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New York Regents Chemistry June 2003

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The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY Tuesday, June 24, 2003 9:15 a.m. to 12:15 p.m., only This is a test of your knowledge of chemistry. Use that knowledge to answer all questions in this examination. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry. 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. The answers to the questions in Part B 2 and Part C are to be written in your separate answer booklet. Be sure to fill in the heading on the front 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 35): 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 The atomic number of an atom is always equal to the number of its (1) protons, only (2) neutrons, only (3) protons plus neutrons (4) protons plus electrons 7 Alpha particles are emitted during the radioactive decay of (1) carbon-14 (3) calcium-37 (2) neon-19 (4) radon-222 8 Which is an empirical formula? (1) P2O5 (3) C2H4 (2) P4O6 (4) C3H6 2 Which subatomic particle has no charge? (1) alpha particle (3) neutron (2) beta particle (4) electron 9 Which substance can be decomposed by a chemical change? (1) Co (3) Cr (2) CO (4) Cu 3 When the electrons of an excited atom return to a lower energy state, the energy emitted can result in the production of (1) alpha particles (3) protons (2) isotopes (4) spectra 10 The percent by mass of calcium in the compound calcium sulfate (CaSO4) is approximately (1) 15% (3) 34% (2) 29% (4) 47% 4 The atomic mass of an element is calculated using the (1) atomic number and the ratios of its naturally occurring isotopes (2) atomic number and the half-lives of each of its isotopes (3) masses and the ratios of its naturally occurring isotopes (4) masses and the half-lives of each of its isotopes 11 What is represented by the dots in a Lewis electron-dot diagram of an atom of an element in Period 2 of the Periodic Table? (1) the number of neutrons in the atom (2) the number of protons in the atom (3) the number of valence electrons in the atom (4) the total number of electrons in the atom 5 The region that is the most probable location of an electron in an atom is (1) the nucleus (3) the excited state (2) an orbital (4) an ion 12 Which type of chemical bond is formed between two atoms of bromine? (1) metallic (3) ionic (2) hydrogen (4) covalent 6 Which is a property of most nonmetallic solids? (1) high thermal conductivity (2) high electrical conductivity (3) brittleness (4) malleability P.S./Chem. June 03 13 [2] Which of these formulas contains the most polar bond? (1) H Br (3) H F (2) H Cl (4) H I 14 According to Table F, which of these salts is least soluble in water? (1) LiCl (3) FeCl2 (2) RbCl (4) PbCl2 22 Which statement correctly describes an endothermic chemical reaction? (1) The products have higher potential energy than the reactants, and the H is negative. (2) The products have higher potential energy than the reactants, and the H is positive. (3) The products have lower potential energy than the reactants, and the H is negative. (4) The products have lower potential energy than the reactants, and the H is positive. 15 Which of these terms refers to matter that could be heterogeneous? (1) element (3) compound (2) mixture (4) solution 23 At standard pressure when NaCl is added to water, the solution will have a (1) higher freezing point and a lower boiling point than water (2) higher freezing point and a higher boiling point than water (3) lower freezing point and a higher boiling point than water (4) lower freezing point and a lower boiling point than water 16 In which material are the particles arranged in a regular geometric pattern? (1) CO2(g) (3) H2O( ) (2) NaCl(aq) (4) C12H22O11(s) 17 Which change is exothermic? (1) freezing of water (2) melting of iron (3) vaporization of ethanol (4) sublimation of iodine 24 Which element has atoms that can form single, double, and triple covalent bonds with other atoms of the same element? (1) hydrogen (3) fluorine (2) oxygen (4) carbon 18 Which type of change must occur to form a compound? (1) chemical (3) nuclear (2) physical (4) phase 25 Which compound is an isomer of pentane? (1) butane (3) methyl butane (2) propane (4) methyl propane 19 Which formula correctly represents the composition of iron (III) oxide? (1) FeO3 (3) Fe3O (2) Fe2O3 (4) Fe3O2 26 In which substance does chlorine have an oxidation number of +1? (1) Cl2 (3) HClO (2) HCl (4) HClO2 20 Given the reaction: PbCl2(aq) + Na2CrO4(aq) PbCrO4(s) + 2 NaCl(aq) 27 Which statement is true for any electrochemical cell? (1) Oxidation occurs at the anode, only. (2) Reduction occurs at the anode, only. (3) Oxidation occurs at both the anode and the cathode. (4) Reduction occurs at both the anode and the cathode. What is the total number of moles of NaCl formed when 2 moles of Na2CrO4 react completely? (1) 1 mole (2) 2 moles (3) 3 moles (4) 4 moles 21 Which hydrocarbon is saturated? (1) propene (3) butene (2) ethyne (4) heptane P.S./Chem. June 03 [3] [OVER] 32 Which type of radioactive emission has a positive charge and weak penetrating power? (1) alpha particle (3) gamma ray (2) beta particle (4) neutron 28 Given the equation: 2 Al + 3 Cu2+ 2 Al3+ + 3 Cu The reduction half-reaction is (1) Al Al3+ + 3e (2) Cu2+ + 2e Cu (3) Al + 3e Al3+ (4) Cu2+ Cu + 2e 33 Which substance contains metallic bonds? (1) Hg( ) (3) NaCl(s) (2) H2O( ) (4) C6H12O6(s) 29 Which 0.1 M solution contains an electrolyte? (3) CH3OH(aq) (1) C6H12O6(aq) (2) CH3COOH(aq) (4) CH3OCH3(aq) 34 What is the name of the process in which the nucleus of an atom of one element is changed into the nucleus of an atom of a different element? (1) decomposition (3) substitution (2) transmutation (4) reduction 30 Which equation represents a neutralization reaction? (1) Na2CO3 + CaCl2 2 NaCl + CaCO3 (2) Ni(NO3)2 + H2S NiS + 2 HNO3 (3) NaCl + AgNO3 AgCl + NaNO3 (4) H2SO4 + Mg(OH)2 MgSO4 + 2 H2O Note that question 35 has only three choices. 35 A catalyst is added to a system at equilibrium. If the temperature remains constant, the activation energy of the forward reaction (1) decreases (2) increases (3) remains the same 31 An Arrhenius acid has (1) only hydroxide ions in solution (2) only hydrogen ions in solution (3) hydrogen ions as the only positive ions in solution (4) hydrogen ions as the only negative ions in solution P.S./Chem. June 03 [4] Part B 1 Answer all questions in this part. Directions (36 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. 36 The nucleus of an atom of K-42 contains (1) 19 protons and 23 neutrons (2) 19 protons and 42 neutrons (3) 20 protons and 19 neutrons (4) 23 protons and 19 neutrons 43 The potential energy diagram below represents a reaction. Potential Energy B 37 What is the total number of electrons in a Cu+ ion? (1) 28 (3) 30 (2) 29 (4) 36 38 Which list of elements is arranged in order of increasing atomic radii? (1) Li, Be, B, C (3) Sc, Ti, V, Cr (2) Sr, Ca, Mg, Be (4) F, Cl, Br, I D Reaction Coordinate Which arrow represents the activation energy of the forward reaction? (1) A (2) B 39 Which isotope is most commonly used in the radioactive dating of the remains of organic materials? (3) 32P (1) 14C 16 (2) N (4) 37K (3) C (4) D 44 Given the formulas of four organic compounds: H H O (a) H C C C 40 According to Reference Table H, what is the vapor pressure of propanone at 45 C? (1) 22 kPa (3) 70. kPa (2) 33 kPa (4) 98 kPa H O H H H H (c) H C C C H H H OH H (d) H C C C H H H H OH H Which pair below contains an alcohol and an acid? (1) a and b (2) a and c 42 Hexane (C6H14) and water do not form a solution. Which statement explains this phenomenon? (1) Hexane is polar and water is nonpolar. (2) Hexane is ionic and water is polar. (3) Hexane is nonpolar and water is polar. (4) Hexane is nonpolar and water is ionic. [5] H H H H O (b) H C C C 41 The freezing point of bromine is (1) 539 C (3) 7 C (2) 539 C (4) 7 C P.S./Chem. June 03 C A (3) b and d (4) c and d [OVER] 45 Which type of reaction is represented by the equation below? Note: n and n are very large numbers equal to about 2000. H H n C H C H H (1) esterification (2) fermentation C H C H H n (3) saponification (4) polymerization 46 A diagram of a chemical cell and an equation are shown below. 