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New York Regents Chemistry January 2006

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PS/CHEMISTRY The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY Thursday, January 26, 2006 1:15 to 4:15 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 you to use while taking this examination. The use of any communications device is strictly prohibited when taking this examination. If you use any communications device, no matter how briefly, your examination will be invalidated and no score will be calculated for you. DO NOT OPEN THIS EXAMINATION BOOKLET UNTIL THE SIGNAL IS GIVEN. PS/CHEMISTRY Part A Answer all questions in this part. Directions (1 30): For each statement or question, write on the separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry. 1 Which two nuclides are isotopes of the same element? (1) 20 Na 11 (2) 39 19K and 20 10Ne and 40 20Ca (3) 39 K 19 and 42 19K (4) 14C 6 6 The element in Group 14, Period 3 on the Periodic Table is classified as a (1) metal (3) metalloid (2) noble gas (4) nonmetal and 14 7N 7 Which trends are observed when the elements in Period 3 on the Periodic Table are considered in order of increasing atomic number? (1) The atomic radius decreases, and the first ionization energy generally increases. (2) The atomic radius decreases, and the first ionization energy generally decreases. (3) The atomic radius increases, and the first ionization energy generally increases. (4) The atomic radius increases, and the first ionization energy generally decreases. 2 An atom of oxygen is in an excited state. When an electron in this atom moves from the third shell to the second shell, energy is (1) emitted by the nucleus (2) emitted by the electron (3) absorbed by the nucleus (4) absorbed by the electron 3 The charge of a beryllium-9 nucleus is (1) +13 (3) +5 (2) +9 (4) +4 8 What is the chemical formula for sodium sulfate? (1) Na2SO3 (3) NaSO3 (2) Na2SO4 (4) NaSO4 4 Which sequence represents a correct order of historical developments leading to the modern model of the atom? (1) the atom is a hard sphere most of the atom is empty space electrons exist in orbitals outside the nucleus (2) the atom is a hard sphere electrons exist in orbitals outside the nucleus most of the atom is empty space (3) most of the atom is empty space electrons exist in orbitals outside the nucleus the atom is a hard sphere (4) most of the atom is empty space the atom is a hard sphere electrons exist in orbitals outside the nucleus 9 Given the structural formula: H H H H HO C C C C OH H H What is the empirical formula of this compound? (1) CH3O (2) C2H5O 5 Which statement describes a chemical property of oxygen? (1) Oxygen has a melting point of 55 K. (2) Oxygen can combine with a metal to produce a compound. (3) Oxygen gas is slightly soluble in water. (4) Oxygen gas can be compressed. P.S./Chem. Jan. 06 H H (3) C4H10O2 (4) C8H20O4 10 Which chemical equation is correctly balanced? (1) (2) (3) (4) [2] H2(g) + O2(g) H2O(g) N2(g) + H2(g) NH3(g) 2NaCl(s) Na(s) + Cl2(g) 2KCl(s) 2K(s) + Cl2(g) 11 Compared to a calcium atom, the calcium ion Ca2+ has (1) more protons (3) more electrons (2) fewer protons (4) fewer electrons 18 Given the balanced equation: I2(s) + energy I2(g) As a sample of I2(s) sublimes to I2(g), the entropy of the sample (1) increases because the particles are less randomly arranged (2) increases because the particles are more randomly arranged (3) decreases because the particles are less randomly arranged (4) decreases because the particles are more randomly arranged 12 Which type of bond is found in sodium bromide? (1) covalent (3) ionic (2) hydrogen (4) metallic 13 Which substance can not be decomposed by ordinary chemical means? (1) methane (3) ethanol (2) mercury (4) ammonia 19 The multiple covalent bond in 1-butene is a (1) double covalent bond that electrons (2) double covalent bond that electrons (3) triple covalent bond that electrons (4) triple covalent bond that electrons 14 A mixture of crystals of salt and sugar is added to water and stirred until all solids have dissolved. Which statement best describes the resulting mixture? (1) The mixture is homogeneous and can be separated