AP Chemistry Summer Assignment Notes

AP Chemistry Summer Assignment Notes (Summary)

• Contact and materials

  • For help or clarification, email: jmacdonald@stfrancishs.org
  • Textbook: Chemistry, AP edition by Raymond Chang and Kenneth Goldsby; ISBN: $9780076656103$
  • Students should obtain a copy; some classmates may have one for sale and letters were written
  • Units to complete: Units 1 and 2
  • Much of the material is review from previous chemistry courses; some content is new. Review is essential because class time will emphasize understanding over memorization
  • Khan Academy resources are available but not the sole learning resource; the Khan Academy class link will be provided

• Summer Assignment (summary of tasks to be completed before the first day of class)
  1) Complete this packet; memorize required information; complete reading, notes, and homework problems
  2) Watch “A Different Look at Stoichiometry” lecture videos on Schoology
  3) Read and sign the Safety Handout; have parents sign as well; due on the first day of class; submit to Schoology when available
  4) Take Safety Quiz on Schoology; 100% to participate in labs; retakes allowed until passing; must be completed before the first day of class

  • If internet access is an issue, notify the teacher ahead of time to arrange access
    5) Khan Academy lectures are available in the unit in the correct order for the units we will cover
    6) AP Classroom access for summer work is being pursued; updates will be posted in a different color with dates; no additions after July 31

• Page 2: Knowledge to memorize and test details

  • You will be tested on material within the first 2–3 days of school; test is worth 100 points
  • SI base units (Le Système International d’Unites)
  • A. 7 base units – memorize these; mass and temperature are the trickiest
    • Length: ext{meter}
      ightarrow m
    • Mass: ext{kilogram}
      ightarrow kg
    • Time: ext{second}
      ightarrow s
    • Thermodynamic temperature: ext{kelvin}
      ightarrow K
    • Amount of substance: ext{mole}
      ightarrow mol
    • Additional base units (often introduced): ext{ampere}
      ightarrow A, ext{ candela}
      ightarrow cd
    • Note: The provided packet emphasizes mass and temperature as the challenging ones to memorize
  • B. Important prefixes (multipliers) – memorize these; they are used to form units of various sizes
    • Prefix signs and meanings: M
      ightarrow 10^{6}, \ k
      ightarrow 10^{3}, \ c
      ightarrow 10^{-2}, \ m
      ightarrow 10^{-3}, \ bc
      ightarrow 10^{-6}, \ n
      ightarrow 10^{-9}
    • Example multipliers (using meters as the base unit):
    • $1~ ext{Mm} = 10^{6}~ ext{m}$
    • $1~ ext{km} = 10^{3}~ ext{m}$
    • $1~ ext{cm} = 10^{-2}~ ext{m}$
    • $1~ ext{mm} = 10^{-3}~ ext{m}$
    • 1~rac{}{}~rac{}{} ~ ext{(micro)} ~ o ~10^{-6} (for clarity: $1~ ext{μm} = 10^{-6}~ ext{m}$)
    • $1~ ext{nm} = 10^{-9}~ ext{m}$
    • Note: $10^{9}~ ext{nm} = 1~ ext{m}$
  • Solubility rules (ionic compounds):
    1) Ionic compounds containing Group 1 elements and ammonium ion (NH4+) are soluble.
    2) Ionic compounds containing acetates (CH3COO−) and nitrates (NO3−) are soluble.
    3) Ionic compounds containing halogens (except F−) are soluble except those of Ag+, Hg2+, and Pb2+ (lead).
    4) Ionic compounds containing sulfates (SO4 2−) are soluble except Ca2+, Sr2+, Ba2+, Ag+, Hg2+, and Pb2+.
    5) Hydroxides are soluble only with alkali metals and heavier alkaline earth metals (Ca2+, Sr2+ are partially soluble).
    6) Assume other ionic compounds are insoluble.

