* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download Midterm Practice Exam Key
Inorganic chemistry wikipedia , lookup
Chemical equilibrium wikipedia , lookup
Supramolecular catalysis wikipedia , lookup
Acid dissociation constant wikipedia , lookup
History of chemistry wikipedia , lookup
Metastable inner-shell molecular state wikipedia , lookup
X-ray photoelectron spectroscopy wikipedia , lookup
Nucleophilic acyl substitution wikipedia , lookup
Biochemistry wikipedia , lookup
Chemical thermodynamics wikipedia , lookup
Process chemistry wikipedia , lookup
Nuclear chemistry wikipedia , lookup
Artificial photosynthesis wikipedia , lookup
Water splitting wikipedia , lookup
Marcus theory wikipedia , lookup
Chemical reaction wikipedia , lookup
Rate equation wikipedia , lookup
Photoredox catalysis wikipedia , lookup
Hydrogen-bond catalysis wikipedia , lookup
Rutherford backscattering spectrometry wikipedia , lookup
Hydroformylation wikipedia , lookup
Evolution of metal ions in biological systems wikipedia , lookup
George S. Hammond wikipedia , lookup
Acid–base reaction wikipedia , lookup
Click chemistry wikipedia , lookup
Hydrogen atom wikipedia , lookup
Electron configuration wikipedia , lookup
Lewis acid catalysis wikipedia , lookup
Stoichiometry wikipedia , lookup
Physical organic chemistry wikipedia , lookup
Electrolysis of water wikipedia , lookup
Strychnine total synthesis wikipedia , lookup
Electrochemistry wikipedia , lookup
Transition state theory wikipedia , lookup
Metalloprotein wikipedia , lookup
Atomic theory wikipedia , lookup
Gr ade 12 Chemistry Midterm Practise Examination Answer Key y e rK Name: ______________________________________ e sw Student Number:_____________________________ Attending q Non-Attending n A q Phone Number: ______________________________ For Marker’s Use Only Date: ___________________________ Final Mark _______ /100 = ________% Comments: Address:____________________________________ ____________________________________________ ____________________________________________ Instructions You have a maximum of 3 hours to complete your final examination. The final examination will be weighted as follows: n Modules 1 to 3: 100% The format of the examination will be as follows: n n n Part A: Multiple Choice (27 x 1 = 27 marks) Part B: Fill-in-the-Blanks (23 x 1 = 23 marks) Part C: Short Answer (50 marks) Include units with all answers as required. You will need the following in order to complete this examination: n n n n writing utensils and eraser or correction fluid scrap paper a ruler a graphing or scientific calculator The following resources are provided at the end of this examination: n n n n n n n n Periodic Table of Elements Alphabetical Listing of the Elements and Their Atomic Masses Table of Electronegativities Relative Strengths of Acids Table Solubility Chart Table of Standard Reduction Potentials with Values Names, Formulas, and Charges of Common Ions Common Ions Midterm Practise Examination Answer Key 1 of 28 Part A: Multiple Choice (27 marks total) Use the answer sheet found at the end of this examination to answer the multiple‑choice questions in this section. Shade in the circle that corresponds to your answer. DO NOT circle your answers directly on the examination. Aqueous Reactions (7 marks) 1. Oxidation is defined as a a. gain of electrons b. gain of hydrogen c. loss of electrons d. loss of oxygen 2. Which of the following statements about an oxidation number is FALSE? a. The number can be positive. b. The number can be assigned to a molecule. c. The number can be negative. d. The numbers are assigned according to a set of rules. 3. As a free element, the oxidation number of chlorine is a. +1 b. –1 c. +2 d. 0 4. In which reaction is oxidation occurring? a. Mg2+ + 2e– → Mg b. Ba2+ + S2– → BaS c. NH3 + H+ → NH4+ d. 2Cl– → Cl2 + 2e– 5. Identify the reducing agent in the following reaction: Na(s) + H2O(l) → NaOH(aq) + H2 (g) a. Na b. H2O c. NaOH d. H2 2 of 28 Grade 12 Chemistry Name: ___________________________________________ 6. Determine what happens in the following reaction: S + Cl2 → SCl2 a. Chlorine is oxidized. b. Chlorine is reduced. c. Sulphur is reduced. d. Sulfur is the oxidizing agent. 