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New York Regents Chemistry June 2014

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P.S./CHEMISTRY The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY Tuesday, June 24, 2014 9:15 a.m. to 12:15 p.m., only The possession or use of any communications device is strictly prohibited when taking this examination. If you have or use any communications device, no matter how briefly, your examination will be invalidated and no score will be calculated for you. 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 2011 Edition Reference Tables for Physical Setting/Chemistry. You are to answer all questions in all parts of this examination according to the directions provided in this examination booklet. A separate answer sheet for Part A and Part B 1 has been provided to you. Follow the instructions from the proctor for completing the student information on your answer sheet. Record your answers to the Part A and Part B 1 multiple-choice questions on this separate answer sheet. Record your answers for the questions in Part B 2 and Part C in your separate answer booklet. Be sure to fill in the heading on the front of your answer booklet. All answers in your answer booklet 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 or in your answer booklet as directed. When you have completed the examination, you must sign the statement printed on 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 2011 Edition Reference Tables for Physical Setting/Chemistry must be available for you to use while taking this examination. DO NOT OPEN THIS EXAMINATION BOOKLET UNTIL THE SIGNAL IS GIVEN. P.S./CHEMISTRY Part A Answer all questions in this part. Directions (1 30): For each statement or question, record on your 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 2011 Edition Reference Tables for Physical Setting/Chemistry. 1 Compared to the charge of a proton, the charge of an electron has (1) a greater magnitude and the same sign (2) a greater magnitude and the opposite sign (3) the same magnitude and the same sign (4) the same magnitude and the opposite sign 6 The atomic mass of magnesium is the weighted average of the atomic masses of (1) all of the artificially produced isotopes of Mg (2) all of the naturally occurring isotopes of Mg (3) the two most abundant artificially produced isotopes of Mg (4) the two most abundant naturally occurring isotopes of Mg 2 Which atom has the largest atomic radius? (1) potassium (3) francium (2) rubidium (4) cesium 7 Which element has atoms that can form halide ions? (1) iodine (3) strontium (2) silver (4) xenon 3 In the wave-mechanical model of the atom, an orbital is defined as (1) a region of the most probable proton location (2) a region of the most probable electron location (3) a circular path traveled by a proton around the nucleus (4) a circular path traveled by an electron around the nucleus 8 Two forms of solid carbon, diamond and graphite, differ in their physical properties due to the differences in their (1) atomic numbers (2) crystal structures (3) isotopic abundances (4) percent compositions 4 When an excited electron in an atom moves to the ground state, the electron (1) absorbs energy as it moves to a higher energy state (2) absorbs energy as it moves to a lower energy state (3) emits energy as it moves to a higher energy state (4) emits energy as it moves to a lower energy state 9 Which quantity can be calculated for a solid compound, given only the formula of the compound and the Periodic Table of the Elements? (1) the density of the compound (2) the heat of fusion of the compound (3) the melting point of each element in the compound (4) the percent composition by mass of each element in the compound 5 Which polyatomic ion is found in the compound represented by the formula NaHCO3? (1) acetate (3) hydrogen sulfate (2) hydrogen carbonate (4) oxalate P.S./Chem. June 14 10 Which terms identify types of chemical reactions? (1) decomposition and sublimation (2) decomposition and synthesis (3) deposition and sublimation (4) deposition and synthesis [2] 11 The greatest amount of energy released per gram of reactants occurs during a (1) redox reaction (2) fission reaction (3) substitution reaction (4) neutralization reaction 17 