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Name: _____________________________
AP Chemistry – Summer 2018 Work Packet
Directions – Print Out TWO things:
1) This PACKET (single-sided)
2) The FLASHCARDS (double-sided)
Each section of this packet contains 3 parts:
EXPECTATIONS: Be sure to read this section completely. These are topics and/or skills which were
previously covered during your Honors Chemistry/Summer Chemistry course that you are expected to
know. AP Chemistry will cover these topics/skills in more depth, so having a good understanding of
them prior to the start of the course is in your best interest.
RESOURCES: This sections list links to online resources you can reference Should you find that you
need some additional help with topics on listed on this page.
PRACTICE PROBLEMS: These problems are meant to help you practice the skills you have already
learned in your previous Chemistry course. Make sure to read the directions provided for each set of
problems and to answer ALL the problems provided. If you need more space to show your work, do so
on the backside of each page.
This packet will be collected on the FIRST DAY OF CLASS
and count as your first assignment.
You will be tested on the topics listed in the “EXPECTATIONS”
sections of this packet on the SECOND DAY OF CLASS.
You will be tested on nomenclature EVERY CLASS for at least the 1st month of this course.
SSeeccttiioonn OOnnee:: AAttoommiicc SSttrruuccttuurree && CChheemmiiccaall NNoommeennccllaattuurree
EXPECTATIONS
Calculate average atomic mass and natural
abundance
Find the numbers of subatomic particles for a
given atom
Identify elements given atomic symbol
Memorize common ions
Memorize polyatomic ions
Nomenclature (formula standardized names
& standardized names formula)
o Binary ionic compounds
o Binary molecular compounds
o Acids
RESOURCES
How To Calculate Avg. Atomic Mass: https://www.youtube.com/watch?v=r5JO8aeYy0E
How To Calculate Abundances: https://www.youtube.com/watch?v=QVP1Z2ESCI0
How To Find The Number of Subatomic Particles: https://www.youtube.com/watch?v=G3ImfVYSxoc
Acid Nomenclature: https://www.youtube.com/watch?v=5Jb2u9ihfm4
Finding Binary Ionic Compound Chemical Formulas: https://www.youtube.com/watch?v=URc75hoKGLY
Finding Binary Molecular Compound Chemical Formulas: https://www.youtube.com/watch?v=DFw3AW2BFUw
Naming Binary Ionic Compounds: https://www.youtube.com/watch?v=CkCzceecCrc
Naming Binary Molecular Compounds: https://www.youtube.com/watch?v=NJn76CR70oU
AP Exam Periodic Table & Element Name, Common Ion, Polyatomic Ion Flash Cards: see email for other
attachments
PRACTICE PROBLEMS
Directions: For each problem, fill in all empty cells in the chart. When calculating average atomic mass or natural abundance, show your work in the space provided or a separate sheet of paper. When writing symbols, include both the mass number and the atomic number. If an isotope’s natural abundance is “trace” assume that this is 0.
Isotope Mass
Number
# of
protons
# of
neutrons
Atomic
number
Symbol Natural
Abundance
Atomic Mass
(amu)
Atomic
Weight (amu)
Carbon-12 12 98.90 12 (exactly)
Carbon-13 13 1.10 13.003
Carbon-14 14 trace 14.003
Isotope Mass
Number
# of
protons
# of
neutrons
Atomic
number
Symbol Natural
Abundance
Atomic Mass
(amu)
Atomic
Weight (amu)
Oxygen-16 16 15.994
15.9994 Oxygen-17 17 16.999
Oxygen-18 18 0.200 17.999
SECTION ONE - PRACTICE PROBLEMS PAGE 2
Isotope Mass
Number
# of
protons
# of
neutrons
Atomic
number
Symbol Natural
Abundance
Atomic Mass
(amu)
Atomic
Weight (amu)
Zirconium-90 51.45 89.904
Zirconium-91 11.22 90.905
Zirconium-92 17.15 91.905
Zirconium-94 93.906
Zirconium-96 2.80 95.908
Isotope Mass
Number
# of
protons
# of
neutrons
Atomic
number
Symbol Natural
Abundance
Atomic Mass
(amu)
Atomic
Weight (amu)
Copper-63 63 62.929
63.546 Copper-65 65 64.927
Directions: If given the chemical formula, provide the chemical name. If given the chemical name, provide the chemical
formula. (Cl = chlorine)
1. BeCl2 _____________________________________
2. NO2 _____________________________________
3. Fe2S3 _____________________________________
4. HCl _____________________________________
5. Ca(OH)2 ___________________________________
6. HNO3 _____________________________________
7. CH4 _____________________________________
8. Phosphorus pentabromide ____________________
9. Iron (II) bromide ____________________________
10. Hydrofluoric acid ____________________________
11. Manganese (V) Oxide ________________________
12. Tin (II) nitrate _______________________________
13. Sulfuric acid ________________________________
14. Strontium hydroxide ________________________
SSeeccttiioonn 22:: CChheemmiiccaall RReeaaccttiioonnss && SSttooiicchhiioommeettrryy
EXPECTATIONS
Find empirical and molecular formulas
when given chemical analysis information
Balancing chemical equations
Stoichiometry
Solve limiting/excess reagent problems
Calculate percent yield
RESOURCES
Finding Empirical and Molecular Formulas: https://www.youtube.com/watch?v=_H009sTvYE0
How to Balance Chemical Equations: https://www.youtube.com/watch?v=2Juem0lcifE
Stoichiometry Help: https://www.youtube.com/watch?v=XnfATaoubzA
How to Identify Limiting Reagents: https://www.youtube.com/watch?v=0d4LBzOgq3g
How To Calculate Percent Yield: https://www.youtube.com/watch?v=0ZFUdxetdls
PRACTICE PROBLEMS
Directions: Balance the chemical equations provided below. If the chemical requires a 1 as the coefficient, DO NOT to
write it on the line.
