RELEASED. NC Final Exam. Chemistry. Released Items. Student Name:

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1 Released Items Student Name: hemistry RELESE Public Schools of North arolina epartment of Public Instruction State oard of Education ivision of ccountability Services/North arolina Testing Program N Final Exam opyright 2018 by the North arolina epartment of Public Instruction. ll rights reserved.

2 HEMISTRY RELESE I TEMS 1 Which isotope has the greatest number of protons? Pa-238 U-240 Np-238 Pu neutral atom of a certain element has the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 4. How many valence electrons does the atom have? What color of light does a hydrogen atom emit when an electron transitions from the n=6 energy level to the n=2 energy level? orange yellow blue violet RELESE 1 Go to the next page.

3 HEMISTRY RELESE I TEMS 4 The equation below represents the radioactive decay of a gold isotope. u Ir +? Which choice correctly completes this equation? alpha particle beta particle photon neutron 5 neutral atom has a ground state electron configuration of 1s 2 2s 2 2p 6 3s 2. The neutral atom becomes an ion during a chemical reaction. Which is the most likely charge of the ion? How many electrons are in the outermost energy level of a neutral carbon atom? RELESE 2 Go to the next page.

4 HEMISTRY RELESE I TEMS 7 The compound sodium chloride is placed in water and separates into ions. What are the correct names for these ions? The chloride and sodium ions are cations. The chloride and sodium ions are anions. The sodium ion is the anion, and the chloride ion is the cation. The sodium ion is the cation, and the chloride ion is the anion. 8 Which element will form covalent bonds with chlorine? carbon aluminum magnesium potassium 9 Which type of bonding or intermolecular forces is/are weakest? London dispersion forces hydrogen bonding dipole-dipole forces covalent bonding RELESE 3 Go to the next page.

5 HEMISTRY RELESE I TEMS 10 What is the chemical formula for chromium(iii) oxide? ro ro 2 r 2 O 3 r 3 O 2 11 Test results on two white crystalline solids are shown in the table below: ased on the information in the table, what can be concluded? Solid X oth solids contain only ionic bonds. oth solids contain only covalent bonds. Solid Y Melting Point Solubility in Water (grams per grams of water) Electrical onductivity (molten state) good conductor nonconductor RELESE Solid X contains only covalent bonds, and Solid Y contains only ionic bonds. Solid X contains only ionic bonds, and Solid Y contains only covalent bonds. 4 Go to the next page.

6 HEMISTRY RELESE I TEMS 12 What is the name of the compound with the chemical formula of 3? fluorocobalt cobalt trifluoride cobalt(iii) fluoride fluorine(iii) cobalt 13 Which statement best compares how bond strengths affect the physical properties of iron and lead? Iron has a higher melting point because the bonds in iron are stronger. Iron has a higher melting point because the bonds in iron are weaker. Lead has a higher density because the bonds in lead are stronger. Lead has a higher density because the bonds in lead are weaker. 14 How is copper (u) classified based on its location on the periodic table? a nonmetal an alkaline earth metal a transition metal an alkali metalrelese 5 Go to the next page.

7 HEMISTRY RELESE I TEMS 15 The table below shows the electron configurations of three elements. Element Electron onfiguration Element 1 1s 2 2s 2 2p 2 Element 2 1s 2 2s 2 2p 5 Element 3 1s 2 2s 2 2p 4 What is the order of the elements from smallest to largest atomic radius? Element 1, Element 2, Element 3 Element 1, Element 3, Element 2 Element 2, Element 1, Element 3 Element 2, Element 3, Element 1 16 Which three elements are arranged according to increasing electronegativity values? N,, N, P, s N, O, F F, O, N 17 Which group of elements is arranged in order of increasing atomic radii? O, S, Se, Te Fe, Ni, g, u Rb, K, Na, Li Y, Zr, Nb, MoRELESE 6 Go to the next page.

8 HEMISTRY RELESE I TEMS 18 Which statement describes equilibrium between liquid water and water vapor? The rate of vaporization equals the rate of condensation. The rate of vaporization is greater than the rate of condensation. The rate of vaporization equals the rate of sublimation. The rate of vaporization is greater than the rate of sublimation. 19 phase diagram is shown below. 2.0 Pressure (atm) 1.0 RELESE Temperature ( ) Which choice describes the state of the substance at X? X boiling liquid is in equilibrium with its vapor. subliming solid is in equilibrium with its vapor. freezing liquid is in equilibrium with its solid. melting solid is in equilibrium with its liquid. 7 Go to the next page.

