SPRING 2017 CHEMISTRY FINAL EXAM REVIEW

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1 SPRING 2017 CHEMISTRY FINAL EXAM REVIEW Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. BONDING What is the formula for diphosphorus pentaoxide? a. P 2PeO 5 c. P 2O 4 b. PO 5 d. P 2O 5 2. Name the compound N 2O 4. a. binitrogen tetraoxide. c. dinitrogen quadraoxide. b. dinitride tetraoxide. d. dinitrogen tetraoxide. 3. Name the compound P 3Cl 6. a. triphosphorus heptachloride c. triphosphide hexachloride b. triphosphorus hexachloride d. triphosphorus pentachloride 4. Name the compound MgCl 2. a. magnesium chloride II c. magnesium chloride b. magnesium chlorine d. magnesium dichloride 5. Based on the location of the element, nitrogen, how many more electrons does nitrogen need to be stable or happy like the Noble gases? a. 1 c. 5 b. 3 d To show the oxidation number for transition metals, a must be used in the name of the compound. a. symbol c. Roman numeral b. letter d. number 7. What is the formula for copper II chloride? a. Cu 2Cl c. CuCl b. CuCl 2 d. CoCl 8. Using the criss-cross method, what would be the compound formed from Li and O? a. Li 2O c. LiO 2 b. LiO d. LiOH 9. Which of the following is a cation? a. Argon c. Oxygen b. Chlorine d. Magnesium 10. Which kind of bond forms between nitrogen and fluorine? (Hint: look at EN differences!) a. polar c. both b. non-polar d. neither 11. Which of the following is an anion? a. Argon c. Sodium b. Chlorine d. Magnesium

2 12. Which kind of bond forms between sulfur and bromine? (Hint: look at EN differences!) a. polar c. both b. non-polar d. neither 13. If the atoms that share electrons have an unequal attraction for the electrons, the bond is called a. nonpolar. c. ionic. b. polar. d. dipolar. 14. The chemical bond formed when one atom transfers electrons to another is called a(n) a. ionic bond. c. Lewis structure. b. orbital bond. d. covalent bond. 15. If the atoms that share electrons have an equal attraction for the electrons, the bond is called a. nonpolar. c. ionic. b. polar. d. dipolar. 16. MOLE CONVERSIONS/MOLAR MASS What is the correct empirical formula for glucose (C 6H 12O 6)? a. C 3H 6O 3 c. CH 2O b. C 2H 4O 2 d. C 6H 12O How many atoms of hydrogen are found in the compound, NH 4C 2H 3O 2? a. 3 c. 7 b. 4 d Which of the following is an empirical formula? a. C 5H 10 c. H 2O 2 b. C 3H 6O 2 d. P 4O How many molecules are in one mole of C 6H 12O 6? (Hint: Look at mole conversion factors!!) a. 6 molecules c. 24 molecules b x molecules d molecules 20. Which of the following compounds would have the empirical formula, CH 2? a. C 2H 3 c. C 4H 6 b. C 8H 4 d. C 4H What is the number 6.02 x referred to as? a. Shakespeare s Number c. Avogadro s Number b. Bohr s Number d. Rutherford s Number 22. What is the molar mass of Mg(NO 2) 2? a g c g b g d g 23. What is the molar mass of CaCO 3? a g c g b g d g 24. How many molecules are found in 1.92 mol of CO 2? a x molecules CO 2 c molecules CO 2 b x molecules CO 2 d molecules CO 2

