AP CHEMISTRY SUMMER ASSIGNMENT

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1 WELCOME TO Hi! My name is Ms. Scheffel. I will be your AP Chemistry teacher next school year. As the school year is coming to an end, I wanted to get out some information about class for next school year. I am excited to meet all of you and begin another fun year of AP Chemistry. Over the summer I have an assignment that I would like you to complete, see below. I will be at school on and off over the summer if you want to come in and work with me on the assignment. Please me ahead of time and we can schedule a time to meet. I also suggest meeting with others that have signed up for the class so you can work on the assignment together. This assignment will allow you to review some important material and get a jump start on the material for the first unit of the school year. There will also be the AP Summer Bridge Program at CT towards the end of summer. You will be receiving information about the opportunity in the mail or look on the website for the latest details. AP CHEMISTRY SUMMER ASSIGNMENT Please Note: This assignment is a requirement, and is NOT for extra credit! This assignment will be looked at as a completion grade. You will not be graded for correctness, but whether or not the assignment was completed on time. This assignment is due on the first day of class. The whole assignment should take 2-4 hours to complete. If you have taken Chemistry Honors I would make flashcards to use over the summer and do the actual naming and mole conversion practice closer to the start of the school year as a refresher. If you are taking chemistry for the first time consider starting with naming and doing practice throughout the summer. Sciencegeek.net is a great website for additional practice. Go to school website and printout the summer assignment. (Or you can me and I will send it to you.) a. me. In this please tell me a little about yourself. What grade will you be in? What science classes have you taken at CT? What are your hobbies? Do you have a job? Tell me anything else you would like to tell me. b. Make flashcards for elements and polyatomic ions with oxidation states. c. Complete naming/writing formulas practice, molar mass and mole conversions. d. Soon after the school year begins you will have a naming and formula writing quiz. You MUST show mastery of naming on this quiz to receive credit. Details on the first day of class. Please feel free to stop in and see me before the end of the school year with any questions that you may have or me this summer if you would like to meet for some additional help. Thank you! Julie Scheffel Science Teacher and Department Coordinator

2 Welcome to AP Chemistry! Most of you already have a background in chemistry from your Chemistry or Honors Chemistry class, but AP Chemistry is very different. Rather than memorizing how to do particular types of problems, you must really conceptually understand the chemistry and be able to apply it to all sorts of different situations. It is not all about memorization; however, having these items memorized is essential for success in learning the concepts covered in the course. Make flashcards, have your friends and family quiz you, take the lists with you on vacation, or do whatever it takes to get this information firmly planted in your head. Do not wait until the night before school begins. NO LATE ASSIGNMENTS WILL BE ACCEPTED!!! AP CHEMISTRY FIRST WEEK QUIZ Tips for Learning the Ions From the Table 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 Polyatomic Anions Most of the work on memorization occurs with these ions, but there are a number of patterns that can greatly reduce the amount of memorizing that one must do. 1. ate anions have one more oxygen then 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 SO 4 2-, so sulfite has the same charge but one less oxygen (SO 3 2- ) b. nitrate is NO 3-, so nitrite has the same charge but one less oxygen (NO 2- ) 2. If you know that a sulfate ion is SO 4 2- then to get the formula for 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 on the new ion is less negative by one. a. Example: PO 4 3- HPO 4 2- H 2PO 4 - phosphate hydrogen phosphate dihydrogen phosphate 3. Learn the hypochlorite chlorite chlorate perchlorate series, and you also know the series containing iodite/iodate as well as bromite/bromate. 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, hypothermic or hypoglycemia ) i. Hypochlorite is under chlorite, meaning it has one less oxygen c. The prefix hyper means above or too much (think hyperkinetic ) 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 - ClO 2 - ClO 3 - ClO 4 - hypochlorite chlorite chlorate perchlorate

3 Rules for Naming Ionic Compounds - REVIEW 1. Balance Charges (charges should equal zero) 2. Cation is always written first (for name and formula, use roman numerals in name when using transition metals with multiple charges) 3. Change the ending of the anion to ide 4. Watch out for polyatomic used in ionic compounds, see list below Rules for Naming an Acid REVIEW 1. When the name of the anion ends in ide, the acid name begins with the prefix hydro-, the stem of the anion has the suffix ic and it is followed by the word acid. -ide becomes hydro ic acid Example: Cl - is the chloride ion so HCl = hydrochloric acid 2. When the anion name ends in ite, the acid name is the stem of the anion with the suffix ous, followed by the word acid. -ite becomes ous acid Example: ClO 2 - is the chlorite ion so HClO 2 = chlorous acid. 3. When the anion name ends in ate, the acid name is the stem of the anion with the suffix ic, followed by the word acid. -ate becomes ic acid Example: ClO 3 - is the chlorate ion so HClO 3 = chloric acid. Strong Acids HCl, HI, HBr, HClO 4, HNO 3, H 2SO 4

4 Polyatomic Ions MAKE FLASHCARDS Name Symbol/Charge ammonium NH +1 4 acetate C 2H 3O 1-2 or CH 3COO 1- perbromate BrO 1-4 bromate BrO 1-3 bromite BrO 1-2 hypobromite BrO 1- perchlorate ClO 1-4 chlorate ClO 1-3 chlorite ClO 1-2 hypochlorite ClO 1- periodate IO 1-4 iodate IO 1-3 iodite IO 1-2 hypoiodite IO 1- cyanide CN 1- dihydrogen phosphate H 2PO 1-4 hydrogen carbonate HCO 1-3 hydrogen sulfate HSO 1-4 hydrogen sulfite HSO 1-3 hydrogen sulfide HS 1- hydroxide OH 1- nitrate NO 1-3 nitrite NO 1-2 permanganate MnO 1-4 thiocyanate SCN 1- amide NH 1-2 carbonate CO 2-3 chromate CrO 2-4 dichromate Cr 2O 2-7 peroxide O 2-2 oxalate C 2O 2-4 selenite SeO 2-4 thiosulfate S 2O 2-3 sulfate SO 2-4 sulfite SO 2-3 phosphate PO 3-4 phosphite PO 3-3 borate BO 3-3

5 Elements to Know MAKE FLASHCARDS you need to know names and symbols only Aluminum Argon Barium Beryllium Boron Bromine Calcium Carbon Cesium Chlorine Chromium Copper Fluorine Francium Gold Helium Hydrogen Iodine Iron Krypton Lead Lithium Magnesium Manganese Mercury Neon Nickel Nitrogen Oxygen Phosphorus Potassium Radon Rubidium Silicon Silver Sodium Sulfur Tin Tungsten Uranium Zinc

6 Writing Basic Ionic Formulas Video tutorial: Practice write the formulas for the following names: sodium oxide potassium fluoride calcium chloride aluminum sulfide magnesium oxide lithium bromide cesium phosphide aluminum iodide strontium phosphide Practice write the names for the following formulas: K 2O NaCl Li 2S SrO AlBr 3 MgF 2 LiF CaO Mg 3P 2 Writing Formulas with Polyatomic Ions Video tutorial: Write the chemical formula for the following names magnesium nitrate sodium nitrate potassium carbonate ammonium chloride calcium sulfate lithium ethanoate strontium hydroxide magnesium phosphate potassium dichromate Write the name for the following formulas NaOH K 2SO 4 Ca(C 2H 3O 2) 2 NaCr 2O 7 (NH 4) 2O KMnO 4 Ca(NO 3) 2 NaHCO 3 Sr(MnO 4) 2

7 Writing Formulas with Transition Metals Video tutorials: Into to transition metals in ionic formulas: Writing transition metal formulas: Write the chemical formula for the following names iron (II) oxide iron (III) oxide manganese (IV) chloride copper (I) oxide copper (II) oxide chromium (III) oxide lead (II) hydroxide iron (III) nitrate copper (I) nitride Video tutorial: Naming transition metals in ionic compounds CuS FeCl 3 FeO PbO 2 SnCl 4 SnO 2 Cu 2S Fe(OH) 2 Au 3PO 4

8 Intro to chemical reactions and reaction balancing. Video tutorial and notes for this page can be found here: Balance the following reactions: 1) N 2 + H 2 NH 3 2) KClO 3 KCl + O 2 3) NaCl + F 2 NaF + Cl 2 4) H 2 + O 2 H 2O 5) Pb(OH) 2 + HCl H 2O + PbCl 2 6) AlBr 3 + K 2SO 4 KBr + Al 2(SO 4) 3 7) CH 4 + O 2 CO 2 + H 2O 8) C 3H 8 + O 2 CO 2 + H 2O 9) C 8H 18 + O 2 CO 2 + H 2O 10) FeCl 3 + NaOH Fe(OH) 3 + NaCl 11) P + O 2 P 2O 5 12) Na + H 2O NaOH + H 2 13) Ag 2O Ag + O 2 14) S 8 + O 2 SO 3 15) CO 2 + H 2O C 6H 12O 6 + O 2 16) K + MgBr 2 KBr + Mg 17) HCl + CaCO 3 CaCl 2 + H 2O + CO 2 18) HNO 3 + NaHCO 3 NaNO 3 + H 2O + CO 2 19) H 2O + O 2 H 2O 2 20) NaBr + CaF 2 NaF + CaBr 2 21) H 2SO 4 + NaNO 2 HNO 2 + Na 2SO 4

9 The mole concept and mass/mole conversions. Video tutorial and notes: 1) What is a mole? 2) Sample A contains a mole of gold atoms. Sample B contains a mole of zinc atoms. a) Which sample contains more atoms? Or are they the same? Explain. b) Which sample is heavier? Or are they the same? Explain. Find the molar mass of the following substances. 1) Cl 2 2) KOH 3) BeCl 2 4) Fe 2O 3 5) Ca(NO 3) 2 6) CCl 2F 2 7) Mg(OH) 2 8) Na 2SO 4 10 H 2O 9) MgSO 4 7H 2O 10) Be(NO 3) 2 4H 2O

10 Mole Conversions Video tutorial : Given the following, find the number of moles: 1) grams of H 3PO 4 2) 25.0 grams of HF 3) grams of NaHCO 3 4) 1.10 grams of FeCl 3 5) 987 grams of Ra(OH) 2 6) 564 grams of copper 7) 12.3 grams of CuSO 4 5H 2O 8) 89.0 grams of Pb(CH 3COO) 4 Given the following, find the number of grams: 9) 4 moles of Cu(CN) 2 10) 5.6 moles of C 6H 6 11) 21.3 moles of BaCO 3 12) 1.2 moles of (NH 4) 3PO 3 13) 9.3 x 10-3 moles of SmO 14) 6.6 moles of ZnO 15) 5.4 moles of K 2SO 4 16) 88.4 moles of NI 3