Lab Chemistry - Final Exam Review 1. Express in scientific notation. A) D) B) E) C)

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1 Lab Chemistry - Final Exam Review 1. Express in scientific notation. A) D) B) E) C) What is the result of the following multiplication expressed in scientific notation to the correct number of significant figures? ( )( ) = A) B) C) D) E) Using the rules of significant figures, calculate the following: = A) B) 25 C) 20 D) E) The number rounded to four significant figures is A) D) B) E) none of these C) How many significant figures are in the number ? A) 3 B) 4 C) 5 D) 6 E) 7 6. Convert 17.7 cm to inches (2.54 cm = 1 in). A) 45.0 in B) 4.50 in C) 6.97 in D) 69.7 in E) in 7. Convert: 84.6 mg = lb. A) lb D) lb B) lb E) lb C) lb 8. If kg equals lb, what is the mass in pounds of a human who weighs kg? A) lb D) lb B) lb E) none of these C) lb 9. Calculate the mass of a rectangular solid that has a density of 2.73 g/cm 3 and measures 2.50 cm by 1.80 cm by 3.00 cm. A) 4.95 g B) 36.9 g C) 6.82 g D) 19.9 g E) 39.9 g 10. Convert: 52.4 L = ml. A) ml D) ml B) ml E) 5.24 ml C) ml 11. Which of the following is an SI unit for expressing the mass of a block of Au? A) m B) g C) L D) pound 12. Density is an example of a A) chemical property D) chemical change B) physical property E) physical change C) qualitative property 13. Which of the following processes require(s) chemical methods? A) Separating a homogeneous mixture into pure substances. B) Separating a heterogeneous mixture into pure substances. C) Distilling a saltwater mixture. D) Breaking a compound into its constituent elements. E) At least two of the above (a-d) require chemical methods.

2 14. Which of the following is a homogeneous mixture? A) pure water D) soil B) gasoline E) copper metal C) jar of jelly beans 15. A change involves a change in the fundamental components of the substance; a given substance changes into a different substance or substances. A) chemical B) physical C) mixed D) potential E) kinetic 16. The first scientist to develop the theory that all atoms of a given element are identical was A) John Dalton D) Ernest Rutherford B) J. J. Thomson E) James Chadwick C) Lord Kelvin 17. Which particle has the smallest mass? A) neutron B) proton C) electron D) helium nucleus 18. The mass number of an atom equals A) the number of neutrons per atom B) the atomic mass of the element C) the atomic number of the element D) the number of protons plus the number of neutrons per atom E) none of the above 19. An atom that has 54 protons, 54 electrons, and 78 neutrons is A) B) C) D) E) 20. The number of protons in the nucleus of an atom is called its A) mass number D) atomic number B) valence E) none of these C) isotope number 21. The form of EMR that has more energy per photon than ultraviolet rays but less energy per photon than gamma rays is A) microwaves D) infrared rays B) radio waves E) none of these C) X rays 22. When an electron in the ground state absorbs energy, it goes to a(n) state. A) excited B) lower C) frenetic D) ionic E) stable 23. A d sublevel can hold a maximum of A) 5 electrons D) 32 electrons B) 10 electrons E) none of these C) 14 electrons 24. The maximum number of electrons allowed in the fourth energy level is A) 2 B) 4 C) 8 D) 18 E) Classify each of the following as a physical (P) or a chemical (C) change. a. cooking an egg b. boiling water c. ironing a shirt d. burning gasoline

3 26. Classify each of the following as an element (E), a compound (C), a Homogeneous mixture (Hom), or a Heterogeneous mixture (Het). a. gold b. ice c. aluminum d. distilled water e. tap water 27. Write the electron configuration for Al. 28. Draw the orbital diagram (using arrows) for the ground state of oxygen. 1s 2s 2p 29. Write the electron configuration for B. Determine the number of protons and the number of neutrons for each of the following.!!!!!! 30. Pb C The element with 3 energy levels and 5 valence elctrons is A) Y B) P C) In D) Cl Use the following to answer questions Write the correct chemical formula for each of the following compounds. 33. iron(iii) phosphide 34. sodium sulfide

4 35. carbon monoxide 36. potassium carbonate 37. lead(ii) sulfite 38. lithium oxide 39. iron (III) chloride 40. ammonium dichromate 41. calcium hydroxide Use the following to answer questions Write the correct name for each of the following compounds. 42. LiC 2 H 3 O K 2 CO Fe(OH) CO Al(OH) SiO K 2 S 49. Mn(NO 3 ) 2

