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Source: http://www.doksinet XIX. Chemistry, High School Source: http://www.doksinet 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.doemassedu/frameworks/currenthtml 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 Source: http://www.doksinet 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:298325 B Common EQ ID:281323 A Common EQ An equation for a chemical reaction is 1 shown below. 2H 2 (g) O 2 (g) H 2 O( l ) A student observed that the rate of 2 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? 571.6 kJ Which of the following statements indicates that this reaction is exothermic? A. The surface area of the product particles decreased. A. Energy is released B. A compound is formed B. The collision rate of the reactant particles increased. C. The reactants are two different gases. C. The concentrations of the reactant particles increased. D. There are more reactants than products. D. The concentrations of the product particles decreased. 344 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet Chemistry Session 1

ID:281214 D Common EQ ID:244829 244829 ASTDAV69.eps [opt A Common EQ Which of the following statements best 3 describes the current atomic theory? Which of the following equations shows 5 a fusion reaction? A. Electrons move in circular orbits around the nucleus. A. B. Electrons are held in an atom by their attraction to each other. 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. ID:273012 D Common EQ Which of the following molecules has a 4 nonpolar covalent bond? A. H–Br B. H–Cl C. H–F D. H–H 345 MCAS 2013 Gr10 CHEM RID 3 H 1 1 n 0 2 H 1 4 He 2 B. 238 U 92 234 Th 90 4 He 2 C. 24 Na 11 24 Mg 12 0 e –1 D. 01n 235 U 92 92 Kr 36 141 Ba 56 301n Source: http://www.doksinet Chemistry Session 1 ID:287594 A Common EQ ID:229548 D Common EQ Which of the following statements 6 describes what happens in a buffer

How many atoms of oxygen (O) are 7 required to form two molecules of solution when a strong acid is added? sulfuric acid (H2SO4)? A. The H ions from the strong acid combine with basic ions in the buffer. A. 2 B. The H ions from the strong acid combine with acidic ions in the buffer. C. 6 B. 4 D. 8 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. 346 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet Chemistry Session 1 ID:261464 B Common EQ Magnesium metal reacts with iron(III) sulfate to produce iron metal and magnesium sulfate, as 8 shown in the equation below. The molar mass of iron(III) sulfate is 3999 g/mol 3 Mg(s) Fe 2 ( SO4 )3 ( aq ) 2 Fe (s) 3MgSO4 ( aq ) How many grams of iron(III) sulfate are needed to completely react 6.0 g of magnesium? A. 20 g B. 33 g C. 99 g D. 300 g ID:264320 C Common EQ 9 ID:252675 C Common EQ 10 When a sample of a gas is

cooled, it condenses into a liquid. In which of the 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 following ways do the molecules of the original gas sample compare with the molecules of the liquid? energy A. The molecules are larger as a gas than they are as a liquid. After the reaction reaches equilibrium, which of the following changes would shift the equilibrium to the left? B. The molecules weigh less as a gas than they do as a liquid. A. adding more compound X to the equilibrium C. The molecules move faster as a gas than they do as a liquid. B. adding more compound Y to the equilibrium D. The molecules are closer together as a gas than they are as a liquid. C. increasing the temperature of the equilibrium D. decreasing the temperature of the equilibrium 347 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet 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 5.23 g Mass of crucible and iron powder 7.46 g x Mass of iron powder Mass of sulfur added to crucible 1.28 g Mass of crucible and contents after reaction 8.74 g Mass of iron-sulfur compound 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 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet 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? heat H2 O ( g ) B. H2 O ( l ) H2 O ( s ) C. H2 O ( l ) Na 2 O(s ) 2 Na ( aq ) 2OH (aq ) D. H2 O ( l ) NaCl(s ) Na (aq ) Cl (aq ) A. H2 O ( l ) heat ID:280897 280897 HI dot.eps [opt a0 A Common EQ heat H2 O ( l ) ID:281317 B Common EQ 13 Which of the following is a Lewis dot structure for hydrogen iodide (HI)? 14 Which of the following elements has both metallic and nonmetallic properties?

