Honors Chemistry Final Study Key
Honors Chemistry Final Exam Study Guide Multiple Choice- (51 points @ 1/2 point ea.)
Identify the letter of the choice that best completes the statement or answers the question. ____ 1. The pair of elements that forms a bond with the least ionic character is
|a. |Na and Cl. |c. |O and Cl. |
|b. |K and Cl. |d. |Mg and Cl. |
____ 2. The B—F bond in BF3 (electronegativity for B is 2.0; electronegativity for F is 4.0) is
|a. |polar covalent. |c. |nonpolar covalent. …show more content…
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|b. |ionic. |d. |metallic. |
____ 3. In the three molecules, O2, HCl, and F2, what atom would have a partial negative charge?
|a. |oxygen |c. |chlorine |
|b. |hydrogen |d. |fluorine |
____ 4. The percentage ionic character and the type of bond in Br2 (electronegativity for Br is 2.8) is
|a. |0%; nonpolar covalent. |c. |0%; pure ionic. |
|b. |100%; polar covalent. |d. |100%; pure ionic. |
____ 5. The substance whose Lewis structure shows three covalent bonds is
|a. |H2O. |c. |NH3. |
|b. |CH2Cl2. |d. |CCl4. |
____ 6. What is the correct Lewis structure for hydrogen chloride, HCl? [pic][pic] |a. |A |c. |C |
|b. |B |d. |D |
____ 7. How many extra electrons are in the Lewis structure of the phosphate ion, PO43–?
|a. |0 |c. |3 |
|b. |2 |d. |4 |
____ 8. How many electrons must be shown in the Lewis structure of the hydroxide ion, OH–?
|a. |1 |c. |9 |
|b. |8 |d. |10 |
____ 9. Use VSEPR theory to predict the shape of the hydrogen chloride molecule, HCl.
|a. |tetrahedral |c. |bent |
|b. |linear |d. |trigonal-planar |
____ 10. Use VSEPR theory to predict the shape of the magnesium hydride molecule, MgH2.
|a. |tetrahedral |c. |bent |
|b. |linear |d. |octahedral |
____ 11. Use VSEPR theory to predict the shape of the carbon tetraiodide molecule, CI4.
|a. |tetrahedral |c. |bent |
|b. |linear |d. |trigonal-planar |
____ 12. Use VSEPR theory to predict the shape of the chlorate ion, ClO3–.
|a. |trigonal-planar |c. |trigonal-pyramidal |
|b. |octahedral |d. |bent |
____ 13. Use VSEPR theory to predict the shape of carbon dioxide, CO2.
|a. |tetrahedral |c. |bent |
|b. |linear |d. |octahedral |
____ 14. The following molecules contain polar bonds. The only polar molecule is
|a. |CCl4. |c. |NH3. |
|b. |CO2. |d. |CH4. |
____ 15. What is the formula for zinc fluoride?
|a. |ZnF |c. |Zn2F |
|b. |ZnF2 |d. |Zn2F3 |
____ 16. What is the formula for the compound formed by calcium ions and chloride ions?
|a. |CaCl |c. |CaCl3 |
|b. |Ca2Cl |d. |CaCl2 |
____ 17. What is the formula for the compound formed by lead(II) ions and chromate ions?
|a. |PbCrO4 |c. |Pb2(CrO4)3 |
|b. |Pb2CrO4 |d. |Pb(CrO4)2 |
____ 18. What is the formula for aluminum sulfate?
|a. |AlSO4 |c. |Al2(SO4)3 |
|b. |Al2SO4 |d. |Al(SO4)3 |
____ 19. What is the formula for barium hydroxide?
|a. |BaOH |c. |Ba(OH)2 |
|b. |BaOH2 |d. |Ba(OH) |
____ 20. Name the compound Ni(ClO3)2.
|a. |nickel(II) chlorate |c. |nickel(II) chlorite |
|b. |nickel(II) chloride |d. |nickel(II) peroxide |
____ 21. Name the compound Zn3(PO4)2.
|a. |zinc potassium oxide |c. |zinc phosphate |
|b. |trizinc polyoxide |d. |zinc phosphite |
____ 22. Name the compound Fe(NO3)2.
|a.
|iron(II) nitrate |c. |iron(III) nitrate |
|b. |iron(II) nitrite |d. |iron(III) nitride |
____ 23. Name the compound Al2S3.
|a. |aluminum sulfate |c. |aluminum(II) sulfate |
|b. |aluminum sulfur |d. |aluminum sulfide |
____ 24. What is the oxidation number of hydrogen in H2O?
|a. |0 |c. |+2 |
|b. |+1 |d. |+3 |
____ 25. What is the oxidation number of sulfur in SO2?
|a. |0 |c. |+2 |
|b. |+1 |d. |+4 …show more content…
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____ 26. What is the oxidation number of sulfur in H2SO4?
|a. |–2 |c. |+4 |
|b. |0 |d. |+6 |
____ 27. What is the oxidation number of oxygen in CO2?
|a.
|–4 |c. |0 |
|b. |–2 |d. |+4 |
____ 28. Name the compound N2O2 using the Stock system.
|a. |dinitrogen monoxide |c. |nitrogen(II) oxide |
|b. |nitrogen dioxide |d. |nitrogen oxide(II) |
____ 29. Name the compound SO2 using the Stock system.
|a. |sulfur(II) oxide |c. |sulfur dioxide |
|b. |sulfur(IV) oxide |d. |sulfur oxide |
____ 30. Name the compound CCl4 using the Stock system.
|a. |carbon(IV) chloride |c. |carbon chloride |
|b. |carbon tetrachloride |d. |carbon hypochlorite |
____ 31. Name the compound H2O using the Stock
system.