• Page 3: Common ions and acids/bases

  • Monatomic cations (examples): H+, Ag+, Zn2+, Fe3+, Fe2+, Cu2+, Cu+, Sn4+, Sn2+, Pb4+, Pb2+, Ni2+
  • Polyatomic anions (examples): OH−, NO3−, PO4 3−, CO3 2−, HCO3−, SO4 2−, ClO3−, CH3COO−, MnO4−, Cr2O7 2−, CrO4 2−, O2 2−, C2O4 2−, etc.
  • Polyatomic cation: NH4+ (ammonium)
  • Important note: All ion names must be spelled correctly on tests; small spelling differences can change the ion
  • Strong acids (examples): $ext{HCl}, ext{HBr}, ext{HI}, ext{H}<em>2 ext{SO}</em>4, ext{HNO}<em>3, ext{HClO}</em>4, ext{HClO}_3$
  • The first proton in $ext{H}<em>2 ext{SO}</em>4$ is ionized completely; the second proton is only partially ionized; sulfuric acid is the only polyprotic acid with this property; other polyprotic acids are weak and are written in molecular forms in NIE
  • Strong bases: soluble hydroxides include alkali metal hydroxides and Ba(OH)2; slightly soluble hydroxides include Ca(OH)2 and Sr(OH)2; all other common acids/bases are weak

• Page 4–5: Chapter-specific terms to know and study plan

  • Chapter 1: Terms to know & be able to use (you should be able to use these terms and perform related tasks)
  • macroscopic vs microscopic, qualitative vs quantitative, matter, substances, mixtures, homogeneous, heterogeneous, element, compound, solid, liquid, gas, melting point, boiling point, physical property, chemical property, extensive property, intensive property, density, mass vs weight, accuracy, precision
  • Be able to: perform mathematical operations without a calculator, count significant figures, report answers with correct sig figs, dimensional analysis
  • Review sections to do: pages 10, 11, 18; Problems: 12, 16, 30, 32 (without calculator), 34, 36, 38, 42, 44, 54, 56, 77
  • Chapter 2: Terms to know & be able to use
  • Law of definite proportions, atom, subatomic particles, radiation, atomic number, mass number, isotopes, periods, groups/families, metal, nonmetal, metalloid, alkali metals, alkaline earth metals, halogens, noble gases, monatomic, molecule, polyatomic, ion, cation, anion, ionic compound, monatomic vs polyatomic ion, chemical formula, molecular formula, empirical formula, acid, oxyacid, base, hydrate
  • Be able to: list the 7 elements that exist as diatomic molecules, interconvert between ionic compound names and formulas, name-to-formula relationships for binary molecular compounds, name/ formula interconversion for acids, recognize hydrates from formulas, call isotopes by name (e.g., uranium-235)
  • Special note: skim section 2.2; focus on atom and nucleus, charge and relative mass of e−, p, n; skip 2.8 completely
  • Review sections: pages 50, 56; Problems: 14, 16 (first 3 examples), 18, 26, 32, 36, 44, 46, 50, 58 (except i), 60 (except e and j), 63, 64a&b, 66, 68, 72, 76, 80, 82, 112, 114
  • Chapter 3: Important: watch the “A Different Look at Stoichiometry” videos; Terms to know & be able to use
  • atomic mass, atomic mass unit, mole, Avogadro’s number, average atomic mass, molar mass, molecular mass, mass spectrometer, chemical reaction, chemical equation, reactants, products, (g), (l), (s), (aq), stoichiometry, limiting reagent, excess reagent, theoretical yield, actual yield, percent yield
  • Be able to: perform stoichiometry calculations, percent composition, empirical formula calculations (note: do not need to calculate empirical formula from CO2 and H2O produced when burned as in pg 88–89), determination of molecular formulas, percent yield calculations
  • Khan Academy Unit 1 explanations available for this topic
  • Review sections: pages 77, 81, 88, 99, 102; Problems: 5, 14, 16, 20, 26, 28 (carbon only), 30, 40, 46, 50 (a only), 52, 54, 63, 64, 66, 70, 78, 81, 82, 84, 86, 94, 97, 98, 104, 118, 123, 128
  • Chapter 4: Terms to know & be able to use
  • solution, solute, solvent, electrolyte, nonelectrolyte, dissociation, hydration, ionization, reversible reaction, chemical equilibrium, precipitation reaction, metathesis/double displacement, solubility, soluble, insoluble, molecular equation, ionic equation, spectator ions, net ionic equation, hydronium ion, monoprotic acids, diprotic acid, neutralization, salt, redox reaction, half-reaction, oxidation/reduction, oxidation number/state, various reaction types (combination, decomposition, combustion, displacement), concentration, molarity (M), dilution, titration, standard solution, equivalence point, indicator
  • Know properties of acids and bases on page 127 (ignore litmus specifics)
  • Memorize oxidation number rules 1–6 on page 136
  • Review sections: pages 125, 129, 144; Problems: 7, 8, 10, 12, 17, 18, 20, 22, 32, 46, 48, 50, 52, 54, 56 (except d), 62, 74, 76, 82, 84, 90, 92, 96, 98, 108, 110, 126, 142

