Chemistry Exam 1 Key

Chem 101 - Exam 1 1. Which of the following properties of sulfur is a chemical property? a) It melts at 112 C. b) It boils att 444 C. c) It is a yellow solid. d) It combines with Cd to form a yellow solid. 2. Which of the following is NOT true? a) Temperature is an example of an intensive property. b) The mass percentage of calcium in calcium phosphate is an extensive property. c) Separations of a solid from a liquid by filtration is an example of a physical process. d) Density is an intensive property. 3. A car uses oil at a rate of 1.5 quarts per 4250 miles. What is the rate of oil usage in milliliters/ kilometer? (1 Liter = 1.06 qt., 1 mile = 5280 ft., 1 ft = 12 in.) a) 1.35 mL/km b) 0.21 mL/km c) 890 mL/km d) 0.14 mL/km 4. Which of the following is NOT paired with the proper classification? a) iron/element b) chromium (III) oxide/compound c) pizza/heterogenous mixture d) a solution of aqueous sulfuric acid/heterogenous mixture 5. A graduated cylinder is filled to the 12.0 mL line with water. A solid with a mass of 4.52g is placed in the graduated cylinder and is completely immersed in the water. The level of the water is now 14.5 mL. What is the density of the solid? a) 1.81 g/mL b) 0.377 g/mL c) 0.311 g/mL d) 4.52 g/mL 6. Which of the following element/symbol combinations is NOT correct? a) lead/Pb b) sodium/Na c) carbon/C d) potassium/Po 7. The number of moles of potassium permanganate, KMnO4, in 95 g of that compound is: a) 1.7 b) 0.60 c) 1.5 x 104 d) 0.48 e) 0.075 8. Which of the following ionic formulas is INCORRECT? a) K2O b) Fe2(SO4)3 c) CuPO4 d) (NH4)2S e) CaBr2 9. The formula weight of chromic acetate, Cr(C2H3O2)3 is: a) 215 b) 222 c) 170 d) 229 e) 114 10. Potassium tartrate is composed of 34.6% potassium, 21.2% carbon, 1.78% hydrogen and 42.4% oxygen. What is the oxygen subscript in the empirical (simplest) formula? a) 1 b) 2 c) 3 d) 4 e) 5 11. The atomic mass unit (amu) is defined as: a) the mass of a proton. b) 1/16 the mass of the most common atom of oxygen. c) the atomic weight expressed in grams. d) the mass of the most common atom of hydrogen. e) 1/12 the mass of the most common atom of carbon. 12. Which of the following name/formula pairs is INCORRECT? a) calcium carbonate, Ca(CH3COO)2 b) magnesium hydroxide, Mg(OH)2 c) ammonium nitrate, NH4NO3 d) aluminum chloride, AlCl3 e) zinc sulfate, ZnSO4 13. The percent nitrogen in ammonium oxalate, (NH4)2C2O4 is: a) 13.2 b) 22.6 c) 29.0 d) 19.4 e) 11.3 14. Which of the following is closest to having exactly one mole of oxygen atoms? a) 42 g HNO3 b) 32 amu O2 c) 7.3 x 10-23g CO2 d) 1.5 x 1023 molecules of H2SO4 e) 1 mole Ba(OH) 2 15. What volume of 0.300 M HCl is required to completely neutralize 50.0 mL of 0.800 M Ca(OH) 2? 2 HCl + Ca(OH) 2 ---> CaCl2 + 2 H2O a) 133 mL b) 18.7 mL c) 1470 mL d) 267 mL 16. In the following balanced reaction 3.00 grams each of NO and Br2 are reacted together. How many grams of product can be produced? 2NO + Br2 ---> 2 NOBr a) 6.00 g b) 9.00 g c) 4.12 g d) 18.9 g 17. Balance the following equation using the set of smallest whole-number coefficients. What is the sumof these coefficients? (be sure to include coefficients of "1" in the sum ). ____PbO + ___NH3 ---> ___Pb + ___N2 + ___H2O a) 9 b) 15 c) 14 d) 12 18. If 10.0g of methanol CH3OH are dissolved in enough water to make 30.0 mL of aqueous solution, what is the concentration of methanol in molarity units? a) 10.4 M b) 0.312 M c) 0.333 M d) 1.04 x 10-2 M 19. Ethylene glycol C2H6O2 (MW = molar