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Name______________________________Date____________Period________ Final Exam Review Answers June 2009 1. List the rules for naming acids. Oxyacid - – ic from - ate, - ous from – ite Binary Acid – hydro – root – ic from ide 2. Write the formulas for the following acids. chloric acid ____HClO3-1_______________ phosphorous acid ____ H3PO3-3_________ sulfuric acid _____ H2SO4-2________ 3. Name the following acids. HCl ___Hydrochloric Acid______________ H2S ____Hydrosulfuric Acid________________ HNO2 ____Nitrous Acid______________ 4. Define the term isotope. Give an example. Different numbers of neutrons, same atomic number Carbon – 12 Carbon – 14 5. The isotope 70 Zn has how many protons? 30 (70 is the mass number) 30 6. Write the correct oxidation number (charge) for each of the following. sodium ___Na+1____ barium ___Ba+2_____ bromine ___Br-1____ sulfur ___S-2______ aluminum ___Al+3____ nitrogen ___N-3______ nitrate ___NO3-1__ hydroxide ___OH-1______ acetate __C2H3O2-1__ sulfite ___SO3-2_____ 7. In a balanced compound, the charge of the cation plus the charge of the anion should equal zero. 8. Ionic compounds are made up of a __metal__ and a __non-metal____ , and covalent compounds are made up of two __non-metals__. 9. How many atoms are in the compound Pb(CrO4)2 ? 11 (1 + 2 + 8) 10. Lead (II) oxide is obtained by roasting galena, lead (II) sulfide, in air. 2 PbS (s) + 3 O2 (g) 2 PbO (s) + 2 SO2 (g) a. Balance the equation and determine the theoretical yield of PbO if 200.0 g PbS is heated. 200 gPbS 1mol PbS 2 mol PbO 223.3 g PbO = 186.57 g PbO 239.27 g PbS 2 mol PbS 1 mol PbO b. What is the percent yield if 170.0 g PbO is obtained. 170.0 g PbO x 100 = 91.12% 186.57 g PbO 11. Predict whether the following reactions will occur. If yes, finish the reaction by writing the products and balancing the equation. a. ____ Fe + __2_ HCl FeCl2 + H2 b. ____ CuO + ____ Ag NR c. _2__ Al + _3__ H2SO4 Al2(SO4)3 + 3H2 d. ____ MgBr2 + ____ Fe NR 12. Work the following problems. a. Calculate the mass of 3.57 moles of aluminum. (mole to mass) 3.57 mol Al 26.98 g Al = 96.32 g Al 1 mol Al b. How many moles are in 25.0 g of Fe2O3? (mass to mole) 25.0 g Fe2O3 1 mol Fe2O3 = 0.16 mol Fe2O3 159.7 g Fe2O3 c. Calculate the number atoms in 2.50 moles of Zinc. (moles to particles) 2.50 mol Zn 6.02 x 1023 atoms Zn = 1.51 x 1024 atoms Zn 1 mol Zn d. Determine the number of moles for 3.58 x 1023 formula units ZnCl2? (particles to moles) 3.58 x 1023 formula units ZnCl2 1 mol ZnCl2 = 0.59 mol ZnCl2 6.02 x 1023 formula units ZnCl2 13. List 5 properties of bases. (1) Bitter (2) OH(3) Slippery (4) pH 7.1 -- 14 (5) Red Litmus turns Blue add caustic 14. List 5 properties of acids. (1) sour (2) H+ (3) pH 1-6.9 (4) Blue Litmus turns Red (5) Corrosive to metal 15. When an acid reacts with a base, a _salt_ and __water__ form. 16. Show the general equation for a neutralization reaction then give an example of one that doesn’t include hydrochloric acid or sodium hydroxide. Acid + base salt + water Mg(OH)2 + 2HBr MgBr2 + 2H2O CsOH + HBr CsBr + H2O 17. What is the pH and pOH of a solution if the [OH-]= 1.0 x 10-3. Is this an acid, a base, or neutral? pOH = - (log 1.0 + log 10-3) pOH = -(0 + -3) pOH = 3 pH = 11 Basic 18. What is the pH and pOH of a solution if the [H+]= 4.0 x 10-6. Is this an acid, a base, or neutral? pH = -(log 4 + log 10-6) pH = - (.60 + -6) pH = 5.4 pOH = 8.6 Acidic 19. What is the charge on the hydronium ion? H+1 20. Define pH, and explain the pH scale (see page 610). pH is the negative logarithm of the hydrogen ion concentration (percent hydrogen) used to determine acids & bases scale from 1-14 (below 7 = acid, 7 = neutral; above 7= base) 21. Balance the following equations, label the reactants (left of arrow) and products (right of arrow), then name the type of reaction. a. 2NaOH(aq) + CaBr2 (aq) Ca(OH)2(s) + 2NaBr(aq) -- double replacement b. 2C4H10(g) + c. 3Fe(s) + d. H2(g) + 13O2(g) 8CO2(g) 4H2O(l) F2(g) Fe3O4(s) + 10H2O(g) -- combustion + 4H2(g) -- single replacement 2HF(g) -- synthesis 22. Predict the Products for the following reactions – for double replacement reactions be able to identify soluble and insoluble substances using the solubility chart, for single replacement reactions you must use the activity series to identify if the reaction will occur, a. Combustion of C8H18 2C8H18 + 25O2 16 CO2 + 18H2O b. Decomposition of magnesium bromide Mg + Br2 Mg + Br2 c. Synthesis reaction between hydrogen and iodine H2 + I2 2HI d. Single replacement reactions: i. Nickel + magnesium chloride Ni + MgCl2 NR ii. Calcium + copper (II) bromide Ca + CuBr2 CaBr2 + Cu e. Double replacement reaction sodium phosphate + manganese (II) chloride 2Na3PO4 + 3MnCl2 Mn3(PO4)2 (↓) + 6NaCl (aq) 23. List the 7 diatomic elements. Br2 I2 N2 Cl2 H2 O2 F2 24. The calculation of quantities in a chemical reaction is known as __stoichiometry__. 25. List 5 indicators that tell you when a chemical reaction has occurred. (1) heat (temperature change) (2) precipitate (3) color change (4) different odor (5) light 26. Write chemical equations for the following, then balance the equations. a. hydrogen(g) + bromine(g) hydrogen bromide(g) H2 + Br2 2HBr b. potassium chlorate(s) potassium chloride(s) + oxygen(g) 2KClO3 (s) 2KCl (s) + 3O2 (g) c. Bubbling hydrogen sulfide gas through manganese(II) chloride dissolved in water results in the formation of the precipitate manganese(II) sulfide and hydrochloric acid. H2S (g) + MnCl2 (aq) MnS (s) + 2HCl (aq) d. Chloroform (CHCl3), an important solvent, is produced by a reaction between methane and chlorine. Given the following balanced equation, tell how many grams CH4 is needed to produce 50.0 g CHCl3? (stoichiometric mass to mass) CH4(g) + 3Cl2(g) CHCl3(g) + 3HCl(g) 50 gCHCl3 1 mol CHCl3 119.37 g CHCl3 1 mol CH4 1 mol CHCl3 16.043 g CH4 = 6.72 g CH4 1 mol CH4 27. 50°C is equal to ___50 + 273 = 323 Kelvin. 28. When measuring pressure, ____760___ torr = ___1_____ atm = ___760__ mm Hg = 101.3 KPa 29. When the temperature of a gas decreases, what effect does this have on the volume of the gas? Charles’ Law – temperature and volume are directly related, as temp decreases volume decreases 30. A gas at 89°C occupies a volume of 0.67 L. At what Celsius temperature will the volume increases to 1.12L? (Charles’s law) p. 424 V1 = V2 .67 L = 1.12 L T2 = 605.13 K T2 = 605.13 – 273 = 332.13oC T1 T2 362 K T2 31. The pressure of a sample of helium in a 1.00-L container is 0.988 atm. What is the new pressure if the sample is placed in a 2.00-L container? (Boyle’s law) p. 422 V1P1 = V2P2 1.00 L x 0.988 atm = 2.00 L x P2 P2 = .499 atm 32. The air in a dry, sealed 2-L soda bottle has a pressure of 0.998 atm at sealevel at a temperature of 34.0°C. What will be its pressure if it is brought to a higher altitude where the temperature is only 23.0°C? (combined gas law) p.428 P1V1 = P2V2 .998 atm x 2 L = P2 x 2 L P2 = .962 atm T1 T2 307 K 296 K 33. The pressure in an automobile tire is 1.88 atm at 25.0°C. What will be the pressure if the temperature warms up to 37.0°C? (Gay-Lussac’s law) p. 426 P1 = P2 1.88 atm = P2 P2 = 1.96 atm T1 T2 298 K 310 K 34. Determine the density of chlorine gas at 22.0°C and 1.00 atm of pressure. (ideal gas law) p. 434 D = MP RT D = 70.9 g/mol x 1 atm = 2.93 g/L 0.0821 L atm x 295 K mol K 35. What does the ideal gas law allow a scientist to calculate that the other gas laws do not? Number of moles, density and molar mass if pressure, volume and temperature are known 36. Standard temperature and pressure (STP) are equal to ___1atm___ and ___0oC_____. 37. Define coefficient, superscript and subscript. Coefficient: In a chemical equation, the number written in front of the formula; tells the smallest number of particles of the substance involved in the reaction. Superscript: exponent Subscript: identifies the number of atoms of an element in a compound or formula (little number to the right of the atom) 38. What is the molarity of 1.5 L of solution in which 6.0 moles of potassium chloride is dissolved? Molarity = moles = 6.0 mol = 4 mol Liter 1.5 L L 39. List the factors that affect solubility. Size of particles, agitation, temperature & concentration (solubility of gases is affected by pressure and temperature – dissolve more easily at high pressure and /or low temperature) 40. Draw the Lewis dot structure for sodium, calcium, carbon, oxygen and bromine. 41. Convert 8.00 liters of H2O to moles. (volume to mole) 8.00 L 1 mol = .357 mol H2O 22.4 L 42. Where would you look to obtain mole ratios? (multiple choice) D a. the periodic table b. the molar masses c. the polyatomic ion sheet d. a balanced chemical equation 43. Calculate molar mass for the following. a. AlBr3 26.98 + 3(79.90) = 266.68 g/mol b. H2O2 c. H3PO4 2(1.01) + 2(16) = 35.03 g/mol 3(1.01) + 30.97 + 4(16) = 98 g/mol 44. Caffeine, a stimulant found in coffee, has the chemical formula C8H10N4O2. Determine the percent composition of caffeine. 8(12.01)+10(1.01)+4(14.01)+2(16)=194.2 g/mol 96.08 x 100 = 49.47% C 194.2 10.1 x 100 = 5.19% H 194.2 56.04 x 100 = 28.86% N 194.2 32 x 100 = 16.48% O 194.2 45. Compare molecular and empirical formulas. Molecular – actual atom combination within a formula Empirical – lowest whole number ratio of atoms of a formula 46. Determine the molecular formula for ibuprofen, a common headache remedy. Analysis of ibuprofen yields a molar mass of 206 g/mol and a percent composition of 75.7% C, 8.80% H an d15.5% O. (find the empirical formula first) 75.7 g C = 6.3 ÷ .96 = 6.56 x 2 = 13 12.01 8.80 g H = 8.71 ÷ .96 = 9.07 = 9 x 2 = 18 1.01 Empirical Formula C13H18O2 15.5 g O = .96 ÷ .96 = 1 x 2 = 2 16 molar mass of Empirical Formula = 206.31 g/mol n = 206 g/mol = .998 = 1 206.31 g/mol 1 (C13H18O2) = C13H18O2 47. Which group of elements on the periodic table is most likely to donate one electron? Alkali Metals (group 1) 48. Which other elements on the periodic table are most similar to chlorine in their bonding characteristics? All group 17 nonmetals 49. What is the value of Avogadro’s number? 6.02 x 1023 50. What are the rules for multiplying and dividing with significant figures? Multiply and dividing significant figures – keep smallest value of all factors 51. Define: a. Hydrate: a compound that has a specific number of water molecules bound at its atoms b. Precipitate: a solid produced during a chemical reaction in a solution c. Reactant: the starting substance in a chemical reaction d. Product: a substance produced during a chemical reaction 52. Use the chemical equation to answer the questions. 2CH4(g) + S8(s) 2CS2(l) + 4H2S(g) a) Calculate the mol CS2 produced when 1.50 mol S8 is used. (stoichiometric mole to mole) 1.5 mol S8 2 mol CS2 1 mol S8 = 3 mol CS2 b) How many grams of sulfur would you need if you had 24.0 grams of methane? (stoichiometric mass to mass) 24 g CH4 1 mol CH4 16.05 g CH4 1 mol S8 2 mol CH4 c) What is the ratio of reactants to products? 2CH4/2CS2 2CH4/4H2S 1S8/2CS2 256.56 g S8 1 mol S8 = 191.82g S8 1S8/4H2S 53. How many atoms (molecules), how much volume and how many grams does one mole of chlorine gas have? 1 mol Cl2 = 22.4 Liters 1 mol Cl2 = 6.02 x 1023 molecules 1 mol Cl2 = 70.90 grams 54. State the Law of Conservation of Mass. States that mass is neither created nor destroyed in any process but is conserved 55. Compare covalent and ionic bonding. Covalent: results from the sharing of valence electrons; between 2 non-metals Ionic: electrostatic force that holds oppositely charged particles together in an ionic compound, formed between metal and non-metal, transfer of electrons 56. What is the difference between physical and nuclear chemistry? Physical Chemistry – studies the behavior and changes of matter and the related energy changes (deals with how substances bond) Nuclear Chemistry – involves the nucleus, structure of the atomic nuclei and the changes they undergo 57. Compare fission and fusion. (define and identify uses) Fission: the splitting of a nucleus into fragments Fusion: the combining of atomic nuclei 58. Compare alpha, beta and gamma particles. Alpha: a particle with twp protons and two neutrons, with a 2+ charge; is equivalent to a helium -4 nucleus, can be represented by x, and is emitted during radioactive decay. Beta: a high-speed electron with a 1- charge that is emitted during radioactive decay. Gamma: high energy radiation that has no electrical charge and no mass, is not deflected by electric or magnetic fields, usually accompanies alpha and beta radiation, accounts for most energy lost during radioactive decay 59. Define radioactivity. The process in which some substances spontaneously emit radiation. 60. How much of a 100.0 g sample of 198Au is left after 8.10 days if its half-life is 2.70 days? Sample Size Time # of ½ lives 100 gram 0 days 0 – ½ lives 50 gram 2.7 days 1 – ½ lives 25 gram 5.4 days 2 – ½ lives 12.5 gram 8.1 days 3 – ½ lives Answer – 12. 5 grams 61. Describe a saturated, unsaturated, and supersaturated solution. a. Saturated: Contains the maximum amount of dissolved solute for a given amount of solvent at a specific temperature and pressure b. Unsaturated: contains lee dissolved solute for a given temperature and pressure than a saturated solution; has further capacity to hold more solute c. Supersaturated: contains more dissolved solute than a saturated solution at the same temperature Use the following graph to answer the questions below. 62. What are the solubilities of the following solutes at 60oCelcius? a. KI -- 230 g/100 cm3 water b. NaNO3 -- 123 g/100 cm3 water c. KClO3 -- 27 g/100 cm3 water 63. What type of solution is prepared when 160 g of KI is added to 100 grams of water at 15oC? supersaturated 64. Which substance is most soluble at 45oC? KI 65. Which substance is least soluble at 30oC? KClO3 Know all conversion factors used in mole calculations.