|a. |water |c. |hydrogen(I) oxide |
|b. |hydrogen dioxide |d. |hydrogen(II) oxide |
____ 32. Name the compound PBr5 using the Stock system.
|a. |potassium hexabromide |c. |phosphorus(V) bromide |
|b. |phosphorus(V) pentabromide |d. |phosphoric acid |
____ 33. What is the formula mass of magnesium chloride, MgCl2?
|a. |46 amu |c. |95.21 amu |
|b. |59.76 amu |d. |106.35 amu |
____ 34. What is the formula mass of ethyl alcohol, C2H5OH?
|a. |30.33 amu |c. |45.06 amu |
|b. |33.27 amu |d. |46.08 amu |
____ 35. What is the formula mass of (NH4)2SO4?
|a. |114.09 amu |c. |128.06 amu |
|b. |118.34 amu |d. |132.16 amu |
____ 36. The molar mass of NO2 is 46.01 g/mol. How many moles of NO2 are present in 114.95 g?
|a. |0.4003 mol |c. |2.498 mol |
|b. |1.000 mol |d. |114.95 mol |
____ 37. The molar mass of CCl4 is 153.81 g/mol. How many grams of CCl4 are needed to have 5.000 mol?
|a. |5 g |c. |769.0 g |
|b. |30.76 g |d. |796.05 g |
____ 38. The molar mass of H2O is 18.02 g/mol. How many grams of H2O are present in 0.20 mol?
|a. |0.2 g |c. |35.9 g |
|b. |3.6 g |d. |89.9 g |
____ 39. 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 |
____ 40. What is the mass of 0.240 mol glucose, C6H12O6?
|a. |24.0 g |c. |180.16 g |
|b. |43.2 g |d. |750. g |
____ 41. How many Cl– ions are present in 2.00 mol of KCl?
|a. |1.20 [pic] 1024 |c. |2.00 |
|b. |6.02 [pic] 1024 |d. |0.5 |
____ 42. How many OH– ions are present in 3.00 mol of Ca(OH)2?
|a. |3.00 |c. |3.61 [pic] 1024 |
|b. |6.00 |d. |2.06 [pic] 1023 |
____ 43. How many oxygen atoms are there in 0.500 mol of CO2?
|a. |6.02 [pic]€1023 |c. |15.9994 |
|b. |3.01 [pic] 1023 |d. |11.0 |
____ 44. How many Mg2+ ions are found in 1.00 mol of MgO?
|a. |3.01 [pic] 1023 |c. |12.04 [pic] 1023 |
|b. |6.02 [pic] 1023 |d. |6.02 [pic] 1025 |
____ 45. If 0.500 mol of Na+ combines with 0.500 mol of Cl– to form NaCl, how many formula units of NaCl are present?
|a. |3.01 [pic] 1023 |c. |6.02 [pic] 1024 |
|b. |6.02 [pic] 1023 |d. |1 |
____ 46. How many molecules are there in 5.0 g of methyl alcohol, CH3OH?
|a. |9.4 [pic] 1022 |c. |3.6 [pic] 1024 |
|b. |3.0 [pic] 1024 |d. |3.8 [pic] 1024 |
____ 47. What is the percentage composition of CuCl2?
|a. |33% Cu, 66% Cl |c. |65.50% Cu, 34.50% Cl |
|b. |50% Cu, 50% Cl |d. |47.27% Cu, 52.73% Cl |
____ 48. What is the mass percentage of OH– in Ca(OH)2?
|a. |45.9% |c. |75% |
|b. |66.6% |d. |90.1% |
____ 49. What is the mass percentage of chlorine in NaCl?
|a. |35.45% |c. |60.7% |
|b. |50% |d. |64.5% |
____ 50. What is the empirical formula for a compound that is 31.9% potassium, 28.9% chlorine, and 39.2% oxygen?
|a. |KClO2 |c. |K2Cl2O3 |
|b. |KClO3 |d. |K2Cl2O5 |
____ 51. What is the empirical formula for a compound that is 53.3% O and 46.7% Si?
|a. |SiO |c. |Si2O |
|b. |SiO2 |d. |Si2O3 |
____ 52. A compound contains 259.2 g of F and 40.8 g of C. What is the empirical formula for this compound?
|a. |CF4 |c. |CF |
|b. |C4F |d. |CF2 |
____ 53. A compound contains 64 g of O and 8 g of H. What is the empirical formula for this compound?
|a. |H2O |c. |HO2 |
|b. |H2O2 |d. |HO |
____ 54. A compound contains 27.3 g of C and 72.7 g of O. What is the empirical formula for this compound?
|a. |CO |c. |C2O |
|b. |CO2 |d. |C2O4 |
____ 55. The molecular formula for vitamin C is C6H8O6. What is the empirical formula?
|a. |CHO |c. |C3H4O3 |
|b. |CH2O |d. |C2H4O2 |
____ 56. Of the following molecular formulas for hydrocarbons, which is an empirical formula?
|a. |CH4 |c. |C3H6 |
|b. |C2H2 |d. |C4H10 |
____ 57. Which of the following molecular formulas does not have the corresponding empirical formula XY2Z?
|a. |X2Y4Z2 |c. |X6Y12Z6 |
|b. |XYZ |d. |X3Y6Z3 |
____ 58. A compound's empirical formula is C2H5. If the formula mass is 58 amu, what is the molecular formula?
|a. |C3H6 |c. |C5H8 |
|b. |C4H10 |d. |C5H15 |
____ 59. A compound's empirical formula is N2O5. If the formula mass is 108 amu, what is the molecular formula?
|a. |N2O5 |c. |NO3 |
|b. |N4O10 |d. |N2O4 |
____ 60. A compound's empirical formula is NO2. If the formula mass is 92 amu, what is the molecular formula?
|a. |NO |c. |NO4 |
|b. |N2O2 |d. |N2O4 |
____ 61. A compound's empirical formula is CH3. If the formula mass is 30 amu, what is the molecular formula?
|a. |CH3 |c. |C2H6 |
|b. |CH4 |d. |C3H9 |
____ 62. A compound's empirical formula is HO. If the formula mass is 34 amu, what is the molecular formula?
|a. |H2O |c. |HO3 |
|b. |H2O2 |d. |H2O3 |
____ 63. When the equation Fe3O4 + Al → Al2O3 + Fe is correctly balanced, what is the coefficient of Fe?
|a. |3 |c. |6 |
|b. |4 |d. |9 |
____ 64. Which coefficients correctly balance the formula equation
NH4NO2(s)→ N2(g) + H2O(l)?