7. Which of these is not a strong acid? a. hydrochloric acid (HCl) b. hydrobromic acid (HBr) c. sulfuric acid (H2SO4) d. acetic acid (CH3COOH) Atomic Structure (10 marks) 8. The electron configuration for calcium is a. 1s22s22p63s23p64s23d104p65s25p4 b. 1s22s22p63s23p64s2 c. 1s22s22p63s23p64s23d2 d. none of the above 9. Which of the following elements has the HIGHEST first ionization energy? a. N b. As c. P d. Bi 10. Which of the following elements is the LEAST electronegative? a. Cl b. K c. I d. Ge 11. The number of valence electrons for the selenium atom is a. 34 b. 16 c. 4 d. 6 Midterm Practice Examination Answer Key 3 of 28 12. Which atom has the smallest atomic radius? a. Mg b. Al c. Si d. S 13. What is the highest principal quantum number (n), according to the quantum mechanical model? a. 2 b. 7 c. 4 d. 1 14. How many electrons can be accommodated in the third principle energy level? a. 2 b. 8 c. 18 d. 34 15. Write the complete electronic configuration for the Zn2+ ion. a. 1s22s22p63s23p64s03d10 b. 1s22s22p63s23p64s23d10 c. 1s22s22p63s23p64s23d8 d. [Ar]4s03d10 16. The quantum mechanical model of the atom a. defines the exact path of an electron around the nucleus b. was proposed by Neils Bohr c. defines the propability of finding an electron in a certain position d. states that electrons can be found in circular orbitals around the nucleus 17. Stable electron configurations are likely to contain a. filled energy sublevels b. unfilled s-orbitals c. electrons with a clockwise spin d. filled d sublevels 4 of 28 Grade 12 Chemistry Name: ___________________________________________ Kinetics (10 marks) 18. Which of these is the reason that a reaction will speed up when there is an increase in temperature? a. Chemical bonds are more likely to break. b. Collisions between reactant molecules are more accurate. c. There are more collisions with greater energy. d. The activation energy increases as temperature increases. 19. Which expression represents a reaction rate? time mass energy time a. mass time mass energy time mass energy time b. mass time mass energy time mass energy time c. mass time mass energy time mass energy time d. mass time mass energy 20. The rate of a chemical reaction usually a. increases as reactant concentration increases b. decreases as reactant concentration increases c. decreases as temperature increases d. is slowed down by a catalyst 21. If a catalyst is used in a reaction, a. the activation energy will increase b. the reaction rate increases c. different products will be made d. the reaction rate decreases 22. Assuming it occurs in a single step, what is the rate law for the following reaction? A + 2B → C + D a. Rate = K[A][B] b. Rate = K[A]2[B] c. Rate = K[A][B]2 d. Rate = K[A][B]½ Midterm Practice Examination Answer Key 5 of 28 23. Given a first order reaction where the concentration of the reactants is doubled, which of the following is true? a. The rate does not change. b. The rate doubles. c. The rate quadruples. d. The rate decreases. 24. An elementary reaction a. has only elements as reactants b. has one single step c. has only elements as products d. never needs a catalyst 25. What information is not given by an overall balanced chemical equation? a. the reaction mechanism b. the number of atoms participating in the reaction c. the probable order of the reaction d. the relative number of molecules used in the reaction 26. Given the following reaction and assuming a single step, 2 SO2(g) + O2(g) → 2 SO3(g) ΔH = –91 kcal, if the volume of the enclosing vessel is halved, the reaction rate will ______________. a. double b. quadruple c. increase eight-fold d. decrease by half 