[PDF] 2016 AP Chemistry Practice Exam MCQ Multiple Choice Questions with Answers Advanced Placement.pdf

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Filename:	[PDF] 2016 AP Chemistry Practice Exam MCQ Multiple Choice Questions with Answers Advanced Placement.pdf
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Description:	Download file or read online AP past exam paper 2016 AP Chemistry Practice Exam MCQ Multiple Choice Questions with Answers and FRQ Free Response Questions with Scoring Guidelines - Collegeboard Advanced Placement.

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AP ® Chemistry Practice Exam From the 2 016 Administration NOTE: This is a modified version of the 2016 AP Chemistry Exam. This exam ma y no t be posted on school or persona l websites , no r electronically redistribute d fo r an y reason . Thi s Released Exa m is provided by th e Colleg e Boar d for AP Exam preparation . Teacher s ar e permitted to download th e material s an d mak e copies to use wit h thei r student s in a classroo m settin g onl y. To maintai n th e securit y of this exam , teacher s shoul d collec t all material s afte r thei r administratio n an d keep them in a secure location . Fu rther distribution o f thes e material s outsid e of the secur e Colleg e Board sit e disadvantages teachers wh o rel y on uncirculated questions fo r classroo m testing . An y additional distributio n is in violation of the Colleg e Board ’s copyrigh t policies and ma y resul t in the terminatio n of Practice Exam acces s fo r you r school as well as the removal of access to othe r onlin e service s suc h as the A P T eacher Communit y an d Onlin e Scor e Repo rts.

Contents Exam Instructions Student Answer Sheet for the Multiple -Choice Section Section I: Multiple -Choice Questions Section II: Free -Response Questions Multiple -Choice Answer Key Free- Response Scoring Guidelines Scoring Worksheet Question Descriptors and Performance Data Note: This publication shows the page numbers that appeared in the 201 5−16 AP Exam Instructions book and in th e actual exam. This publication was not repaginated to begin with page 1. © 2016 The College Board. College Board, Advanced Placement Program, AP, SAT and the acorn logo are registered trademarks of the College Board. All other products and services may be trademarks of their respective owners. Permission to use copyrighted College Board materials may be requested online at: www.collegeboard.com/inquiry/cbpermit.html.

Exam Instructions The following contains instructions taken from the 2015−16 AP Exam Instructions book.

43 CHEMISTRY What Proctors Need to Bring to This Exam • Exam packets • Ans wer sheets • AP Student Packs • 2015-16 AP Coordinator’s Manual • Thi s book — AP Exam Instructions • AP E xam Seating Chart template(s) • Sc hool Code and Home-School/Self- Study Codes • Ex tra calculators • Pen cil sharpener • Co ntainer for students’ electronic devices (if needed) • Ex tra No. 2 pencils with erasers • Ex tra pens with black or dark blue ink • Ex tra paper • S tapler • Wa t c h • Si gns for the door to the testing room – “ Exam in Progress” – “ Cell phones are prohibited in the testing room” AP® Chemistry Exam Regularly Scheduled Exam Date: Monday morning, May 2, 2016 Late-Testing Exam Date: Thursday afternoon, May 19, 2016 Section I Total Time: 1 hr. 30 min. Section II Total Time: 1 hr. 45 min. Section I Total Time: 1 hour 30 minutes Calculator not permitted Percent of Total Score: 50% Writing Instrument: Pencil required Number of Questions: 60* *The number of questions may vary slightly depending on the form of the exam. Section II Total Time: 1 hour 45 minutes Calculators allowed for all of Section II Percent of Total Score: 50% Writing Instrument: Either pencil or pen with black or dark blue ink Number of Questions: 7 (3 ten-point and 4 four-point questions; 105 minutes) Note: Tables of equations and constants are provided in the exam booklets for both sections of the exam. Students are not allowed to use calculators in Section I of the AP Chemistry Exam. However, st udents are permitted to use four-function, scientific, or graphing calculators to answer questions in Section II. Before starting the exam administration, make sure that each student has an appropriate calculator and that any student with a graphing calculator has a model from the approved list on page 47 of the 2015-16 AP Coordinator’s Manual . See pages 44–47 of the AP Coordinator’s Manual for more information. If a student does not have an appropriate calculator or has a graphing calculator not on the approved list, you may provide one from your supply. If the student does not want to use the calculator you provide, or does not want to use a calculator at all, he or she must hand copy, date, and sign the release statement on page 45 of the AP Coordinator’s Manual . ? 2016 The College Board. Visit the College Board on the Web: www.col\ legeboard.org.

44 Chemistry During the administration of Section II students may have no more than two calculators on their desks. Calculators may not be shared. Calculator memories do not need to be cleared before or after the exam. Students with Hewlett-Packard 48–50 Series and Casio FX-9860 graphing calculators may use cards designed for use with these calculators. Proctors should make sure infrared ports (Hewlett-Packard) are not facing each other. Since graphing calculators can be used to store data, including text, proctors should monitor that students are using their calculators appropriately. Attempts by students to use the calculator to remove exam questions and/or answers from the room may result in the cancellation of AP Exam scores. Students will be allowed to use the table of equations and constants on both sections of the exam. SECTION I: Multiple Choice ! Do not begin the exam instructions below until you have completed the appropriate General Instructions for your group. Make sure you begin the exam at the designated time. Remember, you must complete a seating chart for this exam. See pages 305–306 for a seating chart template and instructions. See the 2015-16 AP Coordinator’s Manual for exam seating requirements (pages 49–52). If you are giving the regularly scheduled exam, say: It is Monday morning, May 2, and you will be taking the AP Chemistry Exam. If you are giving the alternate exam for late testing, say: It is Thursday afternoon, May 19, and you will be taking the AP Chemistry Exam. In a moment, you will open the packet that contains your exam materials. By opening this packet, you agree to all of the AP Program’s policies and procedures outlined in the 2015-16 Bulletin for AP Students and Parents . You may now remove the shrinkwrap from your exam packet and take out the Section I booklet, but do not open the booklet or the shrinkwrapped Section II materials. Put the white seals aside. . . . Carefully remove the AP Exam label found near the top left of your exam booklet cover. Now place it on page 1 of your answer sheet on the light blue box near the top right-hand corner that reads “AP Exam Label.” If students accidentally place the exam label in the space for the number label or vice versa, advise them to leave the labels in place. They should not try to remove the label; their exam can still be processed correctly. Read the statements on the front cover of Section I and look up when you have finished. . . . Sign your name and write today’s date. Look up when you have finished. . . . Now print your full legal name where indicated. Are there any questions? . . . Turn to the back cover of your exam booklet and read it completely. Look up when you have finished. . . . ? 2016 The College Board. Visit the College Board on the Web: www.col\ legeboard.org.

