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New York Regents Chemistry June 2004

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PS/CHEMISTRY The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY Wednesday, June 23, 2004 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. PS/CHEMISTRY Part A Answer all questions in this part. Directions (1 33): 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. 7 Given the reaction: N2(g) + 3 H2(g) 1 The modern model of the atom is based on the work of (1) one scientist over a short period of time (2) one scientist over a long period of time (3) many scientists over a short period of time (4) many scientists over a long period of time What is the mole-to-mole ratio between nitrogen gas and hydrogen gas? (1) 1:2 (2) 1:3 2 Which statement is true about the charges assigned to an electron and a proton? (1) Both an electron and a proton are positive. (2) An electron is positive and a proton is negative. (3) An electron is negative and a proton is positive. (4) Both an electron and a proton are negative. (3) 2:2 (4) 2:3 8 What is the percent by mass of oxygen in propanal, CH3CH2CHO? (1) 10.0% (3) 38.1% (2) 27.6% (4) 62.1% 9 Covalent bonds are formed when electrons are (1) transferred from one atom to another (2) captured by the nucleus (3) mobile within a metal (4) shared between two atoms 3 In the wave-mechanical model, an orbital is a region of space in an atom where there is (1) a high probability of finding an electron (2) a high probability of finding a neutron (3) a circular path in which electrons are found (4) a circular path in which neutrons are found 10 Which type of molecule is CF4? (1) polar, with a symmetrical distribution of charge (2) polar, with an asymmetrical distribution of charge (3) nonpolar, with a symmetrical distribution of charge (4) nonpolar, with an asymmetrical distribution of charge 4 What is the charge of the nucleus in an atom of oxygen-17? (1) 0 (3) +8 (2) 2 (4) +17 5 Which pair of symbols represents a metalloid and a noble gas? (1) Si and Bi (3) Ge and Te (2) As and Ar (4) Ne and Xe 11 Which change occurs when a barium atom loses two electrons? (1) It becomes a negative ion and its radius decreases. (2) It becomes a negative ion and its radius increases. (3) It becomes a positive ion and its radius decreases. (4) It becomes a positive ion and its radius increases. 6 Which statement describes a chemical property of iron? (1) Iron can be flattened into sheets. (2) Iron conducts electricity and heat. (3) Iron combines with oxygen to form rust. (4) Iron can be drawn into a wire. P.S./Chem. June 04 2 NH3(g) [2] 12 Conductivity in a metal results from the metal atoms having (1) high electronegativity (2) high ionization energy (3) highly mobile protons in the nucleus (4) highly mobile electrons in the valence shell 18 Which sample contains particles in a rigid, fixed, geometric pattern? (1) CO2(aq) (3) H2O( ) (2) HCl(g) (4) KCl(s) 19 Given the reaction at 25 C: Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g) 13 Which of these elements has the least attraction for electrons in a chemical bond? (1) oxygen (3) nitrogen (2) fluorine (4) chlorine The rate of this reaction can be increased by using 5.0 grams of powdered zinc instead of a 5.0-gram strip of zinc because the powdered zinc has (1) (2) (3) (4) 14 Recovering the salt from a mixture of salt and water could best be accomplished by (1) evaporation (2) filtration (3) paper chromatography (4) density determination 20 Which statement about a system at equilibrium is true? (1) The forward reaction rate is less than the reverse reaction rate. (2) The forward reaction rate is greater than the reverse reaction rate. (3) The forward reaction rate is equal to the reverse reaction rate. (4) The forward reaction rate stops and the reverse reaction rate continues. 