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New York Regents Chemistry June 2013

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P.S./CHEMISTRY The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY Tuesday, June 18, 2013 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 According to the wave-mechanical model of the atom, an orbital is a region of the most probable location of (1) an alpha particle (3) an electron (2) a gamma ray (4) a proton 6 Which substances have atoms of the same element but different molecular structures? (1) He(g) and Ne(g) (3) K(s) and Na(s) (2) O2(g) and O3(g) (4) P4(s) and S8(s) 7 An atom that has 13 protons and 15 neutrons is an isotope of the element (1) nickel (3) aluminum (2) silicon (4) phosphorus 2 Which particles have approximately the same mass? (1) an electron and an alpha particle (2) an electron and a proton (3) a neutron and an alpha particle (4) a neutron and a proton 8 Which elements have the most similar chemical properties? (1) Si, As, and Te (3) Mg, Sr, and Ba (2) N2, O2, and F2 (4) Ca, Cs, and Cu 3 During a flame test, a lithium salt produces a characteristic red flame. This red color is produced when electrons in excited lithium atoms (1) are lost by the atoms (2) are gained by the atoms (3) return to lower energy states within the atoms (4) move to higher energy states within the atoms 9 Which list includes three types of chemical formulas for organic compounds? (1) covalent, metallic, isotopic (2) covalent, metallic, molecular (3) empirical, structural, isotopic (4) empirical, structural, molecular 4 Compared to the energy and charge of the electrons in the first shell of a Be atom, the electrons in the second shell of this atom have (1) less energy and the same charge (2) less energy and a different charge (3) more energy and the same charge (4) more energy and a different charge 10 In a bond between an atom of carbon and an atom of fluorine, the fluorine atom has a (1) weaker attraction for electrons (2) stronger attraction for electrons (3) smaller number of first-shell electrons (4) larger number of first-shell electrons 5 Which quantity can vary among atoms of the same element? (1) mass number (2) atomic number (3) number of protons (4) number of electrons P.S./Chem. June 13 11 A sample of CO2(s) and a sample of CO2(g) differ in their (1) chemical compositions (2) empirical formulas (3) molecular structures (4) physical properties [2] 12 Which statement defines the temperature of a sample of matter? (1) Temperature is a measure of the total electromagnetic energy of the particles. (2) Temperature is a measure of the total thermal energy of the particles. (3) Temperature is a measure of the average potential energy of the particles. (4) Temperature is a measure of the average kinetic energy of the particles. 18 Powdered sulfur is yellow, and powdered iron is gray. When powdered sulfur and powdered iron are mixed at 20 C, the powdered iron (1) becomes yellow (3) remains ionic (2) becomes a liquid (4) remains magnetic 19 An effective collision between reactant particles requires the particles to have the proper (1) charge and mass (2) charge and orientation (3) energy and mass (4) energy and orientation 13 For a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is equal to the (1) heat of fusion (2) heat of reaction (3) activation energy of the forward reaction (4) activation energy of the reverse reaction 20 Which term is defined as a measure of the disorder of a system? (1) heat (3) kinetic energy (2) entropy (4) activation energy 21 Which process is used to determine the concentration of an acid? (1) chromatography (3) electrolysis (2) distillation (4) titration 14 Which equation represents sublimation? (1) Hg( ) Hg(s) (3) NH3(g) NH3( ) (2) H2O(s) H2O(g) (4) CH4( ) CH4(g) 15 Which statement describes the particles of an ideal gas, based on the kinetic molecular theory? (1) The motion of the gas particles is orderly and circular. (2) The gas particles have no attractive forces between them. (3) The gas particles are larger than the distances separating them. (4) As the gas particles collide, the total energy of the system decreases. 