XIX. Chemistry, High School
High School Chemistry Test The spring 2013 high school Chemistry test was based on learning standards in the Chemistry content strand of the Massachusetts Science and Technology/Engineering Curriculum Framework (2006). These learning standards appear on pages 69 73 of the Framework. The Science and Technology/Engineering Curriculum Framework is available on the Department website at www.doe.mass.edu/frameworks/current.html. Chemistry test results are reported under the following four MCAS reporting categories: Atomic Structure and Periodicity Bonding and Reactions Properties of Matter and Thermochemistry Solutions, Equilibrium, and Acid-Base Theory Test Sessions The high school Chemistry test included two separate test sessions, which were administered on consecutive days. Each session included multiple-choice and open-response questions. Reference Materials and Tools Each student taking the high school Chemistry test was provided with a Chemistry Formula and Constants Sheet/Periodic Table of the Elements. Copies of both sides of this formula sheet follow the final question in this chapter. Each student also had sole access to a calculator with at least four functions and a square-root key. The use of bilingual word-to-word dictionaries was allowed for current and former English language learner students only, during both Chemistry test sessions. No other reference tools or materials were allowed. Cross-Reference Information The table at the conclusion of this chapter indicates each item s reporting category and the framework learning standard it assesses. The correct answers for multiple-choice questions are also displayed in the table. 343
Chemistry Session 1 DIRECTIONS This session contains twenty-one multiple-choice questions and two open-response questions. Mark your answers to these questions in the spaces provided in your Student Answer Booklet. You may work out solutions to multiple-choice questions in the test booklet. ID:281323 A Common EQ 1 An equation for a chemical reaction is shown below. 2H (g) O (g) H O( l ) 571.6 kj 2 2 2 Which of the following statements indicates that this reaction is exothermic? A. Energy is released. B. A compound is formed. C. The reactants are two different gases. D. There are more reactants than products. ID:298325 B Common EQ 2 A student observed that the rate of a chemical reaction increased as the temperature of the system increased. Which of the following statements best explains why thermal energy caused an increase in the reaction rate? A. The surface area of the product particles decreased. B. The collision rate of the reactant particles increased. C. The concentrations of the reactant particles increased. D. The concentrations of the product particles decreased. 344
Chemistry Session 1 ID:281214 D Common EQ 3 Which of the following statements best describes the current atomic theory? ID:244829 244829_ASTDAV69.eps [opt_ A Common EQ 5 Which of the following equations shows a fusion reaction? A. Electrons move in circular orbits around the nucleus. A. 3 H 1 2 H 1 4 He 2 1 n 0 B. Electrons are held in an atom by their attraction to each other. B. 238 U 92 234 Th 90 4 He 2 C. Electrons are evenly distributed throughout a mixture of positive and neutral particles. D. Electrons exist in specific energy levels and have both wave and particle characteristics. C. D. 1 n 0 24 Na 11 235 U 92 24 Mg 0 e 12 1 92 Kr 36 141 Ba 56 3 1 n 0 ID:273012 D Common EQ 4 Which of the following molecules has a nonpolar covalent bond? A. H Br B. H Cl C. H F D. H H 345
Chemistry Session 1 ID:287594 A Common EQ 6 Which of the following statements describes what happens in a buffer solution when a strong acid is added? A. The H ions from the strong acid combine with basic ions in the buffer. B. The H ions from the strong acid combine with acidic ions in the buffer. C. The OH ions from the strong acid combine with acidic ions in the buffer. D. The OH ions from the strong acid combine with basic ions in the buffer. ID:229548 D Common EQ 7 How many atoms of oxygen (O) are required to form two molecules of sulfuric acid (H 2 SO 4 )? A. 2 B. 4 C. 6 D. 8 346