48 A student was given four unknown solutions. Each solution was checked for conductivity and tested with phenolphthalein. The results are shown in the data table below. Switch V Voltmeter 1.0 M Pb2+(aq) Pb(s) + Cu2 +(aq) Poor Colorless Good Pink Poor Pink Based on the data table, which unknown solution could be 0.1 M NaOH? 1.0 M Cu2+(aq) (1) A (2) B Pb2 +(aq) + Cu(s) (3) C (4) D 239 49 In the reaction 239 93Np 94Pu + X, what does X represent? (1) a neutron (3) an alpha particle (2) a proton (4) a beta particle the Pb(s) to the Cu(s) the Cu(s) to the Pb(s) the Pb2+(aq) to the Pb(s) the Cu2+(aq) to the Cu(s) Note that question 50 has only three choices. 50 As carbon dioxide sublimes, its entropy (1) decreases (2) increases (3) remains the same 47 Which ion has the same electron configuration as an atom of He? (3) Na+ (1) H 2 (4) Ca2+ (2) O P.S./Chem. June 03 Colorless C When the switch is closed, electrons will flow from (1) (2) (3) (4) Good B Cu(s) Color with Phenolphthalein D Pb(s) Conductivity A Salt bridge Solution [6] Part B 2 Answer all questions in this part. Directions (51 63): 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 51 and 52 on the electron configuration table shown below. Element Electron Configuration X 2 8 8 2 Y 2 8 7 3 Z 2 8 8 51 What is the total number of valence electrons in an atom of electron configuration X? [1] 52 Which electron configuration represents the excited state of a calcium atom? [1] Base your answers to questions 53 and 54 on the information below. Given: Samples of Na, Ar, As, Rb 53 Which two of the given elements have the most similar chemical properties? 54 Explain your answer in terms of the Periodic Table of the Elements. [1] [1] Base your answers to questions 55 and 56 on the information below. Diethyl ether is widely used as a solvent. 55 In the space provided in your answer booklet, draw the structural formula for diethyl ether. [1] 56 In the space provided in your answer booklet, draw the structural formula for an alcohol that is an isomer of diethyl ether. [1] P.S./Chem. June 03 [7] [OVER] Base your answers to questions 57 and 58 on the information below. Two chemistry students each combine a different metal with hydrochloric acid. Student A uses zinc, and hydrogen gas is readily produced. Student B uses copper, and no hydrogen gas is produced. 57 State one chemical reason for the different results of students A and B. [1] 58 Using Reference Table J, identify another metal that will react with hydrochloric acid to yield hydrogen gas. [1] 59 Given the reaction between two different elements in the gaseous state: + + Box A below represents a mixture of the two reactants before the reaction occurs. The product of this reaction is a gas. In Box B provided in your answer booklet, draw the system after the reaction has gone to completion, based on the Law of Conservation of Matter. [2] Box A System Before Reaction 60 As a neutral sulfur atom gains two electrons, what happens to the radius of the atom? [1] 61 After a neutral sulfur atom gains two electrons, what is the resulting charge of the ion? [1] 62 a In the space provided in your answer booklet, calculate the heat released when 25.0 grams of water freezes at 0 C. Show all work. [1] b Record your answer with an appropriate unit. [1] 63 State one difference between voltaic cells and electrolytic cells. Include information about both types of cells in your answer. [1] P.S./Chem. June 03 [8] Part C Answer all questions in this part. Directions (64 79): 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 64 and 65 on the diagram below, which shows a piston confining a gas in a cylinder. 