22 The compounds CH3OCH3 and CH3CH2OH have different functional groups. Therefore, these compounds have different (1) chemical properties (2) gram-formula masses (3) percent compositions by mass (4) numbers of atoms per molecule 23 Which term identifies the occurs at the anode of an chemical cell? (1) oxidation (3) (2) reduction (4) 16 Two grams of potassium chloride are completely dissolved in a sample of water in a beaker. This solution is classified as (1) an element (2) a compound (3) a homogeneous mixture (4) a heterogeneous mixture neutralization transmutation 24 During the operation of a voltaic cell, the cell produces (1) electrical energy spontaneously (2) chemical energy spontaneously (3) electrical energy nonspontaneously (4) chemical energy nonspontaneously 17 Which compound has the strongest hydrogen bonding between its molecules? (1) HBr (3) HF (2) HCl (4) HI P.S./Chem. June 13 half-reaction that operating electro- [3] [OVER] 25 In which type of chemical reaction are electrons transferred? (1) organic addition (2) oxidation-reduction (3) double replacement (4) acid-base neutralization 28 Which compound is an electrolyte? (3) C6H12O6 (1) CCl4 (2) CH3OH (4) Ca(OH)2 29 Which term identifies a type of nuclear reaction? (1) fermentation (3) reduction (2) deposition (4) fission 26 A substance that dissolves in water and produces hydronium ions as the only positive ions in the solution is classified as (1) an alcohol (3) a base (2) an acid (4) a salt 30 Which radioisotopes have the same decay mode and have half-lives greater than 1 hour? (1) Au-198 and N-16 (3) I-131 and P-32 (2) Ca-37 and Fe-53 (4) Tc-99 and U-233 27 According to one acid-base theory, a base is an (1) H acceptor (3) Na acceptor (2) H donor (4) Na donor P.S./Chem. June 13 [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 The diagram below represents the bright-line spectra of four elements and a bright-line spectrum produced by a mixture of three of these elements. Bright-Line Spectra 400 500 600 700 750 500 600 700 750 Element A Element D Element X Element Z Mixture 400 Wavelength (nm) Which element is not present in the mixture? (1) A (3) X (2) D (4) Z 32 What is the overall charge of an ion that has 12 protons, 10 electrons, and 14 neutrons? (1) 2 (3) 4 (2) 2 (4) 4 34 Which electron configuration represents the electrons of a sulfur atom in an excited state? (1) 2-6-6 (3) 2-8-4 (2) 2-7-7 (4) 2-8-6 33 As the elements in Period 3 are considered in order of increasing atomic number, there is a general decrease in (1) atomic mass (2) atomic radius (3) electronegativity (4) first ionization energy 35 Given the word equation: P.S./Chem. June 13 sodium chlorate sodium chloride oxygen Which type of chemical reaction is represented by this equation? (1) double replacement (3) decomposition (2) single replacement (4) synthesis [5] [OVER] 36 Which compound has the highest percent composition by mass of strontium? (1) SrCl2 (3) SrO (2) SrI2 (4) SrS 42 Which particle diagram represents a sample of matter that can not be broken down by chemical means? Key = atom of one element 37 Given the formula for hydrazine: = atom of a different element H H N N H H How many pairs of electrons are shared between the two nitrogen atoms? (1) 1 (3) 3 (2) 2 (4) 4 (1) (3) (2) (4) 38 Which formulas represent one ionic compound and one molecular compound? (1) N2 and SO2 (3) BaCl2 and N2O4 (2) Cl2 and H2S (4) NaOH and BaSO4 39 Which Kelvin temperature is equal to 200. C? (1) 73 K (3) 200. K (2) 73 K (4) 473 K 43 Which formula represents an unsaturated hydrocarbon? 