Dr. Woodbury Practice EXAM 1 Name _____________________________ Dr. Erik Woodbury CHEMISTRY 1A PRACTICE EXAM 1 Multiple Choice Circle one 1. A B C D E 2. A B C D E permitted. All information required is contained on the exam. Place all work 3. A B C D E in the space provided. If you require additional space, use the back of the 4. A B C D E 5. A B C D E 6. A B C D E (1) Read each question carefully. 7. A B C D E (2) For Part I, there is no partial credit given and only answers marked on 8. A B C D E 9. A B C D E 10. A B C D E Instructions: CLOSED BOOK EXAM! No books, notes, or additional scrap paper are exam. A scientific calculator may be used. Please remember that the De Anza Code of Academic Conduct applies to this exam and all other graded work in the class. This exam has 11 pages. this cover page will be graded. (3) The last page contains some useful information. You may remove it for easy access. (4) If you finish early, RECHECK YOUR ANSWERS! 1-10 total (5) This practice Exam is longer than the lecture exam will be. It 11. A B C D E 12. A B C D E 13. A B C D E intentionally covers a greater breadth of questions than the lecture exam can. Possible Points Points # 1–10 (2 points each) / 20 14. A B C D E # 11-15 (4 points each) / 20 15. A B C D E # 16-19 / 32 # 20-22 / 18 # 23 / 16 #25-27 / 27 # 28-32 / 42 / 175 Total Score (175) 1 11-15 total: Dr. Woodbury Practice EXAM 1 Part I: Multiple Choice, Concepts (2 points each) Select the best answer and enter your choice on the cover sheet – No partial credit 1) Ionic bonds tend to form between a. Metals and metals b. Non metals and non metals c. Noble gases and non metals d. Non metals and metals e. Metalloids and metals 2) According to the Scientific Method, a series of observations are summarized by a/an a. Hypothesis b. Law c. Theory d. Model e. Experiment 3) Blood’s ability to fix oxygen is an example of a. A Physical property b. A Nuclear property c. A Biological property d. A Chemical property e. A Mechanical property 4) Elements differ from compounds in that compounds a. Cannot be broken down farther by physical means b. Cannot be broken down farther by chemical means c. Can be broken down farther by chemical means d. Can be broken down farther by physical means e. Contain only one type of atom 5) In order to create a cation, an atom must a. Gain a neutron b. Lose a neutron c. Gain an electron d. Lose an electron e. Lose a proton 2 6) Which of the following states that compounds always contain the same relative amounts of elements by mass? a. Law of Conservation of Mass b. Law of Multiple Proportions c. Law of Definite Proportions d. Law of Conservation of Energy e. None of the above 7) Group 2 is also called the a. Halogens b. Noble Metals c. Chalcogens d. Alkaline Earth Metals e. Alkali Metals 8) Ionic bonds tend to form between a. Metals and metals b. Metals and non metals c. Non metals and non metals d. Metalloids and metals e. Noble gases and noble metals 9) Data that is close to the desired value can be said to a. Be precise b. Contain systematic error c. Be accurate d. Contain random error e. None of the above 10) Which of the following is likely to be the best conductor of electricity? a. Pure water b. A mixture of water and magnesium bromide c. A mixture of water and magnesium carbonate d. A mixture of water and acetic acid e. A mixture of water and copper metal Dr. Woodbury Practice EXAM 1 Part II: Multiple Choices, Short Calculations (4 points each) Select the best answer and enter your choice on the cover sheet – No partial credit 11) How many atoms does 0.357 mol of CaCl2 contain? A. 7.38x1022 atoms B. 2.15x1023 atoms C. 7.16x1022 atoms D. 6.45x1023 atoms E. 1.81x1024 atoms 12) What is the percent mass of carbon in C6H5O3N? A. 27.94 % B. 48.20 % C. 51.80 % D. 57.60 % E. 72.06 % 13) 286 K is what temperature on the Fahrenheit scale? A. 1038 °F B. 974 °F C. -8.6 °F D. 55.4 °F E. none of the above 14) For the following balanced equation how many moles of oxygen gas are needed to make 6.73 mols of iron oxide? 