AP Chemistry Summer Assignment

Transcription

1 AP Chemistry Summer Assignment Print this out and take it to a quiet place. Get a highlighter, a pencil, and a planner. Read this entire document in one sitting. Plan out when you will set aside time to complete this assignment and turn it in by the due date. I am thrilled that you have chosen to take AP Chemistry this year! This course will cover all of the material that is typically covered in the first two semesters of college chemistry. Needless to say, the curriculum is packed with material that we will try to complete by the end of April so that we will have a few days of review before the May exam. If you re not passionate about chemistry, if you re not able to produce consistent, high-quality academic work, or if you re looking for a course that you can manage with minimal effort walk away NOW. You will have at least one hour of homework every evening in order to keep up with the pace of this course. Many of you who have breezed through other science courses will struggle in this class. However, if you enjoy learning for its own sake, if you re motivated by academic challenges, and if you re prepared to engage in college-level laboratory analysis read on! This course will reward you in many ways. ASSIGNMENT 1 (Due by 11:59 PM, June 26, 2017) me at julianne.hall@dpsnc.net with a paragraph about yourself. Subject Line: AP Chemistry , Your Name Body: Your full name, nickname that you go by if you have one, and stuff about you! Who was your last science teacher? What class? What science classes have you taken? What other science classes are you taking? What are you looking forward to the most in AP Chemistry? What are you most anxious about in AP Chemistry? Why are you taking AP Chemistry? What do you hope to accomplish/gain? Include any other relevant details that can help me develop a sense of who you are and how you learn. Describe your plan for succeeding in this class and overcoming any challenges that you will face. Also include your requirements for me how can I help to make this year a success? While you may be tempted to make this message informal, especially if I have taught you before, please keep in mind that you are representing yourself in writing in an academic setting. Therefore, you should use appropriate formatting, grammar, and language. Don t type this on your phone. Hopefully, this will be the only time I ll need to remind you of this during the year. You must hold yourself to the highest academic standards in this class. ASSIGNMENT 2 (Due by 4:00 PM, August 14, 2017) During the first two weeks of the course, we will review material from the first four chapters of the text. To be ready, you will complete the following work from your textbook on lined or graph paper and return a hard copy to Ms. Hall by Monday, August 14 th. You may either mail it to school or drop it by the school office. I will have them graded before the first day of class. My hope is that you will begin to recall some of the chemistry that you handled with ease during your first year of chemistry, and build on a few of these topics. My intent is to get a quick start on this review so that we can maximize the number of days to cover the AP level material. If the exercise requires a calculation, include it in your work. Remember that the set-up of the problem is far more important than the final answer!

2 You can pick up a copy of the text from Ms. Hall in Room S201. Please stop in sometime during the first week of June to pick up your text. You should use only the following materials to complete these problems: Brown & Lemay s Chemistry: The Central Science, 12 th ed. (your textbook) AP periodic table (attached) Scientific calculator Pencil and paper (please do NOT do this assignment in pen) Please make sure that you obey the significant figure rules from Chapter 1 throughout your calculations. Note that the addition/subtraction rules (which we did not cover in first year chemistry) are outlined in this chapter. They should be obeyed from this point forward! The multiplication/division rules are the same as in first year chemistry. Also, please NUMBER YOUR WORK (Chapters & Problem Number) so that I can easily determine which problem you re answering and WRITE NEATLY. Finally, I do not expect this assignment to be easy. Many of these problems will challenge you, especially from Chapter 4 which contains some new material. Read the chapter carefully, and accept this challenge. Welcome to AP Chemistry! Chapter 1: Matter and Measurement Read the entire chapter. You want to have a good command of the metric system, significant figures, and the factor-unit method of problem solving. Write out your answers to these exercises on pgs : 1, 2, 6, 8, 11, 12, 14, 20, 23, 24, 26, 28, 32, 37, 40, 42, 44, 47, 58, 59, 63, 71 Chapter 2: Atoms, Molecules, and Ions Read the entire chapter. You want to have a good command of the fundamental structure of an atom (protons and neutrons in nucleus and electrons outside nucleus), isotopes, basic layout of the Periodic Table, and naming ionic compounds. Write out your answers to these exercises on pgs : 2, 5, 7, 11, 14, 17, 19, 24, 26, 27, 30, 32, 38, 39, 43, 46, 48, 56, 58, 60, 66, 68, 70, 72, 74, 78, 90, 104 Chapter 3: Stoichiometry Read the entire chapter. This chapter reviews balancing reactions and mole calculations. Write out your answers to these exercises on pgs : 4, 5, 14, 16, 18, 24ace, 32, 34, 40, 46a, 50, 52b, 54b, 58, 60, 64, 70, 76, 82, 97, 109 Chapter 4: Chemical Reactions and Solution Chemistry Read the entire chapter. This chapter reviews some important reaction types as well as calculations involving molarity. Write out your answers to these exercises on pgs : 2, 4, 6, 7, 8, 9, 12, 14, 16, 18, 20, 24, 26, 30, 31, 34, 38, 40, 42, 45, 46, 48, 50, 51, 54, 56, 62, 68, 70, 72, 74, 78, 80, 82a&d, 87, 92, 94, 97a&b, 109

3 ASSIGNMENT 3 In order to jump in to the detailed AP Chemistry curriculum, you will need to have a strong grasp on chemical nomenclature. You should already be familiar with the names and symbols of the elements, but if you are not, please review this material. I have attached a copy of the AP Periodic Table that you will use all year. You will notice that it does not include the names of the elements. You must be able to produce the names of each element when looking at this periodic table. You must also memorize the names, formulas, and charges of the common ions we will be using in AP Chemistry this year. On the second day of class, you ll be given a quiz on the common ions. You ll be asked to: Write the names of these ions when given the formula and charge Write the formula and charge when given the names In this packet, I have included a list of the ions that you must know for this quiz, and some suggestions for making the process of memorization easier. Many of you will remember that most of the monatomic ions have charges that are directly related to their placement on the periodic table. There are naming patterns that greatly simplify the learning of the polyatomic ions as well. Please make a set of flashcards for the ions that you have not already committed to memory with the name of the ion on one side, and the formula on the other. You will NOT turn these flashcards in to me, but if you choose not to make them, you will be at a significant disadvantage on Day 1. This is not material that you should cram for in one night. Some of you may be able to cram well enough to do well on this first quiz. However, those of you who make this choice will quickly forget these ions, and struggle every time they are used in lecture, homework, quizzes, tests, and labs. All research on human memory shows that frequent, short periods of study, spread over long periods of time will produce much greater retention than long periods of study over a short period of time. I m giving these to you now, instead of on the first day of school, to give you a fair chance to succeed in this class. Use every modality possible as you learn these speak them, write them, visualize them. It may also help if you color-code these flashcards in a way that you see fit. Finally, I d like to share with you my class philosophy for AP Chemistry. There are many other courses that will not challenge you in this way. If you re right for this course, you personally desire rigorous academics for the sake of self-development. I truly believe that there is REAL VALUE in struggling to improve intellectually. Many talented high school students have impressive GPAs because they ve mastered this system they complete assignments and study hard and that s great. However, many of those same students haven t actually acquired any academic skills of value since middle school. This course is about going far beyond what is required of you at DSA, at this level. It will prepare you for academic excellence in highly competitive undergraduate and graduate programs around the world. I am available and excited to help you, and this includes over the summer. Please contact me as often as needed! Sincerely, Julianne Hall (513) (use this for emergencies only) julianne.hall@dpsnc.net

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5 Common Ions and Their Charges A mastery of these ions, their formulas, and their charges, is essential to success in AP Chemistry. You are expected to know all of these ions on the first day of class. You will always be allowed the AP periodic table, which makes identifying the ions on the left automatic. For tips on learning these ions, see the back of this page. From the table: Ions to Memorize Cations Name Cations Name H + Hydrogen Ag + Silver Li + Lithium Zn 2+ Zinc Na + Sodium Hg2 2+ Mercury(I) K + Potassium NH4 + Ammonium Rb + Rubidium Anions Name Cs + Cesium NO2 - Nitrite Be 2+ Beryllium NO3 - Nitrate Mg 2+ Magnesium SO3 2- Sulfite Ca 2+ Calcium SO4 2- Sulfate Ba 2+ Barium HSO4 - Hydrogen sulfate (bisulfate) Sr 2+ Strontium OH - Hydroxide Al 3+ Aluminum CN - Cyanide PO4 3- Phosphate Anions Name HPO4 2- Hydrogen phosphate H - Hydride H2PO4 - Dihydrogen phosphate F - Fluoride NCS - Thiocyanate Cl - Chloride CO3 2- Carbonate Br - Bromide HCO3 - Hydrogen carbonate (bicarbonate) I - Iodide ClO - Hypochlorite O 2- Oxide ClO2 - Chlorite S 2- Sulfide ClO3 - Chlorate Se 2- Selenide ClO4 - Perchlorate N 3- Nitride BrO - Hypobromite P 3- Phosphide BrO2 - Bromite As 3- Arsenide BrO3 - Bromate BrO4 - Perbromate Type II Cations Name IO - Hypoiodite Fe 3+ Iron(III) IO2 - Iodite Fe 2+ Iron(II) IO3 - Iodate Cu 2+ Copper(II) IO4 - Periodate Cu + Copper(I) C2H3O2 - Acetate Co 3+ Cobalt(III) MnO4 - Permanganate Co 2+ Cobalt(II) Cr2O7 2- Dichromate Sn 4+ Tin(IV) CrO4 2- Chromate Sn 2+ Tin(II) O2 2- Peroxide Pb 4+ Lead(IV) C2O4 2- Oxalate Pb 2+ Lead(II) NH2 - Amide Hg 2+ Mercury(II) BO3 3- Borate S2O3 2- Thiosulfate

6 Tips for Learning the Ions From the Table These ions can be organized into two groups. 1) Their place on the table suggests the charge on the ion, since the neutral atom gains or loses a predictable number of electrons in order to obtain a noble gas configuration. This was a focus in first year chemistry, so if you are unsure what this means, get help BEFORE the start of the year. a) All Group 1 Elements (alkali metals) lose one electron to form an ion with a 1+ charge b) All Group 2 Elements (alkaline earth metals) lose two electrons to form an ion with a 2+ charge c) Group 13 metals like aluminum lose three electrons to form an ion with a 3+ charge d) All Group 17 Elements (halogens) gain one electron to form an ion with a 1- charge e) All Group 16 nonmetals gain two electrons to form an ion with a 2- charge f) All Group 15 nonmetals gain three electrons to form an ion with a 3- charge Notice that cations keep their name (sodium ion, calcium ion) while anions get an -ide ending (chloride ion, oxide ion). 2) Metals that can form more than one ion will have their positive charge denoted by a roman numeral in parenthesis immediately next to the name of the ion. Polyatomic Anions Most of the work on memorization occurs with these ions, but there are a number of patterns that greatly reduce the amount of memorizing that you must do. 1) ate anions have one more oxygen than the ite ion, but the same charge. If you memorize the ate ions, then you should be able to derive the formula for the ite ion and vice-versa. a) Sulfate is SO4 2-, so sulfite has the same charge but one less oxygen (SO3 2- ) b) Nitrate is NO3 -, so nitrite has the same charge but one less oxygen (NO2 - ) 2) If you know that a sulfate ion is SO4 2-, then to get the formula for the hydrogen sulfate ion, you add a hydrogen ion to the front of the formula. Since a hydrogen ion has a 1+ charge, the net charge of the new ion is less negative by one. a) Example: PO4 3- HPO4 2- H2PO4 - Phosphate hydrogen phosphate dihydrogen phosphate 3) Learn the hypochlorite chlorite chlorate perchlorate series, and you also know the series containing bromite/bromate as well as iodite/iodate. a) The relationship between the ite and ate ion is predictable, as always. Learn one and you know the other. b) The prefix hypo means under or too little (think hypodermic or hypotonic ) i. Hypochlorite is under chlorite, meaning it has one less oxygen c) The prefix hyper means above or too much (think hyperactive or hypertonic ) i. The prefix per is derived from hyper so perchlorate (hyperchlorate) has one more oxygen than chlorate. d) Notice how this sequence increases in oxygen while retaining the same charge: ClO - ClO2 - ClO3 - ClO4 - hypochlorite chlorite chlorate perchlorate

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