Chemistry Session 1 ID:261464 B Common EQ 8 Magnesium metal reacts with iron(iii) sulfate to produce iron metal and magnesium sulfate, as shown in the equation below. The molar mass of iron(iii) sulfate is 399.9 g/mol. 3Mg(s) Fe ( SO ) ( aq) 2Fe (s) 3MgSO ( aq) 2 4 3 4 How many grams of iron(iii) sulfate are needed to completely react 6.0 g of magnesium? A. 2.0 g B. 33 g C. 99 g D. 300 g ID:264320 C Common EQ 9 In an experiment, a student mixes two compounds, X and Y, which react to give off energy and form compound Z, as shown in the equilibrium equation below. X Y Z energy After the reaction reaches equilibrium, which of the following changes would shift the equilibrium to the left? A. adding more compound X to the equilibrium B. adding more compound Y to the equilibrium C. increasing the temperature of the equilibrium D. decreasing the temperature of the equilibrium ID:252675 C Common EQ 10 When a sample of a gas is cooled, it condenses into a liquid. In which of the following ways do the molecules of the original gas sample compare with the molecules of the liquid? A. The molecules are larger as a gas than they are as a liquid. B. The molecules weigh less as a gas than they do as a liquid. C. The molecules move faster as a gas than they do as a liquid. D. The molecules are closer together as a gas than they are as a liquid. 347
Chemistry Session 1 Question 11 is an open-response question. BE SURE TO ANSWER AND LABEL ALL PARTS OF THE QUESTION. Show all your work (diagrams, tables, or computations) in your Student Answer Booklet. If you do the work in your head, explain in writing how you did the work. Write your answer to question 11 in the space provided in your Student Answer Booklet. ID:273070 273070_notebookpage.eps Common EQ 11 A page from a lab notebook is shown below. The page displays data needed to find the empirical formula of a compound. Mass of crucible Mass of crucible and iron powder Mass of iron powder Mass of sulfur added to crucible Mass of crucible and contents after reaction Mass of iron-sulfur compound 5.23 g 7.46 g x 1.28 g 8.74 g y a. Calculate the values for x and y. Show your calculations and include units in your answer. b. Assume all the iron and sulfur reacted to form an iron-sulfur compound. Calculate the number of moles of sulfur and the number of moles of iron that reacted to form the compound. Show your calculations and include units in your answer. c. Determine the empirical formula for the iron-sulfur compound. Show your calculations or explain your reasoning. 348
Chemistry Session 1 Mark your answers to multiple-choice questions 12 through 22 in the spaces provided in your Student Answer Booklet. Do not write your answers in this test booklet, but you may work out solutions to multiple-choice questions in the test booklet. ID:244815 C Common EQ 12 Which of the following equations shows a chemical change? A. H O( l ) heat H O( g) 2 2 B. H O( l ) H O( s) heat 2 2 2 2 2 C. H O( l ) Na O(s) Na ( aq) 2OH (aq) heat D. H O( l ) NaCl(s) Na (aq) Cl (aq) H O( l ) 2 2 ID:280897 280897_HI_dot.eps [opt_a0 A Common EQ 13 Which of the following is a Lewis dot structure for hydrogen iodide (HI)? A. H I B. H I ID:281317 B Common EQ 14 Which of the following elements has both metallic and nonmetallic properties? A. Ar B. Ge C. Mg D. S C. H I D. H I 349
Chemistry Session 1 ID:258906 C Common EQ 15 Uranium-234 decays to lead-214 through a series of alpha decays. Which of the following is the total number of alpha particles emitted in this decay series? A. 1 B. 2 C. 5 D. 10 ID:274049 A Common EQ 16 The chemical equation below represents the reaction of 1 mol of hydrogen gas (H 2 ) with 1 mol of chlorine gas (Cl 2 ) in a sealed container at STP. The reaction produces 2 mol of hydrogen chloride gas (HCl) in the sealed container. H 2 1 Cl 2 2HCl What is the pressure in the container at standard temperature after the reaction is complete? A. 1 atm B. 2 atm C. 3 atm D. 4 atm 350
