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Unit #1 Matter, Chemical Trends, And Chemical Bonding (p8- 105) Significant Figures The Structure of the Atom (atomic mass, atomic number, #p, #e, #n) Isotopes, Radioisotopes, Half-life The Periodic Table Periodic Table Trends (electronegativity, ionization energy, atomic radius, reactivity, electron affinity) Ionic and Molecular Compound Physical Properties Lewis Dot Diagrams (electron dot diagrams)and Structure Formulas Ionic and Covalent Bonding Polarity of Bonds and Polar Molecules Intermolecular Bonds (Dipole-dipole, VanderWaals, LDF, Hydrogen Bonding) The Names and Formulas of all Compounds Practice: 1. How many significant digits are in a) 200 152 ......... 1.0040 x 106 ........... 0.0048 ............ 7.0 ......... 2. 18.987 g / 3.06 = ............................... ............... which has ................. significant digits 3. What is an example of a physical property of matter 4. What is an example of a chemical property of matter 5. What is an example of a physical change 6. What is an example of a chemical change 7. What is an example of a quantitative property of matter 8. If a mixture has only one phase it is said to be .............................................. 2 phases ? .................................................. 9. Isotopes of the elements contain different numbers of ..........................but the same # of ............................. & ........................... 10. An alpha particle contains ..................... protons & ................ neutrons and weighs ................, symbol = ................... 11. When an isotope emits a beta particle the atomic# of the substance ..............................& the at mass .............................. 12. The isotope cobalt-60 ( 6027Co ) has .................... protons & ............. neutrons in its nucleus with ............... electrons around it 13. The isotopic ion 5625Mn 2+ has............ protons & .............. neutrons in its nucleus with .................... electrons around it. 14.Fill in the following table Chemical Formula Name of substance Identify the Type of Molecule HNO3(aq) Aqueous Ammonium hydroxide N2H4 Iron(III) sulphide Copper(II)chromate pentahydrate 15. Complete the table below. Element name fluorine Element symbol Atomic number Group number Family name Period number noble gas 3 Metal or nonmetal Ba 16. Use electron dot diagrams to explain the formula for Mg3P2. 17. Draw the Lewis diagram for carbon dioxide, water and methane, nitrogen triiodide, and oxygen gas. Include dipoles, type of bonding ( intermolecular and intramolecular), and whether the molecule is polar or nonpolar. 18. List all families on the periodic table and state two properties of each. 19. Explain all periodic trends, state the trend for periods and groups. 4. Unit #2 Chemical Reactions (p106- 153) Conservation of Mass Write Word Equations, and Balanced Chemical Equations with States. Types of Reactions (synthesis, decomposition, single and double displacement, incomplete and complete combustion) Reactivity Series for single displacement reactions Solubilty Chart for double displacement reactions Neutralization Reactions Chemical Reactions for the formation of acids and bases from metal oxides and non-metal oxides Practice: 1. Predict the products and write a balanced chemical equation for the following chemical reaction: Hydrochloric acid is neutralized by an aluminum hydroxide suspension. 2. Predict the products and write a balanced chemical equation for the following chemical reaction. Charcoal (pure carbon) is burned in a barbecue. 