4 Fe (s) + 3 O2 (g) 2 Fe2O3 (s) A. 10.1 moles B. 4.47 moles C. 2.24 moles D. 13.46 moles E. 5.05 moles 15) How many moles of NaOH would be needed to completely react with 25 mL of 0.150 M H2SO4? A. 3.75 E-3 mol B. 7.50 E-3 mol C. 3.75 mol D. 7.50 mol E. 1.88 E-3 mol 3 Dr. Woodbury Practice EXAM 1 Part III: Short Answer 16) Identify whether the following are Elements, Compounds, Heterogeneous Mixtures or Homogeneous Mixtures. (6 points) Milk _______________ Bronze ____________ Gold _______________ Sugar ____________ An Orange ____________ Diamond _______________ 17) Identify whether the following is a physical (P) or chemical (C) property of mercury (6 points) Melts at 234K ________ Shiny Poisonous ________ Is much denser than water __________ Flame retardant _________ 18) __________ Reacts with air to form HgO _________ Draw a representation of the atom according to JJ Thomson’s theory and according to Rutherford’s theory (8 points) 19) Give the number of protons, electrons and neutrons in each atom below: (12 points) Atom / Ion 13 Protons Neutrons C 43 Fe2+ 37 Cl- 238 U 4 Electrons Dr. Woodbury 20) Practice EXAM 1 Explain how Millikan’s oil-drop experiment worked and what it found. Feel free to use diagrams if you wish: (6pts) 21) Using the attached solubility rules, write the balanced, total ionic and net ionic equations for the reaction of aqueous silver nitrate and aqueous lithium phosphate. (6 pts) 22) Write the molecular formula for ionic compounds made from the following atom pairs: (6pts) a. Sodium and Bromine ____________ b. Nitrogen and Magnesium ____________ c. ____________ Potassium and Oxygen 5 Dr. Woodbury 23) Practice EXAM 1 (16 pts.) Nomenclature Name the following compounds: a. KOH __________________________ b. H3PO4 __________________________ c. CH4 __________________________ d. P2S2 __________________________ e. Sn(NO2)4 __________________________ f. Mg3N2 __________________________ g. Hg2SO3 __________________________ h. (NH4)2CO3 __________________________ Give the correct formula for the following compounds: i. Xenon tetrafluoride __________________________ j. Lead (II) bicarbonate __________________________ k. Nitrogen triiodide __________________________ l. Cesium acetate __________________________ m. Copper (II) chromate __________________________ n. Hydrosulfuric acid __________________________ o. Mercury (II) sulfide __________________________ p. Stannic Oxide __________________________ 6 Dr. Woodbury 24) Practice EXAM 1 Balance the following reactions by filling in the missing coefficients. (12 points) a. ____C4H4 (g) + _______O2 (g) ______CO2 (g) + ______H2O (g) b. _____NaCl (aq) + _____Pb(NO3)2 (aq) _____NaNO3 (aq) + _____PbCl2 (s) c. _____H2SO4 (aq) + _____KOH (aq) _____K2SO4 (aq) + _____H2O (l) 7 Dr. Woodbury 25) Practice EXAM 1 For each of the following molecules, give the oxidation number for each atom. (7 pts) a. Na2SO3 b. NH4ClO3 Na_____ S_____ O_____ N _____ H_____ Cl_____ O_____ 26) For the following reaction, identify the reducing agent and the oxidizing agent ( 4 pts) Fe2O3 (s) + 2 Al (s) 2 Fe (l) + Al2O3 (l) (the thermite reaction! Note the liquid iron.) 27) Using solubility rules and the activity table as necessary predict the