1. ____ CO2 + ____ H2O ____ C6H12O6 + ____O2
2. ____ K + ____ MgBr2 ____ KBr + ____ Mg
3. ____ HCl + ____ CaCO3 ____ CaCl2 + ____H2O + ____ CO2
4. ____ Al(OH)3 + ____ H2SO4 ____ Al2(SO4)3 + ____ H2O
5. ____ HNO3 + ____ NaHCO3 ____ NaNO3 + ____ H2O + ____ CO2
Directions: Solve the stoichiometry-related problems below. Remember to SHOW ALL YOUR WORK, BOX your final
answer, and to include the proper SIG FIGS and COMPLETE UNITS.
1. 2 C6H6 + 15 O2 12 CO2 + 6 H2O
a. If 79.8 g of C6H6 reacts, how many moles of H2O is formed?
b. If 55.1 g of CO2 is made, how many grams of C6H6 reacted?
2. 2 KMnO4 + 16 HCl → 2 KCl + 2 MnCl2 + 8 H2O + 5 Cl2
Given: 103.6 g KMnO4, 219.2 g HCl
a. What is the limiting reagent? b. How many moles of Cl2 can be
made?
SECTION TWO - PRACTICE PROBLEMS PAGE 2
3. Fe2O3 + 3 CO 2 Fe + 3 CO2 Given: 25.1 mol of Fe2O3 reacts with 62.9 mol of CO a. What is the limiting reagent? b. How many moles of CO2 can be
made?
4. H3PO4 + 3 KOH K3PO4 + 3 H2O If 49.0 g of H3PO4 is used,
a. What is the theoretical yield of K3PO4? b. What is the percent yield of K3PO4 if you isolate 49.0 g of K3PO4?
5. H2SO4 + Ba(OH)2 BaSO4 + 2 H2O If 98.0 g of H2SO4 reacts,
a. What is the theoretical yield of BaSO4? b. determine the percent yield if you isolate 213.7 g of BaSO4.
6. A particular sugar is determined to have the following composition: 40.0% carbon, 6.7% hydrogen, and 53.5%
oxygen. The compound has a molar mass of 180.0 g/mol. What are the sugar’s empirical and molecular
formulas?
SSeeccttiioonn TThhrreeee:: SSoolluuttiioonnss
EXPECTATIONS
Know what a solution is
Know the parts of a solution
Know what concentration is
Know solubility rules
Construct net ionic equations
Solve for all variables involved in the
Molarity formula
RESOURCES
What’s A Solution?: https://www.youtube.com/watch?v=9h2f1Bjr0p4
Solving Molarity Problems: https://www.youtube.com/watch?v=SXf9rDnVFao
How To Remember Solubility Rules: https://www.youtube.com/watch?v=AsCLuLS-yZY
How To Write Net Ionic Equations: https://www.youtube.com/watch?v=EQIqcT9a7DY
PRACTICE PROBLEMS
Directions: Look at the compounds below. For each write whether they are SOLUBLE or INSOLUBLE in water.
1. Potassium hydroxide _____________________
2. Lead (II) sulfate ________________________
3. Mercury (I) fluoride ______________________
4. Lithium oxide ___________________________
Directions: Complete & balance the following reactions. Show BOTH the complete ionic and net ionic equation for each.
1. SrCl2(aq) + AgNO3(aq)
2. KNO3(aq) + LiC2H3O2(aq)
Directions: Solve the following molarity problem. SHOW YOUR WORK, BOX your answer, and include PROPER UNITS in
your answer.
