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AP Chemistry Summer Assignment: Essential Review Topics

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Chemistry
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Dec 10, 2024
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AP Chemistry Summer AssignmentWelcome to AP Chemistry!In order to effectively cover all the material in this course, we will have to move quickly through the topics thatyou are already familiar with from Honors Chemistry. Therefore, you are expected to review several topics(listed below) on your own prior to September. These topics are covered in the first three chapters of your APtextbook (Chemistry, The Molecular Nature of Matter and Change, Silberberg 7e).Problems (with answers) have been included below to help you. Although these practice problems will not becollected,you can expect a graded primary assessment with similar problems on the third classmeeting of the school year. Therefore, you should complete this assignment thoroughly, preferably in Augustso that the material is fresh when we begin. If you would like more practice, additional problems with answerscan be found at the end of each chapter.If you run into trouble, or have any questions about the course, please email me. I will be checking my emailperiodically, but not daily. Good luck, and enjoy your summer. I look forward to meeting you in the fall!Mrs. Felixlfelix@eccrsd.usObjective Checklist (with relevant chapters):___ Use the Unit Factor Method (Dimensional Analysis) to convert from one quantity to another (1.4)___ Report answers with correct units (1.4)___ Report answers to the correct number of significant figures (1.5)___ Distinguish between accuracy and precision (1.5)___ Describe the structure of the atom (2.5)___MEMORIZEcharges, formulas, and names of common monatomic and polyatomic ions foundon the last page of this assignment___ Quickly name and write formulas for ionic and covalent compounds (2.8)___ Convert between moles, mass, and number of particles (3.1)___ Determine the formula of an unknown compound (3.2)___ Write and balance chemical equations (3.3)___ Use stoichiometry to calculate quantities of reactant and product (3.4)1
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Part I: Review “Ch 1: Keys to the Study of Chemistry” (textbook). Then, solve the following problems.Solve the following using the factor label method. Show all work: You must write out all conversion factors andshow how units cancel. Report all answers with units and to the correct number of significant figures.Example: If you ate 2.0 pounds of jelly beans, how many jelly beans did you eat? (Given: 1 jelly bean = 1.18 g;454 g = 1 lb.)2.0 lbx454 gx1 jelly bean=770 jelly beans1 lb1.18 g.1.What is the length, in inches, of a 100. m soccer field, given that 1 in = 2.54 cm?2.The average radius of a molecule of lysozyme, an enzyme in tears, is 1430 pm. What is its radius in nanometers(nm)?3.The radius of a barium atom is 2.22 x 10–10m. What is its radius in angstroms (Å)?(Note: 10–12m = 1 pm; 100 pm = 1Å)4.The center on your school’s basketball team is 6 ft 10 in tall. How tall is the player in millimeters (mm)?(Note: 1 cm = 10 mm; 1 in = 2.54 cm; 12 in = 1 ft)5.The speed of light in a vacuum is 2.9983 x 108m/s. What is its speed in...a.km/h?b.mi/min? (Note: 1 km = 0.62 mi)6.A small hole in the wing of a space shuttle requires a 20.7 cm2patch.a.What is the patch’s area in square kilometers (km2)?b.If the patching material costs NASA $3.25/in2, what is the cost of the patch?7.The area of a telescope lens is 7903 mm2. (Note: 2.54 cm = 1 in and 12 in = 1 ft).a.What is the area in square feet (ft2)?b.If it takes a technician 45 s to polish 135 mm2, how long does it take her to polish the entire lens?2