40 A 10.0-gram sample of H2O( ) at 23.0 C absorbs 209 joules of heat. What is the final temperature of the H2O( ) sample? (1) 5.0 C (3) 28.0 C (2) 18.0 C (4) 50.0 C H H2O H H H C C C H C (2) OH (3) H H [6] H H H H Ag (aq) Cl (aq) When the concentration of Cl (aq) is increased, the concentration of Ag (aq) (1) decreases, and the amount of AgCl(s) increases (2) decreases, and the amount of AgCl(s) decreases (3) increases, and the amount of AgCl(s) increases (4) increases, and the amount of AgCl(s) decreases P.S./Chem. June 13 C H (1) 41 Given the equation representing a system at equilibrium: AgCl(s) C H H H H H O C C H (4) H 44 When the pH of a solution is changed from 4 to 3, the hydronium ion concentration of the solution (1) decreases by a factor of 10 (2) increases by a factor of 10 (3) decreases by a factor of 100 (4) increases by a factor of 100 48 Given the equation representing a nuclear reaction in which X represents a nuclide: 232 90 Th 4 2 He X Which nuclide is represented by X? (1) 236 92 U 228 88Ra (4) 228 88 U 1 __ 49 After decaying for 48 hours, 16 of the original mass of a radioisotope sample remains unchanged. What is the half-life of this radioisotope? (1) 3.0 h (3) 12 h (2) 9.6 h (4) 24 h 46 A 10.0-milliliter sample of NaOH(aq) is neutralized by 40.0 milliliters of 0.50 M HCl. What is the molarity of the NaOH(aq)? (1) 1.0 M (3) 0.25 M (2) 2.0 M (4) 0.50 M 50 Which balanced equation represents nuclear fusion? 2 2 4 (1) 1 H 1 H 2 He (2) 2H2 O2 2H2O 47 Radiation is spontaneously emitted from hydrogen-3 nuclei, but radiation is not spontaneously emitted from hydrogen-1 nuclei or hydrogen-2 nuclei. Which hydrogen nuclei are stable? (1) nuclei of H-1 and H-2, only (2) nuclei of H-1 and H-3, only (3) nuclei of H-2 and H-3, only (4) nuclei of H-1, H-2, and H-3 P.S./Chem. June 13 (3) (2) 45 Three samples of the same solution are tested, each with a different indicator. All three indicators, bromthymol blue, bromcresol green, and thymol blue, appear blue if the pH of the solution is (1) 4.7 (3) 7.8 (2) 6.0 (4) 9.9 236 92 Ra 6 1 3 4 (3) 3 Li 0 n 1 H 2 He (4) CaO CO2 CaCO3 [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. Base your answers to questions 51 through 53 on the information below and on your knowledge of chemistry. When magnesium is ignited in air, the magnesium reacts with oxygen and nitrogen. The reaction between magnesium and nitrogen is represented by the unbalanced equation below. Mg(s) N2(g) Mg3N2(s) 51 Balance the equation in your answer booklet for the reaction between magnesium and nitrogen, using the smallest whole-number coefficients. [1] 52 In the ground state, which noble gas has atoms with the same electron configuration as a magnesium ion? [1] 53 Explain, in terms of electrons, why an atom of the metal in this reaction forms an ion that has a smaller radius than its atom. [1] Base your answers to questions 54 through 56 on the information below and on your knowledge of chemistry. The balanced equation below represents a reaction. O2(g) energy O(g) O(g) 54 Identify the type of chemical bond in a molecule of the reactant. [1] 55 In the space in your answer booklet, draw a Lewis electron-dot diagram of one oxygen atom. [1] 56 Explain, in terms of bonds, why energy is absorbed during this reaction. [1] P.S./Chem. June 13 [8] Base your answers to questions 57 through 59 on the information below and on your knowledge of chemistry. Starting as a solid at 25 C, a sample of H2O is heated at a constant rate until the sample is at 125 C. This heating occurs at standard pressure. The graph below represents the relationship between temperature and heat added to the sample. Heating Curve for H2O 125 F D 100. E 75 50. 25 0 B C 25 A 4 12 20. 