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New York Regents Chemistry January 2003

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The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY Wednesday, January 29, 2003 9:15 a.m. to 12:15 p.m., only You are to answer all questions in all parts of this examination according to the directions provided in the examination booklet. Your answer sheet for Part A and Part B 1 is the last page of this examination booklet. Turn to the last page and fold it along the perforations. Then, slowly and carefully, tear off your answer sheet and fill in the heading. Your answer booklet for Part B 2 and Part C is stapled in the center of this examination booklet. Open the examination booklet, carefully remove your answer booklet, and close the examination booklet. Then fill in the heading of your answer booklet. Record the number of your choice for each Part A and Part B 1 multiple-choice question on your separate answer sheet. Write your answers to the Part B 2 and Part C questions in your answer booklet. All work should be written in pen, except for graphs and drawings, which should be done in pencil. You may use scrap paper to work out the answers to the questions, but be sure to record all your answers on your separate answer sheet and in your answer booklet. When you have completed the examination, you must sign the statement printed at the end of your separate answer sheet, indicating that you had no unlawful knowledge of the questions or answers prior to the examination and that you have neither given nor received assistance in answering any of the questions during the examination. Your answer sheet and answer booklet cannot be accepted if you fail to sign this declaration. Notice. . . A four-function or scientific calculator and a copy of the Reference Tables for Physical Setting/Chemistry must be available for your use while taking this examination. DO NOT OPEN THIS EXAMINATION BOOKLET UNTIL THE SIGNAL IS GIVEN. Part A Answer all questions in this part. Directions (1 30): For each statement or question, write on the separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry. 1 Which statement best describes electrons? (1) They are positive subatomic particles are found in the nucleus. (2) They are positive subatomic particles are found surrounding the nucleus. (3) They are negative subatomic particles are found in the nucleus. (4) They are negative subatomic particles are found surrounding the nucleus. 6 Which Group of the Periodic Table contains atoms with a stable outer electron configuration? (1) 1 (3) 16 (2) 8 (4) 18 and and and 7 From which of these atoms in the ground state can a valence electron be removed using the least amount of energy? (1) nitrogen (3) oxygen (2) carbon (4) chlorine and 2 During a flame test, ions of a specific metal are heated in the flame of a gas burner. A characteristic color of light is emitted by these ions in the flame when the electrons (1) gain energy as they return to lower energy levels (2) gain energy as they move to higher energy levels (3) emit energy as they return to lower energy levels (4) emit energy as they move to higher energy levels 8 What is the percent by mass of oxygen in H2SO4? [formula mass = 98] (1) 16% (3) 65% (2) 33% (4) 98% 9 An atom of carbon-12 and an atom of carbon-14 differ in (1) atomic number (2) mass number (3) nuclear charge (4) number of electrons 3 In which list are the elements arranged in order of increasing atomic mass? (1) Cl, K, Ar (3) Te, I, Xe (2) Fe, Co, Ni (4) Ne, F, Na 10 The strength of an atom s attraction for the electrons in a chemical bond is the atom s (1) electronegativity (3) heat of reaction (2) ionization energy (4) heat of formation 4 In which compound does chlorine have the highest oxidation number? (1) NaClO (3) NaClO3 (2) NaClO2 (4) NaClO4 11 Which type or types of change, if any, can reach equilibrium? (1) a chemical change, only (2) a physical change, only (3) both a chemical and a physical change (4) neither a chemical nor a physical change 5 Which event must always occur for a chemical reaction to take place? (1) formation of a precipitate (2) formation of a gas (3) effective collisions between reacting particles (4) addition of a catalyst to the reaction system P.S./Chem. Jan. 03 12 An increase in the average kinetic energy of a sample of copper atoms occurs with an increase in (1) concentration (3) pressure (2) temperature (4) volume [2] 16 One similarity between all