15 The average kinetic energy of water molecules is greatest in which of these samples? (1) 10 g of water at 35 C (2) 10 g of water at 55 C (3) 100 g of water at 25 C (4) 100 g of water at 45 C 16 Helium is most likely to behave as an ideal gas when it is under (1) high pressure and high temperature (2) high pressure and low temperature (3) low pressure and high temperature (4) low pressure and low temperature 21 A catalyst increases the rate of a chemical reaction by (1) lowering the activation energy of the reaction (2) lowering the potential energy of the products (3) raising the temperature of the reactants (4) raising the concentration of the reactants 17 At STP, the element oxygen can exist as either O2 or O3 gas molecules. These two forms of the element have (1) the same chemical and physical properties (2) the same chemical properties and different physical properties (3) different chemical properties and the same physical properties (4) different chemical and physical properties P.S./Chem. June 04 lower kinetic energy lower concentration more surface area more zinc atoms 22 Which element must be present in an organic compound? (1) hydrogen (3) carbon (2) oxygen (4) nitrogen 23 Which compound is a saturated hydrocarbon? (1) hexane (3) hexanol (2) hexene (4) hexanal [3] [OVER] 24 Given the reaction: O O CH3C O C2H5 + H2O CH3C OH + HOC2H5 This reaction is an example of (1) fermentation (2) saponification (3) hydrogenation (4) esterification 25 Which of these compounds has chemical properties most similar to the chemical properties of ethanoic acid? (1) C3H7COOH (3) C2H5COOC2H5 (2) C2H5OH (4) C2H5OC2H5 30 Which compound could serve as a reactant in a neutralization reaction? (1) NaCl (3) CH3OH (2) KOH (4) CH3CHO 31 Which of these particles has the greatest mass? (1) alpha (3) neutron (2) beta (4) positron 26 Given the reaction that occurs in an electrochemical cell: Zn(s) + CuSO4(aq) ZnSO4(aq) + Cu(s) During this reaction, the oxidation number of Zn changes from (1) 0 to +2 (2) 0 to 2 32 In a nuclear fusion reaction, the mass of the products is (1) less than the mass of the reactants because some of the mass has been converted to energy (2) less than the mass of the reactants because some of the energy has been converted to mass (3) more than the mass of the reactants because some of the mass has been converted to energy (4) more than the mass of the reactants because some of the energy has been converted to mass (3) +2 to 0 (4) 2 to 0 27 A voltaic cell spontaneously converts (1) electrical energy to chemical energy (2) chemical energy to electrical energy (3) electrical energy to nuclear energy (4) nuclear energy to electrical energy 28 Which pair of formulas represents two compounds that are electrolytes? (1) HCl and CH3OH (2) HCl and NaOH (3) C5H12 and CH3OH (4) C5H12 and NaOH 33 Which of these types of radiation has the greatest penetrating power? (1) alpha (3) gamma (2) beta (4) positron 29 Hydrogen chloride, HCl, is classified as an Arrhenius acid because it produces (1) H+ ions in aqueous solution (2) Cl ions in aqueous solution (3) OH ions in aqueous solution (4) NH4+ ions in aqueous solution P.S./Chem. June 04 [4] Part B 1 Answer all questions in this part. Directions (34 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. 34 How many electrons are contained in an Au3+ ion? (1) 76 (3) 82 (2) 79 (4) 197 Temperature 40 The graph below represents the uniform heating of a substance, starting with the substance as a solid below its melting point. 