AP Chemistry Summer Assignment 2013-2014
1. Read over Course Requirements, Expectations, and Grading Procedures.
2. The syllabus for the AP Chemistry course will be available in the summer
assignment folder by the end of July.
3. The periodic table that is used on the AP Exam is included in this packet. You
will see that only the symbols of the elements are provided!! This means that you
must memorize the name of the element that corresponds to each symbol for
elements with atomic numbers 1-95.. The periodic table that you used in Year I
chemistry has the names and symbols of the elements. A copy of this table is
available in the Summer Assignment folder.
4. On the back of the periodic table you will find a list of common ions. These are
not provided on the AP Exam so you must memorize the symbol and charge for
each ion that appears on this sheet. You must also memorize the numerical
prefixes that are listed on page 63 of the text book.
5. Complete the Chapter 1 & 2 Summer Assignment that is included in this
packet. No written work is required but a test will be given on this information.
6. Complete the Chapter 3 Stoichiometry Summer Assignment that is included
in this packet. *All work will be collected on the first day of class. * Please
follow these guidelines as you complete the assignment:
a. The work must be completed in the order given.
b. Label each problem with the exercise number and the page number if the
problem is from the text book.
c. Neatness counts!! If I can’t read it easily, I will assume that it is wrong.
d. You must show your work.
e. Circle answers and label answers with appropriate units.
f. Answers should reflect the correct number of significant digits. You
should be within one digit of the correct number of significant digits.
7. Read pages 223-248 and complete the Chapter 7 Periodic Table Reading
Assignment.
8. Please cover your text book(new textbooks will be provided at the start of the
school year).
AP Chemistry
Course Requirements
1. You must put a book cover on your text and keep it covered for the remainder of the year. Do not
store handouts in your book, as it will break the binding. If you lose the book, you must pay for it
before I can issue a new one to you.
2. You must have a folder/notebook in which you keep class notes, homework assignments, and
handout sheets. A three ring binder is strongly recommended since you will receive numerous
handouts!
3. You must have a calculator that you know how to operate.
4. You must bring items 1-3 to class every day, including lab day. Failure to do so may result in
loss of credit if these items are needed to complete class assignments!!
Student Expectations
1. Be on time for class. Remember 3 unexcused tardies = 1 unexcused absence. If you need to
return to your locker to get your book, homework, etc. you will still receive a tardy if you are not in
the classroom when the bell rings.
2. Ask questions in class and/or seek extra help if you do not understand the subject material. Review
the subject material on a daily basis rather than waiting until the night before the test.
3. Arrangements to complete work missed due to excused absence should be made as soon as you
return to school. If the work is not made up within the allotted time (2 days for every one day
absent) 0% will result. In the case of school required absences arrangements should be made
before you leave as the work is due when you return. If you know that you will be absent from
class (other than school required absences) and would like assignments ahead of time, the request
must go through the main office so please plan well in advance.
Grading Procedures
1. Grades will be based on the following:
Tests, Quizzes: 70%
Labs: 20%
Homework: 10%
2. In order to receive credit for assignments all answers must be legible. Homework may be
collected, checked in class or reviewed during class. Homework that is collected or checked will
be accepted only at the beginning of class on the date it is due. If you are absent it is your
responsibility to show me the work on the day that you return. If you fail to do so a 0% will
be given.
3. In order to receive full credit for lab reports, you must follow the proper procedure for writing up
the lab and it must be legible. Labs will be accepted one day late but you will be penalized one
letter grade. If you are absent on lab day, you will be given a copy of the lab with a set of data
that you must use to complete the lab report. You must maintain a portfolio of all labs that you
complete.
4. All tests and quizzes will be announced in advance. All quizzes/tests missed due to excused
absence must be made up as soon as you return to school.
5. If you miss work due to excused absence it is your responsibility to see me about making up this
work.
6. If you are caught copying any assignment, you will receive a 0% as will your collaborator
who is supporting your laziness. The same applies if caught cheating on a quiz or a test.