28 36 44 52 60. Heat Added (kJ) 57 Describe what happens to both the potential energy and the average kinetic energy of the molecules in the H2O sample during interval AB. [1] 58 Using the graph, determine the total amount of heat added to the sample during interval CD. [1] 59 Explain, in terms of heat of fusion and heat of vaporization, why the heat added during interval DE is greater than the heat added during interval BC for this sample of water. [1] P.S./Chem. June 13 [9] [OVER] Base your answers to questions 60 through 62 on the information below and on your knowledge of chemistry. Cylinder A has a movable piston and contains hydrogen gas. An identical cylinder, B, contains methane gas. The diagram below represents these cylinders and the conditions of pressure, volume, and temperature of the gas in each cylinder. Cylinder A Cylinder B Hydrogen gas P = 1.2 atm V = 1.25 L T = 293 K Methane gas P = 1.2 atm V = 1.25 L T = 293 K 60 Compare the total number of gas molecules in cylinder A to the total number of gas molecules in cylinder B. [1] 61 State a change in temperature and a change in pressure that will cause the gas in cylinder A to behave more like an ideal gas. [1] 62 In the space in your answer booklet, show a numerical setup for calculating the volume of the gas in cylinder B at STP. [1] P.S./Chem. June 13 [10] Base your answers to questions 63 through 65 on the information below and on your knowledge of chemistry. There are several isomers of C6H14. The formulas and boiling points for two of these isomers are given in the table below. Isomer Formula Boiling Point at 1 atm ( C) H H H H H H C C C C C C H 1 H H H H H H H 68.7 H H 2 H C H H C H C H C H H H C C H H H 49.7 H 63 Identify the homologous series to which these isomers belong. [1] 64 Write the empirical formula for isomer 1. [1] 65 Explain, in terms of intermolecular forces, why isomer 2 boils at a lower temperature than isomer 1. [1] P.S./Chem. June 13 [11] [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. Before atomic numbers were known, Mendeleev developed a classification system for the 63 elements known in 1872, using oxide formulas and atomic masses. He used an R in the oxide formulas to represent any element in each group. The atomic mass was listed in parentheses after the symbol of each element. A modified version of Mendeleev s classification system is shown in the table below. Modified Version of Mendeleev s Table Group I Oxide formulas II III IV V VI VII R2O RO R2O3 RO2 R2O5 RO3 R2O7 H(1) 2 Li(7) Be(9.4) B(11) C(12) N(14) O(16) F(19) 3 Na(23) Mg(24) Al(27.3) Si(28) P(31) S(32) Cl(35.5) 4 K(39) Ca(40) Ti(48) V(51) Cr(52) Mn(55) 5 Cu(63) Zn(65) As(75) Se(78) Br(80) 6 Rb(85) Sr(87) Yt(88) Zr(90) Nb(94) Mo(96) 7 Ag(108) Cd(112) In(113) Sn(118) Sb(122) Te(125) 8 Series 1 Cs(133) Ba(137) Di(138) Ce(140) I(127) 66 Identify one characteristic used by Mendeleev to develop his classification system of the elements. [1] 67 Based on Mendeleev s oxide formula, what is the number of electrons lost by each atom of the elements in Group III? [1] 68 Based on Table J, identify the least active metal listed in Group I on Mendeleev s table. [1] 69 Explain, in terms of chemical reactivity, why the elements in Group 18 on the modern Periodic Table were not identified by Mendeleev at that time. [1] P.S./Chem. June 13 [12] Base your answers to questions 70 through 73 on the information below and on your knowledge of chemistry. In a laboratory apparatus, a sample of lead(II) oxide reacts with hydrogen gas at high temperature. The products of this reaction are liquid lead and water vapor. As the reaction proceeds, water vapor and excess hydrogen gas leave the glass tube. The diagram and balanced equation below represent this reaction. Glass tube H2O(g) and H2(g) H2(g) PbO(s) Pb( ) Laboratory burner PbO(s) + H2(g) + heat Pb( ) + H2O(g) 70 Determine the