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AP CHEMISTRY SUMMER ASSIGNMENT 2012 MR. NILSEN Welcome to Advanced Placement Chemistry. AP Chem is a fast paced course, with higher orders of thinking. You will be expected to pull on previous knowledge constantly to solve problems. Along the way, we will see some fun demonstrations and perform some intense chemical experiments. The attached summer assignment is a recommended assignment, but will not be collected. I will field questions via email all summer (except the last week of August) at [email protected]. To aid you, you should read (and cover) the Brown and LeMay Chemistry the Central Science book. The assignment focuses on chapters 1,2,3 and chapter 10 up to, and including, section 10.6. You must also spend some time memorizing the common ion chart at the end of this packet. Also at the end of the assignment is a sheet of elements. You do not have to turn this sheet in, but you must learn the symbols and names of those elements. After this page is a page of common ions for reference, you are expected to know these ions for the AP test and thus for this course The packet is important, but more important is that you understand the material on this. As such you will be tested on each chapter. The test on chapters one and two will be on September 7th. On the 10th we will review chapter 3 and then on the 11th we will test on chapter 2. On the 12th we will review chapter 10, and then we will take the chapter 10 test on the 13th. Of course, these are tentative dates. Despite what you are thinking as you look this over, I am not trying to kill you. I am trying to ensure that you remember enough of your honors Chemistry course so that we can achieve the pace we need to make the AP Chemistry exam a success for everyone. Name ___________________________________ AP Chemistry Summer Assignment 2012 SIGNIFICANT FIGURES APPLY TO ALL NUMERIC ANSWERS. ALL NECESSARY WORK MUST BE SHOWN FOR QUANTITATIVE PROBLEMS. Unit 1 – Introduction to Matter and Measurement 1) Indicate whether the following substances are heterogeneous Mixtures, or homogeneous Solutions, Compounds, or Elements. Seawater ____ sand ____ platinum ____ orange juice ____ Italian salad dressing ____ Epsom salt (magnesium sulfate) ____ methanone _____ Brass alloy ____ europium _____ coca-cola _____ ammonia ____ 2) The best way to separate the components of a mixture would be: a) distillation b) filtration c) both distillation and filtration d) something else 3) The best way to separate the solute from the solvent of a solution would be: a) distillation b) filtration c) both distillation and filtration d) something else 4) Name these elements (try to do this without a book/periodic table): Au ________________ Mo ____________________ Sn _____________________ Pb ________________ Sb _____________________ Na _____________________ Fe ________________ K_______________________ W ______________________ 5) Write the chemical symbols for these elements (try to do this without a book/periodic table): fluorine _______ arsenic _______ plutonium _____ krypton _______ mercury _______ silver ______ copper ______ manganese ______ 6) Indicate whether the following are Chemical changes or Physical changes. corrosion of aluminum metal _____ melting of ice _____ pulverizing an aspirin _____ digesting a candy bar _____ 7) Write the following without scientific notation, using only metric prefixes. 6.5 x 10-6 m = __________________ 6.34 x 10-4 L = ____________________ 2.5 x 10-3 L = __________________ 4.23 x 10-9 m3 = ___________________ 12.5 x 10-8 kg = ___________________ 3.5 x 10-11 s = _____________________ 8) Convert the following: 25.5 mg = __________________ g 4.0 x 10-10 m = __________________ nm .575 mm = _________________ m 14.7 km = ______________________ cm 9) A liquid has a mass of 39.73 g and a volume of 25.0 ml. What is its density in g/cm3? Answer _________________________ 10) The density of platinum is 21.45 g/cm at 25 C. What is the mass of 75.00 ml of platinum at this temperature? 3 o Answer _________________________ 11) The density of titanium is 4.51 g/cm at 25 C. What is the volume of 175 g of titanium at this temperature? 