Chemistry Final Exam Review 2021

i Toombs 2015 CHEMISTRY 11 FINAL EXAM REVIEW This is a GENERAL OVERVIEW ...it by no means serves as a complete review it will give you an idea of which sections you need to focus on most! (This does not cover definitions and theory from your class notes) INTRODUCTION TO WORKING in the LABORATORY 1. The term that refers to the reproducibility of a laboratory measurement is a) precision b) repeatability c) accuracy d) exactness 2. The marks on the following target represent someone who is: a) accurate, but not precise. b) precise, but not accurate, c) both accurate and precise. d) neither accurate nor precise 3. a) Clearly state the temperature in 0C, read from the thermometer illustrated to the right: b) How many significant digits should be reported in the correct answer? c) What is the uncertainty of this measurement? d) State this temperature in Kelvin 4. The number of significant digits in 0.30500 is a) 1 b) 2 c) 3 d) 4 e) 5 5. The result of2.350 x (4.0 + 6.311) is, a) 24 b) 24.2 c) 24.21 d) 24.205 6. Make the following Metric System conversions using "unit analysis" (you may use scientific notation): a) 825 cm = km b) 19 mL = cL c) 18 eg = Hg INTRO TO CHEMISTRY 1. Write the combining capacity of each element in: a) MgS: Mg b) CU2O: Cu S O c) P+(Mn02)2: Pt _____ AAn O _____ 2. List two diatomic elements: 3. List the most metallic element on the periodic table: 4. 5. 6. 7. a) As Which of the following is a metalloid? Which of the following is a transition metal? Which of the following is an alkali metal? Which of the following is a lanthanide? a) CI a) Mg a) Xe b) Ag b) Ni b) Kr b) Eu b) Au c) S c) P c) K c) Cd d) Pb e) He d) Ca e) C e) H e) W e) Hg d) Al d) P Which element has the highest melting point? a) Pb c) Os d) W 9. Define anion and give one example of a monatomic and one example of a polyatomic anion. 8. 10. FILL IN 1PHE FOLLOWING CHART: Combination Bond Type Formula Name (ionic or covalent) C / CI SC3N5 iron (III) perarsenate triselenium nonaiodide 12. Define endothermic reaction and give one example that is a physical change. (You should be able to write a realistic example). 13. Define exothermic reaction and give one example that is a chemical change. (You may use fictitious substances such as A2B(a Al + Mn?* b) KOH + CI2 —> KCI + KCIO3 + H20 c) KMn04 + Cr —> d) Calcium bicarbonate reacts when heated... e) C3H8 + 02 —> 2. A reaction between Lead and Oxygen produced 68.6 g of Pb304. How many grams of oxygen and lead were involved? 3. 57 g of calcium hydroxide is reacted with 91 g of oxalic acid. What are the two products in this reaction, and how many grams of each product are formed? 4. Define molecular formula, structural formula and empirical formula, and give one example of each. 5. An ionic compound contains 29.0% Na, 40.6% 5, and 30.4 % 0. What is the empirical formula for the compound? 6. Find the percentage composition for sulphuric acid. 4 Toombs 2015 CHEMISTRY 1FINAL EXAM REVIEW SOLUTIONS 1. What volume of 3.5 M phosphoric acid solution can be made using 75 g of phosphoric acid? 2. When barium nitrate and lithium sulphate are mixed, the products will be: a) both aqueous b) both solid precipitates c) one aqueous solution and one solid precipitate d) the reaction will not proceed 3. The following two solutions are mixed: 300. ml of 0.50 M AI2S3 (aq) and 150 ml of 0.30 M 5r(OH)2 (aq). a) State the concentrations of each of the ions after mixing. Include the dissociation equation(s) in your answer. b) Identify the precipitate that forms. Write the net ionic equation for this precipitation reaction. c) State the limiting and excess reagents. d) Clearly list all ion concentrations AFTER mixing and precipitation is complete. 