change in oxidation number for the hydrogen that reacts. [1] 71 Write a balanced half-reaction equation for the reduction of the Pb2 ions in this reaction. [1] 72 Explain why the reaction that occurs in this glass tube can not reach equilibrium. [1] 73 State one change in reaction conditions, other than adding a catalyst, that would cause the rate of this reaction to increase. [1] P.S./Chem. June 13 [13] [OVER] Base your answers to questions 74 through 77 on the information below and on your knowledge of chemistry. In the late 19th century, the Hall-Herroult process was invented as an inexpensive way to produce aluminum. In this process, Al2O3( ) extracted from bauxite is dissolved in Na3AlF6( ) in a graphite-lined tank, as shown in the diagram below. The products are carbon dioxide and molten aluminum metal. Hall-Heroult Process Power source Graphite rod Graphite-lined tank 74 Compare the chemical properties of a 300.-kilogram sample of Al2O3( ) with the chemical properties of a 600.-kilogram sample of Al2O3( ). [1] 75 Write the chemical name for the liquid compound dissolved in the Na3AlF6( ). [1] 76 What is the melting point of the substance that collects at the bottom of the tank? [1] 77 Compare the density of the Al( ) with the density of the mixture of Al2O3( ) and Na3AlF6( ). [1] Base your answers to questions 78 through 80 on the information below and on your knowledge of chemistry. One process used to manufacture sulfuric acid is called the contact process. One step in this process, the reaction between sulfur dioxide and oxygen, is represented by the forward reaction in the system at equilibrium shown below. 2SO2(g) O2(g) 2SO3(g) 394 kJ A mixture of platinum and vanadium(V) oxide may be used as a catalyst for this reaction. The sulfur trioxide produced is then used to make sulfuric acid. 78 Determine the amount of energy released when 1.00 mole of sulfur trioxide is produced. [1] 79 Write the chemical formula for vanadium(V) oxide. [1] 80 On the labeled axes in your answer booklet, complete the potential energy diagram for the forward reaction represented by this equation. [1] P.S./Chem. June 13 [14] Base your answers to questions 81 and 82 on the information below and on your knowledge of chemistry. Two very stable compounds, Freon-12 and Freon-14, are used as liquid refrigerants. A Freon-12 molecule consists of one carbon atom, two chlorine atoms, and two fluorine atoms. A Freon-14 molecule consists of one carbon atom and four fluorine atoms. 81 In the space in your answer booklet, draw a structural formula for Freon-12. [1] 82 To which class of organic compounds do Freon-12 and Freon-14 belong? [1] Base your answers to questions 83 through 85 on the information below and on your knowledge of chemistry. Chemical concepts are applied in candy making. A recipe for making lollipops is shown below. Hard-Candy Lollipops Recipe Ingredients: 414 grams of sugar 177 grams of water 158 milliliters of light corn syrup Step 1: In a saucepan, mix the sugar and water. Heat this mixture, while stirring, until all of the sugar dissolves. Step 2: Add the corn syrup and heat the mixture until it boils. Step 3: Continue boiling the mixture until the temperature reaches 143 C at standard pressure. Step 4: Remove the pan from the heat and allow it to stand until the bubbling stops. Pour the mixture into lollipop molds that have been coated with cooking oil spray. 83 Explain, in terms of the polarity of sugar molecules, why the sugar dissolves in water. [1] 84 Determine the concentration, expressed as percent by mass, of the sugar dissolved in the mixture produced in step 1. [1] 85 Explain, in terms of the concentration of sugar molecules, why the boiling point of the mixture in step 3 increases as water evaporates from the mixture. [1] P.S./Chem. June 13 [15] 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 18, 2013 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 .....3..... 9 .....4..... 17 . . . . . 3 . . . . . 25 . . . . . 2 . . . . . 2 .....4..... 10 . . . . . 2 . . . . . 18 . . . . . 4 . . . . . 26 . . . . . 2 . . . . . 3 .....3..... 11 . . . . . 4 . . . . . 19 . . . . . 4 . . . . . 27 . . . . . 1 . . . . . 4 .....3..... 12 . . . . . 4 . . . . . 20 . . . . . 2 . . . . . 28 . . . . . 4 . . . . . 5 .....1..... 13 . . . . . 2 . . . . . 21 . . . . . 4 . . . . . 29 . . . . . 4 . . . . . 6 .....2..... 14 . . . . . 2 . . . . . 22 . . . . . 1 . . . . . 30 . . . . . 3 . . . . . 7 .....3..... 15 . . . . . 2 . . . . . 23 . . . . . 1 . . . . . 8 .....3..... 16 . . . . . 3 . . . . .. 24 . . . . . 1 . . . . . Part B 1 31 . . . . . 3 . . . . . 36 . . . . . 3 . . . . . 41 . . . . . 1 . . . . . 46 . . . . . 2 . . . . . 32 . . . . . 2 . . . . . 37 . . . . . 1 . . . . . 42 . . . . . 4 . . . . . 47 . . . . . 1 . . . . . 33 . . . . . 2 . . . . . 38 . . . . . 3 . . . . . 43 . . . . . 2 . . . . . 48 . . . . . 2 . . . . . 34 . . . . . 2 . . . . . 39 . . . . . 4 . . . . . 44 . . . . . 2 . . . . . 49 . . . . . 3 . . . . . 35 . . . . . 3 . . . . . 40 . . . . . 3 . . . . . 45 . . . . . 4 . . . . . 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 18, 2013. 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 13 [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 for ___ 3 Mg(s) ___ N2(g) ___ Mg3N2(s). Allow credit even if the coefficient 1 is written in front of N2(g) and/or Mg3N2(s). 52 [1] Allow 1 credit for Ne or neon. 53 [1] Allow 1 credit. Acceptable responses include, but are not limited to: An atom of magnesium loses its outer shell electrons to form the Mg2+ ion. The electron configuration of a magnesium atom is 2-8-2, and the electron configuration of the magnesium ion is 2-8. An atom of the metal loses electrons to form the ion. 54 [1] Allow 1 credit. Acceptable responses include, but are not limited to: covalent double covalent nonpolar double 55 [1] Allow 1 credit. Examples of 1-credit responses: O XX X OX X X O P.S./Chem. Rating Guide June 13 [3] 56 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Energy is needed to break the bonds in O2. 57 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The potential energy remains the same, but the average kinetic energy of the H2O molecules increases. There is no change in potential energy. There is an increase in the average kinetic energy. 58 [1] Allow 1 credit for 8 kJ 1 kJ. 59 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The heat of vaporization of water is 2260 J/g and the heat of fusion for water is only 334 J/g. The heat of fusion of water is much less than its heat of vaporization. 60 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The number of gas molecules in cylinder A is the same as the number of gas molecules in cylinder B. 61 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Temperature: above 293 K Pressure: below 1.2 atm Temperature: higher Pressure: lower 62 [1] Allow 1 credit. Acceptable responses include, but are not limited to: (1.2 atm)(1.25 L) (1.0 atm)(V2 ) 293 K 273 K (27 73)(1.2)(1.25) 293 P.S./Chem. Rating Guide June 13 [4] 63 [1] Allow 1 credit. Acceptable responses include, but are not limited to: alkanes CnH2n 2 64 [1] Allow 1 credit for C3H7. The order of the elements can vary. 65 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Isomer 2 boils at a lower temperature because it has weaker intermolecular forces than isomer 1. The intermolecular forces in isomer 1 are stronger. P.S./Chem. Rating Guide June 13 [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: increasing atomic mass atomic mass oxide formulas 67 [1] Allow 1 credit. Acceptable responses include, but are not limited to: three electrons three 3 68 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Ag silver 69 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Since the Group 18 elements tend not to react with other elements, there were no oxide compounds for Mendeleev to study. Group 18 elements are generally unreactive. 70 [1] Allow 1 credit. Acceptable responses include, but are not limited to: From 0 to 1 From zero to one 71 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Pb2 2e Pb 72 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The glass tube is not a closed system. Gases are entering and leaving the system. The reaction is not reversible under these conditions. P.S./Chem. Rating Guide June 13 [6] 73 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Increase the temperature. Increase the concentration of the hydrogen gas in the tube. Grind the metal oxide to increase its surface area. 74 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Both samples have the same chemical properties. 75 [1] Allow 1 credit. Acceptable responses include, but are not limited to: aluminum oxide 76 [1] Allow 1 credit for 933 K. 77 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The density of the aluminum is greater than the density of the Al2O3 and Na3AlF6 mixture. The density of Al( ) is greater. 78 [1] Allow 1 credit for 197 kJ. 79 [1] Allow 1 credit. Acceptable responses include, but are not limited to: V2O5 O5V2 80 [1] Allow 1 credit. Potential Energy Example of a 1-credit response: Reaction Coordinate P.S./Chem. Rating Guide June 13 [7] 81 [1] Allow 1 credit. Examples of 1-credit responses: Cl F C F CI Cl F C Cl F 82 [1] Allow 1 credit. Acceptable responses include, but are not limited to: halide halocarbon 83 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The polarity of sugar molecules is similar to the polarity of water molecules. Both substances consist of polar molecules. 84 [1] Allow 1 credit for 70.1%. Significant figures do not need to be shown. 85 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The boiling point of the mixture increases as water evaporates because the concentration of dissolved molecules increases. An increase in the concentration of sugar particles increases the boiling point. P.S./Chem. Rating Guide June 13 [8] Regents Examination in Physical Setting/Chemistry June 2013 Chart for Converting Total Test Raw Scores to Final Examination Scores (Scale Scores) The Chart for Determining the Final Examination Score for the June 2013 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 18, 2013. 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 13 [9] Map to Core Curriculum June 2013 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 39, 62 51, 58, 60 Math Key Idea 3 32, 36, 40, 46, 49, 53, 62, 64 33, 53, 54, 56, 59, 61, 63, 65 67, 70, 78, 79, 84 37, 38, 47, 50, 51, 53, 56, 60, 65 67, 69, 70, 75, 79, 82, 85 47 76 81 Science Inquiry Key Idea 1 Science Inquiry Key Idea 2 Science Inquiry Key Idea 3 66, 68, 69, 72, 73, 74, 77, 83, 85 Engineering Design Key Idea 1 Standard 2 Key Idea 1 Key Idea 2 Standard 6 Key Idea 1 Key Idea 2 Key Idea 3 Key Idea 4 Key Idea 5 34 44 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 13 Standard 4 Process Skills 31, 33, 34, 35, 39, 41, 42, 43, 45, 51, 55, 62, 63, 64 40, 48, 49, 57, 58, 59 52, 54, 65 Standard 4 1, 2, 3, 4, 5, 7, 8, 31, 32, 33, 34, 35, 9, 11, 15, 16, 18, 36, 41, 42, 43, 44, 19, 20, 21, 22, 23, 45, 46, 47, 51, 60, 24, 25, 26, 27, 28 61, 62, 63, 64 12, 13, 14, 29, 30 39, 40, 48, 49, 50, 57, 58, 59 6, 10, 17 37, 38, 52, 53, 54, 55, 56, 65 Reference Tables 2, 7, 8, 10, 17, 22, 33, 34, 36, 38, 39, 28, 30 40, 45, 46, 47, 48, 52, 53, 55, 59, 62, 63 [10] 66, 67, 68, 71, 81, 83, 84 78, 80, 82 66, 67, 68, 70, 71, 72, 73, 74, 75, 76, 77, 79, 81, 82, 83, 84, 85 78, 80 69 68, 69, 70, 71, 75, 76, 79, 81, 82, 84

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