Chemistry Session 1 ID:226997 3160092_AR1.eps [opt_a01, D Common EQ 17 Some manufacturers place rubber plugs in the bottoms of pressurized aerosol cans to prevent structural failure if the cans are exposed to excessive heat. The normal pressure inside an aerosol can is 2.0 atm at 27 C. When the temperature of the gas in the can is increased to 250 C, the pressure reaches 3.5 atm and the plug pops out. Which of the following graphs best shows the relationship of pressure to the temperature inside the can? A. 4.0 C. 4.0 Pressure (atm) 3.0 2.0 1.0 Pressure (atm) 3.0 2.0 1.0 0 27 250 Temperature ( C) 0 27 250 Temperature ( C) B. 4.0 D. 4.0 Pressure (atm) 3.0 2.0 1.0 Pressure (atm) 3.0 2.0 1.0 0 27 250 Temperature ( C) 0 27 250 Temperature ( C) 351
Chemistry Session 1 ID:281282 C Common EQ 18 A student puts an ice cube into a beaker and allows it to melt. Which of the following statements best describes what happens to the water molecules during this investigation? A. The molecules move apart until the entire beaker is filled. B. The molecules move apart until they are no longer touching each other. C. The molecules become randomly arranged and can slide past each other. D. The molecules become arranged in a pattern and maintain fixed positions. ID:229556 3152531_AR1.eps B Common EQ 19 The diagram below shows a partial periodic table. ID:275910 C Common EQ 20 The table below provides data about a gas sample. Volume 1.0 L Pressure Temperature 303.9 kpa 323 K Which of the following can be determined using the data? A. the chemical composition of the gas B. the condensation temperature of the gas C. the number of gas molecules in the sample D. the distance between gas molecules in the sample O F The electron configuration of oxygen is 1s 2 2s 2 2p 4. On the periodic table, fluorine is one space to the right of oxygen. Which of the following electron configurations represents fluorine? A. 1s 2 2s 2 2p 3 B. 1s 2 2s 2 2p 5 C. 1s 2 2s 2 2p 6 3s 2 3p 3 D. 1s 2 2s 2 2p 6 3s 2 3p 5 352
Chemistry Session 1 ID:298323 A Common EQ 21 What is the name of the compound with the chemical formula (NH ) S? A. ammonium sulfide B. hydrogen sulfate C. sulfur hydride D. sulfuric acid 4 2 ID:287275 ASTDAV252_periodictable.e B Common EQ 22 The diagram below shows the relative locations of five unidentified elements in the periodic table: E, X, G, J, and L. E X J G L Element X has an atomic number of z. Which unidentified element has an atomic number of z 1 2? A. element E B. element G C. element J D. element L 353
Chemistry Session 1 Question 23 is an open-response question. BE SURE TO ANSWER AND LABEL ALL PARTS OF THE QUESTION. Show all your work (diagrams, tables, or computations) in your Student Answer Booklet. If you do the work in your head, explain in writing how you did the work. Write your answer to question 23 in the space provided in your Student Answer Booklet. ID:272994 BELROB144.eps Common EQ 23 Particle models of four different types of matter are shown in the diagram below. Model 1 Model 2 Model 3 Model 4 a. Identify which of the four models best represents a pure compound. Explain your answer and give a specific example of a compound. b. Identify which of the four models best represents a homogeneous mixture. Explain your answer and give a specific example of a homogeneous mixture. c. Describe one method that could be used to separate a homogeneous mixture. 354
Chemistry Session 2 DIRECTIONS This session contains nineteen multiple-choice questions and three open-response questions. Mark your answers to these questions in the spaces provided in your Student Answer Booklet. You may work out solutions to multiple-choice questions in the test booklet. ID:273221 B Common EQ 24 A sample of vinegar has a ph of 5, and a sample of rainwater has a ph of 6. Which of the following statements best describes these two substances? A. Both samples are bases, and vinegar is more basic. B. Both samples are acids, and vinegar is more acidic. C. Both samples are bases, and rainwater is more basic. D. Both samples are acids, and rainwater is more acidic. ID:281263 C Common EQ 25 The masses of the reactants and the theoretical yields of the products for a chemical reaction are shown below. 3Sb 3I 2 2SbI 3 Sb (1.2 g) (2.4 g) (3.2 g) (0.4 g) When this reaction was performed in the laboratory, the actual yield for SbI 3 was 2.4 g. What was the percent yield for SbI 3? A. 25% B. 67% C. 75% D. 100% 355
Chemistry Session 2 ID:287272 ASTDAV249.eps B Common EQ 26 A student pours hydrochloric acid (HCl) into an open beaker that contains a piece of magnesium (Mg). A chemical reaction occurs, as shown in the equation below. 2HCl (aq) Mg (s) MgCl 2 (aq) H2( g) The data for the reaction are shown in the table below. Mass of Mg Mass of HCl Solution Total Mass of Substances in Beaker before the Reaction Total Mass of Substances in Beaker after the Reaction 0.24 g 5.49 g 5.73 g 5.71 g ID:260920 A Common EQ 27 The equation below represents an equilibrium reaction. HNO 3(aq) NH3( aq) NO 3 (aq) NH 4 (aq) Which chemical in the forward reaction is a Brønsted-Lowry acid? A. HNO 3 B. NH 3 C. NO 3 D. NH 4 Which of the following statements best explains why the total mass of the substances in the beaker before the reaction is different from the total mass after the reaction? A. The HCl and Mg react slowly. B. The hydrogen produced is a gas. C. The HCl and Mg react to form a precipitate. D. The magnesium chloride produced is soluble. 356
Chemistry Session 2 ID:261469 B Common EQ 28 A 20.0 ml sample of 0.15 M hydrochloric acid (HCl) is needed to neutralize a 10.0 ml sample of potassium hydroxide (KOH). A balanced equation for the reaction is shown below. HCl KOH KCl H 2 O What is the molarity of the KOH solution? ID:261188 B Common EQ 30 An ionic solid is placed in a beaker of water. Which of the following occurs when there is a strong attraction between the solute and the solvent? A. The solute melts. B. The solute dissolves. C. The solute remains intact. D. The solute reacts to form a precipitate. A. 0.15 M B. 0.30 M C. 0.60 M D. 0.75 M ID:274067 A Common EQ 29 The white pigment in many paints is titanium dioxide (TiO 2 ). It is made by burning titanium(iv) chloride. The other product in this reaction is chlorine gas. What is the balanced equation for this reaction? A. TiC1 TiO 2C1 4 O 2 2 2 B. 2TiC14 O2 TiO2 4C1 C. TiC1 2O 2TiO C1 4 2 2 2 D. 2TiC14 2O2 2TiO2 C14 357
Chemistry Session 2 ID:252651 A Common EQ 31 Calcium and boron react to form calcium boride, as represented by the chemical equation below. Ca 6B CaB 6 Which type of reaction is shown by this equation? A. combination B. decomposition C. double displacement D. single displacement ID:294713 D Common EQ 32 Methane gas (CH 4 ) reacts with oxygen gas (O 2 ) according to the equation below. CH 2O CO 2H O energy 4 2 2 2 This reaction releases 890 kj of energy for each mole of methane gas that is consumed. Which of the following statements best describes this reaction? A. The reaction is endothermic; CO 2 and H 2 O have more chemical potential energy than CH 4 and O 2. B. The reaction is endothermic; CO 2 and H 2 O have less chemical potential energy than CH 4 and O 2. C. The reaction is exothermic; CO 2 and H 2 O have more chemical potential energy than CH 4 and O 2. D. The reaction is exothermic; CO 2 and H 2 O have less chemical potential energy than CH 4 and O 2. 358
Chemistry Session 2 Question 33 is an open-response question. BE SURE TO ANSWER AND LABEL ALL PARTS OF THE QUESTION. Show all your work (diagrams, tables, or computations) in your Student Answer Booklet. If you do the work in your head, explain in writing how you did the work. Write your answer to question 33 in the space provided in your Student Answer Booklet. ID:260794 ASTDAV148.eps Common EQ 33 Formaldehyde (CH 2 O) occurs in smoke from forest fires and in automobile exhaust. a. Calculate the total number of valence electrons in one molecule of formaldehyde. Show your calculations. Carbon is the central atom in a CH 2 O molecule. b. Draw a Lewis dot structure for formaldehyde. c. Identify the shape of the formaldehyde molecule predicted by valence-shell electron-pair repulsion (VSEPR) theory. Explain your answer. 359
