Study your notes. quizzes, unit tests, assignments and labs. There will be no surprises on this exam. Breakdown: multiple choice, short answer, problem solving), lab based extended response. Be able to complete the Self Quiz questions at the end of each chapter, as well as the review questions. Answers to numerical problems are at the back of the text book. — UnitS: Gases and Atmospheric Chemistry (what ever gets covered) • States of matter and molecular motion • Gas Laws understand role of temperature, pressure and volume on gases. • • • Solutions and Soiubility solute, solvent, solutions: know about polar and non-polar solutes Solution concentration (v/v. w!v, wM. ppm) FOCUS ON MOLAR CONCENTRATION (CnN) Solution preparation o From a solid (c=mass salute I volume solution, or c=nlv) o Dilution 2 =c 1 (c ) v Soiubility know how to use the table to predict if a precipitate wit form Quantitative analysis of a solution Acid and bases o pH and (H] calculations o Titration Unit 4: • • • - Quantities In Chemical Reactions Relative atomic mass and Isotopic abundance Mole and molar mass Percentage composition Empirical and Molecular formulas (and how to calculate them) Quantitative vs. Qualitative analysis Balancing Chemical Equations Calculating the mass of reactants and products Umiting and Excess reagents Percentage Yield Unit 3: • • • • • • • • • Unit 2: Chemical Reactions • Types of chemical reactions o synthesIs, decomposition, single displacement, double displacement, combustion o balancing equations o writing word equations from chemical formulas and vice versa o predict products of reactions (be able to use activity series and solubility table) Unit 1: Matter and Chemical Bonding • Penodic table o Trends (atomic & Ionic radius, Ionization energy, electronegailvity, electron affinity) • Models of an atom • Isotopes • Types of bonding (ionic vs. covalent) and Intermolecular forces (London dispersion, hydrogen bonding. dipoie.dipole)l • Electronegativity, polar bonds and polar molecules • Nomenclature (naming compounds) o Ionic— monovalent and multivalent metals, polyatomic ions o Molecular o Acids and bases o Hydrates > SCH 3U Exam Review 0 2nd (eV) 47.286 15.035 40.962 3rd (eV) 71.64 80.143 63.45 Classical name IUPAC name 10. Predict the products arid write a balanced chemical equation for the lbllowing chemical reaction: Copper wire is added to an aqueous solution of silver nitrate to recover the silver. 9. Predict the products for the following chemical reaction: A sulfuric acid spill is neutralized by a sodium hydroxide solution. 8. Draw Lewis Dot diagrams and structural diagrams for the following molecules: 0,, HCN, SiO,, PCI,, H,O . Which of these molecules are polar? Which of these molecules contain at least one polar 4 and CF covalent bond? 7. Use election dot diagrams to explain why oxygen and fluorine are diatomic elements. 6. Briefly describe how polar covalent bonds omur. (c) Hl) (b)BNOi . 4 q 3 (a) HClO 5. Provide both the classical name and the IIJPAC name for the following acids. a. List the gases Ihat will dissolve by writing down their corresponding numbers. b. List the gases that are polar. c. List the types of intennolecular forms that exist between each type gas. 4. For a science fair project, a student wants to design a simple device for removing certain gases from polluted air. He knows that polar molecules dissolve well in water, so he bubbles polluted air through sjug of water to remove unwanted gases. For his project, the student uses air containing the following gases: l.N) 5.CH) 2.O,) 6.OCl) 3.HF, H) 3 7.C 4. NH 3 8. CH OCH 3 ElementX ElementY Element Z 1st (eV) 5.139 7.646 21.564 3. Examine the following 1st, 2nd, and 3rd ionization energies and state which element is most likely a noble gas. 2. Explain how anions fonn. Explain how cations form. Are metal ions generally larger or smailer than their atom? Are non-metal lana generally larger or smaller than their atom? EXPLAIN. 1. Ust the followig elements In order of inmeasing atomIc radius, electroneqatbaty and Ionization energy. EXPLAIN your reasoning. a. U and Sr c. Na, Ca, Rb b. SandAl d. Ne,Ar,B Additional Review Questions c. 4.6 x 10° molecules of carbon dioxide B. 3.45 x 100 molecules of sodium chloride b. 4.67 g of copper 0 29. Explain the difference between dilute and concentrated solutions. 28. Explain in detail how you would make 1 .OL a 0.5 molIL solution of sodium hydroxide starting from a 6.0 moth stock solution. Describe the equipment you would use. 27. What volume of 4.0 moIIL hydrochloric acid Is required to make 500.0 mL of a 2.3 mollL solution? 26. How many grams of sodium nitrate are needed to make 2.0 L of a 2.5 moIIL solution? 25. A solution of cupric sulphate is used at blood donor clinics to teat donor Hood ibr low iron. Calculate the 4 crystals are dissolved in 1.0 L of water. concentration ofthis solution, in mol/L, if 125 g of QiSO 24 Anunonium nitrate is produced when ammonia is combined with concentrated nitric acid as shown in the following balanced equation: NH 3 + HNO 3 .-* NH NO, 4 In an experiment; 404.2 g of anmonium nitrate is produced when 112.5 gof ammonia and excess nitric acid are combined. Determine the percentage yield of the product. 4 + 202 — CO 23. Consider the following reaction: CH 0 2 2 + 2H How many grams of carbon dioxide will be produced when 15.0 g of CH 4 and 30.0 g of02 are available for reaction? . . 41. A toy balloon filled with air has an internal pressure of 1.25 aIm and a volume of 2.50 L. If I take the balloon to the bottom of the ocean where the pressure is 95 atmospheres, what will the new volume of the balloon be? How many moles of gas does the balloon hold? (Assume T = 285 K) 40. WI initially have a gas with a pressure of 84 kPa and a temperature of 35°C and I heat it an additional 230 degrees, what will the new pressure be? Assume the volume of the container is constant. 39. A3.5 L balloon released on the ground at25 C rises to an altitude of5O 000 km above the ground. At this new altitude the volume has changed to 2.45 L. What is the temperature at this altitude? 38. What is a titration? What equipment do you need to perform a titration? 21. A compound was found to contain 33.0% Si and 67.0% F, by mass. If the molar mass ofthe compound is 170.0 g/mol, calculate its molecular formula. PO + 3Zn(NO —* 2 3 2Li Consider the following balanced equation: 4 3 (PQt) + 6LINO 3 Zn Determine the mass of lithium nitrate that will be produced when 415.0 g of zinc nitrate is combined with excess lithium phosphate. 37. A student has accidentally spilled 100.0 mL of 3.0 mol/L nitric acid onto the lab bench. What mass of sodium bicarbonate would the teacher need to sprinkle on this spill to neutralize and clean it up? 1 (, + NaHC0, 3 HNO ) 1 1 -÷ C0 + 1120(I) + NaNO 36. Coffee has a pH of 5.0 and grapefruit juice has a pH of 3.0. Calculate the hydrogen ion concentration for both drinks and determine how many times morn concentrated the hydrogen ion is in the juice compared to the coffee. 35. Calculate the pH of seawater which has a hydrogen ion concentration of I x l0 molIL. 34. Calculate the pH of vinegar which has a hydrogen ion concentration of lx 102 molIL. 33. Students in a chemistry lab are making the compound cobalt(ll) carbonate. It can be made by reacting sodium carbonate solution with cobalt(ll) chloride solution. Calculate the volume of 1.0 molfL cobalt(ll) chloride solution required to completely react with 250 mL of 1.5 m&L sodium carbonate. 32. A chemist mixes aqueous potassiwn iodide with lead(U) acetate to produce a bright yellow precipitate for her chemistry magic show. Write the net ionic equation fbr this reaction. For this reaction, write (a) a balanced chemical equation (b) a total ionic equation (c) a net ionic equation 31. Consider the following reaction aqueous nickel(ll) nitrate reacts with aqueous sodium sulphite, 30. Differentiate between the terms saturated, taisaturated, and supersaturated. 20. ‘.Vhat is the empirical fonnula of a compound whose percentage composition is found to be 2.20% hydrogen, 26.7% cabon, and 71.I%oxygen? 19. Magnesium hydroxide, MOH) , can be commonly found in antacids. Calculate the percentage 2 composition, by mass, of each element in magnesium hydroxide. . 3 18. Calculate the number of molecules found in 425.0 g of SiF 17. How many atoms carbon are present in 3.53g of butane, ? 15 H 4 C 16. How many grams are there in a. 1.5 x io moles of lead? a. 5.25g ofsodium carbonate 15. How many MOLES are present in 14. What are isotopes? How many protons, neutrons and electrons exist in uranium-235 and in barium-I 14? 13. What are the products ofthe reaction between butane, C Hlg), and oxygen? Write a balanced chemical 4 equation lbr this reaction. 12. Predict the products aid write a balanced chemical equation for the fbllowing chemical reaction: Steel wool is burned in a hot flame to produce a fireworks-like efibet. 11 Predict the products and write a balanced chemical equation for the fbllowing chemical reaction: Aqueous calcium chloride is added to a small amount of solution suspected to contain sodium phosphate. electroneg: Sr < Li IE: Sr < Li a) atomic radius: U <Sr electroneg: Al < S IE: Al <S b) atomic radius: S <Al c) atomic radius: Na < Ca< Rb electroneg: Rb < Ca < Na lE: Rb< Ca < Na IE: B < noble gases electroneg: Ar and Ne < B d) atomic radius: b) 3,4, 6 - c) 1, 2, 5,7 and 8—London dispersion 13,4 — hydrogen bonding.i 6— dIpole-dipole :-F: + + + 6NaCI) — all the polar molecules as well as CF4. 17. 1.46x1O atoms of Carbon 0 19.41.67% magnesium, 54.87% oxygen, and 3.46°.4, l’drogen. 18.5 c. 7.4 x 10” grams 5 b. 1.19x10 b. 0.073 mol grams 5 16. a. 3.loxl0 15. a. 0.050 mol — 14. Isotopes atoms with same atomic # but different # of neutrons. U-235: #p92, #N = 143. Ba-i 14: #p = 56 #N= 58 + A) NazSO) (,,) —a ) 4 2Na,PO 4 ( 3 Ca . 2 PO O,) 2 3O, —a 2Fe + 13. water and carbon dioxide 12. 4Fe, 11. 3CaCl 2 + , Cu(NO ) (,q) —a 3 3 2AgNO ) 0 2H0H 10. Cut.) — + 9. H SO 2 2NaOlj 8. polar HCN, PCI3, H20. contain at least one polar bond :ö=o: 7. To obtain stable octets, two oxygen atoms will share electrons with one another. Fluorine does the same. The result is explained by the following diagrams. 6. When two nonmetals react with each other, they tzy to form stable octet& To th this, they share electrons. If one atom is much more electronegative than the other, they will not share the electrons equally. Thus, one end of the bond is more negative than the other and the bond is polar. Classical name IUPAC name 5. aqueous hydrogen chlorate (s) HCIO) chioric acid aqueous hydrogen nitrite (b) HNO nitrous acid hydroiodic acid aqueous hydrogen iodide (c) H1 4. a) 3.4,6 and 8 — — 2. anions non-metal gains electrons. Anions are generally larger than their respective atom. Cations metals lose electrons. Catlona are generally smaller than their respective atoms. Discuss nuclear charge and role of electrons repulsion 3. Z 1. Answer Key to Exam Review 2r(.,) — PbI + 2Na + . 38. A lab technique used to determine the precise concentration of a solution. Buret. burnt clamp, Erlenmeyer flask, retort stand and base. Likely also need pipet and bulb, droppers for Indicators, 37. The teacher would sprinkle 25.2 g of baking soda to neutralize the acid spill. 36. The hydrogen ion concentration is lOOx greater in grapefruit juice than it is in coffee. Therefore, grapefruitjuice is lOOx more acidic than coffee. 35. Seawater has a pH of 8.0. 34. The pH of vinegar solution is 2.0. 33. The volume of cobalt(l1) chloride required is 380 mL. + SO —a NiSO + 2NaNO 2 ), + Na 3 (s)Ni(NO 2 + 2NO 2 —a NISON.) 3 (b) )4j 5 + N5(.q) + SO *(.qt + SO 2 (c)Ni (, —a NiSO. 2 3 32. 1 (. 2 Pb ) 31. 30. A saturated solution is one that cannot dissolve any more solute at a specific temperature. An unsaturated solution is one that contains less solute than it can usually hold at a given temperature. A supersaturated solution is one that contains more solute than it can usually hold at a given temperature. 29. Dilute solutions contain very little dissolved solute in the solvent. Concentrated solutions contain a relatively large amount of dissolved solute in the solvent. 28. need 0.0833L of concentrated acid In IL volumetric flask.. Top with water to meniacus. Cap and shake 27.0.288 L 26.425 grams 23. The mass of cabon dioxide produced is 20.6 g 24. The percentage yield is 76.47%. 25. The molar concentration of the solution is 0.78 mauL. 20. HCO 2 6 F 2 21.Si 22. The mass of lithium nitrate that will be produced is 302.1 g.