|a. |1, 2, 2 |c. |2, 1, 1 |
|b. |1, 1, 2 |d. |2, 2, 2 |
____ 65. The complete balanced equation for the reaction between zinc hydroxide and acetic acid is
|a. |ZnOH + CH3COOH → ZnCH3COO + H2O. |
|b. |Zn(OH)2 + CH3COOH → Zn + 2CO2 +3H2O. |
|c. |Zn(OH)2 + 2CH3COOH → Zn(CH3COO)2 + 2H2O. |
|d. |Zn(OH)2 + 2CH3COOH → Zn(CH3COO)2 + H2 + O2. |
____ 66. What is the balanced equation for the combustion of sulfur?
|a. |S(s) + O2(g) → SO(g) |
|b. |S(s) + O2(g) → SO2(g) |
|c. |2S(s) + 3O2(g) → SO3(s) |
|d. |S(s) + 2O2(g) → SO42–(aq) |
____ 67. Which equation is not balanced?
|a. |2H2 + O2 → 2H2O |
|b. |4H2 + 2O2 → 4H2O |
|c. |H2 + H2 + O2 → H2O + H2O |
|d. |2H2 + O2 → H2O |
____ 68. The reaction of calcium oxide, CaO, with water yields
|a. |calcium and oxygen gas. |c. |calcium and a salt. |
|b. |calcium hydroxide. |d. |carbon dioxide and water. |
____ 69. Predict the product of the reaction represented by the following equation:
MgO + CO2 →
|a. |MgCO3 |c. |MgC + O3 |
|b. |Mg + CO3 |d. |MgCO2 + O |
____ 70. Magnesium hydroxide decomposes to yield magnesium oxide and
|a. |hydrogen. |c. |water. |
|b. |oxygen. |d. |salt. |
____ 71. When sodium chlorate, NaClO3, decomposes, the products are
|a. |sodium hydroxide and water. |c. |sodium and chlorine oxide. |
|b. |sodium oxide and chlorine. |d. |sodium chloride and oxygen. |
____ 72. If chlorine gas is produced by halogen replacement, the other halogen in the reaction must be
|a. |bromine. |c. |astatine. |
|b. |iodine. |d. |fluorine. |
____ 73. What is the balanced equation when aluminum reacts with copper(II) sulfate?
|a. |Al + Cu2S → Al2S + Cu |
|b. |2Al + 3CuSO4 → Al2(SO4)3 + 3Cu |
|c. |Al + CuSO4 → AlSO4 + Cu |
|d. |2Al + Cu2SO4 → Al2SO4 + 2Cu |
____ 74. Predict what happens when calcium metal is added to a solution of magnesium chloride.
|a. |No reaction occurs. |c. |Magnesium calcite forms. |
|b. |Calcium chloride forms. |d. |Gaseous calcium is produced. |
____ 75. Predict what happens when zinc is added to water.
|a. |No reaction occurs. |c. |Zinc oxide forms. |
|b. |Steam is produced. |d. |Hydrogen is released. |
____ 76. Predict what happens when lead is added to nitric acid.
|a. |No reaction occurs. |c. |Lead oxide forms. |
|b. |Oxygen is released. |d. |Hydrogen is released. |
____ 77. Predict what happens when nickel is added to a solution of potassium chloride.
|a. |No reaction occurs. |c. |Potassium nickel chloride forms. |
|b. |Nickel chloride forms. |d. |Hydrochloric acid forms. |
____ 78. Magnesium bromide (aq) + chlorine (g) yields
|a. |Mg(s) and BrCl(aq). |c. |MgBrCl(aq). |
|b. |MgCl(aq) and Br2(l). |d. |MgCl2(aq) and Br2(l). |
____ 79. Which reaction does not occur?
|a. |2HF(aq) + Cl2(g) → F2(g) + 2HCl(aq) |
|b. |2Na(s) + ZnF2(aq) → 2NaF(aq) + Zn(s) |
|c. |Fe(s) + CuCl2(aq) → FeCl2(aq) + Cu(s) |
|d. |2HCl(aq) + Mg(s) → MgCl2(aq) + H2(g) |
____ 80. Which reaction can be predicted from the activity series?
|a. |2Cl(g) → Cl2(g) |
|b. |HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) |
|c. |2H2O(aq) + 2Na(s) → 2NaOH(aq) + H2(g) |
|d. |Cl2(g) → 2Cl(g) |
____ 81. If 63.5 g of copper (Cu) combine with 16 g of oxygen (O) to form the compound CuO, how many grams of oxygen will be needed to combine with the same amount of copper to form the compound CuO2?
|a. |16 g |c. |64 g |
|b. |32 g |d. |127 g |
____ 82. Carbon-14 (atomic number 6), the radioactive nuclide used in dating fossils, has
|a. |6 neutrons. |c. |10 neutrons. |
|b. |8 neutrons. |d. |14 neutrons. |
____ 83. Phosphorus-33 (atomic number 15) contains
|a. |33 protons. |c. |33 neutrons. |
|b. |18 neutrons. |d. |18 protons. |
____ 84. The mass of a sample containing 3.5 mol of silicon atoms (atomic mass 28.0855 amu) is approximately
|a. |28 g. |c. |72 g. |
|b. |35 g. |d. |98 g. |
____ 85. A prospector finds 39.39 g of pure gold (atomic mass 196.9665 amu). She has
|a. |1.204 × 1023 atoms of Au. |c. |4.306 × 1023 atoms of Au. |
|b. |2.308 × 1023 atoms of Au. |d. |6.022 × 1023 atoms of Au. |
____ 86. A sample of tin (atomic mass 118.71 amu) contains 3.01 × 1023 atoms. The mass of the sample is
|a. |3.01 g. |c. |72.6 g. |
|b. |59.3 g. |d. |11 g. |
____ 87. According to Bohr, electrons cannot reside at ____ in the figure below. [pic] |a. |point A |c. |point C |
|b. |point B |d. |point D |
____ 88. A sample of gold has a mass of 96.5 g and a volume of 5.00 cm3. The density of gold is
|a. |0.0518 g/cm3. |c. |101.5 g/cm3. |
|b. |19.3 g/cm3. |d. |483 g/cm3. |
____ 89. When 5.7 m is divided by 2 s, the quotient is correctly reported as
|a. |2.8 m/s. |c. |2.9 m/s. |
|b. |2.85 m/s. |d. |3 m/s. |
____ 90. How would 0.00930 m be expressed in scientific notation?
|a. |93 × 10–4 m |c. |9.30 × 10–3 m |
|b. |9.3 × 10–4 m |d. |9.30 × 10–5 m |
____ 91. The speed of light is 300 000 km/s. In scientific notation, this speed is written to one significant figure as
|a. |3 × 105 km/s. |c. |3. × 106 km/s. |
|b. |3.0 × 105 km/s. |d. |3.0 × 106 km/s. |
____ 92. When 1.92 × 10–6 kg is divided by 6.8 × 102 mL, the quotient equals
|a. |2.8 × 10–4 kg/mL. |c. |2.8 × 10–8 kg/mL. |
|b. |2.8 × 10–5 kg/mL. |d. |2.8 × 10–9 kg/mL. |
____ 93. Which coefficients correctly balance the formula equation CaO + H2O → Ca(OH)2?
|a. |2, 1, 2 |c. |1, 2, 1 |
|b. |1, 2, 3 |d. |1, 1, 1 |
____ 94. The formulas for the products of the reaction between sodium hydroxide and sulfuric acid are
|a. |Na2SO4 and H2O. |c. |SI4 and Na2O. |
|b. |NaSO4 and H2O. |d. |S + O2 and Na. |
____ 95. Which word equation represents the reaction that produces water from hydrogen and oxygen?
|a. |Water is produced from hydrogen and oxygen. |
|b. |Hydrogen plus oxygen yields water. |
|c. |H2 + O2 → water. |
|d. |Water can be separated into hydrogen and oxygen. |
____ 96. The reaction represented by the equation Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq) is a
|a. |composition reaction. |c. |single-displacement reaction. |
|b. |decomposition reaction. |d. |double-displacement reaction. |
____ 97. The reaction represented by the equation Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) is a
|a. |double-displacement reaction. |c. |decomposition reaction. |
|b. |synthesis reaction. |d. |combustion reaction. |
____ 98. An active metal and a halogen react to form a(n)
|a. |salt. |c. |acid. |
|b. |hydroxide. |d. |oxide. |
____ 99. When a binary compound decomposes, what is produced?
|a. |an oxide |c. |a tertiary compound |
|b. |an acid |d. |two elements |
____ 100. Many metal hydroxides decompose when heated to yield metal oxides and
|a. |metal hydrides. |c. |carbon dioxide. |
|b. |water. |d. |an acid. |
____ 101. In the equation 2Al(s) + 3Fe(NO3)2(aq) → 3Fe(s) + 2Al(NO3)3(aq), iron has been replaced by
|a. |nitrate. |c. |aluminum. |
|b. |water. |d. |nitrogen. |
____ 102. If a certain metal is placed in an ionic solution containing another metal and no reaction occurs, then the metal originally in the solution is
|a. |a halogen. |c. |not on the activity series. |
|b. |higher on the activity series. |d. |unreactive. |
Short Answer- 10 points ( 5 points ea.) 103. How does the figure below illustrate Hund's rule? [pic] 104. How does the figure above illustrate the Pauli exclusion principle? Problem- Please complete all problem solving during homework assignments. On the exam only 5 will be selected. (10 points) 105. How many atoms are present in 80.0 mol of zirconium? 106. Determine the mass in grams of 10.0 mol of bromine. The molar mass of bromine is 79.90 g/mol. 107. Calculate the mass in grams of 9.00 mol of potassium (molar mass 39.10 g/mol). 108. Calculate the number of atoms in 10.0 g of sulfur (molar mass 32.07 g/mol). Use the periodic table below to answer the following questions. [pic] 109. Write the noble-gas electron configuration for silicon. 110. Which element has the following electron configuration: [Ar] 4s2 3d10 4p5? 111. Draw the orbital diagram for phosphorus. 112. Draw the orbital diagram for argon. 113. What is the half-life of an isotope if after 2.00 weeks you have 31.25 g remaining from a 250.0 g starting sample size? 114. Write the electron configuration for nitrogen, atomic number 7. 115. Write the noble-gas electron configuration represented in the orbital diagram below. [pic] 116. Draw a Lewis structure for the oxalate ion, C2O42–. 117. Draw a Lewis structure for the nitrate ion, [pic]. Use VSEPR theory to predict its molecular geometry. 118. Tell what type of chemical reaction is represented by the following formula equation. Then balance the equation.