3 o Answer _________________________ 12) Convert the following temperatures: 62 oF = _______ oC 216.7 oC = __________ oF 233 oC = __________ K 315 K = _______ oF 12.5 K = __________ oC 2500 oF = ___________ K 13) Perform the following conversions indicated. SHOW ALL WORK! 50.0 days = _____________ s 43 miler per hour = _______________ meters per second 13.8 g/cm3 = ______________ kg/m3 22.50 gal/min = _____________ liters/second 14) A certain silver dollar as a mass of 26.73 g and is 90.0% silver. If the value of silver is $5.30 per troy ounce, what is the current value of a dozen silver dollars? Answer _________________________ 15) A sample of ascorbic acid contains 1.50 grams of carbon and 2.00 grams of oxygen. Another sample of ascorbic acid contains 6.35 grams of carbon. How many grams of oxygen would this sample have? Answer _________________________ 16) The density of silver is 10.5 g/cm and the density of aluminum is 2.70 g/cm3. Two spheres of equal mass are constructed, one of silver and one of aluminum. The silver sphere has a radius of 12.0 cm. What is the radius of the aluminum sphere? Vsphere = 4/3r3 3 Answer _________________________ 17) Complete the following math using appropriate significant figures: 12.34 cm x 8.4 cm x 13.1 cm = ______________________ 187.245 ml + 43.1 ml + 391.55 ml = _____________________ (37 + 273.15 K) * 321 J/K = _______________________ 18) What is the difference between metric units and SI units? The test for unit one will include naming and writing symbols for elements. Unit 2 –Atoms, Molecules, and Ions 19) The radius of a krypton atom is about 1.9 Angstroms. a) How many krypton atoms would have to be lined up to span 1.0 mm? _____________ b) What is the volume of this spherical atom (in cm3)? ___________ 20) Complete the chart below: (only mass #s are given, you must look up the atomic #s) # of protons # of neutrons # of electrons 28 Si 60 Ni 195 Pt 238 U 21) Complete the chart for neutral atoms: 121 Symbol Sb Protons 38 94 Neutrons 50 108 Electrons 74 57 Mass # 139 239 22) From the data below, determine the average atomic mass of the given element. Isotope (Mass #) 203.97302 204.97444 206.97587 Abundance by % 1.40000% 24.10000% 22.10000% 207.97663 52.40000% 23) Indicate the formal family name to which each of the indicated elements belong: iodine _______________________ potassium _____________________ argon _______________________ strontium ______________________ tellurium _______________________ 24) Of the elements listed in question 21: (list them by their chemical symbols) a) which elements are metals? _____________________________________ b) which elements are nonmetals? ___________________________________ c) which elements are metalloids? ___________________________________ 25) A compound has two boron atoms and six hydrogen atoms. a) what is its empirical formula? ___________________ b) what is its molecular formula? ___________________ 26) How many hydrogen atoms are present in one molecule of: a) ethanol? _______ b) calcium acetate? ________ c) ammonium phosphate? _______ 27) Write the empirical formula for: a) Al2Br6 _____________ b) C8H10 _____________ d) P4O10 ______________ c) C4H8O2 _______________ e) C6H4Cl2 _____________ f) B3N3H6 _______________ 28) Based on its location in the periodic table, what is the most stable ion for: a) Al _______ b) Ca _______ c) S ________ d) I _________ e) Cs ______ 29) Based on their locations in the periodic table, write the formula of the ionic compounds formed between: a) gallium and fluorine ____________ b) lithium and iodine ____________ c) aluminum and oxygen ____________ d) magnesium and nitrogen ___________ 30) Name the following ionic compounds: a) AlF3 _______________________________ b) Fe(OH)2 ________________________________ c) Cu(NO3)2 ____________________________ d) Ba(ClO4)2 ______________________________ e) Li3PO4 _______________________________ f) Hg2S ___________________________________ g) Ca(C2H3O2)2 __________________________ h) Cr2(CO3)3 _______________________________ i) K2Cr2O7 _______________________________ j) NH4MnO4 _______________________________ 31) Write the chemical formulas for the following ionic compounds a) potassium chromate ___________________ b) magnesium chlorate __________________ c) iron (III) carbonate ___________________ d) tin (IV) sulfate ____________________ e) lead (IV) arsenate ____________________ f) antimony (V) perchlorate ________________ g) silver sulfide _____________________ h) barium nitrite _____________________ i) manganese (II) oxalate _________________ j) aluminum cyanide ___________________ 32) Name the following acids: a) HBr __________________________ b) HClO __________________________ c) H2CO3 _________________________ d) HCN ___________________________ e) H3AsO4 __________________________ f) HI ______________________________ 33) Write