mass = 62.07) is produced from the following (balanced) reaction. If 49.47 grams of C2H4Cl2 (MW = molar mass = 98.95 g/mol) are reacted with excess Na2CO3 and H2O, 26.10 grams of C2H6O2 are collected, what is the percent yield? C2H4Cl2 + Na2CO3 + H2O ---> C2H6O2 + 2 NaCl + CO2 a) 84.11% b) 52.76% c) 33.09% d) 96.01% 20. Lime, CaO, dissolves in "muriatic acid", HCl, to form CaCl2 and water. How many grams of HCl are required to dissolve 28.0g of CaO? The reaction is: CaO + 2HCl ---> CaCl2 + H2O a) 36.5 g (typo fixed on 10/10/99) b) 18.2 g c) 43.0 g d) 56.0 g 21. Concentrated aqueous hydrofluoric acid solution is 49.0% HF by mass and has a specific gravity of 1.17. How many grams of HF are present in a 100.0 mL sample of the solution? a) 49.0 g b) 57.3 g c) 41.9 g d) 47.0 g 22. Which elements is NOT correctly classified? a) H, non-metal b) Ge, metalloid c) S, metalloid d) Li, metal e) In, metal 23. Which response include all the following that are properties of most metals, and no other properties? I. They tend to form cations. II. They are good heat insulators. III. Some are gases at room temperatures. IV. They tend to form ionic compounds when they combine with the elements of Group VIIA. a) I, II, and III b) II, III, and IV c) III and IV d) I and IV e) I and III 24. Which response contains all of the following that are oxidation-reduction reactions and no others? I. PCl3 + 3H2O ---> 3 HCl(aq) + H3PO3(aq) II. Fe2O3(s) + 3 CO(g) ---> 2 Fe(s) + 3CO2(g) III. CaCO3(s) + 2 HClO3 Ca(ClO3)2(aq) + CO2(g) + H2O a) I b) II c) III d) II and III e) I and II 25. Which one of the following salts is INSOLUBLE in water? a) MgSO4 b) KNO3 c) AgCl d) FeCl3 e) NaBr 26. Which one of the following compounds is NOT a salt? a) LiI b) Al(ClO4)3 c) HI d) Fe(ClO3)3 e) NH4Br 27. Which one of the following is a WEAK acid? a) HClO4 b) HCl c) HBr d) HI e) HCN 28. Which is the oxidation number of the element chromium in K2CrO4. a) +1 b) +2 c) +3 d) +4 e) +6 29. Will a precipitate form when aqueous solutions of CaCl2 and K2CO3 are mixed? If a precipitate does form, identify the precipitate and give the NET ionic equation for the reaction. a) KCl precipitates. K+(aq) + Cl-(aq) ---> KCl(s) b) CaC2 precipitates. Ca2+(aq) + 2 CO32-(aq) -- -> CaC2(s) + 3 O2(g) c) CaCO3 precipitates. Ca2+(aq) + CO32-(aq) -- -> CaCO3(s) d) CaCO3 precipitates. Ca2+(aq) + K2CO3(aq) - --> CaCO3(s) + 2 K+(aq) e) No precipitate forms. 30. Which one of the following represents the NET ionic equation for the reaction of nitric acid with aluminum hydroxide? a) 3 H+(aq) + Al (OH) 3(s) ---> Al3+(aq) + 3 H2O( ) b) 3 HNO3(aq) + Al (OH)3(s) ---> 2 Al(NO3)3(aq) + 3 H2O( ) c) 2 H+(aq) + Al (OH)2(s) ---> Al2+(aq) + 2 H2O( ) d) H+(aq) + OH-(aq) ---> H2O( ) e) 3 NO3-(aq) + Al3+(aq) ---> Al(NO3)3(aq) KEY 1)d 2)b 3)b 4)d 5)a 6)d 7)b 8)c 9)d 10)c 11)e 12)a 13)b 14)d 15)d 16)c 17)d 18)a 19)a 20)a 21)b 22)c 23)d 24)b 25)c 26)c 27)e 28)e 29)c 30)a 1. Which element is INCORRECTLY matched with its symbol? a) Silver = Ag b) Sulfur = S c) Silicon = Si d) Cadmium = Ca e) Copper = Cu 2. Which of the following properties of a sample are INCORRECTLY matched? a) volume = extensive property b) density = extensive property c) temperature = intensive property d) chemical reactivity = intensive property e) mass = extensive property 3. Which of the following statements is INCORRECT? a) Physical properties can be used to identify a pure substance. b) A chemical change produces products containing different elements from the reactants. c) A physical change results when a pure substance goes from one physical state to another. d) Chemical properties are exhibited when a pure substance undergoes a chemical change. 