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Instructions for AP/IB 2 Chem Summer Assignment Note: Future AP/IB chemistry students are expected to learn the material in this packet before class starts in the fall. Most of this is a review of names, formulas and reactions that were learned in pre-AP/IB chemistry. Since this class is AP and IB chemistry combined, there will not be enough time to review this material in class. Study the examples before completing the questions. For more detailed information, download the chemical reactions power point from my webpage (AP/IB 2 chemistry). Or go back and review your Chem I notes on ionic bonding, covalent bonding and chemical reactions. This assignment will count as a major grade and is due the second day of class. It will be spot checked for correctness (i.e. it’s not just a completion grade; it will be scanned and points deducted for things that are obviously not even close to the correct answer). AP/IB 2 Chemistry: Summer Assignment Name_______________________ Memorize these element names and symbols: H= hydrogen He = helium Li = lithium Be = beryllium B = boron C = carbon N = nitrogen O = oxygen F = fluorine Ne = neon Na =sodium Mg = magnesium Al = aluminum Si = silicon P = phosphorus S = sulfur Cl = chlorine Ar = argon K = potassium Ca = calcium Sc = scandium Ti = titanium V = vanadium Cr = chromium Mn = manganese Fe = iron Co = cobalt Ni = nickel Cu = copper Zn = zinc As = arsenic Se = selenium Br = bromine Kr = krypton Rb = rubidium Sr = strontium Pt = platinum Ag = silver Cd = cadmium Sb = antimony I = iodine Xe = xenon Cs = cesium Ba = barium Au = gold Hg = mercury Sn = tin Pb = lead Rn = radon Ra = radium U = uranium Pu = plutonium Bi = bismuth Memorize these ion oxidation numbers: A groups: generally metals are cations (+) and nonmetals are anions (-) Group # 1 A (alkali metals) 2 A (alkaline earth metals) 3A 4A 5A 6A 7 A (halogens) 8 A (noble gases) Oxidation # +1 +2 +3 +4 or -4 (depends) -3 (except Bi5+) -2 -1 No ions; no compounds examples Li+, Na+, K+ Mg2+, Ca2+, Ba2+ Al3+, Ga3+, In3+ C4+, C4names end in –ide N3-, P3-, As3O2-, S2-, Se2Ex: oxide, chloride F-, Cl-, Br-. I- B groups (and tin and lead): Transition metals; most have multiple oxidation numbers Ag+, Zn2+ , Cd2+ , Ni2+, Ni3+ Hg+, Hg2+, Cu+, Cu2+ Mn2+, Mn3+, Mn4+, Mn7+ Fe2+, Fe3+, V2+, V3+, V4+, V5+ +2 is most common Co2+, Co3+, Cr2+, Cr3+, Cr6+ Pb2+, Pb4+, Sn2+, Sn4+ Polyatomic ions (Memorize these!): NO3- = nitrate CN- = cyanide MnO4- = permanganate NO2- = nitrite SCN- = thiocyanate IO3- = iodate BrO3- = bromate SO42- = sulfate HSO4- = hydrogen sulfate S2O32- = thiosulfate NH4+ = ammonium (bisulfate) SO32- = sulfite HSO3- = hydrogen sulfite C2O42- = oxalate OH- = hydroxide (bisulfite) PO43- = phosphate HPO42- = hydrogen phosphate CO32- = carbonate PO33- = phosphite H2PO4- = dihydrogen phosphate HCO3- = hydrogen carbonate (bicarbonate) - ClO3 = chlorate - ClO2 = chlorite - 2- ClO4 = perchlorate CrO4 = chromate - Cr2O72- = dichromate ClO = hypochlorite C2H3O2- or CH3COO- acetate or ethanoate Determining the formula of a compound: I. Ionic Compounds (have a metal and a nonmetal). Use the oxidation numbers to put the ions together in the correct lowest whole number ratio. Ex: sodium oxide iron (III) chloride zinc sulfate aluminum hydroxide Na+ and O2- = Na2O Fe3+ and Cl- = FeCl3 (roman numeral III means +3) Zn2+ and SO42- = ZnSO4 Al3+ and OH- = Al(OH)3 use ( ) if 2 or more of polyatomic ion • You try; write the formula 1. ______________ sodium phosphate 2. ______________ ammonium bromide 3______________ lead (II) nitrate 4.