45 AP Exam Instructions CHEMISTRY Are there any questions? . . . You will now take the multiple-choice portion of the exam. You should have in front of you the multiple-choice booklet and your answer sheet. Open your answer sheet to page 2. You may never discuss these specific multiple-choice questions at any time in any form with anyone, including your teacher and other students. If you disclose these questions through any means, your AP Exam score will be canceled. The answer sheet has circles A–E for each question. For Chemistry, you will use only the circles marked A–D. You must complete the answer sheet using a No. 2 pencil only. Mark all of your responses beginning on page 2 of your answer sheet, one response per question. Completely fill in the circles. If you need to erase, do so carefully and completely. No credit will be given for anything written in the exam booklet. Scratch paper is not allowed, but you may use the margins or any blank space in the exam booklet for scratch work. Calculators are not allowed for this section. Please put your calculators under your chair. Are there any questions? . . . You have 1 hour and 30 minutes for this section. Open your Section I booklet and begin. 126 3 9 Note Start Time here . Note Stop Time here . Check that students are marking their answers in pencil on their answer sheets and that they are not looking at their shrinkwrapped Section II booklets. After 1 hour and 20 minutes, say: There are 10 minutes remaining. After 10 minutes, say: Stop working. Close your booklet and put your answer sheet on your desk, face up. Make sure you have your AP number label and an AP Exam label on page 1 of your answer sheet. Sit quietly while I collect your answer sheets. Collect an answer sheet from each student. Check that each answer sheet has an AP number label and an AP Exam label. After all answer sheets have been collected, say: Now you must seal your exam booklet using the white seals you set aside earlier. Remove the white seals from the backing and press one on each area of your exam booklet cover marked “PLACE SEAL HERE.” Fold each seal over the back cover. When you have finished, place the booklet on your desk, face up. I will now collect your Section I booklet. . . . Collect a Section I booklet from each student. Check that each student has signed the front cover of the sealed Section I booklet. There is a 10-minute break between Sections I and II. When all Section I materials have been collected and accounted for and you are ready for the break, say: Please listen carefully to these instructions before we take a 10-minute break. All items you placed under your chair at the beginning of this exam must stay there, and you are not permitted to open or access them in any way. Leave your shrinkwrapped Section II packet on top of your desk during the break. You are not allowed to consult teachers, other students, notes, or textbooks during the break. You may not make phone calls, send text ? 2016 The College Board. Visit the College Board on the Web: www.col\ legeboard.org.

46 Chemistry messages, check email, use a social networking site, or access any electronic or communication device. Remember, you may never discuss the multiple- choice questions at any time in any form with anyone, including your teacher and other students. If you disclose these questions through any means, your AP Exam score will be canceled. Are there any questions? . . . 126 3 9 You may begin your break. Testing will resume at . SECTION II: Free Response After the break, say: May I have everyone’s attention? Place your Student Pack on your desk. . . . You may now remove the shrinkwrap from the Section II packet, but do not open the exam booklet until you are told to do so. . . . Read the bulleted statements on the front cover of the exam booklet. Look up when you have finished. . . . Now take an AP number label from your Student Pack and place it on the shaded box. If you don’t have any AP number labels, write your AP number in the box. Look up when you have finished. . . . Read the last statement. . . . Using a pen with black or dark blue ink, print the first, middle, and last initials of your legal name in the boxes and print today’s date where indicated. This constitutes your signature and your agreement to the statements on the front cover. . . . Turn to the back cover and, using your pen, complete Item 1 under “Important Identification Information.” Print the first two letters of your last name and the first letter of your first name in the boxes. Look up when you have finished. . . . In Item 2, print your date of birth in the boxes. . . . In Item 3, write the school code you printed on the front of your Student Pack in the boxes. . . . Read Item 4. . . . Are there any questions? . . . I need to collect the Student Pack from anyone who will be taking another AP Exam. You may keep it only if you are not taking any other AP Exams this year. If you have no other AP Exams to take, place your Student Pack under your chair now. . . . Read the information on the back cover of the exam booklet. Do not open the exam booklet until you are told to do so. Look up when you have finished. . . . ? 2016 The College Board. Visit the College Board on the Web: www.col\ legeboard.org.

47 AP Exam Instructions CHEMISTRY Collect the Student Packs. Then say: Are there any questions? . . . Calculators may be used for Section II. You may get your calculators from under your chair and place them on your desk. . . . You have 1 hour and 45 minutes to complete Section II. You are responsible for pacing yourself, and you may proceed freely from one question to the next. You must write your answers in the exam booklet using a pen with black or dark blue ink or a No. 2 pencil. If you use a pencil, be sure that your writing is dark enough to be easily read. If you need more paper during the exam, raise your hand. At the top of each extra sheet of paper you use, be sure to write only your AP number and the question number you are working on. Do not write your name. Are there any questions? . . . You may begin. 126 3 9 Note Start Time here . Note Stop Time here . Proctors should also make sure that Hewlett-Packard calculators’ infrared ports are not facing each other and that students are not sharing calculators. After 1 hour and 35 minutes, say: There are 10 minutes remaining. After 10 minutes, say: Stop working and close your exam booklet. Place it on your desk, face up. . . . If any students used extra paper for a question in the free-response section, have those students staple the extra sheet(s) to the first page corresponding to that question in their exam booklets. Complete an Incident Report. A single Incident Report may be completed for multiple students per exam subject per administration (regular or late testing) as long as all of the required information is provided. Include all exam booklets with extra sheets of paper in an Incident Report return envelope (see page 60 of the 2015-16 AP Coordinator’s Manual for complete details). Then say: Remain in your seat, without talking, while the exam materials are collected. . . . Collect a Section II booklet from each student. Check for the following: • Exam booklet front cover: The student placed an AP number label on the shaded box and printed his or her initials and today’s date. • E xam booklet back cover: The student completed the “Important Identification Information” area. When all exam materials have been collected and accounted for, return to students any electronic devices you may have collected before the start of the exam. ? 2016 The College Board. Visit the College Board on the Web: www.col\ legeboard.org.

48 Chemistry If you are giving the regularly scheduled exam, say: You may not discuss or share these specific free-response questions with anyone unless they are released on the College Board website in about two days. Your AP Exam score results will be available online in July. If you are giving the alternate exam for late testing, say: None of the questions in this exam may ever be discussed or shared in any way at any time. Your AP Exam score results will be available online in July. If any students completed the AP number card at the beginning of this exam, say: Please remember to take your AP number card with you. You will need the information on this card to view your scores and order AP score reporting services online. Then say: You are now dismissed. All exam materials must be placed in secure storage until they are returned to the AP Program after your school’s last administration. Before storing materials, check the “School Use Only” section on page 1 of the answer sheet and: • Fill in the appropriate section number circle in order to access a separate AP Instructional Planning Report (for regularly scheduled exams only) or subject score roster at the class section or teacher level. See “Post-Exam Activities” in the 2015-16 AP Coordinator’s Manual . • C heck your list of students who are eligible for fee reductions and fill in the appropriate circle on their registration answer sheets. Be sure to give the completed seating chart to the AP Coordinator. Schools must retain seating charts for at least six months (unless the state or district requires that they be retained for a longer period of time). Schools should not return any seating charts in their exam shipments unless they are required as part of an Incident Report. ? 2016 The College Board. Visit the College Board on the Web: www.col\ legeboard.org.

Student Answer Sheet for the Multiple -Choice Section Use this section to capture student responses. (Note that the following answer sheet is a sample, and may differ from one used in an actual exam. )