4. Which of the following properties of a sample are INCORRECTLY matched? a) boiling point = physical property b) malleability = physical property c) highly reactive with oxygen = chemical property d) temperature = chemical property e) mass = physical property 5. "There is no observable change in the total mass during a chemical reaction or a physical change." This is a statement of: a) The Law of Definite Proportions b) The Law of Chemical Reactivity c) The Law of Conservation of Matter d) The Law of Conservation of Mass and Energy 6. The recent Mars probe crashed on the back side of Mars and wasted millions of dollars of taxpayer money because NASA engineers (who got their degree at MTSU) confused English and metric units for mass. The titanium alloy that formed the hull of the doomed space craft has a density of 4.5 g/cm3. What is the density in pounds per cubic inch? Given 1 pound = 453.6 g and 1 inch = 2.54 cm. a) 5.2 x 103 lb/in3 b) 0.025 lb/in3 c) 3.3 x 104 lb/in3 d) 0.16 lb/in3 e) 0.89 lb/in3 7. Which compound/formula name combination is INCORRECT? a) FeSO4 is iron(II) sulfate b) BaCO3 is barium carbonate c) NaS is sodium sulfide d) Al(OH)3 is aluminum hydroxide e) CaF2 is calcium fluoride 8. Identify the INCORRECT statement below: a) Equal masses of different elements contain equal numbers of atoms. b) Avogadro's number is the number of atoms in exactly 12 grams of Carbon- 12. c) The electron and the proton have charges equal in magnitude and opposite in sign. d) The atomic number is the number of protons in the nucleus. e) The number above the element symbol on the periodic chart is the atomic number. 9. Determine the simplest empirical formula of a compound which has the composition by mass: 26.9% S, 13.4% O, 59.6% Cl. a) ClS02 b) SOCl c) S2O2Cl3 d) SO4Cl e) SOCl2 10. Which compound below is a molecular compound (or molecular substance)? a) NH3 b) CaCl2 c) KBr d) AgNO3 11. Calculate the mass in grams of a single oxygen molecule, O2. a) 32.0 g b) 16.0 g c) 5.3 x 10-23g d) 2.6 x 10-23g e) 1.66 x 10-24g 12. How many moles of NO3 are present in 16.4 grams of Ca(NO3)2? a) 0.20 mol b) 2.0 mol c) 0.10 mol d) 32.8 mol 13. What is the mass of 0.50 moles of SF6? a) 146 g b) 73 g c) 0.50 g d) 103 g e) 175 g 14. Calculate the molecular weight (molar mass) of the antiseptic phenol, which has the formula C6H5OH. a) 94.1 g/mol b) 93.1 g/mol c) 78.1 g/mol d) 172 g/mol e) 108 g/mol 15. Calculate the percent carbon by mass in phenol. (See above problem for formula). a) 76.6% b) 12.7% c) 7.6 x 10-1% d) 66.7% e) 83.5% 16. Dalton's Atomic Theory consisted of all of the following ideas EXCEPT: a) a given element consists of different kinds of atoms. b) elements are composed of indivisible particles called atoms. c) atoms of different elements have different properties. d) atoms combine in fixed, whole-number ratios. e) in chemical reactions, atoms are not destroyed or created. 17. The rusting process is described by the reaction 4Fe(s) + 3O2(g) ----> 2Fe2O3(s). The maximum amount of Fe2O3 that can be produced from 56.0 g of Fe and 32.0 g of O2 is: a) 160. g b) 80.0 g c) 40.0 g d) 120. g e) 110. g 18. A solution is 5.00% acetic acid by mass, and has a specific gravity of 1.11. What mass of glucose is present in 50.0 mL of this solution? a) 5.55 g b) 2.78 g c) 11.10 g d) 6.12 g 19. How many grams of NaCl are contained in 350. mL of a 0.250 M solution of NaCl? a) 41.7 g b) 5.11 g c) 14.6 g d) 87.5 g e) none of these 20. What volume of 18.0 M H2SO4 is required to prepare 12.0 L of 0.156 M H2SO4? a) 1.87 mL b) 52.0 mL c) 208 mL d) 104 mL e) 1.04 L 21. A 20.0 g sample of HF is dissolved in enough water to give 2.0 x 102 mL of solution. The concentration of the solution is: a) 1.0 M b) 3.0 M c) 0.10 M d) 5.0 M e) 10.0 M 22. Calculate the concentration of a NaOH solution of which 23.09 mL reacts exactly with 16.95 mL of 0.156 M HCl by the reaction: NaOH + HCI ---> NaCI + H2O. a) 0.228 M b) 0.0573 M c) 0.115 M d) 0.212 M 23. How many grams of Ca(NO3)2 can be produced by reacting excess HNO3 with 7.40 grams of Ca(OH)2. The reaction is Ca(OH)2 + 2HNO3 ---> Ca(NO3)2 + 2H2O a) 10.2 g b) 16.4 g c) 32.8 g d) 8.22 g e) 7.40 24. Consider the fermentation reaction of glucose: C6H12O6 ---> 2C2H5OH + 2CO2 . If a 1.00 mole sample of C6H12O6 was fermented, and 46.0 g of C2H5OH was obtained, what was the percent yield? a) 50.0% b) 56.0% c) 100.% d) 42.0% e) none of these 25. What is the name for the family (or group) which includes F, Cl, Br, I, and At? a) The non-metals b) the halogens c) the alkalis d) the alkaline earths e) the rare earths 26. Which of the following is NOT a property or characteristic of the metals in the periodic chart? a} electrically conductive b) lose electrons to form cations c) form molecular compounds with nonmetals d) are malleable and ductile e) thermally conductive 27. Which of the following is an example of a metalloid? a) Na b) F c) C d) B e) Ca 28. Which of the following would NOT be classified as a strong electrolyte? a) NH4Cl b) Na2SO4 c) acetic acid, HC2H3O2 d) HNO3 e) HBr 29. In which of the following lists are NOT ALL of the elements listed in the same family (or group)? a) He, Ar, Kr b) Ni, Pd, Pt c) Na, K, Rb d) B, C, N e) O, S, Po 30. Which of the following is NOT a characteristic of a strong electrolyte? a) Strong electrolytes are always molecular compounds. b) Solutions of strong electrolytes conduct an electrical current. c) Strong electrolytes dissociate (or ionize) completely in aqueous solution. d) A strong electrolyte may be a strong acid, a strong, soluble base, or a soluble salt. KEY 1)d 2)b 3)b 4)d 5)c 6)d 7)c 8)a 9)e 10)a 11)c 12)a 13)b 14)a 15)a 16)a 17)b 18)b 19)b 20)d 21)d 22)c 23)b 24)a 25)b 26)c 27)d 28)c 29)d 30)a 1. Which of the following statements is INCORRECT? a) A body in motion possesses kinetic energy because of its motion. b) An object possesses potential energy because of its position or composition. c) Nuclear energy is an important kind of potential energy. d) Chemical reactions and physical changes that release energy to their surroundings are endothermic. e) The Law of Conservation of Matter and Energy states that the combined amount of matter and energy in the universe is fixed. 2. All of the following are properties of antimony. Which one is NOT a physical property? a) It is a solid at room temperature. b) It has both yellow and gray forms (allotropes) in the solid state. c) It burns in an atmosphere of chlorine. d) It is one of the few substances that expands upon freezing. e) The gray form melts at 631°C. 3. Which statement is FALSE? a) A compound is a substance that can be decomposed by chemical means into simpler substances. b) All samples of a particular pure substance have the same composition and properties. c) An example of a homogeneous mixture is one prepared by mixing two liquids, ethyl alcohol (grain alcohol) and water. d) An example of a heterogeneous mixture is one prepared by dissolving the solid, sodium chloride (table salt), in the liquid, water. e) Different mixtures of the same two substances can have different compositions. 