• Page 6–7: Science Laboratory Safety Rules (summary of the rules in order)

  • 1) Protective goggles are required in the lab; no entry without goggles
  • 2) Inform the instructor if wearing contact lenses in the lab
  • 3) Lab coat/apron required to protect clothing
  • 4) Prepare a safe workspace: bags off floor, chairs pushed in
  • 5) No running, shouting, shoving, or fooling around in the lab
  • 6) Appropriate apparel; no long hanging necklaces or bulky jewelry; fully covered feet
  • 7) Long hair secured; keep away from face and lab materials
  • 8) Know location and use of safety equipment: fire extinguisher, eyewash, fire blanket, exits, shower, gas shut-off
  • 9) Never taste chemicals; avoid touching unless instructed
  • 10) Do not return unused reagents to stock bottles
  • 11) Dispose of waste properly in designated containers
  • 12) Be cautious with odors; fan odors to your nose
  • 13) Never point open flames/tubes at yourself or others
  • 14) Use fume hoods for irritating fumes
  • 15) Do not leave reactions unattended or burners on when not in use
  • 16) A clean lab is a safe lab; return materials and keep your area tidy
  • 17) Report accidents to the teacher immediately
  • 18) NEVER WORK ALONE in the laboratory; always be under supervision
  • 19) No food, drinks, or gum in the lab (unless authorized)

• Page 7 (continuation of safety rules)

  • 20) Understand dangers and hazards of each experiment before starting
  • 21) Follow all written and verbal instructions
  • 22) Do not mix chemicals unless instructed
  • 23) Hot items require gloves or tongs
  • 24) Use small amounts of flammable liquids
  • 25) When lighting a Bunsen burner, light the match first then turn on gas
  • 26) Avoid cracked/broken glassware
  • 27) Dispose of broken glassware in proper container
  • 28) Do not trash in sinks
  • 29) When cleaning glassware, turn on water then rinse under faucet
  • 30) Label glassware properly when reagents look similar to avoid cross-contamination
  • Closing sentiment: A safe laboratory makes chemistry FUN!

• Page 8: Science Class Safety Agreement (summary)

  • All students must pass a laboratory safety test before participating in lab activities
  • Students may be removed from the science activity area if: (A) appearance/dress risks injury, (B) unsafe behavior, (C) not following safety rules, (D) going into unsafe areas, (E) not completing pre-experiment activities
  • Safety agreement form includes spaces for student and parent/guardian signatures, as well as a section to disclose medical conditions that could affect learning
  • A cut-in section indicates the form's physical/parental acknowledgment requirements

• Additional study and preparation reminders

  • You will be tested on the material within the first 2–3 days; be prepared to answer without a calculator (sig figs, dimensional analysis, etc.)
  • Submit all work to Schoology as required; read and sign safety handout with parents prior to labs
  • Use Khan Academy videos as supplementary material and reference for Unit 1 concepts; ensure you understand the core concepts rather than just memorizing procedures
  • Chapter prerequisites emphasize understanding over rote memorization; connect review material to new content to build deep understanding

• Quick reference: key numerical/conceptual items to remember

  • Base units (SI): $m,\, kg,\, s,\, A,\, K,\, mol,\, cd$
  • 7 base units include length, mass, time, current, temperature, amount, luminous intensity
  • Common conversions: $1~ ext{Mm} = 10^{6}~ ext{m},\, 1~ ext{km} = 10^{3}~ ext{m},\ 1~ ext{cm} = 10^{-2}~ ext{m},\ 1~ ext{mm} = 10^{-3}~ ext{m},\ 1~ ext{μm} = 10^{-6}~ ext{m},\ 1~ ext{nm} = 10^{-9}~ ext{m},\ 10^{9}~ ext{nm} = 1~ ext{m}$
  • Sulfuric acid is the only polyprotic acid where the first proton ionizes completely and the second partially; other polyprotic acids are weak
  • Oxidation number rules (to memorize): rules 1–6 (as listed on page 136 of the packet)

Note: This compilation mirrors the content and order of the provided transcript handout and serves as a comprehensive study aide for Units 1–4 and the introductory safety protocol. Be sure to consult the actual textbook and Schoology/ Khan Academy resources for worked examples and full problem sets.