AP Chemistry Summer Assignment
Paul Blazer High School
Mr. Imel
justin.imel@ashland.kyschools.us
Congratulations on taking AP Chemistry at Paul Blazer High School!
This course is designed to be the equivalent of the general chemistry course taken during the first
college year. For some students, this course enables them to undertake, as a freshman, second-year
work in the chemistry sequence at their institution or to register for courses in other fields where
general chemistry is a prerequisite.
Your summer assignment has a dual purpose. 1) The chapter’s you’ll read and the material you’ll
learn/memorize will make the remainder of this year’s course work run much more smoothly if you
know it before we meet. 2) This course is meant to simulate a college chemistry course. Therefore your
study habits and responsibility should reflect that of a college student. Your results on the first week’s
tests will allow me to gauge the amount of time and energy you have given this assignment. All of the
information for the summer assignment should be considered review material from your general
chemistry course.
Text:
Brown, Theodore E.; Lemay, H. Eugene; Bursten, Bruce E.; Murphy, Catherine; Woodward, Patrick
(2008), Chemistry: The Central Science (11th ed.), New York: Prentice-Hall, ISBN 0136006175
Summer Assignment:
Over the summer, you should read Chapters 1 and 2 of your AP Chemistry text and complete the
following questions in preparation to begin class. This assignment is due the first day of school,
WEDNESDAY, AUGUST 12, 2015.
Chapter 1 Questions (40 POINTS)
Beginning on page 30: 1, 2, 5, 11, 13, 15, 19, 21, 23, 26, 28, 35, 37, 39, 43, 53, 57, 61, 67, 74
Chapter 2 Questions (60 POINTS)
Beginning on Page 70: 4, 6, 7, 13, 19, 21, 22, 23, 24, 26, 31, 33, 35, 37, 40, 41, 43, 49, 53, 57, 60, 61, 66,
68, 70, 71, 73, 79, 87, 104, 106
Periodic Table:
In addition to the summer assignment, you should become quite familiar with the most useful tool
in Chemistry… the periodic table. It is your responsibility to review the periodic table and be familiar
with: symbols and locations of common elements (#’s 1-36, and groups 1A, 2A, 7A, and 8A), atomic
number, atomic mass, and periodic table trends (atomic radius, ionic radius, electronegativity, first
ionization energy). You should also be able to tell an element’s number of valence electrons by its
position on the periodic table. There are many good websites to help you with this information. Also,
you may use your book.
Memorization and Application Materials:
AP Chemistry is a challenging course. It is not all about memorization; however, having these items
memorized is essential for success in learning the concepts covered in this course. Make flashcards,
have your friends and family quiz you, take the lists with you on vacation, or do whatever it take to get
the information firmly planted in your head. Do not wait until the night before school begins. The first
tests will cover four areas of memorization. Handouts are provided with the expected information.
These tests will be given the first full class period of the new school year. You should arrive your
first day ready to test on all of this information. Total value= 100 POINTS.
1. Common Polyatomic Ions
 Test format will have the ions rearranged from the format given on the handout. If the
formula is given, you must provide the correct name (be careful of –ite vs. –ate); if the
name is given you will provide the correct formula and charge (make sure the charges
are superscripts and the number of atoms of each element are subscripts)
2. Variable Valances for Metal Ions
 Test format will have the ions rearranged from the format given on the handout. If the
formula is given, you must provide the correct stock name; if one name is given you will
provide the correct symbol and charge and the other name
3. Rules for Naming Acids
 Questions about the rules will be asked
 Formulas of various acids will be given and you will provide the name of the acid; if the
name is given, you should provide the correct acid formula
4. Rules for Naming Ionic Compounds and Molecular Compounds
 You will be given 2 elements or ions (monatomic and polyatomic). You will provide the
name of the compound formed from the given elements/ions. If given an ionic or
molecular compound name or formula, you should be able to identify the ions present
(formula and charge).
These tests may require the first days of class, but learning the information ahead of time will make
the remainder of the year more manageable. If you are confused by any information or need any help,
please email me. I will check my email daily and will respond as soon as I receive your e-mail. Please
realize though, that I too am on summer break and I may not check my mail again until the next day if I
have already responded to emails for that day.
I look forward to seeing you next year.
Mr. Imel
1. Common Polyatomic Ions
Name
Formula
Dihydrogen phosphate H2PO4-1
Acetate
C2H3O2-1
Hydrogen sulfite
HSO3-1
Hydrogen sulfate
HSO4-1
Hydrogen carbonate
HCO3-1
Nitrite
NO2-1
Nitrate
NO3-1
Cyanide
CN-1
Hydroxide
OH-1
Permanganate
MnO4-1
Hypochlorite
ClO-1
Chlorite
ClO2-1
Chlorate
ClO3-1
Perchlorate
ClO4-1
Hydrogen phosphate
HPO4-2
Oxalate
C2O4-2
Sulfite
SO3-2
Sulfate
SO4-2
Carbonate
CO3-2
Chromate
CrO4-2
Dichromate
Cr2O7-2
Silicate
SiO3-2
Phosphite
PO3-3
Phosphate
PO4-3
Ammonium
NH4+1
2. Variable Valances for Metal Ions
Symbol
Stock Name
Cu+1
Copper (I) ion
Cu+2
Copper (II) ion
Fe+2
Iron (II) ion
+3
Fe
Iron (III) ion
Hg2+2
Mercury (I) ion
+2
Hg
Mercury (II) ion
Pb+2
Lead (II) ion
+4
Pb
Lead (IV) ion
Sn+2
Tin (II) ion
+4
Sn
Tin (IV) ion
Cr+2
Chromium (II) ion
+3
Cr
Chromium (III) ion
Mn+2
Manganese (II) ion
+3
Mn
Manganese (III) ion
Co+2
Cobalt (II) ion
+3
Co
Cobalt (III) ion
3. Rules for Naming Acids
Acids are compounds that produce an H+1 when dissolved in water.
 Rule 1: HnX
 -X is an anion ends in –ide
 -hydro (stem) ic acid
 Rule 2: Polyatomic anion name ends in –ite
 Change -ite to –ous
 Stem –ous acid
 Rule 3: Polyatomic anion ends in –ate.
 Change ending to ic
 Stem – ic acid
4. Rules for Naming Ionic and Molecular Compounds
Naming Ionic Compounds
 To name, place the cation name first, followed by the anion name.
Examples: LiF, Lithium Fluoride; KOH, Potassium Hydroxide
Naming Binary Molecular Compounds
 Name the elements in the order listed in the formula.
 Use prefixes to indicate the number of each kind of atom.
Prefix
Mono- DiTriTetra- Penta- Hexa- Hepta- Octa- Nona- DecaNumber 1
2
3
4
5
6
7
8
9
10
 Omit the prefix mono- when the formula contains only one atom of the first element in the
name.
 The suffix of the name of the second element is -ide.
Examples: CO2, Carbon dioxide; SF6, Sulfur hexafluoride