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8.The volume of a certain bacterial cell is 2.56 um3. (Note: 1 mL = 1 cm3)a.What is its volume in cubic millimeters (mm3)?b.What is the volume of 105cells in L?9.Answer the following, given that 1 quart = 946.4 mL, 1 gallon = 4 quarts, and 1 mL = 1 cm3.a.How many cubic meters of milk are in 1 qt?b.How many liters of milk are in 835 gal?10. Perform the following conversions:a.20.oC (a pleasant spring day) to Kb.–164oC (the boiling point of methane, the main component of natural gas) to Kc.0 K (absolute zero, theoretically the coldest possible temperature) tooCd.6.1 x 103K (the surface temperature of the Sun) tooC11. Round off each measurement to the indicated number of significant figures.a.0.0003554 m (to 2 sf)d.231.554 kg(to 4 sf)b.35.8348 g (to 4 sf)e.144,000 mL (to 2 sf)c.22.4555 s (to 3 sf)f.1.030 x 103L (to 2 sf)12. Carry out the following calculations, and record your answer with the correct number of significant figures.a.1.110 cm + 17.3 cm + 108.2 cm + 316 cmb.2.420 g + 15.6 g4.8 gc.7.87 mL.16.1 mL - 8.44 mLd.V =𝜋r2h, where r = 6.23 cm and h = 4.630 cm13. Which statements include exact numbers?a.Angel Falls is 3212 ft high.b.There are 8 known planets in the Solar System.c.There are 453.59 g in 1 lb.d.There are 1000 mm in 1 m.Answers: 1) 3.94 x 103in 2) 1.43 nm 3) 2.22Å4) 2.1 X 103mm 5a) 1.0794 x 109km/h 5b) 1.1 x 107mi/min 6a) 2.07 x10-9 km26b) $10.43 7a) 8.507 x 10–2ft27b) 2.6 x 103s 8a) 2.56 x 10–9mm38b) 10-10L 9a) 9.464 x 10–4m39b) 3.16 x103L 10a) 293 K 10b) 109 K 10c) –273oC 10d) 5.8 x 103 oC 11a) 0.00036 m11b) 35.83 g 11c) 22.5 s 11d) 231.6 kg11e) 140,000 mL 11f) 1.0 x 103L 12a) 443 cm 12b) 3.8 12c) 1.0 12d) 565 cm313) b,d3
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Part II: Review “Chapter 2: The Components of Matter.” Then, answer the following questions.1.Complete the table below for the following neutral atoms.Name# ofProtons# ofNeutrons# ofElectronsAtomicNumber (Z)MassNumber (A)NuclideSymbol2630Cl17351737Iodine-12716172.Write the nuclide symbol (X notation) for each of the following.𝑍𝐴3.Draw atomic representations for the atoms below (similar to those shown in the previous problem).a.48Tib.79Sec.11B4.Atom “A” has 11 neutrons and Atom “B” also has 11 neutrons. Are these atoms isotopes? Explain.5.The atomic masses of elements are generally not whole numbers. Explain why.4
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6.Naturally occurring chlorine is 75.78% Cl - 35 (34.9689 amu) and 24.22% Cl - 37 (36.9659 amu). Calculate theaverage atomic mass.7.An element is found to gain three electrons when it forms an ion.a.What group number would this element be found in?b.Is there enough information provided to determine what period it is in? Explain.8.Look at the average atomic mass of Ar and K.a.Explain why early scientists might have been tempted to have K follow Cl on the periodic table.b.Propose two reasons as to why they placed Ar after Cl instead of K9.Identify the following elements.a.An alkali metal in the 5th period.d.Period 3 element that has two valence electronsb.A transition metal in period 4e.Group 17 element with fewer than 15 protonsc.An atom in the 3rd period that forms a –1 ionf.Noble gas in period 510. Explain why atoms tend to gain or lose electrons relative to the number of valence electrons. How can youpredict the number of electrons lost or gained?11. Classify each