Chem 1411 (Test 1) Review

Transcription

1 Name: Class: Date: Chem 1411 (Test 1) Review 1. Which of the following metric relationships is incorrect? A) 1 microliter = 10 6 liters B) 1 gram = 10 3 kilograms C) 10 3 milliliters = 1 liter D) 1 gram = 10 2 centigrams E) 10 decimeters = 1 meter 2. For which pair is the SI prefix not matched correctly with its meaning? A) mega 10 6 B) kilo 1000 C) deci 10 D) nano 10 9 E) centi As part of the calibration of a new laboratory balance, a g mass is weighed with the following results: Trial Mass The balance is: A) Both accurate and precise. B) Accurate but imprecise. C) Precise but inaccurate. D) Both inaccurate and imprecise. E) Accuracy and precision are impossible to determine with the available information. 4. In March 2008, gold reached a milestone value of $1000 per troy ounce. At that price, what was the cost of a gram of gold? (1 troy ounce = g) A) less than $1 B) between $1 and $10 C) between $10 and $50 D) between $50 and $100 E) over $100 1

2 Name: 5. The melting point of indium is C. At 323 F, what is the physical state of indium? T F T C 9F 5C 32F A) Solid. B) Liquid. C) Gas. D) Not enough information. E) At 323 F, the indium is partially solid and partially liquid; there is an equilibrium between the two states. 6. The density of gasoline is g/ml at 20 C. When gasoline is added to water: A) It will float on top. B) It will sink to the bottom. C) It will mix so, you can't see it. D) The mixture will improve the running of the motor. E) None of these things will happen. 7. Which of the following statements is false? A) Solutions are always homogeneous mixtures. B) The terms atom and element can have different meanings. C) Elements can exist as atoms or molecules. D) Compounds can exist as atoms or molecules. E) At least two of the above statements (A-D) are false. 8. An example of a pure substance is A) elements B) compounds C) pure water D) carbon dioxide E) all of these 9. What are the components of the scientific method? 10. On a new temperature scale ( Y), water boils at Y and freezes at 0.00 Y. Calculate the normal human body temperature using this temperature scale. On the Fahrenheit scale, normal human body temperature is 98.6 F, and water boils at F and freezes at 32.0 F. 11. Give three physical methods used by chemists to separate mixtures and identify the type of mixture best suited for each process. 12. How many significant figures are in A) 2 C) 4 B) 3 D) 5 2

3 Name: 13. Which of the following is not a fundamental metric unit? A) meter C) kilogram B) second D) liter 14. How should the number x 10 3 be properly expressed as a decimal? A) 1230 C) B) D) Calculate and report to the correct number of significant figures. A) 3.1 C) B) D) Which of the following pairs can be used to illustrate the law of multiple proportions? A) SO and SO 2 B) CO and CaCO 3 C) H 2 O and C 12 H 22 O 11 D) H 2 SO 4 and H 2 S E) KCl and KClO If the Thomson model of the atom had been correct, Rutherford would have observed: A) Alpha particles going through the foil with little or no deflection. B) Alpha particles greatly deflected by the metal foil. C) Alpha particles bouncing off the foil. D) Positive particles formed in the foil. E) None of the above observations is consistent with the Thomson model of the atom. 18. Which of the following atomic symbols is incorrect? A) B) C) D) E) 3

4 Name: 19. Which among the following represent a set of isotopes? Atomic nuclei containing: I. 20 protons and 20 neutrons II. 21 protons and 19 neutrons III. 22 neutrons and 18 protons IV. 20 protons and 22 neutrons V. 21 protons and 20 neutrons A) I, II, III B) III, IV C) I, V D) I, IV and II, V E) No isotopes are indicated. 20. Which of the following statements is true? A) Ions are formed by adding or removing protons or electrons. B) Scientists believe that solids are mostly open space. C) Heating water with a Bunsen burner results in a 2:1 mixture of hydrogen and oxygen gases. D) At least two of the above statements (A-C) are true. E) All of the statements (A-C) are false. 21. has A) 20 protons, 20 neutrons, and 18 electrons B) 22 protons, 20 neutrons, and 20 electrons C) 20 protons, 22 neutrons, and 18 electrons D) 22 protons, 18 neutrons, and 18 electrons E) 20 protons, 20 neutrons, and 22 electrons 22. Which of the following statements is (are) true? A) and have the same number of neutrons. B) and are isotopes of each other because their mass numbers are the same. C) has the same number of electrons as. D) A and B E) A and C 23. An ion is formed A) By either adding or subtracting protons from the atom. B) By either adding or subtracting electrons from the atom C) By either adding or subtracting neutrons from the atom. D) All of the above are true. E) Two of the above are true. 4