64 Using the set of axes provided in your answer booklet, sketch the general relationship between the pressure and the volume of an ideal gas at constant temperature. [1] 65 The gas volume in the cylinder is 6.2 milliliters and its pressure is 1.4 atmospheres. The piston is then pushed in until the gas volume is 3.1 milliliters while the temperature remains constant. a In the space provided in your answer booklet, calculate the pressure, in atmospheres, after the change in volume. Show all work. [1] b Record your answer. [1] 66 A student recorded the following buret readings during a titration of a base with an acid: Standard 0.100 M HCl Unknown KOH Initial reading 9.08 mL 0.55 mL Final reading 19.09 mL 5.56 mL a In the space provided in your answer booklet, calculate the molarity of the KOH. Show all work. [1] b Record your answer to the correct number of significant figures. [1] 67 John Dalton was an English scientist who proposed that atoms were hard, indivisible spheres. In the modern model, the atom has a different internal structure. a Identify one experiment that led scientists to develop the modern model of the atom. [1] b Describe this experiment. [1] c State one conclusion about the internal structure of the atom, based on this experiment. [1] P.S./Chem. June 03 [9] [OVER] Base your answers to questions 68 through 73 on the information below and on your knowledge of chemistry. Nuclear Waste Storage Plan for Yucca Mountain In 1978, the U.S. Department of Energy began a study of Yucca Mountain which is located 90 miles from Las Vegas, Nevada. The study was to determine if Yucca Mountain would be suitable for a long-term burial site for high-level radioactive waste. A threedimensional (3-D) computer scale model of the site was used to simulate the Yucca Mountain area. The computer model study for Yucca Mountain included such variables as: the possibility of earthquakes, predicted water flow through the mountain, increased rainfall due to climate changes, radioactive leakage from the waste containers, and increased temperatures from the buried waste within the containers. The containers that will be used to store the radioactive waste are designed to last 10,000 years. Within the 10,000-year time period, cesium and strontium, the most powerful radioactive emitters, would have decayed. Other isotopes found in the waste would decay more slowly, but are not powerful radioactive emitters. In 1998, scientists discovered that the compressed volcanic ash making up Yucca Mountain was full of cracks. Because of the arid climate, scientists assumed that rainwater would move through the cracks at a slow rate. However, when radioactive chlorine-36 was found in rock samples at levels halfway through the mountain, it was clear that rainwater had moved quickly down through Yucca Mountain. It was only 50 years earlier when this chlorine-36 isotope had contaminated rainwater during atmospheric testing of the atom bomb. Some opponents of the Yucca Mountain plan believe that the uncertainties related to the many variables of the computer model result in limited reliability of its predictions. However, advocates of the plan believe it is safer to replace the numerous existing radioactive burial sites around the United States with the one site at Yucca Mountain. Other opponents of the plan believe that transporting the radioactive waste to Yucca Mountain from the existing 131 burial sites creates too much danger to the United States. In 2002, after years of political debate, a final legislative vote approved the development of Yucca Mountain to replace the existing 131 burial sites. 68 State one uncertainty in the computer model that limits the reliability of this computer model. [1] 69 Scientists assume that a manufacturing defect would cause at least one of the waste containers stored in the Yucca Mountain repository to leak within the first 1,000 years. State one possible effect such a leak could have on the environment near Yucca Mountain. [1] 70 State one risk associated with leaving radioactive waste in the 131 sites around the country where it is presently stored. [1] 71 If a sample of cesium-137 is stored in a waste container in Yucca Mountain, how much time must elapse until only 1 32 of the original sample remains unchanged? [1] 72 The information states Within the 10,000-year time period, cesium and strontium, the most powerful