Which substance can not be broken down by a chemical change? (1) ammonia (3) propanal (2) ethanol (4) zirconium 18 According to Table I, which equation represents a change resulting in the greatest quantity of energy released? (1) 2C(s) 3H2(g) C2H6(g) (2) 2C(s) 2H2(g) C2H4(g) (3) N2(g) 3H2(g) 2NH3(g) (4) N2(g) O2(g) 2NO(g) 12 Which element has atoms with the strongest attraction for electrons in a chemical bond? (1) chlorine (3) fluorine (2) nitrogen (4) oxygen 13 Compared to the physical and chemical properties of the compound NO2, the compound N2O has (1) different physical properties and different chemical properties (2) different physical properties and the same chemical properties (3) the same physical properties and different chemical properties (4) the same physical properties and the same chemical properties 19 Which element is a liquid at STP? (1) bromine (3) francium (2) cesium (4) iodine 20 Which statement describes a reversible reaction at equilibrium? (1) The activation energy of the forward reaction must equal the activation energy of the reverse reaction. (2) The rate of the forward reaction must equal the rate of the reverse reaction. (3) The concentration of the reactants must equal the concentration of the products. (4) The potential energy of the reactants must equal the potential energy of the products. 14 Which phrase describes a molecule of CH4, in terms of molecular polarity and distribution of charge? (1) polar with an asymmetrical distribution of charge (2) polar with a symmetrical distribution of charge (3) nonpolar with an asymmetrical distribution of charge (4) nonpolar with a symmetrical distribution of charge 21 Given the balanced equation representing a reaction: O2 O O What occurs during this reaction? (1) Energy is absorbed as bonds are broken. (2) Energy is absorbed as bonds are formed. (3) Energy is released as bonds are broken. (4) Energy is released as bonds are formed. 15 Which sample of copper has atoms with the lowest average kinetic energy? (1) 10. g at 45 C (3) 30. g at 25 C (2) 20. g at 35 C (4) 40. g at 15 C 22 In terms of entropy and energy, systems in nature tend to undergo changes toward (1) lower entropy and lower energy (2) lower entropy and higher energy (3) higher entropy and lower energy (4) higher entropy and higher energy 16 Which change results in the formation of different substances? (1) burning of propane (2) melting of NaCl(s) (3) deposition of CO2(g) (4) solidification of water P.S./Chem. June 14 [3] [OVER] 23 Which term is defined as the difference between the potential energy of the products and the potential energy of the reactants in a chemical reaction? (1) activation energy (3) heat of fusion (2) thermal energy (4) heat of reaction 27 Which compound is an electrolyte? (1) CH3CHO (3) CH3COOH (2) CH3OCH3 (4) CH3CH2CH3 28 Which statement describes one acid-base theory? (1) An acid is an H acceptor, and a base is an H donor. (2) An acid is an H donor, and a base is an H acceptor. (3) An acid is an H acceptor, and a base is an H donor. (4) An acid is an H donor, and a base is an H acceptor. 24 What is the atomic number of the element whose atoms bond to each other in chains, rings, and networks? (1) 10 (3) 6 (2) 8 (4) 4 25 How many pairs of electrons are shared between two adjacent carbon atoms in a saturated hydrocarbon? (1) 1 (3) 3 (2) 2 (4) 4 29 Which compounds are classified as Arrhenius acids? (1) HCl and NaOH (2) HNO3 and NaCl (3) NH3 and H2CO3 (4) HBr and H2SO4 26 Given the balanced equation representing a reaction: 4Al(s) 3O2(g) 2Al2O3(s) 30 Which statement describes the stability of the nuclei of potassium atoms? (1) All potassium atoms have stable nuclei that spontaneously decay. (2) All potassium atoms have unstable nuclei that do not spontaneously decay. (3) Some potassium atoms have unstable nuclei that spontaneously decay. (4) Some potassium atoms have unstable nuclei that do not spontaneously decay. As the aluminum loses 12 moles of electrons, the oxygen (1) gains 4 moles of electrons (2) gains 12 moles of electrons (3) loses 4 moles of electrons (4) loses 12 moles of electrons P.S./Chem. June 14 [4] Part B 1 Answer all questions in this part. Directions (31 50): For each statement or question, record on your 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 2011 Edition Reference Tables for Physical Setting/Chemistry. 