5 Name: 24. All of the following are true except: A) Ions are formed by adding electrons to a neutral atom. B) Ions are formed by changing the number of protons in an atom's nucleus. C) Ions are formed by removing electrons from a neutral atom. D) An ion has a positive or negative charge. E) Metals tend to form positive ions. 25. Which of the following are incorrectly paired? A) K, alkali metal B) Ba, alkaline earth metal C) O, halogen D) Ne, noble gas E) Ni, transition metal 26. Which of the following are incorrectly paired? A) Copper, Cu B) Carbon, C C) Cobalt, Co D) Calcium, Ca E) Cesium, Ce 27. All of the following are characteristics of nonmetals except: A) poor conductors of electricity B) often bond to each other by forming covalent bonds C) tend to form negative ions in chemical reactions with metals D) appear in the upper left-hand corner of the periodic table E) do not have a shiny (lustrous) appearance 28. Which of the following has 61 neutrons, 47 protons, and 46 electrons? A) Pm B) Ag + C) Pd D) Cd + E) Ag 29. Which of the following names is incorrect? A) cobalt(ii) chloride B) magnesium oxide C) aluminum(iii) oxide D) diphosphorus pentoxide E) All of the above names are correct. 5

6 Name: 30. All of the following are in aqueous solution. Which is incorrectly named? A) H 2 SO 4, sulfuric acid B) H 2 CO 3, carbonic acid C) H 3 PO 4, phosphoric acid D) HCN, cyanic acid E) HCl, hydrochloric acid 31. Which of the following pairs is incorrect? A) NH 4 Br, ammonium bromide B) K 2 CO 3, potassium carbonate C) BaPO 4, barium phosphate D) CuCl, copper(i) chloride E) MnO 2, manganese(iv) oxide 32. Which of the following name(s) is(are) correct? 1. sulfide, S 2 2. ammonium chloride, NH 4 Cl 3. acetic acid, HC 2 H 3 O 2 4. barium oxide, BaO A) all B) none C) 1, 2 D) 3, 4 E) 1, 3, Three samples of a solid substance composed of elements A and Z were prepared. The first contained 4.31 g A and 7.70 g Z. The second sample was 35.9% A and 64.1% Z. It was observed that g A reacted with Z to form 2.00 g of the third sample. Show that these data illustrate the law of definite composition. 34. Complete the following table. Symbol # Protons # Neutrons # Electrons Net Charge 206 Pb Mn Arsenopyrite is a mineral containing As, Fe, and S. Classify each element as metal, nonmetal, or metalloid. 6

7 Name: 36. Write the chemical formulas for the following compounds or ions. a) nitrate ion _ b) aluminum oxide _ c) ammonium ion _ d) perchloric acid _ e) copper(ii) bromide _ Name the following compounds: 37. Al 2 (SO 4 ) NaH 39. AgCl 40. CaSO N 2 O SnI 2 Write the formula for: 43. sodium thiosulfate 44. dichlorine heptoxide 45. cobalt(ii) chloride 46. aluminum hydroxide 47. nitric acid 48. phosphorus trichloride 49. Which of these statements is a consequence (follows from) the Law of Definite Proportion? A) All samples of chlorine contain 35 Cl and 37 Cl in the same (definite) ratio. B) The mass of oxygen that is combined with a fixed mass of nitrogen in each of the binary nitrogen oxides can be expressed as a ratio of small whole numbers. C) The atomic masses of all of the elements in the periodic table have fixed values. D) The % lead by mass in the compound galena is the same for all pure samples obtained from any source. E) None of these is correct 7