KBr(aq) + Mg(OH)2(aq) [pic] KOH(aq) + MgBr2(aq) 119. Phosphorus-32 has a half-life of 14.3 days. How many milligrams of phosphorus-32 remain after 71.5 days if you start with 4.00 mg of the isotope? Essay-- Please choose ONE Essay. Submit a two- page summary, size 12 font and double-spaced. Bring the essay the DAY OF THE FINAL EXAM TO CLASS. READY TO BE SUBMITTED. (30 points) 120. Why are enzymes essential to life? Why are enzymes classified as catalysts? 121. Even though some animals are completely carnivorous, eating only other animals, their energy actually comes from the sun. Explain.
Honors Chemistry Final Exam Study Guide
Answer Section MULTIPLE CHOICE 1. ANS: D DIF: III REF: 1 OBJ: 5 2. ANS: B DIF: III REF: 1 OBJ: 5 3. ANS: C DIF: III REF: 1 OBJ: 5 4. ANS: A DIF: III REF: 1 OBJ: 5 5. ANS: C DIF: III REF: 2 OBJ: 5 6. ANS: D DIF: III REF: 2 OBJ: 5 7. ANS: C DIF: III REF: 3 OBJ: 4 8. ANS: B DIF: III REF: 3 OBJ: 4 9. ANS: B DIF: III REF: 5 OBJ: 2 10. ANS: B DIF: III REF: 5 OBJ: 2 11. ANS: A DIF: III REF: 5 OBJ: 2 12. ANS: C DIF: III REF: 5 OBJ: 2 13. ANS: B DIF: III REF: 5 OBJ: 2 14. ANS: C DIF: III REF: 5 OBJ: 5 15. ANS: B DIF: III REF: 1 OBJ: 2 16. ANS: D DIF: III REF: 1 OBJ: 2 17. ANS: A DIF: III REF: 1 OBJ: 2 18. ANS: C DIF: III REF: 1 OBJ: 2 19. ANS: C DIF: III REF: 1 OBJ: 2 20. ANS: A DIF: III REF: 1 OBJ: 3 21. ANS: C DIF: III REF: 1 OBJ: 3 22. ANS: A DIF: III REF: 1 OBJ: 3 23. ANS: D DIF: III REF: 1 OBJ: 3 24. ANS: B DIF: III REF: 2 OBJ: 2 25. ANS: D DIF: III REF: 2 OBJ: 2 26. ANS: D DIF: III REF: 2 OBJ: 2 27. ANS: B DIF: III REF: 2 OBJ: 2 28. ANS: C DIF: III REF: 2 OBJ: 3 29. ANS: B DIF: III REF: 2 OBJ: 3 30. ANS: A DIF: III REF: 2 OBJ: 3 31. ANS: C DIF: III REF: 2 OBJ: 3 32. ANS: C DIF: III REF: 2 OBJ: 3 33. ANS: C DIF: III REF: 3 OBJ: 1 34. ANS: D DIF: III REF: 3 OBJ: 1 35. ANS: D DIF: III REF: 3 OBJ: 1 36. ANS: C
Solution:
[pic] DIF: III REF: 3 OBJ: 2 37. ANS: C
Solution:
[pic] DIF: III REF: 3 OBJ: 2 38. ANS: B
Solution:
[pic] DIF: III REF: 3 OBJ: 2 39. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 2 40. ANS: B
Solution:
[pic] DIF: III REF: 3 OBJ: 2 41. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 3 42. ANS: C
Solution:
[pic] DIF: III REF: 3 OBJ: 3 43. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 3 44. ANS: B
Solution:
[pic] DIF: III REF: 3 OBJ: 3 45. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 3 46. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 3 47. ANS: D
Solution:
[pic] DIF: III REF: 3 OBJ: 4 48. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 4 49. ANS: C
Solution:
[pic] DIF: III REF: 3 OBJ: 4 50. ANS: B
Solution:
[pic] DIF: III REF: 4 OBJ: 2 51. ANS: B
Solution:
[pic] DIF: III REF: 4 OBJ: 2 52. ANS: A
Solution:
[pic] DIF: III REF: 4 OBJ: 2 53. ANS: A
Solution:
[pic] DIF: III REF: 4 OBJ: 2 54. ANS: B
Solution:
[pic] DIF: III REF: 4 OBJ: 2 55. ANS: C DIF: III REF: 4 OBJ: 3 56. ANS: A DIF: III REF: 4 OBJ: 3 57. ANS: B DIF: III REF: 4 OBJ: 4 58. ANS: B
Solution:
[pic] DIF: III REF: 4 OBJ: 4 59. ANS: A
Solution:
[pic] DIF: III REF: 4 OBJ: 4 60. ANS: D
Solution:
[pic] DIF: III REF: 4 OBJ: 4 61. ANS: C
Solution:
[pic] DIF: III REF: 4 OBJ: 4 62. ANS: B
Solution:
[pic] DIF: III REF: 4 OBJ: 4 63. ANS: D DIF: III REF: 1 OBJ: 4 64. ANS: B DIF: III REF: 1 OBJ: 4 65. ANS: C DIF: III REF: 1 OBJ: 4 66. ANS: B DIF: III REF: 1 OBJ: 4 67. ANS: D DIF: III REF: 1 OBJ: 4 68. ANS: B DIF: III REF: 2 OBJ: 5 69. ANS: A DIF: III REF: 2 OBJ: 5 70. ANS: C DIF: III REF: 2 OBJ: 5 71. ANS: D DIF: III REF: 2 OBJ: 5 72. ANS: D DIF: III REF: 2 OBJ: 5 73. ANS: B DIF: III REF: 2 OBJ: 5 74. ANS: B DIF: III REF: 3 OBJ: 2 75. ANS: A DIF: III REF: 3 OBJ: 2 76. ANS: D DIF: III REF: 3 OBJ: 2 77. ANS: A DIF: III REF: 3 OBJ: 2 78. ANS: D DIF: III REF: 3 OBJ: 2 79. ANS: A DIF: III REF: 3 OBJ: 2 80. ANS: C DIF: III REF: 3 OBJ: 2 81. ANS: B DIF: III REF: 1 OBJ: 1 82. ANS: B DIF: III REF: 3 OBJ: 3 83. ANS: B DIF: III REF: 3 OBJ: 3 84. ANS: D
Solution: [pic] DIF: III REF: 3 OBJ: 5 85. ANS: A
Solution: [pic] DIF: III REF: 3 OBJ: 5 86. ANS: B
Solution: [pic] DIF: III REF: 3 OBJ: 5 87. ANS: C DIF: III REF: 1 OBJ: 4 88. ANS: B
Solution: [pic] DIF: III REF: 2 OBJ: 4 89. ANS: D DIF: III REF: 3 OBJ: 3 90. ANS: C DIF: III REF: 3 OBJ: 4 91. ANS: A DIF: III REF: 3 OBJ: 4 92. ANS: D DIF: III REF: 3 OBJ: 4 93. ANS: D DIF: III REF: 1 OBJ: 4 94. ANS: A DIF: III REF: 2 OBJ: 5 95. ANS: B DIF: II REF: 1 OBJ: 3 96. ANS: C DIF: II REF: 2 OBJ: 2 97. ANS: A DIF: II REF: 2 OBJ: 2 98. ANS: A DIF: II REF: 2 OBJ: 3 99. ANS: D DIF: II REF: 2 OBJ: 3 100. ANS: B DIF: II REF: 2 OBJ: 3 101. ANS: C DIF: II REF: 2 OBJ: 4 102. ANS: B DIF: II REF: 3 OBJ:
Identify the letter of the choice that best completes the statement or answers the question. ____ 1. The pair of elements that forms a bond with the least ionic character is
