AP CHEMISTRY. Summer Assignment

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1 AP CHEMISTRY Summer Assignment Welcome to AP Chemistry! In order to have a smooth transition, students are expected to come in with some strong background knowledge. These are some of the things you need to be able to do: 1. Factor Labeling: You need to be able to show proper work for the AP exam. Attached you will find a sheet that shows the conversion factors that you need to have memorized by the first day of school. 2. Ions: You need to memorize the AP list of ions that is attached. Hopefully, you know many of these ions already from your first year chemistry course. You need to be able to write the formulas of ionic compounds using the charges. 3. Solubility Rules: You need to memorize the general solubility rules that are attached. These rules will allow you to predict whether a precipitate will form during a double replacement reaction. These rules are extremely important to your success in AP Chemistry! 4. Oxidation Numbers: You should be able to determine the oxidation number of an element in a molecule or polyatomic ion. The general rules are attached. 5. Don t forget Avogadro s number! There will be a big quiz during the first week of school covering these topics. Attached you will find a practice quiz that will help you gauge your preparedness. Don t take the practice quiz until the month of August starts. Enjoy your summer. See you next year!

2 CONVERSION FACTORS Memorize these Conversion Factors Metric Prefixes Prefix Symbol Numerical Exponential giga G 1,000,000, mega M 1,000, kilo K 1, hecto H deka Da no prefix means: deci D centi C milli M micro nano N How to Use Metric Prefix Conversions Factors: 1 kilogram = 100 grams 1 centimeter = 0.01 meters 1 nanosecond = 10-9 seconds English System Conversion Factors Length Mass Volume 1 mile = 5280 ft. 1 ton = 2000 lb. 1 gallon = 4 quarts 1 yd. = 3 ft. 1 lb. = 16 oz. 1 quart = 2 pints 1 ft. = 12 in. 1 pint = 2 cups Converting between Different Systems Dimension Primary Conversion Secondary Conversion Length 1 inch = 2.54 cm 1 mile = 1609 meters Mass 1 lb. = 454 grams 1 oz. = grams Volume 1 gallon = 3.78 liters 1 tsp. = 4.93 ml Temperature K = o C o F = (9/5) o C + 32 *** The secondary conversions for length and temperature should also be memorized.

3 Commit to Memory Commons Ions and their Charges Monatomic Cations Name Monatomic Anions Name H +1 Hydrogen H Hydride Li +1 Lithium F Fluoride Na +1 Sodium Cl Chloride K +1 Potassium Br Bromide Mg +2 Magnesium I Iodide Ca +2 Calcium O 2 Oxide Ba +2 Barium S 2 Sulfide Al +3 Aluminum N 3 Nitride Ag +1 Silver P 3 Phosphide Zn +2 Zinc Other Monatomic Cations Name Polyatomic Ions Name Cu +1 Copper (I) +1 NH 4 Ammonium Cu +2 Copper (II) NO 2 Nitrite Fe +2 Iron (II) NO 3 Nitrate Fe +3 Iron (III) 2 SO 3 Sulfite Sn +2 Tin (II) 2 SO 4 Sulfate Sn +4 Tin (IV) OH Hydroxide Pb +2 Lead (II) 3 PO 4 Phosphate Pb +4 Lead (IV) 2 CO 3 Carbonate Cr +2 Chromium (II) ClO 4 Perchlorate Cr +3 Chromium (III) ClO 3 Chlorate Mn +2 Manganese (II) ClO 2 Chlorite Mn +4 Manganese (IV) ClO Hypochlorite +2 Hg 2 Mercury (I) C 2 H 3 O 2 Acetate Hg +2 Mercury (II) 2 CrO 4 Chromate 2 Cr 2 O 7 Dichromate CN Cyanide MnO 4 HCO 3 2 O 2 SCN Permanganate Bicarbonate Peroxide Thiocyanate

4 Rules for Determining Oxidation Number Memorize These Rules Oxidation Number: A number assigned to an atom in a molecular compound or polyatomic ion that indicates the general distribution of electrons among the bonded atoms. 1. The oxidation number of any neutral element is ZERO. 2. The oxidation number of a monatomic ion equals the charge on the ion. 3. The more electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion. 4. The oxidation number of fluorine in a compound is always Oxygen has an oxidation number of -2 unless it is combined with F, when it is +2, or it is in a peroxide, when it is The oxidation state of hydrogen is +1 unless it is combined with a metal, in which case it is In compounds, the elements of groups 1 and 2 as well as aluminum have oxidation number of +1, +2, and +3, respectively. 8. The sum of the oxidation numbers of all atoms in a neutral compound is ZERO. 9. The sum of the oxidation number of all atoms in a polyatomic ion equals the charge of the ion. RULES FOR NAMING ACIDS Memorize These Rules 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 Cl- is the Chloride ion so HCl = hydrochloric acid 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 ClO2-1 is the Chlorite ion so HClO2 = Chlorous acid. 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 ClO3-1 is the Chlorate ion so HClO3 = Chloric acid.