3. Complete the following chemical reaction equation, including states of matter and balancing: FeCl3(aq) + Zn(s) 4. Balance: a) Cu + O2 CuO b) P4 + H2 PH3 c) Al + CuSO4 Al2(SO4)3 + Cu d) H2SO4 + Al Al2(SO4)3 + H2 e) Na + H2O NaOH + H2 f) NH3 + O2 NO2 + H2O g) Na2CO3 + H3PO4 Na3PO4 + H2O + CO2 h) FeS + O2 Fe2O3 + SO2 i) Na2CO3 + FeCl3 + H2O Fe(OH)3 + NaCl + CO2 5. Identify the type the reaction, complete & balance the following reaction equations. Include states a) A chunk of sodium is dropped into a cup of water. b) Some butane is burned in excess oxygen. c) Some butane is burned in limited oxygen. d) A solution of ammonium phosphate is added to a solution of copper(II) sulfate. e) A hydrated salt, magnesium sulfate heptahydrate, is heated vigorously over a burner. f) A solution of platinum(III) nitrate is stirred with a zinc-plated spoon. g) A piece of magnesium is left overnight in a solution of acetic acid h) H3PO3 (aq)+ NH4OH (aq)→ i) CaCO3 (aq) + H3PO4 (aq)→ j) Cu (s) + H2O (l)→ kj) Al (s) + Cu(NO3)2 (aq)→ Unit #3 Quantities in Chemical Reactions (p158- 259) Isotopic Abundance Calculations Law of Definite Proportions The Mole (Avogadro’s Number) Molar Mass Calculations Calculation of particles (molecules, atoms) Mole to Mass Calculations Percentage Composition Empirical and Molecular Formulas Stoichiometry (mass to mass calculations) Limiting and Excess Reactants % Yield Practice: 1. Convert 10.0 g of copper to mol. 2. How many mol is 24.7 g of aluminum? 3. 42.8 g of oxygen gas is how many mol of oxygen gas? 4. Convert 4.62 mol of zinc hydroxide to grams. 5. How many grams is 8.32 mol of calcium phosphate? 6. Determine the number of molecules found in 5.00 mol of water. 7. Determine the number of hydrogen atoms found in 2.50 mol of methane, CH4. 8. Determine the number of atoms in 0.25 mol of sodium. 9. Consider the following balanced equation: Ca(OH)2 + 2HCl CaCl2 + 2H2O Determine the number of moles of calcium chloride produced when 8.0 mol of HCl is combined with excess Ca(OH)2. 10. What mass of FeCO3 is required to form 28.6 g of Fe2O3 ? Balanced equation: 4FeCO3 + O2 2Fe2O3 + 4CO2 11. If 17.5 g of C is dissolved in water and added to a solution containing 39.5 g of SO2, the reaction occurs: 5C + 2SO2 CS2 + 4CO i) Determine the limiting reactant. ii) Determine the mass of CO produced. 12. a) Balance the following equation: KO2(s) + CO2(g) K2CO3(s) + O2(aq) b) If 1.50 g of KO2 was present in the reacting mixture, with excess CO2, calculate the theoretical yield of K2CO3. c) Determine the percentage yield of 1.2 g of K2CO3. 13. Magnesium hydroxide, Mg(OH)2, can be commonly found in antacids. Calculate the percentage composition, by mass, of each element in magnesium hydroxide. 14. What is the empirical formula of a compound whose percentage composition is found to be 2.20% hydrogen, 26.7% carbon, and 71.1% oxygen? 15. Analysis of an air pollutant reveals that the compound is 30.4% nitrogen and 69.6% oxygen. The molar mass of this compound is 92.0 g/mol. What is the molecular formula of this compound? (N2O4) Unit #4 Solutions and Solubility (p264- 411) Solution Terminology (solute, solvent, homogeneous, heterogeneous, electrolytes) Water as a Universal solvent Dissolving (likes dissolve likes) Solution Concentration (%w/w, 5v/v, 5w/v, ppm, molar concentration) Water Treatment Solution preparation (from a solid) Dilution Problems(ccvc = cDvD) Solubility curves (unsaturated, saturated, supersaturated) Reactions in Solutions (Complete and net ionic equations) Qualitative Chemical Analysis(flame test, conductivity, colour of solution, sequential flowchart(ppt test)) Acids/Bases Properties pH and litmus paper Dilution and pH Strong and Weak Acids Arrhenius, Lowry-Bronsted Definitions Acid-Base Titrations Practice: v 1. Determine the concentration of a solution containing 5.6 g sodium nitrate in 250 mL of water. Express your answer in mol/L. 2. Consider the following reaction: Barium chloride solution is mixed with potassium sulphate solution to produce a precipitate barium sulphate and potassium chloride. For this reaction, write (a) a balanced chemical equation (b) a total ionic equation (c) a net ionic equation 3. a)Describe how you would prepare 100 mL of a 0.5 mol/L solution of sodium chloride. Include your calculation and the procedure. b)In a titration 20.0 mL of 0.10 mol/L sodium hydroxide was neutralized by an average of 9.3 mL of hydrochloric acid. Determine the concentration of the acid. 4. A solution of copper(II) sulphate is used at blood donor clinics to test donor blood for low iron. Calculate the concentration of this solution, in mol/L, if 125 g of CuSO4 crystals are dissolved in 1.0 L of water. 5. What volume of a 17.4 mol/L acetic acid stock solution is required to make 2.0 L of a 1.5 mol/L acetic acid solution? 6. For a chemical analysis, 750 mL of a 0.480 mol/L potassium permanganate solution is to be prepared. Calculate the mass of potassium permanganate crystals that will be dissolved to make this solution. 7. Calculate the pH of vinegar which has a hydrogen ion concentration of 5.2 10–2 mol/L. 8. A swimming pool has a pH of 7.5. Calculate the hydrogen ion concentration in the pool. 9. Draw a flow chart illustrating how you could analyze a solution that may contain Pb2+ and/or Sr2+. 10. Use the Bronsted-Lowry concept to identify the reactants as acids or bases in the following reactions. In your answers, indicate the conjugate acid-base pair a) HSO-4 (aq) + HCO3-(aq) SO42-(aq) + H2CO3(aq) b) HS- (aq) + HCO3-(aq) H2S(aq) + CO32-(aq) c) 11. Complete the following chart Substance Litmus Paper pH Conductivity Acid/Base/Neutral? HCl Ca(OH)2 NH3 CH3COOH KNO3 12. Will ammonia dissolve in water? Will carbon dioxide dissolve in ammonia? Explain. Provide the required diagrams. 13. A sample of well water contains 0.24 ppm of dissolved iron(III) sulfate form the surrounding rocks. What mass of iron(II) sulfate is present in 1.2L of water in the kettle? 12. Unit #5 Gases and Atmospheric Chemistry (p417- 499) Kinetic Molecular Theory Properties of the States Pressure and temperature Conversions Gas Laws (Boyles, Charles, Gay-Lussac, Combined Gas Law, Ideal Gas Law, Dalton’s Law of Partial Pressure) Stoichiometry involving Gases Air Quality Practice: 1. What volume does 2.50 mol of oxygen gas occupy at 3.60 atm and 400C? (38.3 L) 2. What temperature is 4.53 mol of gas that occupies 5.78L at 704 torr? (14.4 K) 3. How many mol of gas will occupy 7.42 L at 373K and 200.4 kPa? (0.479 mol) 4. What is the pressure (in atm) of 2.45 x 10-2 mol of gas that occupies 5.68 mL at -35C? (84.2atm) 5. What is the new volume of 750.0 mL of gas at 700.0 torr when the pressure is changed to 800.0 torr? (656.3 torr) 6. 45 mL of gas at 15C and 790 torr is changed to 23C and 810 torr. What is the new volume? (45 mL) 7. 175 mL of gas at –30.0C and 2.57 atm is changed to standard conditions. What is the new volume? (505 mL) 8. What pressure is needed to change 130 mL of gas at 740 torr to 150 mL? (641 torr) 9. What temperature change is needed to change 1.0 L of gas at 10.0C and 800.0 torr to 0.50 L and 760 torr? (-138C change to bring your final temperature to 134K) 10. A 1.0 L rubber bladder is filled with carbon dioxide gas in a 25C room (Pressure = 745 mm Hg). What volume will the gas occupy when it is taken out into the open air where the temperature is 12C and the pressure is 742 mm Hg? (0.96 L) 11. A balloon containing 425 mL of air escapes from a little boy watching a parade. The temperature is 32C at street level and the pressure is 742 torr. When the balloon stops rising, its volume has become 895 mL although the atmospheric pressure has decreased by only 300.0 torr. What is the temperature at this level? (383 K = 110C) 12. To what temperature must 15 L of oxygen gas at 0.0C be heated at 1.00 atm pressure in order to occupy a volume of 23 L, assuming that the pressure increases by 5.0 mm Hg? (421 K = 148C) 13. Determine the volume of a balloon at SATP assuming that it occupies a volume of 20.0 L at a temperature of 12ºC and a pressure of 135 kPa. 14. What is the pressure reading on a scuba tank if the tank is filled with N2 gas at a partial pressure of 115 atm and O2 gas at a partial pressure of 30 atm? 15. Butane from a lighter undergoes combustion in the following manner: 2C4H10 (g) + 13O2 (g) 8CO2 (g) + 10 H2O (g) What volume of butane was burned to produce 325 mL of CO2 (g)? 16. What amount of oxygen, in moles, is available for a combustion reaction in a volume of 12.5 L at STP? 17. Potassium metal with a total mass of 15.0 g is dropped into a beaker of water. What volume of hydrogen gas will be produced if the temperature is 15ºC and the pressure is 100 kPa? Chemical equation: 2K(s) + 2H 2KOH(aq) + H2 (g) 18. What is the initial pressure of a gas if it occupied a volume of 375 mL, but now occupies a volume of 1.25 L at a pressure of 95.5 kPa. Assume that the temperature remains constant throughout the process. 19. Magnesium was added to hydrochloric acid, HCl, and produced 5.25 L of H2 gas at a temperature of 325 K and a pressure of 100 kPa. What mass of Mg was used in this single displacement reaction?