A. H I A. Ar B. Ge B. H I C. Mg D. S C. H I D. H I 349 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet Chemistry Session 1 ID:258906 C Common EQ ID:274049 A Common EQ 15 Uranium-234 decays to lead-214 through a series of alpha decays. Which of the 16 The chemical equation below represents the reaction of 1 mol of hydrogen gas following is the total number of alpha particles emitted in this decay series? A. 1 B. 2 C. 5 (H2) with 1 mol of chlorine gas (Cl2) in a sealed container at STP. The reaction produces 2 mol of hydrogen chloride gas (HCl) in the sealed container. H2 1 Cl2 2HCl What is the pressure in the container at standard temperature after the reaction is complete? D. 10 A. 1 atm B. 2 atm C. 3 atm D. 4 atm 350 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet 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. C. 3.0 2.0 1.0 0 B. 27 D. 2.0 1.0 1.0 27 250 Temperature (°C) 27 250 Temperature (°C) 3.0 2.0 1.0 0 250 Temperature (°C) 351 MCAS 2013 Gr10 CHEM RID 2.0 4.0 Pressure (atm) Pressure (atm) 3.0 27 3.0 0 250 Temperature (°C) 4.0 0 4.0 Pressure (atm) Pressure (atm) 4.0 Source: http://www.doksinet Chemistry Session 1 ID:281282 C Common EQ ID:275910 C Common EQ 18 A student puts an ice cube into a beaker and allows it to melt. Which of the 20 The table below provides data about a gas sample. following statements best describes what happens to the water molecules during this investigation? A. The molecules move apart until the

entire beaker is filled. Volume    1.0 L Pressure 303.9 kPa Temperature 323 K B. The molecules move apart until they are no longer touching each other. Which of the following can be determined using the data? C. The molecules become randomly arranged and can slide past each other. A. the chemical composition of the gas B. the condensation temperature of the gas D. The molecules become arranged in a pattern and maintain fixed positions. C. the number of gas molecules in the sample D. the distance between gas molecules in the sample ID:229556 3152531 AR1.eps B Common EQ 19 The diagram below shows a partial periodic table. O F The electron configuration of oxygen is 1s22s22p4. On the periodic table, fluorine is one space to the right of oxygen. Which of the following electron configurations represents fluorine? A. 1s22s22p3 B. 1s22s22p5 C. 1s22s22p63s23p3 D. 1s22s22p63s23p5 352 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet Chemistry Session 1 ID:287275

ASTDAV252 periodictable.e B Common EQ ID:298323 A Common EQ 21 What is the name of the compound with the chemical formula (NH NH ) S ? 22 The diagram below shows the relative locations of five unidentified elements in 4 2 the periodic table: E, X, G, J, and L. A. ammonium sulfide B. hydrogen sulfate E X G C. sulfur hydride D. sulfuric acid J 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 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet 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 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet 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 ID:281263 C Common EQ 24 A sample of vinegar has a pH of 5, and a sample of rainwater has a pH of 6. 25 The masses of the reactants and the theoretical

yields of the products for Which of the following statements best describes these two substances? a chemical reaction are shown below. 3Sb (1.2 g) A. Both samples are bases, and vinegar is more basic. 2SbI3 (3.2 g) Sb (0.4 g) When this reaction was performed in the laboratory, the actual yield for SbI3 was 2.4 g What was the percent yield for SbI3? B. Both samples are acids, and vinegar is more acidic. C. Both samples are bases, and rainwater is more basic. A. 25% D. Both samples are acids, and rainwater is more acidic. B. 67% C. 75% D. 100% 355 MCAS 2013 Gr10 CHEM RID 3I2 (2.4 g) Source: http://www.doksinet Chemistry Session 2 ID:287272 ASTDAV249.eps B Common EQ ID:260920 A 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) 27 The equation below represents an equilibrium reaction. HNO3(aq) The data for the reaction are

shown in the table below. Mass of Mg Mass of HCl Solution 0.24 g 5.49 g Total Mass of Substances in Beaker before the Reaction 5.73 g Total Mass of Substances in Beaker after the Reaction 5.71 g A. HNO3 B. NH3 C. NO3 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 MCAS 2013 Gr10 CHEM RID NO3 (aq) NH 4 (aq) Which chemical in the forward reaction is a Brønsted-Lowry acid? H 2(g) MgCl 2(aq) NH3(aq) Source: http://www.doksinet Chemistry Session 2 ID:261469 B Common EQ ID:261188 B Common EQ 30 An ionic solid is placed in a beaker of water. Which of the following occurs 28 A 20.0 mL sample of 015 M hydrochloric acid (HCl) is needed when there is a strong attraction between

the solute and the solvent? to neutralize a 10.0 mL sample of potassium hydroxide (KOH). A balanced equation for the reaction is shown below. HCl KOH KCl H2O A. The solute melts B. The solute dissolves C. The solute remains intact What is the molarity of the KOH solution? D. The solute reacts to form a precipitate A. 015 M B. 030 M C. 060 M D. 075 M ID:274067 A Common EQ 29 The white pigment in many paints is titanium dioxide (TiO ). It is made by 2 burning titanium(IV) chloride. The other product in this reaction is chlorine gas. What is the balanced equation for this reaction? A. TiC14 O2 TiO 2 2 C12 B. 2 TiC14 O2 TiO 2 4 C1 C. TiC14 2 O2 2 TiO 2 C12 D. 2 TiC14 2 O2 2 TiO 2 C14 357 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet Chemistry Session 2 ID:252651 A Common EQ ID:294713 D Common EQ 31 Calcium and boron react to form calcium boride, as represented by the 32 Methane gas (CH ) reacts with oxygen gas (O ) according to the 4 2