1. What is the molarity of 3.00L of solution created from 2.5mol of NaCl?
2. If you have 1.5L of a 3M MgCl2 solution, how many grams of MgCl2 do you have?
3. How much solution do you have if you use 455g of BeO to make a .75M BeO solution?
SSeeccttiioonn FFoouurr:: EElleeccttrroonneeggaattiivviittyy,, EElleeccttrroonn CCoonnffiigguurraattiioonnss,, LLiigghhtt && WWaavveess
EXPECTATIONS
Know what electronegativity is
Know Periodic Table trends for
electronegativity
Construct ground state electron
configurations
Know parts of a wave and how they are
related to each other
Solve math problems involving the
following formulas:
o c = λν
o
o c = speed of light = 3.00 x 108 m/s
RESOURCES
Electronegativity Trends: https://www.youtube.com/watch?v=5z54GfoBP0k
Constructing Electron Configurations: https://www.youtube.com/watch?v=jTI-ZkrVvE4
Parts of Wave Review: https://www.youtube.com/watch?v=EEgAWW4vuiI
Solving Energy, Wavelength, & Frequency Problems: https://www.youtube.com/watch?v=Wj2_4aZtBq0
PRACTICE PROBLEMS
Directions: Using periodic table trends, circle which element has the larger Electronegativity:
Choice 1 Choice 2 Choice 1 Choice 2 Choice 3
K Br Cl Br S
Na Mg Na Mg K
Fr F Fr F Rh
Directions: Solve the following word problems. SHOW YOUR WORK, BOX your answer, and include PROPER UNITS & SIG FIGS in your answer.
1. What is the wavelength and energy of a light that has a frequency of 7.1 x 1013 Hz ?
2. What is the frequency of electromagnetic radiation that has a wavelength of 8.8 x 10-4 m? How much energy does the radiation have?
3. What is the frequency and wavelength of electromagnetic radiation that has energy of 5.6 x 1062 J?
SECTION FOUR - PRACTICE PROBLEMS PAGE 2
Directions: Provide BOTH the full and noble gas ground state electron configurations for the elements below. Make sure
to label which one is which.
1. Fluorine
2. Zinc
3. Lead
4. Iridium
SSeeccttiioonn FFiivvee:: LLeewwiiss DDoott SSttrruuccttuurreess && VVSSEEPPRR TThheeoorryy
EXPECTATIONS
Construct Lewis Dot Structures for simple
compounds
Know Electron-Domain and Molecular
Geometry
o Names
o Shapes
o Bond Angles
o Hybridized Orbitals
RESOURCES
How To Draw Lewis Dot Structures: https://www.youtube.com/watch?v=b2p-BtAt1T8
How to Draw Lewis Dot Structures for Polyatomic Ions: https://www.youtube.com/watch?v=4vgxsF4QXEc
VSEPR Tutorials: https://www.youtube.com/playlist?list=PL3hPm0ZdYhyw5Gn0nUgH7809B6W7sLP3s
Hybridized Orbital Help: https://www.youtube.com/watch?v=-M_XvKDX8WY
PRACTICE PROBLEMS
Directions: For each molecule given below a) Draw the correct Lewis Dot Structure
b) Draw the correct 3D drawing of the molecule using your VSEPR chart and the name of its molecular shape and hybridized orbitals
Chemical Formula
Lewis Dot Structure 3D Drawing & Molecular Shape Name
Molecular Shape Name & Hybridized Orbitals
BeCl2
Shape: ____________________
Hybridized Orbitals: _________
PCl5
Shape: ____________________
Hybridized Orbitals: _________
H3O+
Shape: ____________________
Hybridized Orbitals: _________
SSeeccttiioonn SSiixx:: GGaass LLaawwss
EXPECTATIONS
Know relationships between
o Pressure
o Volume
o Temperature
Calculate unit conversions between various
units of pressure
Solve problems involving
o Boyle’s Law
o Charles’ Law
o Gay-Lussac’s Law
o Combined Gas Law
o Ideal Gas Law
RESOURCES
Converting Between Different Units of Pressure: https://www.youtube.com/watch?v=e1A2KKrlXvQ
The Laws and Pressure Explained: https://www.youtube.com/watch?v=ehvLyvwAEYc
Solving Gas Law Problems: https://www.youtube.com/watch?v=kzESbNoNTn4
Solving Ideal Gas Law Problems: https://www.youtube.com/watch?v=C6zluQSNc2c
PRACTICE PROBLEMS
Directions: Solve the pressure unit conversion problems below. SHOW YOUR WORK, BOX your answer, and include PROPER
UNITS & SIG FIGS in your answer.
1. The air pressure for a certain tire is 109 kPa. What is this pressure in atmospheres?
2. The air pressure inside a submarine is 0.62 atm. What would be the height of a column of mercury balanced by this pressure?
Directions: Solve the gas law problems below. SHOW YOUR WORK, BOX your answer, and include PROPER UNITS & SIG FIGS in
your answer.
1. A gas has a volume of 2.87L at 29.5°C. What will its temperature be, in Kelvins, if the volume is reduced to 1.79 L?
2. What will the final pressure in a container be if 290.0mL of air at 4.72kPa is compressed to fit a container whose volume is 1.00L?
3. A gas is heated from 220.0 °C to 310.5 °C and the volume is increased from 10.2 L to 30.09 L by moving a large piston within
a cylinder. If the original pressure was 50.1 kPa, what would the final pressure be?
4. What temperature, in Kelvins, must a gas be if you are able to fill a 8.5L container with 2.8mols of gas and it is at a pressure of 131.02kPa?