AP Chemistry Summer Assignment ( )

Transcription

1 AP Chemistry Summer Assignment ( ) You are responsible for reading and knowing the content from chapters 13 (Matter and Measurement; Atoms, Molecules, and Ions; Stoichiometry) when you show up for the first day of school in September. This is largely a review of what you covered in Chemistry. Check out a textbook and the corresponding study book on June 13 th, from Ms. Bain. Bring the following textbook problems completed the first day of school to turn in (show all work): Chapter 1 (p. 3336): 1, 14, 22, 24, 36, 38, 42 Chapter 2 (p. 7378): 4, 5, 7, 24, 28, 30, 36, 52, 56, 60, 62, 64, 66, 72, 74, 76, 78, 95 Chapter 3 (p ): 2, 14, 16, 22, 24, 26, 38, 54, 60, 62, 66, 80, 84 In addition, you will need to memorize the polyatomic ions and prefixes that you're accustomed to seeing on your pink sheet and be able to appropriately name acids and organic compounds. I ve attached some hints and flashcards you can cut out to help you memorize the polyatomic ones. Come prepared for a naming quiz on the first day of school, Tuesday, September 7 th. The only tool you will be able to use is the periodic table designated for AP that is included in your packet. Please note that it only has element symbols. For example you will need to know if S is sodium or sulfur. The types of quiz questions you will encounter will include: What is the formula for calcium carbonate? What is the name of Mg3(PO4)2? We have 33 weeks to cover 19 chapters (<2 weeks/chapter) to ensure you are prepared for the AP Chemistry Exam on May 7 th. Like a college course, we will move quickly, so staying on top of assignments (especially this summer homework), asking questions, and being in class will be essential to your success. I have and will continue to post additional resources at Other Notes: Be ready for 0 period lab on Friday s throughout the school year starting September 8 th. You will need a composition notebook (not a spiral notebook) for your labs so make sure you acquire one before school starts. It would be incredibly helpful if you had a scientific calculator to use at home. If you need to borrow one for the summer please let me know. Our first test over chapters 13 will be the third week of school. We will go over some of the newer concepts as a class and review anything you feel like you need more practice with beforehand. I m really excited to start this AP Chemistry journey with you! I will check my periodically ;) over the summer so feel free to me with any questions. This will be a challenge but one we will face and conquer together, Malia Turner mturner@ohsd.net

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3 AP CHEMISTRY EQUATIONS AND CONSTANTS Throughout the exam the following symbols have the definitions specified unless otherwise noted. L, ml = liter(s), milliliter(s) mm Hg = millimeters of mercury g = gram(s) J, kj = joule(s), kilojoule(s) nm = nanometer(s) V = volt(s) atm = atmosphere(s) mol = mole(s) ATOMIC STRUCTURE E = hν c = λν E = energy ν = frequency λ = wavelength Planck s constant, h = Js Speed of light, c = ms 1 Avogadro s number = mol 1 Electron charge, e = coulomb EQUILIBRIUM K c = c d [C] [D] a [A] [B] b ( P K p = C ) ( P D ) a ( P ) ( P ) A c b B, where a A + b B c C + d D d [H ][A ] K a = [HA] [OH ][HB ] K b = [B] K w = [H + ][OH ] = at 25 C = K a K b ph = log[h + ], poh = log[oh ] 14 = ph + poh ph = pk a + log [A ] [HA] Equilibrium Constants K c (molar concentrations) K p (gas pressures) K a (weak acid) K b (weak base) K w (water) pk a = logk a, pk b = logk b KINETICS ln[a] t ln[a] 0 = kt 1 1 = kt At A 0 t ½ = k k = rate constant t = time t ½ = halflife 3

4 GASES, LIQUIDS, AND SOLUTIONS PV = nrt P A = P total X A, where X A = P total = P A + P B + P C +... n = m M K = C D = m V KE per molecule = 1 2 mv 2 moles A total moles Molarity, M = moles of solute per liter of solution A = abc THERMODYNAMICS / ELECTROCHEMISTRY q = mc T S = S products S reactants H = DH products DH reactants f G = DG products DG reactants G = H T S = RT ln K = n E I = q t f f f P = pressure V = volume T = temperature n = number of moles m = mass M = molar mass D = density KE = kinetic energy v = velocity A = absorbance a = molar absorptivity b = path length c = concentration Gas constant, R = J mol 1 K 1 = L atm mol 1 K 1 = L torr mol 1 K 1 1 atm = 760 mm Hg = 760 torr STP = K and 1.0 atm Ideal gas at STP = 22.4 L mol 1 q = heat m = mass c = specific heat capacity T = temperature S = standard entropy H = standard enthalpy G = standard Gibbs free energy n = number of moles E = standard reduction potential I = current (amperes) q = charge (coulombs) t = time (seconds) Faraday s constant, = 96,485 coulombs per mole of electrons 1 joule 1 volt = 1 coulomb 4