the formulas for the following acids: a) hydrofluoric _______________________ b) nitrous _________________________ c) bromic ___________________________ d) oxalic _________________________ e) phosphous ________________________ f) hydrochloric ______________________ 34) Write the formulas of the following binary covalent compounds: a) tetraphosphorus decoxide ______________ b) dinitrogen tetroxide __________________ c) sulfur trioxide _____________________ d) trinitrogen monoxide _________________ 35) Write the names of the following binary covalent compounds: a) SCl6 _____________________________ b) IBr5 _______________________________ c) XeF4 _____________________________ d) NO _______________________________ For the test on unit two, you will have to know your common ions. No charts will be provided. Unit 3 – Calculations with Chemical Formulas and Equations 36) Balance the following equations a) ____ P2O5 (s) + ____ H2O (l) ____ H3PO4 (aq) b) ____ CH4 (g) + ____ Cl2 (g) ____ CCl4 (l) + ____ HCl (g) c) ____ Al4C3 (s) + ____ H2O (l) ____ Al(OH)3 (s) + ____ CH4 (g) d) ____ C4H10O (l) + ____ O2 ____ CO2 + ____ H2O e) ____ Fe(OH)3 (s) + ____ H2SO4 (aq) ____ Fe2(SO4)3 (aq) + ____ H2O (l) 37) Write out the complete balanced equation for the reaction indicated. INCLUDE PHASES. a) Solid zinc metal reacts with sulfuric acid to produce hydrogen gas and a solution of zinc sulfate. b) When liquid phosphorus trichloride is added to water it reacts to form phosphous acid (sometimes called phosphorous acid) and hydrochloric acid. c) When gaseous phosphorus trihydride is combusted in air, water is formed as well as an insoluble solid tetraphosphorus decoxide. d) When solid mercury (II) nitrate is heated, it decomposes into solid mercury (II) oxide, gaseous nitrogen dioxide and oxygen. e) Copper metal reacts with sulfuric acid to form solid copper (II) sulfate, sulfur dioxide gas, and water. 38) Balance the following reactions, then indicate whether they are synthesis (S), decomposition (D), single replacement (SR), double replacement (DR), or combustion(C). a) ___ Mg + ___ AlF3 ___ MgF2 + ___ Al ____ b) ___ Cu(ClO3)2 ___ CuCl2 + ___ O2 ____ c) ___ NH3 + ___ O2 ___ NO2 + ___ H2O ____ d) ___ N4O10 + ___ H2O ___ HNO3 ____ e) ___ KI + ___ Fe2S3 ___ K2S + ___ FeI3 ____ 39) Determine the molar mass of: a) H2S _____________________ b) NiCO3 ______________________ c) (NH4)3AsO3 _____________________ d) Sb2(S2O3)5 ______________________ 40) Calculate the percentage (by mass) of oxygen in: a) sulfur dioxide ________________ b) ethanoic acid _________________ c) potassium phosphate _________________ d) aluminum nitrate ________________ e) dinitrogen pentoxide _______________ 41) Rank the following quantities from the one with the most atoms to the one with the least atoms: .500 mol of water 23.0 g of sodium 6.02 x 1023 nitrogen molecules ________________ most atoms __________________ ___________________ least atoms 42) Calculate the following quantities a) the mass, in grams, of 1.73 mol of calcium hydroxide __________________ b) the number of moles of magnesium nitrate in 6.50 grams of the substance ________________ c) the number of molecules in .775 moles of methanol _____________________ d) the number of hydrogen atoms in 1.24 mol butane _____________________ e) the number of electrons in 88.0 grams of carbon dioxide ______________________ 43) A sample of glucose, C6H12O6, contains 5.77 x 1020 atoms of carbon. a) How many atoms of oxygen are present? ___________________ b) What mass, in grams, of glucose does it contain? _________________ 44) Determine the empirical formula of a compound that contains: a) .0130 mol carbon, .0390 mol hydrogen, and .0065 mol oxygen ___________________ b) 11.66 g of iron and 5.01 g of oxygen ____________________ c) 40.0 % carbon, 6.7% hydrogen and 53.3% oxygen ____________________ d) 53.3% potassium, 14.6% phosphorus and 30.1% oxygen ____________________ e) 62.1% carbon, 5.21% hydrogen, 12.1% nitrogen, 20.7% oxygen ____________________ 45) Determine the empirical and molecular formula of a compound that contains: a) 49.5 % carbon, 5.15% hydrogen, 28.9% nitrogen and 16.5 % oxygen with a molar mass of 195 g/mol. Empirical formula = ___________________ Molecular Formula = _______________________ b) 57.14 % carbon, 6.16% hydrogen, 9.52% nitrogen, and 27.18 % oxygen with a molar mass of 276 g/mol. Empirical formula = ___________________ Molecular Formula = _______________________ c) 59.0 % carbon, 7.1% hydrogen, 7.7% nitrogen, and 26.2 % oxygen with