27. For the rate law expression, rate = k[A]2[B][C]2, the reaction is __________ order overall. a. second b. third c. fifth d. seventh 6 of 28 Grade 12 Chemistry Name: ___________________________________________ Part B: Fill-in-the-Blank (23 marks total) Use the answer sheet found at the end of this examination to answer the fill-in-the-blank questions of this section. Write your answer in the space provided that corresponds to the question. DO NOT write your answers directly on the examination. Using a term from the word bank provided below, complete each of the statements that follow. Each blank is worth one mark; therefore, some questions have a total value of two marks. There are MORE terms provided than you need, so read over the list carefully and choose the terms you want to use. 4 increase probability absorbed kinetic product(s) activation energy kinetic energy rate amplitude loss rate law Aufbau Principle mechanism reactant(s) collision theory molecules reaction mechanism concentration motion reaction rate configuration n reducing agent d neutralization reduction decrease nine s dissociate opposite salt dissolution orbital(s) Schrödinger effective order separate effective collision orientation solubility energy level oxidation soluble excited oxidation number solvation f oxidizing agent speed frequency p sublevels gain Pauli Exclusion titration ground peak valence Heisenberg Uncertainty photon(s) water Hund’s Rule precipitation wavelike Midterm Practice Examination Answer Key 7 of 28 Aqueous Reactions (5 marks) 1. A substance is considered ____________ if it will dissolve in a specific solvent. 2. An ____________ in the oxidation number of an atom signifies oxidation, while a ____________ in the oxidation number signifies reduction. 3. A ____________ reaction is one in which the aqueous (dissolved) ions combine to form a solid that is not readily soluble. 4. ____________ is the addition of a known amount of solution to determine the volume (or concentration) of another solution. Atomic Structure (10 marks) 5. The ____________ orbitals are only present in the fourth energy level and up. 6. Energy is ____________ when an electron moves from ground state to excited state. 7. Electron orbitals are areas of high ____________ of finding electrons. 8. Pauli said that two electrons can only occupy the same orbital if they have ____________ spins. 9. The electrons on the highest numbered subshells are the ____________ electrons. 10. The ____________ ____________ states that electrons must be added to the lowest energy state before adding electrons to a higher energy level. 11. The ____________ of a wave is the height of the wave from the origin to the top of the crest. 12. Einstein proposed that light is composed of particles, or quanta, known as ____________. 13. The quantum mechanical model of the atom was proposed by ____________. Kinetics (8 marks) 14. The ____________ of a chemical reaction can be determined from the balanced chemical equation. 15. A reaction mechanism describes the ____________ in which bonds break and atoms rearrange in a chemical reaction. 16. If changing the concentration of a product does not change the rate, it does not appear in the ____________ ____________. 17. In an ____________ ____________, the particles are oriented in a favourable position that allows bonds to break and atoms to rearrange. 18. The difference between the energy at the peak of the activation diagram and the energy of the reactants is called the ____________ ____________. 