5 50. CaCl2 51. SnO What is the differnce between Ionic and Covalent bonding? 53. A reaction that involves a transfer of electrons is called a(n) reaction. A) precipitation D) double-displacement B) acid-base E) none of these C) oxidation-reduction 54. An aqueous solution of sodium sulfate is allowed to react with an aqueous solution of calcium nitrate. Identify the solid in the reaction. A) Na 2 SO 4 B) Ca(NO 3 ) 2 C) CaSO 4 D) NaNO An aqueous solution of calcium chloride is mixed with an aqueous solution of sodium sulfate. Use the following to answer questions Balance each of the following equations and state the reaction type. 56. MgCl 2 + K 3 PO 4 Mg 3 (PO 4 ) 2 + KCl 57. C 6 H 14 + O 2 CO 2 + H 2 O 58. Si(s) + HF(aq) SiF 4 (g) + H 2 (g) 59. Zn(s) + H 3 PO 4 (aq) Zn 3 (PO 4 ) 2 (s) + H 2 (g) 60. Al(s) + CaCl 2 (aq) Cu(s) + AlCl 3 (aq) 61. Sb(s) + O 2 (g) Sb 2 O 3 (s) 62. Fe(NO 3 ) 2 (aq) + H 2 S(g) FeS(s) + HNO 3 (aq) Use the following to answer questions Show all of your work and use units for each of the following calculations g of Cr represents how many atoms?

6 64. A 79.5-g sample of SO 2 contains how many moles of SO 2? 65. How many moles of Ca are in g Ca? 66. The mass of 0.56 mol of H 2 is g. 67. A sample of metal weighing 2.62 g is combined with oxygen; the metal oxide weighs 3.01 g. The mass percent of oxygen in the compound is. 68. A compound contains 12.8% C, 2.1% H, and 85.1% Br. Calculate the empirical formula. 69. What is the percent (by mass) of carbon in glucose, C 6 H 12 O 6? 70. Nitrogen molecule: N Consider the reaction 4Fe + 3O 2 --> 2Fe 2 O 3! If 12.7 g of iron(iii) oxide (rust) is produced from a certain amount of iron, how many grams of oxygen are needed for this reaction? 72. For the reaction! if 4.78 g of S is reacted with 10.0 g of O 2, how many grams of SO 3 will be produced? 73. In the reaction between CO and Fe 3 O 4, the theoretical yield in an experiment is calculated to be 47.2 g Fe. When a careless chemistry student carries out the experiment, the actual yield is 34.4 g Fe. Calculate the percentage yield. 74. For the reaction! if 6.0 mol of CO 2 are produced, how many moles of O 2 were reacted?

7 75. How many molecules of carbon dioxide will be formed if 4.94 g of propane is burned in the following reaction?!

8 Answer Key - Final Exam Review - Jun B 2. C 3. D 4. A 5. E 6. C 7. E 8. A 9. B 10. B 11. B 12. B 13. D 14. B 15. A 16. A 17. C 18. D 19. A 20. D 21. C 22. A 23. B 24. E 25. a. C b. P c. P d. C 26. a. E b. C c. E d. C e. Hom 27. [Ne] 3s 2 3p number or arrows: s 2s 2p 29. 1s 2 2s 2 2p protons, 125 neutrons protons, 8 neutrons 32. B 33. FeP 34. Na 2 S 35. CO

9 37. PbSO Li 2 O 39. FeCl (NH 4 ) 2 Cr 2 O Ca(OH) lithium acetate 43. potassium carbonate 44. iron(iii) hydroxide 45. carbon dioxide 46. aluminum hydroxide 47. silicon dioxide 48. potassium sulfide 49. manganese (II) nitrate 50. calcium chloride 51. tin (IV) oxide 52. Ionic transfers valence electrons (forming ions); covalent shares valence electrons. 53. C 54. C 55. CaCl 2 (aq) + Na 2 SO 4 (aq) CaSO 4 (s) + 2 NaCl(aq) 56. 3MgCl 2 + 2K 3 PO 4 Mg 3 (PO 4 ) 2 + 6KCl Double Replacement 57. 2C 6 H O 2 12CO H 2 O comubustion, oxidation-reduction 58. Si(s) + 4HF(aq) SiF 4 (g) + 2H 2 (g) SR, O-R 59. 3Zn(s) + 2H 3 PO 4 (aq) Zn 3 (PO 4 ) 2 (s) + 3H 2 (g) single replacement, oxidation-reduction 60. 2Al(s) + 3CuCl 2 (aq) 3Cu(s) + 2AlCl 3 (aq) SR, O-R 61. 4Sb(s) + 3O 2 (g) 2Sb 2 O 3 (s) S 62. Fe(NO 3 ) 2 (aq) + H 2 S(g) FeS(s) + 2HNO 3 (aq) DR atoms mol mol g % 68. CH 2 Br C 2 H 4 Br % 70. linear g g

10 mol molecules

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