8 Name: 50. How many protons, neutrons and electrons, in that order are present in the anion formed by one atom of 125 I? A) 53, 74, 54 D) 53, 72, 54 B) 52, 72, 53 E) 54, 74, 54 C) 54, 72, Which of the following compounds is incorrectly named? A) Mg(OH) 2 is magnesium dihydroxide D) K 3 PO 4 is potassium phosphate B) CaO is calcium oxide E) MgSO 3 is magnesium sulfite C) NH 4 NO 3 is ammonium nitrate 52. You have a sample of zinc (Zn) and a sample of aluminum (Al). You have an equal number of atoms in each sample. Which of the following statements concerning the masses of the samples is true? A) The mass of the zinc sample is more than twice as great as the mass of the aluminum sample. B) The mass of the zinc sample is more than the mass of the aluminum sample, but it is not twice as great. C) The mass of the aluminum sample is more than twice as great as the mass of the zinc sample. D) The mass of the aluminum sample is more than the mass of the zinc sample, but it is not twice as great. E) The masses of each sample are equal. 53. Which of the following equations is not balanced? A) 4Al + 3O 2 2Al 2 O 3 B) C 2 H O 2 2 2CO 2 + 3H 2 O C) 2KClO 3 2KCl O 2 D) 4P 4 + 5S 8 4P 4 S 10 E) P 4 + 5O 2 P 4 O Which of the following equations correctly describes the combustion of CH 4 and O 2 to produce water (H 2 O) and carbon dioxide (CO 2 )? A) CH O 2 CO 2 + H 2 O B) CH 4 + O 2 CO 2 + 2H 2 O C) CH 4 + 2O 2 CO 2 + 2H 2 O D) CH 4 + 3O 2 2CO 2 + H 2 O E) 2CH 4 + 3O 2 2CO 2 + 2H 2 O 8

9 Name: 55. The limiting reactant in a reaction A) has the lowest coefficient in a balanced equation B) is the reactant for which you have the fewest number of moles C) has the lowest ratio of moles available/coefficient in the balanced equation D) has the lowest ratio of coefficient in the balanced equation/moles available E) none of these 56. SO 2 reacts with H 2 S as follows: 2H 2 S + SO 2 3S + 2H 2 O When 7.50 g of H 2 S reacts with g of SO 2, which statement applies? A) 6.38 g of sulfur are formed. B) 10.6 g of sulfur are formed. C) moles of H 2 S remain. D) 1.13 g of H 2 S remain. E) SO 2 is the limiting reagent. 57. A 15-g sample of lithium is reacted with 15 g of fluorine to form lithium fluoride: 2Li + F 2 2LiF. After the reaction is complete, what will be present? A) 2.16 moles lithium fluoride only B) moles lithium fluoride only C) 2.16 moles lithium fluoride and moles fluorine D) moles lithium fluoride and 1.37 moles lithium E) none of these 58. The characteristic odor of pineapple is due to ethyl butanoate, a compound containing carbon, hydrogen, and oxygen. Combustion of 2.78 g of ethyl butanoate leads to formation of 6.32 g of CO 2 and 2.58 g of H 2 O. The properties of the compound suggest that the molar mass should be between 100 and 150 g/mol. What is the molecular formula? 59. One of the major commercial uses of sulfuric acid is in the production of phosphoric acid and calcium sulfate. The phosphoric acid is used for fertilizer. The reaction is Ca 3 (PO 4 ) 2 + 3H 2 SO 4 3CaSO 4 + 2H 3 PO 4. What mass of concentrated H 2 SO 4 (98% by mass) must be used to react completely with g of calcium phosphate? 9

10 Chem 1411 (Test 1) Review Answer Section 1. ANS: B PTS: 1 DIF: Easy REF: 1.3 KEY: Chemistry general chemistry general concepts measurement SI unit prefixes MSC: Quantitative 2. ANS: C PTS: 1 DIF: Easy REF: 1.3 KEY: Chemistry general chemistry general concepts measurement SI unit prefixes 3. ANS: C PTS: 1 DIF: Easy REF: 1.4 KEY: Chemistry general chemistry general concepts measurement 4. ANS: C PTS: 1 DIF: Easy REF: 1.7 KEY: Chemistry general chemistry general concepts measurement dimensional analysis MSC: Quantitative 5. ANS: D PTS: 1 DIF: Moderate REF: 1.8 KEY: Chemistry general chemistry general concepts measurement SI unit temperature 6. ANS: A PTS: 1 DIF: Easy REF: 1.9 KEY: Chemistry general chemistry general concepts measurement SI unit density 7. ANS: D PTS: 1 DIF: Easy REF: 1.1 KEY: Chemistry general chemistry general concepts matter 8. ANS: E PTS: 1 DIF: Easy REF: 1.1 KEY: Chemistry general chemistry general concepts matter 9. ANS: 1) Making observations (collecting data) 2) Suggesting a possible explanation (formulating a hypothesis) 3) Doing experiments to test the possible explanation (testing the hypothesis) Depending on the data from the experiments, the hypothesis may be modified and retested. See Sec. 1.2 of Zumdahl, Chemistry. PTS: 1 DIF: Easy REF: 1.2 KEY: Chemistry general chemistry general concepts scientific method 10. ANS: 57.3 Y The formula derived from the data is Y=(155/180)(F-32). PTS: 1 DIF: Difficult REF: 1.8 KEY: Chemistry general chemistry general concepts measurement SI unit temperature MSC: Quantitative 1