element as metal, nonmetal, or metalloid. What ion(s) would each element be likely to form?a.nitrogenc. sulfure. hydrogeng. bromineb.calciumd. carbonf. oxygenh. aluminum12. How many total ions (cations and anions) are present in the following compounds?a.sodium acetatec. copper(II) chloridee. carbon dioxideb.Aluminum nitrated. copper (I) chloridef. calcium phosphate13. Aluminum reacts with a certain nonmetallic element to form a compound with the general formula Al2X3. ElementX must be from which group on the periodic table?14. Complete the table on the next page. (No answer key - these can be easily checked online.)5
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Chemical FormulaChemical NameType of compound1NaISodium iodideIonic2KNO23(NH4)2SO34CuSO4●5H2OIonic5AuNO26Al2(CrO4)3Ionic7IF7Covalent8Cu(OH)29NO10CO2Covalent11CuI212P4O1013Manganese II sulfide14Potassium peroxide15Lithium permanganate16Mercury (I) chloride17Aluminum cyanide18Manganese (II) nitride19Ammonium sulfide20Diphosphorus pentoxide21Barium hydroxide octahydrate22Sodium acetate23Aluminum nitrate24Copper (II) chloride25Iron (III) CarbonateAnswers: 1) iron-56, 26e–, Z=26, A=56; chlorine-35, 17p+, 18n, 17e–, Z=17, A=35; chlorine-37, 20n, 17e-, Z=17, A=37;53p+, 74n, 53e-, Z=53, A=74 2a) Z=18 and A=38, Ar 2b) Z=25 and A=55, Mn 2c) Z=47 and A=109, Ag 3a) 22p+, 26n,22e–3b) 34p+, 45n, 34e–3c) 5p+, 6n, 5e–4) No, isotopes have same Z (# of protons), but different A (# ofprotons+neutrons) 5) Weighted average of all isotopes 6) 35.45 amu 7a) group 15 7b) No 8a) K has a greater averageatomic mass than Ar 8b) Ar behaves like other group 18 elements 9a) Rb 9b) Any element Z= 21 to 30 9c) Cl 9d) Mg9e) F9f) Xe 10) metals gain nonmetals lose to get same # of e-s as the nearest noble gas11a) NM 3– 11b) M 2+ 11c)NM 2– 11d) NMl 4+ or 4– 11e) NM +1 11f) NM 2– 11g) NM 1–11h) M +3 12a) 2 15b) 4 12c) 3 12d) 2 12e) 0, it’scovalent12f) 5 13) group 166
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Part III: Review “Chapter 3: Stoichiometry of Formulas and Equations.” Then, solve the following problems.Solve the following using the factor label method. Show all work: You must write out all conversion factors andshow how units cancel. Report all answers with units and to the correct number of significant figures.1.Answer the following questions for the compound aluminum sulfate.a.What is the molar mass of this compound?b.What is the mass of a 1.5 mole sample?c.How many oxygen atoms are present in the 1.5 mol sample?2.Consider a 0.433 mol sample of calcium nitrate.a.Calculate the mass of the sample in grams.b.How many formula units of calcium nitrate are present?c.How many nitrate ions are present?3.Answer the following questions for the compound aluminum chloride.a.What is the molar mass of this compound?b.What is the mass of a 0.65 mole sample?c.How many formula units are in the 0.65 mole sample?d.How many ions are in the 0.65 mole sample?e.How many protons are in the 0.65 mole sample?7
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4.What mass of rhodium contains the same number of atoms as there area.gallium atoms in 36.0 g galliumb.indium atoms in 36.0 g indium5.Carbon has two isotopes C-12 (99%) and C-13 (1%).a.How many atoms of C would be present in a 34 gram sample of pure diamond (pure carbon)?b.How many atoms of those are C-13 atoms?6.Calculate each of the following quantities.a.Mass (in g) of 6.4 x 10–2mol of manganese (II) sulfateb.Amount (in moles) of formula units in 15.8 kg of Fe(ClO4)3c.Number of nitrogen atoms in 92.6 mg of ammonium nitrite7.A sample of Ni(CO)4, a toxic transition-metal complex, has 5.23 × 1024atoms of carbon. How many atoms of Nidoes it contain?8.Calculate each of the following:a.Mass % of H in ammonium bicarbonateb.Percent by mass of Mn in potassium permanganate8