chemical equation below. Ca 6B CaB6 equation below. CH 4 Which type of reaction is shown by this equation? 2O 2 CO 2 2H 2O energy 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. combination B. decomposition A. The reaction is endothermic; CO 2 and H 2O have more chemical potential energy than CH 4 and O 2. C. double displacement D. single displacement B. The reaction is endothermic; CO 2 and H 2O have less chemical potential energy than CH 4 and O 2. C. The reaction is exothermic; CO 2 and H 2O have more chemical potential energy than CH 4 and O 2. D. The reaction is exothermic; CO 2 and H 2O have less chemical potential energy than CH 4 and O 2. 358 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet 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 O) occurs in smoke from forest fires and in automobile exhaust. 2 a. Calculate the total number of valence electrons in one molecule of formaldehyde Show your calculations. Carbon is the central atom in a CH2O 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 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet 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 ID:252565 C Common EQ 34 One mole of which of the following substances has the greatest entropy? 36 Which of the following is the electron configuration for sulfur? A. ethanol (l ) A. 1s 22s 22p 4 B. iron (s) B. 1s 22s 22p 63s 2 C. neon (g) C. 1s 22s 22p 63s 23p 4 D. water (l ) D. 1s 22s 22p 63s 23p 64s 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 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet Chemistry Session 2 ID:273186 A Common EQ ID:281218 281218 decay.eps B Common EQ 37 Uranium-238 undergoes radioactive decay according to the incomplete 39 Which of the following identifies the number and location of protons

in a equation below. 238U 92 lithium atom? 4He 2 X A. 3 protons, located in the nucleus What is the decay product represented by X? B. 7 protons, located in the nucleus A. 232 90 Th D. 7 protons, located in an atomic orbital C. 3 protons, located in an atomic orbital B. 234 90 Th ID:294699 D Common EQ C. 242 94 Pu D. 244 94 Pu 40 Although H O and H S have similar molecular geometries, they exist as 2 different states of matter at 20°C and 1 atm. Which of the following statements best explains why H 2O is a liquid and H 2S is a gas under these conditions? ID:281919 D Common EQ 38 Which of the following statements applies the law of multiple proportions to A. H 2O is less dense than H 2S B. H 2O is less chemically reactive than H 2S. the relationship between carbon monoxide (CO) and carbon dioxide (CO2)? C. H 2O has a smaller molecular mass than H 2S. A. The mass of a mole of CO is exactly half that of a mole of CO2. D. H 2O has stronger intermolecular forces

than H 2S. B. There will always be half as much CO as CO2 in a sample of gas. C. The proportion of oxygen atoms in CO molecules is the same as it is in CO2 molecules. D. The mass of oxygen in CO compared to that in CO2 can be expressed as a whole number ratio. 361 MCAS 2013 Gr10 CHEM RID 2 Source: http://www.doksinet Chemistry Session 2 ID:264326 B Common EQ ID:216954 C Common EQ 41 Based on valence electron configurations, which of the following 43 Particles of which of the following substances are farthest apart at STP? is a formula for a compound formed from sodium (Na) and oxygen (O)? A. aluminum (s) B. helium (g) A. NaO C. mercury (l ) B. NaO2 D. sodium (s) C. Na2O D. Na2O3 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 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet 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 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet 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 20 g sugar cube into 150 mL of 10°C water 2. Place an identical 20 g sugar cube into 150 mL of 50°C water 3. Place 20 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 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet Massachusetts Comprehensive Assessment System Chemistry Formula and Constants Sheet Common Polyatomic Ions Ion Ionic Formula Ammonium NH41 Carbonate CO32- Hydroxide OH- Nitrate NO3- Phosphate PO43- Sulfate SO42P1 V1 PV 5 2 2 T1 T2 Combined Gas Law: Ideal Gas Law: PV 5 nRT Dilution Formula: M1V1 5 M2V2 Molar Volume of Ideal Gas at STP: 22.4 L/mol Ideal Gas Constant: R 5 0.0821 L • atm/mol • K 5

831 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 [H3O1] 5 2log [H1] Avogadro’s Number: 6.02 3 1023 particles/mol Nuclear Symbols Name Symbol Alpha particle  or 42 He Beta particle b or −01 e Gamma ray  Neutron 1 0n 365 MCAS 2013 Gr10 CHEM RID MCAS 2013 Gr10 CHEM RID 366 Mg Ca 40.08 Sc 44.96 3B 3 Ti 47.88 4B 4 V 50.94 5B 5 atomic weight Symbol atomic number Name Cr 52.00 6B 6 Mn 54.94 7B 7 Sr 87.62 Ra Zr 91.22 Nb 92.91 Actinide Series Ta 180.95 W 183.85 Re 186.21 43 Tc (98) Os 190.23 44 Ru 101.07 89 Actinium Ac (227) 57 Pd 106.42 28 Nickel Ni 58.69 10 Sg (271) Bh (272) Hs (277) Mt (276) 77 Iridium Ir 192.22 Ds (281) 78 Platinum Pt 195.08 Ce 140.12 Pa 231.04 U 238.03 Np (237) 61 Pm (145) Pu (244) 62 Sm 150.36 Eu 151.96 Am (243) 92 94 90 93 91 95 Thorium Protactinium Uranium Neptunium Plutonium

Americium Th 232.04 60 Nd 144.24 80 Mercury Hg 200.59 48 Cadmium Cd 112.41 30 Zinc Zn 65.39 2B 12 P S Br 79.90 17 Chlorine Cl 81 Thallium Tl 204.38 49 Indium In 82 Lead Pb 207.2 50 Tin Sn 118.71 Te Po (209) At (210) 53 Iodine I 126.91 83 84 85 Bismuth Polonium Astatine Bi 208.98 51 52 Antimony Tellurium Sb 121.75 127.60 Se 78.96 16 Sulfur 35.45 9 Fluorine F 19.00 7A 17 114.82 As 74.92 Phosphorus 15 32.06 8 Oxygen O 16.00 6A 16 34 35 Selenium Bromine Ge 72.59 14 Silicon Si 30.97 7 Nitrogen N 14.01 5A 15 31 33 32 Gallium Germanium Arsenic Ga 69.72 13 Aluminum Al Gd 157.25 Tb 158.93 Dy 162.50 Ho 164.93 96 Curium Cm (247) 86 Radon Rn (222) 54 Xenon Xe 131.29 36 Krypton Kr 83.80 18 Argon Ar 39.95 10 Neon Ne 20.18 98 Cf (251) 99 Es (252) Fm (257) 68 Erbium Er 167.26 Yb 173.04 Lu 174.97 Md (258) No (259) Lr (262) 69 70 71 Thulium Ytterbium Lutetium Tm 168.93 100

102 103 101 Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium 97 Bk (247) 65 63 67 64 66 Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium 59 Pr 140.91 Roentgenium 111 Rg (280) 79 Gold Au 196.97 47 Silver Ag 107.87 29 Copper Cu 63.55 1B 11 28.09 6 Carbon 5 Boron 26.98 C 12.01 4A 14 B 10.81 3A 13 2 Helium He 4.00 8A 18 Mass numbers in parentheses are those of the most stable or most common isotope. 105 107 108 110 109 106 Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Db (268) 58 Lanthanum Cerium La 138.91 Rutherfordium 104 Rf (267) Rh 102.91 27 Cobalt Co 58.93 9 8B 45 46 Molybdenum Technetium Ruthenium Rhodium Palladium 42 Mo 95.94 26 Iron Fe 55.85 8 72 73 74 75 76 Hafnium Tantalum Tungsten Rhenium Osmium Hf 178.49 39 40 41 Yttrium Zirconium Niobium Y 88.91 Lanthanide Series 87 88 Francium Radium Fr (226) 56 Barium 55 Cesium (223) Ba

137.33 Cs 132.91 37 38 Rubidium Strontium Rb 85.47 19 20 21 22 23 24 25 Potassium Calcium Scandium Titanium Vanadium Chromium Manganese K 39.10 11 12 Sodium Magnesium Na 24.31 4 Beryllium 3 Lithium 22.99 Be 9.01 2A 2 Li 6.94 1 1 Hydrogen H Key: Periodic Table of the Elements *Revised based on IUPAC Commission on Atomic Weights and Isotopic Abundances, “Atomic Weights of the Elements 2007.” 7 6 5 4 3 2 1 1.01 Group (Family) 1A 1 Massachusetts Comprehensive Assessment System Source: http://www.doksinet Period Source: http://www.doksinet High School Chemistry Spring 2013 Released Items: Reporting Categories, Standards, and Correct Answers* Standard Correct Answer (MC)* Properties of Matter and Thermochemistry 6.4 A 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 Item No. Page No. 1 344 2 Reporting Category 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 MCAS 2013 Gr10 CHEM RID Source: http://www.doksinet Reporting Category Standard Correct Answer (MC)* Item No. Page No. 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 MCAS 2013 Gr10 CHEM RID