31 Which notations represent different isotopes of the element sodium? (1) 32S and 34S (3) Na and Na0 2 6 (2) S and S (4) 22Na and 23Na 36 Which equation represents a single replacement reaction? (1) 2H2O2 2H2O O2 (2) 2H2 O2 2H2O (3) H2SO4 Mg H2 MgSO4 (4) HCl KOH KCl H2O 32 Which electron configuration represents the electrons in an atom of Ga in an excited state? (1) 2-8-17-3 (3) 2-8-18-3 (2) 2-8-17-4 (4) 2-8-18-4 37 The accepted value for the percent by mass of water in a hydrate is 36.0%. In a laboratory activity, a student determined the percent by mass of water in the hydrate to be 37.8%. What is the percent error for the student s measured value? (1) 5.0% (3) 1.8% (2) 4.8% (4) 0.05% 33 Which statement describes the general trends in electronegativity and first ionization energy as the elements in Period 3 are considered in order from Na to Cl? (1) Electronegativity increases, and first ionization energy decreases. (2) Electronegativity decreases, and first ionization energy increases. (3) Electronegativity and first ionization energy both increase. (4) Electronegativity and first ionization energy both decrease. 38 The boiling points, at standard pressure, of four compounds are given in the table below. Boiling Points of Four Compounds Compound Boiling Point ( C) H2O H2S 2.0 Which type of attraction can be used to explain the unusually high boiling point of H2O? (1) ionic bonding (2) hydrogen bonding (3) polar covalent bonding (4) nonpolar covalent bonding Al2(SO4)3 6NaOH 2Al(OH)3 3Na2SO4 The mole ratio of NaOH to Al(OH)3 is (1) 1:1 (3) 3:1 (2) 1:3 (4) 3:7 P.S./Chem. June 14 41.3 H2Te 35 Given the balanced equation representing a reaction: 59.6 H2Se 34 What is the gram-formula mass of Fe(NO3)3? (1) 146 g/mol (3) 214 g/mol (2) 194 g/mol (4) 242 g/mol 100.0 39 Which formula represents a molecule with the most polar bond? (1) CO (3) HI (2) NO (4) HCl [5] [OVER] Temperature 40 The graph below represents the uniform heating of a substance from the solid to the gas phase. 44 Given the equation representing a reaction at equilibrium: 2SO2(g) O2(g) 2SO3(g) heat Which change causes the equilibrium to shift to the right? (1) adding a catalyst (2) adding more O2(g) (3) decreasing the pressure (4) increasing the temperature F D E B C A 45 Given the formula representing a compound: H H Which line segment of the graph represents boiling? (1) AB (3) CD (2) BC (4) DE H C C C H H C C H H H What is a chemical name of this compound? (1) 2-pentene (3) 3-pentene (2) 2-pentyne (4) 3-pentyne 41 A 1-gram sample of a compound is added to 100 grams of H2O( ) and the resulting mixture is then thoroughly stirred. Some of the compound is then separated from the mixture by filtration. Based on Table F, the compound could be (1) AgCl (3) NaCl (2) CaCl2 (4) NiCl2 46 What is the oxidation number of manganese in KMnO4? (1) 7 (3) 3 (4) 4 (2) 2 47 When the pH of an aqueous solution is changed from 1 to 2, the concentration of hydronium ions in the solution is (1) decreased by a factor of 2 (2) decreased by a factor of 10 (3) increased by a factor of 2 (4) increased by a factor of 10 42 At standard pressure, the total amount of heat required to completely vaporize a 100.-gram sample of water at its boiling point is (1) 2.26 10 J (3) 2.26 103 J 2 (2) 2.26 10 J (4) 2.26 105 J 48 What is the color of the indicator thymol blue in a solution that has a pH of 11? (1) red (3) pink (2) blue (4) yellow 43 A sample of helium gas is in a sealed, rigid container. What occurs as the temperature of the sample is increased? (1) The mass of the sample decreases. (2) The number of moles of gas increases. (3) The volume of each atom decreases. (4) The frequency of collisions between atoms increases. P.S./Chem. June 14 H H Time [6] 49 Which formulas represent compounds that are isomers of each other? H H and H H H C H C H C H H H H C C C H H H H H H H OH H H and H C C C H O H H H (3) H C H H (1) HO and H H C H H H C C C H OH OH H H H (2) OH H H and H C C H H H (4) 50 One beneficial use of radioisotopes is (1) detection of disease (2) neutralization of an acid spill (3) decreasing the dissolved O2(g) level in seawater (4) increasing the concentration of CO2(g) in the atmosphere P.S./Chem. June 14 [7] [OVER] Part B 2 Answer all questions in this part. Directions (51 65): Record your answers in the spaces provided in your answer booklet. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry. 51 Draw a Lewis electron-dot diagram for a molecule of bromomethane, CH3Br. [1] 52 Explain, in terms of atomic structure, why Group 18 elements on the Periodic Table rarely form compounds. [1] 53 Explain, in terms of electrons, why the radius of a potassium atom is larger than the radius of a potassium ion in the ground state. [1] 54 Identify the type of bonding in solid potassium. [1] Base your answers to questions 55 and 56 on the information below and on your knowledge of chemistry. A 2.50-liter aqueous solution contains 1.25 moles of dissolved sodium chloride. The dissolving of NaCl(s) in water is represented by the equation below. HO 2 NaCl(s) Na (aq) Cl (aq) 55 Determine the molarity of this solution. [1] 56 Compare the freezing point of this solution to the freezing point of a solution containing 0.75 mole NaCl per 2.50 liters of solution. [1] Base your answers to questions 57 and 58 on the information below and on your knowledge of chemistry. A 1.00-mole sample of glucose, C6H12O6 , completely reacts with oxygen, as represented by the balanced equation below. C6H12O6(s) 6O2(g) 6CO2(g) 6H2O( ) energy 57 Write the empirical formula for glucose. [1] 58 Using the axes in your answer booklet, complete the potential energy curve for the reaction of glucose with oxygen. [1] P.S./Chem. June 14 [8] Base your answers to questions 59 through 61 on the information below and on your knowledge of chemistry. Ethane, C2H6, has a boiling point of 89 C at standard pressure. Ethanol, C2H5OH, has a much higher boiling point than ethane at standard pressure. At STP, ethane is a gas and ethanol is a liquid. 59 Identify the class of organic compounds to which ethanol belongs. [1] 60 A liquid boils when the vapor pressure of the liquid equals the atmospheric pressure on the surface of the liquid. Based on Table H, what is the boiling point of ethanol at standard pressure? [1] 61 Compare the intermolecular forces of the two substances at STP. [1] Base your answers to questions 62 through 65 on the information below and on your knowledge of chemistry. An operating voltaic cell has zinc and iron electrodes. The cell and the unbalanced ionic equation representing the reaction that occurs in the cell are shown below. Voltaic Cell V Wire Voltmeter Salt bridge Zn(s) electrode 2+ Fe(s) electrode 3+ Zn (aq) Fe (aq) 3+ 2+ Zn(s) + Fe (aq) Zn (aq) + Fe(s) 62 Identify the subatomic particles that flow through the wire as the cell operates. [1] 63 Balance the equation in your answer booklet for the redox reaction that occurs in this cell, using the smallest whole-number coefficients. [1] 64 Identify one metal from Table J that is more easily oxidized than Zn. [1] 65 Explain, in terms of Zn atoms and Zn ions, why the mass of the Zn electrode decreases as the cell operates. [1] P.S./Chem. June 14 [9] [OVER] Part C Answer all questions in this part. Directions (66 85): Record your answers in the spaces provided in your answer booklet. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry. Base your answers to questions 66 through 69 on the information below and on your knowledge of chemistry. A student compares some models of the atom. These models are listed in the table below in order of development from top to bottom. Models of the Atom Model Observation Conclusion Dalton model Matter is conserved during a chemical reaction. Atoms are hard, indivisible spheres of different sizes. Thomson model Cathode rays are deflected by magnetic/electric fields. Atoms have small, negatively charged particles as part of their internal structure. Rutherford model Most alpha particles pass straight through gold foil but a few are deflected. An atom is mostly empty space with a small, dense, positively charged nucleus. Bohr model Unique spectral lines are emitted by excited gaseous elements. Packets of energy are absorbed or emitted by atoms when an electron changes shells. 