|a. |Na and Cl. |c. |O and Cl. |
|b. |K and Cl. |d. |Mg and Cl. |
____ 2. The B—F bond in BF3 (electronegativity for B is 2.0; electronegativity for F is 4.0) is
|a. |polar covalent. |c. |nonpolar covalent. …show more content…
|
|b. |ionic. |d. |metallic. |
____ 3. In the three molecules, O2, HCl, and F2, what atom would have a partial negative charge?
|a. |oxygen |c. |chlorine |
|b. |hydrogen |d. |fluorine |
____ 4. The percentage ionic character and the type of bond in Br2 (electronegativity for Br is 2.8) is
|a. |0%; nonpolar covalent. |c. |0%; pure ionic. |
|b. |100%; polar covalent. |d. |100%; pure ionic. |
____ 5. The substance whose Lewis structure shows three covalent bonds is
|a. |H2O. |c. |NH3. |
|b. |CH2Cl2. |d. |CCl4. |
____ 6. What is the correct Lewis structure for hydrogen chloride, HCl? [pic][pic] |a. |A |c. |C |
|b. |B |d. |D |
____ 7. How many extra electrons are in the Lewis structure of the phosphate ion, PO43–?
|a. |0 |c. |3 |
|b. |2 |d. |4 |
____ 8. How many electrons must be shown in the Lewis structure of the hydroxide ion, OH–?
|a. |1 |c. |9 |
|b. |8 |d. |10 |
____ 9. Use VSEPR theory to predict the shape of the hydrogen chloride molecule, HCl.
|a. |tetrahedral |c. |bent |
|b. |linear |d. |trigonal-planar |
____ 10. Use VSEPR theory to predict the shape of the magnesium hydride molecule, MgH2.
|a. |tetrahedral |c. |bent |
|b. |linear |d. |octahedral |
____ 11. Use VSEPR theory to predict the shape of the carbon tetraiodide molecule, CI4.
|a. |tetrahedral |c. |bent |
|b. |linear |d. |trigonal-planar |
____ 12. Use VSEPR theory to predict the shape of the chlorate ion, ClO3–.
|a. |trigonal-planar |c. |trigonal-pyramidal |
|b. |octahedral |d. |bent |
____ 13. Use VSEPR theory to predict the shape of carbon dioxide, CO2.
|a. |tetrahedral |c. |bent |
|b. |linear |d. |octahedral |
____ 14. The following molecules contain polar bonds. The only polar molecule is
|a. |CCl4. |c. |NH3. |
|b. |CO2. |d. |CH4. |
____ 15. What is the formula for zinc fluoride?
|a. |ZnF |c. |Zn2F |
|b. |ZnF2 |d. |Zn2F3 |
____ 16. What is the formula for the compound formed by calcium ions and chloride ions?
|a. |CaCl |c. |CaCl3 |
|b. |Ca2Cl |d. |CaCl2 |
____ 17. What is the formula for the compound formed by lead(II) ions and chromate ions?
|a. |PbCrO4 |c. |Pb2(CrO4)3 |
|b. |Pb2CrO4 |d. |Pb(CrO4)2 |
____ 18. What is the formula for aluminum sulfate?
|a. |AlSO4 |c. |Al2(SO4)3 |
|b. |Al2SO4 |d. |Al(SO4)3 |
____ 19. What is the formula for barium hydroxide?
|a. |BaOH |c. |Ba(OH)2 |
|b. |BaOH2 |d. |Ba(OH) |
____ 20. Name the compound Ni(ClO3)2.
|a. |nickel(II) chlorate |c. |nickel(II) chlorite |
|b. |nickel(II) chloride |d. |nickel(II) peroxide |
____ 21. Name the compound Zn3(PO4)2.
|a. |zinc potassium oxide |c. |zinc phosphate |
|b. |trizinc polyoxide |d. |zinc phosphite |
____ 22. Name the compound Fe(NO3)2.
|a.
|iron(II) nitrate |c. |iron(III) nitrate |
|b. |iron(II) nitrite |d. |iron(III) nitride |
____ 23. Name the compound Al2S3.
|a. |aluminum sulfate |c. |aluminum(II) sulfate |
|b. |aluminum sulfur |d. |aluminum sulfide |
____ 24. What is the oxidation number of hydrogen in H2O?
|a. |0 |c. |+2 |
|b. |+1 |d. |+3 |
____ 25. What is the oxidation number of sulfur in SO2?
|a. |0 |c. |+2 |
|b. |+1 |d. |+4 …show more content…
|
____ 26. What is the oxidation number of sulfur in H2SO4?
|a. |–2 |c. |+4 |
|b. |0 |d. |+6 |
____ 27. What is the oxidation number of oxygen in CO2?
|a.
|–4 |c. |0 |
|b. |–2 |d. |+4 |
____ 28. Name the compound N2O2 using the Stock system.
|a. |dinitrogen monoxide |c. |nitrogen(II) oxide |
|b. |nitrogen dioxide |d. |nitrogen oxide(II) |
____ 29. Name the compound SO2 using the Stock system.
|a. |sulfur(II) oxide |c. |sulfur dioxide |
|b. |sulfur(IV) oxide |d. |sulfur oxide |
____ 30. Name the compound CCl4 using the Stock system.
|a. |carbon(IV) chloride |c. |carbon chloride |
|b. |carbon tetrachloride |d. |carbon hypochlorite |
____ 31. Name the compound H2O using the Stock
system.
|a. |water |c. |hydrogen(I) oxide |
|b. |hydrogen dioxide |d. |hydrogen(II) oxide |
____ 32. Name the compound PBr5 using the Stock system.
|a. |potassium hexabromide |c. |phosphorus(V) bromide |
|b. |phosphorus(V) pentabromide |d. |phosphoric acid |
____ 33. What is the formula mass of magnesium chloride, MgCl2?
|a. |46 amu |c. |95.21 amu |
|b. |59.76 amu |d. |106.35 amu |
____ 34. What is the formula mass of ethyl alcohol, C2H5OH?
|a. |30.33 amu |c. |45.06 amu |
|b. |33.27 amu |d. |46.08 amu |
____ 35. What is the formula mass of (NH4)2SO4?
|a. |114.09 amu |c. |128.06 amu |
|b. |118.34 amu |d. |132.16 amu |
____ 36. The molar mass of NO2 is 46.01 g/mol. How many moles of NO2 are present in 114.95 g?
|a. |0.4003 mol |c. |2.498 mol |
|b. |1.000 mol |d. |114.95 mol |
____ 37. The molar mass of CCl4 is 153.81 g/mol. How many grams of CCl4 are needed to have 5.000 mol?
|a. |5 g |c. |769.0 g |
|b. |30.76 g |d. |796.05 g |
____ 38. The molar mass of H2O is 18.02 g/mol. How many grams of H2O are present in 0.20 mol?
|a. |0.2 g |c. |35.9 g |
|b. |3.6 g |d. |89.9 g |
____ 39. 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 |
____ 40. What is the mass of 0.240 mol glucose, C6H12O6?
|a. |24.0 g |c. |180.16 g |
|b. |43.2 g |d. |750. g |
____ 41. How many Cl– ions are present in 2.00 mol of KCl?
|a. |1.20 [pic] 1024 |c. |2.00 |
|b. |6.02 [pic] 1024 |d. |0.5 |
____ 42. How many OH– ions are present in 3.00 mol of Ca(OH)2?
|a. |3.00 |c. |3.61 [pic] 1024 |
|b. |6.00 |d. |2.06 [pic] 1023 |
____ 43. How many oxygen atoms are there in 0.500 mol of CO2?
|a. |6.02 [pic]€1023 |c. |15.9994 |
|b. |3.01 [pic] 1023 |d. |11.0 |
____ 44. How many Mg2+ ions are found in 1.00 mol of MgO?
|a. |3.01 [pic] 1023 |c. |12.04 [pic] 1023 |
|b. |6.02 [pic] 1023 |d. |6.02 [pic] 1025 |
____ 45. If 0.500 mol of Na+ combines with 0.500 mol of Cl– to form NaCl, how many formula units of NaCl are present?
|a. |3.01 [pic] 1023 |c. |6.02 [pic] 1024 |
|b. |6.02 [pic] 1023 |d. |1 |
____ 46. How many molecules are there in 5.0 g of methyl alcohol, CH3OH?
|a. |9.4 [pic] 1022 |c. |3.6 [pic] 1024 |
|b. |3.0 [pic] 1024 |d. |3.8 [pic] 1024 |
____ 47. What is the percentage composition of CuCl2?
|a. |33% Cu, 66% Cl |c. |65.50% Cu, 34.50% Cl |
|b. |50% Cu, 50% Cl |d. |47.27% Cu, 52.73% Cl |
____ 48. What is the mass percentage of OH– in Ca(OH)2?
|a. |45.9% |c. |75% |
|b. |66.6% |d. |90.1% |
____ 49. What is the mass percentage of chlorine in NaCl?
|a. |35.45% |c. |60.7% |
|b. |50% |d. |64.5% |
____ 50. What is the empirical formula for a compound that is 31.9% potassium, 28.9% chlorine, and 39.2% oxygen?
|a. |KClO2 |c. |K2Cl2O3 |
|b. |KClO3 |d. |K2Cl2O5 |
____ 51. What is the empirical formula for a compound that is 53.3% O and 46.7% Si?
|a. |SiO |c. |Si2O |
|b. |SiO2 |d. |Si2O3 |
____ 52. A compound contains 259.2 g of F and 40.8 g of C. What is the empirical formula for this compound?
|a. |CF4 |c. |CF |
|b. |C4F |d. |CF2 |
____ 53. A compound contains 64 g of O and 8 g of H. What is the empirical formula for this compound?
|a. |H2O |c. |HO2 |
|b. |H2O2 |d. |HO |
____ 54. A compound contains 27.3 g of C and 72.7 g of O. What is the empirical formula for this compound?
|a. |CO |c. |C2O |
|b. |CO2 |d. |C2O4 |
____ 55. The molecular formula for vitamin C is C6H8O6. What is the empirical formula?
|a. |CHO |c. |C3H4O3 |
|b. |CH2O |d. |C2H4O2 |
____ 56. Of the following molecular formulas for hydrocarbons, which is an empirical formula?
|a. |CH4 |c. |C3H6 |
|b. |C2H2 |d. |C4H10 |
____ 57. Which of the following molecular formulas does not have the corresponding empirical formula XY2Z?
|a. |X2Y4Z2 |c. |X6Y12Z6 |
|b. |XYZ |d. |X3Y6Z3 |
____ 58. A compound's empirical formula is C2H5. If the formula mass is 58 amu, what is the molecular formula?
|a. |C3H6 |c. |C5H8 |
|b. |C4H10 |d. |C5H15 |
____ 59. A compound's empirical formula is N2O5. If the formula mass is 108 amu, what is the molecular formula?
|a. |N2O5 |c. |NO3 |
|b. |N4O10 |d. |N2O4 |
____ 60. A compound's empirical formula is NO2. If the formula mass is 92 amu, what is the molecular formula?
|a. |NO |c. |NO4 |
|b. |N2O2 |d. |N2O4 |
____ 61. A compound's empirical formula is CH3. If the formula mass is 30 amu, what is the molecular formula?
|a. |CH3 |c. |C2H6 |
|b. |CH4 |d. |C3H9 |
____ 62. A compound's empirical formula is HO. If the formula mass is 34 amu, what is the molecular formula?
|a. |H2O |c. |HO3 |
|b. |H2O2 |d. |H2O3 |
____ 63. When the equation Fe3O4 + Al → Al2O3 + Fe is correctly balanced, what is the coefficient of Fe?
|a. |3 |c. |6 |
|b. |4 |d. |9 |
____ 64. Which coefficients correctly balance the formula equation
NH4NO2(s)→ N2(g) + H2O(l)?
