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?