8 of 28 Grade 12 Chemistry Name: ___________________________________________ Part C: Short Answer (50 marks total) Answer each of the following questions using the space provided. Pay attention to the number of marks that each question is worth, as this may help you decide how much information to provide for full marks. For questions that involve calculations, show your work and check your final answer for the correct number of significant figures as well as the appropriate unit. Aqueous Reactions (25 marks) 1. Give the oxidation number for each atom in Na3AlF6. Show your work. (4 marks) Na = +1; Al = +3; F = –1 (1 mark each) Show your work. (1 mark) 2. Complete the dissociation equation for the following ionic compound. (2 marks) NaF(s) → Na+(aq) + F–(aq) Midterm Practice Examination Answer Key 9 of 28 3. Balance the following redox reaction using the oxidation-number change method. You will earn up to 5 marks for the following steps: QQ 1 mark: assigning correct oxidation numbers QQ 1 mark: showing electron loss QQ 1 mark: showing electron gain QQ 1 mark: assigning correct coefficients QQ 1 mark: simplifying the terms that appear on both sides of the equation Al(s) + MnO2(s) → Al2O3(s) + Mn(s) 4Al(s) + 3MnO2(s) → 2Al2O3(s) + 3Mn(s) 4. Why must oxidation and reduction occur together? (2 marks) Oxidation and reduction must occur together because the number of electrons lost must equal the number of electrons gained. This assures that charge is conserved on both sides of the equation; therefore, an oxidation-reduction reaction, or redox reaction, is a reaction in which electrons are transferred (lost or gained) between reactants. 10 of 28 Grade 12 Chemistry Name: ___________________________________________ 5. If 40.8 mL of 0.106 mol/L sulfuric acid neutralizes 61.8 mL of potassium hydroxide solution, answer the following questions to determine the concentration of the base a. Write the balanced chemical equation for the neutralization reaction. (2 marks) H2SO4(aq) + 2 KOH(aq) → K2SO4(aq) + 2 H2O(l) b. Use the concentration and volume of the known acid or base to calculate the moles of the known substance (acid or base). (2 marks) 0.106 mol H2 SO4 × 0.0408 L = 0.00432 mol H 2 SO4 L c. Use the coefficients from the balanced equation to determine the moles of the unknown substance (acid or base). (2 marks) mol H 2 SO4 mol KOH = coefficient H 2 SO4 coefficient KOH 0.00432mol H 2 SO4 mol KOH = 1 mol H2 SO4 2 mol KOH 0.00864 mol KOH = mol KOH Midterm Practice Examination Answer Key 11 of 28 d. Calculate the required concentration of the base. (2 marks) C= moles 0.00864 mol KOH = = 0.140 mol/L volume 0.0618 L 6. Write the balanced neutralization reaction given the following reactants. (2 marks) 2 HCl + Mg(OH)2 → 2 H2O + MgCl2 7. Use the solubility rules to predict whether a precipitate will form when the following pair of aqueous solutions are mixed. If a precipitate forms, write the balanced net ionic equation for the reaction. (2 marks) Pb(C2H3O2)2(aq) and LiCl(aq) Precipitate will form. Pb2+(aq) + 2 Cl–(aq) → PbCl2(s) 12 of 28 Grade 12 Chemistry Name: ___________________________________________ Atomic Structure (8 marks) 8. Write the electron configuration and noble gas configuration for a chlorine atom. (2 marks) electron configuration (1 mark): 1s22s22p63s23p5 noble gas configuration (1 mark): [Ne] 3s23p5 9. Outline the contributions of Neils Bohr, Werner Heisenberg, and Erwin Schrödinger in relation to our understanding of the quantum mechanical model of the atom. (3 marks) Neils Bohr interpreted the Bohr model of the atom, whereby he proposed that electrons are found in specific circular orbits around the nulceus of an atom. (1 mark) This led to the development of the Heisenberg Uncertainty Principle by Werner Heisenberg, which states that it is impossible to know the exact location of an electron and where it is going at the same time. (1 mark) Erwin Schrödinger used complex math to develop an equation that represents the statistical probability of finding an electron in a particular space in the atom. (1 mark) Midterm Practice Examination Answer Key 13 of 28 10. Write the electronic configurations for the valence electrons of each of the following. (3 marks) a. Mg2+ 2s22p6 b. S2– 3s23p6 c. sodium 3s1 Kinetics (17 marks) 11. For the reaction CH3COCH3 + I2 → CH3COCH2I + HI, the