mixtures and compounds is that both (1) are heterogeneous (2) are homogeneous (3) combine in a definite ratio (4) consist of two or more substances 13 The empirical formula of a compound is CH2. Which molecular formula is correctly paired with a structural formula for this compound? C2H4 H C C H (1) H H C3H8 H H H H C C C H (3) H C H C2H4 C H (2) H 17 Which phase change results in the release of energy? (1) H2O(s) H2O( ) (2) H2O(s) H2O(g) (3) H2O( ) H2O(g) (4) H2O(g) H2O( ) H H H 18 Which compound has an isomer? H H (1) H C H H C3H8 H H C C C H (4) H H H H H (2) H C C H H H (3) H C C C H H H H H H H H H H H H (4) H C C C C H H H H H 14 Given the equation: F + 1e 19 What occurs when NaCl(s) is added to water? (1) The boiling point of the solution increases, and the freezing point of the solution decreases. (2) The boiling point of the solution increases, and the freezing point of the solution increases. (3) The boiling point of the solution decreases, and the freezing point of the solution decreases. (4) The boiling point of the solution decreases, and the freezing point of the solution increases. F This equation represents the formation of a (1) fluoride ion, which is smaller in radius than a fluorine atom (2) fluoride ion, which is larger in radius than a fluorine atom (3) fluorine atom, which is smaller in radius than a fluoride ion (4) fluorine atom, which is larger is radius than a fluoride ion 20 Which radioisotope is a beta emitter? (1) 90Sr (3) 37K (2) 220Fr (4) 238U 15 The high electrical conductivity of metals is primarily due to (1) high ionization energies (2) filled energy levels (3) mobile electrons (4) high electronegativities P.S./Chem. Jan. 03 21 When a mixture of water, sand, and salt is filtered, what passes through the filter paper? (1) water, only (2) water and sand, only (3) water and salt, only (4) water, sand, and salt [3] [OVER] 22 A hydrate is a compound that includes water molecules within its crystal structure. During an experiment to determine the percent by mass of water in a hydrated crystal, a student found the mass of the hydrated crystal to be 4.10 grams. After heating to constant mass, the mass was 3.70 grams. What is the percent by mass of water in this crystal? (1) 90.% (3) 9.8% (2) 11% (4) 0.40% 27 When a neutral atom undergoes oxidation, the atom s oxidation state (1) decreases as it gains electrons (2) decreases as it loses electrons (3) increases as it gains electrons (4) increases as it loses electrons 28 Given the equation: C(s) + H2O(g) CO(g) + H2(g) Which species undergoes reduction? 23 Which of these 1 M solutions will have the highest pH? (1) NaOH (3) HCl (2) CH3OH (4) NaCl (1) C(s) (2) H+ 29 Which equation is an example of artificial transmutation? 4 12 1 (1) 9 4Be + 2He 6C + 0n (2) U + 3 F2 UF6 (3) Mg(OH)2 + 2 HCl 2 H2O + MgCl2 (4) Ca + 2 H2O Ca(OH)2 + H2 24 Which physical property makes it possible to separate the components of crude oil by means of distillation? (1) melting point (3) solubility (2) conductivity (4) boiling point 30 Which species can conduct an electric current? (1) NaOH(s) (3) H2O(s) (2) CH3OH(aq) (4) HCl(aq) 25 In saturated hydrocarbons, carbon atoms are bonded to each other by (1) single covalent bonds, only (2) double covalent bonds, only (3) alternating single and double covalent bonds (4) alternating double and triple covalent bonds 26 Which formula correctly represents the product of an addition reaction between ethene and chlorine? (1) CH2Cl2 (3) C2H4Cl2 (2) CH3Cl (4) C2H3Cl P.S./Chem. Jan. 03 (3) C2+ (4) H2(g) [4] Part B 1 Answer all questions in this part. Directions (31 50): For each statement or question, write on the separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry. 31 According to Table N, which radioactive isotope is best for determining the actual age of Earth? (1) 238U (3) 60Co 90 (2) Sr (4) 14C 36 Hydrogen has three isotopes with mass numbers of 1, 2, and 3 and has an average atomic mass of 1.00794 amu. This information indicates that (1) equal numbers of each isotope are present (2) more isotopes have an atomic mass of 2 or 3 than of 1 (3) more isotopes have an atomic mass of 1 than of 2 or 3 (4) isotopes have only an atomic mass of 1 32 Given the following solutions: Solution A: pH of 10 Solution B: pH of 7 Solution C: pH of 5 Which list has the solutions placed in order of increasing H+ concentration? (3) C, A, B (4) C, B, A 33 Which statement explains why nuclear waste materials may pose a problem? (1) They frequently have