66 State the model that first included electrons as subatomic particles. [1] 67 State one conclusion about the internal structure of the atom that resulted from the gold foil experiment. [1] 68 Using the conclusion from the Rutherford model, identify the charged subatomic particle that is located in the nucleus. [1] 69 State one way in which the Bohr model agrees with the Thomson model. [1] P.S./Chem. June 14 [10] Base your answers to questions 70 through 72 on the information below and on your knowledge of chemistry. Paintball is a popular recreational activity that uses a metal tank of compressed carbon dioxide or nitrogen to launch small capsules of paint. A typical tank has a volume of 508 cubic centimeters. A 340.-gram sample of carbon dioxide is added to the tank before it is used for paintball. At 20. C, this tank contains both CO2(g) and CO2( ). After a paintball game, the tank contains only CO2(g). 70 Determine the total number of moles of CO2 added to the tank before it is used for paintball. [1] 71 In the box in your answer booklet, use the key to draw a particle diagram to represent the two phases of CO2 in a newly filled tank. Your response must include at least six molecules of CO2 in each phase. [1] 72 After the paintball game, the tank has a gas pressure of 6.1 atmospheres and is at 293 K. If the tank is heated to 313 K, the pressure in the tank will change. Show a numerical setup for calculating the pressure of the gas in the tank at 313 K. [1] Base your answers to questions 73 through 75 on the information below and on your knowledge of chemistry. Many breads are made by adding yeast to dough, causing the dough to rise. Yeast is a type of microorganism that produces the catalyst zymase, which converts glucose, C6H12O6, to ethanol and carbon dioxide gas. The balanced equation for this reaction is shown below. zymase C6H12O6(aq) _____ 2C2H5OH(aq) 2CO2(g) 73 Draw a structural formula for the ethanol formed during this reaction. [1] 74 Describe how the catalyst, zymase, speeds up this reaction. [1] 75 Determine the total mass of ethanol produced when 270. grams of glucose reacts completely to form ethanol and 132 grams of carbon dioxide. [1] P.S./Chem. June 14 [11] [OVER] Base your answers to questions 76 through 79 on the information below and on your knowledge of chemistry. During a laboratory activity, a student places 25.0 mL of HCl(aq) of unknown concentration into a flask. The student adds four drops of phenolphthalein to the solution in the flask. The solution is titrated with 0.150 M KOH(aq) until the solution appears faint pink. The volume of KOH(aq) added is 18.5 mL. 76 What number of significant figures is used to express the concentration of the KOH(aq)? [1] 77 Complete the equation in your answer booklet for the neutralization reaction that occurs during the titration. [1] 78 Determine the concentration of the HCl(aq) solution, using the titration data. [1] 79 Describe one laboratory safety procedure that should be used if a drop of the KOH(aq) is spilled on the arm of the student. [1] Base your answers to questions 80 through 82 on the information below and on your knowledge of chemistry. A few pieces of dry ice, CO2(s), at 78 C are placed in a flask that contains air at 21 C. The flask is sealed by placing an uninflated balloon over the mouth of the flask. As the balloon inflates, the dry ice disappears and no liquid is observed in the flask. 80 State the direction of heat flow that occurs between the dry ice and the air in the flask. [1] 81 Write the name of the process that occurs as the dry ice undergoes a phase change in the flask. [1] 82 Compare the entropy of the CO2 molecules in the dry ice to the entropy of the CO2 molecules in the inflated balloon. [1] P.S./Chem. June 14 [12] Base your answers to questions 83 through 85 on the information below and on your knowledge of chemistry. Illuminated EXIT signs are used in public buildings such as schools. If the word EXIT is green, the sign may contain the radioisotope tritium, hydrogen-3. The tritium is a gas sealed in glass tubes. The emissions from the decay of the tritium gas cause a coating on the inside of the tubes to glow. 83 State, in terms of neutrons, how an atom of tritium differs from an atom of hydrogen-1. [1] 84 Determine the fraction of an original sample of tritium that remains unchanged after 24.62 years. [1] 85 Complete the nuclear equation in your answer booklet for the radioactive decay of tritium, by writing a