by filtration. (2) The mixture is homogeneous and cannot be separated by filtration. (3) The mixture is heterogeneous and can be separated by filtration. (4) The mixture is heterogeneous and cannot be separated by filtration. a molecule of has 6 shared has 4 shared has 6 shared has 4 shared 20 In an oxidation-reduction reaction, reduction is defined as the (1) loss of protons (3) loss of electrons (2) gain of protons (4) gain of electrons 15 Under which conditions of temperature and pressure would a sample of H2(g) behave most like an ideal gas? (1) 0 C and 100 kPa (2) 0 C and 300 kPa (3) 150 C and 100 kPa (4) 150 C and 300 kPa 21 What is the oxidation number assigned to manganese in KMnO4? (1) +7 (3) +3 (2) +2 (4) +4 22 Which of the following aqueous solutions is the best conductor of electricity? (3) 0.10 M NaOH (1) 0.10 M CH3OH (2) 1.0 M CH3OH (4) 1.0 M NaOH 16 In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is defined as the (1) activation energy (2) ionization energy (3) heat of reaction (4) heat of vaporization 23 One acid-base theory states that an acid is + (3) an H donor (1) an H donor + (2) an H acceptor (4) an H acceptor 17 Which substance is an Arrhenius base? (1) KCl (3) KOH (2) CH3Cl (4) CH3OH P.S./Chem. Jan. 06 [3] [OVER] 24 Positrons are spontaneously emitted from the nuclei of (1) potassium-37 (3) nitrogen-16 (2) radium-226 (4) thorium-232 28 Which structural formula is correct for 2-methyl-3-pentanol? H H H H 25 The amount of energy released from a fission reaction is much greater than the energy released from a chemical reaction because in a fission reaction (1) mass is converted into energy (2) energy is converted into mass (3) ionic bonds are broken (4) covalent bonds are broken H C C H H C C C H H H H H C C H H C H H H H H H OH C C C H H H H C H OH H (1) (3) H 26 Which Lewis electron-dot diagram is correct for CO2? H H (1) O C O H C C C H H H H H H H H C C C C H H H OH H C H H (4) Note that questions 29 and 30 have only three choices. 29 When an atom becomes a positive ion, the radius of the atom (1) decreases (2) increases (3) remains the same (4) 27 Types of nuclear reactions include fission, fusion, and (1) single replacement (2) neutralization (3) oxidation-reduction (4) transmutation P.S./Chem. Jan. 06 H (2) O C O (2) C H H H OH (3) O C O C H H O C O C 30 Compared to the freezing point of 1.0 M KCl(aq) at standard pressure, the freezing point of 1.0 M CaCl2(aq) at standard pressure is (1) lower (2) higher (3) the same [4] Part B 1 Answer all questions in this part. Directions (31 50): For each statement or question, write on the separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry. 31 Which electron configuration represents the electrons in an atom of chlorine in an excited state? (1) 2-7-7 (3) 2-8-7 (2) 2-7-8 (4) 2-8-8 34 The atomic mass of element A is 63.6 atomic mass units. The only naturally occurring isotopes of element A are A-63 and A-65. The percent abundances in a naturally occurring sample of element A are closest to (1) 31% A-63 and 69% A-65 (2) 50% A-63 and 50% A-65 (3) 69% A-63 and 31% A-65 (4) 100% A-63 and 0% A-65 32 Given the particle diagram representing four molecules of a substance: 35 Elements Q, X, and Z are in the same group on the Periodic Table and are listed in order of increasing atomic number. The melting point of element Q is 219 C and the melting point of element Z is 7 C. Which temperature is closest to the melting point of element X? (1) 7 C (3) 219 C (2) 101 C (4) 226 C Which particle diagram best represents this same substance after a physical change has taken place? 36 Given the balanced equation: 2C + 3H2 C2H6 (1) What is the total number of moles of C that must completely react to produce 2.0 moles of C2H6? (3) (1) 1.0 mol (2) 2.0 mol (3) 3.0 mol (4) 4.0 mol 37 Given the balanced equation: 2KClO3 2KCl + 3O2 Which type of reaction is represented by this equation? (2) (4) (1) (2) (3) (4) 33 What is the percent composition by mass of nitrogen in NH4NO3 (gram-formula mass = 80.0 grams/mole)? (1) 17.5% (3) 52.5% (2) 35.0% (4) 60.0% P.S./Chem. Jan. 06 [5] synthesis decomposition single replacement double replacement [OVER] 38 A solid substance was tested in the laboratory. The test results are listed below. dissolves in water is an electrolyte melts at a high temperature 43 Given the potential energy diagram for a chemical reaction: 60. 