4. What volume of 0.50 M hydrochloric acid solution will neutralize 30. ml of 0.01 M barium hydroxide (aq). Write the full formula equation for this reaction. If you were to write a net ionic equation, what would it be? 5. If a solution conducts a current, it must contain: a) an ionic compound b) a covalent compound c) an exothermic reaction d) neutrons 6. State whether each statement is True or False and explain your choice. a) Ionic compounds which dissociate in solution will conduct electricity b) Covalent molecules do not dissociate in solution and conduct a current c) 500. mL of a 2.0 M solution is more concentrated than 150 mL of a 3.5 M solution d) Adding more water to a solution improves the dissociation of the ionic compound 5 Toombs 2015 CHEMISTRY 11 FINAL EXAM REVIEW Toombs 2012 CHEMISTRY 11 FINAL EXAM REVIEW - ANSWERS INTRODUCTION TO WORKING in the LAB ANSWERS: 1A 2D 3a) 27.5 0C 3b) 3 SF (because we can estimate to ± i of a reading, so that gives the 1 dec place and thus the 3SF) 3c) ± 0.5 0£ 3d) sig fig rules so the answer is 300. K or 3.00 x 102 K for 3 SF 4E 5B 6a) 8.25 x lO"3 km 6b) 1.9 cL 6c) 1.8 x 103 (xg INTRO TO CHEMISTRY ANSWERS: 1. Write the combining capacity of each element in: a) MgS: AAg = +2 S = -2 b) CugO: Cu = +1 O = -2 c) Pt(Mn02)2'- Ft +2 since MnOa = -1 and O = -2 then Mn = +3 2. List two diatomic elements: N, O, F, CI, Br, I, At 3. List the most metallic element on the periodic table: Fr 4a 5b 6c 7b 8d 9. An anion is an element that has gained electrons in its valence shell, or a group of elements that has gained electron(s). Monatomic examples: F"1 and N*3 and a polyatomic example is PO4"3 10. FILL IN THE FOLLOWING CHART: Combination Bond Type (ionic or covaient) Formula Name C / CI Covalent ionic ecu Carbon tetrachloride SC3N5 Scandium (V) nitride Ionic Covalent FeAs05 iron (III) perarsenate triselenium nonaiodide Sc5 / N3 Fe3 / As053 Se/I 5c3l9 12. In an endothermic reaction, heat is absorbed by the reactants in order to make products. For example: H2O (I) + heat H2O (g) is a physical change. 13. In an exothermic reaction the reactants combine to form products, and energy in the form of heat or light is also produced and given off to the surroundings. For example: AgB (Qq) + CD2 (aq) -> 2AD (aq) + BC (aq) + 450 kj This is a chemical change. 450 kj of energy is released. 14. Symbol Number of protons Number of neutrons Number of electi ons Name 15. 69.50% 63Cu and 30.50% 65Cu 65 Cu 86 Kr 29 36 78 36 36 117 75 46 29 50 36 Copper Kryploo. Platinum, ion Krypton 195pt+3 82Kr 36 Toombs 2015 CHEMISTRY 11 FINAL EXAM REVIEW THE MOLE CONCEPT ANSWERS: 1. 6.02x 1023 2. 35 L 3. 4.29 x 1023 atoms 4. 4.4x1024atoms 5. Equal moles of two gases at the same temperature and pressure conditions occupy the same volume. 6. 71.2 g/mole. Gas # 2 = CI? (g) GAS LAWS ANSWERS: 1. PV = nRT V = 40 L 3. V1P1 = V2P2 \/Z - 3.33 x 10"5 L 2. Vi/Ti= V2/T2 V2 = 4.22 L 4. V = 130 L 5. V = 520 L CHEMICAL CHANGE 1. a) 3Mn2+ + 5A!3+ 3CI2 -» b) 6KOH + c) 2KMn04 + Cr d) Ca(HC03)2 -» Ca(s) e) C3H8 + 502 ^ 2. 6.40 g O2 and 62.2 g Pb ANSWERS: + 5AI 5KCI + Cr(Mn04) 2 H2 (g) 3C02 (g) 3Mn7+ IKCIO3 + 3H20 2K + 2C(s) + + 4H20 (1) 302 (g) 3Pb + 202 ^Pb304 3. 27.7 g HzO and 98.6 g CaC204 limiting reagent: Ca(OH) 2 Excess reagent: 0.24 moles of excess H2C2O4 The L of C of M applies to all reactions and therefore all calculation questions. US = 148 g. RS = 27.7 g + 98.6 g + 21.6 g excess = 147.9g 4. refer to your notes or text 5. Na2S203 6. 2.06%H 32.7%S 65.2%0 7. refer to your notes or text. ATOMIC STRUCTURE AND BONDINS SOLUTIONS ANSWERS: ANSWERS: 1. 0.22 L 2 c) one aqueous solution and one solid precipitate 3 a) After mixing (dilution and dissociation), but BEFORE precipitation, the ion concentrations are: [Sr+2] = 0.10 M [S-2] = 0.99 M [Al+3] = 0.66M [OH"] = 0.20M b) Ar3+ 30H"-> Al(OH)3 (s) | c) limiting reagent: [OH"] and excess reagent: [AF3] d) After precipitation, the ion concentrations are: [Sr*2] = 0.10 M [AF3] = 0.59 M [S~2] = 0.99 M [OH~] = ZERO 4. 1.2 mL Net ionic equation of all neutraliazation reactions: H+(aq) + OH" (aq) H2O (I) 5. a) an ionic compound 6a) TRUE. When ions dissociate as they dissolve in aqueous solution, a current can be conducted. 6b) TRUE. Covalent molecules do not do not dissociate in solution and therefore no electrical conductivity 6c) FALSE. 3.5 M (or moles per litre) > 2.0M regardless of the 'sample size' (how many mL you have) 6d) FALSE . Diluting the solution means there is a higher volume of solution in the ratio of moles of solute: Litres of solution. The solution becomes less concentrated, less saturated, and the MOLARITY of each of the ions in solution decreases. Adding more water to the solution, does not, however, improve the ability of the substance to dissolve and dissociate.