4. Which of the following are heterogeneous mixtures? I. sugar II. sugar dissolved in water III. an aqueous suspension of magnesium hydroxide (milk of magnesia) IV. samples of nitrogen and oxygen in the same container V. samples of argon and iron in the same container a) III only b) I, II, and IV c) III and V d) III and IV e) II, IV, and V 5. Which element symbol - name combination is INCORRECT? a) Mn manganese b) Zn zinc c) Sn tin d) Sr strontium e) Co - copper 6. Assuming a magnesium atom is spherical, calculate its volume in nm3. The radius of a magnesium atom is 1.60 Å . The volume of a sphere is V = (4/3) r3. 1 Å = 1 x 10-10 m and 1 nm = 1 x 10-9 m (Both of these relationships are exact.)  = 3.14 a) 5.57 x 103 nm3 b) 2.34 x 10-22 nm3 c) 5.57 x 10-24 nm3 d) 1.71 x 10-2 nm3 e) 5.57 x 10-3 nm3 7. The 1970 standard established by the U.S. government for carbon monoxide emission for automobiles limited exhaust to 23.0 grams of CO per vehicle-mile. Assume that in a given metropolitan area there are 82,700 automobiles, driven an average of 13.5 miles per 24-hour period. How many tons/day of CO could legally be discharged into the area's atmosphere? a) 270 tons/day b) 0.155 tons/day c) 28.3 tons/day d) 0.0535 tons/day e) 39.0 tons/day 8. Caffeine, a stimulant in coffee and some cola drinks, is 49.47% carbon, 5.19% H, 28.8% N, 16.48% O. What is the mass of carbon contained in 37.1 g of caffeine? a)18.4 g b) 36.8 g c) 6.11 g d) 1840 g e) 24.3 g 9. The specific gravity of ethyl chloride, an external painkiller, is 1.37 at 10°C. What is the mass of 47.4 mL of the liquid? a) 64.9 g b) 0.346 g c) 34.6 g d) 52.5 g e) 56.6 g 10. All atoms of the same element have the same number of __________ . a) neutrons b) protons c) protons and neutrons d) electrons and neutrons e) protons, neutrons, and electrons 11. All of the following groups are considered main group elements EXCEPT: a) group 2 b) group 7 c) group 14 d) group 17 e) group 18 12. How many elements are contained in period 4? a) 3 b) 8 c) 10 d) 18 e) 32 13. Which statement is FALSE? a) The charge on a proton is positive, the charge on a neutron is negative. b) Molecules are the smallest unit of a compound. c) The nucleus of an atom is very small and massive. d) Electrons are smaller particles than protons. e) Compounds consist of more than one type of element. 14. What is the correct classification for SCN-? a) polyatomic molecule b) monatomic cation c) polyatomic cation d) polyatomic anion e) monatomic anion 15. From the following compounds choose the name-formula pair that is INCORRECTLY matched. a) sodium sulfite; Na2SO3 b) ammonium fluoride; NH4F c) copper(II) carbonate; CuCO3 d) iron(III) chloride; FeCl2 e) copper(I) sulfide; CuS 16. Which element has a mass approximately 32 times that of a H atom? a) C b) S c) Mo d) Cu e) Ar 17. A sample of ethane, C2H6, contains a total of 16N atoms, where N = 6.02 x 1023. How much C2H6 is in the sample? a) 2.0 g b) 30 g c) 60 g d) 16 mol e) 4 mol 18. What mass of FeCl3 would contain the same TOTAL number of ions as 16.8 g of Al2(SO4)3? a) 7.96 g b) 9.95 g c) 10.8 g d) 13.3 g e) 8.01 g 19. What is the empirical formula for a compound containing 68.3% lead, 10.6% sulfur and the remainder oxygen? a) PbSO2 b) PbSO3 c) PbS2O3 d) PbSO4 