Some Common Ions
Cations
Anions
ammonium
NH4+
acetate
C2H3O2─
copper (I)
Cu+
chlorate
ClO3─
silver
Ag+
chlorite
ClO2─
cadmium
Cd2+
cyanide
CN─
chromium (II)
Cr2+
hydroxide
OH─
cobalt (II)
Co2+
hypochlorite
ClO─
copper (II)
Cu2+
nitrate
NO3─
iron (II)
Fe2+
nitrite
NO2─
lead (II)
Pb2+
perchlorate
ClO4─
permanganate
MnO4─
manganese (II) Mn2+
`
mercury (I)
Hg22+
carbonate
CO32─
mercury (II)
Hg2+
chromate
CrO42─
nickel (II)
Ni2+
dichromate
Cr2O72─
tin (II)
Sn2+
peroxide
O22─
zinc
Zn2+
sulfate
SO42─
aluminum
Al3+
sulfite
SO32─
chromium (III) Cr3+
phosphate
PO43─
Fe3+
phosphite
PO33─
iron(III)
Certain polyatomic anions having charges of “2─” or “3─” may combine with one or more H+ ions. When only one hydrogen
is present, the ion is most simply named by using the prefix bi or just write hydrogen before the ion’s regular name. If two
hydrogens are present, dihydrogen is used as a prefix.
AP Chemistry Chapters 1 & 2 Summer Assignment
*****Written work IS NOT required for this assignment.*****
Chapter 1 Introduction: Matter and Measurement
1. Read pages 1-18 and 21-30.
2. Review the following Exercises on pages 31-33:
3,5, 6, 11,13,15,21,23,25,27,29c,31,33,34,35,37,38,39,41,54,55
The answers for most of these are provided in the back of the text book.
Answers to exercises not given in the text book:
6. Add mixture to water, filter and then distill.
34. (a) 5 (b) 2 (c) 5 (d) 4 (e) 6
38. (a) -2.3 X 103
(b) 8.260 X 107
(c) 3.4 X 104 (d) 7.62 X 105
55. Density, temperature and color are intensive properties.
3. Convert the following measurements:
a. 156 m2 to km2
(Answer: 1.56 X 10-4 km2)
3
b. 385 mL to dm
(Answer: 0.385 dm3)
c. 4.56 X 105 cm3 to m3
(Answer: 4.56 X 10-1 m3)
4. You must memorize the SI prefixes (omit femto) in Table 1.5 on page 15 and the volume relationships
in Figure 1.19 on page 17.
Chapter 2 Atoms, Molecules, and Ions
1. Read pages 37-64 and review the Naming Compounds Writing Formulas PowerPoint slides found in the
Summer Assignment folder on my website..
2. Review the following exercises on pages 65-68:
1,5,7,9,13,15,1719,21,23,25,29,31,33,39,43,45,47,49,51,54,60, and 68.
The answers are provided in the back of the text book.
Chapter 1 and 2 Objectives (on the back of this sheet)
Read over the objectives as you are responsible for each of these.
A test, based on this assignment and on the Chapter 1 and 2 objectives listed on the back
of this sheet, will be given when you return to class. You will have an opportunity to ask
questions on this material prior to taking the test.
AP Chemistry Chapter 1 and 2 Objectives
After completing Chapter 1 and Chapter 2 (pp. 37-55) the student should be able to:
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Differentiate between the three states of matter.
Understand the difference between elements, compounds, and mixtures.
Describe techniques used to separate components of a mixture.
Distinguish between physical and chemical properties and changes.
Define intensive and extensive property and provide an example of each.
Be familiar with the units of the metric system of measurement and be able to convert
measurements within the metric system by using dimensional analysis.
Determine the number of significant figures in a measurement and be able to express the
results of a calculation with the proper number of significant figures.
Distinguish between precision and accuracy.
Convert temperatures between the Celsius and Kelvin scales.
Perform calculations involving density.
State Dalton’s atomic theory.
State the law of constant composition and the law of conservation of mass.
Be familiar with the experiments of Thomson, Millikan, and Rutherford.
Distinguish between protons, neutrons, and electrons, and be able to describe the composition
of an atom of any particular element in terms of these subatomic particles.
Write the chemical symbol for an element, having been given its mass number and atomic
number, and perform the reverse operation.
Know the difference between an atom, an ion, and a molecule.
Write the symbol and charge for an atom or ion having been given the number of protons,
neutrons, electrons and perform the reverse operation.
Have a basic knowledge of the periodic table, which includes being able to predict whether an
element is a metal, nonmetal or metalloid, and what will be the probable charge of its ion.
Distinguish between empirical, molecular, and structural formulas.
Write the names and the formulas of inorganic compounds (ionic, acids, binary molecular).
AP Chemistry Chapter 3 Stoichiometry Summer Assignment
*****Written work IS required for this assignment.*****
***All work will be collected on the first day of class.***
Review of Year 1 Stoichiometry
Read pages 71-98 and study the Stoich PowerPoint slides found in the Summer Assignment folder on my
website BEFORE you begin this assignment. Study the Sample Exercises BEFORE you attempt each of the
exercises assigned below.