3 25. How many moles are found in 9.74 x molecules of H 2O? a x mol H 2O c x mol H 2O b x mol H 2O d mol H 2O 26. CHEMICAL REACTIONS The reaction Pb(NO 3) 2 + 2KI PbI 2 + 2KNO 3 is a a. synthesis reaction. c. double replacement reaction. b. combustion reaction. d. decomposition reaction. 27. The reaction Cu + 2AgNO 3 2Ag + Cu(NO 3) 2 is a a. single replacement reaction. c. combustion reaction. b. double replacement reaction. d. decomposition reaction. 28. The reaction 2CH 4O + 3O 2 2CO 2 + 4H 2O is a a. synthesis reaction. c. single replacement reaction. b. double replacement reaction. d. combustion reaction. 29. Why can t the subscripts be changed to balance an equation? a. Subscripts are unique to each compound s formula; changing the subscripts changes the formula into a new compound. b. Subscripts are not important in balancing equations. c. Subscripts are already balanced. d. Subscripts can be changed; coefficients cannot be changed. 30. The reaction 2Mg + O 2 2MgO is a a. double replacement reaction. c. single replacement reaction. b. synthesis reaction. d. decomposition reaction. 31. The reaction 2HgO 2Hg + O 2 is a a. combustion reaction. c. decomposition reaction. b. synthesis reaction. d. single replacement reaction. 32. In an equation, the symbol for a substance that is dissolved in water is followed by a. (s). c. (l). b. (g). d. (aq). 33. According to the law of conservation of mass, the total mass of the reacting substances is a. always less than the total mass of the products. b. sometimes more and sometimes less than the total mass of the products. c. always more than the total mass of the products. d. always equal to the total mass of the products. 34. A chemical equation is balanced when the a. products and reactants are the same chemicals. b. subscripts of the reactants equal the subscripts of the products. c. same number of each kind of atom appears in the reactants and in the products. d. coefficients of the reactants equal the coefficients of the products. 35. Which coefficient ratio correctly balances the formula equation: Ca + NaCl Na + CaCl 2? a. 1, 2, 2, 1 c. 2, 2, 2, 1 b. 2, 1, 1, 2 d. 1, 2, 1, 1

4 36. Which coefficient ratio correctly balances the formula equation: H 2O 2 O 2 + H 2O? a. 1, 2, 2 c. 2, 2, 2 b. 2, 1, 2 d. 1, 1, Which coefficient ratio correctly balances the formula equation: Fe + MgCl 2 FeCl 3 + Mg? a. 1, 3, 1, 3 c. 2, 3, 2, 3 b. 4, 6, 4, 6 d. 1, 2, 1, Which coefficient ratio correctly balances the formula equation: NH 4NO 2 N 2 + H 2O? a. 1, 2, 2 c. 2, 2, 2 b. 2, 1, 1 d. 1, 1, Which coefficient ratio correctly balances the formula equation: P + O 2 P 2O 5? a. 1, 5, 2 c. 4, 5, 2 b. 2, 2, 1 d. 2, 3, STOICHIOMETRY When calculating a moles to moles conversion, what part of a chemical equation represents mole ratios? a. subscripts c. reactants b. coefficients d. products 41. What is the mole ratio of nitrogen (N 2) to ammonia (NH 3) in the following chemical equation? N 2 + 3H 2 2NH 3 a. 1:1 c. 1:3 b. 1:2 d. 2:3 42. What is an excess reactant? a. The reactant in a chemical reaction that limits the amount of product made. b. The reactant in a chemical reaction that is left after at the end of reaction. c. The product in a chemical reaction that is formed. d. The product in a chemical reaction that reacts explosively. 43. What is the theoretical yield? a. The amount of product that is actually made from doing a lab experiment. b. The amount of reactants used in a lab experiment. c. The amount of product that is possible to make, based on calculations. d. The amount of both reactants and products. 44. What part of a chemical reaction limits the amount of product that can be made? a. all reactants b. excess reactant c. limiting reactant d. all products 45. In the equation 2KClO 3 2KCl + 3O 2, how many moles of O 2 are produced when 3.0 mol of KClO 3 decompose? a. 1.0 mol O 2 c. 3.0 mol O 2 b. 2.5 mol O 2 d. 4.5 mol O The number of moles in 20 grams of CaCO 3 is: a mol CaCO 3 c mol CaCO 3 b mol CaCO 3 d mol CaCO 3