5 SOLUBILITY RULES Memorize These Rules Compounds containing Generally are Exceptions include those of Alkali metals Soluble None Ammonium Soluble None Nitrate, Acetate, Chlorate Soluble None Compounds containing Generally are Exceptions include those of Chloride, Bromide, Iodide Soluble Lead(II), Silver, Mercury(I) Sulfate Soluble Lead(II), Silver, Mercury(I), Calcium, Strontium, Barium Compounds containing Generally are Exceptions include those of Hydroxide Insoluble Alkali metals, Calcium, Strontium, Barium Carbonate, Phosphate, Chromate Insoluble Ammonium, Alkali metals Lead(II) is Pb +2 Mercury(I) is Hg2 +2 Common Student Misconceptions 1. Like always dissolves like. This is only a generalization and there are exceptions. For example, acetic acid is totally miscible in water, and also miscible in nonpolar solvents like benzene and carbon tetrachloride. 2. The solubility of a solid in a liquid increases with increasing temperature. This is not always true. For example, sodium sulfite, calcium acetate, and lithium sulfate have solubilities that decrease with an increase in temperature. 3. Insoluble compounds do not dissolve. This is not really true. All ionic compounds, even those we classify as insoluble dissolve to some slight extent in water.

6 GENERAL SOLUBILITY RULES FOR IONIC COMPOUNDS 1. Most alkali metal compounds and ammonium compounds are soluble in water. 2. Most nitrates, acetates, and chlorates are soluble in water. 3. Most chlorides, bromides, and iodides are soluble, except those of silver, lead(ii), and mercury(i). 4. Most sulfates are soluble, except those of calcium, barium, strontium, silver, lead (II) and mercury(i). 5. Most hydroxides are insoluble, except those of alkali metals, ammonium, calcium, barium, and strontium. 6. Most carbonates and phosphates are insoluble, except those of alkali metals and ammonium.

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8 AP Chemistry Summer Assignment / Practice Quiz Name Solve the following problems showing all work using factor-labeling. Pay attention to sig figs! 1. The recommended adult dose of Elixophyllin, a drug used to treat asthma, is 6 mg/kg of body mass. Calculate the dose in milligrams for a 150. lb. person. 2. If an automobile is able to travel 254 mile on 11.2 gallons of gasoline, what is the gas mileage in km/l? 3. A pound of coffee beans yields 50.0 cups of coffee. How many milliliters of coffee can be obtained from a 1.00 gram of coffee beans? 4. What is the engine displacement in liters of an engine whose displacement is listed as 450. in. 3? 5. The density of air at ordinary atmospheric pressure and 25.0 o C is 1.19 g/l. What is the mass, in kilograms, of the air in a room that measures 12.5 x 15.5 x 8.00 ft? 6. Automobile batteries contain sulfuric acid, which is commonly referred to as battery acid. Calculate the number of grams of sulfuric acid in L of battery acid, if the solution has a density of 1.28 g/ml and is 38.1% sulfuric acid by mass.

9 Name the following ionic compounds. 7. MgO 8. AlCl 3 9. Li 3 PO Ba(ClO 4 ) Cu(NO 3 ) Fe(OH) Ca(C 2 H 3 O 2 ) Cr 2 (CO 3 ) K 2 CrO (NH 4 ) 2 SO 4 Write the chemical formulas for the following compounds. 17. Sodium phosphate 18. zinc nitrate 19. barium bromate 20. iron (II) perchlorate 21. cobalt (II) bicarbonate 22. Chromium (III) acetate 23. Potassium dichromate 24. Calcium hydroxide 25. Copper (I) oxide 26. Mercury (II) bromide

10 Fill in the following solubility rules table. Always Soluble Ion Exceptions Usually Soluble Ion Exceptions Usually Insoluble Ion Exceptions

11 Identify each of the following as soluble or insoluble. 27. PbSO Na 3 PO KClO SrSO Ba(NO 3 ) AgNO MgCO Mg(C 2 H 3 O 2 ) K 2 SO AgCl Write the balanced net ionic equations for the following. 37. Aqueous sodium carbonate and aqueous calcium nitrate are mixed. 38. Aqueous barium hydroxide and aqueous sodium carbonate are mixed. 39. Aqueous ammonium sulfate and aqueous barium chloride are mixed. 40. Aqueous sodium chloride and aqueous calcium bromide are mixed.

12 Oxidation Numbers Practice 1. What is the oxidation number of hydrogen in each of the following species? a. H 2 O d. NaH b. HCl e. H 2 c. HClO 3 f. NH 3 2. Determine the oxidation number of -2 a. S in SO 3-2 b. S in SO 4 d. Cr in Cr 2 O 7-2 e. Cu in Cu 2 O c. S in SO 2 f. O in H 2 O 2

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