Show all work for each exercise and circle your final answer. Label all answers with appropriate units.
Exercises must be completed in the order assigned and you need to include the page and number for each
exercise that you complete.
No credit will be given if your work does not support your final answer. All answers are in the back of the text
book or are provided below. ***All work will be collected on the first day of class.***
Calculating Average Atomic Mass
Study Sample Exercise 3.4 on page 79 and then complete exercises 15 and 16 on page 100.
for #16: 24.32 amu)
(Answer
Calculating Percent Abundance
Study the Sample Problem and then complete the two problems listed below it.
Sample Problem:
Chlorine is made up of two isotopes, Cl-35 atomic mass = 34.969 amu and Cl- 37 atomic mass = 36.966
amu. Given chlorine’s atomic weight of 35.453, what is the % abundance of each isotope?
34.969(x) + (36.966) (1-x) = 35.453
34.969x + 36.966 – 36.966x = 35.453
x = .7576
75.76% Cl-35 and 24.24% Cl-37
1. Calculate the percent abundances of copper-63 and copper-65 if the atomic weight is 63.54 amu and the
exact mass of the isotopes are: copper-63, 62.93 amu and copper-65, 64.93 amu. Assume that no other
isotopes exist. (Answer: 69.5% Cu-63, 30.5% Cu-65)
2. Antimony has two stable isotopes: Sb-121 has a mass of 120.90 amu and Sb-123 has a mass of 122.90
amu. Calculate the percent abundances of the two isotopes. The atomic weight of Sb is 121.75 amu.
(Answer: 57.5% Sb-121, 42.5% Sb-123)
Formula and Molecular Weights
Study Sample Exercise 3.5 on page 80 and then complete exercises 17 c and d on page 100.
Percentage Composition
Study Sample Exercise 3.6 on page 80 and then complete exercises 19 b, c, and d on page 100.
The Mole
Study Sample Exercises 3.7 through 3.11 on pages 82-86 and then complete exercises 27, 29, and 37 on page
101.
Empirical and Molecular Formulas
Study Sample Exercises 3.12 and 3.13 on pages 87-89 and then complete exercises 41, 45, and 51 on pages
101-102.
Quantitative Information from Balanced Equations
Study Sample Exercises 3.14 and 3.15 on pages 92-93 and then complete exercise 59 on page 102.
Limiting Reactants
Study Sample Exercises 3.16 and 3.17 on pages 95-96 and then complete exercise 67 on page 102.
Theoretical Yield and Percent Yield
Study Sample Exercise 3.18 on pages 97-98 and then complete exercise 73 on page 103.
A test based on this material will be given when you return to school. You will have an
opportunity to ask questions on this material before the test is given.
AP Chemistry Chapter 7 Periodic Table Reading Assignment
Name _____________________
A test based on this material will be given when you return to school. You will have an
opportunity to ask questions on this material before the test is given.
1.
What scientist was responsible for the concept of atomic number? ______________________
How did he determine the atomic numbers?
2. How does atomic radius vary:
a. Within a group _____________________________________________ EXPLAIN.
b. Within a period _____________________________________________ EXPLAIN.
c. Referring to Figure 7.5, describe the atomic radius trend (left to right) for the transition elements.
Suggest a reason for this trend.
3. Define ionization energy.
4. How does ionization energy vary:
a. In a group? ____________________________________________________ WHY?
b. In a period? ____________________________________________________ WHY?
5. When successive electrons are removed from an atom, at a certain point there is a large jump in
ionization energy. How can you predict when this will occur (at the removal of which electron)?
6. Define electron affinity.
7. What is meant by the term METALLOID?
List the elements that are classified as metalloids.
8. List the common name for each of the following groups:
1A_______________________
2A _______________________
7A ________________________
8A ________________________
9. How does metallic character vary on the periodic table across a period?
How does metallic character vary on the periodic table down a group?
10. Where are the most reactive metals located?
11. Where are the most reactive nonmetals located?
12. Use the details of modern atomic theory to explain each of the following experimental observations.
a. Within a family (group) such as the alkali metals, the ionic radius increases as the atomic number
increases.
b. The radius of the chlorine atom is smaller than the radius of the chloride ion, Cl- (Radii: Cl atom
= 0.99Å; Cl- ion = 1.81 Å).
c. The first ionization energy of aluminum is lower than the first ionization energy of magnesium.
d. For magnesium, the difference between the second and third ionization energies is much larger
than the difference between the first and the second ionization energies.