5 47. For the reaction 2Na + 2H 2O 2NaOH + H 2, how many grams of NaOH are produced from 3.0 moles of H 2O? a g NaOH c g NaOH b g NaOH d g NaOH 48. What is the mass in grams of 2.00 moles of SO 2? a g SO 2 c g SO 2 b g SO 2 d g SO What is the actual yield? a. The amount of product that is actually made from doing a lab experiment. b. The amount of reactants used in a lab experiment. c. The amount of product that is possible to make, based on calculations. d. The amount of both reactants and products. 50. What is a limiting reactant? a. The reactant in a chemical reaction that limits the amount of product made. b. The reactant in a chemical reaction that is left after at the end of reaction. c. The product in a chemical reaction that is formed. d. The product in a chemical reaction that reacts explosively. 51. What part of a chemical reaction has a left over amount after the product is made? a. all reactants b. excess reactant c. limiting reactant d. all products 52. WATER AND SOLUTIONS The rule like dissolves like refers to a. polar dissolves polar c. polar dissolves everything b. polar dissolves non-polar d. polar does not dissolve anything 53. A paper clip can rest on the surface of water because the hydrogen bonds stay intact. This property of water is called a. high boiling point c. high surface tension b. polar bonds d. capillary action 54. The ability for water molecules to stick to other water molecules is called a. capillary action. c. cohesion. b. adhesion. d. friendship. 55. Which of the following does NOT increase the rate of dissolving a solid in water? a. raising the temperature c. using larger pieces of solid b. stirring d. crushing the solid into smaller pieces 56. Which of the following will dissolve the fastest? a. sugar cubes in cold water c. powdered sugar in cold water b. sugar cubes in hot water d. powdered sugar in hot water 57. Using the solubility graph, what type of solution would be formed from a 120 g sample of NaNO 3 at 30 C? a. unsaturated c. supersaturated b. saturated d. super duper saturated

6 58. What property of water describes water resembling a magnet (having + and - ends)? a. Hydrogen bonds c. High surface tension b. High boiling point d. Polar bonds 59. If the amount of dissolved solute in a solution at a given temperature is more than the amount that can permanently remain in solution at that temperature, the solution is said to be a. saturated. c. supersaturated. b. unsaturated. d. diluted. 60. Using the solubility graph, which salt s solubility is least affected by a change in temperature? a. KCl c. NaCl b. KNO 3 d. NH Which of the following will dissolve the slowest? a. large salt crystals in unstirred water c. small salt crystals in unstirred water b. large salt crystals in stirred water d. small salt crystals in stirred water 62. What phase change is water going through when the temperature remains constant at 100 C while adding energy? a. freezing c. condensing b. melting d. boiling 63. What state of matter is water found in between 0 C and 100 C? a. solid c. gas b. liquid d. plasma 64. Using the solubility graph, which salt has the greatest INCREASE in solubility as the temperature increases? a. NaNO 4 c. NaCl b. KNO 3 d. NH If the amount of solute present in a solution at a given temperature is less than the maximum amount that can dissolve at that temperature, the solution is said to be a. saturated. c. supersaturated. b. unsaturated. d. concentrated. 66. As temperature increases, solubility of gases in liquids (think of soda!) a. increases. c. can increase or decrease. b. decreases. d. is not affected. 67. Using the solubility graph, how many grams of KNO 3 can be dissolved at 60 C to make a saturated solution? a. 100 g c. 110 g b. 105 g d. 115 g 68. Using the solubility graph, which salt has the highest solubility at 10 C? a. KClO 3 c. SO 2 b. KNO 3 d. KI 69. Using the solubility graph, which 2 salts have the same solubility at about 43 C? a. NaNO 3 and HCl c. NH 4Cl and Na 2SO 4 b. NH 3 and Na 2SO 4 d. KClO 3 and Na 2SO 4

