Trending ▼   ResFinder  

New York Regents Chemistry August 2009

28 pages, 81 questions, 0 questions with responses, 0 total responses,    0    0
New York State Regents Exams
   		+Fave Message
ProfileTimelineUploadsQ & A
 Home > regents >

Formatting page ...

PS/CHEMISTRY The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY Thursday, August 13, 2009 12:30 to 3:30 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 particle has the least mass? (3) 1 (1) 4 2He 0n 1 0e (2) 1H (4) 1 6 Which statement describes a chemical property of bromine? (1) Bromine is soluble in water. (2) Bromine has a reddish-brown color. (3) Bromine combines with aluminum to produce AlBr3. (4) Bromine changes from a liquid to a gas at 332 K and 1 atm. 2 What information is necessary to determine the atomic mass of the element chlorine? (1) the atomic mass of each artificially produced isotope of chlorine, only (2) the relative abundance of each naturally occurring isotope of chlorine, only (3) the atomic mass and the relative abundance of each naturally occurring isotope of chlorine (4) the atomic mass and the relative abundance of each naturally occurring and artificially produced isotope of chlorine 7 An atom of aluminum in the ground state and an atom of gallium in the ground state have the same (1) mass (2) electronegativity (3) total number of protons (4) total number of valence electrons 3 In an atom of argon-40, the number of protons (1) equals the number of electrons (2) equals the number of neutrons (3) is less than the number of electrons (4) is greater than the number of electrons 8 Which type of matter is composed of two or more elements that are chemically combined in a fixed proportion? (1) solution (2) compound (3) homogeneous mixture (4) heterogeneous mixture 4 An electron in a sodium atom moves from the third shell to the fourth shell. This change is a result of the atom (1) absorbing energy (3) gaining an electron (2) releasing energy (4) losing an electron 9 Which type of substance can conduct electricity in the liquid phase but not in the solid phase? (1) ionic compound (2) molecular compound (3) metallic element (4) nonmetallic element 5 Which statement describes oxygen gas, O2(g), and ozone gas, O3(g)? (1) They have different molecular structures, only. (2) They have different properties, only. (3) They have different molecular structures and different properties. (4) They have the same molecular structure and the same properties. P.S./Chem. Aug. 09 10 Why is a molecule of CO2 nonpolar even though the bonds between the carbon atom and the oxygen atoms are polar? (1) The shape of the CO2 molecule is symmetrical. (2) The shape of the CO2 molecule is asymmetrical. (3) The CO2 molecule has a deficiency of electrons. (4) The CO2 molecule has an excess of electrons. [2] 19 How do the boiling point and freezing point of a solution of water and calcium chloride at standard pressure compare to the boiling point and freezing point of water at standard pressure? (1) Both the freezing point and boiling point of the solution are higher. (2) Both the freezing point and boiling point of the solution are lower. (3) The freezing point of the solution is higher and the boiling point of the solution is lower. (4) The freezing point of the solution is lower and the boiling point of the solution is higher. 