short half-lives and remain radioactive for brief periods of time. (2) They frequently have short half-lives and remain radioactive for extended periods of time. (3) They frequently have long half-lives and remain radioactive for brief periods of time. (4) They frequently have long half-lives and remain radioactive for extended periods of time. 38 Given the reaction: S(s) + O2(g) SO2(g) + energy Potential Energy Which diagram best represents the potential energy changes for this reaction? Potential Energy (1) A, B, C (2) B, A, C 37 Which list of elements contains two metalloids? (1) Si, Ge, Po, Pb (3) Si, P, S, Cl (2) As, Bi, Br, Kr (4) Po, Sb, I, Xe Reaction Coordinate (1) Potential Energy 35 Which of the following solids has the highest melting point? (3) SO2(s) (1) H2O(s) (2) Na2O(s) (4) CO2(s) P.S./Chem. Jan. 03 (3) Potential Energy 34 A compound whose water solution conducts electricity and turns phenolphthalein pink is (1) HCl (3) NaOH (2) HC2H3O2 (4) CH3OH Reaction Coordinate Reaction Coordinate (2) [5] Reaction Coordinate (4) [OVER] 39 A chemist performs the same tests on two homogeneous white crystalline solids, A and B. The results are shown in the table below. Solid A Solid B Melting Point High, 801 C Low, decomposes at 186 C Solubility in H2O (grams per 100.0 g H2O at 0 C) 35.7 3.2 Electrical Conductivity (in aqueous solution) Good conductor Nonconductor The results of these tests suggest that (1) both solids contain only ionic bonds (2) both solids contain only covalent bonds (3) solid A contains only covalent bonds and solid B contains only ionic bonds (4) solid A contains only ionic bonds and solid B contains only covalent bonds 40 Solubility data for four different salts in water at 60 C are shown in the table below. Salt Solubility in Water at 60 C A 10 grams / 50 grams H2O B 20 grams / 60 grams H2O C 30 grams / 120 grams H2O D 43 A student intended to make a salt solution with a concentration of 10.0 grams of solute per liter of solution. When the student s solution was analyzed, it was found to contain 8.90 grams of solute per liter of solution. What was the percent error in the concentration of the solution? (1) 1.10% (3) 11.0% (2) 8.90% (4) 18.9% 40 grams/ 80 grams H2O 44 What is the molarity of a solution of NaOH if 2 liters of the solution contains 4 moles of NaOH? (1) 0.5 M (3) 8 M (2) 2 M (4) 80 M Which salt is most soluble at 60 C? (1) A (2) B (3) C (4) D 45 A gas occupies a volume of 40.0 milliliters at 20 C. If the volume is increased to 80.0 milliliters at constant pressure, the resulting temperature will be equal to 41 Which phase change represents a decrease in entropy? (1) solid to liquid (3) liquid to gas (2) gas to liquid (4) solid to gas (1) 20 C P.S./Chem. Jan. 03 80.0 mL 40.0 mL 40.0 mL 80.0 mL (4) 293 K 40.0 mL 80.0 mL 46 According to Reference Table J, which of these metals will react most readily with 1.0 M HCl to produce H2(g)? (1) Ca (3) Mg (2) K (4) Zn How many moles of oxygen are required to react completely with 1.0 mole of C2H2? (1) 2.5 (2) 2.0 (3) 293 K (2) 20 C 42 Given the equation: 2 C2H2(g) + 5 O2(g) 4 CO2(g) + 2 H2O(g) 80.0 mL 40.0 mL (3) 5.0 (4) 10 [6] 47 The graph below represents the heating curve of a substance that starts as a solid below its freezing point. Temperature ( C) 120 90 60 30 Time (minutes) What is the melting point of this substance? (1) 30 C (2) 55 C 48 Given the unbalanced equation: __Fe2O3 + __CO __Fe + __CO2 50 Given the system at equilibrium: N2O4(g) + 58.1 kJ 2 NO2(g) When the equation is correctly balanced using the smallest whole-number coefficients, what is the coefficient of CO? (1) 1 (2) 2 What will be the result of an increase in temperature at constant pressure? (1) The equilibrium will shift to the left, and the concentration of NO2(g) will decrease. (2) The equilibrium will shift to the left, and the concentration of NO2(g) will increase. (3) The equilibrium will shift to the right, and the concentration of NO2(g) will decrease. (4) The equilibrium will shift to the right, and the concentration of NO2(g) will increase. (3) 3 (4) 4 49 Which type of organic compound is represented by the structural formula shown below? H (1) aldehyde (2) alcohol P.S./Chem. Jan. 03 H C C C H H H (3) 90 C (4) 120 C OH H H (3) ether (4) ester [7] [OVER] Part B 2 Answer all questions in this part. Directions (51 61): Record your answers in the spaces provided in your answer booklet. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry. 51 In the boxes provided in your answer booklet: a Draw two different compounds, one in each box, using the representations for atoms of element X and element Z given below. [1] Atom of element X = Atom of element Z = b Draw a mixture of these two compounds. [1] 52 At equilibrium, nitrogen, hydrogen, and ammonia gases form a mixture in a sealed container. The data table below gives some characteristics of these substances. Data Table Gas Boiling Point Melting Point Solubility in Water Nitrogen 196 C 210 C insoluble Hydrogen 252 C 259 C insoluble Ammonia 33 C 78 C soluble Describe how to separate ammonia from hydrogen and nitrogen. [1] Base your answers to questions 53 through 55 on the diagram of a voltaic cell provided in your answer booklet and on your knowledge of chemistry. 53 On the diagram provided in your answer booklet, indicate with one or more arrows the direction of electron flow through the wire. [1] 54 Write an equation for the half-reaction that occurs at the zinc electrode. 55 Explain the function of the salt bridge. [1] [1] 56 Given the nuclear equation: 235U 92 142 91 1 +1 0n 56Ba + 36Kr + 3 0n + energy a State the type of nuclear reaction represented by the equation. [1] b The sum of the masses of the products is slightly less than the sum of the masses of the reactants. Explain this loss of mass. [1] c This process releases greater energy than an ordinary chemical reaction does. Name another type of nuclear reaction that releases greater energy than an ordinary chemical reaction. [1] P.S./Chem. Jan. 03 [8] Base your answers to questions 57 through 60 on the information below. Each molecule listed below is formed by sharing electrons between atoms when the atoms within the molecule are bonded together. Molecule A: Cl2 Molecule B: CCl4 Molecule C: NH3 57 In the box provided in your answer booklet, draw the electron-dot (Lewis) structure for the NH3 molecule. [1] 58 Explain why CCl4 is classified as a nonpolar molecule. [1] 59 Explain why NH3 has stronger intermolecular forces of attraction than Cl2. [1] 60 Explain how the bonding in KCl is different from the bonding in molecules A, B, and C. [1] 61 How is the bonding between carbon atoms different in unsaturated hydrocarbons and saturated hydrocarbons? [1] P.S./Chem. Jan. 03 [9] [OVER] Part C Answer all questions in this part. Directions (62 74): Record your answers in the spaces provided in your answer booklet. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry. Base your answers to questions 62 through 64 on the information and diagram below. One model of the atom states that atoms are tiny particles composed of a uniform mixture of positive and negative charges. Scientists conducted an experiment where alpha particles were aimed at a thin layer of gold atoms. Most of the alpha particles passed directly through the gold atoms. A few alpha particles were deflected from their straight-line paths. An illustration of the experiment is shown below. Alpha particles Deflected alpha particle Gold atoms 62 Most of the alpha particles passed directly through the gold atoms undisturbed. What does this evidence suggest about the structure of the gold atoms? [1] 63 A few of the alpha particles were deflected. What does this evidence suggest about the structure of the gold atoms? [1] 64 How should the original model be revised based on the results of this experiment? P.S./Chem. Jan. 03 [10] [1] Base your answers to questions 65 through 67 on the information below. When cola, a type of soda pop, is manufactured, CO2(g) is dissolved in it. 65 A capped bottle of cola contains CO2(g) under high pressure. When the cap is removed, how does pressure affect the solubility of the dissolved CO2(g)? [1] 66 A glass of cold cola is left to stand 5 minutes at room temperature. How does temperature affect the solubility of the CO2(g)? [1] 67 a In the space provided in your answer booklet, draw a set of axes and label one of them Solubility and the other Temperature. [1] b Draw a line to indicate the solubility of CO2(g) versus temperature on the axes drawn in part a. [1] Base your answers to questions 68 through 70 on the graph below, which shows the vapor pressure curves for liquids A and B. 800 700 Pressure (mm Hg) 600 500 400 A 300 B 200 100 0 0 10 20 30 40 50 60 70 80 90 100 110 120 Temperature ( C) 68 What is the vapor pressure of liquid A at 70 C? Your answer must include correct units. [2] 69 At what temperature does liquid B have the same vapor pressure as liquid A at 70 C? Your answer must