9 HEMISTRY RELESE I TEMS 20 sample of metal has a mass of 5.2 g and absorbs 20.0 J of energy as it is heated from 30.0 to What is the identity of the metal? iron gold copper magnesium liter closed container holds 1.0 mole of an ideal gas at a certain temperature and pressure. Which closed container will hold 3.0 moles of this ideal gas at the same temperature and pressure? a 3.0-liter container a 6.0-liter container a 9.0-liter container a 12.0-liter container RELESE 8 Go to the next page.

10 HEMISTRY RELESE I TEMS 22 phase diagram is shown below. X Pressure (kpa) RELESE Temperature ( ) What is the condition of the sample at point X? The sample is in a gaseous state. The sample is in a liquid state. The sample is at its critical point. The sample is at its triple point. 9 Go to the next page.

11 HEMISTRY RELESE I TEMS 23 What is the approximate temperature of 1.4 moles of a gas with a pressure of 3.25 atmospheres in a liter container? 180 K 170 K 150 K 130 K RELESE 10 Go to the next page.

12 HEMISTRY RELESE I TEMS 24 potential energy diagram of a chemical reaction is shown below. Potential Energy of a hemical Reaction 10 Which choice would be changed by the addition of a catalyst to the reaction? R Potential Energy (J) R S Reaction oordinate RELESE U T S T U 11 Go to the next page.

13 HEMISTRY RELESE I TEMS 25 student conducts the following demonstration: 15-g sample of NaHO 3 is placed in a test tube. The bottom of the test tube is heated with an open flame. ondensation forms on the inside walls of the test tube. burning splint is extinguished when placed at the mouth of the test tube. What can the student conclude after conducting this demonstration? The burning splint was extinguished because of a lack of O 2 in the test tube. The burning splint was extinguished because of a lack of H 2 O vapor. ecomposition produced O 2 and H 2 O. ombustion produced O 2 and H 2 O. 26 chemical equation is shown below. aso 4 + lr 3 ar 2 + l 2 (SO 4 ) 3 What will be the coefficient of ar 2 when the equation is balanced using the smallest possible whole-number coefficients? RELESE 12 Go to the next page.

14 HEMISTRY RELESE I TEMS 27 The equation below represents a chemical reaction. Zn (s) + 2Hl (aq) Znl 2 (aq) + H 2 (g) 5.00-g sample of zinc is added to hydrochloric acid. The amount of hydrochloric acid is sufficient to allow the zinc to react completely. What mass of hydrogen gas does this reaction produce? g g g g 28 What is the molecular formula of a compound with the empirical formula H 2 O and a molecular mass of 60 g/mol? H 2 O 2 H 4 O 2 2 H 4 O 4 2 H 2 O 2 RELESE 13 Go to the next page.

15 HEMISTRY RELESE I TEMS 29 student experimented with magnesium ribbon and hydrochloric acid. The student placed a piece of solid magnesium ribbon in a test tube containing hydrochloric acid solution. The student observed that vigorous bubbling occurred. The student collected some of the gas generated by the bubbles in a test tube. The student tested the gas produced with a burning wood splint, which ignited quickly with a popping sound. What can the student conclude about the experiment? chemical reaction occurred because new atoms were created. chemical reaction occurred because a new substance was formed. The popping sound provided evidence that the acid changed physical states. The popping sound provided evidence that the magnesium atoms were destroyed. 30 How many O 2 particles are in 2.50 moles of O 2 at Standard Temperature and Pressure (STP)? particles particles particles particles RELESE 14 Go to the next page.

16 HEMISTRY RELESE I TEMS 31 Why does an increase in temperature usually increase the rate of a chemical reaction? because the activation energy of the reaction increases because the surface area of reacting particles increases because the proper orientation of reacting particles improves because the number of effective collisions between reacting particles increases 32 The chemical equation below represents a reaction at equilibrium in a closed flask. Which action will cause the reaction to shift to the left? heating the flask with a hot plate placing the flask in an ice bath removing H 2 O from the flask adding O to the flask RELESE 15 Go to the next page.

