Summer Assignment for AP Chemistry: I hope you are all ready for a fun, yet challenging year. You have a good foundation in basic chemistry from Chem

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1 Summer Assignment for AP Chemistry: I hope you are all ready for a fun, yet challenging year. You have a good foundation in basic chemistry from Chem 1, but AP Chem will be a little different. Rather than just memorizing how to do particular types of problems, you must instead really understand the chemistry behind each process and be able to apply it to all sorts of different situations. Students who finish AP Chem come out with a better understanding of the world around them. They also come out with a sense of accomplishment. AP Chem is a difficult class, but with determination and perseverance, you will surely succeed. Even though AP Chem is about using chemistry, there are some items that you must have memorized in order to keep up with the class. Having these items memorized is essential for success in learning the concepts covered in the AP Chemistry curriculum. Make flash cards, 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. The lists that you need to have memorized to ensure success are below, and are attached to this document. There will be a quiz on these seven lists on the first day of classes in August. 1. Ionic Charges, including the polyatomic ions 2. Polyatomic elements 3. Common Metric prefixes 4. Rules for naming Acids 5. Rules for naming ionic compounds 6. Solubility rules 7. Oxidation numbers assigning rules Like almost all AP level courses, this course comes with a summer assignment. Don t procrastinate! Start out the year on a good note. If you need help with the assignment, you will find it in your Chem 1 notes or on the internet. You may also feel free to work together with other students enrolled in the class. The assignment is designed to force you to review topics covered in Chem 1 that I expect you to be familiar with and having retained. Those topics include: Naming and writing formulas for ionic compounds and acids Empirical and Molecular formula calculations Stoichiometric calculations Balancing reaction equations Predicting products of the basic types of reactions The summer assignment is due the first day of school in August. And there will be a test on this material within the first two weeks of school. We will begin the year with a brief project that will very quickly review the material listed above, and then test on that material. However, you will want to be able to do the simple tasks attached to this document, before the project. There is no guarantee of a 5 on the AP Chemistry Exam, but I will guarantee you the opportunity to learn chemistry at a substantially deeper level than you ve seen it thus far. You will however only get out of the class what you put into it. Welcome aboard and I am excited about getting the opportunity to work with you for another year. I know that we will learn so much together and keep each other challenged throughout the year to give our best on everything covered. If you have any questions this summer as you begin to prepare, feel free to me at jason.swango@fayette.kyschools.us.

2 Naming and writing chemical formulas is an essential skill to know before starting AP Chemistry. Use your Chem I notes and the link below to review the concept. In Chem I you learned some polyatomic ions. For a little help try this link: I. Chemical Bonding IA. Chemical Formulas 1. Write formulas for the following substances: (A) Barium sulfate 2. Name each of the following compounds (Give acid names where appropriate) (B) Ammonium chloride (A) CuSO 4 (C) Chlorine monoxide (B) PCl 3 (D) Silicone tetrachloride (C) Li 3N (E) Magnesium fluoride (D) BaSO 3 (F) Sodium oxide (E) N 2F 4 (G) Sodium peroxide (F) KClO 4 (H) Copper (I) iodide (G) NaH (I) Zinc sulfide (H) (NH 4) 2Cr 2O 7 (J) Potassium carbonate (I) HNO 2 (K) Hydrobromic acid (J) Sr 3P 2 (L) Perchloric acid (K) Mg(OH) 2 (M) Lead (II) acetate (L) Al 2S 3 (N) Sodium permanganate (M) AgBr (O) Lithium oxalate (N) P 4O 10 (P) Potassium cyanide (O) HC 2H 3O 2 (Q) Iron (III) hydroxide (P) CaI 2 (R) Silicone dioxide (Q) MnO 2 (S) Nitrogen trifluoride (R) Li 2O (T) Chromium (III) oxide (S) FeI 3 (U) Calcium chlorate (T) Cu 3PO 4 (V) Sodium thiocyanate (U) PCl 3 (W) Cobalt (III) nitrate (V) NaCN (X) Nitrous acid (W) Cs 3N (Y) Ammonium phosphate (X) Zn(NO 3) 2 (Z) Potassium chromate (Y) N 2O (Z) HF IIB. Covalent Bonding For each compound in this list draw their lewis structure, determine their 3-Dimensional shape, decide if they are polar or nonpolar, and what type of Intermolecular Forces between each molecule. H 2O, CH 4, CO 2, CO, NO 2, CO 3, NH 4 +1, NH 3