35 Which electron configuration represents the electrons of an atom in an excited state? (1) 2 4 (3) 2 7 2 (2) 2 6 (4) 2 8 2 36 In comparison to an atom of 19 9 F in the ground state, an atom of 12 C in the ground state has 6 (1) three fewer neutrons (2) three fewer valence electrons (3) three more neutrons (4) three more valence electrons E D B C A Time Which line segment represents an increase in potential energy and no change in average kinetic energy? (1) AB (2) BC 37 Element X is a solid that is brittle, lacks luster, and has six valence electrons. In which group on the Periodic Table would element X be found? (1) 1 (3) 15 (2) 2 (4) 16 (3) CD (4) EF 41 Using your knowledge of chemistry and the information in Reference Table H, which statement concerning propanone and water at 50 C is true? (1) Propanone has a higher vapor pressure and stronger intermolecular forces than water. (2) Propanone has a higher vapor pressure and weaker intermolecular forces than water. (3) Propanone has a lower vapor pressure and stronger intermolecular forces than water. (4) Propanone has a lower vapor pressure and weaker intermolecular forces than water. 38 What is the empirical formula for the compound C6H12O6? (3) C3H6O3 (1) CH2O (2) C2H4O2 (4) C6H12O6 39 The bonds between hydrogen and oxygen in a water molecule are classified as (1) polar covalent (2) nonpolar covalent (3) ionic (4) metallic P.S./Chem. June 04 F 42 A solution that is at equilibrium must be (1) concentrated (3) saturated (2) dilute (4) unsaturated [5] [OVER] 47 Which structural formula represents an ether? 43 Given the reaction: N2(g) + O2(g) + 182.6 kJ 2 NO(g) H Which change would cause an immediate increase in the rate of the forward reaction? (1) (2) (3) (4) H H C C C C H H C H H H H H C C H (1) (2) (3) (4) C C C H H H (3) (2) H H C C C H H H (2) P.S./Chem. June 04 H C O C H H H (4) Al + 3e Al3+ Al Al3+ + 3e O2 + 4e 2 O2 O2 2 O2 + 4e 1 2 (4) 7 8 Note that question 50 has only three choices. C H H H OH H 49 Based on Reference Table N, what fraction of a sample of gold-198 remains radioactive after 2.69 days? (1) 1 (3) 3 4 4 H H H (1) C C H Which half-reaction correctly represents the oxidation that occurs? H H H H O C OH 48 Given the reaction for the corrosion of aluminum: 4 Al + 3 O2 2 Al2O3 H H H H (2) 46 Which structural formula represents 2-pentyne? H C (3) H 45 Which pH indicates a basic solution? (1) 1 (3) 7 (2) 5 (4) 12 H H C H H H (1) H2O(g) at 120 C H2O( ) at 80 C H2O( ) at 20 C H2O(s) at 0 C H C H H increasing the concentration of NO(g) increasing the concentration of N2(g) decreasing the reaction temperature decreasing the reaction pressure 44 Which 10-milliliter sample of water has the greatest degree of disorder? (1) (2) (3) (4) C H O H H H H C H C H H C C H C 50 As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element generally (1) decreases (2) increases (3) remains the same H H (4) [6] Part B 2 Answer all questions in this part. Directions (51 64): 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 through 53 on the balanced chemical equation below. 2 H2O 2 H2 + O2 51 What type of reaction does this equation represent? [1] 52 How does the balanced chemical equation show the Law of Conservation of Mass? [1] 53 What is the total number of moles of O2 produced when 8 moles of H2O is completely consumed? [1] Base your answers to questions 54 and 55 on the unbalanced redox reaction below. Cu(s) + AgNO3(aq) Cu(NO3)2(aq) + Ag(s) 54 Write the reduction half-reaction. [1] 55 Balance the redox equation in your answer booklet, using the smallest whole-number coefficients. [1] Base your answers to questions 56 through 58 on the information below. A student titrates 60.0 mL of HNO3(aq) with 0.30 M NaOH(aq). Phenolphthalein is used as the indicator. After adding 42.2 mL of NaOH(aq), a color change remains for 25 seconds, and the student stops the titration. 