11 Which formula represents a molecular compound? (1) HI (3) KCl (2) KI (4) LiCl 12 Which element has the greatest density at STP? (1) scandium (3) silicon (2) selenium (4) sodium 13 Particles are arranged in a crystal structure in a sample of (3) Ar(g) (1) H2(g) (2) Br2( ) (4) Ag(s) 20 Under which conditions of temperature and pressure does a sample of neon behave most like an ideal gas? (1) 100 K and 0.25 atm (2) 100 K and 25 atm (3) 400 K and 0.25 atm (4) 400 K and 25 atm 14 The relatively high boiling point of water is due to water having (1) hydrogen bonding (2) metallic bonding (3) nonpolar covalent bonding (4) strong ionic bonding 15 Matter is classified as a (1) substance, only (2) substance or as a mixture of substances (3) homogenous mixture, only (4) homogenous mixture or as a heterogeneous mixture 21 According to the kinetic molecular theory, which statement describes the particles in a sample of an ideal gas? (1) The force of attraction between the gas particles is strong. (2) The motion of the gas particles is random and straight-line. (3) The collisions between the gas particles cannot result in a transfer of energy between the particles. (4) The separation between the gas particles is smaller than the size of the gas particles themselves. 16 Which substance can not be decomposed by a chemical change? (1) ammonia (3) propanol (2) copper (4) water 17 A beaker contains both alcohol and water. These liquids can be separated by distillation because the liquids have different (1) boiling points (3) particle sizes (2) densities (4) solubilities 22 The activation energy of a chemical reaction can be decreased by the addition of (1) a catalyst (3) electrical energy (2) an indicator (4) thermal energy 18 Which term is defined as a measure of the average kinetic energy of the particles in a sample of matter? (1) activation energy (3) temperature (2) potential energy (4) entropy P.S./Chem. Aug. 09 23 A straight-chain hydrocarbon that has only one double bond in each molecule has the general formula (1) CnH2n 6 (3) CnH2n (2) CnH2n 2 (4) CnH2n+2 [3] [OVER] 24 Why can an increase in temperature lead to more effective collisions between reactant particles and an increase in the rate of a chemical reaction? (1) The activation energy of the reaction increases. (2) The activation energy of the reaction decreases. (3) The number of molecules with sufficient energy to react increases. (4) The number of molecules with sufficient energy to react decreases. 27 Which substance is an electrolyte? (3) HCl (1) CCl4 (2) C2H6 (4) H2O 28 One acid-base theory defines a base as an (3) H donor (1) H+ donor (2) H+ acceptor (4) H acceptor 29 A change in the nucleus of an atom that converts the atom from one element to another element is called (1) combustion (3) polymerization (2) neutralization (4) transmutation 25 Which reaction results in the production of soap? (1) esterification (3) polymerization (2) fermentation (4) saponification 30 Which particle is emitted from a hydrogen-3 nucleus when it undergoes radioactive decay? (1) (3) + (2) (4) 26 Which substance is always a product when an Arrhenius acid in an aqueous solution reacts with an Arrhenius base in an aqueous solution? (1) HBr (3) KBr (2) H2O (4) KOH P.S./Chem. Aug. 09 [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 an excited state for a potassium atom? (1) 2-8-7-1 (3) 2-8-8-1 (2) 2-8-7-2 (4) 2-8-8-2 37 Which formula represents strontium phosphate? (3) Sr2(PO4)3 (1) SrPO4 (2) Sr3PO8 (4) Sr3(PO4)2 38 Which Lewis electron-dot diagram represents calcium oxide? 32 A sample of an element is malleable and can conduct electricity. This element could be (1) H (3) S (2) He (4) Sn 2+ Ca O Ca (1) 33 Which general trend is demonstrated by the Group 17 elements as they are considered in order from top to bottom on the Periodic Table? (1) a decrease in atomic radius (2) a decrease in electronegativity (3) an increase in first ionization energy (4) an increase in nonmetallic behavior (2) 35 Which equation represents a decomposition reaction? CaCO3(s) CaO(s) + CO2(g) Cu(s) + 2AgNO3(aq) 2Ag(s) + Cu(NO3)2(aq) 2H2(g) + O2(g) 2H2O( ) KOH(aq) + HCl(aq) KCl(aq) + H2O( ) 2 O (4) 40 What is the mass of NH4Cl that must dissolve in 200. grams of water at 50. C to make a saturated solution? (1) 26 g (3) 84 g (2) 42 g (4) 104 g 36 A compound has the empirical formula CH2O and a gram-formula mass of 60. grams per mole. What is the molecular formula of this compound? (1) CH2O (3) C3H8O (2) C2H4O2 (4) C4H8O4 P.S./Chem. Aug. 09 Ca 39 Which statement describes the transfer of heat energy that occurs when an ice cube is added to an insulated container with 100 milliliters of water at 25 C? (1) Both the ice cube and the water lose heat energy. (2) Both the ice cube and the water gain heat energy. (3) The ice cube gains heat energy and the water loses heat energy. (4) The ice cube loses heat energy and the water gains heat energy. 