an intermediate A molecular compound that has a partial charge is called: A. polar molecule B. nonpolar molecule C. ionic compound D. metalllic compound 4
40. Reaction rates can be sped up by: A. decreasing concentration B. increasing temperature C. adding an inhibitor 41. What is the percent of sulfur in Al 2 (SO 4 ) 3? A. 9.4 % B. 28 % C. 56 % D. 37 % 42. What is the VSEPR shape of CH 4? A. Trigonal planar B. tetrhedral C. linear D. trigonal pyramidal 43. 44. Activation energy is the minimum energy required to A. start a chemical reaction C. boil a liquid B. freeze a liquid D. melt a solid Which of the following is an example of a metalloid? A. I B. In C. Br D. B 45. In the reaction 2 KClO 3 à 2 KCl + 3 O 2 oxygen is a A. reactant B. coefficient C. product D. subscript 46. 47. 48. 49. During condensation, the particles of a substance undergo a A. loss of potential energy C. gain of kinetic energy B. loss of kinetic energy D. gain of potential energy The type of bond that is formed as a result of the transfer of electrons is A. metallic B. intermolecular C. ionic D. covalent The coefficient placed before aluminum when the following equation is balanced is. Al + MnO --à Al 2 O 3 + Mn A. 4 B. 1 C. 3 D. 2 A balance is used to determine the of an object. A. heat B. temperature C. weight D. mass 50. 50ml of a liquid were found to have a mass of 38.4g. The proper set-up for the calculation of the density of the liquid would be: A. 38.4 g +50 ml B. 38.4g divided by 50 ml C 50 ml divided by 38.4 g D50 ml x38.4g 51. 52. 53. Heat is considered to be a form of: A. energy B. matter C. a chemical compound D a chemical element All of the following are physical changes EXCEPT: a. breaking of glass b. rusting of iron c. boiling of water d. melting of ice Which of the following represents a change of state? a. rain becomes ground water b. tide water recedes c. an icicle drips d. a snowflake comes to rest e. all of the above 54. How many atoms are in the compound H 3 PO 4? a.3 b. 7 c. 8 d. 9 5
55. 56. 57. 58. The formula for mercury (II) chloride is: a. HgCl b. HgCl 2 c. Hg 2 Cl d. HgCl 3 Which of the following is most likley to be IONIC? a. an element b. a compound melting at 25c c. a compound formed between two nonmetals d. a compound formed between a metal and nonmetal e. a compound formed with covalent bonds Which kind of bond predominates in Group I-A (alkali metal) halides? a. ionic b. covalent c. metallic d. van der Waals Mixing an acid and a base causes a reaction known as: a. oxidation-reduction b. neutralization c. precipitation d. endothermic e. analysis 59. How many liters of carbon dioxide at STP will be formed by the complete combustion of 15.0 g of ethane, C 2 H 6? a. a. 60.0 b. 30.0 c. 22.4 d. 4.00 e. 44.8 60. The reason that elements in the same group of the periodic table have similar chemical properties is that A. their atomic numbers differ by 8 B. they have the same outer electron congiurations C. each member of a group has one additional valence electron D. the valence electrons of each member occupy the same energy level 61. Consider the following melting points of Group VIIA elements: F = -223 C Br = -7.2 C Cl = -101.6 C and I = 113.5 C Which value would be a reasonable prediction for the melting point of astatine (# 85)? A. 150 C B. 50 C C. 50 C D. 100 C E. 200 C 62. An atom is considered inert when it is not chemicallly active under standard conditions. This inactivity is due to the fact that it has: A. its outer energy level is relatively far away from its nucleus B. its outer energy level is relatively close to its nucleus C. more than 4 electrons in its outer energy level D. 8 electrons in its outer level 63. 64. 65. 66. The arrangement of atoms in a water molecule is best described as: A. ring B. bent C. linear D. spherical When the atom gains an electron, the resulting particle is a(n): A. ion B. molecule C. isotope D. neutron E. proton At the same temperature, which gas has the slowest speed of diffusion? A. H 2 B. N 2 C. CH 4 D. CO 2 What is the relationship between temperature and kinetic energy A. Higher temp, high KE C. lower Temp, higher KE B. no correlation 6
67. 68. is: 69. If a 0.30 L sample of a gas is heated from 100 K to 300 K what will be the resulting volume? A. 0.06 L B. 0.60 L C. 0.12 L D. 0.90 L E. 0.10 L If the pressure on a confined gas is doubled at constant temperature, the quantity which is halved A. the mass B. the volume C. the density D. the kinetic energy The simplest formula of benzene is CH, its molecular mass is 78. Taking the atomic mass of hydrogen to be 1 and that of carbon to be 12, find the molecular formula of benzene. A. CH B. C 2 H 2 C. CH 6 D. C 6 H 5 E. C 6 H 6 70. Given: Ca(OH) 2 + 2HCl à CaCl 2 + 2 H 2 O. How many moles of calcium hydroxide, will be neutralized by one mole of hydrochloric acid? A. 1.0 B. 2.0 C. 1.5 D. 0.5 E. 4.0 71. 72. 73. When the ph of your solution decreases, the ratio of [H+]/[OH-]: A. increases B. decreases C. remains the same A solution which turns red litmus blue may contain: A. sugar B. sulfuric acid C. sodium hydroxide D. sodium chloride What is the ph of a 0.01 M potassium hydroxide solution? A. 0.01 B. 3 C. 10 D. 12 74. What is the oxidation number of nitrogen in N 2 O? A. 0 B. 2 C. +1 D. +2 E. +4 75. You place a substance in a flask of water, then you place a light bulb attached to an electric current into the solution. The bulb lights up brightly. You conclude the solution is: A. a nonelectrolyte B. a weak electrolyte C. a strong electrolyte D. a molecular compound 7