AP CHEMISTRY SUMMER ASSIGNMENT 2013
Flowing Wells High School
The AP Chemistry course is designed to be the equivalent of the general chemistry course
usually taken during the first college year. It is an extension of either Pre AP or Chem 1-2 you
have had in the past and will be adding a significant amount of content and knowledge to your
understanding of the subject.
Because AP Chemistry serves as a general chemistry course taken in college, a good
understanding of the topics discussed in Pre AP/ Chem. 1-2 is essential. To prepare for the
rigors of this course, you will be required to complete the worksheet which summarizes many of
the important topics of your previous chemistry class. Expect a quiz in the beginning of the
year school-year!
RESOURCES to help you:
For question 1-3 use this tutorial to help you (significant figures):
http://www.chem.sc.edu/faculty/morgan/resources/sigfigs/index.html
Here is some good website to get help on chemistry topic if you do not remember how to complete a
problem:
http://www.chemtutor.com/struct.htm
http://chemed.chem.purdue.edu/genchem/topicreview/index.php
http://chemistrylecturenotes.com/
On line class text ebook and resource site at
http://wps.prenhall.com/wps/esm_brown_chemistry_11
Username: eastapchem
Password: eastapchem12
Focus on chapter 1-3
ASSIGNMENT:
 Complete the assigned work on the next pages.
 These problems will be checked for completion on the first day of school.
 A quiz on this material will be given by the end of the second week.
 This assignment should take you approximately 3-4 hours to complete depending how
readily recourses are available.
Best of luck and cannot wait to see you next year!
Mr. Golden
william.golden@fwusd.org
AP CHEMISTRY SUMMER ASSIGNMENT 2013
Naming Compounds Flow Chart
NO
Does the Formula begin with H
YES
Does it begin with a metal which has more than
one oxidation number? (e.g.; Fe, Ni, Cu, Sn, Hg)
NO
YES
Name the first element
followed by its oxidation
number (Roman numeral)
Does the formula contain a polyatomic ion?
NO
YES
Are both elements nonmetals
NO
YES
Name the first element,
Then the second element
With the –ide ending.
It is an Acid (must be aqueous)
Does the acid contain a polyatomic ion?
YES
NO
Ending of polyatomic ion
-ate
-ite
Name the polyatomic
ion, replacing the –ate
ending with –ic. Add
the word acid.
Name the polyatomic
ion, replacing the –ite
ending with –ous. Add
the word acid.
Name the first element
using the proper prefix.
(never mono-). Name the
second element with the
proper prefix (including
mono- and –ide ending. )
1 mono2 di3 tr4 tetra5 penta6 hexa7 hepta8 octa9 nano10 decaName the first element, then the
polyatomic ion. If two elements
are present, name both, then the
polyatomic ion. (e.g.; NaHCO3
Is sodium hydrogen carbonate)
Write the prefix hydro, then
the name of the second
element with –ic ending.
Add the word acid
AP CHEMISTRY SUMMER ASSIGNMENT 2013
AP CHEMISTRY SUMMER ASSIGNMENT 2013
Short Answer
Each of the following is an example of some of the types of questions that you had answered while
in Chemistry. Please answer each of these questions, and show all work with appropriate units and
significant digits. A short quiz will be given on these problems once this sheet has been reviewed.
1.
The following length measurements were taken by students using several different measuring
devices. Find the average of the measurements. Make sure that your answer has the correct number
of significant figures. 10.05 cm, 10.1 cm, 9.741 cm, 10.6 cm, 10.5 cm
2.
How many significant figure are in the following numbers?
a. 2.34g
d.
10 000.0km
b. 0.0045mL
e.
3.21x10-45
c. 10 000km
f.
12.45x105
3.
Perform the following operation: 3.43 cm × 5.2 cm. Make sure that your answer has the correct
number of significant figures.
4.
5.
What is the temperature 128 K expressed in degrees Celsius?
6.
What is the volume of an object with a density of 7.73 g/cm3 and a mass of 5.4 × 102 g?