Sign your legal name as it will appear on your college applications. Date To maintain the security of the exam and the validity of my AP score, I w\ ill allow no one else to see the multiple-choice questions. I will seal the multiple-choice booklet when asked to do so, and I will not dis\ cuss these questions with anyone at any time after completing the section. I am aware of and agree to the AP Program’s policies and procedures as outlined in the 2015-16 Bulletin for AP Students and Parents, including using testing accommodations (e.g., extended time, computer\ , etc.) only if I have been preapproved by College Board Services for Students with Disabilities.COMPLETE THIS AREA AT EVERY EXAM.USE NO. 2 PENCIL ONLY A. SIGNATURE PAGE 1 AP Exam Label (from Section I Booklet) AP Number Label (from Student Pack) Answer Sheet 2 016 B. LEGAL NAME Omit apostrophes, Jr., II. Legal First Name ? First 12 Letters Legal Last Name ? First 15 Letters MI A A A A A A A A A A A A A A A B B B B B B B B B B B B B B B C C C C C C C C C C C C C C C D D D D D D D D D D D D D D D E E E E E E E E E E E E E E E F F F F F F F F F F F F F F F G G G G G G G G G G G G G G G H H H H H H H H H H H H H H H I I I I I I I I I I I I I I I J J J J J J J J J J J J J J J K K K K K K K K K K K K K K K L L L L L L L L L L L L L L L M M M M M M M M M M M M M M M N N N N N N N N N N N N N N N O O O O O O O O O O O O O O O P P P P P P P P P P P P P P P Q Q Q Q Q Q Q Q Q Q Q Q Q Q Q R R R R R R R R R R R R R R R S S S S S S S S S S S S S S S T T T T T T T T T T T T T T T U U U U U U U U U U U U U U U V V V V V V V V V V V V V V V W W W W W W W W W W W W W W W X X X X X X X X X X X X X X X Y Y Y Y Y Y Y Y Y Y Y Y Y Y Y Z Z Z Z Z Z Z Z Z Z Z Z Z Z Z – – – – – – – – – – – – – 1 2 3 4 5 6 7 8 9 A A A A A A A A A A A A A B B B B B B B B B B B B B C C C C C C C C C C C C C D D D D D D D D D D D D D E E E E E E E E E E E E E F F F F F F F F F F F F F G G G G G G G G G G G G G H H H H H H H H H H H H H I I I I I I I I I I I I I J J J J J J J J J J J J J K K K K K K K K K K K K K L L L L L L L L L L L L L M M M M M M M M M M M M M N N N N N N N N N N N N N O O O O O O O O O O O O O P P P P P P P P P P P P P Q Q Q Q Q Q Q Q Q Q Q Q Q R R R R R R R R R R R R R S S S S S S S S S S S S S T T T T T T T T T T T T T U U U U U U U U U U U U U V V V V V V V V V V V V V W W W W W W W W W W W W W X X X X X X X X X X X X X Y Y Y Y Y Y Y Y Y Y Y Y Y Z Z Z Z Z Z Z Z Z Z Z Z Z – – – – – – – – – – 0 0 0 0 0 0 0 0 1 1 1 1 1 1 1 1 2 2 2 2 2 2 2 2 3 3 3 3 3 3 3 3 4 4 4 4 4 4 4 4 5 5 5 5 5 5 5 5 6 6 6 6 6 6 6 6 7 7 7 7 7 7 7 7 8 8 8 8 8 8 8 8 9 9 9 9 9 9 9 9 0 0 1 1 2 2 3 3 4 5 6 7 8 9 6 12 7 1 8 2 9 3 10 4 11 5 0 0 0 0 0 0 0 0 0 0 1 1 1 1 1 1 1 1 1 1 2 2 2 2 2 2 2 2 2 2 3 3 3 3 3 3 3 3 3 3 4 4 4 4 4 4 4 4 4 4 5 5 5 5 5 5 5 5 5 5 6 6 6 6 6 6 6 6 6 6 7 7 7 7 7 7 7 7 7 7 8 8 8 8 8 8 8 8 8 8 9 9 9 9 9 9 9 9 9 9 S D. EXAM DATE C. YOUR AP NUMBER Month AM PM F. MULTIPLE-CHOICE BOOKLET SERIAL NUMBER H. AP EXAM I AM TAKING USING THIS ANSWER SHEET Exam Name: Form Code: Form: COMPLETE THIS AREA ONLY ONCE. SCHOOL USE ONLY Fee Reduction Granted Section Number Option 1 Option 2 E. EXAM START TIME 0 0 1 1 2 3 4 5 6 7 8 9 1 2 0 0 0 1 1 1 2 2 2 3 3 3 4 4 4 5 5 5 6 6 6 7 7 7 8 8 8 9 9 9 G. ONLINE PROVIDER CODE Day O. STUDENT SEARCH SERVICE ® Colleges and scholarship programs may request your information to inform you of educational opportunities and financial aid. Would you like us to supply your information? If you don’t answer and previously chose to participate in this service, we will continue providing your information. Yes No 0 0 0 0 0 0 0 0 0 1 1 1 1 1 1 1 1 1 2 2 2 2 2 2 2 2 2 3 3 3 3 3 3 3 3 3 4 4 4 4 4 4 4 4 4 5 5 5 5 5 5 5 5 5 6 6 6 6 6 6 6 6 6 7 7 7 7 7 7 7 7 7 8 8 8 8 8 8 8 8 8 9 9 9 9 9 9 9 9 9 L. SOCIAL SECURITY NUMBER (Optional) 108603-00657 • TF216E4757.5 • Printed in U.S.A. Q4068/1- 4 COLLEGE CODE 0 0 0 0 1 1 1 1 2 2 2 2 3 3 3 3 4 4 4 4 5 5 5 5 6 6 6 6 7 7 7 7 8 8 8 8 9 9 9 9 M. COLLEGE TO RECEIVE YOUR AP SCORE REPORT College Name State Country Using the college code listed in the AP Student Pack, indicate the ONE college that you want to receive your AP score report. City SCHOOL CODE 0 0 0 0 0 0 1 1 1 1 1 1 2 2 2 2 2 2 3 3 3 3 3 3 4 4 4 4 4 4 5 5 5 5 5 5 6 6 6 6 6 6 7 7 7 7 7 7 8 8 8 8 8 8 9 9 9 9 9 9 School Name State Country J. SCHOOL YOU ATTEND City 0 0 0 0 0 0 0 0 0 0 1 1 1 1 1 1 1 1 1 1 2 2 2 2 2 2 2 2 2 2 3 3 3 3 3 3 3 3 3 3 4 4 4 4 4 4 4 4 4 4 5 5 5 5 5 5 5 5 5 5 6 6 6 6 6 6 6 6 6 6 7 7 7 7 7 7 7 7 7 7 8 8 8 8 8 8 8 8 8 8 9 9 9 9 9 9 9 9 9 9 INTERNATIONAL PHONE I. AREA CODE AND PHONE NUMBER 0 0 0 0 1 1 1 1 2 2 2 2 3 3 3 3 4 4 4 5 5 5 6 6 6 7 7 7 8 8 8 9 9 9 Jan Feb Mar Apr May Jun Jul Aug Sep Oct Nov Dec Month DayYear K. DATE OF BIRTH N. CURRENT GRADE LEVEL Not yet in 9th grade 9th 10th B123456789T 785208 11th 12th No longer in high school

Q. LANGUAGE — Do not complete this section unless instructed to do so. 1 2 34 5 67 8 9 A B C D E F G H I A B C D E F G H I A B C D E F G H I A B C D E F G H I A B C D E F G H I A B C D E F G H I A B C D E F G H I A B C D E F G H I A B C D E F G H I If this answer sheet is for the French Language and Culture, German Language and Culture, Italian Language and Culture, Spanish Language and Culture, or Spanish Literature and Culture Exam, please answer the following questions. Your responses will not affect your score. 1. Have you lived or studied for one month or more in a country where the language of the exam you are now taking is spoken? Yes No DO NOT WRITE IN THIS AREA P. SURVEY QUESTIONS — Answer the survey questions in the AP Student Pack. Do not put responses to exam questions in this section. PAGE 2 COMPLETE THIS AREA AT EACH EXAM (IF APPLICABLE). Indicate your answers to the exam questions in this section (pages 2 and 3). Mark only one response per question for Questions 1 through 120. If a question has only four answer options, do not mark option E. Answers written in the multiple-choice booklet will not be scored. A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 5051 52 53 54 55 56 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 72 73 74 75 QUESTIONS 1–75 Yes No 2. Do you regularly speak or hear the language at home? A B C D A B C D You must use a No. 2 pencil and marks must be complete. Do not use a mechanical pencil. It is very important that you fill in the entire circle darkly and completely. If you change your response, erase as completely as possible. Incomplete marks or erasures may affect your score. COMPLETE MARK EXAMPLES OF INCOMPLETE MARKS SELECTED MEDIA EXAMS R W O OTHER EXAMS R W O PT02 TOTAL PT03 Subscore (if applicable) PT04 Subscore (if applicable) ETS USE ONLY Exam Exam 0 1 2 3 4 5 6 7 8 9 0 1 2 3 4 5 6 7 8 9 0 1 2 3 4 5 6 7 8 9 0 1 2 3 4 5 6 7 8 9