following data was obtained: Experiment Initial [CH3COCH3] Initial [I2] Reaction Rate (mol/L · s) 1 0.100 mol/L 0.100 mol/L 1.16 x 10–7 2 0.0500 mol/L 0.100 mol/L 5.18 x 10–8 3 0.0500 mol/L 0.500 mol/L 5.18 x 10–8 a. Write the rate expression for the reaction. (1 mark) Rate = K[CH3COCH3]1[ I2]0 b. What order is the reaction with respect to each of the reactants? (2 marks) 14 of 28 With respect to CH3COCH3, the order is 1. With respect to I2, the order is 0. Grade 12 Chemistry Name: ___________________________________________ c. What is the overall order of this reaction? (1 mark) Overall order is 1 + 0 = 1 (1st order) d. Calculate the specific rate constant. (2 marks) 1.16 x 10 –7 = k[0.100]1 k = 1.16 x 10 –6 e. What is the reaction rate if the initial concentrations are both 0.045 mol/L? (2 marks) Rate = k[0.045]1 = (1.16 x 10 –6)(0.045) = 5.22 x 10 –8 12. List two ways in which reaction rates can generally be increased. (2 marks) Any two of the following can be listed for 1 mark each: increase the reactant concentration, decrease the volume of the vessel containing gaseous reactants, increase the temperature, decrease the particle size, and add a catalyst. Midterm Practice Examination Answer Key 15 of 28 13. Consider the following reaction mechanism. H2O2 + I– → H2O + IO– H2O2 + IO– → H2O + O2 + I– (slow) ΔH = 45 kJ (fast) ΔH = 35 kJ a. What is (are) the intermediate(s)? (1 mark) IO– b. What is the overall equation? (2 marks) 2 H2O2 → 2 H2O + O2 c. Draw a potential energy diagram for the reaction. (3 marks) 0.5 mark for the “PE” label on the y-axis. 0.5 mark for the “Reaction Pathway” label on the x-axis. 1 mark for the activated complex at 45 kJ. 1 mark showing the activated complex of fast step to be 35 kJ. d. In which step would a catalyst be most useful? (1 mark) 16 of 28 It would be most useful in step 1 (the slowest step). Grade 12 Chemistry 7 6 5 4 3 2 1 20 Ca Calcium 40.1 38 Sr Strontium 87.6 56 Ba Barium 137.3 88 Ra Radium (226) 19 K Potassium 39.1 37 Rb Rubidium 85.5 55 Cs Cesium 132.9 87 Fr Francium (223) Inner Transition Elements 12 Mg Magnesium 24.3 11 Na Sodium 23.0 3 89–103 Actinide Series Actinide Series 4 5 90 Th Thorium 232.0 89 Ac Actinium (227) 105 Db Dubnium (268) 73 Ta Tantalum 180.9 41 Nb Niobium 92.9 23 V Vanadium 50.9 58 Ce Cerium 140.1 (261) Rutherfordium 104 Rf 72 Hf Hafnium 178.5 40 Zr Zirconium 91.2 22 Ti Titanium 47.9 57 La Lanthanum 138.9 57–71 Lanthanide Series 39 Y Yttrium 88.9 21 Sc Scandium 45.0 Lanthanide Series 4 Be Beryllium 9.0 2 3 Li Lithium 6.9 1 H Hydrogen 1.0 Group 1 6 7 25 Mn Manganese 54.9 107 Bh Bohrium (272) 75 Re Rhenium 186.2 91 Pa Protactinium 231.0 92 U Uranium 238.0 60 Nd Praseodymium Neodymium 140.9 144.2 59 Pr 106 Sg Seaborgium (271) 74 W Tungsten 183.8 42 43 Mo Tc Molybdenum Technetium 96.0 (98) 24 Cr Chromium 52.0 Name Atomic Number 93 Np Neptunium (237) 61 Pm Promethium (145) 108 Hs Hassium (270) 76 Os Osmium 190.2 44 Ru Ruthenium 101.1 26 Fe Iron 55.8 8 19 K Potassium 39.1 9 10 78 Pt Platinum 195.1 46 Pd Palladium 106.4 28 Ni Nickel 58.7 79 Au Gold 197.0 47 Ag Silver 107.9 29 Cu Copper 63.5 11 80 Hg Mercury 200.6 48 Cd Cadmium 112.4 30 Zn Zinc 65.4 12 94 Pu Plutonium (244) 62 Sm Samarium 150.4 95 Am Americium (243) 63 Eu Europium 152.0 96 Cm Curium (247) 64 Gd Gadolinium 157.2 97 Bk Berkelium (247) 65 Tb Terbium 158.9 109 110 111 112 Mt Ds Rg Cn Meitnerium Darmstadium Roentgenium Copernicium (276) (281) (280) (285) 77 Ir Iridium 192.2 45 Rh Rhodium 102.9 27 Co Cobalt 58.9 Relative Atomic Mass Symbol 82 Pb Lead 207.2 50 Sn Tin 118.7 32 Ge Germanium 72.6 14 Si Silicon 28.1 6 C Carbon 12.0 14 83 Bi Bismuth 209.0 51 Sb Antimony 121.8 33 As Arsenic 74.9 15 P Phosphorus 31.0 7 N Nitrogen 14.0 15 84 Po Polonium (209) 52 Te Tellurium 127.6 34 Se Selenium 79.0 16 S Sulphur 32.1 8 O Oxygen 16.0 16 98 Cf Californium (251) 66 Dy Dysprosium 162.5 99 Es Einsteinium (252) 67 Ho Holmium 164.9 100 Fm Fermium (257) 68 Er Erbium 