34 Which element is a liquid at 758 K and standard pressure? (1) gold (3) platinum (2) silver (4) thallium (1) (2) (3) (4) (3) 2+ Ca O 2 O [5] [OVER] 41 Given the bright-line spectra of three elements and the spectrum of a mixture formed from at least two of these elements: Bright-Line Spectra Element D Element E Element G Mixture 750 nm 360 nm Which elements are present in this mixture? (1) E and D, only (2) E and G, only (3) D and G, only (4) D, E, and G 42 Given the balanced particle-diagram equation: Key = an atom of an element = an atom of a different element + Which statement describes the type of change and the chemical properties product and reactants? (1) The equation represents a physical change, with the product and reactants different chemical properties. (2) The equation represents a physical change, with the product and reactants identical chemical properties. (3) The equation represents a chemical change, with the product and reactants different chemical properties. (4) The equation represents a chemical change, with the product and reactants identical chemical properties. P.S./Chem. Aug. 09 [6] of the having having having having 43 Which quantity of heat is equal to 200. joules? (1) 20.0 kJ (3) 0.200 kJ (2) 2.00 kJ (4) 0.0200 kJ 47 Which formula represents an unsaturated hydrocarbon? H 44 Which graph represents the relationship between pressure and volume for a sample of an ideal gas at constant temperature? C C H H C C H H (1) H (3) H H Pressure Pressure H O H H H H C C H H C C OH H H (2) (3) 48 What is the oxidation state of nitrogen in the compound NH4Br? (1) 1 (3) 3 (2) +2 (4) +4 Pressure (1) (4) Volume Pressure Volume H H Volume Volume (2) 49 A student completes a titration by adding 12.0 milliliters of NaOH(aq) of unknown concentration to 16.0 milliliters of 0.15 M HCl(aq). What is the molar concentration of the NaOH(aq)? (1) 0.11 M (3) 1.1 M (2) 0.20 M (4) 5.0 M (4) 50 What is the half-life of a radioisotope if 25.0 grams of an original 200.-gram sample of the isotope remains unchanged after 11.46 days? (1) 2.87 d (3) 11.46 d (2) 3.82 d (4) 34.38 d 45 The entropy of a sample of H2O increases as the sample changes from a (1) gas to a liquid (3) liquid to a gas (2) gas to a solid (4) liquid to a solid 46 Ethanol and dimethyl ether have different chemical and physical properties because they have different (1) functional groups (2) molecular masses (3) numbers of covalent bonds (4) percent compositions by mass P.S./Chem. Aug. 09 [7] [OVER] Part B 2 Answer all questions in this part. Directions (51 63): 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 Identify the element in Period 3 of the Periodic Table that reacts with oxygen to form an ionic compound represented by the formula X2O. [1] 52 Given the balanced equation representing a reaction: 2C2H6 + 7O2 4CO2 + 6H2O Determine the total number of moles of oxygen that react completely with 8.0 moles of C2H6. [1] 53 On the potential energy diagram in your answer booklet, draw an arrow to represent the activation energy of the forward reaction. [1] 54 Describe the electrons in an atom of carbon in the ground state. Your response must include: the charge of an electron [1] the location of electrons based on the wave-mechanical model [1] the total number of electrons in a carbon atom [1] 55 Determine the mass of 5.20 moles of C6H12 (gram-formula mass = 84.2 grams/mole). [1] Base your answers to questions 56 through 58 on the information below. A 1.0-gram strip of zinc is reacted with hydrochloric acid in a test tube. The unbalanced equation below represents the reaction. Zn(s) + HCl(aq) H2(g) + ZnCl2(aq) 56 Balance the equation in your answer booklet for the reaction of zinc and hydrochloric acid, using the smallest whole-number coefficients. [1] 57 Explain, using information from Reference Table F, why the symbol (aq) is used to describe the product ZnCl2. [1] 58 Explain, in terms of collision theory, why using 1.0 gram of powdered zinc, instead of the 1.0-gram strip of zinc, would have increased the rate of the reaction. [1] P.S./Chem. Aug. 09 [8] Base your answers to questions 59 through 63 on the information below. Bond energy is the amount of energy required to break a chemical bond. The table below gives a formula and the carbon-nitrogen bond energy for selected nitrogen compounds. Selected Nitrogen Compounds Compound Formula Carbon-Nitrogen Bond Energy (kJ/mol) hydrogen cyanide H C N 890. H N C O 615 isocyanic acid H methanamine H C N H 293 H H 59 Describe, in terms of electrons, the type of bonding between the carbon atom and the nitrogen atom in a molecule of methanamine. [1] 60 Identify the noble gas that has atoms in the ground state with the same electron configuration as the nitrogen in a molecule of isocyanic acid. [1] 61 State the relationship between the number of electrons in a carbon-nitrogen bond and carbon-nitrogen bond energy. [1] 62 Explain, in terms of charge distribution, why a molecule of hydrogen cyanide is polar. [1] 63 A 3.2-gram sample of air contains 0.000 74 gram of hydrogen cyanide. Determine the concentration, in parts per million, of the hydrogen cyanide in this sample. [1] P.S./Chem. Aug. 09 [9] [OVER] Part C Answer all questions in this part. Directions (64 81): 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. 64 Based on data collected during a laboratory investigation, a student determined an experimental value of 322 joules per gram for the heat of fusion of H2O. Calculate the student s percent error. Your response must include a correct numerical setup and the calculated result. [2] Base your answers to questions 65 through 67 on the information below. A student used blue litmus paper and phenolphthalein paper as indicators to test the pH of distilled water and five aqueous household solutions. Then the student used a pH meter to measure the pH of the distilled water and each solution. The results of the student s work are recorded in the table below. Testing Results Liquid Tested Color of Blue Litmus Paper Color of Measured pH Phenolphthalein Value Using a Paper pH Meter 2% milk blue colorless 6.4 distilled water blue colorless 7.0 household ammonia blue pink 11.5 lemon juice red colorless 2.3 tomato juice red colorless 4.3 vinegar red colorless 3.3 65 Identify the liquid tested that has the lowest hydronium ion concentration. [1] 66 Explain, in terms of the pH range for color change on Reference Table M, why litmus is not appropriate to differentiate the acidity levels of tomato juice and vinegar. [1] 67 Based on the measured pH values, identify the liquid tested that is 10 times more acidic than vinegar. [1] P.S./Chem. Aug. 09 [10] Base your answers to questions 68 through 72 on the information below. Biodiesel is an alternative fuel for vehicles that use petroleum diesel. Biodiesel is produced by reacting vegetable oil with CH3OH. Methyl palmitate, C15H31COOCH3, a compound found in biodiesel, is made from soybean oil. One reaction of methyl palmitate with oxygen is represented by the balanced equation below. 