e) Pb2SO4 20. Give (in order) the correct coefficients to balance the following reaction: Na2CO3 + HCl ---> CO2 + NaCl + H2O a) 3,6,6,3,4 b) 8,6,5,10,5 c) 5,10,10,5,5 d) 1,2,1,2,1 21. Under heat and pressure, methane reacts with water according to the following equation: CH4 + H2O ---> CO + 3 H2 How much methane is needed to react with 36 grams of water? a) 32 grams b) 16 grams c) 8.0 grams d) 4.0 grams 22. A 15.00 g sample of lithium is reacted with 15.00 g of fluorine to form lithium fluoride: 2 Li + F2 ---> 2 LiF After the reaction is complete, what will be present? a) 2.16 mol lithium fluoride only. b) 0.789 moles lithium fluoride only. c) 2.16 mol lithium fluoride and 0.395 mol fluorine. d) 0.789 mol lithium fluoride and 1.37 mol lithium. e) a really, really big mess! 23. Ammonia (NH3) is produced using the following equation: N2 + 3 H2 ---> 2 NH3 When 6.00 grams of H2 and 28.0 grams of N2 were reacted, 30.0 grams of ammonia were produced. What was the percent yield? a) 113% b) 88.2% c) 70.6% d) 67.8% 24. How many grams of NaCl are contained in 350. mL of a 0.250 M solution of sodium chloride? a) 41.7 g b) 5.11 g c) 14.6 g d) 87.5 g 25. What volume of 12.0 M nitric acid is required to prepare 6.00 L of 0.100 M nitric acid? a) 1.20 L b) 1.00 L c) 0.500 L d) 0.0500 L e) 0.0200 L 26. What volume of 0.130 M HCl solution will exactly react with 0.424 g of Ba(OH)2? The equation is: 2 HCl + Ba(OH)2 ---> BaCl2 + 2 H2O a) 38.1 mL b) 32.6 mL c) 24.1 mL d) 18.6 mL 27. Which of the following answers is CORRECT? a) Cl, metal b) Na, non-metal c) Si, metalloid d) Bi, metalloid 28. Which of the following answers is INCORRECT? a) NH4Cl, strong electrolyte b) CH3OH, non-electrolyte c) CH3COOH, weak electrolyte d) C6H12O6, weak electrolyte 29. Which of the following is a weak acid? a) H2SO4 b) HNO3 c) CH3COOH d) HClO4 30. Which of the following is NOT a base? a) NaOH b) KOH c) NH3 d) CH3NH2 e) HClO KEY 1)d 2)c 3)d 4)c 5)e 6)d 7)c 8)a 9)a 10)b 11)b 12)d 13)a 14)d 15)d 16)b 17)c 18)b 19)d 20)d 21)a 22)d 23)b 24)b 25)d 26)a 27)c 28)d 29)c 30)e h = 6.63 x 10-34 J-s c = 3.0 x 108 m/s R = 1.097 x 107m-1 1. An atom has a mass number of 131 and its nucleus contains 78 neutrons. The element is: a) platinum b) iodine c) gallium d) gold e) palladium 2. Which of the following methods will NOT result in the production of O2? a) Fe(s) + H2O(g) ---------> (heat) b) HgO(s) ---------> c) H2O(l) (electric current) ---------> (heat) d) KClO3 ---------> 3. Which of the following is a peroxide? a) NaO2 b) Na2O2 c) Na2O d) Na3O 4. Which of the following statements concerning hydrogen is FALSE? a) H2 is formed when hot iron reacts with water. b) Many molecular hydrides are acids. c) Ionic hydrides, such as LiH, react with water to form H2 and LiOH. d) Hydrogen reacts with halogens to form compounds of the formula H2X, where X is a halogen. 5. What is the formula for the binary ionic compound of aluminum and sulfur? a) AlS b) Al2S c) AlS2 d) Al3S2 e) Al2S3 6. Which of the following is the NET IONIC equation for the reaction between AgNO3(aq) and Na3PO4(aq)? a) Ag3+(aq) + PO43-(aq) ---> AgPO4(s) b) Ag+(aq) + NO3-(aq) + Na+(aq) + PO43-(aq) ---> AgPO4(s) + Na+(aq) + NO3-(aq) c) 3Ag+(aq) + 3NO3-(aq) + 3Na+(aq) + PO43-(aq) ---> Ag3PO4(s) + 3Na+(aq) + 3NO3-(aq) d) 3Ag+(aq) + PO43-(aq) ---> Ag3PO4(s) e) There is no reaction between AgNO3(aq) and Na3PO4(aq) 7. Which of the following will NOT, with typical concentrations, produce a precipitate when mixed? a) Na2S + MnCl2 b) BaCl2 + H2SO4 c) Na3PO4+ Ca(NO3)2 