167.3 101 Md Mendelevium (258) 69 Tm Thulium 168.9 113 114 115 116 Uut Uuq Uup Uuh Ununtrium Ununquadium Ununpentium Ununhexium (284) (289) (288) (293) 81 Tl Thallium 204.4 49 In Indium 114.8 31 Ga Gallium 69.7 13 Al Aluminum 27.0 5 B Boron 10.8 13 102 No Nobelium (259) 70 Yb Ytterbium 173.0 85 At Astatine (210) 53 I Iodine 126.9 35 Br Bromine 79.9 17 Cl Chlorine 35.5 9 F Fluorine 19.0 17 103 Lr Lawrencium (262) 71 Lu Lutetium 174.9 118 Uuo Ununoctium (294) 86 Rn Radon (222) 54 Xe Xenon 131.3 36 Kr Krpton 83.8 18 Ar Argon 39.9 10 Ne Neon 20.2 2 He Helium 4.0 18 7 6 5 4 3 2 1 Name: ___________________________________________ Periodic Table of Elements Midterm Practice Examination Answer Key 17 of 28 Alphabetical Listing of the Elements and Their Atomic Masses Element Atomic Mass Element Atomic Mass Element Atomic Mass Actinium (227) Gold 197.0 Praseodymium 140.9 Aluminum 27.0 Hafnium 178.5 Promethium (145) Americium (243) Hassium (265) Protactinum (231) Antimony 121.7 Helium 4.0 Radium (226) Argon 39.9 Holmium 164.9 Radon (222) Arsenic 74.9 Hydrogen 1.0 Rhenium 186.2 Astatine (210) Indium 114.8 Rhodium 102.9 Barium 137.3 Iodine 126.9 Rubidium 85.5 Berkelium (247) Irdium 192.2 Ruthenium 101.1 Beryllium 9.0 Iron 55.8 Rutherfordium (261) Bismuth 209.0 Krypton 83.8 Samarium 150.4 Bohrium (264) Lanthanum 138.9 Scandium 45.0 Boron 10.8 Lawrencium (257) Seaborgium (263) Bromine 79.9 Lead 207.2 Selenium 79.0 Cadmium 112.4 Lithium 6.9 Silicon 28.1 Calcium 40.1 Lutetium 175.0 Silver 107.9 Californium (251) Magnesium 24.3 Sodium 23.0 Carbon 12.0 Manganese 54.9 Strontium 87.6 Cerium 140.1 Meitnerium (266) Sulfur 32.1 Cesium 132.9 Mendelevium (256) Tantalum 180.9 Chlorine 35.5 Mercury 200.6 Technetium (98) Chromium 52.0 Molybdenum 95.9 Tellurium 127.6 Cobalt 58.9 Neodymium 144.2 Terbium 158.9 Copernicium (277) Neon 20.2 Thallium 204.4 Copper 63.5 Neptunium (237) Thorium 232.0 Curium (247) Nickel 58.7 Thulium 168.9 Dubnium (262) Niobium 92.9 Tin 118.7 Dysprosium 162.5 Nitrogen 14.0 Titanium 47.9 Einstienium (254) Nobelium (259) Tungsten 183.8 Erbium 167.3 Osmium 190.2 Uranium 238.0 Europium 152.0 Oxygen 16.0 Vanadium 50.9 Fermium (257) Palladium 106.4 Xenon 131.3 Fluorine 19.0 Phosphorus 31.0 Ytterbium 173.0 Francium (223) Platinum 195.1 Yttrium 88.9 Gadolinium 157.2 Plutonium (244) Zinc 65.4 Gallium 69.7 Polonium (209) Zirconium 91.2 Germanium 72.6 Potassium 39.1 18 of 28 Grade 12 Chemistry 7 6 5 4 3 2 1 2 20 Ca 1.04 38 Sr 0.99 56 Ba 0.97 88 Ra 0.97 19 K 0.91 37 Rb 0.89 55 Cs 0.86 87 Fr 0.86 Inner Transition Elements 12 Mg 1.23 11 Na 1.01 3 89–103 Actinide Series 57–71 Lanthanide Series 39 Y 1.11 21 Sc 1.20 Actinide Series Lanthanide Series 4 Be 1.47 4 5 6 7 8 9 10 11 12 13 58 Ce 1.08 90 Th 1.11 89 Ac 1.00 105 Db — 73 Ta 1.33 41 Nb 1.23 23 V 1.45 57 La 1.08 104 Rf — 72 Hf 1.23 40 Zr 1.22 22 Ti 1.32 91 Pa 1.14 59 Pr 1.07 106 Sg — 74 W 1.40 42 Mo 1.30 24 Cr 1.56 92 U 1.30 60 Nd 1.07 107 Bh — 75 Re 1.46 43 Tc 1.36 25 Mn 1.60 93 Np 1.29 61 Pm 1.07 108 Hs — 76 Os 1.52 44 Ru 1.42 26 Fe 1.64 94 Pu 1.25 62 Sm 1.07 109 Mt — 77 Ir 1.55 45 Rh 1.45 27 Co 1.70 95 Am — 63 Eu 1.01 110 Ds — 78 Pt 1.44 46 Pd 1.35 28 Ni 1.75 96 Cm — 64 Gd 1.11 111 Rg — 79 Au 1.42 47 Ag 1.42 29 Cu 1.75 97 Bk — 65 Tb 1.10 112 Cn — 80 Hg 1.44 48 Cd 1.46 30 Zn 1.66 98 Cf — 66 Dy 1.10 113 Uut — 81 Tl 1.44 49 In 1.49 31 Ga 1.82 13 Al 1.47 5 B 2.01 14 99 Es — 67 Ho 1.10 114 Uuq — 82 Pb 1.55 50 Sn 1.72 32 Ge 2.02 14 Si 1.74 6 C 2.50 15 100 Fm — 68 Er 1.11 115 Uup — 83 Bi 1.67 51 Sb 1.82 33 As 2.20 15 P 2.06 7 N 3.07 16 101 Md — 69 Tm 1.11 116 Uuh — 84 Po 1.76 52 Te 2.01 34 Se 2.48 16 S 2.44 8 O 3.50 17 102 No — 70 Yb 1.06 85 At 1.90 53 I 2.21 35 Br 2.74 17 Cl 2.83 9 F 4.10 103 Lr — 71 Lu 1.14 118 Uuo — 86 Rn — 54 Xe — 36 Kr — 18 Ar — 10 Ne — 2 He — 1 H 2.20 3 Li 0.97 18 Group 1 7 6 5 4 3 2 1 Name: ___________________________________________ Table of Electronegativities Midterm Practice Examination Answer Key 19 of 28 Relative