56 What color change does phenolphthalein undergo during this titration? [1] 57 In the space provided in your answer booklet, show a correct numerical setup for calculating the molarity of the HNO3(aq). [1] 58 According to the data, how many significant figures should be present in the calculated molarity of the HNO3(aq)? [1] P.S./Chem. June 04 [7] [OVER] Base your answers to questions 59 through 61 on the data table below, which shows three isotopes of neon. Isotope Atomic Mass Percent Natural (atomic mass units) Abundance 20Ne 19.99 90.9% 21Ne 20.99 0.3% 22Ne 21.99 8.8% 59 In terms of atomic particles, state one difference between these three isotopes of neon. [1] 60 Based on the atomic masses and the natural abundances shown in the data table, in the space provided in your answer booklet, show a correct numerical setup for calculating the average atomic mass of neon. [1] 61 Based on natural abundances, the average atomic mass of neon is closest to which whole number? [1] 62 Based on the Periodic Table, explain why Na and K have similar chemical properties. [1] 63 In the space to the right of the reactants and arrow provided in your answer booklet, draw the structural formula for the product of the reaction shown. [1] 64 Given the nuclear equation: 58 Cu 29 58 28 Ni + X What nuclear particle is represented by X? P.S./Chem. June 04 [8] [1] Part C Answer all questions in this part. Directions (65 85): 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 65 through 67 on the information and equation below. Antacids can be used to neutralize excess stomach acid. Brand A antacid contains the acidneutralizing agent magnesium hydroxide, Mg(OH)2. It reacts with HCl(aq) in the stomach, according to the following balanced equation: 2 HCl(aq) + Mg(OH)2(s) MgCl2(aq) + 2 H2O( ) 65 In the space provided in your answer booklet, show a correct numerical setup for calculating the number of moles of Mg(OH)2 (gram-formula mass = 58.3 grams/mole) in an 8.40-gram sample. [1] 66 If a person produces 0.050 mole of excess HCl in the stomach, how many moles of Mg(OH)2 are needed to neutralize this excess hydrochloric acid? [1] 67 Brand B antacid contains the acid-neutralizing agent sodium hydrogen carbonate. Write the chemical formula for sodium hydrogen carbonate. [1] Base your answers to questions 68 through 70 on the information below. Naphthalene, a nonpolar substance that sublimes at room temperature, can be used to protect wool clothing from being eaten by moths. 68 Explain, in terms of intermolecular forces, why naphthalene sublimes. 69 Explain why naphthalene is not expected to dissolve in water. [1] [1] 70 The empirical formula for naphthalene is C5H4 and the molecular mass of naphthalene is 128 grams/mole. What is the molecular formula for naphthalene? [1] P.S./Chem. June 04 [9] [OVER] Base your answers to questions 71 through 74 on the data table below, which shows the solubility of a solid solute. The Solubility of the Solute at Various Temperatures Solute per Temperature 100 g of H2O(g) ( C) 0 18 20 20 40 24 60 29 80 36 100 49 71 On the grid provided in your answer booklet, mark an appropriate scale on the axis labeled Solute per 100 g of H2O(g). An appropriate scale is one that allows a trend to be seen. [1] 72 On the same grid, plot the data from the data table. Circle and connect the points. [1] Example: 73 Based on the data table, if 15 grams of solute is dissolved in 100 grams of water at 40 C, how many more grams of solute can be dissolved in this solution to make it saturated at 40 C? [1] 74 According to Reference Table G, how many grams of KClO3 must be dissolved in 100 grams of H2O at 10 C to produce a saturated solution? [1] Base your answers to questions 75 through 78 on the information below. A weather balloon has a volume of 52.5 liters at a temperature of 295 K. The balloon is released and rises to an altitude where the temperature is 252 K. 75 How does this temperature change affect the gas particle motion? [1] 76 The original pressure at 295 K was 100.8 kPa and the pressure at the higher altitude at 252 K is 45.6 kPa. Assume the balloon does not burst. In the space provided in your answer booklet, show a correct numerical setup for calculating the volume of the balloon at the higher altitude. [1] 77 What Celsius temperature is equal to 252 K? [1] 78 What pressure, in atmospheres (atm), is equal to 45.6 kPa? [1] P.S./Chem. June 04 [10] Base your answers to questions 79 and 80 on the information and equation below. Human blood