d) NaOH + FeCl3 e) all of these will produce a precipitate 8. Which of the following is NOT true? a) The reaction by which H+(aq) reacts with OH-(aq) to form H2O is call neutralization. b) NaBr(aq) can be formed by the reaction of NaOH(aq) with HBr(aq). c) Strong acids are acids which have a high concentration in water. d) The net ionic reaction for all strong acids with strong, soluble bases that form soluble salts is H+(aq) + OH-(aq) ---> H2O. e) The total formula unit reaction for HCl(aq) with Fe(OH)2 is 2HCl(aq) + Fe(OH)2(s) ---->2H2O + FeCl2(aq). 9. In which of the following is the oxidation number of nitrogen +3? a) NO2 b) HNO2 c) HNO3 d) N2O4 e) N2O5 10. In which of the following equations is iron being REDUCED? a) 2Fe2O3(s) + 3H2 ---> 4Fe(s) +3 H2O b) FeCl3(aq) + 3NaOH(aq) ---> Fe(OH)3 (s)+ 3H2O c) 2Fe(s) + 6HCl(aq) ---> 2FeCl3(aq)+ 3H2(g) d) 4Fe(s) + 3O2 ---> 2Fe2O3 e) Iron is not being reduced in any of these. 11. Ba is more active than Fe, and Fe is more active than Pd. Which of the following reactions WILL NOT occur? a) Fe(s) + PdSO4 (aq) ---> FeSO4(aq) + Pd b) Ba(NO3)2(aq) + Fe(s) ---> Fe(NO3)2(aq) + Ba c) Ba(s) + PdCl2(aq) ---> Pd(s) + BaCl2(aq) d) all of these will occur 12. From the following list of observations chose the one that most clearly supports the following conclusion: atoms contain electrons. a) Emission spectrum of hydrogen b) The photoelectric effect c) Diffraction d) Scattering of alpha particles by metal foil e) Cathode "rays" 13. How many grams of NaOH are needed to prepare 30.0 mL of a solution with a molarity of 2.20 M? a) 6.60 g b) 2.64 x 103 g c) 3.96 g d) 2.64 g e) 0.0660 g 14. If 20.0 grams of KBr are dissolved in enough solvent to make 1.90 Liters of solution, what is the concentration of this solution in molarity units? a) 0.412 M b) 10.5 M c) 1.25 x 10 3 M d) 0.0885 M e) 1.09 M 15. How many moles of Na+ are present in 10.00 mL of a 1.80 M solution of NaOH? a) 18.0 moles b) 5.56 moles c) 0.0180 moles d) 0.0360 moles e) 0.360 moles 16. If 20.0 mL of a 2.50 M solution of KBr is diluted to a final volume of 200. mL, what is the new concentration? a) 25.0 M b) 0.188 M c) 0.250 M d) 0.125 M e) 0.0400 M 17. For the reaction 2Mg + O2 -> 2MgO how many grams of O2 are required to completely consume 94.5 grams of Mg ? a) 143. g b) 62.2 g c) 71.7 g d) 47.2 g e) 35.9 g 18. For the neutralization reaction of HF with KOH, 12.14 mL of the acid are required to titrate to the endpoint against 30.00 mL of 1.70 M base. What is the concentration of the acid? a) 4.20 M b) 2.20 M c) 1.70 M d) 0.510 M e) 0.0510 M 19. For the reaction CH4 + 2O2 -> CO2 + 2H2O, 4.00 grams of CO2 are collected when 1.50 grams of CH4 react with an excess of amount of O2 . What is the percent yield? a) 37.6 % b) 72.8 % c) 26.6 % d) 97.2 % e) 11.6 % 20. Suppose 10.0 grams of sodium metal and 10.0 grams of oxygen gas are reacted in a closed vessel and the reaction proceeds to completion to produce Na2O with no other products. Which reactant is the limiting reagent, and how much of the reagent in excess will be left over? a) sodium is limiting reagent, and 3.48 g of O2 will be left over. b) oxygen is limiting reagent, and 9.37 g of Na will be left over. c) sodium is limiting reagent, and 6.52 g of O2 will be left over. d) oxygen is limiting reagent, and 0.631 g of Na will be left over. e) neither is limiting; both will be completely used up. 21. For the neutralization reaction of H2SO4 with Al(OH)3 how many mL of 3.40 x 10-3 M acid are required to titrate to the