Welcome to AP Chemistry!
Students enrolled in AP chemistry will be asked to reinforce skills and knowledge accumulated in the
first year chemistry class (Honors Chemistry) during the summer before the beginning of the AP
course. This will allow us to focus our attention on the advanced chemistry topics and 16 suggested
labs that will be tested on the AP exam in May 2016.
Your summer assignment consists of the following:
1. Set up the AP Chemistry Lab Notebook. Directions are given on page 2. This lab
notebook is due on Monday, August 24th, 2015.
2. Review the objectives taught in Chemistry Honors for the Atomic Structure &
Periodicity, Stoichiometry and Chemical Reactions units. A diagnostic exam to test
your readiness for AP Chemistry will be given the second day the class meets.
3. Review the Solubility Rules, Polyatomic Ions, Strong Acids and Bases, and General Rules
for Completing Chemical Equations (all attached). A quiz will be given on the second
week of school.
4. Create an Appendix for your AP Chemistry Lab Notebook with names, pictures, uses
and procedures of the most common equipment and apparatuses that will be use in the
course. (page 4) due on Monday, August 24th, 2015.
5. Optional, yet strongly recommended: Purchase “5 Steps to a 5: AP Chemistry” 2016, 8th
Edition by John Moore and Richard Langley, McGraw Hill ISBN-13: 978-0071850315 /
ISBN-10: 0071850317
6. http://www.amazon.com/Steps-Chemistry-Advanced-PlacementExaminations/dp/0071850317/ref=sr_1_2?s=books&ie=UTF8&qid=1432141242&sr
=1-2&keywords=5+steps+to+a+5+ap+chemistry+2016
Take the diagnostic exam without much review or looking up answers – see how you
would perform before taking the course.
7. Print out the assignment included in this document, starting on page 5 and answer ALL
questions in the space provided. Assignment due on Friday, August 28th, 2015.
Please take the assignment seriously and start in early August—there’s a lot to do and you won’t be
able to complete it all on the night before it’s due!
If at any time you would like to ask me a question, please email me at
[email protected]. Have a great summer. I look forward to beginning our journey
together in August.
Mrs. Minsal 
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Setting Up Your AP Chemistry Laboratory Notebook
Due Monday, August 24th, 2015
The laboratory activities are comprised of “hands-on” labs so the students can accomplish multiple
trials and can use statistical analysis to derive conclusions. Students are required to have a bound
student laboratory notebook which will be used as their lab portfolio. For each lab, students
complete a lab report that includes replicated data tables and answers to the post lab discussion.
1. The AP Chemistry Laboratory notebook must be bound and preferentially Quadrille Ruled.
Acceptable lab notebooks can be purchased at office supply stores or online. Acceptable
notebooks are marble composition notebooks or ones that are specifically made for lab
notebooks
2. Your lab notebook is your chemistry diary. You must make entries in ink, only. If you make
a mistake, draw a SINGLE line through the error, initial it, and continue.
3. Before any entries are made, each page in the lab notebook must be numbered, beginning
with page 1.
4. Page 1 will be a table of contents containing the title of labs, the page on which the lab
begins, and the page on which the lab ends. Please set the headings up. For example:
“ Chromatographic study of colored compounds” …………………………………..14-27
5. Now that you have completed the setup process, here are some things you need to know
about how we will enter data into our lab notebooks:


We will only have writings on the front page.
Every lab will have the following format in this order:
 Title of the experiment, date of the experiment.
 begin with answers to Pre-lab questions
 Procedure from your laboratory manual or handout lab sheet. Graphic organizers
and images are encouraged. If procedures are changed, the changes must be
included in the report. You do not need to re-type the procedure, instead, you can
cut and paste the procedure given to you.
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 Data Collection tables are created to show the gathered data both, qualitative and
quantitative, in an organized manner. Either create your own table or cut and paste
from lab handout or manual.
 Calculations that are made must be recorded, with all calculations, including
formulas and work, in a neat, organized manner.
 Argumentation and Documentation where you discuss, explain, conclude, and
suggest ways to improve the experiment.
 at the end of the lab, the answers to Post-lab questions must be recorded.
6. At no time will there be any "I" or any first person references in it. Use passive voice. The
lab notebook is for recording data and observations, not for sharing personal opinions or
inferences. For example: “The analysis of the data gathered indicates that the compounds experience
similar chemical and physical properties and therefore they must belong to the same family. Furthermore, …”
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Appendix. As any Appendix, this one goes at the end of the notebook.
Part One: Identifying Laboratory Equipment (38 points) due on Monday, August 24th, 2015.
Create a table containing the name, picture, and function of the following pieces of lab
equipment:
Beaker
Filter Flask
Stirring Rod
Buchner Funnel
Funnel
Test Tubes
Buret
Gooch Crucible
Test Tube Rack
Buret Clamp
Graduated Cylinder
Test Tube Holder
Clamp
Mortar and Pestle
Tongs