notation for the missing product. [1] P.S./Chem. June 14 [13] P.S./CHEMISTRY Printed on Recycled Paper P.S./CHEMISTRY FOR TEACHERS ONLY The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION P.S. CH PHYSICAL SETTING/CHEMISTRY Tuesday, June 24, 2014 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 2 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. Check this web site at: http://www.p12.nysed.gov/assessment/ and select the link Scoring Information for any recently posted information regarding this examination. This site should be checked before the rating process for this examination begins and several times throughout the Regents Examination period. Part A and Part B 1 Allow 1 credit for each correct response. Part A 1 .....4..... 9 .....4..... 17 . . . . . 4 . . . . . 25 . . . . . 1 . . . . . 2 .....3..... 10 . . . . . 2 . . . . . 18 . . . . . 3 . . . . . 26 . . . . . 2 . . . . . 3 .....2..... 11 . . . . . 2 . . . . . 19 . . . . . 1 . . . . . 27 . . . . . 3 . . . . . 4 .....4..... 12 . . . . . 3 . . . . . 20 . . . . . 2 . . . . . 28 . . . . . 2 . . . . . 5 .....2..... 13 . . . . . 1 . . . . . 21 . . . . . 1 . . . . . 29 . . . . . 4 . . . . . 6 .....2..... 14 . . . . . 4 . . . . . 22 . . . . . 3 . . . . . 30 . . . . . 3 . . . . . 7 .....1..... 15 . . . . . 4 . . . . . 23 . . . . . 4 . . . . . 8 .....2..... 16 . . . . . 1 . . . . .. 24 . . . . . 3 . . . . . Part B 1 31 . . . . . 4 . . . . . 36 . . . . . 3 . . . . . 41 . . . . . 1 . . . . . 46 . . . . . 1 . . . . . 32 . . . . . 2 . . . . . 37 . . . . . 1 . . . . . 42 . . . . . 4 . . . . . 47 . . . . . 2 . . . . . 33 . . . . . 3 . . . . . 38 . . . . . 2 . . . . . 43 . . . . . 4 . . . . . 48 . . . . . 2 . . . . . 34 . . . . . 4 . . . . . 39 . . . . . 4 . . . . . 44 . . . . . 2 . . . . . 49 . . . . . 3 . . . . . 35 . . . . . 3 . . . . . 40 . . . . . 4 . . . . . 45 . . . . . 1 . . . . . 50 . . . . . 1 . . . . . Directions to the Teacher Follow the procedures below for scoring student answer papers for the Regents Examination in Physical Setting/Chemistry. Additional information about scoring is provided in the publication Information Booklet for Scoring Regents Examinations in the Sciences. Do not attempt to correct the student s work by making insertions or changes of any kind. If the student s responses for the multiple-choice questions are being hand scored prior to being scanned, the scorer must be careful not to make any marks on the answer sheet except to record the scores in the designated score boxes. Marks elsewhere on the answer sheet will interfere with the accuracy of the scanning. Allow 1 credit for each correct response. At least two science teachers must participate in the scoring of the Part B 2 and Part C open-ended questions on a student s paper. 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 more than approximately one-half of the open-ended questions on a student s answer paper. Teachers may not score their own students answer papers. Students responses must be scored strictly according to the Scoring Key and Rating Guide. For openended 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. On the student s separate answer sheet, for each question, record the number of credits earned and the teacher s assigned rater/scorer letter. Fractional credit is not allowed. Only whole-number credit may be given for a response. If the student gives more than one answer to a question, only the first answer should be rated. Units need not be given when the wording of the questions allows such omissions. For hand scoring, raters should enter the scores earned in the appropriate boxes printed on the separate answer sheet. Next, the rater should add these scores and enter the total in the box labeled Total Raw Score. Then the student s raw score should be converted to a scale score by using the conversion chart that will be posted on the Department s web site at: http://www.p12.nysed.gov/assessment/ on Tuesday, June 24, 2014. The student s scale score should be entered in the box labeled Scale Score on the student s answer sheet. The scale score is the student s final examination score. Schools are not permitted to rescore any of the open-ended questions on this exam after each question has been rated once, regardless of the final exam score. Schools are