Strengths of Acids Table Acid Reaction Ka Perchloric acid HClO4 + H2O → H3O+ + ClO4– very large Hydriodic acid Hl + H2O → H3O + I very large Hydrobromic acid HBr + H2O → H3O+ + Br – very large Hydrochloric acid HCl + H2O → H3O+ + Cl– very large + – HNO3 + H2O → H3O+ + NO3– Nitric acid H2SO4 + H2O → H3O + HSO4 Sulfuric acid + very large H2C2O4 + H2O → H3O + HC2O4 Oxalic acid very large – + – 5.4 x 10–2 Sulfurous acid H2SO3 + H2O → H3O+ + HSO3– 1.7 x 10–2 Hydrogen sulfate ion HSO4– + H2O → H3O+ + SO42– 1.3 x 10–2 H3PO4 + H2O → H3O+ + H2PO4– 7.1 x 10–3 Fe(H2O)63+ + H2O → H3O+ + Fe(H2O)5(OH)2+ 6.0 x 10–3 H2Te + H2O → H3O+ + HTe– 2.3 x 10–3 HF + H2O → H3O+ + F– 6.7 x 10–4 Nitrous acid HNO2 + H2O → H3O+ + NO2– 5.1 x 10–4 Hydrogen selenide H2Se + H2O → H3O+ + HSe– 1.7 x 10–4 Chromic ion Cr(H2O)63+ + H2O → H3O+ + Cr(H2O)5(OH)2+ 1.5 x 10–4 Benzoic acid C6H5COOH + H2O → H3O+ + C6H5COO– 6.6 x 10–5 HC2O4– + H2O → H3O+ + C2O42– 5.4 x 10–5 HC2H3O2 + H2O → H3O+ + C2H3O2– 1.8 x 10–5 Aluminum ion Al(H2O)63+ + H2O → H3O+ + Al(H2O)5(OH)2+ 1.4 x 10–5 Carbonic acid H2CO3 + H2O → H3O+ + HCO3– 4.4 x 10–7 H2S + H2O → H3O+ + HS– 1.0 x 10–7 H2PO4– + H2O → H3O+ + HPO42– 6.3 x 10–8 HSO3– + H2O → H3O+ + SO32– 6.2 x 10–8 NH4+ + H2O → H3O+ + NH3 5.7 x 10–10 HCO3– + H2O → H3O+ + CO32– 4.7 x 10–11 HTe– + H2O → H3O+ + Te2– 1.0 x 10–11 H2O2 + H2O → H3O+ + HO2– 2.4 x 10–12 HPO42– + H2O → H3O+ + PO43– 4.4 x 10–13 HS– + H2O → H3O+ + S2– 1.2 x 10–15 H2O + H2O → H3O+ + OH– 1.8 x 10–16 Phosphoric acid Ferric ion Hydrogen telluride Hydrofluoric acid Hydrogen oxalate ion Acetic acid Hydrogen sulfide Dihydrogen phosphate ion Hydrogen sulfite ion Ammonium ion Hydrogen carbonate ion Hydrogen telluride ion Hydrogen peroxide Monohydrogen phosphate Hydrogen sulfide ion Water Hydroxide ion NH3 + H2O → H3O+ + NH2– Ammonia 20 of 28 OH– + H2O → H3O+ + O2– Grade 12 Chemistry < 10–36 very small Name: ___________________________________________ Solubility Chart Negative Ions Positive Ions Solubility essentially all alkali ions (Li+, Na+, K+, Rb+, Cs+) soluble essentially all hydrogen ion H+(aq) soluble essentially all ammonium ion (NH4+) soluble nitrate, NO3– essentially all soluble acetate, CH3COO– essentially all (except Ag+) soluble Ag+, Pb2+, Hg22+, Cu+, Tl+ low solubility all others soluble Ca2+, Sr2+, Ba2+, Pb2+, Ra2+ low solubility all others soluble alkali ions, H+(aq), NH4+, Be2+, Mg2+, Ca2+, Sr2+, Ba2+, Ra2+ soluble all others low solubility alkali ions, H+(aq), NH4+, Sr2+, Ba2+, Ra2+, Tl+ soluble all others low solubility alkali ions, H+(aq), NH4+ soluble all others low solubility Ba2+, Sr2+, Pb2+, Ag+ low solubility all others soluble chloride, Cl– bromide, Br– iodide, I– sulfate, SO42– sulfide, S 2– hydroxide, OH – phosphate, PO43– carbonate, CO32– sulfite, SO32– chromate, CrO42– Midterm Practice Examination Answer Key 21 of 28 Table of Standard Reduction Potentials with Values Oxidized species ↔ Reduced Species E°/V Li+(aq) + e– ↔ Li(s) –3.04 K+(aq) + e– ↔ K(s) –2.93 Ca2+(aq) + 2e– ↔ Ca(s) –2.87 Na+(aq) + e– ↔ Na(s) –2.71 Mg2+(aq) + 2e– ↔ Mg(s) –2.37 Al3+(aq) + 3e– ↔ Al(s) –1.66 Mn2+(aq) + 2e– ↔ Mn(s) –1.19 H2O(l) + e– ↔ ½H2(g) + OH–(aq) –0.83 Zn2+(aq) + 2e– ↔ Zn(s) –0.76 Fe2+(aq) + 2e– ↔ Fe(s) –0.45 Ni2+(aq) + 2e– ↔ Ni(s) –0.26 Sn2+(aq) + 2e– ↔ Sn(s) –0.14 Pb2+(aq) + 2e– ↔ Pb(s) –0.13 H+(aq) + e– ↔ ½H2(g) 0.00 Cu2+(aq) + e– ↔ Cu+(aq) +0.15 SO42–(aq) + 4 H+(aq) + 2e– ↔ H2SO3(aq) + H2O(l) +0.17 Cu2+(aq) + 2e– ↔ Cu(s) +0.34 2OH–(aq) +0.40 Cu(s) +0.52 ½O2(g) + H2O(l) + 2e– Cu+(aq) + e– 22 of 28 ½I2(s) + e– ↔ I–(aq) +0.54 Fe3+(aq) + e– ↔ Fe2+(aq) +0.77 Ag+(aq) + e– ↔ Ag(s) +0.80 ½Br2(l) + e– ↔ Br – (aq) +1.07 ½O2(g) + 2H+(aq) + 2e– ↔ H2O(l) +1.23 Cr2O72–(aq) + 14H+(aq) + 6e– ↔ 2Cr3+(aq) + 7H2O(l) +1.33 ½Cl2(g) + e– ↔ Cl– (aq) +1.36 MnO4–(aq) + 8H+(aq) + 5e– ↔ Mn2+(aq)+ 4H2O(l) +1.51 ½F2(g) + e– ↔ F– (aq) +2.87 Grade 12 Chemistry Name: ___________________________________________ Names, Formulas, and Charges of Common Ions