Ring
Universal
Condenser
Crucible and Cover


Pipette



Beral-type
Graduated
Volumetric
Crucible
Beaker
Volumetric Flask
Wash Bottle
Clay triangle
Pipette Bulb
Watch Glass
Cuvet
Ring Stand
Wire Gauze
Dessicator
Round Bottom Flask
Erlenmeyer Flask
Rubber Policeman
Eudiometer Tube
Spatula
This can either be typed on separate sheets or handwritten directly in the notebook. Pictures can be
drawn or cut and paste from other sources.
Part Two: Laboratory Apparatuses and Procedures (14 points)
Use words and diagrams to describe the following:
o The proper way to fold filter paper.
o Apparatus for heating liquids in beaker over a flame.
o Apparatus for heating liquids or solids in a test tube over a flame.
o Rank glassware for measuring volume from most precise to least precise.
o The process for making solutions.
o The correct way to dilute acids and an explanation as to why.
o The proper way to prepare a burette for titration.
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Name: __________________________________
AP Chemistry
Date: _____________________________
Mrs. Minsal
Due on Friday, August 28th, 2015.
Directions: Answer the following five questions in the spaces provided.
1.
a) Write the ground state electron configuration for a selenium atom, showing the number of electrons
in each subshell.
__________________________________________________________________________
b) Predict the charge on the selenium ion. _________________________________________
c) Write the ground state electron configuration for a selenium ion, showing the number of electrons in
each subshell.
___________________________________________________________________________
d) Is an isolated selenium atom in the ground state paramagnetic or diamagnetic? Explain briefly.
________________________________________________________________________
________________________________________________________________________
_______________________________________________________________________
e) Explain how the electron configuration of the selenium atom in the ground state is consistent with
the existence of the following known compounds: Na2Se, SeCl2.
_________________________________________________________________________
__________________________________________________________________________
__________________________________________________________________________
__________________________________________________________________________
__________________________________________________________________________
2. Explain each of the following observations using principles of atomic structure and/or bonding.
a) Potassium has a lower first-ionization energy than lithium.
__________________________________________________________________________
__________________________________________________________________________
__________________________________________________________________________
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b) The ionic radius of N3- is larger than that of O2-.
____________________________________________________________________________
_____________________________________________________________________________
_____________________________________________________________________________
c) A calcium atom is larger than a zinc atom.
_____________________________________________________________________________
_____________________________________________________________________________
_____________________________________________________________________________
3.
a) Calculate the volume of 8.20 M H2SO4 that can be completely neutralized with 15.6 grams of sodium
bicarbonate NaHCO3.
b) The molarity of nitric acid is to be determined using titration. A 25.00 mL sample of the acid is titrated
with 0.100 M of barium hydroxide. The equivalence point was achieved with 48.6 mL of the base.
Calculate the molarity of the nitric acid.
c) What is the pH of the nitric acid?
4. Answer the following questions about MgSO4 (s) and its hydrate.
a) Calculate the mass percent of sulfur in the hydrated form of the solid that has the formula MgSO4 ∙ 7
H2O
b) When heated to 310.°C, MgSO4 ∙ 7 H2O (s) dehydrates completely as represented below.
MgSO4 ∙ 7 H2O (s) —> MgSO4 (s) + 7 H2O(g)
If 5.48 g of MgSO4 ∙ 7 H2O (s) is heated to 310.°C, calculate
i.
the mass of MgSO4 (s) formed, and,
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ii.
the volume of the H2O(g) released, measured at 310.°C and 740 mm Hg.
5. A 2.00 x 10-3 mole sample of pure acetylsalicylic acid (a monoprotic acid) was dissolved in 15.00 mL of
water and then titrated with 0.100 M NaOH(aq). Calculate:
a) The molarity of the acetylsalicylic acid.
b) The number of molecules of acetylsalicylic acid in the solution before titration.
c) The volume of NaOH required to react with the acid.
6.
Fe(s) +
O2(g) —> Fe2O3(s)
Iron reacts with oxygen to produce iron(III) oxide, as represented by the equation above.
A 65.0 g sample of Fe(s) is mixed with 10.7 L of O2(g) at 2.15 atm and 298 K.
a) Calculate the number of moles of each reactant before the reaction begins.
b) Identify the limiting reactant when the mixture is heated to produce Fe2O3(s). Support your answer
with calculations.
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c) Calculate the number of moles of Fe2O3 (s) produced when the reaction proceeds to completion.
7. For the molecules below
i.
Draw the Lewis structure
ii.
State the molecular symmetry
iii.
State the strongest intermolecular force present between the molecules of the same compound.
a) CF4
i
ii
iii
i
i
i
b) NCl3
c) H2O
d) CH3OH
ii
iii
ii
iii
ii
iii
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Polyatomic Ion Names
Must be memorized by the first day of school!
1+
ammonium, NH4+
hydronium, H3O+
1acetate, C2H3O2-, or CH3COO perchlorate, ClO4chlorate, ClO3chlorite, ClO2hypochlorite, ClOcyanide, CNhydrogen carbonate, HCO3- (also called bicarbonate)
hydrogen sulfate, HSO4hydroxide, OHnitrate, NO3nitrite, NO2permanganate, MnO4thiocyanate, SCN 2carbonate, CO3 2chromate, CrO4 2dichromate, Cr2O7 2oxalate, C2O4 2peroxide, O2 2sulfate, SO4 2sulfite, SO3 2thiosulfate, S2O32-
Strong Acids
HCl
HBr
HI
H2SO4
HNO3
HClO4
HClO3
3phosphate, PO4 3phosphite, PO3 3arsenate, AsO4 3-
Strong Bases.
Group I hydroxides (LiOH, NaOH, KOH, etc)
Ca(OH)2
Sr(OH)2
Ba(OH)2
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Solubility Rules
1. All compounds that contain a group I element (alkali metal) are soluble.
2. All compounds that contain an ammonium ion (NH4+) are soluble.
3. All compounds that contain a nitrate ion (NO3-) or acetate ion (C2H3O2-) are soluble.
4. All compounds that contain a group VII element (halogen) are soluble except those halides that contain
Ag+, Hg+, or Pb2+. (This one is not perfect, check out the fluorides in the chart below.)
5. All compounds that contain a sulfate ion (SO42-) are soluble except that that contain Ba2+, Sr2+, or
Pb2+.
6. All other compounds are INSOLUBLE.
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