Chemistry Session 2 Mark your answers to multiple-choice questions 34 through 43 in the spaces provided in your Student Answer Booklet. Do not write your answers in this test booklet, but you may work out solutions to multiple-choice questions in the test booklet. ID:260916 C Common EQ 34 One mole of which of the following substances has the greatest entropy? A. ethanol (l ) B. iron (s) C. neon (g) D. water (l ) ID:252565 C Common EQ 36 Which of the following is the electron configuration for sulfur? A. 1s 2 2s 2 2p 4 B. 1s 2 2s 2 2p 6 3s 2 C. 1s 2 2s 2 2p 6 3s 2 3p 4 D. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 ID:288269 D Common EQ 35 Which of the following statements explains why people spread salt on icy sidewalks in the winter? A. The salt causes the ice to undergo sublimation. B. The salt lowers the surface tension of melted ice. C. The ice-salt mixture has a higher density than ice has. D. The ice-salt mixture melts at a lower temperature than ice does. 360
Chemistry Session 2 ID:281218 281218_decay.eps B Common EQ 37 Uranium-238 undergoes radioactive decay according to the incomplete equation below. 238 U 4 92 2 He X What is the decay product represented by X? A. 232 90Th ID:273186 A Common EQ 39 Which of the following identifies the number and location of protons in a lithium atom? A. 3 protons, located in the nucleus B. 7 protons, located in the nucleus C. 3 protons, located in an atomic orbital D. 7 protons, located in an atomic orbital B. 234 90Th C. 242 94 Pu D. 244 94 Pu ID:281919 D Common EQ 38 Which of the following statements applies the law of multiple proportions to the relationship between carbon monoxide (CO) and carbon dioxide (CO 2 )? A. The mass of a mole of CO is exactly half that of a mole of CO 2. B. There will always be half as much CO as CO 2 in a sample of gas. C. The proportion of oxygen atoms in CO molecules is the same as it is in CO 2 molecules. D. The mass of oxygen in CO compared to that in CO 2 can be expressed as a whole number ratio. ID:294699 D Common EQ 40 Although H 2 O and H 2 S have similar molecular geometries, they exist as different states of matter at 20 C and 1 atm. Which of the following statements best explains why H 2 O is a liquid and H 2 S is a gas under these conditions? A. H 2 O is less dense than H 2 S. B. H 2 O is less chemically reactive than H S 2. C. H 2 O has a smaller molecular mass than H S 2. D. H 2 O has stronger intermolecular forces than H S 2. 361
Chemistry Session 2 ID:216954 C Common EQ 41 Based on valence electron configurations, which of the following is a formula for a compound formed from sodium (Na) and oxygen (O)? A. NaO B. NaO 2 C. Na 2 O ID:264326 B Common EQ 43 Particles of which of the following substances are farthest apart at STP? A. aluminum (s) B. helium (g) C. mercury (l ) D. sodium (s) D. Na 2 O 3 ID:287563 D Common EQ 42 Which of the following statements describes a difference between a chemical change and a physical change in a substance? A. A physical change occurs only in elements; a chemical change occurs only in compounds. B. A chemical change occurs only in elements; a physical change occurs only in compounds. C. The result of a physical change is a different composition; in a chemical change, the composition remains the same. D. The result of a chemical change is a different composition; in a physical change, the composition remains the same. 362