required to ensure that the raw scores have been added correctly and that the resulting scale score has been determined accurately. Because scale scores corresponding to raw scores in the conversion chart may change from one administration to another, it is crucial that, for each administration, the conversion chart provided for that administration be used to determine the student s final score. P.S./Chem. Rating Guide June 14 [2] 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. The position of the electrons can vary. Examples of 1-credit responses: H H C Br H H H C H Br 52 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Group 18 elements rarely form compounds because their atoms have stable electron configurations. Their valence shells are completely filled. All the elements have maximum numbers of valence electrons. Atoms of Group 18 have a stable octet except He, which is stable with two electrons. 53 [1] Allow 1 credit. Acceptable responses include, but are not limited to: A potassium atom has four electron shells and a potassium ion has three electron shells. A potassium atom has one more electron shell than a potassium ion. A K ion has one fewer electron than a K atom. 54 [1] Allow 1 credit. Acceptable responses include, but are not limited to: metallic bonding metallic P.S./Chem. Rating Guide June 14 [3] 55 [1] Allow 1 credit. Acceptable responses include, but are not limited to: 0.500 M 0.50 M .5 M 56 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The solution that contains 1.25 moles of NaCl has a lower freezing point. lower for the first one higher for the solution with 0.75 mol The 0.30 M solution has a higher freezing point than the 0.50 M solution. This solution has a lower f.p. 57 [1] Allow 1 credit for CH2O. The order of the elements can vary. 58 [1] Allow 1 credit for showing both a peak that is higher than the beginning and the end of the curve and that the PE of the products is lower than the PE of the reactants. Potential Energy Example of a 1-credit response: Reaction Coordinate 59 [1] Allow 1 credit. Acceptable responses include, but are not limited to: alcohol alcohols primary alcohol monohydroxy alcohols P.S./Chem. Rating Guide June 14 [4] 60 [1] Allow 1 credit for any value from 78 C to 80. C, inclusive. 61 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Ethane has weaker intermolecular forces (IMF) than ethanol. Ethanol has hydrogen bonding. Van der Waals forces are weaker in C2H6. 62 [1] Allow 1 credit. Acceptable responses include, but are not limited to: electrons e e 3 Zn(s) _____ 2 Fe3 (aq) _____ 3 Zn2 (aq) _____ 2 Fe(s). 63 [1] Allow 1 credit for _____ 64 [1] Allow 1 credit for the symbol or name of any metal listed above Zn on Table J. 65 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Zinc atoms from the electrode are oxidized to zinc ions in the solution, decreasing the mass of the electrode. Zinc atoms become Zn2 (aq). The atoms become ions dissolved in the water. Zn atoms lose electrons, producing ions in solution. P.S./Chem. Rating Guide June 14 [5] Part C Allow a total of 20 credits for this part. The student must answer all questions in this part. 66 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Thomson model Thomson plum pudding model 67 [1] Allow 1 credit. Acceptable responses include, but are not limited to: An atom is mainly empty space. It has a nucleus. The small, dense nucleus is positively charged. 68 [1] Allow 1 credit. Acceptable responses include, but are not limited to: proton p p 1 1p 1 1H H 69 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Atoms have electrons. Atoms have small, negatively charged particles. Both models show an internal structure. Atoms are neutral. 70 [1] Allow 1 credit for 7.73 mol or for any value from 7.7 mol to 8 mol, inclusive. P.S./Chem. Rating Guide June 14 [6] 71 [1] Allow 1 credit. Molecules of the gas must be drawn farther apart than the molecules of the liquid. Examples of 1-credit responses: 72 [1] Allow 1 credit. Acceptable responses include, but are not limited to: 6.1 atm P2 313 K 293 K P2 6.1 atm 293 K 313 K (6.1)(508)(313) (293)(508) 73 [1] Allow 1 credit. Examples of 1-credit responses: H C C O H H H H H OH C C P.S./Chem. Rating Guide June 14 [7] 74 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Zymase is a catalyst that provides an alternative pathway, which requires less energy. decreases the activation energy changes the reaction mechanism 75 [1] Allow 1 credit for 138 g or for any value from 137.8 g to 138.3 g, inclusive. 