7 70. Using the solubility graph, if a solution contains 90 grams of NaNO 3 at 40 C, is the solution saturated, unsaturated, or supersaturated? a. saturated c. supersaturated b. unsaturated d. super-duper saturated 71. Using the solubility graph, how many grams of NH 4Cl are needed at 70 C to make a saturated solution? a. 60 g c. 50 g b. 35 g d. 45 g 72. You need to make a 4 L of a 0.75 M solution of NaOH. What would the original volume have been if the original concentration was 12 M? Use: C 1V 1 = C 2V 2. a L c L b. 3 L d. 4 L 73. In your water phase change graph, what state of matter is water found in between points A and B? a. solid c. gas b. liquid d. plasma 74. How many moles are in 3.5 L solution with a concentration of 2.5 M? Use: C = mol V a mol c. 1.4 mol b mol d. 6 mol 75. What is the concentration of a solution that has 12.8 mol of KOH in a 250 ml solution? Use: C = mol V a M c M b M d M 76. ACIDS, BASES, AND ph Acids react with a. bases to produce salts and water. c. water to produce bases and salts. b. salts to produce bases and water. d. neither bases, salts, nor water. 77. What is the correct formula for nitrous acid? a. HNO 3 c. H(NO 2) 2 b. HNO 2 d. HN 78. What is the correct name for H 2SO 4? a. Hydrosulfuric acid c. Sulfuric acid b. Hydrogen sulfide d. Sulfurous acid 79. What is the correct name for HCl? a. hydroiodic acid c. chlorous acid b. chloric acid d. hydrochloric acid 80. What is the correct name for KOH? a. potassium oxide c. sodium hydroxide b. potassium hydroxide d. potassium oxygen hydrogen

8 81. What is the correct name for Ca(OH) 2? a. Carbon hydroxide c. Calcium II hydroxide b. Calcium hydride d. Calcium hydroxide 82. What is the correct name for H 3PO 4? a. Hydrophosphoric acid c. Hydrogen phosphide b. Phosphorous acid d. Phosphoric acid 83. Given the data below, identify the sample that is most likely the most acidic. Sample ph meter reading A B 9.35 C 1.30 D 5.23 WATER 7.00 a. Sample A c. Sample C b. Sample B d. Sample D 84. What is an Arrhenius acid? a. a compound that increases the concentration of hydrogen ions in solution b. a compound that increases the concentration of hydroxide ions in solution c. a compound that decreases the concentration of hydrogen ions in solution d. a compound that decreases the concentration of hydroxide ions in solution 85. A proton acceptor is a a. traditional base. c. Brønsted-Lowry base. b. Brønsted-Lowry acid. d. Lewis base. 86. Bases taste a. soapy. c. sweet. b. sour. d. bitter. 87. Acids generally release H 2 gas when they react with a. nonmetals. c. metals. b. semimetals. d. gases. 88. Determine the type of salt from the following neutralization reaction: HNO 3 + LiOH H 2O + LiNO 3 a. acidic c. neutral b. basic d. none of the above 89. Determine the type of salt from the following neutralization reaction: H 3PO 4 + Ca(OH) 2 H 2O + Ca 3(PO 4) 2 a. acidic c. neutral b. basic d. none of the above 90. A chemical that changes color in the presence of an acid or a base is a(n). a. buffer c. indicator b. solvent d. electrolyte

9 91. Which of the following is a binary acid? a. H 2SO 4 c. HBr b. HNO 2 d. NaOH 92. A property that is shared by acids and bases is a. both have a ph less than 7. c. both taste bitter. b. both conduct electricity. d. both have hydroxide ions. 93. A substance that produces OH -1 ions in a water solution is a(n) a. acid c. salt b. base d. non-electrolyte 94. Acids taste a. soapy. c. sweet. b. sour. d. bitter. 95. What is an Arrhenius base? a. a compound that increases the concentration of hydrogen ions in solution b. a compound that increases the concentration of hydroxide ions in solution c. a compound that decreases the concentration of hydrogen ions in solution d. a compound that decreases the concentration of hydroxide ions in solution 96. Which of the following is an oxyacid? a. H 2CO 3 c. HCl b. HBr d. NaOH 97. A substance that produces H +1 ions in a water solution is a(n) a. acid c. salt b. base d. non-electrolyte 98. A proton donor is a a. traditional base. c. Brønsted-Lowry base. b. Brønsted-Lowry acid. d. Lewis base. 99. Soda has a ph of 4. Based on the ph value, what type of substance is this? a. acidic c. neutral b. basic d. none of the above 100. Baking soda is used to neutralize hydrochloric acid, which was spilled in the lab. What type of substance is baking soda? a. acidic c. neutral b. basic d. none of the above

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