Chemistry Session 2 Questions 44 and 45 are open-response questions. BE SURE TO ANSWER AND LABEL ALL PARTS OF EACH QUESTION. Show all your work (diagrams, tables, or computations) in your Student Answer Booklet. If you do the work in your head, explain in writing how you did the work. Write your answer to question 44 in the space provided in your Student Answer Booklet. ID:274045 Common EQ 44 Since elements are listed in the periodic table in order of increasing atomic number and arranged so that elements with similar properties fall into the same group, the periodic table can be used to predict similarities and differences between elements. a. Bromine and fluorine are both in group 17 (7A) of the periodic table. Describe two properties of bromine and fluorine that are the same. b. Bromine and fluorine are in different periods in the periodic table. Describe two properties of bromine and fluorine that are different. c. Based on their positions in the periodic table, bromine and fluorine are most likely to form ionic compounds with an element from which group: group 1 (1A), group 14 (4A), or group 18 (8A)? Explain your choice. 363
Chemistry Session 2 Write your answer to question 45 in the space provided in your Student Answer Booklet. ID:294716 Common EQ 45 A student follows the procedure below to determine how two variables will affect the dissolution rate of sugar in water. 1. Place a 2.0 g sugar cube into 150 ml of 10 C water. 2. Place an identical 2.0 g sugar cube into 150 ml of 50 C water. 3. Place 2.0 g of granulated sugar into 150 ml of 50 C water. 4. Stir the three sugar-water mixtures equally. 5. Measure the time it takes for all of the sugar in each mixture to dissolve. a. Identify the two variables being tested in the procedure. b. Describe the most likely effect each variable in part (a) has on the rate at which the sugar dissolves in water. Explain your reasoning. c. Write a procedure to test the effect solvent volume has on the rate at which sugar dissolves in water. d. Describe the expected results for the procedure you wrote in part (c). Explain your reasoning. 364
Massachusetts Comprehensive Assessment System Chemistry Formula and Constants Sheet Common Polyatomic Ions Ion Ionic Formula Ammonium NH 1 4 Carbonate CO 2-3 Hydroxide OH - Nitrate NO - 3 Phosphate PO 3-4 Sulfate SO 2-4 Combined Gas Law: P V T 1 1 Ideal Gas Law: PV 5 nrt 1 5 P V T 2 2 2 Dilution Formula: M 1 V 1 5 M 2 V 2 Molar Volume of Ideal Gas at STP: 22.4 L/mol Ideal Gas Constant: R 5 0.0821 L atm/mol K 5 8.31 L kpa/mol K STP: 1 atm (101.3 kpa), 273 K (0 C) Absolute Temperature Conversion: K 5 C 1 273 Definition of ph: ph 5 2log [H 3 O 1 ] 5 2log [H 1 ] Avogadro s Number: 6.02 3 10 23 particles/mol Nuclear Symbols Name Alpha particle Beta particle Gamma ray Symbol or 4 2 He b or 0 1 e Neutron 1 0n 365
Group (Family) 1A 1 1 2 3 4 5 6 7 1.01 H 1 Hydrogen 6.94 1 Li 3 Lithium 22.99 Na 11 Sodium 39.10 K 19 Potassium 85.47 Rb 37 Rubidium 132.91 Cs 55 Cesium (223) Fr 87 Francium 2A 2 9.01 Be 4 Beryllium 24.31 Mg 12 Magnesium 40.08 Ca 20 Calcium 87.62 Sr 38 Strontium 137.33 Ba 56 Barium (226) Ra 88 Radium 3B 3 44.96 Sc 21 Scandium 88.91 Y 39 Yttrium Key: atomic weight Symbol atomic number Name 4B 4 47.88 Ti 22 Titanium 91.22 Zr 40 Zirconium 178.49 Hf 72 Hafnium (267) Rf 104 Rutherfordium Massachusetts Comprehensive Assessment System 5B 5 50.94 V 23 Vanadium 92.91 Nb 41 Niobium 180.95 Ta 73 Tantalum (268) Db 105 Dubnium 6B 6 52.00 Cr 24 Chromium 95.94 Mo 42 Molybdenum 183.85 W 74 Tungsten (271) Sg 106 Seaborgium Periodic Table of the Elements 7B 7 54.94 Mn 25 Manganese (98) Tc 43 Technetium 186.21 Re 75 Rhenium (272) Bh 107 Bohrium 55.85 Fe 26 Iron 101.07 Ru 44 8B 8 9 10 Ruthenium 190.23 Os 76 Osmium (277) Hs 108 Hassium 58.93 Co 27 Cobalt 102.91 Rh 45 Rhodium 192.22 Ir 77 Iridium (276) Mt 109 Meitnerium 58.69 Ni 28 Nickel 106.42 Pd 46 Palladium 195.08 Pt 78 Platinum (281) 110 1B 11 63.55 Cu 29 Copper 107.87 Ag 47 Silver 196.97 Au 79 Gold (280) Ds Rg 111 Darmstadtium Roentgenium 2B 12 65.39 Zn 30 Zinc 112.41 Cd 48 Cadmium 200.59 Hg 80 Mercury 3A 13 10.81 B 5 Boron 26.98 Al 13 Aluminum 69.72 Ga 31 Gallium 114.82 In 49 Indium 204.38 Tl 81 Thallium 4A 14 12.01 C 6 Carbon 28.09 Si 14 Silicon 72.59 Ge 32 Germanium 118.71 Sn 50 Tin 207.2 Pb 82 Lead 5A 15 14.01 N 7 Nitrogen 30.97 P 15 Phosphorus 74.92 As 33 Arsenic 121.75 Sb 51 Antimony 208.98 Bi 83 Bismuth 6A 16 16.00 O 8 Oxygen 32.06 S 16 Sulfur 78.96 Se 34 Selenium 127.60 Te 52 Tellurium (209) Po 84 Polonium 7A 17 19.00 F 9 Fluorine 35.45 Cl 17 Chlorine 79.90 Br 35 Bromine 126.91 I 53 Iodine (210) At 85 Astatine 8A 18 4.00 He 2 Helium 20.18 Ne 10 Neon 39.95 Ar 18 Argon 83.80 Kr 36 Krypton 131.29 Xe 54 Xenon (222) Rn 86 Radon Mass numbers in parentheses are those of the most stable or most common isotope. Lanthanide Series Actinide Series 138.91 La 57 Lanthanum (227) Ac 89 Actinium 140.12 Ce 58 Cerium 232.04 Th 90 Thorium 140.91 Pr 59 Praseodymium 231.04 Pa 91 Protactinium 144.24 Nd 60 Neodymium 238.03 U 92 Uranium (145) Pm 61 Promethium (237) Np 93 Neptunium 150.36 Sm 62 Samarium (244) Pu 94 Plutonium 151.96 Eu 63 Europium (243) Am 95 Americium 157.25 Gd 64 Gadolinium (247) Cm 96 Curium 158.93 Tb 65 Terbium (247) Bk 97 Berkelium 162.50 Dy 66 Dysprosium (251) Cf 98 Californium 164.93 Ho 67 Holmium (252) Es 99 Einsteinium 167.26 Er 68 Erbium (257) Fm 100 Fermium 168.93 Tm 69 Thulium (258) Md 101 Mendelevium 173.04 Yb 70 Ytterbium (259) No 102 Nobelium 174.97 Lu 71 Lutetium (262) Lr 103 Lawrencium *Revised based on IUPAC Commission on Atomic Weights and Isotopic Abundances, Atomic Weights of the Elements 2007. Period 366
High School Chemistry Spring 2013 Released Items: Reporting Categories, Standards, and Correct Answers* Item No. Page No. Reporting Category Standard Correct Answer (MC)* 1 344 Properties of Matter and Thermochemistry 6.4 A 2 344 Solutions, Equilibrium, and Acid-Base Theory 7.5 B 3 345 Atomic Structure and Periodicity 2.1 D 4 345 Bonding and Reactions 4.3 D 5 345 Atomic Structure and Periodicity 2.7 A 6 346 Solutions, Equilibrium, and Acid-Base Theory 8.3 A 7 346 Bonding and Reactions 5.3 D 8 347 Bonding and Reactions 5.5 B 9 347 Solutions, Equilibrium, and Acid-Base Theory 7.6 C 10 347 Properties of Matter and Thermochemistry 6.3 C 11 348 Bonding and Reactions 5.4 12 349 Properties of Matter and Thermochemistry 1.1 C 13 349 Bonding and Reactions 4.2 A 14 349 Atomic Structure and Periodicity 3.2 B 15 350 Atomic Structure and Periodicity 2.5 C 16 350 Properties of Matter and Thermochemistry 6.2 A 17 351 Properties of Matter and Thermochemistry 6.1 D 18 352 Properties of Matter and Thermochemistry 1.3 C 19 352 Atomic Structure and Periodicity 3.3 B 20 352 Properties of Matter and Thermochemistry 6.2 C 21 353 Bonding and Reactions 4.6 A 22 353 Atomic Structure and Periodicity 3.1 B 23 354 Properties of Matter and Thermochemistry 1.2 24 355 Solutions, Equilibrium, and Acid-Base Theory 8.2 B 25 355 Bonding and Reactions 5.6 C 26 356 Atomic Structure and Periodicity 2.3 B 27 356 Solutions, Equilibrium, and Acid-Base Theory 8.1 A 28 357 Solutions, Equilibrium, and Acid-Base Theory 7.2 B 29 357 Bonding and Reactions 5.1 A 30 357 Solutions, Equilibrium, and Acid-Base Theory 7.1 B 31 358 Bonding and Reactions 5.2 A 32 358 Properties of Matter and Thermochemistry 6.4 D 33 359 Bonding and Reactions 4.4 34 360 Properties of Matter and Thermochemistry 6.5 C 35 360 Solutions, Equilibrium, and Acid-Base Theory 7.4 D 36 360 Atomic Structure and Periodicity 2.4 C 37 361 Atomic Structure and Periodicity 2.6 B 38 361 Atomic Structure and Periodicity 2.3 D 39 361 Atomic Structure and Periodicity 2.2 A 40 361 Bonding and Reactions 4.5 D 367
Item No. Page No. Reporting Category Standard Correct Answer (MC)* 41 362 Bonding and Reactions 4.1 C 42 362 Properties of Matter and Thermochemistry 1.1 D 43 362 Properties of Matter and Thermochemistry 1.3 B 44 363 Atomic Structure and Periodicity 3.4 45 364 Solutions, Equilibrium, and Acid-Base Theory 7.3 * Answers are provided here for multiple-choice items only. Sample responses and scoring guidelines for open-response items, which are indicated by shaded cells, will be posted to the Department s website later this year. 368