3 Writing chemical equations is also an essential skill. In Chem I, you used the rxns packet to help you predict products of reactions. In AP Chem, you have to memorize all of that information and more! Zoikes! Don t worry; you ll learn it a little at a time. But, you should at least be able to do it with the cheat sheet (rxns packet). If you need help, there are several excellent links on this page: II. Chemical Equations For each equation below, identify the type (synthesis, decomposition, single replacement, double replacement, or combustion), predict the products, and then write the balanced reaction. Remember to use the solubility rules for double replacement reactions and the activity series for single replacement reactions. Hint: when writing these reactions, ignore all of the information about heat, or bubbling, or mixing. These are just excess words used to make complete sentences. Simply pull out the chemical formulas. For example: Solutions of silver nitrate and magnesium iodide are combined. This is a double replacement reaction. 2AgNO 3 + MgI 2 2AgI + Mg(NO 3) 2 1. Ammonium sulfate reacts with barium nitrate. 2. Zinc metal is added to a solution of copper (II) chloride. 3. Propane gas (C 3H 8) is burned in excess oxygen. 4. Solid calcium chlorate is heated strongly. 5. Magnesium and nitrogen gas are heated together. 6. Chlorine gas is bubbled through a solution of sodium bromide. 7. Solutions of lead nitrate and calcium iodide are combined. 8. Sulfuric acid is combined with sodium hydroxide. 9. Isopropyl alcohol (C 3H 7OH) is burned in oxygen. 10. Iron metal shavings are added to hydrochloric acid. 11. Solid sodium carbonate is heated in a crucible. 12. Sodium metal is added to distilled water.

4 The final summer topic is stoichiometry. For help on percent composition or empirical formulas, try this link: For help with stoichiometry or mole conversions, try one of the many links on this page: III. Stoichiometry 1) Find the mass percent of nitrogen in each of the following compounds: a. NO b. NO 2 c. N 2 O 4 d. N 2 O 2) Benzene contains only carbon and hydrogen and has a molar mass of 78.1 g/mol. Analysis shows the compound to be 7.74% H by mass. Find the empirical and molecular formulas of benzene. 3) Calcium carbonate decomposes upon heating, producing calcium oxide and carbon dioxide gas. (A) Write a balanced chemical equation for this reaction. (B) How many grams of calcium oxide will be produced after g of calcium carbonate is completely decomposed? (C) What volume of carbon dioxide gas is produced from this amount of calcium carbonate, at STP?

5 4) Hydrogen gas and bromine gas react to form hydrogen bromide gas. (A) Write a balanced chemical equation for this reaction. (B) 3.2 g of hydrogen gas and 9.5 g of bromine gas react. Which is the limiting reagent? (C) How many grams of hydrogen bromide gas can be produced using the amounts in (b)? (D) How many grams of the excess reactant are left unreacted? (E) What volume of HBr, measured at STP, is produced in (B)? 5) When ammonia gas, oxygen gas and methane gas (CH 4) are combined, the products are hydrogen cyanide gas and water. (A) Write a balanced chemical equation for this reaction. (B) Calculate the mass of each product produced when 225 g of oxygen gas is reacted with an excess of the other two reactants. (C) If the actual yield of the experiment in (B) is 105 g of HCN, calculate the percent yield. 6) When solutions of potassium iodide and lead (II) nitrate are combined, the products are potassium nitrate and lead (II) iodide. (A) Write a balanced equation for this reaction, including (aq) and (s). (B) Calculate the mass of precipitate produced when 50.0mL of 0.45M potassium iodide solution and 75mL of 0.55M lead (II) nitrate solution are mixed. (C) Calculate the volume of 0.50M potassium iodide required to react completely with 50.0mL of 0.50M lead (II) nitrate.