11 11. ANS: Three common methods are distillation, filtration, and chromatography. Distillation is useful for mixtures of volatile liquids (or mixtures of gases that can be condensed). Filtration is useful to separate a mixture of a solid and a liquid. Chromatography may be used for mixtures of volatile substances (gas chromatography) or soluble substances (paper chromatography). See Sec of Zumdahl, Chemistry. PTS: 1 DIF: Moderate REF: 1.1 KEY: Chemistry general chemistry general concepts matter mixture 12. ANS: B PTS: 1 DIF: Easy REF: 1.5 KEY: Chemistry general chemistry general concepts measurement significant figures 13. ANS: D PTS: 1 DIF: Easy REF: 1.3 KEY: Chemistry general chemistry general concepts measurement SI unit base unit 14. ANS: D PTS: 1 DIF: Easy REF: 1.5 KEY: Chemistry general chemistry general concepts measurement significant figures scientific notation 15. ANS: C PTS: 1 DIF: Easy REF: 1.5 KEY: Chemistry general chemistry general concepts measurement significant figures MSC: Quantitative 16. ANS: A PTS: 1 DIF: Easy REF: 2.2 KEY: Chemistry general chemistry early atomic theory atomic theory of matter 17. ANS: A PTS: 1 DIF: Easy REF: 2.4 KEY: Chemistry general chemistry early atomic theory atomic theory of matter structure of the atom nuclear model of atom 18. ANS: E PTS: 1 DIF: Easy REF: 2.5 KEY: Chemistry general chemistry early atomic theory atomic theory of matter structure of the atom 19. ANS: D PTS: 1 DIF: Easy REF: 2.5 KEY: Chemistry general chemistry early atomic theory atomic theory of matter isotope 20. ANS: B PTS: 1 DIF: Moderate REF: 2.5 KEY: Chemistry general chemistry early atomic theory 21. ANS: A PTS: 1 DIF: Easy REF: 2.6 KEY: Chemistry general chemistry early atomic theory atomic theory of matter isotope 22. ANS: E PTS: 1 DIF: Easy REF: 2.6 KEY: Chemistry general chemistry early atomic theory atomic theory of matter isotope 2

12 23. ANS: B PTS: 1 DIF: Easy REF: 2.6 KEY: Chemistry general chemistry early atomic theory chemical substance chemical formula ionic substance 24. ANS: B PTS: 1 DIF: Easy REF: 2.6 KEY: Chemistry general chemistry early atomic theory chemical substance chemical formula ionic substance 25. ANS: C PTS: 1 DIF: Easy REF: 2.7 KEY: Chemistry general chemistry early atomic theory periodic table group 26. ANS: E PTS: 1 DIF: Easy REF: 2.7 KEY: Chemistry general chemistry early atomic theory periodic table 27. ANS: D PTS: 1 DIF: Easy REF: 2.7 KEY: Chemistry general chemistry early atomic theory periodic table nonmetal 28. ANS: B PTS: 1 DIF: Easy REF: 2.7 KEY: Chemistry general chemistry early atomic theory periodic table 29. ANS: C simple compound 30. ANS: D simple compound acid 31. ANS: C simple compound ionic compound 32. ANS: A simple compound 33. ANS: Sample (1): ratio of masses (Z/A) = 7.70/4.13 = Sample (2): ratio of masses (Z/A) = 64.1/35.9 = Sample (3): ratio of masses (Z/A) = ( )/0.718 = These three samples thus illustrate that a given compound always contains the same proportion of elements by mass. See Sec. 2.2 of Zumdahl, Chemistry. PTS: 1 DIF: Moderate REF: 2.2 KEY: Chemistry general chemistry early atomic theory atomic theory of matter Dalton's atomic theory 3