a molar mass of 180 g/mol. Empirical formula = ___________________ Molecular Formula = _______________________ 46) Given the reaction: ___ Na2SiO3 + ___ HF ____ H2SiF6 + ____ NaF + _____ H2O a) how many moles of HF are needed to react with .300 mol of Na2SiO3? _______________________ b) How many grams of NaF form when .500 mol of HF are completely consumed? _________________ c) How many grams of water form if 125 g of NaF formed? ______________________ 47) Given the reaction: ___ C6H12O6 ___ C2H5OH + ___ CO2 a) How many moles of carbon dioxide are produced when .400 mol of glucose (C6H12O6) reacts completely? _____________________________ b) How many grams of glucose are needed to form 7.50 g of ethanol? _____________________ c) how many grams of carbon dioxide form when 7.50 g of ethanol are produced? _________________ 48) Given the reaction: ____ C6H14 + ____ O2 ____ CO2 + ____ H2O a) 42.0 grams of hexane are combined with 80.0 of oxygen at STP. What is the limiting reagent(reactant) ? ________________ b) what mass of carbon dioxide is produced? _________________ c) what mass of water vapor is produced? _________________ d) What mass of the excess reagent is left over? ________________ e) If the actual yield of water vapor is 20.6 grams, then what is the percent yield? _____________ 49) A simple hydrocarbon (no oxygen) is combusted completely, producing 6.28 grams of carbon dioxide and 2.57 grams of water vapor. What is the empirical formula of this hydrocarbon? 50) 2.78 grams of an oxy-hydrocarbon is combusted completely, producing 6.32 grams of carbon dioxide and 2.58 grams of water vapor. If its molar mass is about 116 g/mol, what is its molecular formula? 51) One student measures the volume of a gas at 216 mL when the pressure was 1.25 atm. Another student comes in and lowers the pressure to 87900 Pa. If the temperature remained the same, what is the new volume of the same sample of gas? 52) On a hot day, 104 oF, the volume of gas in a tire is 3.46 liters. What is the volume of the gas on a cold winter day, -13.0 oF, if the pressure and amount of gas have not changed? 53) On a warm day, .0500 moles of neon would have a volume of about 1.27 liters. On the same day, given the same temperature and pressure, what would the volume be for 1.33 moles of neon? 54) A fixed metal tank has a volume of 52.4 liters. The tank is filled on a cold day (0.00 oC) with hydrogen gas under a pressure of 2.00 atm. The tank exploded on a hot day (100.0 oC). Assuming the volume of the tank didn’t change (until it exploded) what was the pressure in the tank just before it exploded? 55) A latex balloon was filled with exactly 1.000 liters of helium when the temperature was 32.50 oC and the air pressure was 1.17 atm. Later on a storm comes in, dropping the air pressure to 720. Torr and dropping the temperature to 25.80 oC. What is the new volume of the balloon? 56) A .275 mole sample of helium is kept under a pressure of 2.00 atm and at a temperature of 75 oC. What is the volume of the gas? 57) A 6.125 gram sample of neon is used in a sign. The neon is kept under a pressure of 75,330 Pa. When the temperature is 27 oC, what is the volume of the gas? 58) What is the density of fluorine gas when the pressure is 125, 000 Pa and the temperature is 95 oF? 59) A 2.0 L tank of nitrogen gas at 1.0 atm and 25 oC is connected to a 3.0 L tank of oxygen at 2.0 atm and 25 oC. When the valve is opened, allowing the gases to mix, but not react: a) What is the new pressure of the nitrogen? b) what is the new pressure of the oxygen? c) What is the total pressure of the system? d) What is the mole fraction of nitrogen in this system? 60) A 10 liter tank contains oxygen at 1.00 atm and 298 K. A 12 liter tank contains helium at .75 atm and 298 K. The valve that connects the two tanks is opened, allowing the gases to mix, but obviously they do not react. What is the mole fraction of the helium in the system after mixing has occurred? 61) What are the densities of CO2, N2O, and Cl2 at STP? 62) A neon sign is made from cylindrical glass tubing with a diameter of 4.5 cm and whose length is 5.3 m. If the sign contains neon at 2.03 Torr and 35 oC, what mass of neon is in the tube? Remember that 1 liter is the same as 1 dm3. 63) A gas with an empirical formula of CH3 has a density of 1.218 g/L at 27oC and 2 atm. What is its molecular formula? 64) A mixture containing 3.15 g each of CH4, C2H4 and C4H10 is contained in a 2.00 liter flask at a temperature of 64 oC. a) Calculate the partial pressure of each gas. b) Calculate the total pressure of the mixture. 