contains dissolved carbonic acid, H2CO3, in equilibrium with carbon dioxide and water. The equilibrium system is shown below. H2CO3(aq) CO2(aq) + H2O( ) 79 Explain, using LeChatelier s principle, why decreasing the concentration of CO2 decreases the concentration of H2CO3. [1] 80 What is the oxidation number of carbon in H2CO3(aq)? [1] Base your answers to questions 81 through 84 on the information below. A safe level of fluoride ions is added to many public drinking water supplies. Fluoride ions have been found to help prevent tooth decay. Another common source of fluoride ions is toothpaste. One of the fluoride compounds used in toothpaste is tin(II) fluoride. A town located downstream from a chemical plant was concerned about fluoride ions from the plant leaking into its drinking water. According to the Environmental Protection Agency, the fluoride ion concentration in drinking water cannot exceed 4 ppm. The town hired a chemist to analyze its water. The chemist determined that a 175-gram sample of the town s water contains 0.000 250 gram of fluoride ions. 81 In the box provided in your answer booklet, draw a Lewis electron-dot diagram for a fluoride ion. [1] 82 What is the chemical formula for tin(II) fluoride? [1] 83 How many parts per million of fluoride ions are present in the analyzed sample? [1] 84 Is the town s drinking water safe to drink? Support your decision using information in the passage and your calculated fluoride level in question 83. [1] 85 A plan is being developed for an experiment to test the effect of concentrated strong acids on a metal surface protected by various coatings. Some safety precautions would be the wearing of chemical safety goggles, an apron, and gloves. State one additional safety precaution that should be included in the plan. [1] P.S./Chem. June 04 [11] The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING Tear Here CHEMISTRY Wednesday, June 23, 2004 9:15 a.m. to 12:15 p.m., only ANSWER SHEET Student .............................................. Sex: Male Female Grade ........... Teacher .............................................. School . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Record your answers to Part A and Part B 1 on this answer sheet. Part B 1 Part A 1 ............ 12 . . . . . . . . . . . . 23 . . . . . . . . . . . 34 . . . . . . . . . . . . 43 . . . . . . . . . . . . 2 ............ 13 . . . . . . . . . . . . 24 . . . . . . . . . . . 35 . . . . . . . . . . . . 44 . . . . . . . . . . . . 3 ............ 14 . . . . . . . . . . . . 25 . . . . . . . . . . . 36 . . . . . . . . . . . . 45 . . . . . . . . . . . . 4 ............ 15 . . . . . . . . . . . . 26 . . . . . . . . . . . 37 . . . . . . . . . . . . 46 . . . . . . . . . . . . 5 ............ 16 . . . . . . . . . . . . 27 . . . . . . . . . . . 38 . . . . . . . . . . . . 47 . . . . . . . . . . . . 6 ............ 17 . . . . . . . . . . . . 28 . . . . . . . . . . . 39 . . . . . . . . . . . . 48 . . . . . . . . . . . . 7 ............ 18 . . . . . . . . . . . . 29 . . . . . . . . . . . 40 . . . . . . . . . . . . 49 . . . . . . . . . . . . 8 ............ 19 . . . . . . . . . . . . 30 . . . . . . . . . . . 41 . . . . . . . . . . . . 50 . . . . . . . . . . . . 9 ............ 20 . . . . . . . . . . . . 31 . . . . . . . . . . . 42 . . . . . . . . . . . . 10 . . . . . . . . . . . . 21 . . . . . . . . . . . . 32 . . . . . . . . . . . 11 . . . . . . . . . . . . 22 . . . . . . . . . . . . 33 . . . . . . . . . . . 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 PS/CHEMISTRY Tear Here Tear Here PS/CHEMISTRY FOR TEACHERS ONLY The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PS CH PHYSICAL SETTING/CHEMISTRY Wednesday, June 23, 2004 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. Updated information regarding the rating of this examination may be posted on the New York State Education Department s web site during the rating period. Visit the site http://www.emsc.nysed.gov/osa/ and select the link Latest Information for any recently posted information regarding this examination. This site should be checked before the rating process for this examination begins and at least one more time before the final scores for the examination are recorded. Part A and Part B 1 Allow 1 credit for each correct response. Part B 1 Part A 1 . . . . . .4 ...... 