13 34. ANS: Symbol # Protons # Neutrons # Electrons Net Charge 206 Pb Ga Te Mn PTS: 1 DIF: Easy REF: 2.5 KEY: Chemistry general chemistry early atomic theory atomic theory of matter nuclear structure 35. ANS: As = metalloid, Fe = metal, S = nonmetal PTS: 1 DIF: Easy REF: 2.7 KEY: Chemistry general chemistry early atomic theory periodic table 36. ANS: a) NO 3 b) Al 2 O 3 c) NH 4 + d) HClO 4 e) CuBr 2 KEY: Chemistry general chemistry early atomic theory chemical substance chemical formula ionic substance 37. ANS: aluminum sulfate simple compound ionic compound 38. ANS: sodium hydride simple compound ionic compound 39. ANS: silver chloride simple compound ionic compound 4

14 40. ANS: calcium sulfate simple compound ionic compound 41. ANS: dinitrogen trioxide simple compound binary molecular compound 42. ANS: tin(ii) iodide simple compound ionic compound 43. ANS: Na 2 S 2 O 3 KEY: Chemistry general chemistry early atomic theory chemical substance chemical formula ionic substance 44. ANS: Cl 2 O 7 KEY: Chemistry general chemistry early atomic theory chemical substance chemical formula molecular substance 45. ANS: CoCl 2 KEY: Chemistry general chemistry early atomic theory chemical substance chemical formula ionic substance 46. ANS: Al(OH) 3 KEY: Chemistry general chemistry early atomic theory chemical substance chemical formula ionic substance 5

15 47. ANS: HNO 3 simple compound acid 48. ANS: PCl 3 simple compound binary molecular compound 49. ANS: D PTS: 1 DIF: Easy REF: 2.2 KEY: Chemistry general chemistry early atomic theory atomic theory of matter Dalton's atomic theory 50. ANS: D PTS: 1 DIF: Moderate REF: 2.8 KEY: Chemistry general chemistry early atomic theory atomic theory of matter isotope periodic table 51. ANS: A simple compound ionic compound 52. ANS: A PTS: 1 DIF: Easy REF: 3.3 KEY: Chemistry general chemistry stoichiometry mass and moles of substance mole 53. ANS: C PTS: 1 DIF: Easy REF: 3.9 KEY: Chemistry general chemistry early atomic theory chemical equation balancing chemical equation 54. ANS: C PTS: 1 DIF: Easy REF: 3.9 KEY: Chemistry general chemistry early atomic theory chemical equation balancing chemical equation 55. ANS: C PTS: 1 DIF: Easy REF: 3.11 KEY: Chemistry general chemistry stoichiometry stoichiometry calculation limiting reactant 56. ANS: B PTS: 1 DIF: Moderate REF: 3.11 KEY: Chemistry general chemistry stoichiometry stoichiometry calculation limiting reactant MSC: Quantitative 57. ANS: D PTS: 1 DIF: Moderate REF: 3.11 KEY: Chemistry general chemistry stoichiometry stoichiometry calculation limiting reactant MSC: Quantitative 6

16 58. ANS: C 6 H 12 O 2 See Sec. 3.7 of Zumdahl, Chemistry g CO 2 * (12.01 g C/44.01 g CO 2 ) = 1.72 g C 2.58 g H 2 O * (2.016 g H/18.02 g H 2 O) = g H 2.78 g ethyl butanoate g C g H = 0.77 g O 1.72 g C * (1 mol C/12.01 g) = mol C ( 0.048) = 3 mol C g H * (1 mol H/1.008 g H) = mol H ( 0.048) = 6 mol H 0.77 g O * (1 mol O/16.00 g) = mol O ( 0.048) = 1 mol O empirical formula = C 3 H 6 O empirical formula mass = g/mol * 2 = 116 g/mol which is between 100 and 150 ( * 3 = 174.2, too much) therefore, molecular formula = 2(C 3 H 6 O) = C 6 H 12 O 2 PTS: 1 DIF: Difficult REF: 3.7 KEY: Chemistry general chemistry stoichiometry determining chemical formulas molecular formula MSC: Quantitative 59. ANS: 97 g H 2 SO 4 See Sec of Zumdahl, Chemistry. (100.00g) * (1 mol Ca 3 (PO 4 ) 2 / g)*(3 mol H 2 SO 4 /1 mol Ca 3 (PO 4 ) 2 )*(98.09 g/1 mol H 2 SO 4 ) *(100 g solution/98 g H 2 SO 4 ) = = 97 g H 2 SO 4 PTS: 1 DIF: Moderate REF: 3.1 KEY: Chemistry general chemistry stoichiometry stoichiometry calculation amounts of substances MSC: Quantitative 7