radioactive emitters, would have decayed. Use information from Reference Table N to support this statement. [1] 73 Why is water flow a crucial factor in deciding whether Yucca Mountain is a suitable burial site? [1] P.S./Chem. June 03 [10] Base your answers to questions 74 through 76 on the information below. A student wishes to investigate how the reaction rate changes with a change in concentration of HCl(aq). Given the reaction: Zn(s) + HCl(aq) H2(g) + ZnCl2(aq) 74 Identify the independent variable in this investigation. [1] 75 Identify one other variable that might affect the rate and should be held constant during this investigation. [1] 76 Describe the effect of increasing the concentration of HCl(aq) on the reaction rate and justify your response in terms of collision theory. [1] Base your answers to questions 77 through 79 on the information below. A truck carrying concentrated nitric acid overturns and spills its contents. The acid drains into a nearby pond. The pH of the pond water was 8.0 before the spill. After the spill, the pond water is 1,000 times more acidic. 77 Name an ion in the pond water that has increased in concentration due to this spill. [1] 78 What is the new pH of the pond water after the spill? 79 What color would bromthymol blue be at this new pH? P.S./Chem. June 03 [11] [1] [1] The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING Tear Here CHEMISTRY Tuesday, June 24, 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 ............ 13 . . . . . . . . . . . . 25 . . . . . . . . . . . 36 . . . . . . . . . . . . 44 . . . . . . . . . . . . 2 ............ 14 . . . . . . . . . . . . 26 . . . . . . . . . . . 37 . . . . . . . . . . . . 45 . . . . . . . . . . . . 3 ............ 15 . . . . . . . . . . . . 27 . . . . . . . . . . . 38 . . . . . . . . . . . . 46 . . . . . . . . . . . . 4 ............ 16 . . . . . . . . . . . . 28 . . . . . . . . . . . 39 . . . . . . . . . . . . 47 . . . . . . . . . . . . 5 ............ 17 . . . . . . . . . . . . 29 . . . . . . . . . . . 40 . . . . . . . . . . . . 48 . . . . . . . . . . . . 6 ............ 18 . . . . . . . . . . . . 30 . . . . . . . . . . . 41 . . . . . . . . . . . . 49 . . . . . . . . . . . . 7 ............ 19 . . . . . . . . . . . . 31 . . . . . . . . . . . 42 . . . . . . . . . . . . 50 . . . . . . . . . . . . 8 ............ 20 . . . . . . . . . . . . 32 . . . . . . . . . . . 43 . . . . . . . . . . . . Part B 1 Score 9 ............ 21 . . . . . . . . . . . . 33 . . . . . . . . . . . 10 . . . . . . . . . . . . 22 . . . . . . . . . . . . 34 . . . . . . . . . . . 11 . . . . . . . . . . . . 23 . . . . . . . . . . . . 35 . . . . . . . . . . . 12 . . . . . . . . . . . . 24 . . . . . . . . . . . . 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 FOR TEACHERS ONLY The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PS CH PHYSICAL SETTING/CHEMISTRY Tuesday, June 24, 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 B 1 Part B 1 Part A 1 . . . . . .1 ...... 13 . . . . . . 3 ...... 25 . . . . . .3. . . . . 36 . . . . .1 ....... 44 . . . . .3 ....... 2 . . . . . .3 ...... 14 . . . . . . 4 ...... 26 . . . . . .3. . . . . 37 . . . . .1 ....... 45 . . . . .4 ....... 3 . . . . . .4 ...... 15 . . . . . . 2 ...... 27 . . . . . .1. . . . . 38 . . . . .4 ....... 46 . . . . .1 ....... 4 . . . . . .3 ...... 16 . . . . . . 4 ...... 28 . . . . . .2. . . . . 39 . . . . .1 ....... 47 . . . . .1 ....... 5 . . . . . .2 ...... 17 . . . . . . 1 ...... 29 . . . . . .2. . . . . 40 . . . . .3 ....... 48 . . . . .3 ....... 6 . . . . . .3 ...... 18 . . . . . . 1 ...... 30 . . . . . .4. . . . . 41 . . . . .4 ....... 49 . . . . .4 ....... 7 . . . . . .4 ...... 19 . . . . . . 2 ...... 31 . . . . . .3. . . . . 42 . . . . .3 ....... 50 . . . . .2 ....... 8 . . . . . .1 ...... 20 . . . . . . 4 ...... 32 . . . . . .1. . . . . 43 . . . . .2 ....... Part B 1 Score 9 . . . . . .2 ...... 21 . . . . . . 4 ...... 33 . . . . . .1. . . . . 10 . . . . . . 2 ...... 22 . . . . . . 2 ...... 34 . . . . . .2. . . . . 11 . . . . . . 3 ...... 23 . . . . . . 3 ...... 35 . . . . . .1. . . . . 12 . . . . . . 