products of the following reactions and write the balanced reaction. Identify each reaction type. If no reaction, write “No Reaction” for type. (16 pts) Al (s) + ZnSO4 (aq) Type________________________ HCl (aq) + Ca(OH)2 (aq) Type________________________ NasS (aq) + Pb(NO3)2 Type________________________ Ni(NO3)2 (aq) + Cu (s) Type________________________ 8 Dr. Woodbury 28) Practice EXAM 1 Which of the following solutions would make a better conductor of electricity? Support your statement quantitatively. (6 pts) 29) Solution A: 0.364M solution of Ca(NO3)2 Solution B: 0.257M solution of Al2(SO4)3 Underline all of those below that are strong acids. Circle those that are weak acids. Put an X through any bases. (5 points) d. CH3COOH g. H2SO3 i. PO43- b. HClO4 e. Ca(OH)2 h. HNO2 j. NH3 c. f. HClO3 a. HI H 2O Calculations. Show all work for full credit. 30) (10 pts each) A compound is analyzed and found to contain the following elements by mass: C: 11.3964 g H: 0.9565 g N: 6.6471 g In addition, the molecular mass is found to be 80.092 g/mol. What is this the empirical formula of the molecule? What is the molecular formula? 9 Dr. Woodbury Practice EXAM 1 31) For the following balanced reaction, determine what the theoretical yield of each product is: Pb(CO3)2 (s) + 2 H2SO4 (aq) Pb(SO4)2 (aq) + 2 H2O (l) + 2 CO2 (g) Starting material: Pb(CO3)2 : 0.4025 g H2SO4 : 0.2254 g What is the percent yield of water if 40.0 mg are obtained? 32) A mad scientist wishes to build his fortune by collecting large amounts of compounds that contain silver. Currently, his aim is to isolate 355 g of silver sulfate. What volume (in mL) of the following two solutions will he need to isolate this amount of product? (I) a. Solution A: 1.25 M AgNO3 b. Solution B: 0.744 M Na2SO4 10 Dr. Woodbury Practice EXAM 1 PERIODIC TABLE Key 1 Atomic Number Symbol Atomic Mass Electronegativity H 1.008 2.20 3 2 He 4.003 - 4 5 6 7 8 9 10 Li Be B C N O F Ne 6.941 0.98 9.012 1.57 10.81 2.04 12.01 2.55 14.01 3.04 16.00 3.44 19.00 3.98 20.18 - Na 11 Mg Al Si 14 15 16 S Cl Ar 22.99 0.93 24.31 1.31 26.98 1.61 28.09 1.90 30.97 2.19 32.06 2.58 35.45 3.16 39.95 - 19 12 21 Ti 22 23 V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 39.10 0.82 40.08 1.00 44.96 1.36 47.90 1.54 50.94 1.63 52.00 1.66 54.94 1.55 55.85 1.83 58.93 1.88 58.70 1.91 63.55 1.90 65.38 1.65 69.72 1.81 72.59 2.01 74.92 2.18 78.96 2.55 79.90 2.96 83.80 - 42 43 26 44 27 45 28 46 29 47 30 48 31 49 32 50 33 51 34 35 18 Sc 41 25 17 Ca 40 24 P K 37 20 13 36 Rb Sr 38 39 Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te 52 53 I Xe 54 85.47 0.82 87.62 0.95 88.91 1.22 91.22 1.33 92.91 1.6 95.94 2.16 (98) 1.9 101.1 2.2 102.9 2.28 106.4 2.20 107.9 1.93 112.4 1.69 114.8 1.78 118.7 1.96 121.8 2.05 127.6 2.1 126.9 2.66 131.3 - 55 56 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 132.9 0.79 87 137.3 0.89 88 175.0 1.27 103 178.5 1.3 104 180.9 1.5 105 183.9 2.36 106 186.2 1.9 107 192.2 2.20 109 195.1 2.28 197.0 2.54 200.6 2.00 204.4 2.04 207.2 2.33 209.0 2.02 (209) 2.0 (210) 2.2 (222) - (223) 0.7 (226) 0.9 (260) - - - - - 190.2 2.2 - Fr Ra Lr Unq 57 Unp 58 Unh 59 Uns 60 61 Une - 62 63 64 65 66 67 68 69 70 La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb 138.9 1.10 140.1 1.12 140.9 1.13 144.2 1.14 (145) 1.13 150.4 1.17 152.0 1.2 157.3 1.20 158.9 1.2 162.5 1.22 164.9 1.23 167.3 1.24 168.9 1.25 173.0 1.1 Ac 89 Th 90 Pa 91 92 U Np 93 Pu 94 Am Cm Bk Cf Es Fm Md No (227) 1.1 232.0 1.3 (231) 1.5 238.0 1.38 (237) 1.36 (244) 1.28 (243) 1.3 (247) 1.3 (247) 1.3 (251) 1.3 (252) 1.3 (257) 1.3 (258) 1.3 (259) 1.3 11 95 96 97 98 99 100 101 102 Dr. Woodbury Practice EXAM 1 12