65) A mixture of gases contains .75 mol N2, .30 mol O2, and .15 mol CO2. If the total pressure of the mixture is 1.56 atm, what is the partial pressure of each component? 66) 6.05 g of O2, 4.92 g of N2, and 1.32 g of H2 are mixed in a container. a) what are the mole fractions of each component? b) What is the partial pressure of each component if it is held in a 12.40 liter vessel at 15 oC? 67) Zinc metal is placed in sulfuric acid. If 159 ml of wet H2 gas is collected over water at 24 oC and the manometric pressure of 738 Torr, how many grams of zinc have been consumed? Hint You will need to look up a water vapor table. 68) Acetylene gas, C2H2 , can be prepared by the reaction: CaC2 (s) + 2 H2O (l) Ca(OH)2 (s) + C2H2 (g) Calculate the volume of C2H2 that is collected over water at 21 oC by reaction of 3.26 g CaC2 if the manometer reads 748 Torr? Hint -You will need to look up a water vapor table. 69) Given the reaction: ___ C3H8 (g) + _ O2 (g) ___ CO2 (g) + ___ H2O (g) a) If 2.50 L of propane reacts completely with excess oxygen, what volume of carbon dioxide will be produced at a constant temperature of 86.0 oF and a constant pressure of 1.75 atm? b) If 4.44 L of propane are mixed with 11.1 L of oxygen at constant STP , i) what is the limiting reagent? ______________________ ii) what volume of the excess reagent is left after the reaction? ______________________ iii) what mass of water vapor is produced? ______________________ c) If 15.0 grams of propane reacts completely, what volume of carbon dioxide is produced? Assume constant STP. +1 hydrogen, H+ cesium,Cs+ copper (I), Cu+ lithium, Li+ potassium, K+ silver, Ag+ sodium, Na+ Common Monatomic ions +2 +3 2+ barium, Ba aluminum, Al3+ 2+ calcium, Ca chromium(III), Cr3+ cobalt(II) Co2+ iron(III), Fe3+ copper(II) , Cu2+ iron(II) , Fe2+ lead(II), Pb2+ magnesium, Mg2+ manganese(II), Mn2+ mercury(II), Hg2+ nickel(II), Ni2+ strontium, Sr2+ tin(II), Sn2+ Zinc, Zn2+ -1 chloride, Clfluoride, Fbromide, Briodide, Ihydride, H- -2 oxide, O2sulfide, S2- +1 ammonium, NH4+ -1 acetate, C2H3O2Acetate, CH3COObicarbonate, HCO3Bisulfate, HSO4bromate, BrO3bromite, BrO2chlorate, ClO3chlorite, ClO2cyanide, CNhydroxide, OHHypobromite, BrOhypochlorite, ClOhypoiodite, IOiodate, IO3Iodite, IO2nitrate, NO3nitrite, NO2permanganate, MnO4perchlorate, ClO4- +4 lead(IV), Pb4+ tin(IV), Sn4+ -3 nitride, N3phosphide, P3- Common Polyatomic ions +2 Mercury(I), Hg22+ -2 carbonate, CO32chromate, CrO42dichromate, Cr2O72oxalate, C2O42peroxide, O22sulfate, SO42sulfite, SO32tartrate, C4H4O62thiosulfate, S2O32- -1 periodate, IO4Thiocyanate, SCN- -3 arsenate, AsO43arsenite, AsO33phosphate, PO43phosphite, PO33- +5 Antimony(V), Sb5+ Elements You Should Know YOU DO NOT HAVE TO TURN THIS IN. THIS IS JUST TO HELP YOU STUDY! Al ________________________ H _______________________ Rb ____________________ Sb ________________________ I ________________________ Sc _____________________ Ar ________________________ Ir _______________________ Se _____________________ As ________________________ Fe _______________________ Si _____________________ Ba ________________________ Kr _______________________ Ag _____________________ Be ________________________ Pb _______________________ Na _____________________ Bi _________________________ Li ________________________ Sr _____________________ B _________________________ Mg _______________________ S ______________________ Br _________________________ Mn _______________________ Te _____________________ Cd ________________________ Hg _______________________ Th _____________________ Ca ________________________ Mo _______________________ C _________________________ Nd _______________________ Sn _____________________ Cs ________________________ Ne _______________________ Ti _____________________ Cl _________________________ Ni _______________________ W _____________________ Cr ________________________ N ________________________ U ______________________ Co ________________________ O ________________________ V ______________________ Cu ________________________ Pd _______________________ Xe _____________________ F _________________________ P ________________________ Zn _____________________ Fr ________________________ Pt ________________________ Zr _____________________ Ga _______________________ Pu _______________________ Ge _______________________ K _______________________ Au _______________________ Ra _______________________ He _______________________ Rn _______________________