12 . . . . . . 4 ...... 23 . . . . . .1 ..... 34 . . . . . 1 ....... 43 . . . . . 2 ....... 2 . . . . . .3 ...... 13 . . . . . . 3 ...... 24 . . . . . .4 ..... 35 . . . . . 3 ....... 44 . . . . . 1 ....... 3 . . . . . .1 ...... 14 . . . . . . 1 ...... 25 . . . . . .1 ..... 36 . . . . . 2 ....... 45 . . . . . 4 ....... 4 . . . . . .3 ...... 15 . . . . . . 2 ...... 26 . . . . . .1 ..... 37 . . . . . 4 ....... 46 . . . . . 4 ....... 5 . . . . . .2 ...... 16 . . . . . . 3 ...... 27 . . . . . .2 ..... 38 . . . . . 1 ....... 47 . . . . . 4 ....... 6 . . . . . .3 ...... 17 . . . . . . 4 ...... 28 . . . . . .2 ..... 39 . . . . . 1 ....... 48 . . . . . 2 ....... 7 . . . . . .2 ...... 18 . . . . . . 4 ...... 29 . . . . . .1 ..... 40 . . . . . 2 ....... 49 . . . . . 2 ....... 8 . . . . . .2 ...... 19 . . . . . . 3 ...... 30 . . . . . .2 ..... 41 . . . . . 2 ....... 50 . . . . . 1 ....... 9 . . . . . .4 ...... 20 . . . . . . 3 ...... 31 . . . . . .1 ..... 42 . . . . . 3 ....... Part B 1 Score 10 . . . . . . 3 ...... 21 . . . . . . 1 ...... 32 . . . . . .1 ..... 11 . . . . . . 3 ...... 22 . . . . . . 3 ...... 33 . . . . . .3 ..... [1] 2 1 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 that will be posted on the Department s web site http://www.emsc.nysed.gov/osa/ on Wednesday, June 23, 2004. 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 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: decomposition analysis redox endothermic electrolysis 52 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: 4 H and 2 O on both sides 4 H = 4 H and 2 O = 2 O same number of each element on both sides 53 [1] Allow 1 credit for 4. 54 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Ag+ + e Ag 2 Ag+ + 2e 2 Ag 55 [1] Allow 1 credit for Cu(s) + 2 AgNO3(aq) Cu(NO3)2(aq) + 2 Ag(s). Allow credit even if the coefficient 1 is written in front of Cu(s) and Cu(NO3)2(aq). 56 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: colorless to pink no color to red [4] PHYSICAL SETTING/CHEMISTRY continued 57 [1] Allow 1 credit for a correct numerical setup. Acceptable responses include, but are not limited to, these examples: (0.30 M)(42.2 mL) 60.0 mL (x)(60) = (.3)(42.2) 58 [1] Allow 1 credit for 2. 59 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Each isotope has a different number of neutrons. different number of neutrons Ne-22 has two more neutrons than Ne-20 and one more neutron than Ne-21. 60 [1] Allow 1 credit for a correct numerical setup. Acceptable responses include, but are not limited to, these examples: (0.909)(19.99) + (0.003)(20.99) + (0.088)(21.99) (90.9%)(19.99) + (0.3%)(20.99) + (8.8%)(21.99) (90.9)(19.99) + (0.3)(20.99) + (8.8)(21.99) 100 61 [1] Allow 1 credit for 20. 62 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: They have the same number of valence electrons. form 1+ ions are located in same group both alkali metals [5] [OVER] PHYSICAL SETTING/CHEMISTRY continued 63 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: H H H C C C C H H H Br Br H H Br C C C C Br CH CH Br CH3 CH3 Br CH3CHBr CHBr CH3 64 + 0 [1] Allow 1 credit for+0 1e or +1 or or positron. [6] PHYSICAL SETTING/CHEMISTRY continued Part C Allow a total of 21 credits for this part. The student must answer all questions in this part. 65 [1] Allow 1 credit for a correct numerical setup. Acceptable responses include, but are not limited to, these examples: 8.40 g 1 mole = 58.3 g 8.4 58.3 66 [1] Allow 1 credit for 0.025. 67 [1] Allow 1 credit for NaHCO3. 