AP Chemistry Summer Packet 2017 Lake Braddock Secondary 2019-12-31آ  AP Chemistry Summer Packet 2017

  • View
    0

  • Download
    0

Embed Size (px)

Text of AP Chemistry Summer Packet 2017 Lake Braddock Secondary 2019-12-31آ  AP Chemistry Summer Packet...

  • AP Chemistry Summer Packet 2017

    Lake Braddock Secondary School

    School Year Supply List

    1. 2.5+-inch 3-ring binder with dividers

    2. Composition book with grid/graph paper (Make sure the pages are not perforated)

    3. Graphing calculator

    4. Recommended: A review book (est. cost $10-20). We recommend the Princeton Review

    book. Any review book must be the 2014 edition or later due to course rewrites.

    Summer Assignment

    You must complete this review packet and turn it in on your first day of AP Chemistry.

    This is not optional. It is required and taken for your first grade.

    The material is divided into eight weeks and a sample calendar has been provided. Should you

    choose to follow this calendar the workload will not feel daunting. If you choose to wait until the

    night before school starts to complete this packet, you may feel differently.

    Assessment on Summer Material

    You will take a diagnostic assessment the first week of school. This will cover:

     All Memorized Material (see next pages)

     Chapters 1-3 only in the AP Chem textbook (This is all Chemistry I review content.)

    Your summer assignment includes review material that corresponds to these first three

    chapters. If you still have them, you may find your Chemistry I notes useful, as none of this

    material should be new to you! You will receive your textbook the first day of school, but all of

    this information can be found online or in your old notes.

    AP Chemistry is a difficult course and memorizing the following pages of material is essential for

    success in learning the concepts covered in the course. Make flashcards, have your friends and

    family quiz you, take lists with you on vacation, or do whatever it takes to get this information

    firmly planted in your head. Do not wait until the night before school begins.

  • Material to Memorize

    Oxidation Numbers

    An oxidation number is a number assigned to an atom in a molecular compound or molecular

    ion that indicates the general distribution of electrons among the bonded atoms.

    1. The oxidation number of any free, uncombined element is 0.

    2. The oxidation number of a monatomic ion equals the charge on the ion.

    3. The more electronegative element in a binary compound is assigned the number equal

    to the charge it would have if it were an ion.

    4. The oxidation number of fluorine in a compound is always -1.

    5. Oxygen has an oxidation number of -2 unless it is combined with F, in which case it is

    +2, or it is in a peroxide, in which case it is -1.

    6. The oxidation state of hydrogen in most of its compounds is +1 unless it is combined

    with a metal, in which case it is -1.

    7. In compounds, elements of Groups 1 and 2 as well as aluminum have oxidation

    numbers of +1, +2, and +3, respectively.

    8. The sum of oxidation numbers of all atoms in a neutral compound is zero.

    9. The sum of the oxidation number of all atoms in a polyatomic ion equals the charge of

    the ion.

    Solubility Rules

    Soluble Compounds Insoluble Compounds

    Group 1 and Ammonium Hydroxides (EXCEPT Group 1 and Ammonium. Hydroxides of

    Ca2+, Sr2+, and Ba2+ are slightly soluble,) Nitrates, Hydrogen Carbonates, Chlorates

    and Acetates

    Chlorides, Bromides and Iodides (EXCEPT those of Pb2+, Ag+, and Hg22+)

    Carbonates, Phosphates, Chromates and Sulfides

    (EXCEPT Group 1 and Ammonium. Sulfides of Group 2 are soluble.)

    Sulfates (EXCEPT Ag+, Sr2+, Ba2+, Pb2+, and Ca2+)

    Strong Acids and Bases

    Acids Bases

    HF – weak HCl – strong HBr – strong HI – strong H2SO4 – strong HNO3 – strong HClO3 – strong HClO4 – strong All other acids are weak H2CO3 → H2O + CO2 (very weak acid-breaks down!)

    LiOH – strong NaOH– strong KOH – strong RbOH– strong CsOH– strong Ca(OH)2 – strong Ba(OH)2 – strong Sr(OH)2 – strong NH3 – weak

  • Bromide Br1- Dichromate Cr2O72- Periodate IO41-

    Hypobromite BrO1- Dihydrogen Phosphate

    H2PO41- Permanganate MnO41-

    Bromite BrO21- Ethanoate (Acetate)

    C2H3O21- Nitrate NO31-

    Bromate BrO31- Hydrogen Carbonate

    (Bicarbonate) HCO31- Nitrite NO21-

    Perbromate BrO41- Hydrogen Phosphate HPO42- Oxalate C2O42-

    Carbonate CO32- Hydrogen Sulfate

    (Bisulfate) HSO41- Peroxide O22-

    Hypochlorite ClO1- Hydrogen Sulfide

    (Bisulfide) HS1- Phosphate PO43-

    Chlorite ClO21- Hydrogen Sulfite

    (Bisulfite) HSO31- Phosphite PO33-

    Chlorate ClO31- Hydroxide OH1- Sulfate SO42-

    Perchlorate ClO41- Hypoiodite IO1- Sulfite SO32-

    Chromate CrO42- Iodite IO21- Thiosulfate S2032-

    Cyanide CN1- Iodate IO31- Thiocyanate SCN1-

    Polyatomic Ions – Cut These Out to Make Flashcards!