2C15H31COOCH3 + 49O2 34CO2 + 34H2O + energy 68 Write an IUPAC name for the compound that reacts with vegetable oil to produce biodiesel. [1] 69 Explain, in terms of both atoms and molecular structure, why there is no isomer of CH3OH. [1] 70 Identify the class of organic compounds to which methyl palmitate belongs. [1] 71 Identify the type of organic reaction represented by the balanced equation. [1] 72 State evidence from the balanced equation that indicates the reaction is exothermic. [1] Base your answers to questions 73 through 76 on the information below. In a laboratory investigation, a student constructs a voltaic cell with iron and copper electrodes. Another student constructs a voltaic cell with zinc and iron electrodes. Testing the cells during operation enables the students to write the balanced ionic equations below. Cell with iron and copper electrodes: Cu2+(aq) + Fe(s) Cu(s) + Fe2+(aq) Cell with zinc and iron electrodes: Fe2+(aq) + Zn(s) Fe(s) + Zn2+(aq) 73 State evidence from the balanced equation for the cell with iron and copper electrodes that indicates the reaction in the cell is an oxidation-reduction reaction. [1] 74 Identify the particles transferred between Fe2+ and Zn during the reaction in the cell with zinc and iron electrodes. [1] 75 Write a balanced half-reaction equation for the reduction that takes place in the cell with zinc and iron electrodes. [1] 76 State the relative activity of the three metals used in these two voltaic cells. [1] P.S./Chem. Aug. 09 [11] [OVER] Base your answers to questions 77 through 79 on the information below. A method used by ancient Egyptians to obtain copper metal from copper(I) sulfide ore was heating the ore in the presence of air. Later, copper was mixed with tin to produce a useful alloy called bronze. 77 Calculate the density of a 129.5-gram sample of bronze that has a volume of 14.8 cubic centimeters. Your response must include a correct numerical setup and the calculated result. [2] 78 Convert the melting point of the metal obtained from copper(I) sulfide ore to degrees Celsius. [1] 79 A 133.8-gram sample of bronze was 10.3% tin by mass. Determine the total mass of tin in the sample. [1] Base your answers to questions 80 and 81 on the information below. Scientists are investigating the production of energy using hydrogen-2 nuclei (deuterons) and hydrogen-3 nuclei (tritons). The balanced equation below represents one nuclear reaction between two deuterons. 2H 1 3 1 13 J +2 1 H 2 He + 0 n + 5.23 10 80 State, in terms of subatomic particles, how a deuteron differs from a triton. [1] 81 Identify the type of nuclear reaction represented by the equation. [1] P.S./Chem. Aug. 09 [12] The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING Tear Here CHEMISTRY Thursday, August 13, 2009 12:30 to 3:30 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, August 13, 2009 12:30 to 3:30 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 AA Part Part B 1 Part B 1 1 . . . . .4 ....... 11 . . . . .1 ....... 21 . . . . 2 ....... 31 . . . . . 2 ....... 41 . . . . . 1 ....... 2 . . . . .3 ....... 12 . . . . .2 ....... 22 . . . . 1 ....... 32 . . . . . 4 ....... 42 . . . . . 3 ....... 3 . . . . .1 ....... 13 . . . . .4 ....... 23 . . . . 3 ....... 33 . . . . . 2 ....... 43 . . . . . 3 ....... 4 . . . . .1 ....... 14 . . . . .1 ....... 24 . . . . 3 ....... 34 . . . . . 4 ....... 44 . . . . . 4 ....... 5 . . . . .3 ....... 15 . . . . .2 ....... 25 . . . . 4 ....... 35 . . . . . 1 ....... 45 . . . . . 3 ....... 6 . . . . .3 ....... 16 . . . . .2 ....... 26 . . . . 2 ....... 36 . . . . . 2 ....... 46 . . . . . 1 ....... 7 . . . . .4 ....... 17 . . . . .1 ....... 27 . . . . 3 ....... 37 . . . . . 4 ....... 47 . . . . . 1 ....... 8 . . . . .2 ....... 18 . . . . .3 ....... 28 . . . . 2 ....... 38 . . . . . 4 ....... 48 . . . . . 3 ....... 9 . . . . .1 ....... 19 . . . . .4 ....... 29 . . . . 4 ....... 39 . . . . . 3 ....... 49 . . . . . 2 ....... 10 . . . . .1 ....... 20 . . . . .3 ....... 30 . . . . 2 ....... 40 . . . . . 4 ....... 50 . . . . . 2 ....... 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 check mark 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, August 13, 2009. 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 15 credits for this part. The student must answer all questions in this part. 51 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Na sodium element 11 52 [1] Allow 1 credit. Significant figures do not need to be shown. Acceptable responses include, but are not limited to: 28 mol 53 [1] Allow 1 credit. Potential Energy Example of a 1-credit response: Reaction Coordinate 54 [3] Allow a maximum of 3 credits, allocated as follows: Allow 1 credit for stating that an electron has a negative charge. Allow 1 credit for stating that electrons are located in orbitals or regions of most probable location. Allow 1 credit for stating that a carbon atom has six electrons. [4] PHYSICAL SETTING/CHEMISTRY continued 55 [1] Allow 1 credit. Significant figures do not need to be shown. Acceptable responses include, but are not limited to: 438 g 437.8 g 56 [1] Allow 1 credit for _____ Zn(s) + __2__ HCl(aq) _____ H2(g) + _____ ZnCl2(aq). Allow credit even if the coefficient 1 is written in front of Zn(s), H2(g), and/or ZnCl2(aq). 57 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The product ZnCl2 is soluble in water. 58 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The greater surface area in powdered zinc would have resulted in more frequent collisions between the zinc atoms and the hydrogen ions in the HCl(aq). 59 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The structural formula for methanamine shows electrons being shared, so the bond is covalent. Electrons are shared in the bond. covalent bonding due to shared electrons 60 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Ne neon element 10 [5] [OVER] PHYSICAL SETTING/CHEMISTRY continued 61 [1] Allow 1 credit. Acceptable responses include, but are not limited to: As the number of shared electrons in a carbon-nitrogen bond increases, the bond energy increases. Less energy is required to break a single carbon-nitrogen bond than to break a triple carbon-nitrogen bond. 62 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The molecule has an asymmetrical charge distribution. The molecule has an unequal distribution of charge. 63 [1] Allow 1 credit. Significant figures do not need to be shown. Acceptable responses include, but are not limited to: 230 ppm 2.31 102 ppm [6] PHYSICAL SETTING/CHEMISTRY continued Part C Allow a total of 20 credits for this part. The student must answer all questions in this part. 64 [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: 322 J/g 334 J/g 100 334 J/g 12 100 334 Allow 1 credit for a correct response or for a response consistent with the student s numerical setup. Significant figures do not need to be shown. Acceptable responses include, but are not limited to: 3.6% 4% Note: Do not allow credit for a numerical setup and calculated result that are not related to the concept assessed by the question. 65 [1] Allow 1 credit. Acceptable responses include, but are not limited to: household ammonia NH3(aq) 66 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Because litmus changes color in a pH range of 5.5 to 8.2, litmus cannot be used to differentiate between a pH of 3.3 and 4.3. Litmus is red for all pH values below 5.5. 67 [1] Allow 1 credit for lemon juice. [7] [OVER] PHYSICAL SETTING/CHEMISTRY continued 68 [1] Allow 1 credit for methanol or methyl alcohol. 69 [1] Allow 1 credit. Acceptable responses include, but are not limited to: With only one carbon atom bonded to one oxygen atom, there can be no rings or chains with branches in the molecular structure. There are too few atoms to create a different molecular structure. 70 [1] Allow 1 credit. Acceptable responses include, but are not limited to: ester esters 71 [1] Allow 1 credit. Acceptable responses include, but are not limited to: combustion 72 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The balanced equation shows energy as a product of the reaction. Energy is on the right side of the arrow. 73 [1] Allow 1 credit. Acceptable responses include, but are not limited to: The oxidation number of Cu2+ changes to 0. Iron s oxidation state changes from zero to +2. Oxidation numbers change during the reaction because electrons are transferred. 74 [1] Allow 1 credit. Acceptable responses include, but are not limited to: electrons e 75 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Fe2+ + 2e Fe [8] PHYSICAL SETTING/CHEMISTRY concluded 76 [1] Allow 1 credit. Acceptable responses include, but are not limited to: Zinc is more reactive than iron, and iron is more reactive than copper. The order of decreasing activity is Zn, Fe, Cu. Copper is least active and zinc is most active. 77 [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: 129.5 g d = m = V 14.8 cm3 129.5 14.8 Allow 1 credit for 8.75 g/cm3 or for a response consistent with the student s numerical setup. Significant figures do not need to be shown. Note: Do not allow credit for a numerical setup and calculated result that are not related to the concept assessed by the question. 78 [1] Allow 1 credit for 1084 C. 79 [1] Allow 1 credit. Significant figures do not need to be shown. Acceptable responses include, but are not limited to: 13.8 g 80 [1] Allow 1 credit. Acceptable responses include, but are not limited to: A deuteron has one neutron and a triton has two neutrons. A deuteron has one fewer neutron than a triton. 81 [1] Allow 1 credit. Acceptable responses include, but are not limited to: fusion thermonuclear fusion [9] [OVER] Regents Examination in Physical Setting/Chemistry August 2009 Chart for Converting Total Test Raw Scores to Final Examination Scores (Scaled Scores) The Chart for Determining the Final Examination Score for the August 2009 Regents Examination in Physical Setting/Chemistry will be posted on the Department s web site http://www.emsc.nysed.gov/osa/ on Thursday, August 13, 2009. 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 www.emsc.nysed.gov/osa/exameval. 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. [10] Map to Core Curriculum August 2009 Physical Setting/Chemistry Question Numbers Key Ideas Part A Standard 1 Part B 40, 43 40, 44, 61 36, 37, 48, 49, 52, 63 58, 59 Math Key Idea 1 Math Key Idea 2 Math Key Idea 3 Sci. Inquiry Key Idea 1 Sci. Inquiry Key Idea 2 Part C 64, 69, 77 64, 77, 78, 79 69, 74, 76 31, 32, 33, 34, 37, 42, 46, 48, 51, 57, 62 65, 66, 67, 68, 70, 71, 72, 73, 77 34 63 Sci. Inquiry Key Idea 3 78 Eng. Design Key Idea 1 Standard 2 Key Idea 1 Key Idea 2 Standard 6 39 38, 42 Key Idea 1 Key Idea 2 Key Idea 3 Key Idea 4 Key Idea 5 64 65, 67 Standard 7 Key Idea 1 Key Idea 2 Key Idea 3 Key Idea 4 Standard 4 Process Skills 31, 32, 33, 35, 36, 40, 41, 45, 46, 47, 48, 49, 51, 52, 54, 55, 56, 58, 63 50, 53 65, 66, 67, 70, 71, 75, 76, 80 72, 81 38, 59, 60 Key Idea 5 Standard 4 1, 2, 3, 4, 6, 7, 8, 12, 13, 15, 16, 17, 19, 20, 21, 22, 23, 24, 25, 26, 27, 28 Key Idea 4 18, 30 31, 32, 33, 34, 35, 36, 37, 40, 41, 42, 44, 45, 46, 47, 48, 49, 51, 52, 54, 55, 56, 57, 58, 63 39, 43, 50, 53 Key Idea 5 5, 9, 10, 11, 14, 29 38, 59, 60, 61, 62 Key Idea 3 2002 Edition Reference Tables 1, 2, 3, 7, 11, 12, 31, 32, 33, 34, 36, 23, 30 37, 38, 40, 43, 44, 46, 47, 48, 49, 50, 51, 55, 57, 59, 60, 63 [11] 65, 66, 67, 68, 69, 70, 71, 73, 74, 75, 76, 77, 78, 79, 80 64, 72, 81 64, 65, 66, 68, 70, 75, 77, 78

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

 

  Print intermediate debugging step

Show debugging info


 


Tags : New York State, High School Regents, Examinations, Past exams, solvedTest Papers, Education, Assessment and Testing.  


© 2010 - 2025 ResPaper. Terms of ServiceContact Us Advertise with us

 

regents chat