include correct units. [2] 70 Which liquid will evaporate more rapidly? Explain your answer in terms of intermolecular forces. [2] P.S./Chem. Jan. 03 [11] [OVER] Base your answers to question 71 through 74 on the information and data table below. A titration setup was used to determine the unknown molar concentration of a solution of NaOH. A 1.2 M HCl solution was used as the titration standard. The following data were collected. Trial 1 Trial 2 Trial 3 Trial 4 Amount of HCI Standard Used 10.0 mL 10.0 mL 10.0 mL 10.0 mL Initial NaOH Buret Reading 0.0 mL 12.2 mL 23.2 mL 35.2 mL Final NaOH Buret Reading 12.2 mL 23.2 mL 35.2 mL 47.7 mL 71 Calculate the volume of NaOH solution used to neutralize 10.0 mL of the standard HCl solution in trial 3. Show your work. [2] 72 According to Reference Table M, what indicator would be most appropriate in determining the end point of this titration? Give one reason for choosing this indicator. [2] 73 Calculate the average molarity of the unknown NaOH solution for all four trials. Your answer must include the correct number of significant figures and correct units. [3] 74 Explain why it is better to use the average data from multiple trials rather than the data from a single trial to calculate the results of the titration. [1] P.S./Chem. Jan. 03 [12] The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING Tear Here CHEMISTRY Wednesday, January 29, 2003 9:15 a.m. to 12:15 p.m., only Student ANSWER SHEET . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Sex: Teacher .............................................. Male Female Grade ........... School . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Record your answers to Part A and Part B 1 on this answer sheet. Part B 1 Part A 1 ............ 11 . . . . . . . . . . . . 21 . . . . . . . . . . . 31 . . . . . . . . . . . . 41 . . . . . . . . . . . . 2 ............ 12 . . . . . . . . . . . . 22 . . . . . . . . . . . 32 . . . . . . . . . . . . 42 . . . . . . . . . . . . 3 ............ 13 . . . . . . . . . . . . 23 . . . . . . . . . . . 33 . . . . . . . . . . . . 43 . . . . . . . . . . . . 4 ............ 14 . . . . . . . . . . . . 24 . . . . . . . . . . . 34 . . . . . . . . . . . . 44 . . . . . . . . . . . . 5 ............ 15 . . . . . . . . . . . . 25 . . . . . . . . . . . 35 . . . . . . . . . . . . 45 . . . . . . . . . . . . 6 ............ 16 . . . . . . . . . . . . 26 . . . . . . . . . . . 36 . . . . . . . . . . . . 46 . . . . . . . . . . . . 7 ............ 17 . . . . . . . . . . . . 27 . . . . . . . . . . . 37 . . . . . . . . . . . . 47 . . . . . . . . . . . . 8 ............ 18 . . . . . . . . . . . . 28 . . . . . . . . . . . 38 . . . . . . . . . . . . 48 . . . . . . . . . . . . 9 ............ 19 . . . . . . . . . . . . 29 . . . . . . . . . . . 39 . . . . . . . . . . . . 49 . . . . . . . . . . . . 10 . . . . . . . . . . . . 20 . . . . . . . . . . . . 30 . . . . . . . . . . . 40 . . . . . . . . . . . . 50 . . . . . . . . . . . . Part B 1 Score Part A Score Write your answers to Part B 2 and Part C in your answer booklet. Tear Here The declaration below should be signed when you have completed the examination. I do hereby affirm, at the close of this examination, that I had no unlawful knowledge of the questions or answers prior to the examination and that I have neither given nor received assistance in answering any of the questions during the examination. Signature Tear Here Tear Here The University of the State of New York A Wednesday, January 29, 2003 9:15 a.m. to 12:15 p.m., only ANSWER BOOKLET B 2 14 21 Male Sex: Female Teacher . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . School . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 20 C CHEMISTRY Student s Score 30 B 1 PHYSICAL SETTING Student . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Maximum Score Part REGENTS HIGH SCHOOL EXAMINATION Grade . . . . . . . . . Answer all questions in Part B 2 and Part C. Record your answers in this booklet. Total Written Test Score (Maximum Raw Score: 85) Final Score (from conversion chart) Raters Initials: Rater 1 . . . . . . . . . . Rater 2 . . . . . . . . . . . For Raters Only Part B 2 51 a 51a b b 52 52 [a] [OVER] For Raters Only Voltaic Cell 53 Wire V Voltmeter Wire Salt bridge Zinc strip Electrolyte Copper strip 53 Electrolyte 54 54 55 55 56 a 56a b b c c 57 57 58 58 [b] For Raters Only 59 59 60 60 61 61 Total Score for Part B 2 Part C 62 62 63 63 64 64 65 65 66 66 [c] [OVER] For Raters Only 67 a and b 67a b 68 68 69 69 70 Liquid: Explanation: 70 71 71 mL 72 Indicator: Reason: 72 73 73 74 74 [d] Total Score for Part C FOR TEACHERS ONLY The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PS CH PHYSICAL SETTING/CHEMISTRY Wednesday, January 29, 2003 9:15 a.m. to 12:15 p.m., only SCORING KEY AND RATING GUIDE Directions to the Teacher: Refer to the directions on page 3 before rating student papers. Part A and Part B 1 Allow 1 credit for each correct response. Part A Part Part B 1B 1 1 . . . . . .4 ...... 