5 COMMON IONS CATIONS +1 Charge +2 Charge +3 Charge All group 1 metals All group 2 metals Al 3+ aluminum Li 1+ lithium Be 2+ beryllium Na 1+ sodium Mg 2+ magnesium K 1+ potassium Ca 2+ calcium Rb 1+ rubidium Sr 2+ strontium Cs 1+ cesium Ba 2+ barium Fr 1+ francium Ra 2+ radium and and Ag 1+ silver Cd 2+ cadmium Zn 2+ zinc POLYATOMIC CATION NH4 1+ ammonium All metals visible in the table above have more than one charge possible. (transition metals, submetalloids) Use Roman Numerals to indicate their charge when naming compounds. In a formula you must calculate their charge. ANIONS 1 Charge 2 Charge 3 Charge F 1 fluoride O 2 oxide N 3 nitride Cl 1 chloride S 2 sulfide P 3 phosphide Br 1 bromide I 1 iodide POLY ATOMIC ANIONS CH3CO2 1 acetate also C2H3O2 1 HPO4 2 hydrogen phosphate PO4 3 phosphate ClO 1 hypochlorite CO3 2 carbonate ClO3 1 chlorate O2 2 peroxide ClO4 1 perchlorate CrO4 2 chromate CN 1 cyanide SO3 2 sulfite Cr2O7 2 dichromate 1 HCO 3 hydrogen carbonate 2 SO 4 sulfate (bicarbonate) HS 1 hydrogen sulfide IO3 1 iodate NO2 1 nitrite NO3 1 nitrate OH 1 hydroxide SCN 1 thiocyanate MnO4 1 permanganate

6 COMMON MOLECULES DIATOMIC MOLECULES H2 Hydrogen O2 Oxygen F2 Fluorine Br2 Bromine I2 Iodine N2 Nitrogen Cl2 Chlorine MISCELLANEOUS COMMON MOLECULES H2O H2O2 NH3 CH4 water hydrogen peroxide ammonia (not ammonium! Be careful.) methane COMMON ACIDS HCl hydrochloric acid HCH3CO2 acetic acid (vinegar) HNO3 nitric acid H2SO4 sulfuric acid H3PO4 phosphoric acid H2CO3 carbonic acid PREFIXES FOR NUMBER OF ATOMS for naming nonmetal inorganic compounds mono 1 di 2 tri 3 tetra 4 penta 5 hexa 6 hepta 7 octa 8 nona 9 deca 10 PREFIXES FOR NUMBER OF CARBON ATOMS IN ORGANIC CHEMISTRY NAMES meth 1 eth 2 prop 3 but 4 penta 5 hexa 6 hepta 7 octa 8 nona 9 deca 10

7 Tips for Learning the Ions From the Table These are ions can be organized into two groups. 1. Their place on the table suggests the charge on the ion, since the neutral atom gains or loses a predictable number of electrons in order to obtain a noble gas configuration. This was a focus in first year chemistry, so if you are unsure what this means, get help BEFORE the start of the year. a. All Group 1 Elements (alkali metals) lose one electron to form an ion with a 1+ charge b. All Group 2 Elements (alkaline earth metals) lose two electrons to form an ion with a 2+ charge c. Group 13 metals like aluminum lose three electrons to form an ion with a 3+ charge d. All Group 17 Elements (halogens) gain one electron to form an ion with a 1 charge e. All Group 16 nonmetals gain two electrons to form an ion with a 2 charge f. All Group 15 nonmetals gain three electrons to form an ion with a 3 charge Notice that cations keep their name (sodium ion, calcium ion) while anions get an ide ending (chloride ion, oxide ion). 2. Metals that can form more than one ion will have their positive charge denoted by a roman numeral in parenthesis immediately next to the name of the Polyatomic Anions Most of the work on memorization occurs with these ions, but there are a number of patterns that can greatly reduce the amount of memorizing that one must do. 1. ate anions have one more oxygen then the ite ion, but the same charge. If you memorize the ate ions, then you should be able to derive the formula for the ite ion and viceversa. a. sulfate is SO 4 2, so sulfite has the same charge but one less oxygen (SO 3 2 ) b. nitrate is NO 3, so nitrite has the same charge but one less oxygen (NO 2 ) 2. If you know that a sufate ion is SO 2 4 then to get the formula for hydrogen sulfate ion, you add a hydrogen ion to the front of the formula. Since a hydrogen ion has a 1+ charge, the net charge on the new ion is less negative by one. a. Example: 3 PO 4 2 HPO 4 H 2 PO 4 phosphate hydrogen phosphate dihydrogen phosphate 3. Learn the hypochlorite chlorite chlorate perchlorate series, and you also know the series containing iodite/iodate as well as bromite/bromate. a. The relationship between the ite and ate ion is predictable, as always. Learn one and you know the other. b. The prefix hypo means under or too little (think hypodermic, hypothermic or hypoglycemia ) i. Hypochlorite is under chlorite, meaning it has one less oxygen c. The prefix hyper means above or too much (think hyperkinetic ) i. the prefix per is derived from hyper so perchlorate (hyperchlorate) has one more oxygen than chlorate. d. Notice how this sequence increases in oxygen while retaining the same charge: ClO ClO 2 ClO 3 ClO 4 hypochlorite chlorite chlorate perchlorate

8 Sulfite Sulfate Hydrogen sulfate Phosphate Dihydrogen Phosphate Hydrogen Phosphate Nitrite Nitrate Ammonium Thiocyanate Carbonate Hydrogen carbonate Borate Chromate Dichromate Permanganate Oxalate Amide Hydroxide Cyanide Acetate Peroxide Hypochlorite Chlorite Chlorate Perchlorate Thiosulfate

9 HSO 4 SO 4 2 SO 3 2 HPO 4 2 H 2 PO 4 PO 4 3 NH 4 + NO 3 NO 2 HCO 3 2 CO NCS 3 SCN Cr 2 O 7 2 CrO 4 2 BO 3 3 NH 2 C 2 O 4 2 MnO 4 C 2 H 3 O 2 CH 3 COO CN OH ClO 2 ClO O 2 2 S 2 O 3 2 ClO 4 ClO 3