50. (1) Cu (2) CuBr2 Potential Energy (kJ) Based on these results, the solid substance could be (3) C (4) C6H12O6 39 If 0.025 gram of Pb(NO3)2 is dissolved in 100. grams of H2O, what is the concentration of the resulting solution, in parts per million? (3) 250 ppm (1) 2.5 10 4 ppm (2) 2.5 ppm (4) 4.0 103 ppm 40. 30. 20. 10. 0 Reaction Coordinate 40 Given the balanced equation: 4Fe(s) + 3O2(g) 2Fe2O3(s) + 1640 kJ Which statement correctly describes the energy changes that occur in the forward reaction? Which phrase best describes this reaction? (1) (2) (3) (4) (1) The activation energy is reaction is endothermic. (2) The activation energy is reaction is exothermic. (3) The activation energy is reaction is endothermic. (4) The activation energy is reaction is exothermic. endothermic with H = +1640 kJ endothermic with H = 1640 kJ exothermic with H = +1640 kJ exothermic with H = 1640 kJ 41 A student adds solid KCl to water in a flask. The flask is sealed with a stopper and thoroughly shaken until no more solid KCl dissolves. Some solid KCl is still visible in the flask. The solution in the flask is (1) saturated and is at equilibrium with the solid KCl (2) saturated and is not at equilibrium with the solid KCl (3) unsaturated and is at equilibrium with the solid KCl (4) unsaturated and is not at equilibrium with the solid KCl H O H C C H 50. kJ and the 50. kJ and the H N H This compound is classified as an (1) amide (2) amine (3) aldehyde (4) alcohol 45 Which formula represents an unsaturated hydrocarbon? (1) CH2CHCl (3) CH3CH2CH3 (2) CH3CH2Cl (4) CH3CHCH2 2C2H6 + 7O2 4CO2 + 6 ____ What is the formula of the missing product? P.S./Chem. Jan. 06 10. kJ and the 44 Given the structural formula: 42 Given the incomplete equation for the combustion of ethane: (1) CH3OH (2) HCOOH 10. kJ and the (3) H2O (4) H2O2 [6] 49 Given the nuclear equation: 46 Given the balanced equation for an organic reaction: 1H 1 C2H2 + 2Cl2 C2H2Cl4 4 +X 6 3Li + 2He This reaction is best classified as The particle represented by X is (1) addition (2) esterification (1) 9 4Li (3) (2) 9 4Be (4) (3) fermentation (4) substitution 47 Which indicator is yellow in a solution with a pH of 9.8? (1) methyl orange (3) bromcresol green (2) bromthymol blue (4) thymol blue 10 Be 5 10 C 6 50 The decay of which radioisotope can be used to estimate the age of the fossilized remains of an insect? (1) Rn-222 (3) Co-60 (2) I-131 (4) C-14 48 How many milliliters of 0.100 M NaOH(aq) would be needed to completely neutralize 50.0 milliliters of 0.300 M HCl(aq)? (1) 16.7 mL (3) 150. mL (2) 50.0 mL (4) 300. mL P.S./Chem. Jan. 06 [7] [OVER] Part B 2 Answer all questions in this part. Directions (51 67): Record your answers in the spaces provided in your answer booklet. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry. 51 What is the total number of neutrons in an atom of aluminum-27? [1] 52 Explain, in terms of atomic structure, why the atomic radius of iodine is greater than the atomic radius of fluorine. [1] 53 In the space in your answer booklet, draw a Lewis electron-dot diagram of a selenium atom in the ground state. [1] 54 Explain, in terms of atomic structure, why liquid mercury is a good electrical conductor. [1] 55 Given the structural formula of pentane: H H H H H H C C C C C H H H H H H In the space in your answer booklet, draw a structural formula for an isomer of pentane. [1] 56 Based on Reference Table N, what is the fraction of a sample of potassium-42 that will remain unchanged after 62.0 hours? [1] 57 What is the total number of moles in 80.0 grams of C2H5Cl (gram-formula mass = 64.5 grams/mole)? [1] 58 What is the total amount of heat energy, in joules, absorbed by 25.0 grams of water when the temperature of the water increases from 24.0 C to 36.0 C? [1] Base your answers to questions 59 and 60 on the information and balanced equation below. Given the equation for a reaction at equilibrium: 2SO2(g) + O2(g) 2SO3(g) + energy 59 Explain, in terms of LeChatelier s principle, why the concentration of SO2(g) increases when the temperature is increased. [1] 60 Explain, in terms of collisions between molecules, why increasing the concentration of O2(g) produces a decrease in the concentration of SO2(g). [1] P.S./Chem. Jan. 06 [8] Base your answers to questions 61 through 65 on the table below. Physical Properties of Four Gases hydrogen Density (g/L) at STP hydrogen iodide H Cl H Br H I 188 207 237 0.0899 Boiling Point (K) at 1 Atm hydrogen bromide 20. Molecular Structure hydrogen chloride H H Name of Gas 1.64 ? 5.66 61 The volume of 1.00 mole of hydrogen bromide at STP is 22.4 liters. The gram-formula mass of hydrogen bromide is 80.9 grams per mole. What is the density of hydrogen bromide at STP? [1] 62 The density of hydrogen at STP is 0.0899 gram per liter. Express this density to two significant figures. [1] 63 Explain, in terms of electronegativity difference, why the bond in H Cl is more polar than the bond in H I. [1] 64 Explain, in terms of intermolecular forces, why hydrogen has a lower boiling point than hydrogen bromide. [1] 65 Explain, in terms of molecular polarity, why hydrogen chloride is more soluble than hydrogen in water under the same conditions of temperature and pressure. [1] Base your answers to questions 66 and 67 on the graph below, which represents the cooling of a substance starting at a temperature above its boiling point. 200 Temperature ( C) 180 160 A 140 120 100 C B 80 60 40 E D 20 F 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 Time (min) 66 What is the melting point of this substance? [1] 67 Which segment of the graph represents the gas phase, only? P.S./Chem. Jan. 06 [9] [1] [OVER] Part C Answer all questions in this part. Directions (68 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 68 through 70 on the information and table below. A student conducts an experiment to determine how the temperature of water affects the rate at which an antacid tablet dissolves in the water. The student has three antacid tablets of the same size and composition. The student drops one tablet into each of three beakers containing 200. milliliters of water at different temperatures and measures the time it takes for each tablet to completely dissolve. The results are shown in the table below. Dissolving Data for Three Antacid Tablets Beaker Original Temperature of Water ( C) Time for Tablet to Dissolve (s) 1 20. 40. 2 30. 25 3 40. 10. 68 Describe the effect of water temperature on the rate of dissolving. [1] 69 Explain, in terms of collision theory, how water temperature influences the rate of dissolving. [1] 70 What change, other than temperature, would affect the rate of dissolving? P.S./Chem. Jan. 06 [10] [1] Base your answers to questions 71 through 74 on the passage below. Acid rain lowers the pH in ponds and lakes and over time can cause the death of some aquatic life. Acid rain is caused in large part by the burning of fossil fuels in power plants and by gasoline-powered vehicles. The acids commonly associated with acid rain are sulfurous acid, sulfuric acid, and nitric acid. In general, fish can tolerate a pH range between 5 and 9. However, even small changes in pH can significantly affect the solubility and toxicity of common pollutants. Increased concentrations of these pollutants can adversely affect the behavior and normal life processes of fish and cause deformity, lower egg production, and less egg hatching. 71 Acid rain caused the pH of a body of water to decrease. Explain this pH decrease in terms of the change in concentration of hydronium ions. [1] 72 Write the chemical formula of a negative polyatomic ion present in an aqueous nitric acid solution. [1] 73 Using information in the passage, describe one effect of acid rain on future generations of fish species in ponds and lakes. [1] 74 Sulfur dioxide, SO2, is one of the gases that reacts with water to produce acid rain. According to Reference Table G, describe how the solubility of sulfur dioxide in water is affected by an increase in water temperature. [1] Base your answers to questions 75 through 77 on the information below. A student is instructed to make 0.250 liter of a 0.200 M aqueous solution of Ca(NO3)2. 75 What is the gram-formula mass of Ca(NO3)2? [1] 76 In the space in your answer booklet, show a correct numerical setup for calculating the total number of moles of Ca(NO3)2 needed to make 0.250 liter of the 0.200 M calcium nitrate solution. [1] 77 In order to prepare the described solution in the laboratory, two quantities must be measured accurately. One of these quantities is the volume of the solution. What other quantity must be measured to prepare this solution? [1] P.S./Chem. Jan. 06 [11] [OVER] Base your answers to questions 78 through 80 on the data in Reference Table S. 78 On the data table in your answer booklet, record the boiling points for He, Ne, Ar, Kr, and Xe. [1] 79 On the grid in your answer booklet, plot the boiling point versus the atomic number for He, Ne, Ar, Kr, and Xe. Circle and connect the points. [1] Example: 80 Based on your graph, describe the trend in the boiling points of these elements as the atomic number increases. [1] Base your answers to questions 81 and 82 on the information below. A lightbulb contains argon gas at a temperature of 295 K and at a pressure of 75 kilopascals. The lightbulb is switched on, and after 30 minutes its temperature is 418 K. 81 In the space in your answer booklet, show a correct numerical setup for calculating the pressure of the gas inside the lightbulb at 418 K. Assume the volume of the lightbulb remains constant. [1] 82 What Celsius temperature is equal to 418 K? [1] 83 Because tap water is slightly acidic, water pipes made of iron corrode over time, as shown by the balanced ionic equation below: 2Fe + 6H+ 2Fe3+ + 3H2 Explain, in terms of chemical reactivity, why copper pipes are less likely to corrode than iron pipes. [1] P.S./Chem. Jan. 06 [12] Base your answers to questions 84 and 85 on the information and diagram below. The apparatus shown in the diagram consists of two inert platinum electrodes immersed in water. A small amount of an electrolyte, H2SO4, must be added to the water for the reaction to take place. The electrodes are connected to a source that supplies electricity. O (g) H (g) 2 2 H O( ) + H SO (aq) 2 Platinum electrode 2 4 Platinum electrode (+) ( ) Battery 84 What type of electrochemical cell is shown? [1] 85 What particles are provided by the electrolyte that allow an electric current to flow? [1] P.S./Chem. Jan. 06 [13] The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING Tear Here CHEMISTRY Thursday, January 26, 2006 1:15 to 4:15 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 ............ 11 . . . . . . . . . . . . 21 . . . . . . . . . . . 31 . . . . . . . . . . . . 41 . . . . . . . . . . . . 2 ............ 12 . . . . . . . . . . . . 22 . . . . . . . . . . . 32 . . . . . . . . . . . . 42 . . . . . . . . . . . . 3 ............ 13 . . . . . . . . . . . . 23 . . . . . . . . . . . 33 . . . . . . . . . . . . 43 . . . . . . . . . . . . 4 ............ 14 . . . . . . . . . . . . 24 . . . . . . . . . . . 34 . . . . . . . . . . . . 44 . . . . . . . . . . . . 5 ............ 15 . . . . . . . . . . . . 25 . . . . . . . . . . . 35 . . . . . . . . . . . . 45 . . . . . . . . . . . . 6 ............ 16 . . . . . . . . . . . . 26 . . . . . . . . . . . 36 . . . . . . . . . . . . 46 . . . . . . . . . . . . 7 ............ 17 . . . . . . . . . . . . 27 . . . . . . . . . . . 37 . . . . . . . . . . . . 47 . . . . . . . . . . . . 8 ............ 18 . . . . . . . . . . . . 28 . . . . . . . . . . . 38 . . . . . . . . . . . . 48 . . . . . . . . . . . . 9 ............ 19 . . . . . . . . . . . . 29 . . . . . . . . . . . 39 . . . . . . . . . . . . 49 . . . . . . . . . . . . 10 . . . . . . . . . . . . 20 . . . . . . . . . . . . 30 . . . . . . . . . . . 40 . . . . . . . . . . . . 50 . . . . . . . . . . . . Part B 1 Score Part A Score Write your answers to Part B 2 and Part C in your answer booklet. Tear Here The declaration below should be signed when you have completed the examination. I do hereby affirm, at the close of this examination, that I had no unlawful knowledge of the questions or answers prior to the examination and that I have neither given nor received assistance in answering any of the questions during the examination. Signature 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 Thursday, January 26, 2006 1:15 to 4:15 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 . . . . . .3 ...... 11 . . . . . . 4 ...... 21 . . . . . .1 ..... 31 . . . . . 2 ....... 41 . . . . . 1 ....... 2 . . . . . .2 ...... 12 . . . . . . 3 ...... 22 . . . . . .4 ..... 32 . . . . . 1 ....... 42 . . . . . 3 ....... 3 . . . . . .4 ...... 13 . . . . . . 2 ...... 23 . . . . . .3 ..... 33 . . . . . 2 ....... 43 . . . . . 2 ....... 4 . . . . . .1 ...... 14 . . . . . . 2 ...... 24 . . . . . .1 ..... 34 . . . . . 3 ....... 44 . . . . . 1 ....... 5 . . . . . .2 ...... 15 . . . . . . 3 ...... 25 . . . . . .1 ..... 35 . . . . . 2 ....... 45 . . . . . 4 ....... 6 . . . . . .3 ...... 16 . . . . . . 3 ...... 26 . . . . . .3 ..... 36 . . . . . 4 ....... 46 . . . . . 1 ....... 7 . . . . . .1 ...... 17 . . . . . . 3 ...... 27 . . . . . .4 ..... 37 . . . . . 2 ....... 47 . . . . . 1 ....... 8 . . . . . .2 ...... 18 . . . . . . 2 ...... 28 . . . . . .2 ..... 38 . . . . . 2 ....... 48 . . . . . 3 ....... 9 . . . . . .2 ...... 19 . . . . . . 2 ...... 29 . . . . . .1 ..... 39 . . . . . 3 ....... 49 . . . . . 2 ....... 10 . . . . . . 4 ...... 20 . . . . . . 4 ...... 30 . . . . . .1 ..... 40 . . . . . 4 ....... 50 . . . . . 4 ....... Part B 1 Score [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 Thursday, January 26, 2006. 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 for that administration be used to determine the student s final score. [3] [OVER] PHYSICAL SETTING/CHEMISTRY continued Part B 2 Allow a total of 17 credits for this part. The student must answer all questions in this part. 51 [1] Allow 1 credit for 14. 52 [1] Allow 1 credit. Acceptable responses include, but are not limited to: An iodine atom has more electron shells than a fluorine atom. A fluorine atom has fewer electron shells. Note: Do not allow credit for a response indicating greater atomic number. 53 [1] Allow 1 credit. The correct symbol and six electrons must be shown. The location of single electrons and electron pairs may vary. Example of a 1-credit response: Se 54 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Electrons in liquid mercury are mobile. valence electrons free to move and conduct electric current 55 [1] Allow 1 credit. Examples of a 1-credit response: H H C H H H H H C C C C H H H H H C C C C C [4] PHYSICAL SETTING/CHEMISTRY continued 56 1 [1] Allow 1 credit for 32 or 0.03125. Significant figures do not need to be shown. 57 [1] Allow 1 credit for 1.24 mol. Significant figures do not need to be shown. 58 [1] Allow 1 credit for 1250 J. Significant figures do not need to be shown. 59 [1] Allow 1 credit. Acceptable responses include, but are not limited to: An increase in temperature favors the endothermic reaction, which produces more SO2(g). The reaction shifts to the left, increasing the concentration of SO2(g). 60 [1] Allow 1 credit. Acceptable responses include, but are not limited to: A higher concentration of O2(g) causes more collisions and reactions with SO2(g) molecules, decreasing SO2(g) concentration. More collisions between reactants shift the reaction to the right. 61 [1] Allow 1 credit for 3.61 g/L. Significant figures do not need to be shown. 62 [1] Allow 1 credit for 0.090 g/L or 9.0 10 2 g/L. 63 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The electronegativity difference for HCl is 1.1, which is higher than the 0.6 for HI. The difference for HCl is greater. 64 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Hydrogen has weaker intermolecular forces than HBr. hydrogen weaker forces [5] [OVER] PHYSICAL SETTING/CHEMISTRY continued 65 [1] Allow 1 credit. Acceptable responses include, but are not limited to: HCl s molecular polarity is more similar to water s polarity than H2 s polarity compared to water s. HCl and water both polar, H2 nonpolar, like dissolves like HCl polarity is more similar to water s polarity. 66 [1] Allow 1 credit for 50 C. Significant figures do not need to be shown. 67 [1] Allow 1 credit. Acceptable responses include, but are not limited to: AB from time 0 to 2 minutes [6] PHYSICAL SETTING/CHEMISTRY continued Part C Allow a total of 18 credits for this part. The student must answer all questions in this part. 68 [1] Allow 1 credit. Acceptable responses include, but are not limited to: If the water temperature is higher, the tablet will dissolve at a faster rate. higher temperature, less time to dissolve lower rate in cold water 69 [1] Allow 1 credit. Acceptable responses include, but are not limited to: At higher temperatures the water molecules collide more often and more effectively with the tablet, so the tablet dissolves faster. high temperature more collisions dissolves faster or Allow 1 credit for a response consistent with the student s answer to question 68. 70 [1] Allow 1 credit. Acceptable responses include, but are not limited to: crushing the tablet stirring/shaking/agitating 71 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The pH goes down because there are more hydronium ions in solution. [H3O+] 72 [1] Allow 1 credit for NO3 or NO31 or NO3 1 or OH . 73 [1] Allow 1 credit. Acceptable responses include, but are not limited to: There will be a decrease in the number of fish eggs that hatch. fewer eggs produced more deformities [7] [OVER] PHYSICAL SETTING/CHEMISTRY continued 74 [1] Allow 1 credit. Acceptable responses include, but are not limited to: As the water temperature increases, the solubility of sulfur dioxide decreases. The solubility of SO2 decreases. 75 [1] Allow 1 credit for 164 g/mol. Significant figures do not need to be shown. 76 [1] Allow 1 credit. Acceptable responses include, but are not limited to: mol (0.200 1L ) 0.250 L 0.2 = 77 x 0.25 [1] Allow 1 credit. Acceptable responses include, but are not limited to: mass of Ca(NO3)2 mass of solute mass 78 [1] Allow 1 credit for all five correctly listed boiling points shown below. Allow credit even if the degree sign is shown for the boiling points. Data Table Symbol Atomic Number Boiling Point (K) He Ne Ar Kr Xe 2 10 18 36 54 4 27 87 121 166 [8] PHYSICAL SETTING/CHEMISTRY continued 79 [1] Allow 1 credit for plotting all the points correctly ( 0.3 grid space). Plotted points do not need to be circled or connected. Example of a 1-credit response: Boiling Point Versus Atomic Number for He, Ne, Ar, Kr, and Xe 200. Boiling Point (K) 150. 100. 50. 0 0 20 40 60 Atomic Number or Allow 1 credit for a response consistent with the student s answer to question 78. 80 [1] Allow 1 credit. Acceptable responses include, but are not limited to: As atomic number increases, boiling point increases. or Allow 1 credit for a response consistent with the student s graph in question 79. or Allow 1 credit for a response consistent with the student s data in question 78. [9] [OVER] PHYSICAL SETTING/CHEMISTRY concluded 81 [1] Allow 1 credit. Acceptable responses include, but are not limited to: 75 kPa x = 295 K 418 K (75)(418) 295 P2 = 82 [1] Allow 1 credit for 145 C. 83 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Copper is less reactive than iron. Cu below H2 on Table J 84 [1] Allow 1 credit for electrolytic or electrolysis. 85 [1] Allow 1 credit. Acceptable responses include, but are not limited to: ions charged particles + H3O 2 SO4 [10] The Chart for Determining the Final Examination Score for the January 2006 Regents Examination in Physical Setting/Chemistry will be posted on the Department s web site http://www.emsc.nysed.gov/osa/ on Thursday, January 26, 2006. 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 January 2006 Physical Setting/ Chemistry Question Numbers Part A Part B Standard 1 39,43,48,56,57,58, 61,62,64 34,35 33,51,61 52,59,60 76,77,79,81,82 31,41,47,63,66,67 68,72,78,83,84 Part C 80 69,70,75 71,85 Standard 2 Key Idea 1 Key Idea 2 73 Standard 6 Key Idea 1 Key Idea 2 Key Idea 3 Key Idea 4 Key Idea 5 32,36,49,53,55 41 80 Standard 7 Key Idea 1 Key Idea 2 Standard 4 Process Skills Key Idea 3 34,35,36,37,38,39, 41,42,44,45,46,47, 48,51,52,53,55,57, 59,65 69,74,75,76,77, 81,83,84 Key Idea 4 40,43,49,50,56,58, 66,67 82 Key Idea 5 54,63,64,65 Key Idea 3 Key Idea 4 Key Idea 5 2002 Edition Standard 4 1,2,3,4,5,6,7,8, 31,32,33,34,35,36, 9,10,13,14,15, 37,38,39,41,42,44, 17,18,20,21,22, 45,46,47,48,51,52, 23,24,28,30 55,57,59,60,61 68,69,70,71,72, 73,74,75,76,77, 78,80,81,83,84, 85 16,27 40,43,49,50,56,58, 66,67 11,12,19,25,26, 53,54,63,64,65 29 Reference Tables 3,6,7,8,12,19, 31,33,39,40,44,45, 21,24,26,28 47,48,49,51,52,53, 56,57,58,61,63 [12] 72,74,75,76,78, 81,82,83

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