11 . . . . . . 3 ...... 21 . . . . . .3 ..... 31 . . . . .1 ....... 41 . . . . .2 ....... 2 . . . . . .3 ...... 12 . . . . . . 2 ...... 22 . . . . . .3 ..... 32 . . . . .1 ....... 42 . . . . .1 ....... 3 . . . . . .1 ...... 13 . . . . . . 2 ...... 23 . . . . . .1 ..... 33 . . . . .4 ....... 43 . . . . .3 ....... 4 . . . . . .4 ...... 14 . . . . . . 2 ...... 24 . . . . . .4 ..... 34 . . . . .3 ....... 44 . . . . .2 ....... 5 . . . . . .3 ...... 15 . . . . . . 3 ...... 25 . . . . . .1 ..... 35 . . . . .2 ....... 45 . . . . .3 ....... 6 . . . . . .4 ...... 16 . . . . . . 4 ...... 26 . . . . . .3 ..... 36 . . . . .3 ....... 46 . . . . .2 ....... 7 . . . . . .2 ...... 17 . . . . . . 4 ...... 27 . . . . . .4 ..... 37 . . . . .1 ....... 47 . . . . .2 ....... 8 . . . . . .3 ...... 18 . . . . . . 4 ...... 28 . . . . . .2 ..... 38 . . . . .1 ....... 48 . . . . .3 ....... 9 . . . . . .2 ...... 19 . . . . . . 1 ...... 29 . . . . . .1 ..... 39 . . . . .4 ....... 49 . . . . .2 ....... 10 . . . . . . 1 ...... 20 . . . . . . 1 ...... 30 . . . . . .4 ..... 40 . . . . .4 ....... 50 . . . . .4 ....... [1] [OVER] PHYSICAL SETTING/CHEMISTRY continued Directions to the Teacher Follow the procedures below for scoring student answer papers for the Physical Setting/Chemistry examination. Additional information about scoring is provided in the publication Information Booklet for Administering and Scoring Regents Examinations in the Sciences. Use only red ink or red pencil in rating Regents papers. Do not correct the student s work by making insertions or changes of any kind. On the detachable answer sheet for Part A and Part B 1, indicate by means of a checkmark each incorrect or omitted answer. In the box provided at the end of each part, record the number of questions the student answered correctly for that part. At least two science teachers must participate in the scoring of each student s responses to the Part B 2 and Part C open-ended questions. Each of these teachers should be responsible for scoring a selected number of the open-ended questions on each answer paper. No one teacher is to score all the open-ended questions on a student s answer paper. Students responses must be scored strictly according to the Scoring Key and Rating Guide. For open-ended questions, credit may be allowed for responses other than those given in the rating guide if the response is a scientifically accurate answer to the question and demonstrates adequate knowledge as indicated by the examples in the rating guide. Complete sentences are not required. Phrases, diagrams, and symbols may be used. In the student s answer booklet, record the number of credits earned for each answer in the box printed to the right of the answer lines or spaces for that question. Fractional credit is not allowed. Only whole-number credit may be given to a response. Units need not be given when the wording of the questions allows such omissions. Raters should enter the scores earned for Part A, Part B 1, Part B 2, and Part C on the appropriate lines in the box printed on the answer booklet and then should add these four scores and enter the total in the box labeled Total Written Test Score. Then, the student s raw score should be converted to a scaled score by using the conversion chart printed at the end of this Scoring Key and Rating Guide. The student s scaled score should be entered in the labeled box on the student s answer booklet. The scaled score is the student s final examination score. All student answer papers that receive a scaled score of 60 through 64 must be scored a second time. For the second scoring, a different committee of teachers may score the student s paper or the original committee may score the paper, except that no teacher may score the same open-ended questions that he/she scored in the first rating of the paper. The school principal is responsible for assuring that the student s final examination score is based on a fair, accurate, and reliable scoring of the student s