Name: Oregon City High School AP Chemistry Summer Assignment Welcome to AP chemistry! This homework is meant to be a review of the material covered in Chemistry A and B as well as some memorization of ions and solubility rules that you will need throughout the year. Having the following skills will be essential to your success in AP Chemistry and I will expect that you already have a firm grasp on these topics as we start the year. The following assignment is to be completed over the summer and brought in COMPLETED on the first day of class. AP Chemistry is a challenging course. While it is not all about memorization, having these items memorized is essential for success in learning the concepts covered in the course. I have included several resources in this packet. 1. There is a list of the ions that you must know on the first day. Utilize the suggestions for making the process of memorization easier. For instance, 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. I have included a sheet of flashcards for the polyatomic ions that you must learn. I strongly suggest that you cut them out and begin memorizing them immediately. Use the hints on the common ions sheet to help you reduce the amount of memorizing that you must do. **There will be a test on the first day of class to assess your knowledge of these polyatomic ions Please be prepared!!! 2. Memorize the solubility rules and be able to identify whether a substance will break into ions when dissolved in water. **There will be a test on the first day of class to assess your knowledge of these solubility rules Please be prepared!!! 3. There are a number of questions that are meant to help you review the information that you learned in Chemistry A and B and will be expected to know as we begin AP chemistry. These questions will be DUE ON THE FIRST DAY OF CLASS!!! While you may need to reference materials to help remind you how to do some of these problems (your notes from chemistry A and B, your AP Chemistry textbook, the internet, etc.) please make sure that your work is YOUR OWN as you will be the one responsible for understanding this information. Also included is a copy of the periodic table used in AP Chemistry. Notice that this is not the table used in first year chemistry. The AP table is the same that the College Board allows you to use on the AP Chemistry test. Notice that it has the symbols of the elements but not the written names. You need to take that fact into consideration when studying for the afore-mentioned quiz! Do not let the fact that there are no flashcards for monatomic ions suggest to you that the monatomic ions are not important. They are every bit as important as the polyatomic ions. If you have trouble identifying the charge of monatomic ions (or the naming system) then I suggest that you make yourself some flashcards for those as well. Doubtless, there will be some students who will procrastinate and try to do all of this studying just before the start of school. Those students may even cram well enough to do well on the initial quiz. However, they will quickly forget the ions, and struggle every time that these formulas are used in lecture, homework, quizzes, tests and labs. All research on human memory shows us that frequent, short periods of study, spread over long periods of time will produce much greater retention than long periods of study of a short period of time. I could wait and throw these at you on the first day of school, but I don t think that would be fair to you. Use every modality possible as you try to learn these speak them, write them, visualize them. Make flashcards, form a study group, have your friends and family quiz you, take the lists with you on vacation, or do whatever it takes to get this information imbedded in your head. I look forward to seeing you all at the beginning of the next school year. If you need to contact me during the summer, you can call or email me and I will get back to you quickly. Jenaya Hoffman OCHS Chemistry Teacher jenaya.hoffman@orecity.k12.or.us 503-704-9909
1. Nomenclature Rules for Naming Ionic Compounds (metal +nonmetal) A. Balance Charges (charges should net zero) B. Cation is always written first (in name and in formula) C. Change the ending of the anion to ide (unless polyatomic ion, then named as given). I. Name these binary compounds of two nonmetals. IF 7 N 2 O 5 XeF 2 N 2 O 4 As 4 O 10 SF 6 PCl 3 _ S 2 Cl 2 II. Name these binary compounds with a fixed charge metal. AlCl 3 MgO BaI 2 KI SrBr 2 Na 2 S CaF 2 Al 2 O 3 III. Name these binary compounds of cations with variable charge (use roman numerals). CuCl 2 Fe 2 O 3 SnO PbCl 4 Cu 2 S HgS AuI 3 CoP IV. Name these compounds with polyatomic ions. Fe(NO 3 ) 3 _ NaOH Ca(ClO 3 ) 2 KNO 2 NH 4 NO 2 _ Cu 2 Cr 2 O 7 Cu 2 SO 4 NaHCO 3 Acids-For simplicity, the acids that we will be concerned with naming are really just a special class of ionic compounds where the cation is always H +. So if the formula has hydrogen written first, then this usually indicates that the hydrogen is an H + cation and that the compound is an acid. When dissolved in water, acids produce H + ions (also called protons, since removing the single electron from a neutral hydrogen atom leaves behind one proton). Rules for Naming an Acid A. 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 HCl HI _ H 2 S HF B. 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: ClO2- is the Chlorite ion so HClO2. = Chlorous acid. C. 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: ClO3- is the Chlorate ion so HClO3 = Chloric acid. **I like to remember this rule as I ate something and it was icky. HNO 3, which contains the polyatomic ion nitrate, is called nitric acid. HNO 2, which contains the polyatomic ion nitrite, is called nitrous acid. I. Name the following acids using the correct naming rule. HClO 4 H 3 PO 4 H 2 C 2 O 4 _ H 2 SO 4 HC 2 H 3 O 2 _ HNO 2 H 2 CrO 4 H 2 CO 3
II. Name these compounds appropriately. Hint: some of these compounds are covalently bonded (nonmetal + nonmetal) so you will have to use prefixes to indicate how many of each element is in the compound: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-. CO NH 4 CN _ NI 3 AlP LiMnO 4 HClO HIO 3 OF 2 SO 2 CuCr 2 O 7 K 2 O HF FeF 3 KC 2 H 3 O 2 MnS III. Write the chemical formulas. Tin (IV) phosphide _ copper (II) cyanide Magnesium hydroxide _ sodium peroxide Sulfurous acid _ lithium silicate Potassium nitride _ chromium (III) carbonate Gallium arsenide _ cobalt (II) chromate Zinc fluoride _ dichromic acid 2. Composition Complete the following problems showing all work. 1. A 0.941 gram piece of magnesium metal is heated and reacts with oxygen. The resulting magnesium oxide weighed 1.560 grams. Determine the percent composition of each element in the compound. 2. Determine the empirical formula given the following data for each compound: a) Fe = 63.53%, S = 36.47% b) Fe = 46.55%, S = 53.45% 3. A compound contains 21.6% sodium, 33.0% chlorine, 45.1% oxygen. Determine the empirical formula of the compound.
3. Solubility rules I. Review solubility rules and identify each of the following compounds as soluble or insoluble in water. You must memorize the solubility rules given in this packet. You may want to spend time memorizing the solubility rules before you compete the next two sections, try them without using your solubility chart, and then check them using the chart. Na 2 CO 3 CoCO 3 _ Pb(NO 3 ) 2 _ K 2 S BaSO 4 _ (NH 4 ) 2 S _ AgI Ni(NO 3 ) 2 _ KI _ FeS PbCl 2 _ CuSO 4 _ Li 2 O Mn(C 2 H 3 O 2 ) 2 _ Cr(OH) 3 AgClO 3 Sn(SO 3 ) 4 _ FeF 2 _ II. Write out the balanced chemical equation for each of the following double replacement reactions. Predict whether each of these double replacement reactions will give a precipitate or not based on the solubility of the products. If yes, identify the precipitate. silver nitrate and potassium chloride magnesium nitrate and sodium carbonate strontium bromide and potassium sulfate cobalt (III) bromide and potassium sulfide ammonium hydroxide and copper (II) acetate lithium chlorate and chromium (III) fluoride 4. Balancing Equations I. Balance the following equations with the lowest whole number coefficients. S 8 + O 2 SO 3 C 10 H 16 + Cl 2 C + HCl Fe + O 2 Fe 2 O 3 C 7 H 6 O 2 + O 2 CO 2 + H 2 O KClO 3 KCl + O 2 H 3 AsO 4 As 2 O 5 + H 2 O V 2 O 5 + HCl VOCl 3 + H 2 O Hg(OH) 2 + H 3 PO 4 Hg 3 (PO 4 ) 2 + H 2 O
II. Balance the following equations and indicate the type of reaction taking place: 1) NaBr + H3PO4 Na3PO4 + HBr Type of reaction: 2) Ca(OH)2 + Al2(SO4)3 CaSO4 + Al(OH)3 Type of reaction: 3) Mg + Fe2O3 Fe + MgO Type of reaction: 4) C2H4 + O2 CO2 + H2O Type of reaction: 5) PbSO4 PbSO3 + O2 Type of reaction: 6) NH3 + I2 N2I6 + H2 Type of reaction: 5. Stoichiometry and Limiting Factor 1. Given the equation below, what mass of water would be needed to react with 10.0g of sodium oxide? Na 2 O + H 2 O 2NaOH 2. 2NaClO 3 2NaCl + 3O 2 What mass of sodium chloride is formed along with 45.0g of oxygen gas? 3. 4NH 3 + 5O 2 4NO + 6 H 2 O What mass of water will be produced when 100.0g of ammonia is reacted with excess oxygen? 4. If the reaction in #3 is done with 25.0g of each reactant, which would be the limiting factor? 5. Na 2 S + 2AgNO 3 Ag 2 S + 2NaNO 3 If the above reaction is carried out with 50.0g of sodium sulfide and 35.0g of silver nitrate, which is the limiting factor? What mass of the excess reactant remains? What mass of silver sulfide would precipitate? 6. 6NaOH + 2Al 2Na 3 AlO 3 + 3H 2 What volume of hydrogen gas (measured at STP) would result from reacting 75.0g of sodium hydroxide with 50.0g of aluminum?
You will need to memorize this first table for the rest of the year start memorizing over the summer! SOLUBILITY GUIDELINES Compounds Solubility Exceptions Salts of alkali metals (group 1A) and ammonium (NH + 4 ) Soluble Some lithium compounds All nitrate, chlorate and acetate salts Soluble - Sulfate salts Soluble Cation is Pb, Ag, Hg, Ba, Sr, or Ca Halide (group 7A halogen ions) salts Soluble Cation is Ag, Hg or Pb Acids (H in front) Soluble - carbonates, phosphates, chromates, Cation is alkali metal (group 1A) or Insoluble sulfides, hydroxides and oxides ammonium *salts = ionic compounds SOLUBILITY CHART sulfide sulfate phosphate Perchlorate Oxide Nitrate Iodide Hydroxide Chloride Chlorate Carbonate Bromide Acetate Al S S - S S I S S I S I S d + NH 4 S S S S S S S S - S S S S Ba S S I S S S S S ss S I I d Ca S S I S S S S S ss S I ss I Cu 2+ S S - S S I S S I S I S I Fe 2+ S S I S S I S S I S I S I Fe 3+ S S - S S I S S I S I ss d Li S S ss S S S S S S S ss S S Mg S S I S S I S S I S I S d K S S S S S S S S S S S S S Ag ss I I S I - I S I S I ss I Na S S S S S S S S S S S S S Sr S S I S S S S S S S I I I Zn S S I S S I S S I S I S I S = Soluble Key: ss = slightly soluble d = decomposes in water - = no such compound exists I = insoluble
Common Ions and Their Charges A mastery of the common 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, when I will give you a quiz on them. You will always be allowed a periodic table, which makes indentifying the ions on the left automatic. For tips on learning these ions, see the opposite side of this page.