4 ...... 24 . . . . . . 4 ...... Part A Score [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 15 credits for this part. The student must answer all questions in this part. 51 [1] Allow 1 credit for 2. 52 [1] Allow 1 credit for Y or 2 8 7 3. 53 [1] Allow 1 credit for Na and Rb. 54 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: same number of valence electrons Group 1 Elements in the same group (family) have similar chemical properties. Both lose one electron when they react. 55 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: C C O H H H C H H C C O C C H H 56 C H H H [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: H OH H H H C C C C H H H H H C C C OH C C C C C OH C C C OH C or Allow 1 credit for a response consistent with the student s answer to question 55. [4] PHYSICAL SETTING/CHEMISTRY continued 57 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Cu is less active than hydrogen gas. Zn more reactive Cu is below H2 on the activity series and Zn is above H2. 58 [1] Allow 1 credit for any metal other than Zn, that is above H2 on Table J. Acceptable responses include, but are not limited to, these examples: magnesium or Mg aluminum or Al 59 [2] Allow 1 credit for correctly drawing four particles and one particle. and Allow 1 credit for showing any particles in a gaseous state. Acceptable responses include, but are not limited to, this example: Box B System After Reaction Has Gone to Completion 60 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: gets bigger increases The ion is larger than the atom. 61 [1] Allow 1 credit for 2 or negative. [5] [OVER] PHYSICAL SETTING/CHEMISTRY continued 62 [2] a Allow 1 credit for a correct setup. Writing the formula in the setup is not required. Acceptable responses include, but are not limited to, these examples: q = mHf = (25.0 g)(334 J/g) 25.0(334) b Allow 1 credit for 8350 J or 8350 joules. or Allow 1 credit for a response consistent with the student s setup and that has an appropriate unit. Note: Significant figures do not need to be shown. 63 [1] Allow 1 credit for a correct response. Students must discuss both voltaic and electrolytic cells. Acceptable responses include, but are not limited to, these examples: Voltaic cells produce energy; electrolytic cells consume energy. voltaic changes chemical to electrical, electrolytic opposite Voltaic cells involve spontaneous redox reactions; electrolytic cells involve nonspontaneous redox reactions. voltaic spontaneous/electrolytic not [6] PHYSICAL SETTING/CHEMISTRY continued Part C Allow a total of 20 credits for this part. The student must answer all questions in this part. 64 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: V P P 65 V [2] a Allow 1 credit for a correct setup. Writing the formula in the setup is not required. Units and significant figures do not need to be shown. Acceptable responses include, but are not limited to, these examples: (6.2 mL)(1.4 atm) = (3.1 mL)(P2) P2 = 6.2 mL(1.4 atm) 3.1 mL The volume is halved so pressure must double. b Allow 1 credit for 2.8. or Allow 1 credit for a response consistent with the student s setup. Note: Significant figures do not need to be shown. 66 [2] a Allow 1 credit for a correct setup. Writing the formula and/or the unit in the setup is not required. Acceptable responses include, but are not limited to, these examples: MKOH = (0.100 M)(10.01 mL) 5.01 mL M AV A=M BV B (0.100 M)(10.01 mL) = (MB)(5.01 mL) b Allow 1 credit for 0.200. The response must contain three significant figures. or Allow 1 credit for a response containing two or three significant figures consistent with the student s setup. [7] [OVER] PHYSICAL SETTING/CHEMISTRY continued 67 [3] a Allow 1 credit for identifying one experiment. Acceptable responses include, but are not limited to, these examples: gold foil (Rutherford) cathode rays (Thomson) electron bombardment (Moseley) b Allow 1 credit for a description consistent with the experiment chosen by the student. Acceptable responses include, but are not limited to, this example: In the gold-foil experiment, gold foil was bombarded with alpha particles. Some alpha particles were deflected. c Allow 1 credit for stating a conclusion drawn from the experiment chosen by the student. Acceptable responses include, but are not limited to, these examples: The gold-foil experiment shows that an atom is mostly empty space. An atom has a small dense core. An atom has a positively charged center. 