6 H +1 Li +1 Na +1 K +1 Ag +1 Au +1 Cu +1 NH 4 +1 H 3 O +1 O 2 +1 COMMON IONS AND THEIR CHARGES CATIONS ANIONS Hydrogen Lithium Sodium Potassium Silver Gold Copper I (Cuprous) Ammonium Hydronium Dioxygenyl Be +2 Mg +2 Ca +2 Sr +2 Ba +2 Ra +2 Zn +2 Cu +2 Ni +2 Pb +2 Sn +2 Hg +2 Fe +2 Co +2 *Hg 2 +2 Hg +2 CrO 2 +2 Copper II (Cupric) Nickel II (Nickellous) Lead II (Plumbous) Tin II (Stannous) Mercury II (Mercuric) Iron II (Ferrous) Cobalt II (Cobaltous) Mercury I (Mercurous) Mercury II (Mercuric) Chromyl *The cation Mercury I exists as two Mercury I ions covalently bonded called Dimercury Al +3 Cr +3 Fe +3 Ni +3 Co +3 As +3 Bi +3 Aluminum Chromium III (Chromous) Iron III (Ferric) Nickel III (Nickellic) Cobalt III (Cobaltic) Arsenic III Bismuth III Bold ions mean atoms form multiple ionic charges Suffix -ate means more Oxygen Suffix -ite means less Oxygen Prefix hypo- means less than Prefix hyper- means more than Sn +4 Pb +4 Cr +4 Tin IV (Stannic) Lead IV (Plumbic) Chromium IV (Chromic) +5 As +5 Bi +5 Arsenic V Bismuth V F Cl Br I C 2 H 3 O 2 OH CN MnO 4 NO 3 NO 2 ClO ClO 2 ClO 3 ClO 4 HSO 4 HSO 3 HCO 3 HS H 2 PO 4 SCN IO 2 IO 3 IO 4 BrO 3 O 2 NH 2 HCO 2 Fluoride Chloride Bromide Iodide Acetate Hydroxide Cyanide Permanganate Nitrate Nitrite Hypochlorite Chlorite Chlorate Perchlorate Hydrogensulfate Hydrogensulfite Hydrogencarbonate Hydrogensulfide Dihydrogen phosphate Thiocyanate Iodite Iodate Periodate Bromate Superoxide Amide Formate O S CO 3 SO 4 SO 3 CrO 4 Cr 2 O 7 C 2 O 4 HPO 4 O 2 S 2 O 3 SnO 3 SnO 2 MoO 4 TeO 3 S 2 FeO 4 HAsO 4 Oxide Sulfide Carbonate Sulfate Sulfite Chromate Dichromate Oxalate Monohydrogen phosphate Peroxide Thiosulfate Stannate Stannite Molybdate Tellurite Disulfide Ferrate Hydrogen Arsenate N -3 P -3 PO 4-3 PO 3-3 C 6 H 5 O 7-3 Fe(CN) 6-3 Fe(CN) 6-4 Si 2 O 7-6 TeO 6-6 Nitride Phosphide Phosphate Phosphite Citrate Ferricyanide -4 Ferrocyanide -6 Pyrosilicate Orthotellurate ACID NAMING RULES Dry Name Acid Name Binary acids Hydrogen ide Hydro ic Ternary acids Hydrogen ate ic Ternary acids Hydrogen ite ous

7 Polyatomic Elements hydrogen H 2 nitrogen N 2 oxygen O 2 fluorine F 2 chlorine Cl 2 bromine Br 2 iodine I 2 ozone O 3 phosphorus P 4 sulfur S 8

8 List of the Metric Prefixes Prefix Symbol Numerical Exponential yotta Y 1,000,000,000,000,000,000,000, zetta Z 1,000,000,000,000,000,000, exa E 1,000,000,000,000,000, peta P 1,000,000,000,000, tera T 1,000,000,000, giga G 1,000,000, mega M 1,000, kilo k 1, hecto h deca da no prefix means: deci d centi c milli m micro µ nano n pico p femto f atto a zepto z yocto y