68 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Naphthalene has weak intermolecular forces. They are weak. 69 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Naphthalene is nonpolar; water is polar. Nonpolar won t dissolve in polar. Like dissolves like. 70 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: C10H8 H8C10 [7] [OVER] PHYSICAL SETTING/CHEMISTRY continued 71 and 72 An example of a correct response is shown below. Solubility Curve 50 Solute per 100 g of H2O(g) 40 30 20 10 0 10 20 30 40 50 60 70 80 90 100 Temperature ( C) 71 [1] Allow 1 credit for marking an appropriate scale. An appropriate scale is one that allows a trend to be seen. 72 [1] Allow 1 credit for plotting all the points correctly ( 0.3 grid space). Plotted points do not need to be circled or connected. 73 [1] Allow 1 credit for 9. 74 [1] Allow 1 credit for a response in the range of 6 8. [8] PHYSICAL SETTING/CHEMISTRY continued 75 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Particles move slower. The molecules will slow down as the temperature decreases. The average kinetic energy of the particles decreases. decreases 76 [1] Allow 1 credit for a correct numerical setup. Acceptable responses include, but are not limited to, these examples: (100.8 kPa)(52.5 L) (45.6 kPa)(X) = (295 K) (252 K) 52.5 252 100.8 295 45.6 77 [1] Allow 1 credit for 21. 78 [1] Allow 1 credit for .45 or 0.45. Significant figures do not need to be shown. 79 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Removing CO2 disrupts equilibrium and thus the system must shift to create more CO2 from the H2CO3 in order to restore equilibrium. Equilibrium shifts to the right. H2CO3 decreases to remove the stress of changing the CO2. 80 [1] Allow 1 credit for +4 or 4. 81 [1] Allow 1 credit for a correct response. Brackets do not need to be shown. Acceptable responses include, but are not limited to, this example: [F] [9] [OVER] PHYSICAL SETTING/CHEMISTRY concluded 82 [1] Allow 1 credit for SnF2. 83 [1] Allow 1 credit for 1.43. Significant figures do not need to be shown. 84 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: The water has a fluoride level of 1.43 ppm, which is below the maximum contaminant level for fluoride, so it is safe to drink. F below 4 ppm, safe, below max level Safe: 1.43 ppm < 4 ppm or Allow 1 credit for a response consistent with the student s answer to question 83. 85 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these examples: Perform tests under ventilation (fume) hood. Avoid spills. no open-toed shoes [10] The Chart for Determining the Final Examination Score for the June 2004 Regents Examination in Physical Setting/Chemistry will be posted on the Department s web site http://www.emsc.nysed.gov/osa/ on Wednesday, June 23, 2004. Conversion charts provided for previous administrations of the Regents Examination in Physical Setting/Chemistry must NOT be used to determine students final scores for this administration. [11] [OVER] Map to Core Curriculum Key Ideas 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 June 2004 Physical Setting/ Chemistry Question Numbers Part A Part B Standard 1 58 Part C 71,72,77,78 52,62 41,49,61 85 67,74,80,82 Standard 2 Key Idea 1 Key Idea 2 41,49 Standard 6 Key Idea 1 Key Idea 2 Key Idea 3 Key Idea 4 Key Idea 5 Standard 7 Key Idea 1 Key Idea 2 Key Idea 3 Key Idea 4 84 Standard 4 Process Skills 34,35,36,37,38, 42,43,44,45,46, 47,48,50,51,53, 54,55,56,57,59, 60,63 40,49,64 Key Idea 5 Key Idea 3 39,41 Standard 4 1,2,3,4,5,6,7,8, 14,16,18,19,20, 21,22,23,24,25, 26,27,28,29,30, 31,33 Key Idea 4 15 Key Idea 5 9,10,11,12,13, 17,32 2002 Edition 65,66,69,70,73, 74,75,76,79,83 68,81 34,35,36,37,38, 42,43,44,45,46, 47,48,50,51,52, 53,54,55,56,57, 58,59,60,61,62, 63 40,49,64 65,66,67,69,70, 71,72,73,74,75, 76,78,79,80,82, 83,84,85 34,39,41 68,81 Reference Tables 2,4,5,8,10,11, 34,35,37,39,41, 13,23,24,25,26, 48,49,50,54,56, 31 57 [12] 77 67,74,76,77,78, 80,81,82,83

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