68 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: corrosion rates of the waste containers the area s vulnerability to earthquakes climate changes that increase rainfall 69 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: pollution of fresh water in the area adverse effects on humans, fish, and wildlife Radioactivity would get into the food chain. Groundwater would become contaminated. 70 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: The other sites may be in more populated areas so more people would be at risk. Leaving radioactive waste in sites spread around the country would expose more regions to contamination. terrorism 71 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: any response from 150 to 152 5 half-lives [8] PHYSICAL SETTING/CHEMISTRY continued 72 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: The half-life of cesium-137 is short, and the sample would almost be entirely decayed after 10,000 years. The half-life of strontium-90 is short, and the sample would almost be entirely decayed after 10,000 years. 73 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: because water may transport the radioactive materials cause containers to corrode 74 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: concentration of HCl HCl(aq) HCl [HCl] 75 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: temperature surface area of Zn amount of Zn Zn concentration of Zn [Zn] 76 [1] Allow 1 credit for a response with a correct justification. Acceptable responses include, but are not limited to, these examples: rate , more collisions The rate will increase because the higher concentration of HCl will lead to a greater number of collisions. [9] [OVER] PHYSICAL SETTING/CHEMISTRY concluded 77 [1] Allow 1 credit for H+ or hydrogen or H3O+ or hydronium or NO3 or nitrate. 78 [1] Allow 1 credit for 5. Significant figures do not need to be shown. 79 [1] Allow 1 credit for yellow. or Allow 1 credit for a response consistent with the student s answer to question 78. [10] Regents Examination in Physical Setting/Chemistry June 2003 Chart for Converting Total Test Raw Scores to Final Examination Scores (Scaled Scores) Raw Score 85 84 83 82 81 80 79 78 77 76 75 74 73 72 71 70 69 68 67 66 65 64 Scaled Score 100 98 97 95 94 93 91 90 89 87 86 85 84 83 82 81 80 79 78 77 76 75 Raw Score 63 62 61 60 59 58 57 56 55 54 53 52 51 50 49 48 47 46 45 44 43 42 Scaled Score 74 73 72 72 71 70 69 68 68 67 66 66 65 64 63 62 62 61 60 59 59 58 Raw Score 41 40 39 38 37 36 35 34 33 32 31 30 29 28 27 26 25 24 23 22 21 20 Scaled Score 57 56 55 55 54 53 52 51 50 49 48 47 46 45 44 43 42 41 40 38 37 36 Raw Score 19 18 17 16 15 14 13 12 11 10 9 8 7 6 5 4 3 2 1 0 Scaled Score 35 33 32 30 29 27 26 24 22 21 19 17 15 13 11 9 7 5 2 0 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. Map to Core Curriculum Key Ideas June 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 Part C 66b,74,75 54,60,61 67 56 71,72 Standard 2 Key Idea 1 Key Idea 2 40,41 68 Standard 6 Key Idea 1 Key Idea 2 Key Idea 3 Key Idea 4 Key Idea 5 77 Standard 7 Key Idea 1 Key Idea 2 Key Idea 3 Key Idea 4 69,70,73 Standard 4 Process Skills 36,37,38,41,42, 44,45,46,48,50, 51,52,53,55,57, 58,59,63 39,43,49,62 Key Idea 5 Key Idea 4 Key Idea 5 11,12,13,33,34 2002 Edition 71,72 47 Standard 4 1,2,3,4,5,6,8,9, 36,37,38,42,44, 10,14,15,16,18, 45,46,48,50,51, 19,20,21,23,24, 52,53,54,55,56, 25,26,27,28,29, 57,58,59,63 30,31,32,35 7,17,22 39,43,49,62 Key Idea 3 64,65,66a,76,78, 79 64,65,66,67,74, 75,76,77,78,79 69,70,71,72,73 40,41,47,60,61 Reference Tables 2,7,10,13,14, 36,37,40,41,44, 64,65,66,71,72,79 19,24,26,32 47,48,49,52,53, 54,55,56,57,58, 62 [12]

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