______________ silver sulfide 5.______________ calcium carbonate 6. ______________ potassium dichromate II. Covalent Compounds (have 2 nonmetals; no ions; atoms share electrons) Use the prefixes to determine the number of atoms (1= mono, 2 = di, 3 =tri, 4 tetra, 5= penta, 6 = hexa) Ex: carbon tetrachloride = CCl4 dinitrogen tetroxide = N2O4 • You try; write the formula 7.__________ carbon dioxide 8.___________ diphosphorus pentoxide 9.__________ sulfur hexafluoride 10.___________ sulfur trioxide III. Acids (have H+ with an anion) put the ions together like the ionic ones. There are 6 strong acids (these dissociate completely in aqueous solution; ex: HCl exists as H+ and Cl- ions, not as molecules) Memorize the six strong acids: HCl, HBr, HI, HNO3, H2SO4, HClO4 All others are weak! (dissociate only slightly into ions) Ex: hydrochloric acid: H+ and Cl- = HCl hydro…..ic has the –ide ion (strong) nitric acid; H+ and NO3- = HNO3 -ic has –ate ion (strong) nitrous acid + - H and NO2 = HNO2 -ous has the –ite ion (weak) • You try; write the formula and indicate if weak or strong 11. _____________ acetic acid (ethanoic) 12._____________ hydrofluoric acid 13._____________ carbonic acid 14._____________ hypochlorous acid 15._____________ perchloric acid 16._____________ sulfuric acid Naming Compounds I. Ionic: Name the metal, then the nonmetal; change the ending to –ide, -ite, or –ate depending on the identity of the anion. Indicate the oxidation number if it has one of the metals with more than one oxidation number. Ex: KI = potassium iodide Al2O3 = aluminum oxide Ag2SO3 = silver sulfite (NH4)2Cr2O7 = ammonium dichromate CuCl2 = copper(II) chloride Fe3(PO4)2 = iron(II) phosphate • You try; name the compound 17._________________________ ZnO 18.________________________ KMnO4 19._________________________ NaClO3 20.________________________ NH4OH 21._________________________ LiH2PO4 22.________________________ PbSO4 23.__________________________ AlBr3 24.______________________ Ba(C2H3O2)2 25.__________________________SnCl4 25._______________________ Cu(NO3)2 26.__________________________ CdS 27.______________________ SrCrO4 28.___________________________ CaC2O4 29.______________________ NaCN II. Covalent Compounds (Binary compounds: 2 nonmetals) Use prefixes to indicate the number of atoms (don’t use mono on the first element) Prefixes: mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca Ex: SiF4 = silicon tetrafluoride 30. ________________________ CO 32._________________________ N2O4 ending is -ide S2Cl2 = disulfur dichloride 31.____________________________ PCl3 33.____________________________ CS2 Types of Chemical Equations: Writing Chemical Reactions Learn the general formula for each type of reaction. If the reaction occurs in water solution, you must give the net ionic equation. If it doesn't occur in aqueous solution, the atoms/molecules do not exist as ions. Writing the net ionic equation (water solution only!) 1. First memorize the six strong acids and solubility rules for salts (ionic compounds). Strong Acids hydrochloric, hydrobromic, hydroiodic, sulfuric, nitric, perchloric these are completely dissociated into ions so write them as separated ions: ex: HCl is really H+ and Cl- HNO3 is really H+ and NO3- do not write weak acids like this! acetic acid stays as HC2H3O2 Solubility Rules i) soluble salts: all nitrates, acetates, alkali metals compounds and ammonium compounds are always soluble (no exceptions). ii) insoluble salts: compounds of lead, silver, cadmium and mercury (except those trumped by rule i ) iii) Compounds of calcium, barium, strontium and transition metals are insoluble except halides (and those trumped by rule i) These three rules don't cover every possible compound, but they include most compounds that appear on the AP or IB test. So write soluble compounds as separated ions. Insoluble compounds precipitate from the solution as a solid. Do not separate the ions for a solid. ex: calcium nitrate, Ca(NO3)2 is soluble so it exists as Ca2+ and 2 NO3- in solution lead (II) hydroxide is insoluble so keep it as Pb(OH)2 2. Write the complete equation predicting the products. 3. Cancel the spectator ions. These are ions that are unchanged (must be exactly the same form on both sides of the equation. 4. Balance the equation using lowest whole number coefficients. Double Replacement Reaction: AB + CD → AD + CB (occurs in solution always) Ex: aqueous solutions of silver nitrate and sodium carbonate are mixed. Ag+ + NO3- + Na+ + CO32- → Ag2CO3 + Na+ + NO3- silver carbonate is insoluble sodium nitrate is soluble net ionic: 2 Ag+ + CO32- ---> Ag2CO3 sodium and nitrate are spectator ions; they cancel out and should not appear in the answer Ex: aqueous solutions of barium chloride and copper(II) sulfate are mixed Ba2+ + Cl- + Cu2+ + SO42-→ BaSO4 + Cu2+ + Cl- barium sulfate is insoluble copper(II) chloride is soluble net ionic: Ba2+ + SO42- ---> BaSO4 copper and chloride are spectator ions Ex: 1-molar hydrochloric acid is neutralized by an equal volume of 1-molar potassium hydroxide H+ + Cl- + K+ + OH- → K+ + Cl- + H2O potassium chloride is soluble; water is not an ionic compound (not made of ions) leave it intact net ionic: H+ + OH----> H2O potassium and chloride are spectator ions • You try: Write the net ionic equation for these double replacement reactions: 34. A solution of lead(II) nitrate is added to a solution of sodium iodide. 35. Solutions of calcium acetate (ethanoate) and lithium phosphate are mixed 36. Equal volumes of equimolar nitric acid and sodium hydroxide solutions are mixed 37. A few drops of aqueous nickel (II) nitrate are added to a solution of sodium sulfide 38. Some acetic acid (ethanoic acid) is added to sodium hydroxide solution. Single Replacement Reaction: A + BC → AC + B or BA + C these occur in aqueous solution so give the net ionic form. Ex: a piece of zinc metal is placed in a solution of copper(II) sulfate Zn + Cu2+ + SO42- → Zn2+ + SO42- + Cu zinc sulfate is soluble copper product is solid, metallic copper net ionic: Zn + Cu2+ → Zn2+ + Cu sulfate is a spectator ion; don't cancel the solid metal and its dissolved ion (they are different forms) Ex: chlorine gas is bubbled through a solution of lithium bromide Cl2 + Li+ + Br-→ Br2 + Li+ + Cl- lithium chloride is soluble chlorine gas and elemental bromine are both diatomic (HOBrFINCl) elements net ionic: Cl2 + 2 Br- ---> Br2 + 2 Cl- lithium ions are spectator ions Ex: a piece of magnesium metal is added to a solution of sulfuric acid Mg + H+ + SO4- → Mg2+ + SO42- + H2 magnesium sulfate is soluble net ionic : Mg + 2 H+ ---> Mg2+ + H2 sulfate is spectator; can't cancel solid magnesium metal with dissolved magnesium metals displace hydrogen from an acid. ion ! hydrogen gas is diatomic Ex: sodium metal reacts with water Na + H2O → NaOH + H2 sodium hydroxide is soluble; net ionic: Na + 2 H2O ----> Na+ + 2 OH- + H2 alkali metals and alkaline earth metals react with water to form hydrogen gas. This is why sodium explodes in water. • You try: Write the net ionic equation for these single replacement reactions 39. A piece of copper wire is placed in a test tube containing silver nitrate solution. 