  • July 2017

    M T W T F S S

    June 26

    June 27

    June 28

    June 29

    June 30

    1 2

    3 4 5 6 7 8 9

    10 11 12 13 14 15 16

    17 18 19 20 21 22 23

    24 25 26 27 28 29 30

    August 2017

    M T W T F S S

    July 31

    1 2 3 4 5 6

    7 8 9 10 11 12 13

    14 15 16 17 18 19 20

    21 22 23 24 25 26 27

    28 29 30 31 Sept 1

    Sept 2

    Sept 3

    Complete Week 1

    Complete Week 2

    Complete Week 3

    Complete Week 4

    Complete Week 5

    Sample Summer Assignment

    Calendar

    This is the suggested timeline for you to complete

    your AP Chemistry summer work. Notice that you

    have a week left at the end before school. This

    allows for some flexibility if your family goes on

    vacation or if you have other commitments at

    certain times during the summer. Plan ahead and

    plan wisely so you can get it done!

    Complete Week 6

    Complete Week 7

    Complete Week 8

    School Starts August 28!

  • Week #1

    Significant Figures 1. Give the number of sig figs in each of the following numbers:

    a. 123

    b. 0.078

    c. 89007

    d. 12,000

    e. 1,000,000,000.0

    f. 0.009

    g. 23,000.

    h. 34,000

    i. 34.89

    j. 101

    2. Do the following calculations giving the answer in the appropriate number of sig figs:

    a. 1.23 + 75

    b. 1.89 - .20

    c. 45.6 x 8.2

    d. 234/0.298

    e. 0.887 + 0.3

    f. 2340 - 100

    g. 12.45 x 3

    h. 25,600/ 3.0

    3. Do the following calculations giving the answer in the appropriate number of sig figs:

    a. 45.0 x 9.0 + 89.22/ 75

    b. (2.88 + .5) x ( 23,000 - 0.11)

    c. 0.8897 x 2.15 + 0.002/.1

    d. (8 + 9)/(34.0 – 20.)

    Dimensional Analysis 4. Convert the following measurements to the desired unit:

    a. 0.050 cm = ______ mm

    b. 1872 mg = _______ kg

    c. 1.9 dL = ________ cL

    d. 3.4x10-3 ks = ________ cs

    5. An aluminum block has a density of 2.70 g/mL. If the mass of the block is 24.60 g, find the volume of the substance. 6. A student can eat 4.0 M&Ms every 1.00 seconds. If an M&M has a mass of 63 mg, determine how many kilograms of M&Ms can be eaten by a class of 20 students in 3.75 hours.

  • Week #2 Naming Compounds

    Formula Name

    1. P4O10

    2. ZnBr2

    3. SBr6

    4. CaF2

    5. P2S3

    6. carbon monoxide

    7. sodium hydride

    8. aluminum selenide

    9. xenon hexafluoride

    10. dinitrogen monoxide 11. KClO3 12. Pb(OH)2 13. Ca(MnO4)2 14. N2O4 15. FeCl2

    16. manganese (VII) oxide

    17. francium dichromate

    18. copper (II) phosphide

    19. silver nitrate

    20. ammonium oxalate 21. (NH4)2SO3 22. Ni3(PO4)2 23. Fe(ClO2)3 24. NaBrO3 25. H3PO4

    26. sulfurous acid

    27. hydroiodic acid

    28. mercury (I) nitrate

    29. vanadium (V) oxide

    30. tetraphosphorous decoxide

  • Week #3 Atomic Structure

    1. Fill in the table below based on the given isotopes.

    Isotope Protons Neutrons Electrons 13C 31P

    232U

    Average Atomic Mass

    2. Given the data below determine the average atomic mass

    Isotope % Abundance Isotopic Mass

    Average Atomic Mass

    Question A. Sb-121 57.25% 120.9038 amu

    Sb-123 42.75% 122.0041 amu

    Question B. Ag-107 51.82% 106.90509 amu

    Ag-109 48.18% 108.9047 amu

    The Mole

    3. Convert each of the following to moles. a. 12.64 g NaOH b. 3.00 x 1024 atoms Au c. 40.0 L of Ne gas

    d. 800. g CaBr2 e. 3.011 x 1022 molecules H2O f. 6.78 L of Ar gas

    4. Given 0.250 moles of krypton determine: a. the mass

    b. the number of atoms

    c. the volume at STP

    5. Given 0.750 moles of oxygen determine” a. the mass

    b. the number of atoms

    c. the volume at STP

  • Percent Composition

    6. Calculate the perce