/ / / – . . . . . 0 0 0 0 1 1 1 1 1 2 2 2 2 2 3 3 3 3 3 4 4 4 4 4 5 5 5 5 5 6 6 6 6 6 7 7 7 7 7 8 8 8 8 8 9 9 9 9 9 / / / – . . . . . 0 0 0 0 1 1 1 1 1 2 2 2 2 2 3 3 3 3 3 4 4 4 4 4 5 5 5 5 5 6 6 6 6 6 7 7 7 7 7 8 8 8 8 8 9 9 9 9 9 / / / – . . . . . 0 0 0 0 1 1 1 1 1 2 2 2 2 2 3 3 3 3 3 4 4 4 4 4 5 5 5 5 5 6 6 6 6 6 7 7 7 7 7 8 8 8 8 8 9 9 9 9 9 / / / – . . . . . 0 0 0 0 1 1 1 1 1 2 2 2 2 2 3 3 3 3 3 4 4 4 4 4 5 5 5 5 5 6 6 6 6 6 7 7 7 7 7 8 8 8 8 8 9 9 9 9 9 / / / – . . . . . 0 0 0 0 1 1 1 1 1 2 2 2 2 2 3 3 3 3 3 4 4 4 4 4 5 5 5 5 5 6 6 6 6 6 7 7 7 7 7 8 8 8 8 8 9 9 9 9 9 For Students Taking AP Biology / / / – . . . . . 0 0 0 0 1 1 1 1 1 2 2 2 2 2 3 3 3 3 3 4 4 4 4 4 5 5 5 5 5 6 6 6 6 6 7 7 7 7 7 8 8 8 8 8 9 9 9 9 9 121123 122 124125 126 Write your answer in the boxes at the top of the griddable area and fill in the corresponding circles. Mark only one circle in any column. You will receive credit only if the circles are filled in correctly. PAGE 3 DO NOT WRITE IN THIS AREA A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E A B C D E 76 77 78 79 80 81 82 83 84 85 86 87 88 89 90 91 92 93 94 95 96 97 98 99 10 0 101 10 2 10 3 10 4 10 5 10 6 10 7 10 8 10 9 110111 11 2 11 3 11 4 11 5 11 6 11 7 11 8 11 9 120 Be sure each mark is dark and completely fills the circle. If a question has only four answer options, do not mark option E. QUESTIONS 76–120 © 2015 The College Board. College Board, AP, Student Search Service and the acorn logo are registered trademarks of the College Board. QUESTIONS 121–126 A B C D A B C D A B C D A B C D A B C D A B C D A B C D A B C D A B C D A B C D A B C D A B C D 131 132 133 134 135 136 137 138139 140 141 142 For Students Taking AP Physics 1 or AP Physics 2 Mark two responses per question. You will receive credit only if both correct responses are selected. QUESTIONS 131–142

COMPLETE THIS AREA ONLY ONCE. 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Section I: Multiple -Choice Questions This is the multiple-choice section of the 2016 AP exam. It includes cover material and other administrative instructions to help familiarize students with the mechanics of the exam. (Note that future exams may differ in look from the following content.) For purposes of test security and/or statistical analysis, some questions have been removed from the version of the exam that was administered in 2016 . Therefore, the timing indicated here may not be appropriate for a practice exam.

AP ® Chemistry Exam SECTION I: Multiple Choice 2016 DO NOT OPEN THIS BOOKLET UNTIL YOU ARE TOLD TO DO SO. At a Glance Total Time1 hour, 30 minutes Number of Questions 50 Percent of Total Score 50% Writing InstrumentPencil required Electronic DeviceNone allowed Instructions Section I of this exam contains 50 multiple-choice questions. Fill in only the circles for numbers 1 through 50 on your answer sheet. Pages containing a periodic table and lists containing equations and constants are also printed in this booklet. Indicate all of your answers to the multiple- choice questions on the answer sheet. No credit will be given for anything written in this exam booklet, but you may use the booklet for notes or scratch work. After you have decided which of the suggested answers is best, completely fill in the corresponding circle on the answer sheet. Because this section offers only four answer options for each question , do not mark the ( E ) answer circle for any question. Give only one answer to each question. If you change an answer, be sure that the previous mark is erased completely. Here is a sample question and answer. Use your time effectively, working as quickly as you can without losing accuracy. Do not spend too much time on any one question. Go on to other questions and come back to the ones you have not answered if you have time. It is not expected that everyone will know the answers to all of the multiple- choice questions. Your total score on Section I is based only on the number of questions answered correctly . Points are not deducted for incorrect answers or unanswered questions. Form I Form Code 4MBP4-S 25

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L, mL = liter(s), milliliter(s) mm Hg = millimeters of mercury g = gram(s) E = h c =   = frequency Planck’s constant, h = 6.626  10 34 Js Speed of light, c = 2.998  10 8 ms 1 Avogadro’s number = 6.022  10 23 mol  1 Electron charge, e = 1.602 × 10 19 coulomb K c = [C] [D] [A] [B] c d a b , where a A + b B  c C + d D K p = C D A B () ( ) () ( ) c d a b P P P P K a = [H ][A ] [HA] + - K b = [OH ][HB ] [B] - + K w = [H +][OH ] = 1.0  10 14 at 25 C = K a  K b 灈‽⁰ K a + log [A ] [HA] - Kc (molar concentrations) K w (water) ln[A]t  ln[A] 0 =  kt [] [] 0 A A 1 1 t - = kt t ½ = 0.693 k t ½ = half-life AP ® CHEMISTRY EQUATION S AND CONSTANTS Throughout the exam the following symbols have th e definitions specified unless otherwise noted. J, kJ = joule(s), kilojoule(s) nm = nanometer(s) V = volt(s) atm = atmosphere(s) mol = mole(s) ATOMIC STRUCTURE E = energy  = wavelength EQUILIBRIUM pH = log [H +] , pOH = log [OH ] 14 = pH + pOH p K a = log K a , pK b = log K b Equilibrium Constants K p (gas pressures) K a (weak acid) K b (weak base) KINETICS k = rate constant t = time -3-

1 atm = 760 mm Hg = 760 torr PV = nRT 浯汥猠䄠 PA = P total  X A, where X A = total moles = P A + P B + P C + . . . P total m n = M K = C + 273 D = m V 1 2 KE per molecule = mv 2 A = abc M = molar mass KE = kinetic energy A = absorbance R = 8.314 J mol 1K1 = 62.36 L torr mol 1K1   S = Â S products - Â S reactants   H = Â D H f products - Â DH f reactants   G = Â D G f products - Â DG reactants f G  = H  TS  = RT ln K =  nF E  q I = t S  = standard entropy H  = standard enthalpy G  = standard Gibbs free ener gy E  = standard reduction potential F = 96,485 coulombs per mole of electrons Faraday’s constant, ㄠ橯畬e ㄠ癯汴 㴠 ㄠ捯畬潭戠 GASES, LIQUIDS, AND SOLUTIONS Molarity, M = moles of solute per liter of solution THERMODYNAMICS / ELECTROCHEMISTRY q = mcT P = pressure V = volume T = temperature n = number of moles m = mass D = density v = velocity a = molar absorptivity b = path length c = concentratio n Gas constant, = 0.08206 L atm mol 1K1 STP = 273.15 K and 1.0 atm Ideal gas at STP = 22.4 L mol −1 q = heat m = mass c = specific heat capacity T = temperature n = number of moles I = current (amperes) q = charge (coulombs) t = time (seconds) -4-

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -5- C HEMISTRY Section I 50 Questions Time—90 minutes CALC ULATORS ARE NOT ALLOWED FOR SECTION I. Note: For all questions, assume that the temperature is 298 K, the pressure is 1.0 atm, and solutions are aqueous unless otherwise specified. Directions: Each of the questions or incomplete statements below is followed by four su ggested answers or completions. Select the one that is best in each case and then fill in the corresponding circle on the answer sheet. 1. In which of the following liquids do the intermolecular forces include dipole-dipo le forces? (A) F 2(l) (B)CH 4(l) (C) CF 4(l) (D) CH 2F2(l) 2. Which of the following best helps explain why an increas e in temperature increases the rate of a chemic al reac tion? (A) At higher temperatures, reactions have a lower activati on energy. (B) At higher temperatures, reactions have a higher activation energy. (C) At higher temperatures, every collision results in the formation of product. (D) At higher temperatures, high-energy collisions happen more frequently. 3. A sample of a hard, solid binary compou nd at room temperature did n o t conduct electricity as a pure solid but became highly conducti ve when dissolved in water. Which of the follow ing types of interactions is most likel y found betw een the particles in the substance? (A) Ionic bon ds (B) Metallic bonds (C) Covalent bon ds (D) Hydrogen b o nds N2(g) + 3 H 2(g )   2 NH 3(g ) H < 0 4.NH 3(g) was synthesized at 200 C in the presence of a powdered Os( s) catalyst, leading to the equilibrium system repres ented above. Which of the following changes would result in more NH 3(g ) in the mixture after equilibrium is reestablished ? (A) Replacing the powdered Os(s) with a solid cube of Os( s) of the same total mass (B) Increasing the temperature of the system to 250°C at constant pressure (C) Removing some H2(g) (D) Adding some N2(g ) 5. Which of the following arra nges the molecules N2, O2, and F2 in order of their bond en thalpies, from least to greatest? (A) F 2 < O 2 < N 2 (B) O 2 < N 2 < F 2 (C)N 2 < O 2 < F 2 (D) N 2 < F 2 < O 2

Ion Ionic Radius (pm) Li+ 60 Na + 95 Ca 2+ 99 In 3+ 81 6. Based on Coulomb’s law and the information in the table above, which of the following cations is most likely to have the weakest interaction with an adjacent water molecule in an aqueous solution? (A) Li + (B)Na + (C) Ca 2+ (D)In 3+ Element Electronegativity H 2.1 C 2.5 S 2.5 F 4.0 Cl 3.0 Si 1.8 7. On the basis of the information above, which of the following arranges the binary compounds in order of increasing bond polarity? (A) CH 4 < SiCl 4 < SF 4 (B)CH 4 < SF 4 < SiCl 4 (C) SF 4 < CH 4 < SiCl 4 (D)SiCl 4 < SF 4 < CH 4 Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -6-

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -7- X( g)  X +(g) + e  IE 1 = 740 kJ/mol X +(g )  X 2+(g) + e  IE 2 = 1450 kJ/mol X 2+(g )  X 3+(g) + e  IE 3 = 7730 kJ/mol 8. For element X represented above, which of the following is the most likely explanation fo r the large difference between the second and third ionization energies? (A) The effective nuclear charge decreases with successive ionizations. (B) The shielding of outer electrons increases with successive ionizations. (C) The electron removed during the third i onization is, on average, much closer to the nucleus than the first two electrons removed were. (D) The ionic radius increases with successive ionizations.

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -8- 9. A student performs an acid-base titration and plots the experimental results in the graph above. Which of the following statements best explains the experimental findings? (A) A strong acid was titrated with a strong base, as evidenced by the equivalence point at pH = 7 . (B) A strong acid was titrated with a strong base, as evidenced by the equivalence point at pH > 7. (C) A weak acid was titrated with a strong base, as evidenced by the equivalence point at pH > 7. (D) A weak acid was titrated with a weak base, as evid enced by the equivalence point at pH approximately 7.

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -9- 10. Two samples of Mg( s) of equal mass were placed in equal amounts of HCl(aq) contained in two separate reaction vessels. Particle representations of the mixing of Mg( s) and HCl(aq) in the two reaction vessels are shown in Figure 1 and Figure 2 above . Water molecules are not included in the particle representations. Which of the reactions will initially proceed faster, and why? (A) The reaction in Figure 1, because the atoms of Mg are more concentrated than those in Figure 2 (B) The reaction in Figure 1, because the Mg( s) in Figure 1 has a larger mass than the Mg( s) in Figure 2 (C) The reaction in Figure 2, because more Mg atoms are exposed to HCl(aq) in Figure 2 than in Figure 1 (D) The reaction in Figure 2, because the Mg( s) in Figure 2 has less surface area than the Mg( s) in Figure 1

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -10- 11. A 23.0 g sample of a compound contains 12.0 g of C, 3.0 g of H, and 8.0 g of O. Which of the following is the empirical formula of the compound? (A) CH 3O (B) C 2H6O (C) C 3H9O2 (D) C 4H12O2 Compound K sp PbCl 2 1.2 × 10 5 CuCl 1.6 × 10 7 AgCl 1.8 × 10 10 Hg 2Cl 2 1.4 × 10 18 12. Based on the Ksp values in the table above, a saturated solution of which of the following compounds has the highest [Cl ]  ? (A) PbCl 2 (B) CuCl (C)AgCl (D)Hg 2Cl 2 13. The distribution of speeds of H2(g) molecules at 273 K and 1 atm is shown in the diagram above. Which of the following best shows the speed distribution of He( g) atoms under the same conditions of temperature and pressure? (A) (B) (C) (D)

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -11- Questions 14-15 refer to the following information. 2 H 2O2(aq)  2 H 2O(l) + O 2(g ) E° = 0.55 V The equation and standard cell potential for the decomposition of H2O2(aq) in acidic solution at 25°C is given above. The reduction half-reactions for the process are listed below. O 2(g ) + 2 H +(aq) + 2 e   H 2O2(aq) O2(g) + 4 H +(aq) + 4 e   2 H 2O( l) E = 1.23 V O2(g ) + 2 H +(aq) + 2 e   H 2O2(aq) E = ? 14. What is the standard reduction potential for the half-reaction represented above? (A) 1.78 V (B) 0.68 V (C) +0.68 V (D) +1.78 V 15. Which of the following is true for the decomposition of H2O2(aq) ? (A) DG° > 0 and Keq > 1 (B) DG° > 0 and Keq < 1 (C) DG° < 0 and Keq > 1 (D) DG° < 0 and Keq < 1

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -12- C2H4(g ) + H 2(g)  C 2H6(g) 16. Which of the following will most likely increase the rate of the reaction represented above? (A) Decreasing the temperature of the reaction system (B) Adding a heterogeneous catalyst to the reaction system (C) Increasing the volume of the reaction vessel using a piston (D) Removing some H2(g ) from the reaction system 17. Which of the following molecules is least soluble in water? (A) (B) (C) (D) 18. At room temperature I2(s ) is a molecular solid. Which of the following provides a characteristic of I2(s ) with a correct explanation? (A) It has a high melting point because it has weak intermolecular forces. (B) It is hard because it forms a three- dimensional covalent network. (C) It is not a good conductor of electricity because its valence electrons are localized in bonding and nonbonding pairs. (D) It is very soluble in water because its molecules are polar. Molar Mass (g/mol) Boiling Point (C) CS 2(l ) 76 46.5 CCl 4(l ) 154 76.7 19. Based on the information in the table above, which liquid, CS 2(l) or CCl 4(l), has the higher equilibrium vapor pressure at 25 C, and why? (A) CS 2(l), because it has stronger London dispersion forces (B) CS 2(l), because it has weaker London dispersion forces (C) CCl 4(l), because it has stronger London dispersion forces (D) CCl 4(l), because it has weaker London dispersion forces