answer paper. Because scaled scores corresponding to raw scores in the conversion chart may change from one examination to another, it is crucial that for each administration, the conversion chart provided in the scoring key for that administration be used to determine the student s final score. The chart in this scoring key is usable only for this administration of the examination. [3] [OVER] PHYSICAL SETTING/CHEMISTRY continued Part B 2 Allow a total of 14 credits for this part. The student must answer all questions in this part. 51 [2] a Allow 1 credit for correctly drawing two different compounds. At least two different particles must be touching in each drawing and there must be different combinations drawn of touching atoms. Acceptable responses include, but are not limited to, these examples: Note: No specific bond angle is necessary. b Allow 1 credit for correctly drawing a mixture of the two kinds of particles drawn in part a. There must be at least one drawing of each particle. Acceptable responses include, but are not limited to, this example: 52 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Lower the temperature to condense ammonia. Place all three gases in water. Ammonia will dissolve (is soluble). distillation [4] PHYSICAL SETTING/CHEMISTRY continued 53 [1] Voltaic Cell Wire V Voltmeter Wire Salt bridge Zinc strip Electrolyte Copper strip Electrolyte Allow 1 credit for a correct response. All arrows must be drawn in the correct direction from zinc toward copper through the wire. 54 [1] Allow 1 credit for Zn0 Zn2+ + 2e or Zn0 2e Zn2+. Zn instead of Zn0 is acceptable. Indicating states is acceptable but not required for credit. 55 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: migration of ions maintains neutrality prevents polarization 56 [3] a Allow 1 credit for fission. b Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, this example: The mass is converted to energy. c Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: fusion nuclear decay radioactive decay natural transmutation [5] [OVER] PHYSICAL SETTING/CHEMISTRY continued 57 [1] Allow 1 credit for a correct response. Pairs of dots and/or Xs or single dashes are acceptable for any shared pair. Acceptable responses include, but are not limited to, these examples: N H H H Nx H Hx x H H N H H Note: Accept a correct structure in any rotational orientation. 58 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: The molecule is symmetrical in shape and/or charge. Electrons are evenly distributed. All polar covalent dipoles cancel no dipole moments. no dipoles 59 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: NH3 has polar molecules that attract each other. NH3 has an unshared pair of electrons around the center atom. NH3 is capable of hydrogen bonding. unequal distribution of electrons in strong attraction [6] PHYSICAL SETTING/CHEMISTRY continued 60 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: KCl ionic bond; A, B, C no ionic bonds Atoms do not share electrons when bonding. There is a transfer of electrons from K to Cl. KCl forms by electrostatic attraction. Bonding involves a metal with a nonmetal. 61 [1] Allow 1 credit for a correct response that refers to both saturated and unsaturated compounds. Acceptable responses include, but are not limited to, these examples: Unsaturated hydrocarbons double or triple bonds (multiple bonds) and saturated hydrocarbons all single bonds An unsaturated hydrocarbon has at least one multiple covalent bond between carbon atoms, and a saturated hydrocarbon has single covalent bonds between carbon atoms. Unsaturated hydrocarbons have more than one shared pair of electrons between carbon atoms, and saturated hydrocarbons have only one shared pair of electrons between carbon atoms. [7] [OVER] PHYSICAL SETTING/CHEMISTRY continued Part C Allow a total of 21 credits for this part. The student must answer all questions in this part. 62 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: The atom is mostly empty space. The volume of the atom is mostly unoccupied. 63 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Alpha particles were deflected by the positively charged nucleus. nucleus charged 64 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: The atom has a positively charged nucleus; negative electrons surround the outside. The positive charges are in the nucleus; electrons are not mixed in the nucleus. nucleus smaller than atom 65 [1] Allow 1 credit for a correct response. A reference to solubility and pressure must be in the answer. Acceptable responses include, but are not limited to, this example: Solubility of CO2(g) decreases with a decrease in pressure. Note: Do not allow credit for Soda goes flat. [8] PHYSICAL SETTING/CHEMISTRY continued 66 [1] Allow 1 credit for a correct response. A reference to solubility and temperature must be in the answer. Acceptable responses include, but are not limited to, this example: Solubility decreases as temperature increases. Note: Do not allow credit for Soda goes flat. or Temperature [2] a Solubility 67 Temperature Solubility Allow 1 credit for a correctly drawn and labeled set of axes. or Temperature Solubility b Temperature Solubility Allow 1 credit for a line that starts toward the top of the y-axis and goes downward toward the right end of the x-axis. Note: Assume the origin to be zero unless otherwise labeled. 68 [2] Allow 1 credit for 710 ( 10). and Allow 1 credit for mm Hg as the unit. 69 [2] Allow 1 credit for 114 ( 2). and Allow 1 credit for C as the unit. [9] [OVER] PHYSICAL SETTING/CHEMISTRY concluded 70 [2] Allow 1 credit for liquid A. and Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, this example: The higher vapor pressure of liquid A indicates that the intermolecular forces between its molecules are weaker, allowing the molecules to escape more readily to the vapor phase. 71 [2] Allow 1 credit for 12 mL or 12.0 mL. and Allow 1 credit if the setup is correct, but a computational error is made. 72 [2] Allow 1 credit for phenolphthalein or bromthymol blue or litmus. and Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Strong acid and strong base reach an end point at pH = 7. Phenolphthalein goes from colorless to pink after pH = 7. Bromthymol blue (or litmus) reaches an intermediate color around pH = 7. 73 [3] Allow 1 credit for 1.01 or 1.0 or 1. and Allow 1 credit for two significant figures consistent with the student s calculated answer. and Allow 1 credit for M or moles per liter or an equivalent as the unit. 74 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Multiple trials help to cancel out experimental error in each trial. Each trial involves errors either above or below the true value. Therefore, the average value would contain the least error. Multiple trials ensure better accuracy of results. to correct for inconsistencies between trials (in measurement) [10] Regents Examination in Physical Setting/Chemistry January 2003 Chart for Converting Total Test Raw Scores to Final Examination Scores (Scaled Scores) Raw Scaled Raw Scaled Raw Scaled Raw Scaled Score Score Score Score Score Score Score Score 85 100 63 74 41 60 19 39 84 98 62 73 40 60 18 38 83 97 61 72 39 59 17 36 82 95 60 72 38 58 16 35 81 93 59 71 37 57 15 33 80 92 58 70 36 57 14 31 79 91 57 70 35 56 13 30 78 89 56 69 34 55 12 28 77 88 55 68 33 54 11 26 76 87 54 68 32 54 10 24 75 85 53 67 31 53 9 22 74 84 52 67 30 52 8 20 73 83 51 66 29 51 7 18 72 82 50 66 28 50 6 15 71 81 49 65 27 49 5 13 70 80 48 64 26 48 4 11 69 79 47 64 25 47 3 8 68 78 46 63 24 46 2 5 67 77 45 63 23 44 1 3 66 76 44 62 22 43 0 0 65 75 43 61 21 42 64 75 42 61 20 41 To determine the student s final examination score, find the student s total test raw score in the column labeled Raw Score and then locate the scaled score that corresponds to that raw score. The scaled score is the student s final examination score. Enter this score in the space labeled Final Score on the student s answer sheet. [11] Map to Core Curriculum Key Ideas January 2003 Physical Setting/ Chemistry Question Numbers Part A Part B Standard 1 Math Key Idea 1 Math Key Idea 2 Math Key Idea 3 Sci. Inq. Key Idea 1 Sci. Inq. Key Idea 2 Sci. Inq. Key Idea 3 Eng. Des. Key Idea 1 8,22 Part C 43 71,73 67 51,57,58,59 62,63,64 39,40 68,69,71,74 Standard 2 Key Idea 1 Key Idea 2 Standard 6 Key Idea 1 Key Idea 2 Key Idea 3 Key Idea 4 Key Idea 5 45 50 38,47 Standard 7 Key Idea 1 Key Idea 2 Standard 4 Process Skills 33,34,36,37,40,41, 42,44,45,46,48,49, 50,51,52,53,54,55, 56a,61 31,32,38,47,56c Key Idea 3 Key Idea 4 Key Idea 5 65,66,71,72,73 35,39,56b,57,59,60 70 32,34,36,37,40,41, 42,44,45,46,48,49, 50,51,52,53,61 31,33,38,47,56a, 56c 35,39,56b,57,58, 59,60 62,63,64,65,66, 67,71,72,73,74 Standard 4 Key Idea 3 1,2,3,4,5,7,8,9,11,13, 16,18,19,21,22,23,24, 25,26,27,28,30 Key Idea 4 12,17,20 Key Idea 5 6,10,14,15,29 68,69,70 Reference Tables 2002 Edition 3,4,6,7,20 31,37,44,45,46,53 72

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