76 [1] Allow 1 credit for 3 or three. 77 [1] Allow 1 credit. Acceptable responses include, but are not limited to: KCl(aq) H2O( ) K Cl OH2( ) HOH ClK 78 [1] Allow 1 credit. Acceptable responses include, but are not limited to: 0.111 M 0.11 M 0.1 M 79 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The student should immediately place his/her arm under running water to dilute and wash away the KOH(aq). Tell the teacher. 80 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Heat flows from the air in the flask to the dry ice. air to CO2 to dry ice from air P.S./Chem. Rating Guide June 14 [8] 81 [1] Allow 1 credit. Acceptable responses include, but are not limited to: sublimation subliming 82 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The CO2 molecules in the dry ice have less entropy than the CO2 molecules in the inflated balloon. The CO2 gas in the balloon is more disordered. less for CO2(s) 83 [1] Allow 1 credit. Acceptable responses include, but are not limited to: A tritium atom has two neutrons and an H-1 atom has no neutrons. Only the tritium atom has neutrons. H-1 has no neutrons. 84 [1] Allow 1 credit. Acceptable responses include, but are not limited to: 1 4 0.25 25% 85 [1] Allow 1 credit. Acceptable responses include, but are not limited to: 3 2He helium-3 He-3 3 He P.S./Chem. Rating Guide June 14 [9] Regents Examination in Physical Setting/Chemistry June 2014 Chart for Converting Total Test Raw Scores to Final Examination Scores (Scale Scores) The Chart for Determining the Final Examination Score for the June 2014 Regents Examination in Physical Setting/Chemistry will be posted on the Department s web site at: http://www.p12.nysed.gov/assessment/ on Tuesday, June 24, 2014. 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. Online Submission of Teacher Evaluations of the Test to the Department Suggestions and feedback from teachers provide an important contribution to the test development process. The Department provides an online evaluation form for State assessments. It contains spaces for teachers to respond to several specific questions and to make suggestions. Instructions for completing the evaluation form are as follows: 1. Go to http://www.forms2.nysed.gov/emsc/osa/exameval/reexameval.cfm. 2. Select the test title. 3. Complete the required demographic fields. 4. Complete each evaluation question and provide comments in the space provided. 5. Click the SUBMIT button at the bottom of the page to submit the completed form. P.S./Chem. Rating Guide June 14 [10] Map to Core Curriculum June 2014 Physical Setting/Chemistry Question Numbers Key Ideas/Performance Indicators Part A Standard 1 Part B Part C Math Key Idea 1 Math Key Idea 2 37 40, 47, 60, 63 71, 72, 76, 84 Math Key Idea 3 34, 35, 39, 42, 46, 55 52, 53, 54, 56, 59, 61, 62, 65 70, 75, 78, 85 Science Inquiry Key Idea 1 Science Inquiry Key Idea 2 Science Inquiry Key Idea 3 32, 35, 36, 38, 39, 41, 43, 45, 46, 48, 58, 59, 63, 65 66, 68, 69, 74, 80, 81, 83 79 66, 77, 85 Engineering Design Key Idea 1 Standard 2 Key Idea 1 Key Idea 2 Key Idea 3 33 68, 69 67 42 Standard 6 Key Idea 1 Key Idea 2 Key Idea 3 Key Idea 4 Key Idea 5 37 47 44 40 80 71 Standard 7 Key Idea 1 Key Idea 2 Key Idea 3 Key Idea 4 Key Idea 5 Key Idea 3 Key Idea 4 Key Idea 5 2011 Edition P.S./Chem. Rating Guide June 14 50 Standard 4 Process Skills 31, 32, 33, 34, 36, 44, 48, 49, 55, 57, 59, 62, 63, 64 40, 50, 58 38, 51, 61 Standard 4 1, 2, 3, 4, 6, 7, 9, 10, 13, 16, 17, 19, 20, 22, 24, 25, 26, 27, 28, 29, 30 31, 32, 33, 34, 35, 36, 37, 41, 43, 44, 45, 46, 47, 48, 49, 55, 56, 57, 59, 62, 63, 64, 65 15, 18, 23 40, 42, 50, 58 5, 8, 11, 12, 14, 21 38, 39, 51, 52, 53, 54, 60, 61 Reference Tables 1, 2, 5, 7, 9, 12, 31, 32, 33, 34, 37, 17, 18, 19, 24, 27, 39, 41, 42, 45, 46, 29, 30 48, 51, 52, 53, 54, 55, 59, 60, 64 [11] 66, 67, 68, 69, 70, 71, 72, 73, 75, 77, 78, 82, 83 84, 85 66, 67, 68, 69, 70, 71, 72, 73, 74, 75, 76, 77, 78, 79, 82, 83 80, 81, 84, 85 68, 70, 72, 73, 77, 78, 83, 84, 85

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