9 Rules For Naming Ionic Compounds & Acids 1) Ionic Compounds metals with nonmetals NEVER USE PREFIXES! If the compound is binary: A) The metal (cation) is written first. Name it. If the metal can have more than one type of ion (most transition metals), you must be specific and use either the old system or stock system to name the metal. Stock system has become the accepted norm. See part C below. B) The nonmetal (anion) is written last. Name it and change the ending to ide. C) For the following metals, use the proper naming scheme. (bold on the ion charge sheet) Old System Ion Stock System ferrous Fe +2 Iron (II) ferric Fe +3 Iron (III) cuprous Cu +1 Copper (I) cupric Cu +2 Copper (II) plumbous Pb +2 Lead (II) plumbic Pb +4 Lead (IV) stannous Sn +2 Tin (II) stannic Sn +4 Tin (IV) nickellous Ni +2 Nickel (II) nickellic Ni +3 Nickel (III) cobaltous Co +2 Cobalt (II) cobaltic Co +3 Cobalt (III) mercuric Hg +2 Mercury (II) mercurous +1 Hg 2 Mercury (I) *polyatomic ion 2) Ternary Ionic Compounds metallic ions with polyatomic ions Same as in #2 name the positive ion first and then give the name of the polyatomic ion. examples: FeO is ferrous oxide or Iron (II) oxide Fe 2 O 3 is ferric oxide or Iron (III) oxide Al 2 (SO 4 ) 3 is aluminum sulfate 3) Acids/Hydrogen compounds Ca(OH) 2 is calcium hydroxide SrCl 2 is strontium chloride There are two ways to name acids or hydrogen compounds depending on if they are dry or in solution with water (which makes them acids). Note: these are compounds where hydrogen has the positive oxidation number. In some cases (metals with hydrogen), hydrogen has a negative oxidation number and is written last. These would be named according to the ionic rules. Ex: KH is potassium hydride. Binary compounds Dry name: Hydrogen -ide. Put the name of the atom with the negative oxidation number in the blank and change the ending to ide. Prefixes are usually not used, since the number of hydrogen atoms attached to the negative atom should always be easy to determine. Acid name: Hydro -ic. The name of the atom with the negative oxidation number again goes in the blank with the ending changed to ic. Ex: HCl dry name: hydrogen chloride. acid name: hydrochloric acid. Ternary compounds Dry name: just like ionic names hydrogen and then the polyatomic ion. Acid name: depends on the ending of the polyatomic ion. If the polyatomic ending is ate, then the acid name is -ic, leaving the hydrogen off altogether. If the polyatomic ending is ite, the acid name is -ous, leaving the hydrogen off altogether. Ex: H 2 SO 4 is hydrogen sulfate (dry name) which becomes sulfuric acid in water. H 2 SO 3 is hydrogen sulfite or sulfurous acid.

10 SOLUBILITY RULES 1. Salts of ammonium (NH 4 + ) and Group IA are always soluble. 2. a. All chlorides (Cl - ) are soluble except AgCl, Hg 2 Cl 2, and PbCl 2 which are insoluble. b. All bromides (Br - ) are soluble except AgBr, Hg 2 Br 2, HgBr 2, and PbBr 2 which are insoluble. c. All iodides (I - ) are soluble except AgI, Hg 2 I 2, HgI 2, and PbI 2 which are insoluble. 3. Chlorates (ClO 3 - ), nitrates (NO 3 - ), and acetates (CH 3 COO - ) are soluble. 4. Sulfates (SO 4 ) are soluble except CaSO 4, SrSO 4, BaSO 4, Hg 2 SO 4, HgSO 4, PbSO 4, and Ag 2 SO 4 which are insoluble. 5. Phosphates (PO 4-3 ), and carbonates (CO 3 ) are insoluble except NH 4 + and Group IA compounds. 6. All metallic oxides (O ) are insoluble except NH 4 + and Group IA compounds. 7. All metallic hydroxides (OH - ) are insoluble except NH 4 + and Group IA and Group IIA from calcium down. 8. All sulfides (S ) are insoluble except NH 4 + and Groups IA and IIA.

11 Some Rules for Assigning Oxidation Numbers rule examples 1. Neutral substance that contains atoms of only one element = 0 H2, Na, Cl2 2. Monatomic ions = charge on the ion Fe 2+, Zn 2+, Br - 3. Fluorine always = NaF, ClF3 4. Group IA elements (except H) always = +1 NaCl, KCl 5. Group IIA elements always = +2 MgCl2, CaSO4 6. Group VIIA elements often = BCl3, NaI 7. Oxygen usually =, except in: H2O a. peroxides (contain the O2 2- group) = H2O2 b. superoxides (contain the O2 - group) = /2 KO2 8. Hydrogen can be either +1 or 1: a. when bonded to a metal = NaH b. when bonded to a nonmetal = +1 HCl 9. Sum of oxidation numbers of atoms in molecule = charge on molecule Hints: First, identify the atoms that always have a particular oxidation number. Use rule 9 to calculate the oxidation numbers for atoms which are not described by this set of rules. Oxidation numbers are usually written with the sign followed by the magnitude this is opposite to the way charges on ions are written (magnitude followed by sign).