|a. |1, 2, 2 |c. |2, 1, 1 |
|b. |1, 1, 2 |d. |2, 2, 2 |
____ 65. The complete balanced equation for the reaction between zinc hydroxide and acetic acid is
|a. |ZnOH + CH3COOH → ZnCH3COO + H2O. |
|b. |Zn(OH)2 + CH3COOH → Zn + 2CO2 +3H2O. |
|c. |Zn(OH)2 + 2CH3COOH → Zn(CH3COO)2 + 2H2O. |
|d. |Zn(OH)2 + 2CH3COOH → Zn(CH3COO)2 + H2 + O2. |
____ 66. What is the balanced equation for the combustion of sulfur?
|a. |S(s) + O2(g) → SO(g) |
|b. |S(s) + O2(g) → SO2(g) |
|c. |2S(s) + 3O2(g) → SO3(s) |
|d. |S(s) + 2O2(g) → SO42–(aq) |
____ 67. Which equation is not balanced?
|a. |2H2 + O2 → 2H2O |
|b. |4H2 + 2O2 → 4H2O |
|c. |H2 + H2 + O2 → H2O + H2O |
|d. |2H2 + O2 → H2O |
____ 68. The reaction of calcium oxide, CaO, with water yields
|a. |calcium and oxygen gas. |c. |calcium and a salt. |
|b. |calcium hydroxide. |d. |carbon dioxide and water. |
____ 69. Predict the product of the reaction represented by the following equation:
MgO + CO2 →
|a. |MgCO3 |c. |MgC + O3 |
|b. |Mg + CO3 |d. |MgCO2 + O |
____ 70. Magnesium hydroxide decomposes to yield magnesium oxide and
|a. |hydrogen. |c. |water. |
|b. |oxygen. |d. |salt. |
____ 71. When sodium chlorate, NaClO3, decomposes, the products are
|a. |sodium hydroxide and water. |c. |sodium and chlorine oxide. |
|b. |sodium oxide and chlorine. |d. |sodium chloride and oxygen. |
____ 72. If chlorine gas is produced by halogen replacement, the other halogen in the reaction must be
|a. |bromine. |c. |astatine. |
|b. |iodine. |d. |fluorine. |
____ 73. What is the balanced equation when aluminum reacts with copper(II) sulfate?
|a. |Al + Cu2S → Al2S + Cu |
|b. |2Al + 3CuSO4 → Al2(SO4)3 + 3Cu |
|c. |Al + CuSO4 → AlSO4 + Cu |
|d. |2Al + Cu2SO4 → Al2SO4 + 2Cu |
____ 74. Predict what happens when calcium metal is added to a solution of magnesium chloride.
|a. |No reaction occurs. |c. |Magnesium calcite forms. |
|b. |Calcium chloride forms. |d. |Gaseous calcium is produced. |
____ 75. Predict what happens when zinc is added to water.
|a. |No reaction occurs. |c. |Zinc oxide forms. |
|b. |Steam is produced. |d. |Hydrogen is released. |
____ 76. Predict what happens when lead is added to nitric acid.
|a. |No reaction occurs. |c. |Lead oxide forms. |
|b. |Oxygen is released. |d. |Hydrogen is released. |
____ 77. Predict what happens when nickel is added to a solution of potassium chloride.
|a. |No reaction occurs. |c. |Potassium nickel chloride forms. |
|b. |Nickel chloride forms. |d. |Hydrochloric acid forms. |
____ 78. Magnesium bromide (aq) + chlorine (g) yields
|a. |Mg(s) and BrCl(aq). |c. |MgBrCl(aq). |
|b. |MgCl(aq) and Br2(l). |d. |MgCl2(aq) and Br2(l). |
____ 79. Which reaction does not occur?
|a. |2HF(aq) + Cl2(g) → F2(g) + 2HCl(aq) |
|b. |2Na(s) + ZnF2(aq) → 2NaF(aq) + Zn(s) |
|c. |Fe(s) + CuCl2(aq) → FeCl2(aq) + Cu(s) |
|d. |2HCl(aq) + Mg(s) → MgCl2(aq) + H2(g) |
____ 80. Which reaction can be predicted from the activity series?
|a. |2Cl(g) → Cl2(g) |
|b. |HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) |
|c. |2H2O(aq) + 2Na(s) → 2NaOH(aq) + H2(g) |
|d. |Cl2(g) → 2Cl(g) |
____ 81. If 63.5 g of copper (Cu) combine with 16 g of oxygen (O) to form the compound CuO, how many grams of oxygen will be needed to combine with the same amount of copper to form the compound CuO2?
|a. |16 g |c. |64 g |
|b. |32 g |d. |127 g |
____ 82. Carbon-14 (atomic number 6), the radioactive nuclide used in dating fossils, has
|a. |6 neutrons. |c. |10 neutrons. |
|b. |8 neutrons. |d. |14 neutrons. |
____ 83. Phosphorus-33 (atomic number 15) contains
|a. |33 protons. |c. |33 neutrons. |
|b. |18 neutrons. |d. |18 protons. |
____ 84. The mass of a sample containing 3.5 mol of silicon atoms (atomic mass 28.0855 amu) is approximately
|a. |28 g. |c. |72 g. |
|b. |35 g. |d. |98 g. |
____ 85. A prospector finds 39.39 g of pure gold (atomic mass 196.9665 amu). She has
|a. |1.204 × 1023 atoms of Au. |c. |4.306 × 1023 atoms of Au. |
|b. |2.308 × 1023 atoms of Au. |d. |6.022 × 1023 atoms of Au. |
____ 86. A sample of tin (atomic mass 118.71 amu) contains 3.01 × 1023 atoms. The mass of the sample is
|a. |3.01 g. |c. |72.6 g. |
|b. |59.3 g. |d. |11 g. |
____ 87. According to Bohr, electrons cannot reside at ____ in the figure below. [pic] |a. |point A |c. |point C |
|b. |point B |d. |point D |
____ 88. A sample of gold has a mass of 96.5 g and a volume of 5.00 cm3. The density of gold is
|a. |0.0518 g/cm3. |c. |101.5 g/cm3. |
|b. |19.3 g/cm3. |d. |483 g/cm3. |
____ 89. When 5.7 m is divided by 2 s, the quotient is correctly reported as
|a. |2.8 m/s. |c. |2.9 m/s. |
|b. |2.85 m/s. |d. |3 m/s. |
____ 90. How would 0.00930 m be expressed in scientific notation?
|a. |93 × 10–4 m |c. |9.30 × 10–3 m |
|b. |9.3 × 10–4 m |d. |9.30 × 10–5 m |
____ 91. The speed of light is 300 000 km/s. In scientific notation, this speed is written to one significant figure as
|a. |3 × 105 km/s. |c. |3. × 106 km/s. |
|b. |3.0 × 105 km/s. |d. |3.0 × 106 km/s. |
____ 92. When 1.92 × 10–6 kg is divided by 6.8 × 102 mL, the quotient equals
|a. |2.8 × 10–4 kg/mL. |c. |2.8 × 10–8 kg/mL. |
|b. |2.8 × 10–5 kg/mL. |d. |2.8 × 10–9 kg/mL. |
____ 93. Which coefficients correctly balance the formula equation CaO + H2O → Ca(OH)2?
|a. |2, 1, 2 |c. |1, 2, 1 |
|b. |1, 2, 3 |d. |1, 1, 1 |
____ 94. The formulas for the products of the reaction between sodium hydroxide and sulfuric acid are
|a. |Na2SO4 and H2O. |c. |SI4 and Na2O. |
|b. |NaSO4 and H2O. |d. |S + O2 and Na. |
____ 95. Which word equation represents the reaction that produces water from hydrogen and oxygen?
|a. |Water is produced from hydrogen and oxygen. |
|b. |Hydrogen plus oxygen yields water. |
|c. |H2 + O2 → water. |
|d. |Water can be separated into hydrogen and oxygen. |
____ 96. The reaction represented by the equation Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq) is a
|a. |composition reaction. |c. |single-displacement reaction. |
|b. |decomposition reaction. |d. |double-displacement reaction. |
____ 97. The reaction represented by the equation Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) is a
|a. |double-displacement reaction. |c. |decomposition reaction. |
|b. |synthesis reaction. |d. |combustion reaction. |
____ 98. An active metal and a halogen react to form a(n)
|a. |salt. |c. |acid. |
|b. |hydroxide. |d. |oxide. |
____ 99. When a binary compound decomposes, what is produced?
|a. |an oxide |c. |a tertiary compound |
|b. |an acid |d. |two elements |
____ 100. Many metal hydroxides decompose when heated to yield metal oxides and
|a. |metal hydrides. |c. |carbon dioxide. |
|b. |water. |d. |an acid. |
____ 101. In the equation 2Al(s) + 3Fe(NO3)2(aq) → 3Fe(s) + 2Al(NO3)3(aq), iron has been replaced by
|a. |nitrate. |c. |aluminum. |
|b. |water. |d. |nitrogen. |
____ 102. If a certain metal is placed in an ionic solution containing another metal and no reaction occurs, then the metal originally in the solution is
|a. |a halogen. |c. |not on the activity series. |
|b. |higher on the activity series. |d. |unreactive. |
Short Answer- 10 points ( 5 points ea.) 103. How does the figure below illustrate Hund's rule? [pic] 104. How does the figure above illustrate the Pauli exclusion principle? Problem- Please complete all problem solving during homework assignments. On the exam only 5 will be selected. (10 points) 105. How many atoms are present in 80.0 mol of zirconium? 106. Determine the mass in grams of 10.0 mol of bromine. The molar mass of bromine is 79.90 g/mol. 107. Calculate the mass in grams of 9.00 mol of potassium (molar mass 39.10 g/mol). 108. Calculate the number of atoms in 10.0 g of sulfur (molar mass 32.07 g/mol). Use the periodic table below to answer the following questions. [pic] 109. Write the noble-gas electron configuration for silicon. 110. Which element has the following electron configuration: [Ar] 4s2 3d10 4p5? 111. Draw the orbital diagram for phosphorus. 112. Draw the orbital diagram for argon. 113. What is the half-life of an isotope if after 2.00 weeks you have 31.25 g remaining from a 250.0 g starting sample size? 114. Write the electron configuration for nitrogen, atomic number 7. 115. Write the noble-gas electron configuration represented in the orbital diagram below. [pic] 116. Draw a Lewis structure for the oxalate ion, C2O42–. 117. Draw a Lewis structure for the nitrate ion, [pic]. Use VSEPR theory to predict its molecular geometry. 118. Tell what type of chemical reaction is represented by the following formula equation. Then balance the equation.