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9.Find the molecular formula for each compound.a.Empirical formula CH2(molar mass = 42.08 g/mol)b.Empirical formula NO2(molar mass = 92.02 g/mol)c.Empirical formula CHN (molar mass = 135.14 g/mol)10. Cortisol (molar mass = 362.47 g/mol) is a steroid hormone involved in protein synthesis. Medically, it is used toreduce inflammation from arthritis. Cortisol is 69.6%C, 8.34% H, and 22.1% O by mass. What is its molecularformula?11. Calculate the mass (in grams) of each product formed when 43.82 g of diborane (B2H6) reacts with excess water.B2H6(g)+H2O(l)→H3BO3(s)+H2[unbalanced]12. Calculate the mass of each product formed when 174 g of silver sulfide reacts with excess hydrochloric acid.Ag2S(s)+HCl(aq)→AgCl(S)+H2S(g)[unbalanced]9
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13. Consider the following reaction:4HCl(aq) + MnO2(s) → MnCl2(aq) + 2H2O(g) + Cl2(g)a.How many moles of hydrochloric acid are needed to make 500. g of water?b.What mass, in g, of hydrochloric acid is required to produce 0.88 moles of MnCl2?c.If 25.0 g of hydrochloric acid reacts completely, how many molecules of chlorine gas are formed?14.Consider the formation of copper (I) sulfide from its elements:16Cu(s) + S8(s) → 8Cu2S(s)a.How many moles of sulfur are needed to react with 32.0 moles of copper?b.How many moles of copper (I) sulfide are formed if 32.0 moles of copper react completely?c.How many molecules of S8are consumed during the production of 14.55 g of copper (I) sulfide?15. Consider the following reaction:2C6H6(l) + 7O2(g) → 2C4H2O3(l) + 4H2O(l) + 4CO2(g)a.How many grams of oxygen gas are needed to make 250 grams of maleic anhydride, C4H2O3?b.Continuing from the previous question, what mass of carbon dioxide will be released as a byproduct?Answers: 1a) Al2(SO4)3: 342.145 g/mol 1b) 510 g 1c) 1.1 x 1025O atoms 2a) 71.1 g 2b) 2.61 x 1023formula units 2c)5.21 x 1023nitrate ions 3a) AlCl3:133.33 g/mol 3b) 87 g 3c) 3.9 x 1023formula units 3d) 1.6 x 2024ions 3e) 2.5 x 1025protons 4a) 53.1 g 4b) 32.3 g 5a) 1.71 x 1024atoms C 5b) 1.71 x 1022atoms C-13 6a) 9.7 g MnSO46b) 44.6 molFe(ClO4)36c) 1.74 x 1021N atoms 7) 1.31 x 1024atoms Ni 8a) 6.375 % H 8b) 34.58 % O 9a) C3H69b) N2O49c)C5H5N510) C21H30O511) 195.8 g H3BO3and 19.16 g H212) 201 g AgCl and 23.9 g H2S 13a) 55.5 mol HCl13b) 130 gHCl13c) 1.03 x 1023molecules Cl214a) 2.00 mol S814b) 16.0 mol Cu2S14c) 6.87 x 1021molecules S815a) 280 gO215b) 220 g CO210
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Monatomic Ions11821314151617Li+1Be2+C–4N–3O–2F–1Na+1Mg+23456789101112Al+3P–3S–2Cl–1K+1Ca+2Cr+2Cr+3Mn+2Mn+3Fe+2Fe+3Co+2Co+3Ni+2Ni+3Cu+1Cu+2Zn+2Se–2Br–1Rb+1Sr+2Ag+1Cd+2Sn+2Sn+4Te–2I–1Cs+1Ba+2Hg2+2Hg+2Pb+2Pb+4Polyatomic IonsChargeFormulaNamePolyatomic ions can be altered as follows:●hypo__ite○two less oxygen atoms○ex)hyposulfite, SO22–●__ite○one less oxygen atom○ex) sulfite, SO32–●__ate○unaltered form○ex) sulfate, SO42–●per__ate○one more oxygen atom○ex)persulfate, SO52–●hydrogen __○add a hydrogen atom, increase thecharge by 1○ex)hydrogensulfate, HSO41–+1NH4+ammoniumH3O+hydronium–1CH3COO–acetateCN–cyanideOH–hydroxideClO3–chlorateNO3–nitrateMnO4–permanganate–2CO32–carbonateCrO42–chromateCr2O72–dichromateO22–peroxideC2O42–oxalateSeO42–selenateSO42–sulfateSiO32–silicateC4H4O62–tartrate–3AsO43–arsenateBO33–boratePO43–phosphate11
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