40. Elemental bromine is added to a solution of potassium iodide. 41. Zinc metal is placed in a solution of hydrochloric acid. 42. Calcium metal is added to water. 43. A piece of nickel metal is placed in a solution of copper(II) nitrate 44. A small piece of potassium metal is dropped in a beaker of water. 45. Magnesium metal reacts with a solution of acetic acid (ethanoic acid) Synthesis Reaction: A + B → AB usually do not occur in water solution don't need the net ionic form Ex: A piece of aluminum metal is dropped into a container of iodine vapor. 2 Al + 3 I2 → 2 AlI3 iodine is diatomic; if metal with nonmetal, use oxidation numbers to get the ionic compound formula Ex: Sulfur trioxide gas is streamed into a flask containing calcium oxide SO3 + CaO → CaSO4 two simple compounds make a more complex compound; make sure the product is an actual compound Ex: Nitrogen gas reacts with hydrogen gas in the presence of an iron catalyst Fe 3 H2 + N2 → 2 NH3 The Haber Process (know this one by heart!) Ex: Carbon dioxide gas is bubbled through water CO2 + H2O → H2CO3 nonmetal oxides always react with water to make an acid Ex: Magnesium oxide is added to water MgO + H2O → Mg(OH)2 metal oxides react with water to make a base net ionic: MgO + H2O ----> Mg2+ + 2 OH- this is in water and magnesium hydroxide is slightly soluble • You try: Write balanced equations for these reactions 46. Calcium metal reacts with nitrogen gas 47. A piece of aluminum foil is added to a container of liquid bromine 48. Hydrogen gas reacts with chlorine gas 49 .Sulfur trioxide gas is bubbled through water 50. Solid calcium oxide is added to water 51. Elemental carbon combines with oxygen gas. Decomposition Reaction: AB → A + B usually do not occur in solution Ex: Mercury (II) oxide is heated. 2 HgO → 2 Hg + O2 Ex: Molten sodium chloride is electrolyzed 2 NaCl → 2 Na + Cl2 Ex: Hydrogen peroxide decomposes in the presence of a manganese (IV) oxide catalyst. MnO2 2 H 2 O2 → 2 H 2 O + O 2 Know this reaction !! Ex: Calcium carbonate is heated CaCO3 → CaO + CO2 metal carbonates decompose into the metal oxide and carbon dioxide gas Ex: Sodium chlorate is heated 2 NaClO3 → 2 NaCl + 3 O2 metal chlorates decompose into the metal chloride and oxygen gas Ex: Hydrochloric acid solution is added to solid sodium bicarbonate HCl + NaHCO3 → NaCl + H2CO3 this occurs in solution so need net ionic form H+ + Cl- + NaHCO3 → Na+ + Cl- + H2O + CO2 this reaction is double replacement and decomposition; carbonic acid sodium bicarbonate is a solid (not dissolved) breaks down into water and carbon do not separate a solid into ions dioxide. net ionic: H+ + NaHCO3 ---> Na+ + H2O + CO2 • You try: Write reactions for these decomposition reactions. 53. Molten aluminum oxide is electrolyzed. 54. Electrolysis of water 55. Solid sodium carbonate is heated. 56. Solid potassium chlorate is heated. 57. A catalyst of potassium iodide is added to hydrogen peroxide 58. Several drops of nitric acid are added to solid calcium carbonate Combustion Reaction: CxHyOz + O2 → CO2 + H2O (complete; enough O2) when insufficient oxygen, it also produces CO and C You should know names and formulas of common organic compounds. See the power point on organic chemistry on my web page (on pre-AP chem tab) Ex: butane gas burns in an excess amount of oxygen 2 C4H10 + 13 O2 → 8 CO2 + 10 H2O Ex: Complete combustion of ethanol C2H5OH + 3 O2 → 2 CO2 + 3 H2O • You try: Write reactions for these combustion reactions: 59. Complete combustion of propane gas 60. Complete combustion of methanol