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -13- HX( aq) + Y (aq)   HY( aq) + X (aq) K eq > 1 20. Based on the information given above, which of the following is the strongest acid? (A) HX(aq) (B) Y (aq) (C) HY(aq) (D) X (aq) AgNO 3(aq) + NaCl( aq)  AgCl( s) + NaNO 3(aq ) 21. A student performed an analysis to determine the amount of AgNO 3(aq) in a solution. Excess NaCl( aq) was added to the solution, and the Ag +(aq) precipitated as AgCl(s ). The precipitate was collected by gravity filtration and dried in an oven. Three trials were performed, and in each case, according to the instructor, the mass of precipitate recovered was 5 percent higher than the actual mass of AgCl(s ) that should have formed. Which of the following could account for the error? (A) The pores in the filter paper were too large. (B) Not all of the precipitate was transferred to the filter paper. (C) The NaCl( aq) solution was too concentrated. (D) The precipitate was not rinsed with deionized water before drying.

Questions 22-25 refer to the following information. Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -14- NaOH(aq) + HCl(aq)  NaCl(aq) + H 2O(l) To determine the concentration of a NaOH(aq) solution, a student titrated a 50. mL sample with 0.10 M HCl(aq). The reaction is represented by the equation above. The titration is monitored using a pH meter, and the experimental results are plotted in the graph below. 22. At the point labeled R on the pH curve, which of the following ions are present in the reaction mixture at a concentration greater than 0.01 M ? (A) Na + and Cl  only (B) Na +, Cl , and H+ only (C) Na +, Cl , and OH  only (D) Na +, Cl , H+, and OH  23. One student titrated the NaOH( aq) with 1.0 M HCl(aq ) instead of 0.10 M HCl( aq). How would the student’s titration curve differ from the original curve? (A) The initial pH would be 11 instead of 13. (B) The pH at the equivalence point would be 5 instead of 7. (C) The pH far beyond the equivalence point would be higher than in the original curve. (D) The pH far beyond the equivalence point would be lower than in the original curve.

Trial Volume of 0.10 M HCl Volume of 0.10 M NaOH Amount of Heat Released 1 50. mL 50. mL X 2 100. mL 50. mL Y 24. A student conducted an experiment to determine rxnH D  for the reaction between HCl( aq) and NaOH( aq). The student ran two trials using the volumes of HCl( aq) and NaOH( aq) indicated in the table above, and determined the amount of heat released. Which of the following best explains the relationship between X and Y? (A) Y = 2X , because the volume of HCl(aq) used in trial 2 is twice the volume used in trial 1. (B) Y = X , because the number of moles of acid and base reacting with each other is the same in both trials. (C) 2X Y = 3 , because the heat is distributed over more particles in trial 2 than in trial 1. (D) The relationship between X and Y cannot be predicted. 25. A student mixes a 10.0 mL sample of 1.0 M NaOH(aq) with a 10.0 mL sample of 1.0 M HCl( aq) in a polystyrene container. The temperature of the solutions before mixing was 20.0°C. If the final temperature of the mixture is 26.0°C, what is the experimental value of rxnH D  ? (Assume that the solution mixture has a specific heat of 4.2 J/(g K) and a density of 1.0 g/mL.) (A) 50. kJ/mol rxn (B) 25 kJ/mol rxn (C) 5.0 × 10 4 kJ/mol rxn (D) 5.0 × 10 2 kJ/mol rxn Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -15-

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -16- 2 NO 2(g ) + F 2(g)  2 NO 2F(g) 26. The rate law for the reaction represented by the equation abov e is rate = k [NO 2][F 2]. Which of the following could be the first elementary step of a two-step mechanism for the reaction if the first step is slow and the second step is fast? (A) F 2(g)   F( g) (B) NO 2(g) + F 2(g)  NO 2F(g) + F( g) (C) NO 2(g) + F( g)  NO 2F(g) (D) 2 NO 2(g) + F 2(g)  2 NO 2F(g) 27. Which of the following Lewis electron-dot diagrams represents the molecule that contains the smallest bond angle? (A) (B) (C) (D)

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -17- Ethyl Acetate Butyl Acetate 28. A mixture containing equal numbers of moles of ethyl acetat e and butyl acetate was separated using distilla tion. Based on the diagrams shown above, which of the follow ing identifies the substance that would be initially present in higher concentration in the distillate and correctly explains why that occurs? (A) Ethyl acetate, because it has fewer C C bonds to break (B) Ethyl acetate, because it has a shorter carbon chain and weaker London dispersion forces (C) Butyl acetate, because it has more C C bonds to break (D) Butyl acetate, because it has a longer carbon chain and weaker dipole-dipole attractio\ ns

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -18- Questions 29-31 refer to the investigation described below. C 25H30N3+(aq) + OH (aq)  C 25H30N3OH(aq) violet colorless The reaction between C25H30N3 +(aq) and OH (aq), as represented above, is first order with respect to C25H30N3 +(aq) in the presence of excess OH (aq). A 10.0 mL sample of 0.10 M NaOH(aq) is mixed with a 10.0 mL sample of 2.5  10 5 M C25H30N3 +(aq) . A 5.0 mL sample of the mixture is quickly transferred to a clean cuvette and placed in a spectrophotometer, and the progress of the reaction is measured. The data are given in the table below. Time (s) 030 6090120 150180210 240270300 Absorbance 0.620.54 0.470.410.36 0.310.270.23 0.200.17 0.15 29. Approximately how long did it take for 75 percent of the initial amount of C25H30N3+(aq) to react? (A) 75 s (B) 225 s (C) 300 s (D) 600 s 30. What would be the effect on the reaction rate if the solution of C25H30N3+(aq) is diluted by a factor of two? (A) It would be higher. (B) It would be lower. (C) It would not change. (D) It would initially be higher but then rapidly decrease.

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -19- 31. To choose a wavelength to analyze the progress of the reaction, a student records the absorbance spectra of both C 25H30N3 +(aq) and C25H30N3OH( aq) in the range of 200-800 nm. The two spectra are presented in the graph below. The student wants to use the spectrophotometer to measure [C 25H30N3 +] with the greatest sensitivity as the reaction progresses. Which of the following indicates th e best wavelength setting and explains why it is best? (A) 205 nm, because the colorless form of the molecu le will absorb significantly at this wavelength (B) 205 nm, because both forms of the molecule will absorb significantly at this wavelength (C) 590 nm, because only the violet form of the molecule will absorb significantly at this wavelength (D) 590 nm, because this wavelength falls in the violet region of the visible light spectrum

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -20- CO( g) + H 2O( g)   CO 2(g ) + H 2(g) K c = 1.5  10 3 32. A 2.0 mol sample of CO(g) and a 2.0 mol sample of H2O( g) are introduced into a previously evacuated 100. L rigid container, and the temperature is held constant as the reaction represented above reaches equilibrium. Which of the following is true at equilibrium? (A) [H 2O] > [CO] and [CO 2] > [H 2] (B) [H 2O] > [H 2] (C) [CO 2] > [CO] (D) [CO] = [H 2O] = [CO 2] = [H 2]

CompoundK sp at 298 K Ag 2SO 4 1  10 5 PbSO 4 1  10 8 33. A 1.0 L solution of AgNO 3(aq) and Pb(NO 3)2(aq) has a Ag + concentration of 0.020 M and a Pb 2+ concentration of 0.0010 M. A 0.0010 mol sample of K2SO 4(s ) is added to the solution. Based on the information in the table above, which of the following will occur? (Assume that the volume change of the solution is negligible.) (A) No precipitate will form. (B) Only Ag 2SO 4(s ) will precipitate. (C) Only PbSO 4( s ) will precipitate. (D) Both Ag 2SO 4(s ) and PbSO 4(s) will precipitate. 34. The pH of a 0.01 M HNO 2(aq) solution is in which of the following ranges? (For HNO 2(aq), K a = 4.0 × 10 4) (A) Between 1 and 2 (B) Between 2 and 3 (C) Between 4 and 5 (D) Between 6 and 7 35. The photoelectron spectra of the 1 s electrons of two isoelectronic species, Ca 2+ and Ar , are shown above. Which of the following correctly identifies the species associated with peak X and provides a valid justification? (A) Ar, because it has completely filled energy levels (B) Ar, because its radius is smaller than the radius of Ca 2+ (C) Ca 2+, because its nuclear mass is greater than that of Ar (D) Ca 2+, because its nucleus has two more protons than the nucleus of Ar has 36. A vessel contains Ar( g) at a high pressure. Which of the following statements best helps to explain why the measured pressure is significantly greater than the pressure calculated using the ideal gas law? (A) The molar mass of Ar is relatively large. (B) A significant number of Ar 2 molecules form. (C) The attractive forces among Ar atoms cause them to collide with the walls of the container with less force. (D) The combined volume of the Ar atoms is too large to be negligible compared with the total volume of the container. Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -21-

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -22- Questions 37-39 refer to the following information. When water is added to a mixture of Na 2O2(s) and S( s), a redox reaction occurs, as represented by the equation below. 2 Na 2O2(s) + S(s ) + 2 H 2O(l)  4 NaOH( aq) + SO 2(aq) 298H D = 610 kJ/mol rxn ; 298S D = 7.3 J/(K ·mol rxn ) 37. Two trials are run, using excess water. In the first trial, 7.8 g of Na 2O2(s ) (molar mass 78 g/mol) is mixed with 3.2 g of S( s). In the second trial, 7.8 g of Na 2O2(s ) is mixed with 6.4 g of S( s). The Na 2O2( s ) and S( s) react as completely as possible. Both trials yield the same amount of SO 2(aq). Which of the following identifies the limiting reactant and the heat released, q, for the two trials at 298 K? Limiting Reactant q (A) S 30. kJ (B) S 61 kJ (C) Na 2O2 30. kJ (D) Na 2O2 61 kJ 38. Atoms of which element are reduced in the reaction? (A) S; each atom loses four electrons (B) Na in Na 2O2; each atom loses one electron (C) O in Na 2O2; each atom gains one electron (D) O in H2O; each atom gains one electron 39. Which of the following statements about the thermodynamic favorability of the reaction at 298 K is correct? (A) It is thermodynamically unfavorable. (B) It is thermodynamically favorable and is driven by DS only. (C) It is thermodynamically favorable and is driven by DH  only. (D) It is thermodynamically favorable and is driven by both DH  and DS.

BondBond Energy (kJ/mol) H H 430 Cl Cl 240 H Cl 430 40. Based on the bond energies shown in the table above, which of the following diagrams best represents the change in energy as the reaction represented below proceeds? H 2(g) + Cl 2(g)  2 HCl( g) (A) (B) (C) (D) Ionization Energy (kJ/mol) First 577 Second 1,816 Third 2,745 Fourth 11,577 Fifth 14,482 41. Based on the ionization energies of element X given in the table above, which of the following is most likely the empirical formula of an oxide of element X? (A) XO 2 (B)X 2O (C) X 2O3 (D)X 2O5 Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -23-

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -24- 2 H 2S( g) + CH 4(g )   CS 2( g ) + 4 H 2(g ) K c = 3.4  10 4 42. A 0.10 mol sample of each of the four species in the reaction represented above is injected into a rigid, previously evacuated 1.0 L container. Which of the following species will have the highest concentration when the system reaches equilibrium? (A) H 2S(g) (B) CH 4(g) (C) CS 2(g) (D) H 2(g) 43. At 1.0 atm a sample of ice is heated to liquid water and then to water vapor. The heating curve is shown in the graph above. Which of the following lists the signs for the changes in enthalpy and entropy for the process corresponding to segment X , going from left to right? DH  DS  (A) Positive Negative (B) Positive Positive (C) Negative Negative (D) Negative Positive

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -25- Questions 44-47 refer to the following. CH 3OH( g)  CO( g) + 2 H 2(g ) H° = +91 kJ/mol rxn The reaction represented above goes essentially to completion. The reaction ta kes place in a rigid, insulated vessel that is initially at 600 K. 44. What happens to the temperature of the contents of the vessel as the reaction occurs? (A) The temperature must increase, because according to Le Châtelier’s principle, an increase in temperature c auses more products to form. (B) The temperature must decrease, because the reaction takes place at a temperature above room temperature. (C) The temperature must decrease, because the reaction is endothermic. (D) The temperature does not change, because the vessel is insulated. 45. A sample of CH 3OH( g) is placed in the previously evacuated vessel with a pressure of P 1 at 600 K. What is the final pressure in the vessel after the reaction is complete and the contents of the vessel are returned to 600 K ? (A) 1 9 P (B) 1 3 P (C) P 1 (D)3P 1 46. What can be inferred about S° for the reaction at 600 K? (A) It must be positive, since the reaction is thermodynamically unfavorable at 600 K. (B) It must be negative, since there are more moles of products than reactants. (C) It must be positive, since G° is negative and H° is positive. (D) It must be negative, since G° is positive and H° is positive. 47. Which of the following stat ements about the bonds in the reactants and products is most accurate? (A) The sum of the bond enthalpies of the bonds in the reactant is greater than the sum of the bond enthalpies of the bon ds in the products. (B) The sum of the bond enthalpies of the bonds in the reactant is less than the sum of the bond enthalpies of the bonds in the products. (C) The length of the bond between carbon and oxygen in CH 3OH is shorter than the length of the bond between carbon and oxygen in CO. (D) All of the bonds in the reactant and products are polar.

AcidConcentration pH X 0.005 M 2.3 Y 2.0 M 2.8 Z 3.0 M 2.8 48. Which of the following correctly ranks the three monoprotic acids listed in the table above from the weakest to the strongest? (A) X < Y < Z (B) X < Z < Y (C) Y < Z < X (D) Z < Y < X Element Known Oxides H H 2O, H2O2 Li Li 2O, Li2O2 Na Na 2O, Na 2O2, NaO 2 K K 2O, K2O2, KO 2 49. Based on the informa tion above and periodic trends, which of the following is the best hypothesis regarding the oxide(s) formed by Rb? (A) Rb will form only Rb 2O. (B) Rb will form only RbO 2. (C) Rb will form only Rb 2O and Rb 2O2. (D) Rb will form Rb 2O, Rb 2O2, and RbO 2. Fe(s ) + 2 HCl( aq)  FeCl 2(aq) + H 2(g) 50. When a student adds 30.0 mL of 1.00 M HCl to 0.56 g of powdered Fe, a reaction occurs according to the equation above. When the reaction is complete at 273 K and 1.0 atm, which of the following is true? (A) HCl is in excess, and 0.100 mol of HCl remains unreacted. (B) HCl is in excess, and 0.020 mol of HCl remains unreacted. (C) 0.015 mol of FeCl 2 has been produced. (D) 0.22 L of H2 has been produced. Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -26-

Unauthorized copying or reuse of any part of this page is illegal. -32- END OF SECTION I IF YOU FINISH BEFORE TIME IS CALLED, YOU MAY CHECK YOUR WORK ON THIS SECTION. DO NOT GO ON TO SECTION II UNT IL YOU ARE TOLD TO DO SO. ________________________________ MAK E SURE YOU HAVE DONE THE FOLLOWING.  PLACE D YOUR AP NUMBER LABEL ON YOUR ANSWER SHEET  WRITTEN A ND GRIDDED YOUR AP NUMBER CORRECTLY ON YOUR ANSWER SHEET  TAKEN THE AP EXAM LABEL FROM THE FRONT OF THIS BOOKLET AND PLACED IT ON YOUR ANSWER SHEET

Section I I: Free- Response Questions This is the free-response section of the 201 6 AP exam. It includes cover material and other administrative instructions to help familiarize students with the mechanics of the exam. (Note that future exams may differ in look from the following content.)

AP ® Chemistry Exam SECTION II: Free Response 2016 DO NOT OPEN THIS BOOKLET UNTIL YOU ARE TOLD TO DO SO. At a Glance Total Time 1 hour, 45 minutes Number of Questions 7 Percent of Total Score 50% Writing Instrument Either pencil or pen with black or dark blue ink Electronic Device Calculator allowed Suggested Time Approximately 23 minutes each for questions 1 3 and 9 minutes each for questions 4 7 WeightApproximate weights: Questions 1 3: 22% each Questions 4 7: 9% each Instructions The questions for Section II are printed in this booklet. Pages containing a periodic table and lists containing equations and constants are also printed in this booklet . You may use the pages that the questions are printed on to organize your answers or for scratch work, but you must write your answers in the areas designated for each response. Only material written in the space provided will be scored . Examples and equations may be included in your responses where appropriate. For calculations, clearly show the method used and the steps involved in arriving at your answers. You must show your work to receive credit for your answer. Pay attention to significant figures. Write clearly and legibly. Cross out any errors you make; erased or crossed- out work will not be scored. Manage your time carefully. You may proceed freely from one question to the next. You may review your responses if you finish before the end of the exam is announced . Form I Form Code 4MBP4-S 25

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L, mL = liter(s), milliliter(s) mm Hg = millimeters of mercury g = gram(s) E = h c =   = frequency Planck’s constant, h = 6.626  10 34 Js Speed of light, c = 2.998  10 8 ms 1 Avogadro’s number = 6.022  10 23 mol  1 Electron charge, e = 1.602 × 10 19 coulomb K c = [C] [D] [A] [B] c d a b , where a A + b B  c C + d D K p = C D A B () ( ) () ( ) c d a b P P P P K a = [H ][A ] [HA] + - K b = [OH ][HB ] [B] - + K w = [H +][OH ] = 1.0  10 14 at 25 C = K a  K b 灈‽⁰ K a + log [A ] [HA] - Kc (molar concentrations) K w (water) ln[A]t  ln[A] 0 =  kt [] [] 0 A A 1 1 t - = kt t ½ = 0.693 k t ½ = half-life AP ® CHEMISTRY EQUATION S AND CONSTANTS Throughout the exam the following symbols have th e definitions specified unless otherwise noted. J, kJ = joule(s), kilojoule(s) nm = nanometer(s) V = volt(s) atm = atmosphere(s) mol = mole(s) ATOMIC STRUCTURE E = energy  = wavelength EQUILIBRIUM pH = log [H +] , pOH = log [OH ] 14 = pH + pOH p K a = log K a , pK b = log K b Equilibrium Constants K p (gas pressures) K a (weak acid) K b (weak base) KINETICS k = rate constant t = time -3-

1 atm = 760 mm Hg = 760 torr PV = nRT 浯汥猠䄠 PA = P total  X A, where X A = total moles = P A + P B + P C + . . . P total m n = M K = C + 273 D = m V 1 2 KE per molecule = mv 2 A = abc M = molar mass KE = kinetic energy A = absorbance R = 8.314 J mol 1K1 = 62.36 L torr mol 1K1   S = Â S products - Â S reactants   H = Â D H f products - Â DH f reactants   G = Â D G f products - Â DG reactants f G  = H  TS  = RT ln K =  nF E  q I = t S  = standard entropy H  = standard enthalpy G  = standard Gibbs free ener gy E  = standard reduction potential F = 96,485 coulombs per mole of electrons Faraday’s constant, ㄠ橯畬e ㄠ癯汴 㴠 ㄠ捯畬潭戠 GASES, LIQUIDS, AND SOLUTIONS Molarity, M = moles of solute per liter of solution THERMODYNAMICS / ELECTROCHEMISTRY q = mcT P = pressure V = volume T = temperature n = number of moles m = mass D = density v = velocity a = molar absorptivity b = path length c = concentratio n Gas constant, = 0.08206 L atm mol 1K1 STP = 273.15 K and 1.0 atm Ideal gas at STP = 22.4 L mol −1 q = heat m = mass c = specific heat capacity T = temperature n = number of moles I = current (amperes) q = charge (coulombs) t = time (seconds) -4-

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -6- CHEMISTRY Section II 7 Questions Time—1 hour and 45 minutes YOU MAY USE YOUR CALCULATOR FOR THIS SECTION. Directions: Questions 1–3 are long free-response questions that require about 23 minutes each to answer and are worth 10 points each. Questions 4–7 are short free-response que stions that require about 9 minutes each to answer and are worth 4 points each. Write your response in the space provided following each que stion. Examples and equations may be included in your responses where appropriate. For calculations, clearly show the method used and the steps involved in arriving at your answers. You must show your work to receive cred it for your answer. Pay attention to significant figures. CaO( s) + H 2O( l)  Ca(OH) 2(s ) rxnH D  = 63.7 kJ/mol rxn 1. Calcium oxide, CaO( s) , has been proposed as a substance that can be used to heat water quickly for portable heating packs or for cooking. When placed in water, CaO(s) reacts as shown by the equation above. (a) A student wants to design a heating pad that could heat a 150.0 g sample of water from 25.0C to 60.0 C. (i) Calculate the amount of heat, in joules, that the wa ter must absorb for its temperature to change by this amount. (Assume that the specific heat capacity of the water is 4.18 J/(g C).) (ii) Calculate the minimum mass of CaO( s) that the student would need to use in order to cause this temperature change. (b) The student hypothesizes that the design of the heatin g pad could be changed to enable it to heat 150.0 g of water from 25.0 C to 90.0 C by using a greater mass of CaO( s). (i) Use the data in the table below to determine the standard entropy change, rxnS D  , in J/(K mol rxn ) for the reaction. Substance Absolute Entropy at 25 C (J/(K mol)) CaO( s) 83 H 2O( l) 70. Ca(OH) 2(s ) 40. (ii) Is the reaction thermodynamically favorable at 90.0°C? Justify your answer with a calculation. (Assume that both rxnS D  and rxnH D  are constant between 25.0°C and 90.0°C.)

Unauthorized copying or reuse of any part of this page is illegal. GO ON TO THE NEXT PAGE. -7- The student learns that the Ca(OH) 2 produced from the reaction is relatively insoluble and that it dissolves in water according to the equation below. Ca(OH) 2(s)  Ca 2+(aq) + 2 OH −(aq) (c) The student prepares a saturated solution of Ca(OH) 2 and determines that the [Ca 2+] is 0.011 M . Calculate the value of Ksp for Ca(OH) 2 The student wishes to significantly increase the molar solubility of the . Ca(OH) 2(s) and has access to the following substances. 15 mL of distilled water 15 mL of 1.0 M KOH(aq) 15 mL of 1.0 M CaCl 2(aq)15 mL of 1.0 M HCl(aq) (d) Which substance, when added to the Ca(OH) 2 mixture, would increase the molar solubility most significantly? Justify your choice based on concepts of chemical equilibrium, such as Le Châtelier’s principle.

GO ON TO THE NEXT PAGE. -8- ADDITIONAL PAGE FOR ANSWERING QUESTION 1

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