Positive Ions (Cations) Name Symbol Name Symbol aluminum Al3+ magnesium Mg2+ ammonium NH4+ manganese(II) Mn2+ barium Ba2+ manganese(IV) Mn4+ cadmium Cd2+ mercury(I) Hg22+ calcium Ca2+ mercury(II) Hg2+ chromium(II) Cr2+ nickel(II) Ni2+ chromium(III) Cr3+ nickel(III) Ni3+ copper(I) Cu+ potassium K+ copper(II) Cu2+ silver Ag+ hydrogen H+ sodium Na+ iron(II) Fe2+ strontium Sr2+ iron(III) Fe3+ tin(II) Sn2+ lead(II) Pb2+ tin(IV) Sn4+ lead(IV) Pb4+ zinc Zn2+ lithium Li+ continued Midterm Practice Examination Answer Key 23 of 28 Names, Formulas, and Charges of Common Ions (continued) Negative Ions (Anions) Name Symbol acetate C2H3O2—(CH3COO—) nitrate NO3— azide N3 — nitride N3— bromide Br— nitrite NO2— bromate BrO3— oxalate C2O42— carbonate CO32— hydrogen oxalate HC2O4— hydride H— oxide O2— hydrogen carbonate or bicarbonate HCO3— perchlorate ClO4— chlorate ClO3— permanganate MnO4— chloride Cl— phosphate PO43— chlorite ClO2— monohydrogen phosphate HPO42— chromate CrO42— dihydrogen phosphate H2PO4— citrate C6H5O73— silicate SiO32— cyanide CN— sulfate SO42— dichromate Cr2O72— hydrogen sulfate HSO4— fluoride F— sulfide S2— hydroxide OH— hydrogen sulfide HS— hypochlorite ClO— sulfite SO32— iodide I— hydrogen sulfite HSO3— iodate IO3— thiocyanate SCN— 24 of 28 Grade 12 Chemistry Name Symbol Name: ___________________________________________ Common Ions Cations (Positive Ions) 1+ charge 2+ charge 3+ charge NH4+ Ammonium Ba2+ Barium Al3+ Aluminum Cs+ Cesium Be2+ Beryllium Cr3+ Chromium(III) Cu+ Copper(I) Cd2+ Cadmium Co3+ Cobalt(III) Au+ Gold(I) Ca2+ Calcium Ga3+ Gallium H+ Hydrogen Cr2+ Chromium(II) Au3+ Gold(III) Li+ Lithium Co2+ Cobalt(II) Fe3+ Iron(III) K+ Potassium Cu2+ Copper(II) Mn3+ Manganese Rb+ Rubidium Fe2+ Iron(II) Ni3+ Nickel(III) Ag+ Silver Pb2+ Lead(II) Na+ Sodium Mg2+ Magnesium Mn2+ Manganese(II) Pb4+ Lead(IV) Hg22+ Mercury(I) Mn4+ Manganese(IV) Hg2+ Mercury(II) Sn4+ Tin(IV) Ni2+ Nickel(II) Sr2+ Strontium Sn2+ Tin(II) Zn2+ Zinc 4+ charge (continued) Midterm Practice Examination Answer Key 25 of 28 Common Ions (continued) Anions (Negative Ions) 1— charge 1— charge CH3COO— (C2H3O2—) Acetate (or ethanoate) HS— BrO3— Bromate Br— 2— charge Hydrogen sulfide CO32— Carbonate CrO42— Chromate OH— Hydroxide Cr2O72— Dichromate Bromide IO3— Iodate O2— Oxide ClO3— Chlorate I— Iodide O22— Peroxide Cl— Chloride NO3— Nitrate SO42— Sulfate ClO2— Chlorite NO2— Nitrite S2— Sulfide CN— Cyanide ClO4— Perchlorate SO32— Sulfite F— Fluoride IO4— Periodate S2O32— Thiosulfate H— Hydride MnO4— Permanganate HCO3— Hydrogen carbonate (or bicarbonate) SCN— Thiocynate 3— charge N3— Nitride ClO— Hypochlorite PO43— Phosphate HSO4— Hydrogen sulfate P3— Phosphide PO33— Phosphite 26 of 28 Grade 12 Chemistry Name: ___________________________________________ Midterm Practise Examination Answer Sheet Part A: Multiple Choice (27 marks) For each multiple-choice question, shade in the circle that corresponds to your answer. DO NOT circle your answers directly on the examination. Example: A B C D 1. A B C D 10. A B C D 19. A B C D 2. A B C D 11. A B C D 20. A B C D 3. A B C D 12. A B C D 21. A B C D 4. A B C D 13. A B C D 22. A B C D 5. A B C D 14. A B C D 23. A B C D 6. A B C D 15. A B C D 24. A B C D 7. A B C D 16. A B C D 25. A B C D 8. A B C D 17. A B C D 26. A B C D 9. A B C D 18. A B C D 27. A B C D Part B: Fill-in-the-Blank (23 marks) For each fill-in-the-blank question, write your answer in the space provided that corresponds to the question. DO NOT write your answers directly on the examination. Aqueous Reactions (5 marks) 1. soluble 2. increase decrease 3. precipitation 4. titration continued Midterm Practice Examination Answer Key 27 of 28 Atomic Structure (10 marks) 5. f 6. absorbed 7. probability 8. opposite 9. valence 10. Aufbau Principle 11. amplitude 12. photons 13. Schrödinger Kinetics (8 marks) 14. rate 15. order 16. rate law 17. effective collision 18. activation energy 28 of 28 Grade 12 Chemistry