17 HEMISTRY RELESE I TEMS 33 In a hypothetical reaction, reactants X and Y are combined in an evacuated vessel and allowed to come to equilibrium with product Z at a temperature of 200K. X (g) + Y (g) Z (g) fter equilibrium is established, the temperature is slowly raised, and additional values of K eq are determined as shown in this data table: Temperature K eq 200K K K K Which temperature has the greatest concentration of product Z? 200K 300K 400K 500K RELESE 16 Go to the next page.

18 HEMISTRY RELESE I TEMS 34 n equilibrium is established between substances W, X, Y, and Z. W + X Y + Z How would the conditions of equilibrium be affected by decreasing the concentration of substance W? Substances X and Y would react to replace substance W, and the position of equilibrium would shift to the right. Substances Y and Z would react to replace substance W, and the position of equilibrium would shift to the left. This would increase pressure, causing only substance Y to replace substance W and shifting the equilibrium to the right. This would decrease temperature, causing only substance Z to replace substance W and shifting the equilibrium to the left. 35 solution has a poh of 12. Which best describes the solution? It has a ph of 2 and is a base. It has a ph of 12 and is a base. It has a ph of 2 and is an acid. It has a ph of 12 and is an acid. RELESE 36 student describes a liquid as feeling slippery. The student places red litmus paper into the liquid, and the paper turns blue. What can the student conclude from these observations? The substance is likely a nonmetal. The substance is likely a metal. The substance is likely a base. The substance is likely an acid. 17 Go to the next page.

19 HEMISTRY RELESE I TEMS 37 n acid-base titration is represented by the chemical equation below. soh (aq) + Hr (aq) sr (aq) + H 2 O (l) In the titration, 15.0 ml of soh solution is neutralized by 38.2 ml of M Hr solution. What is the molarity of the soh solution? M M 1.36 M 10.2 M 38 What type of solution is formed when solid sodium hydroxide (NaOH) is dissolved in water? an electrolytic solution, because NaOH will dissociate into ions an electrolytic solution, because NaOH will not dissociate into ions a nonelectrolytic solution, because NaOH will dissociate into ions a nonelectrolytic solution, because NaOH will not dissociate into ions RELESE 18 Go to the next page.

20 HEMISTRY RELESE I TEMS 39 The diagram below shows the solubility of sugar in water. 500 Solubility Graph student dissolves 300 g of sugar in 100 g of water at 80. The solution is then allowed to cool to 40. The appearance of the solution does not change during the cooling. Which term accurately describes the solution at 40? Solubility (in g/100 g of water) suspension Sugar Temperature ( ) RELESE colloid supersaturated unsaturated 19 Go to the next page.

21 HEMISTRY RELESE I TEMS 40 Which statement explains what happens when potassium chloride (Kl) dissolves in water? Water molecules surround the potassium chloride but do not exert forces of attraction strong enough to break any bonds. Water molecules exert forces of attraction that break the potassium chloride apart into potassium ions and chloride ions. Water molecules exert forces of attraction that break the potassium chloride apart into neutral atoms of potassium and neutral atoms of chlorine. Water molecules exert forces of attraction that break the potassium chloride apart into potassium atoms and diatomic chlorine gas. RELESE 20 Go to the next page.

22 HEMISTRY RELESE I TEMS This is the end of hemistry Released Items. irections: 1. Look back over your answers for the test questions. 2. Make sure all your answers are entered on the answer sheet. Only what is entered on your answer sheet will be scored. 3. Put all of your papers inside your test book and close the test book. 4. Place your calculator on top of the test book. 5. Stay quietly in your seat until your teacher tells you that testing is finished. 6. Remember, teachers are not allowed to discuss items from the test with you, and you are not allowed to discuss with others any of the test questions or information contained within the test. RELESE 21

23 HEMISTRY RELESE ITEMS hemistry RELESE Items nswer Key Question Number Question Type orrect nswer Percent orrect 2 Objective 1 M 63% hm M 58% hm M 65% hm M 64% hm M 71% hm M 59% hm M 64% hm M 65% hm M 34% hm M 66% hm RELESE 11 M 66% hm M 72% hm M 61% hm M 84% hm M 36% hm M 73% hm

24 HEMISTRY RELESE ITEMS Question Number Question Type orrect nswer Percent orrect 2 Objective 17 M 65% hm M 62% hm M 72% hm M 59% hm M 90% hm M 70% hm M 55% hm M 71% hm M 38% hm M 79% hm M 40% hm M 76% hm RELESE 29 M 59% hm M 56% hm M 58% hm M 39% hm M 47% hm M 58% hm

25 HEMISTRY RELESE ITEMS Question Number Question Type orrect nswer Percent orrect 2 Objective 35 M 60% hm M 71% hm M 56% hm M 60% hm M 50% hm M 47% hm These released items were administered to students during a previous test administration. This sample set of released items may not reflect the breadth of the standards assessed and/or the range of item difficulty found on the N Final Exam. dditional information about the N Final Exam is available in the ssessment Specification for each exam located at 2 Percent correct is the percentage of students who answered the item correctly during a previous administration. RELESE 24

26 HEMISTRY RELESE ITEMS larifying Objectives escriptions Only clarifying objective descriptions addressed by the released items in this document are listed below. complete list of North arolina Essential Standards for Science may be reviewed at hm (Matter: Properties and hange) nalyze the structure of atoms, isotopes, and ions. hm (Matter: Properties and hange) nalyze an atom in terms of the location of electrons. hm (Matter: Properties and hange) Explain the emission of electromagnetic radiation in spectral form in terms of the ohr model. hm (Matter: Properties and hange) Explain the process of radioactive decay by the use of nuclear equations and half-life. hm (Matter: Properties and hange) ompare (qualitatively) the relative strengths of ionic, covalent, and metallic bonds. hm (Matter: Properties and hange) Infer the type of bond and chemical formula formed between atoms. hm (Matter: Properties and hange) ompare inter-and intra-particle forces. hm (Matter: Properties and hange) Interpret the name and formula of compounds using IUP convention. hm (Matter: Properties and hange) ompare the properties of ionic, covalent, metallic, and network compounds. hm (Matter: Properties and hange) lassify the components of a periodic table (period, group, metal, metalloid, nonmetal, transition). hm (Matter: Properties and hange) Infer the physical properties (atomic radius, metallic and nonmetallic characteristics) of an element based on its position on the Periodic Table. hm (Matter: Properties and hange) Infer the atomic size, reactivity, electronegativity, and ionization energy of an element from its position in the Periodic Table. hm (Energy: onservation and Transfer) Explain the energetic nature of phase changes. hm (Energy: onservation and Transfer) Interpret the data presented in phase diagrams. RELESE 25

27 HEMISTRY RELESE ITEMS hm (Energy: onservation and Transfer) Infer simple calorimetric calculations based on the concepts of heat lost equals heat gained and specific heat. hm (Energy: onservation and Transfer) Explain the relationships between pressure, temperature, volume, and quantity of gas both qualitative and quantitative. hm (Energy: onservation and Transfer) Understand the energy content of a chemical reaction. hm (Energy: onservation and Transfer) nalyze the evidence of chemical change. hm (Energy: onservation and Transfer) nalyze the law of conservation of matter and how it applies to various types of chemical equations (synthesis, decomposition, single replacement, double replacement, and combustion). hm (Energy: onservation and Transfer) nalyze the stoichiometric relationships inherent in a chemical reaction. hm (Energy: onservation and Transfer) nalyze quantitatively the composition of a substance (empirical formula, molecular formula, percent composition, and hydrates) hm (Interactions of Energy and Matter) Explain the factors that affect the rate of a reaction (temperature, concentration, particle size and presence of a catalyst). hm (Interactions of Energy and Matter) Explain the conditions of a system at equilibrium. hm (Interactions of Energy and Matter) Infer the shift in equilibrium when a stress is applied to a chemical system (Le hatelier s Principle). hm (Interactions of Energy and Matter) lassify substances using the hydronium and hydroxide ion concentrations. hm (Interactions of Energy and Matter) Summarize the properties of acids and bases. hm (Interactions of Energy and Matter) Infer the quantitative nature of a solution (molarity, dilution, and titration with a 1:1 molar ratio). hm (Interactions of Energy and Matter) Summarize the properties of solutions. RELESE 26

28 HEMISTRY RELESE ITEMS hm (Interactions of Energy and Matter) Interpret solubility diagrams. hm (Interactions of Energy and Matter) Explain the solution process. RELESE 27

RELEASED. NC Final Exam. Chemistry. Released Items. Student Name:

RELEASED. NC Final Exam. Chemistry. Released Items. Student Name: Released Items Student Name: hemistry 2016 2017 Public Schools of North arolina State oard of Education epartment of Public Instruction Raleigh, North arolina 27699-6314 RELESE N Final Exam opyright 2016