KBr(aq) + Mg(OH)2(aq) [pic] KOH(aq) + MgBr2(aq) 119. Phosphorus-32 has a half-life of 14.3 days. How many milligrams of phosphorus-32 remain after 71.5 days if you start with 4.00 mg of the isotope? Essay-- Please choose ONE Essay. Submit a two- page summary, size 12 font and double-spaced. Bring the essay the DAY OF THE FINAL EXAM TO CLASS. READY TO BE SUBMITTED. (30 points) 120. Why are enzymes essential to life? Why are enzymes classified as catalysts? 121. Even though some animals are completely carnivorous, eating only other animals, their energy actually comes from the sun. Explain.
Honors Chemistry Final Exam Study Guide
Answer Section MULTIPLE CHOICE 1. ANS: D DIF: III REF: 1 OBJ: 5 2. ANS: B DIF: III REF: 1 OBJ: 5 3. ANS: C DIF: III REF: 1 OBJ: 5 4. ANS: A DIF: III REF: 1 OBJ: 5 5. ANS: C DIF: III REF: 2 OBJ: 5 6. ANS: D DIF: III REF: 2 OBJ: 5 7. ANS: C DIF: III REF: 3 OBJ: 4 8. ANS: B DIF: III REF: 3 OBJ: 4 9. ANS: B DIF: III REF: 5 OBJ: 2 10. ANS: B DIF: III REF: 5 OBJ: 2 11. ANS: A DIF: III REF: 5 OBJ: 2 12. ANS: C DIF: III REF: 5 OBJ: 2 13. ANS: B DIF: III REF: 5 OBJ: 2 14. ANS: C DIF: III REF: 5 OBJ: 5 15. ANS: B DIF: III REF: 1 OBJ: 2 16. ANS: D DIF: III REF: 1 OBJ: 2 17. ANS: A DIF: III REF: 1 OBJ: 2 18. ANS: C DIF: III REF: 1 OBJ: 2 19. ANS: C DIF: III REF: 1 OBJ: 2 20. ANS: A DIF: III REF: 1 OBJ: 3 21. ANS: C DIF: III REF: 1 OBJ: 3 22. ANS: A DIF: III REF: 1 OBJ: 3 23. ANS: D DIF: III REF: 1 OBJ: 3 24. ANS: B DIF: III REF: 2 OBJ: 2 25. ANS: D DIF: III REF: 2 OBJ: 2 26. ANS: D DIF: III REF: 2 OBJ: 2 27. ANS: B DIF: III REF: 2 OBJ: 2 28. ANS: C DIF: III REF: 2 OBJ: 3 29. ANS: B DIF: III REF: 2 OBJ: 3 30. ANS: A DIF: III REF: 2 OBJ: 3 31. ANS: C DIF: III REF: 2 OBJ: 3 32. ANS: C DIF: III REF: 2 OBJ: 3 33. ANS: C DIF: III REF: 3 OBJ: 1 34. ANS: D DIF: III REF: 3 OBJ: 1 35. ANS: D DIF: III REF: 3 OBJ: 1 36. ANS: C
Solution:
[pic] DIF: III REF: 3 OBJ: 2 37. ANS: C
Solution:
[pic] DIF: III REF: 3 OBJ: 2 38. ANS: B
Solution:
[pic] DIF: III REF: 3 OBJ: 2 39. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 2 40. ANS: B
Solution:
[pic] DIF: III REF: 3 OBJ: 2 41. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 3 42. ANS: C
Solution:
[pic] DIF: III REF: 3 OBJ: 3 43. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 3 44. ANS: B
Solution:
[pic] DIF: III REF: 3 OBJ: 3 45. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 3 46. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 3 47. ANS: D
Solution:
[pic] DIF: III REF: 3 OBJ: 4 48. ANS: A
Solution:
[pic] DIF: III REF: 3 OBJ: 4 49. ANS: C
Solution:
[pic] DIF: III REF: 3 OBJ: 4 50. ANS: B
Solution:
[pic] DIF: III REF: 4 OBJ: 2 51. ANS: B
Solution:
[pic] DIF: III REF: 4 OBJ: 2 52. ANS: A
Solution:
[pic] DIF: III REF: 4 OBJ: 2 53. ANS: A
Solution:
[pic] DIF: III REF: 4 OBJ: 2 54. ANS: B
Solution:
[pic] DIF: III REF: 4 OBJ: 2 55. ANS: C DIF: III REF: 4 OBJ: 3 56. ANS: A DIF: III REF: 4 OBJ: 3 57. ANS: B DIF: III REF: 4 OBJ: 4 58. ANS: B
Solution:
[pic] DIF: III REF: 4 OBJ: 4 59. ANS: A
Solution:
[pic] DIF: III REF: 4 OBJ: 4 60. ANS: D
Solution:
[pic] DIF: III REF: 4 OBJ: 4 61. ANS: C
Solution:
[pic] DIF: III REF: 4 OBJ: 4 62. ANS: B
Solution:
[pic] DIF: III REF: 4 OBJ: 4 63. ANS: D DIF: III REF: 1 OBJ: 4 64. ANS: B DIF: III REF: 1 OBJ: 4 65. ANS: C DIF: III REF: 1 OBJ: 4 66. ANS: B DIF: III REF: 1 OBJ: 4 67. ANS: D DIF: III REF: 1 OBJ: 4 68. ANS: B DIF: III REF: 2 OBJ: 5 69. ANS: A DIF: III REF: 2 OBJ: 5 70. ANS: C DIF: III REF: 2 OBJ: 5 71. ANS: D DIF: III REF: 2 OBJ: 5 72. ANS: D DIF: III REF: 2 OBJ: 5 73. ANS: B DIF: III REF: 2 OBJ: 5 74. ANS: B DIF: III REF: 3 OBJ: 2 75. ANS: A DIF: III REF: 3 OBJ: 2 76. ANS: D DIF: III REF: 3 OBJ: 2 77. ANS: A DIF: III REF: 3 OBJ: 2 78. ANS: D DIF: III REF: 3 OBJ: 2 79. ANS: A DIF: III REF: 3 OBJ: 2 80. ANS: C DIF: III REF: 3 OBJ: 2 81. ANS: B DIF: III REF: 1 OBJ: 1 82. ANS: B DIF: III REF: 3 OBJ: 3 83. ANS: B DIF: III REF: 3 OBJ: 3 84. ANS: D
Solution: [pic] DIF: III REF: 3 OBJ: 5 85. ANS: A
Solution: [pic] DIF: III REF: 3 OBJ: 5 86. ANS: B
Solution: [pic] DIF: III REF: 3 OBJ: 5 87. ANS: C DIF: III REF: 1 OBJ: 4 88. ANS: B
Solution: [pic] DIF: III REF: 2 OBJ: 4 89. ANS: D DIF: III REF: 3 OBJ: 3 90. ANS: C DIF: III REF: 3 OBJ: 4 91. ANS: A DIF: III REF: 3 OBJ: 4 92. ANS: D DIF: III REF: 3 OBJ: 4 93. ANS: D DIF: III REF: 1 OBJ: 4 94. ANS: A DIF: III REF: 2 OBJ: 5 95. ANS: B DIF: II REF: 1 OBJ: 3 96. ANS: C DIF: II REF: 2 OBJ: 2 97. ANS: A DIF: II REF: 2 OBJ: 2 98. ANS: A DIF: II REF: 2 OBJ: 3 99. ANS: D DIF: II REF: 2 OBJ: 3 100. ANS: B DIF: II REF: 2 OBJ: 3 101. ANS: C DIF: II REF: 2 OBJ: 4 102. ANS: B DIF: II REF: 3 OBJ: