HONORS CHEMISTRY FINAL REVIEW

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1 Allen; June 2012 HONORS CHEMISTRY FINAL REVIEW THE DETAILS: Please refer to the mid-term review for the information you are required to know from the 1 st and 2 nd marking period. Below you will find review information for the remaining 3 rd and 4 th marking period. ***Please note: THE FINAL IS CUMULATIVE OF THE ENTIRE YEAR!! It counts as 1\9 th of your final grade it is reported as a separate grade on your report card. FORMAT: 70 Multiple Choice worth a total of 70 points. WHAT YOU NEED TO BRING: Scientific Calculator, #2 pencils, and your textbook to return to me!! DURING THE EXAM YOU WILL BE PROVIDED WITH: Periodic Table Ion Tables Electronegativity chart Solubility Rules Metal Activity Series Constants (speed of light, specific heats, etc.) SUGGESTIONS FOR STUDYING: The mid-term material is still on my website. Please review the topics and do the practice test. Which topics gave you trouble? Do you still not understand it? Focus your review on these topics. Be sure that all topics are familiar to you do you still remember periodic trends, covalent bonding, etc? How about oxidation

2 numbers? Review your old notes and handouts this is sound advice for any cumulative test review in any course. Also, use the practice test at the end of this review and on the mid-term review you received back in January!! It is good practice but does not contain all of the topics we have covered. TOPICS FROM THE 3 RD AND 4 TH MARKING PERIODS: Organic Chemistry (reference with Ch ) Please reference organic chemistry packet for information Recognize structural, condensed, and molecular formulas of the continuous-chain hydrocarbons containing up to ten carbons. Distinguish between alkanes, alkenes and alkynes. Distinguish between structural and geometric isomers. Define resonance. Define cyclic, saturated, unsaturated, saturated and aromatic compounds. Recognize and identify a molecule s functional groups (alcohol, ester, carboxylic acid, ether). Draw electron dot structures of hydrocarbons. Write the IUPAC name for an alkane, alkene or alkyne given its structural formula. Draw the structural formula of an alkane, alkene or alkyne given its IUPAC name. Relate differences in physical properties of classes of organic compounds to molecular structure. Predict the products in an esterification reaction Chapter 9: Section Identify the charges of monatomic ions by using the periodic table and name the ions. Define a polyatomic ion and write the names and formulas of the most common polyatomic ion Identify the two common endings for the names of most polyatomic ions Apply the rules for naming and writing formulas for binary ionic compounds Apply the rules for naming and writing formulas for compounds with polyatomic ions Interpret the prefixes in the names of molecular compounds in terms of their chemical formulas Apply the rules for naming and writing formulas for binary molecular compounds Apply the three rules for naming acids Apply the rules in reverse to write formulas of acids Apply the rules for naming bases Chapter 11: Section Describe how to write a word equation Describe how to write a skeleton equation (equation unbalanced) Describe the steps for writing a balances chemical equation Describe the five (including combustion) general types of reactions Predict the products of the five general types of reactions (using a metal activity chart, ion sheet, and solubility rules) Predict the formation of a precipitate in a double replacement reaction Show the state of a chemical species Write a molecular equation, complete ionic, and net ionic equation (and know the difference between these three equations!!). Also, be able to accurately write phases for all species. Chapter 20: Oxidation - Reduction Determine the oxidation number of an atom of any element in a pure substance.

3 Identify the oxidizing agent and reducing agent in a redox reaction. Define oxidation and reduction in terms of the loss, gain, or shift of electrons. Use the oxidation number change method to identify atoms being oxidized or reduced in a redox reaction. Distinguish between redox and non-redox reactions. Break a redox reaction into oxidation and reduction half-reactions. When given an unbalanced redox reaction, use the half-reaction method to balance the equation. Chapter 21: Electrochemistry Describe the nature of electrochemical processes Sketch a voltaic cell, labeling the cathode, the anode, and the direction of electron flow. Given a voltaic cell, identify the half-cells in which oxidation and reduction occur. Define cell potential and how it is determined. Use standard electrode potentials to calculate the standard cell potential of a cell. Distinguish between electrolytic and voltaic cells. Chapter 10: Chemical Quantities Name the basic SI unit for measuring the amount of a substance. Identify the representative particle of elements and compounds. Distinguish between the terms gram atomic mass, gram molecular mass, gram formula mass, and molar mass. Distinguish between an empirical and a molecular formula. Chapter 12: Stoichiometry Construct mole ratios from balanced chemical equations for use as conversion factors in stoichiometric problems. Perform stoichiometric calculations with balanced equations using moles, mass, representative particles, and volumes of gases (at STP). Identify the limiting reagent in a reaction. Based on the limiting reagent, calculate the maximum amount of product(s) produced and the amount of any unreacted excess reagent. Given information from which any two of the following may be determined, calculate the third: theoretical yield, actual yield, and percentage yield. Chapter 13: States of matter and Chapter 14: Gases Describe the motion of particles of a gas according to the kinetic theory. Relate temperature to the average kinetic energy of the particles in a substance. Explain the significance of absolute zero, giving its value in degrees Celsius and Kelvin. State the values of standard temperature and pressure. State Avogadro s hypothesis and explain its significance. Describe the nature of a liquid in terms of the attractive forces between its particles. Look through the gas packet for gas laws Calculate pressure volume changes in a gas using Boyle s law. Calculate temperature volume changes in a gas using Charles law. Calculate temperature pressure changes in a gas using Gay-Lussac s law. Calculate an unknown gas variable using the combined gas law. Use Graham s law of diffusion experimentally or theoretically. Chapter 17: Thermochemistry List six possible phase changes that matter can undergo. Identify the following from a heating (cooling) curve of a substance: melting point, boiling point, heat of fusion, heat of vaporization, (heat of solidification, heat of condensation). Identify the triple point, critical temperature, and critical pressure on a phase diagram.

4 List and define the units of heat energy. Identify two factors that determine the heat capacity of an object. Define the enthalpy of a substance. Perform calculations relating to the heat of phase changes. Perform calculations relating to specific heat capacity. Classify reactions as exothermic or endothermic. Relate a change in enthalpy to the heat of reaction or heat of combustion for a reaction. Use standard heats of formation or Hess law to calculate the enthalpy change of a reaction. Chapter 16: Solutions Define the following terms, giving an example of each: solution, aqueous solution, solute, solvent. List factors that determine solubility and rate of solution formation. Explain the difference between saturated, unsaturated, and supersaturated solutions. Define terms of concentration: molarity, molality, and percent (v/v) and (m/v) concentration. Be able to calculate dilution problems. Honors Chemistry Final Review Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. What is the percent composition of chromium in BaCrO? a. 4.87% c. 20.5% b. 9.47% d. 25.2% 2. Which of the following compounds have the same empirical formula? a. CO and SO c. C H and C H b. C H and C H d. C H and C H 3. Chemical equations. a. describe chemical reactions b. show how to write chemical formulas c. give directions for naming chemical compounds d. describe only biological changes 4. When the equation Fe Cl FeCl is balanced, what is the coefficient for Cl? a. 1 c. 3 b. 2 d Chemical equations must be balanced to satisfy. a. the law of definite proportions c. the law of conservation of mass b. the law of multiple proportions d. Avogadro s principle 6. In order for the reaction 2Al 6HCl 2AlCl 3H to occur, which of the following must be true? a. Al must be above Cl on the activity series. b. Al must be above H on the activity series. c. Heat must be supplied for the reaction. d. A precipitate must be formed.

5 7. Which of the following statements is NOT true about the decomposition of a simple binary compound? a. The products are unpredictable. b. The products are the constituent elements. c. The reactant is a single substance. d. The reactant could be an ionic or a molecular compound. 8. What is conserved in the reaction shown below? H (g) + Cl (g) 2HCl(g) a. mass only c. mass, moles, and molecules only b. mass and moles only d. mass, moles, molecules, and volume 9. In the reaction 2CO(g) + O (g) 2CO (g), what is the ratio of moles of oxygen used to moles of CO produced? a. 1:1 c. 1:2 b. 2:1 d. 2:2 10. When iron rusts in air, iron(iii) oxide is produced. How many moles of oxygen react with 2.4 mol of iron in the rusting reaction? 4Fe(s) + 3O (g) 2Fe2O (s) a. 1.2 mol c. 2.4 mol b. 1.8 mol d. 3.2 mol 11. According to the kinetic theory, collisions between molecules in a gas. a. are perfectly elastic c. never occur b. are inelastic d. cause a loss of total kinetic energy 12. What is the SI unit of pressure? a. candela c. pascal b. mole d. newton 13. Which are the first particles to evaporate from a liquid? a. particles with the lowest kinetic energy b. particles with the highest kinetic energy c. particles below the surface of the liquid d. All particles evaporate at the same rate. 14. An increase in the temperature of a contained liquid. a. has no effect on the kinetic energy of the liquid b. causes the vapor pressure above the liquid to decrease c. causes fewer particles to escape from the surface of the liquid d. causes the vapor pressure above the liquid to increase 15. When the external pressure is 505 kpa, what is the vapor pressure of water at its boiling point? a. 0 kpa c. 505 kpa b kpa d kpa 16. What happens to the temperature of a gas when it is compressed? a. The temperature increases. b. The temperature does not change. c. The temperature decreases. d. The temperature becomes unpredictable. 17. An ideal gas CANNOT be. a. condensed c. heated b. cooled d. compressed

6 18. What happens to the partial pressure of oxygen in a sample of air if the temperature is increased? a. It increases. c. It decreases. b. It stays the same. d. The change cannot be determined. 19. Which of the following substances is the most soluble in water? a. sodium chloride c. bromine b. methane d. carbon 20. Which of these would you expect to be soluble in the nonpolar solvent carbon disulfide, CS? a. c. NaCl b. CI d. SnS 21. What type of compound is always an electrolyte? a. polar covalent c. ionic b. nonpolar covalent d. network solid 22. Which of the following expressions is generally used for solubility? a. grams of solute per 100 grams of solvent b. grams of solute per 100 milliliters of solvent c. grams of solute per 100 grams of solution d. grams of solute per 100 milliliters of solution 23. Which of the following occurs as temperature increases? a. Solubility decreases. c. Solubility remains the same. b. Solubility increases. d. Molarity doubles. 24. What mass of Na SO is needed to make 2.5 L of 2.0M solution? (Na = 23 g; S = 32 g; O = 16 g) a. 178 g c. 356 g b. 284 g d. 710 g 25. What is the molality of a solution containing 8.0 grams of solute in 0.50 kg of solvent? (molar mass of solute = 24 g) a. 0.67m c. 1.67m b. 4m d. 0.17m 26. What is the approximate molar mass of a molecular solute if 300 g of the solute in 1000 g of water causes the solution to have a boiling point of 101 C? (K = C/m; K = 1.86 C/m; molar mass of water = 18 g) a. 15 amu c. 150 amu b. 30 amu d. 300 amu 27. What is the amount of heat required to raise the temperature of g of aluminum by 10 C? (specific heat of aluminum = 0.21 ) a. 420 cal c. 42,000 cal b cal d. 420,000 cal 28. When 45 g of an alloy, at 25 C, are dropped into g of water, the alloy absorbs 956 J of heat. If the final temperature of the alloy is 37 C, what is its specific heat? a c b d. 48.8

7 29. In the reaction of calcium with chlorine, which atom is oxidized? a. calcium c. both a and b b. chlorine d. neither a nor b 30. The oxidation number of sulfur in each of the following is +6 EXCEPT for. a. SO c. SO b. Na SO d. S O 31. Which element decreases its oxidation number in the following reaction? I + 2KCl 2KI + Cl a. iodine b. potassium c. chlorine d. No element decreases its oxidation number. 32. What coefficient of H balances the atoms in the following half-reaction? H + MnO Mn + H O a. 1 c. 3 b. 2 d Which of the following is a reduction half-reaction? a. Zn Zn + 2e c. Na Na + e b. NO + 2H O N + 4H + 3e d. 2H + 2e H 34. What happens in a voltaic cell? a. Chemical energy is changed to electrical energy. b. Electrical energy is changed to chemical energy. c. Electrical energy is changed to magnetic energy. d. Magnetic energy is changed to electrical energy. 35. What is the relative standard reduction potential of the half-cell in which reduction occurs? a. positive b. negative c. more negative than the other half-cell d. more positive than the other half-cell 36. At which electrode (anode or cathode) does oxidation occur in an electrolytic cell? a. anode c. both b. cathode d. neither 37. What is the direction of electron flow in an electrolytic cell? a. from cathode to anode c. in either direction b. from anode to cathode d. There is no flow. 38. The first step in most stoichiometry problems is to. a. add the coefficients of the reagents c. convert given quantities to volumes b. convert given quantities to moles d. convert given quantities to masses 39. Which of the following is an INCORRECT interpretation of the balanced equation shown below? 2S(s) + 3O (g) 2SO (g) a. 2 atoms S + 3 molecules O 2 molecules SO b. 2 g S + 3 g O 2 g SO c. 2 mol S + 3 mol O 2 mol SO

8 d. none of the above 40. Calculate the number of moles of Al O that are produced when 0.60 mol of Fe is produced in the following reaction. 2Al(s) + 3FeO(s) 3Fe(s) + Al O (s) a mol c mol b mol d mol 41. How many covalent bonds can each carbon atom form? a. 1 c. 3 b. 2 d Alkanes are hydrocarbons that contain what type of bonds? a. single covalent bonds only c. at least one triple bond b. at least one double bond d. ionic bonds 43. What is the name of the alkane having five carbons? a. propane c. octane b. methane d. pentane 44. The name for an alkyl group that contains two carbon atoms is. a. diphenyl c. dimethyl b. ethyl d. propyl 45. What is the general formula for a straight-chain alkane? a. C H c. C H b. C H d. C H 46. What is the condensed structural formula for 2,2-dimethylbutane? a. CH (CH ) CH c. (CH ) CCH CH b. CH CH CH CH CH d. C H (CH ) 47. Why are the molecules of hydrocarbons nonpolar? a. The intermolecular attractions are strong. b. All the bonds are single covalent bonds. c. The electron pair is shared almost equally in all the bonds. d. Van der Waals forces overcome polarity. 48. What is the name of the smallest alkyne? a. butyne c. methyne b. ethyne d. propyne 49. Which of the following compounds is a structural isomer of butane? a. 2-methylbutane c. 2-methylpropane b. 2,2-dimethylbutane d. 2,2-diethylpropane 50. Which of the following is true about structural isomers? a. Structural isomers have the same molecular formula. b. Structural isomers have different physical and chemical properties. c. Structural isomers have the same elemental composition. d. all of the above 51. In the cis configuration, the methyl groups are placed. a. in between the double bonds c. to the left of the double bond b. on opposite sides of the double bond d. on the same side of the double bond 52. What compound is the simplest aromatic compound? a. methane c. ethyne b. ethene d. benzene

9 53. What is the name of the functional group in the following compound? a. halogen c. carbonyl b. ester d. carboxylic acid 54. The most important way to classify organic compounds is by. a. the number of carbon atoms in the longest chain b. functional group c. the type of carbon carbon bonds d. reactivity 55. What type of compound is CH -O-CH -CH -CH? a. alcohol c. ether b. aldehyde d. ketone 56. Which carbon skeleton represents an ester? a. c. C-C-C-C-C-O-C-C b. d. Honors Chemistry Final Review - Answer Section MULTIPLE CHOICE 1. ANS: C DIF: L2 REF: p. 307 OBJ: ANS: B DIF: L1 REF: p. 309 OBJ: ANS: A DIF: L1 REF: p. 323 OBJ: ANS: C DIF: L1 REF: p. 327, p. 328 OBJ: ANS: C DIF: L1 REF: p. 325 OBJ: ANS: B DIF: L1 REF: p. 333 OBJ: ANS: A DIF: L2 REF: p. 332 OBJ: ANS: D DIF: L1 REF: p. 356 OBJ: ANS: C DIF: L1 REF: p. 356 OBJ: ANS: B DIF: L2 REF: p. 359, p. 360OBJ: ANS: A DIF: L1 REF: p. 385 OBJ: ANS: C DIF: L1 REF: p. 387 OBJ: ANS: B DIF: L1 REF: p. 391 OBJ: ANS: D DIF: L2 REF: p. 392 OBJ: ANS: C DIF: L2 REF: p. 394 OBJ: ANS: A DIF: L1 REF: p. 416 OBJ: ANS: A DIF: L2 REF: p. 428 OBJ: ANS: A DIF: L2 REF: p. 422, p. 432OBJ: ,

10 19. ANS: A DIF: L2 REF: p. 451 OBJ: ANS: B DIF: L3 REF: p. 451 OBJ: ANS: C DIF: L1 REF: p. 452 OBJ: ANS: A DIF: L2 REF: p. 473 OBJ: ANS: B DIF: L2 REF: p. 474 OBJ: ANS: D DIF: L3 REF: p. 481, p. 482 OBJ: ANS: A DIF: L2 REF: p. 491 OBJ: ANS: C DIF: L3 REF: p. 491, p. 494, p. 496OBJ: ANS: A DIF: L1 REF: p. 508 OBJ: ANS: B DIF: L2 REF: p. 509 OBJ: ANS: A DIF: L1 REF: p. 634 OBJ: ANS: D DIF: L2 REF: p. 639, p. 641 OBJ: ANS: A DIF: L2 REF: p. 643 OBJ: ANS: D DIF: L2 REF: p. 650, p. 651 OBJ: ANS: D DIF: L2 REF: p. 650, p. 651 OBJ: ANS: A DIF: L1 REF: p. 665 OBJ: ANS: D DIF: L2 REF: p. 672 OBJ: ANS: A DIF: L2 REF: p. 679 OBJ: ANS: B DIF: L2 REF: p. 679 OBJ: ANS: B DIF: L1 REF: p. 356 OBJ: ANS: B DIF: L2 REF: p. 356 OBJ: ANS: A DIF: L1 REF: p. 359, p. 360OBJ: ANS: D DIF: L1 REF: p. 694 OBJ: ANS: A DIF: L1 REF: p. 694 OBJ: ANS: D DIF: L1 REF: p. 695 OBJ: ANS: B DIF: L1 REF: p. 698 OBJ: ANS: D DIF: L2 REF: p. 695 OBJ: ANS: C DIF: L2 REF: p. 696, p. 698 OBJ: ANS: C DIF: L2 REF: p. 700 OBJ: ANS: B DIF: L1 REF: p. 703 OBJ: ANS: C DIF: L1 REF: p. 704 OBJ: ANS: D DIF: L1 REF: p. 704 OBJ: ANS: D DIF: L1 REF: p. 705 OBJ: ANS: D DIF: L1 REF: p. 710 OBJ: ANS: B DIF: L1 REF: p. 726 OBJ: ANS: B DIF: L1 REF: p. 725 OBJ: ANS: C DIF: L1 REF: p. 735 OBJ: ANS: C DIF: L2 REF: p. 741 OBJ: