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New York Regents Chemistry June 2006

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PS/CHEMISTRY The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY Wednesday, June 21, 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 notation represents an atom of sodium with an atomic number of 11 and a mass number of 24? (1) 24 (3) 13 11Na 11Na (2) 11Na 24 (4) 7 Given the balanced equation representing a reaction: F2(g) + H2(g) 2HF(g) What is the mole ratio of H2(g) to HF(g) in this reaction? 35Na 11 (1) 1:1 (2) 1:2 2 Which element has chemical properties that are most similar to those of calcium? (1) Co (3) N (2) K (4) Sr 8 Which list includes three types of chemical reactions? (1) condensation, double replacement, and sublimation (2) condensation, solidification, and synthesis (3) decomposition, double replacement, and synthesis (4) decomposition, solidification, and sublimation 3 Which element is malleable and can conduct electricity in the solid phase? (1) iodine (3) sulfur (2) phosphorus (4) tin 4 Atoms of different isotopes of the same element differ in their total number of (1) electrons (3) protons (2) neutrons (4) valence electrons 5 Which statement correctly describes of oxygen, O2 and O3? (1) They have identical molecular and identical properties. (2) They have identical molecular and different properties. (3) They have different molecular and identical properties. (4) They have different molecular and different properties. 9 Which type of bond results when one or more valence electrons are transferred from one atom to another? (1) a hydrogen bond (2) an ionic bond (3) a nonpolar covalent bond (4) a polar covalent bond two forms structures 10 What is the total number of electrons shared in the bonds between the two carbon atoms in a molecule of H C C H ? (1) 6 (3) 3 (2) 2 (4) 8 structures structures structures 11 Which formula represents a nonpolar molecule? (1) CH4 (3) H2O (2) HCl (4) NH3 6 What is the IUPAC name for the compound FeS? (1) iron(II) sulfate (3) iron(II) sulfide (2) iron(III) sulfate (4) iron(III) sulfide P.S./Chem. June 06 (3) 2:1 (4) 2:3 [2] 12 Which changes occur as a cadmium atom, Cd, becomes a cadmium ion, Cd2+? (1) The Cd atom gains two electrons and its radius decreases. (2) The Cd atom gains two electrons and its radius increases. (3) The Cd atom loses two electrons and its radius decreases. (4) The Cd atom loses two electrons and its radius increases. 18 Which expression represents the H for a chemical reaction in terms of the potential energy, PE, of its products and reactants? (1) PE of products + PE of reactants (2) PE of products PE of reactants (3) PE of products PE of reactants (4) PE of products PE of reactants 19 Which balanced equation represents an endothermic reaction? (1) C(s) + O2(g) CO2(g) (2) CH4(g) + 2O2(g) CO2(g) + 2H2O( ) (3) N2(g) + 3H2(g) 2NH3(g) (4) N2(g) + O2(g) 2NO(g) 13 Which element has atoms with the greatest attraction for electrons in a chemical bond? (1) beryllium (3) lithium (2) fluorine (4) oxygen 20 Which formula represents propyne? (3) C5H8 (1) C3H4 (2) C3H6 (4) C5H10 14 Two substances, A and Z, are to be identified. Substance A can not be broken down by a chemical change. Substance Z can be broken down by a chemical change. What can be concluded about these substances? (1) Both substances are elements. (2) Both substances are compounds. (3) Substance A is an element and substance Z is a compound. (4) Substance A is a compound and substance Z is an element. 21 Which factors must be equal in a reversible chemical reaction at equilibrium? (1) the activation energies of the forward and reverse reactions (2) the rates of the forward and reverse reactions (3) the concentrations of the reactants and products (4) the potential energies of the reactants and products 15 Which ion, when combined with chloride ions, Cl , forms an insoluble substance in water? (3) Pb2+ (1) Fe2+ 2+ (2) Mg (4) Zn2+ 22 The compounds CH3OCH3 and CH3CH2OH are isomers of each other. These two compounds must have the same (1) density (3) melting point (2) reactivity (4) molecular formula 16 Molarity is defined as the (1) moles of solute per kilogram of solvent (2) moles of solute per liter of solution (3) mass of a solution (4) volume of a solvent 23 Which balanced equation represents a redox reaction? (1) AgNO3 + NaCl AgCl + NaNO3 (2) BaCl2 + K2CO3 BaCO3 + 2KCl (3) CuO + CO Cu + CO2 (4) HCl + KOH KCl + H2O 17 Which formula represents a hydrocarbon? (1) CH3CH2CH2CHO (2) CH3CH2CH2CH3 (3) CH3CH2CH2COOH (4) CH3CH2COOCH3 P.S./Chem. June 06 [3] [OVER] 24 Which process occurs at the anode in an electrochemical cell? (1) the loss of protons (2) the loss of electrons (3) the gain of protons (4) the gain of electrons 28 Which equation represents the radioactive decay of 226 88Ra? (1) (2) (3) (4) 25 Which substance is an electrolyte? (1) CH3OH (3) H2O (4) KOH (2) C6H12O6 4 222 86Rn + 2He 0 226 89Ac + 1e 0 226 87Fr ++1e 1 225 88Ra + 0n 29 Which type of reaction converts one element to another element? (1) neutralization (3) substitution (2) polymerization (4) transmutation 26 Which ion is the only negative ion present in an aqueous solution of an Arrhenius base? (1) hydride ion (3) hydronium ion (2) hydrogen ion (4) hydroxide ion 30 Which nuclear emission has the greatest mass? (1) (3) (2) (4) + 27 According to Reference Table N, which pair of isotopes spontaneously decays? (1) C-12 and N-14 (3) C-14 and N-14 (2) C-12 and N-16 (4) C-14 and N-16 P.S./Chem. June 06 226Ra 88 226Ra 88 226Ra 88 226Ra 88 [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 trends are observed as each of the elements within Group 15 on the Periodic Table is considered in order from top to bottom? (1) Their metallic properties decrease and their atomic radii decrease. (2) Their metallic properties decrease and their atomic radii increase. (3) Their metallic properties increase and their atomic radii decrease. (4) Their metallic properties increase and their atomic radii increase. 36 A metal, M, forms an oxide compound with the general formula M2O. In which group on the Periodic Table could metal M be found? (1) Group 1 (3) Group 16 (2) Group 2 (4) Group 17 37 Given the key: Key = Atom of oxygen = Atom of carbon 32 What is the total number of electrons in a S2 ion? (1) 10 (3) 16 (2) 14 (4) 18 Which particle diagram represents a sample containing the compound CO(g)? 33 A substance has an empirical formula of CH2 and a molar mass of 56 grams per mole. The molecular formula for this compound is (1) CH2 (3) C4H8 (2) C4H6 (4) C8H4 (1) (3) (2) (4) 34 Compared to an atom of phosphorus-31, an atom of sulfur-32 contains (1) one less neutron (3) one more neutron (2) one less proton (4) one more proton 35 In which compound is the percent composition by mass of chlorine equal to 42%? (1) HClO (gram-formula mass = 52 g/mol) (2) HClO2 (gram-formula mass = 68 g/mol) (3) HClO3 (gram-formula mass = 84 g/mol) (4) HClO4 (gram-formula mass = 100. g/mol) P.S./Chem. June 06 38 At standard pressure, which element has a melting point higher than standard temperature? (3) Fe (1) F2 (2) Br2 (4) Hg [5] [OVER] 39 Which Lewis electron-dot diagram represents chloroethene? H H H C C Cl (3) H H H C C Cl H H H O H H H C C Cl H H (1) 45 Given the formula: H H C Cl H (2) H C C C C H N H H H H This compound is classified as (1) an aldehyde (2) an amide (3) an amine (4) a ketone 46 Given the balanced equation with an unknown compound represented by X: C6H12O6(aq) (4) enzyme 2X + 2CO2(g) Which compound is represented by X? 40 A saturated solution of NaNO3 is prepared at 60. C using 100. grams of water. As this solution is cooled to 10. C, NaNO3 precipitates (settles) out of the solution. The resulting solution is saturated. Approximately how many grams of NaNO3 settled out of the original solution? (1) 46 g (3) 85 g (2) 61 g (4) 126 g (1) (2) (3) (4) CH3OH(aq) CH2(OH)4(aq) CH3CH2OH(aq) CH2OHCH2OH(aq) 47 Which reactants form the salt CaSO4(s) in a neutralization reaction? (1) (2) (3) (4) 41 Which kelvin temperature is equivalent to 24 C? (1) 226 K (3) 273 K (2) 249 K (4) 297 K H2S(g) and Ca(ClO4)2(s) H2SO3(aq) and Ca(NO3)2(aq) H2SO4(aq) and Ca(OH)2(aq) SO2(g) and CaO(s) 42 Which substance has the lowest vapor pressure at 75 C? (1) water (3) propanone (2) ethanoic acid (4) ethanol 48 A student tested a 0.1 M aqueous solution and made the following observations: conducts electricity turns blue litmus to red reacts with Zn(s) to produce gas bubbles 43 What is the IUPAC name for the compound that has the condensed structural formula CH3CH2CH2CHO? (1) butanal (3) propanal (2) butanol (4) propanol Which compound could be the solute in this solution? (1) CH3OH (2) LiBr 49 What is the half-life of sodium-25 if 1.00 gram of a 16.00-gram sample of sodium-25 remains unchanged after 237 seconds? (1) 47.4 s (3) 79.0 s (2) 59.3 s (4) 118 s 44 What volume of 0.500 M HNO3(aq) must completely react to neutralize 100.0 milliliters of 0.100 M KOH(aq)? (1) 10.0 mL (3) 50.0 mL (2) 20.0 mL (4) 500. mL P.S./Chem. June 06 (3) HBr (4) LiOH [6] 50 Given the table below that shows students examples of proposed models of the atom: Proposed Models of the Atom Model Location of Protons Location of Electrons A in the nucleus specific shells B in the nucleus regions of most probable location C dispersed throughout the atom specific shells D dispersed throughout the atom regions of most probable location Which model correctly describes the locations of protons and electrons in the wave-mechanical model of the atom? (1) A (3) C (2) B (4) D P.S./Chem. June 06 [7] [OVER] Part B 2 Answer all questions in this part. Directions (51 66): Record your answers in the spaces provided in your answer booklet. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry. Base your answers to questions 51 and 52 on the balanced equation below. Fe(s) + 2HNO3(aq) Fe(NO3)2(aq) + H2(g) 51 What is the total number of oxygen atoms represented in the formula of the iron compound produced? [1] 52 Explain, using information from Reference Table J, why this reaction is spontaneous. [1] Base your answers to questions 53 and 54 on the information below. An atom has an atomic number of 9, a mass number of 19, and an electron configuration of 2 6 1. 53 What is the total number of neutrons in this atom? [1] 54 Explain why the number of electrons in the second and third shells shows that this atom is in an excited state. [1] 55 To which homologous series does CH3CH2CH2CH3 belong? [1] 56 What is the mass of 4.76 moles of Na3PO4 (gram-formula mass = 164 grams/mole)? [1] Base your answers to questions 57 and 58 on the information below. Given the balanced equation for dissolving NH4Cl(s) in water: NH4Cl(s) H2O + NH4 (aq) + Cl (aq) 57 A student is holding a test tube containing 5.0 milliliters of water. When a sample of NH4Cl(s) is placed in the test tube, the test tube feels colder to the student s hand. Describe the direction of heat flow between the test tube and the hand. [1] 58 Using the key in your answer booklet, draw at least two water molecules in the box, showing the correct orientation of each water molecule when it is near the Cl ion in the aqueous solution. [1] P.S./Chem. June 06 [8] Base your answers to questions 59 and 60 on the information below. Given the reaction at equilibrium: 2NO2(g) N2O4(g) + 55.3 kJ 59 Explain, in terms of energy, why the forward reaction is exothermic. [1] 60 Explain, in terms of Le Chatelier s principle, why the equilibrium shifts to the right to relieve the stress when the pressure on the system is increased at constant temperature. [1] Base your answers to questions 61 through 63 on the information below. Given the balanced equation for an organic reaction between butane and chlorine that takes place at 300. C and 101.3 kilopascals: C4H10 + Cl2 C4H9Cl + HCl 61 Identify the type of organic reaction shown. [1] 62 In the space in your answer booklet, draw a structural formula for the organic product. [1] 63 Explain, in terms of collision theory, why the rate of the reaction would decrease if the temperature of the reaction mixture was lowered to 200. C with pressure remaining unchanged. [1] Base your answers to questions 64 through 66 on the information below. Ethanol, C2H5OH, is a volatile and flammable liquid with a distinct odor at room temperature. Ethanol is soluble in water. The boiling point of ethanol is 78.2 C at 1 atmosphere. Ethanol can be used as a fuel to produce heat energy, as shown by the balanced equation below. C2H5OH( ) + 3O2(g) 2CO2(g) + 3H2O( ) + 1367 kJ 64 At 1 atmosphere, compare the boiling point of pure ethanol to the boiling point of a solution in which a nonvolatile substance is dissolved in ethanol. [1] 65 Determine the total amount of heat produced by the complete combustion of 2.00 moles of ethanol. [1] 66 Identify one physical property of ethanol, stated in the passage, that can be explained in terms of chemical bonds and intermolecular forces. [1] P.S./Chem. June 06 [9] [OVER] Part C Answer all questions in this part. Directions (67 84): 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 67 and 68 on the information below. The graph shows the relationship between the solubility of a sequence of primary alcohols in water and the total number of carbon atoms in a molecule of the corresponding alcohol at the same temperature and pressure. A primary alcohol has the OH group located on an end carbon of the hydrocarbon chain. Solubility Versus Total Number of Carbon Atoms Solubility (g/110. g of water) 9 8 7 6 5 4 3 2 1 0 3 4 5 6 7 8 9 10 11 Total Number of Carbon Atoms Adapted from Chemistry, Collins Educational Publishing, pp. 227-231 67 Describe the relationship between the solubility of a primary alcohol in water and the total number of carbon atoms in the primary alcohol. [1] 68 Determine the total mass of 1-pentanol that will dissolve in 110. grams of water to produce a saturated solution. [1] P.S./Chem. June 06 [10] Base your answers to questions 69 and 70 on the information below. Air bags are an important safety feature in modern automobiles. An air bag is inflated in milliseconds by the explosive decomposition of NaN3(s). The decomposition reaction produces N2(g), as well as Na(s), according to the unbalanced equation below. NaN3(s) Na(s) + N2(g) 69 Balance the equation in your answer booklet for the decomposition of NaN3, using the smallest whole-number coefficients. [1] 70 When the air bag inflates, the nitrogen gas is at a pressure of 1.30 atmospheres, a temperature of 301 K, and has a volume of 40.0 liters. In the space in your answer booklet, calculate the volume of the nitrogen gas at STP. Your response must include both a correct numerical setup and the calculated volume. [2] Base your answers to questions 71 and 72 on the information below. A thiol is very similar to an alcohol, but a thiol has a sulfur atom instead of an oxygen atom in the functional group. One of the compounds in a skunk s spray is 2-butene-1-thiol. The formula of this compound is shown below. H H H H C C C C SH H H H 71 Explain, in terms of composition, why this compound is a thiol. [1] 72 Explain, in terms of electron configuration, why oxygen atoms and sulfur atoms form compounds with similar molecular structures. [1] P.S./Chem. June 06 [11] [OVER] Base your answers to questions 73 through 75 on the graph below. The graph shows the relationship between pH value and hydronium ion concentration for common aqueous solutions and mixtures. pH Versus Hydronium Ion Concentration 14 Bleach 12 Aqueous ammonia Milk of magnesia 10. Seawater 8 pH Blood Milk 6 4 2 Tomato juice Lemon juice Stomach fluids (gastric juice) 0 100 10 2 10 4 10 6 10 8 10 10 10 12 10 14 Hydronium Ion Concentration (M) 73 What is the hydronium ion concentration of tomato juice? [1] 74 What color is thymol blue when added to milk of magnesia? [1] 75 According to this graph, which mixture is approximately 100 times more acidic than milk of magnesia? [1] P.S./Chem. June 06 [12] Base your answers to questions 76 and 77 on the information below. Archimedes (287 212 BC), a Greek inventor and mathematician, made several discoveries important to science today. According to a legend, Hiero, the king of Syracuse, commanded Archimedes to find out if the royal crown was made of gold, only. The king suspected that the crown consisted of a mixture of gold, tin, and copper. Archimedes measured the mass of the crown and the total amount of water displaced by the crown when it was completely submerged. He repeated the procedure using individual samples, one of gold, one of tin, and one of copper. Archimedes was able to determine that the crown was not made entirely of gold without damaging it. 76 Identify one physical property that Archimedes used in his comparison of the metal samples. [1] 77 Determine the volume of a 75-gram sample of gold at STP. [1] Base your answers to questions 78 through 81 on the information below. Aluminum is one of the most abundant metals in Earth s crust. The aluminum compound found in bauxite ore is Al2O3. Over one hundred years ago, it was difficult and expensive to isolate aluminum from bauxite ore. In 1886, a brother and sister team, Charles and Julia Hall, found that molten (melted) cryolite, Na3AlF6, would dissolve bauxite ore. Electrolysis of the resulting mixture caused the aluminum ions in the Al2O3 to be reduced to molten aluminum metal. This less expensive process is known as the Hall process. 78 Write the oxidation state for each of the elements in cryolite. [1] 79 Write the balanced half-reaction equation for the reduction of Al3+ to Al. [1] 80 Explain, in terms of ions, why molten cryolite conducts electricity. [1] 81 Explain, in terms of electrical energy, how the operation of a voltaic cell differs from the operation of an electrolytic cell used in the Hall process. Include both the voltaic cell and the electrolytic cell in your answer. [1] P.S./Chem. June 06 [13] [OVER] Base your answers to questions 82 through 84 on the information below. A glass tube is filled with hydrogen gas at low pressure. An electric current is passed through the gas, causing it to emit light. This light is passed through a prism to separate the light into the bright, colored lines of hydrogen s visible spectrum. Each colored line corresponds to a particular wavelength of light. One of hydrogen s spectral lines is red light with a wavelength of 656 nanometers. Tubes filled with other gases produce different bright-line spectra that are characteristic of each kind of gas. These spectra have been observed and recorded. 82 Explain, in terms of electron energy states and energy changes, how hydrogen s brightline spectrum is produced. [1] 83 Explain how the elements present on the surface of a star can be identified using brightline spectra. [1] 84 A student measured the wavelength of hydrogen s visible red spectral line to be 647 nanometers. In the space in your answer booklet, show a correct numerical setup for calculating the student s percent error. [1] P.S./Chem. June 06 [14] The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING Tear Here CHEMISTRY Wednesday, June 21, 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 Wednesday, June 21, 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. Check this web site http://www.emsc.nysed.gov/osa/ and select the link Examination 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 B 1 Part A 1 . . . . .1 ....... 11 . . . . .1 ....... 21 . . . . 2 ....... 31 . . . . . 4 ....... 41 . . . . . 2 ....... 2 . . . . .4 ....... 12 . . . . .3 ....... 22 . . . . 4 ....... 32 . . . . . 4 ....... 42 . . . . . 2 ....... 3 . . . . .4 ....... 13 . . . . .2 ....... 23 . . . . 3 ....... 33 . . . . . 3 ....... 43 . . . . . 1 ....... 4 . . . . .2 ....... 14 . . . . .3 ....... 24 . . . . 2 ....... 34 . . . . . 4 ....... 44 . . . . . 2 ....... 5 . . . . .4 ....... 15 . . . . .3 ....... 25 . . . . 4 ....... 35 . . . . . 3 ....... 45 . . . . . 2 ....... 6 . . . . .3 ....... 16 . . . . .2 ....... 26 . . . . 4 ....... 36 . . . . . 1 ....... 46 . . . . . 3 ....... 7 . . . . .2 ....... 17 . . . . .2 ....... 27 . . . . 4 ....... 37 . . . . . 4 ....... 47 . . . . . 3 ....... 8 . . . . .3 ....... 18 . . . . .2 ....... 28 . . . . 1 ....... 38 . . . . . 3 ....... 48 . . . . . 3 ....... 9 . . . . .2 ....... 19 . . . . .4 ....... 29 . . . . 4 ....... 39 . . . . . 1 ....... 49 . . . . . 2 ....... 10 . . . . .1 ....... 20 . . . . .1 ....... 30 . . . . 1 ....... 40 . . . . . 1 ....... 50 . . . . . 2 ....... Part B 1 Score 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 Scoring Regents Examinations in the Sciences. Use only red ink or red pencil in rating Regents papers. Do not correct the student s work by making insertions or changes of any kind. On the detachable answer sheet for Part A and Part B 1, indicate by means of a checkmark each incorrect or omitted answer. In the box provided at the end of each part, record the number of questions the student answered correctly for that part. At least two science teachers must participate in the scoring of each student s responses to the Part B 2 and Part C open-ended questions. Each of these teachers should be responsible for scoring a selected number of the open-ended questions on each answer paper. No one teacher is to score all the open-ended questions on a student s answer paper. Students responses must be scored strictly according to the Scoring Key and Rating Guide. For open-ended questions, credit may be allowed for responses other than those given in the rating guide if the response is a scientifically accurate answer to the question and demonstrates adequate knowledge as indicated by the examples in the rating guide. Complete sentences are not required. Phrases, diagrams, and symbols may be used. In the student s answer booklet, record the number of credits earned for each answer in the box printed to the right of the answer lines or spaces for that question. Fractional credit is not allowed. Only whole-number credit may be given to a response. Units need not be given when the wording of the questions allows such omissions. Raters should enter the scores earned for Part A, Part B 1, Part B 2, and Part C on the appropriate lines in the box printed on the answer booklet and then should add these four scores and enter the total in the box labeled Total Written Test Score. Then, the student s raw score should be converted to a scaled score by using the conversion chart that will be posted on the Department s web site http://www.emsc.nysed.gov/osa/ on Wednesday, June 21, 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 16 credits for this part. The student must answer all questions in this part. 51 [1] Allow 1 credit for 6 or six. 52 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Iron is more active than hydrogen. Fe is higher on Table J than H2. 53 [1] Allow 1 credit for 10 or ten. 54 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The third shell has one electron before the second shell is completely filled. The electron configuration is not 2-7, which is the ground state for an atom with atomic number 9. Note: Do not allow credit for a response that simply restates that the electron configuration is 2-6-1. 55 [1] Allow 1 credit. Acceptable responses include, but are not limited to: alkanes CnH2n+2 56 [1] Allow 1 credit for 781 g. Significant figures do not need to be shown. 57 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Heat flows from the student s hand to the test tube. The test tube absorbs heat from the hand. [4] PHYSICAL SETTING/CHEMISTRY continued 58 [1] Allow 1 credit. Acceptable responses must show at least two water molecules with at least one hydrogen atom of each water molecule facing toward the Cl ion. Example of a 1-credit response: Cl 59 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Potential energy of the product is less than potential energy of the reactant. More energy is released than absorbed. Energy appears on the right. 60 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Equilibrium shifts toward the fewer number of moles of gas. The reaction shifts to the side that would result in a reduction of pressure. fewer moles of gas, less pressure 61 [1] Allow 1 credit. Acceptable responses include, but are not limited to: substitution chlorination halogenation [5] [OVER] PHYSICAL SETTING/CHEMISTRY continued 62 [1] Allow 1 credit. Examples of a 1-credit response: H H H H Cl C C C C H H H H H Cl C C C C 63 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Particles move slower and collide less frequently. fewer effective collisions between molecules 64 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Ethanol s boiling point is lower than the boiling point of the solution. The solution s boiling point is higher than 78.2 C. 65 [1] Allow 1 credit for 2730 kJ. Significant figures do not need to be shown. 66 [1] Allow 1 credit. Acceptable responses include, but are not limited to: soluble in water boiling point volatility [6] PHYSICAL SETTING/CHEMISTRY continued Part C Allow a total of 19 credits for this part. The student must answer all questions in this part. 67 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The greater the total number of carbon atoms in a molecule of a primary alcohol, the less soluble the alcohol is in water. number of carbons , solubility 68 [1] Allow 1 credit for 2.5 g 0.1 g. 69 [1] Allow 1 credit for 2 NaN3(s) 2 Na(s) + 3 N2(g). 70 [2] Allow a maximum of 2 credits, allocated as follows: Allow 1 credit for a correct numerical setup. Acceptable responses include, but are not limited to: V2 = (273 K)(1.30 atm)(40.0 L) (301 K)(1.00 atm) (273)(1.30)(40.0) (301)(1.00) Allow 1 credit for 47.2 L. Significant figures do not need to be shown. or Allow credit for a response consistent with the student s numerical setup. Note: Do not allow credit for a numerical setup and calculated result that are not related to the concept assessed by the question. 71 [1] Allow 1 credit. Acceptable responses include, but are not limited to: This compound contains an SH functional group. There is a sulfur atom instead of an oxygen atom in the functional group. [7] [OVER] PHYSICAL SETTING/CHEMISTRY continued 72 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Oxygen and sulfur atoms have the same number (six) of valence electrons. Atoms of both elements need two more valence electrons to complete their outer shells. 73 [1] Allow 1 credit. Acceptable responses include, but are not limited to: 10 4 M 0.0001 M 74 [1] Allow 1 credit for blue. 75 [1] Allow 1 credit for seawater. 76 [1] Allow 1 credit. Acceptable responses include, but are not limited to: density mass volume 77 [1] Allow 1 credit. Significant figures do not need to be shown. Acceptable responses include, but are not limited to: 3.9 cm3 3.88 cm3 78 [1] Allow 1 credit. All three oxidation states must be correct to receive credit. Acceptable responses include, but are not limited to: Na: +1 Al: +3 F: 79 1 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Al3+ + 3e Al [8] PHYSICAL SETTING/CHEMISTRY concluded 80 [1] Allow 1 credit. Acceptable responses include, but are not limited to: There are freely moving ions in the molten cryolite. Ions are no longer held together in a crystal lattice. 81 [1] Allow 1 credit for a correct response that includes both processes. Acceptable responses include, but are not limited to: A voltaic cell produces electrical energy and an electrolytic cell used in the Hall process requires electrical energy. Electrolysis uses electrical energy. Voltaic cells produce electrical energy. 82 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The electron of hydrogen absorbs energy and jumps to a higher energy state. The excited electron returns to a lower energy state, releasing light energy. The e absorbs energy and jumps to a higher level. The e falls back to a lower level and releases energy related to a particular color. 83 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The spectrum from a star is compared to spectra of known elements. 84 [1] Allow 1 credit. Acceptable responses include, but are not limited to: % error = 647 nm 656 nm 100 656 nm 647 656 100 656 [9] [OVER] The Chart for Determining the Final Examination Score for the June 2006 Regents Examination in Physical Setting/Chemistry will be posted on the Department s web site http://www.emsc.nysed.gov/osa/ on Wednesday, June 21, 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. The Teacher Evaluation of State Examinations forms will also be posted on the same web site. Please select the link Teacher Evaluation Forms and then the examination title to complete the evaluation form for the June 2006 Regents Examination in Physical Setting/Chemistry. [10] Map to Core Curriculum [11]

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