AP Chemistry Summer Assignment Instructions
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Mr. Lin AP Chemistry Summer Assignment Instructions AP Chemistry AP Chemistry AP Chemistry AP Chemistry AP Chemistry AP Chemistry Silently challenge everything. This does not mean in a contemptuous manner. Challenge your own understanding in your mind. Take on a healthy dose of skepticism without being a cynic. Find insight about your own thinking and improve upon it. Three assignments will be due on the first day of class: Part I, Part II, and Part III Part I 1. Purchase the required text. (Chemistry 8th Ed, Zumdahl) 2. Complete the following: ! Read and outline Ch 1 Ch 1 Problems (26-28, 31, 37, 38, 40, 43, 47, 54, 59, 60, 64, 66, 72, 75, 77, 78, 81, 82, 85, describe distillation, filtration, chromatography) ! Read and outline Ch 2 Ch 2 Problems (32, 35, 40, 47-49, 51, 53, 56, 57, 59, 63, 71, 75, 79, 93, 109, 110) ! Read and outline Ch 3.1-3.2 Ch 3a Problems (23, 36, 37, 39) Part II Included in the packet are the following handouts: common ions, naming compounds flow chart, solubility rules, and naming and solubility worksheet 1. Memorize the names, formulas, and charges of common ions. 2. Memorize the naming compounds flow chart. 3. Memorize the solubility rules. 4. Complete the solubility and naming compounds worksheet. Note: Take time to memorize this information. Do NOT procrastinate. (Procrastination is a five syllable word for sloth.) Flashcards are useful. Knowing this information will make the rest of the year easier. The AP Test is written with the expectation that this information has been memorized. You will be quizzed on the ions, naming compounds, and solubility rules the second day of class. Part III Respond to the following prompts: 1. WHY do chemical bonds form? (five sentence minimum) 2. Explain how ionic compounds form and how molecular compounds form. Be sure to include the words “stable” and “neutral” and use specific examples. Then discuss the similarities and differences between the two types of compounds. (five sentence minimum) 3. Describe everything that you understand about the periodic table. (five sentence minimum) 4. Describe the historical development of the atomic model by describing the Thomson cathode ray experiment, Rutherford gold foil experiment, and the modern view. (ten sentences) Have a great summer! God bless. Names, Formulas, and Charges of Common Ions Positive Ions (Cations) 1+ 2+ 3+ Ammonium Cesium Gold Silver NH4+ Cs+ Au+ Ag+ Nickel(II) Zinc Ni 2+ Zn2+ Copper (I) Cu+ ! Copper(II) Cobalt(II) Chromium(II) Iron(II) Lead(II) Manganese(II) Mercury(II) Tin(II) Cu2+ Co2+ ! Cr2+ ! Fe2+ ! Pb2+ ! Mn2+ ! Hg2+ Sn2+ ! Mercury(I) Hg22+ ! 4+ Antimony(III) Arsenic(III) Bismuth(III) Boron(III) Titanium Sb3+ As3+ Bi3+ B3+ Ti3+ Cobalt(III) Chromium(III) Iron(III) Co3+ Cr3+ Fe3+ Lead(IV) Pb4+ Manganese(IV) Mn4+ Sn4+ Tin(IV) Negative Ions (Anions) 1Acetate Hypochlorite Chlorite Chlorate Perchlorate Nitrite Nitrate Carbide Hydride Cyanide Hydroxide Thiocyanate Permanganate Dihydrogen phosphate Hydrogen oxalate Hydrogen carbonate Hydrogen sulfide Hydrogen sulfite (Bisulfite) Hydrogen sulfate (Bisulfate) 2C 2H 3O 2ClOClO2ClO3ClO4NO2NO3C22HCNOHSCNMnO4- Silicate Peroxide Chromate Dichromate 3SiO32O22CrO42Cr2O72- H2PO4- ! HC2O4- ! HCO3- ! HS- ! HSO3- ! Hydrogen phosphate Oxalate Carbonate Sulfide Sulfite HPO42- ! C2O42CO32S2SO32- HSO4- ! Sulfate SO42- Arsenate Borate Nitride AsO43BO33N3- Phosphide Phosphite P3PO33- Phosphate PO43- ! ! ! ! Li+! ! ! ! N3'! O2'! F'! ! Na+! Mg2+! ! Al3+! ! ! S2'! Cl'! ! K +! Ca2+! ! ! ! Cr2+! Cr3+! Mn2+! Mn3+! Fe2+! Fe3+! Co2+! Co3+! ! Cu+! Cu2+! Zn2+! ! ! ! ! Br'! ! Rb+! Sr2+! ! ! ! ! ! ! ! ! Ag+! Cd2+! ! Sn2+! Sn4+! ! ! I'! ! Cs+! Ba2+! ! ! ! ! ! ! ! ! ! Hg2!2+! Hg!2+! ! Pb2+! Pb4+! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! Naming Compounds Flow Chart Does the Formula begin with H NO YES Does it begin with a metal which has more than one oxidation number? (e.g.; Fe, Ni, Cu, Sn, Hg) NO YES It is an Acid (must be aqueous) Does the acid contain a polyatomic ion? Name the first element followed by its oxidation number (Roman numeral) YES NO Ending of polyatomic ion Does the formula contain a polyatomic ion? NO -ite YES Are both elements nonmetals? NO -ate YES Name the first element, Then the second element With the –ide ending. Name the first element using the proper prefix. (never mono-). Name the second element with the proper prefix (including mono- and –ide ending. 1 mono2 di3 tr4 tetra5 penta6 hexa7 hepta8 octa9 nano10 decaName the first element, then the polyatomic ion. If two elements are present, name both, then the polyatomic ion. (e.g.; NaHCO3 Is sodium hydrogen carbonate) Name the polyatomic ion, replacing the –ate ending with –ic. Add the word acid. Name the polyatomic ion, replacing the –ite ending with –ous. Add the word acid. Write the prefix hydro, then the name of the second element with –ic ending. Add the word acid. Soluble Compounds Exceptions All salts of Na+, K+, and NH4+ All salts of Cl-, Br-, and I- ! Halides of Ag+, Hg22+, and Pb2+ Compounds containing F- ! Fluorides of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ ! Sulfates of Sr2+, Ba2+, Pb2+ Salts of Nitrate, NO3Chlorate, ClO3Perchlorate, ClO4Acetate, CH3COOSalts of Sulfate, SO42- Insoluble Compounds Exceptions All salts of Carbonate, CO32Phosphate, PO43Oxalate, C2O42Chromate, CrO42Sulfide, S2Most metal hydroxides and oxides, OH- and O2- ! Salts of NH4+ and the alkali metal cations (Group I) Mr. Lin Name Per _____ Solubility and Naming Compounds AP Chemistry AP Chemistry AP Chemistry AP Chemistry AP Chemistry AP Chemistry Name the following compounds from their formula: 1. NH4I 2. Fe2(SO3)3 3. H3PO4 (aq) 4. AgClO3 5. SnC2O4 6. NaCN 7. Zn(OH)2 8. Rb2SiO3 9. MnO2 10. H2O2 11. KCl 12. KC2H3O2 13. CaSO4 14. Sb2(Cr2O7)3 15. Li3P Write the chemical formula from the compounds name: 1. Lead (IV) Carbonate 2. Magnesium Fluoride 3. Cesium Arsenate 4. Boron (III) Silicate 5. Francium Nitrite 6. Cobalt (II) Chloride 7. Mercury (I) Permanganate 8. Mercury (I) Fluoride 9. Barium Phosphate 10. Bismuth (III) Hydride 11. Aluminum Borate 12. Gold Oxide 13. Copper (I) Hypochlorite 14. Tin (II) Chlorite 15. Phosphorous Pentachloride Solubility Directions: Two beakers are filled with 250 ml of water. Determine if the following compounds will dissolve in each beaker and if a precipitate will form through double displacement if both beakers are mixed. Write the proper molecular equation. (aq) = aqueous ! soluble (s) = solid ! insoluble Examples: NaCl, NH4NO3 NaCl (aq) + NH4NO3 (aq) ! NaNO3 (aq) + NH4Cl (aq) no reaction SOLUBLE SOLUBLE SOLUBLE SOLUBLE BaNO3, NaSO4 BaNO3 (aq) + Na2SO4 (aq) ! BaSO4 (s) + NaNO3 (aq) precipitate SOLUBLE SOLUBLE INSOLUBLE SOLUBLE AgCl, NaC2H3O2 AgCl (s) + NaC2H3O2 (aq) ! no reaction INSOLUBLE SOLUBLE Beaker 1/ Beaker 2 1) NaCl, Ba(NO3)2 2) SrSO4, NH4ClO4 3) NaCl, AgNO3 4) Au2CO3, PbSO4 5) Ag2S, HCH3CO2 6) Cs2SO4, SrCl2 7) Fe2O3, (NH4)3P 8) CaF2, MgBr2 9) Ag2SO4, PbI2 10) (NH4)2CO3, NaI