endpoint against 50.0 mL of 3.50 x 10-3 M base? a) 25.7 mL b) 77.2 mL c) 34.3 mL d) 92.6 mL e) 154. mL 22. Determine the oxidation number of the underlined element in H2CrO4. a) +1 b) +2 c) +3 d) +4 e) +6 23. Which of the following matched pairs of name and formula has an error? a) FeF3; ferric fluoride b) SnO; stannous oxide c) FeI2; ferrous iodide d) Cu2S; copper(II) sulfide e) CuO; cupric oxide 24. Which of the following matched pairs of name and formula has an error? a) NaClO3; sodium chlorate b) LiClO2; lithium chlorite c) KbrO; potassium hypobromite d) MgClO4; magnesium perchlorate e) NaIO3; sodium iodate 25. Which of the following matched pairs of name and formula has an error? a) H2SO3; sulfurous acid b) HClO3; chloric acid c) H2CO3; carbonic acid d) HBrO4; perbromic acid e) HIO2; hypoiodous acid 26. What are the oxidizing agent and reducing agent in the following reaction? 8 H+(aq) + 3 C2H5OH(aq) + Cr2O72-(aq) ---> 2 Cr3+(aq) + 3 C2H4O(aq) + 7 H2O(l) a) H+ is oxidizing agent and C2H5OH is reducing agent b) Cr2O72- is oxidizing agent and C2H5OH is reducing agent c) Cr3+ is oxidizing agent and Cr2O72- is reducing agent d) C2H5OH is oxidizing agent and Cr2O72- is reducing agent e) H2O is oxidizing agent and H+ is reducing agent 27. Which of the following is BOTH a decomposition reaction AND a reduction-oxidation reaction? a) H2CO3(aq) ---> CO2(g) + H2O(l) b) Zn(s) + CuNO3(aq) ---> Cu(s) + ZnNO3(aq) c) Ca(OH)2(aq) + 2 HCl(aq) ---> CaCl2(aq) + 2 H2O(l) d) 2 NH4NO3(s) ---> 2 N2(g) + O2(g) + 4 H2O(g) e) CaCO3(s) ---> CaO(s) + CO2(g) 28. Which response includes all of the following that are displacement reactions, and no other reactions? I. Li2O(s) + CO2(g) ---> Li2CO3(s) II. Cl2(g) + 2 NaBr(aq) ---> Br2(l) + 2 NaCl(aq) III. HNO3(aq) + KOH(aq) ---> KNO3(aq) + H2O(l) IV. SO3(l) + H2O(l) ---> H2SO4(l) a) I and II b) I and IV c) I, III, and IV d) I, II, and IV e) II 29. Which one of the following elements reacts with water at room temperature to produce hydrogen? a) Ti b) Zn c) Na d) Mg e) Al 30. Which of the following reactions is NOT spontaneous? a) 2 KCl(aq) + F2 (g) ---> 2 KF(aq) + Cl2(g) b) 2 KCl(aq) + I2(s) ---> 2 KI(aq) + Cl2(g) c) 2 Na(s) + 2 H2O(l) ---> 2 NaOH(aq) + H2(g) d) 2 K(s) + ZnSO4(aq) ---> K2SO4(aq) + Zn(s) e) 2 NaI(aq) + Br2(l) ---> 2 NaBr(aq) + I2(s) 31. Write the net ionic equation for the complete reaction of carbonic acid with potassium hydroxide. What is the total charge on the ions on the right side of the equation? a) 1+ b) 2+ c) 3+ d) 2e) 132. Rutherford was very surprised at the results of his gold foil experiment, because the results were not as what he had predicted. If the atom was really put together according to the Thompson ³plum pudding² model, with the electrons and protons all jumbled together, what SHOULD have been the result of his experiment? a) all the alpha particles should have bounced back towards the source b) all of the alpha particles should have passed through the foil with no deflection c) the alpha particles should have been absorbed by the foil d) all the alpha particles should have been deflected by very small angles 33. Which of the following anions represents a peroxide? a) Ob) O2c) O2d) O22e) O334. Write the balanced formula unit equation for the reaction of lithium oxide with water. What is the sum of the coefficients? a) 2 b) 6 c) 3 d) 4 e) 5 KEY 1)b 2)a 3)b 4)d 5)e 6)d 7)e 8)c 9)b 10)a 11)b 12)e 13)d 14)d 15)c 16)c 17)b 18)a 19)d 20)c 21)b 22)e 23)d 24)d 25)e 26)b 27)d 28)e 29)c 30)b 31)d 32)d 33)d 34)d