7.
A cube of a gold-colored metal with a volume of 59 cm has a mass of 980 g. The density of pure
gold is 19.3 g/cm3. Is the metal pure gold? Show calculations to justify your answer.
8.
List the number of protons, neutrons, and electrons in carbon-13.
9.
Consider an element Z that has two naturally occurring isotopes with the following percent
abundances: the isotope with a mass number of 19.0 is 55.0% abundant; the isotope with a mass
number of 21.0 is 45.0% abundant. What is the average atomic mass for element Z?
10. Which group of elements in the periodic table is known as the alkali metals?
11. Which group in the periodic table is known as the noble gases?
12. What is the electron configuration of sulfur?
13. From which orbital (s, p, d, or f) in lithium atom is an electron transferred to form Li+?
14. What orbital is filled when iodine gains an electron to become a negative ion?
15. In which group in the periodic table do the elements have the highest electronegativity values?
16. Draw the trend for electronegativity, radius of an atom, and melting point on the periodic table.
AP CHEMISTRY SUMMER ASSIGNMENT 2013
17. Name the Compound in column I and write the formula for column II
a) NH4I
a) Magnesium Fluoride
b) Fe2(SO3)3
b) Cesium Arsenate
c) H3PO4 (aq)
c) Boron (III) Silicate
d) AgClO3
d) Francium Nitrite
e) SnC2O4
e) Cobalt (II) Chloride
f) NaCN
f) Mercury (I) Permanganate
g) Zn(OH)2
g) Mercury (I) Fluoride
h) Rb2SiO3
h) Barium Phosphate
i) MnO2
i) Bismuth (III) Hydride
j) H2O2
j) Aluminum Borate
k) KCl
k) Gold Oxide
l) KC2H3O2
l) Copper (I) Hypochlorite
m) CaSO4
m) Tin (II) Chlorite
n) Sb2(Cr2O7)3
n) Phosphorous Pentachloride
o) Li3P
o) Lead (IV) Carbonate
18. Find the mass in grams of 3.10 × 1023 molecules of F2.
19. What is the percent composition of NiO, if a sample of NiO with a mass of 41.9 g contains 33.1 g Ni
and 8.8 g O?
20. Complete and balance the following equation.
Cd(NO3)2 + NH4Cl →
21. Write a balanced equation for the following:
Sodium chlorate undergoes decomposition to form sodium chloride and oxygen.
22. Write a balanced equation for the following reaction.
H3PO4(aq) + Ca(OH)2(aq) → Ca3(PO4)2(aq) + H2O(l)
23. If 8.00 mol of NH3 reacted with 14.0 mol of O2, how many moles of H2O will be produced?
4NH3(g) + 7O2(g) → 4NO2 + 6H2O(g)
24. If 5.0 g of H2 are reacted with excess CO, how many grams of CH3OH are produced, based on a
yield of 86%? CO(g) + 2H2(g) → CH3OH(l)
25. A mixture of gases at a total pressure of 95 kPa contains N2, CO2, and O2. The partial pressure of the
CO2 is 24 kPa and the partial pressure of the N2 is 48 kPa. What is the partial pressure of the O2?
26. Determine the oxidation number of each element in the following compound: HMnO4.
AP CHEMISTRY SUMMER ASSIGNMENT 2013
27. For H2SO4, determine the following:
a. A Lewis Structure
d. The molecular geometry
e. The polarity of the molecule.
f. Draw any and all possible resonance structures
28. Calculate the molar heat of vaporization (∆H) of a substance if 0.433 mol of the substance absorbs
4.307 kJ when it melts.
29. Calculate the energy released by freezing 26.6 g of a liquid. Its molar mass is 82.9 g/mol and its
molar heat of fusion is 4.60 kJ/mol.
30. 50.0 g of a metal at 100.0 °C is placed into 20.0 grams of water at 30.0 °C. After mixing, the
temperature is 57.0 °C. What is the specific heat of the metal?