Post on 14-Oct-2020
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AP Chemistry Summer Assignment Robin Stefurak, M.Ed
Welcome to AP Chemistry! This is a demanding, challenging and stimulating course, with
accompanying lab, that will cover the first year of College Chemistry.
In preparation for the up and coming school year, you will want to complete the Summer
Assignment before the first day of school. The material in this packet is a review of some
concepts covered in a Pre-AP / Honors Level Chemistry Course. These are concepts that need
to be firmly in place prior to the first day of AP Chemistry Class.
The number one indicator of how a student will perform in AP Chemistry is SELF
MOTIVATION!!!!!
The Summer Assignment is very reasonable. However, DO NOT wait until the end of summer
break to begin the packet.
Materials needed for class!
1. Completed Summer Assignment Packet (please have completed the first day of
school)
2. Three Ring Binder (2.5 in.)
3. Blue or Black Ink Pen
4. A Pencil
5. A Red Pen
6. A Calculator that you know how to use. A graphing calculator is not necessary. A TI-30
will suffice.
FINALLY, the first Exam will be over the material covered in the Summer
Assignment. It is on the THIRD DAY of school.
Khan Academy is a wonderful resource if you need assistance with any of the material
covered in this assignment. Videos for Khan Academy can be viewed directly from the site or
on Youtube.
NEVER, NEVER, NEVER GIVE UP!!!!!!!!!!!!!!! W. CHURCHILL
You will need to know:
1. Polyatomic Ions. A list of relevant Polyatomic Ions is included. These need to be
memorized prior to the first day of school.
2. Memorize the 7 Diatomic Molecules, N2, O2, F2, Cl2, Br2, I2, and H2 (remember, it
looks like an upside down L or seven on the periodic table and H)
3. Elements #1 (H) – # 88 (Ra) AND Uranium (U) and Plutonium (Pu) on the Periodic
Table. ( You will not be given a periodic table with the names of the elements in AP
Chem. )
4. Know where the metals, nonmetals, metalloids are on the periodic table
5. Nomenclature and formula writing
6. Determine if a compound has covalent bonds, ionic bonds or both
7. Naming Acids
8. Balancing
9. Reaction Types (Synthesis, Decomposition, Double Displacement, Single
Displacement, Combustion)
10. Significant figures
11. Scientific Notation
12. Metric Conversions
13. Molar Conversions
14. Lewis dot structures
15. Polarity
16. Electron configuration
17. Stoichiometry
18. Molarity
19. Half-Life
20. Oxidation Numbers/ Oxidation Reduction Reactions
21. Net Ionic Equations
Many of life's failures are people who did not realize how close
they were to success when they gave up. T. Edison
Good Luck !!!!!
1. List the 7 diatomic molecules.
2. Name or give the symbol for the element or ion and determine if it is a metal,
nonmetal or metalloid.
a. Nitrogen
b. Hydrogen
c. Iron
d. Sodium
e. Bromine
f. Germanium
g. B h. Ca+2
i. Li
j. Mg
k. Pb
l. Zn
m. Si
n. S o. S-2
p. Cl-
q. C
r. Rubidium
s. Silver
t. Gold
u. Cobalt
v. Argon
w. Xe
x. Indium
y. Fluoride
z. Hydride
Don’t practice until you get it right. Practice until
you can’t get it wrong. – Unknown
3. Name or give the formula for the following. Then, determine if the compounds or
polyatomic ions have ionic bonds, covalent bonds, or both.
a. Calcium hydroxide
b. Water
c. Copper (II) chloride
d. NO3
e. NaCl
f. Ammonium hydroxide
g. CO3-2
h. CO2-2
i. LiH
j. Zirconium (II) sulfide
k. CO
l. Zinc sulfate
m. PCl3
n. XeCl
o. Tin (IV) bromide
p. Sulfuric acid
q. iodate
r. Hydrochloric acid
s. Nitric acid
t. Pb(CN)2
u. Carbon dioxide
v. Carbon tetrachloride
w. HClO4
x. HNO3
y. ClO3-1
z. PO4-3
Continuous effort - not strength or intelligence - is the key to unlocking our potential.
W. Churchill
4. Balance the equation for the following reactions. If the reaction is in words write-out
the formulas before balancing it. Then, determine the reaction type (Synthesis,
Decomposition, Single Displacement, Double Displacement or Combustion) (oxidation
number for Zinc is +2, oxidation number for Silver is +1)
Type:
a. H2 + N2 NH3 __________________
b. CH4 + O2 CO2 + H2O __________________
c. H2O2 H2O + O2 __________________
d. zinc + hydrochloric acid hydrogen gas + zinc chloride __________________
e. silver nitrate + zinc chloride silver chloride + zinc nitrate __________________
5. Molar Conversions: Solve the following. Use correct significant figures and units in
your final answer. Show all work. Dimensional Analysis is preferred method for
solving.
1 mole = 6.02 x 1023 molecules ( atoms, ions, formula units, etc. )( 6.02 x 1023 is
Avogadro’s Number)
Molar Mass is the grams of a substance in 1 mole (g/mol) ( Ex. The m.m. of
water is 18.01 g / 1 mole )
1 mole = 22.4 L (at STP) ( STP is standard temp and pressure)
a. 5.5 moles of water are how many grams of water?
b. 45 g of NaCl are how many moles of NaCl?
c. 2.35 x 1025 molecules of CO2 are how many moles of CO2?
How many grams of CO2?
d. 550 liters of oxygen gas (O2) at STP are how many moles of oxygen gas?
How many grams of oxygen gas?
6. Convert the following :
a. 250 mg to ______g
b. .00523 km to ________m
c. 1.30 x 106 mm to _____km
d. 4.50 x 10-5 cm to _____km
e. 1036 mg to _____µg ( µ = micro )
f. 5.46 x 1015 pm to______m (p = pico )
7. Write the Electron Configuration and Lewis Dot Structure for the following atoms.
Then, determine the number of Valence Electrons (the outer electrons) for each atom.
Ex. Fluorine 1s22s22p5 F. 1 valence electron
a. Hydrogen
b. Lithium
c. Oxygen
d. Argon
e. Bromine
f. Radium
8. Draw the Lewis Dot Structure for the following. Determine if the molecule is Polar or
Nonpolar. If the atom is Polar, indicate the partial positive (δ+) and partial negative
ends (δ–) ends.
a. Cl2 e. N2
b. CH4 f. NH3
c. H2O g. HF
d. O2 h. SO3
Failure will never overtake me if my determination to succeed is
strong enough. Og Mandino
9. Stoichiometry: Show all work. Use the correct amount of significant figures and units
in final answers. Dimensional Analysis is the preferred method of solving.
Use the following balanced equation to answer a. – d.
N2 + 3H2 2NH3
a. How many moles of hydrogen are needed to completely react with 2.0 moles of
nitrogen?
b. What volume of hydrogen is necessary to react with 5.0 liters of nitrogen to produce
ammonia? ( Assume STP conditions )
c. How many grams of hydrogen are necessary to react completely with 50.0 g of
nitrogen?
d. What volume of NH3 at STP is produced if 25.0 g of N2 is reacted with an excess of H2?
Use the following balance equation to answer e.-g.
2KClO3 2KCl + 3O2
e. If 5.0 g of KClO3 is decomposed, what volume of O2 is produced at STP?
f. How many moles of KCl will be produced from 5.0 g of KClO3?
g. How many formula units of KCl will be produced from 5.0 g of KClO3?
10. Molarity: Solve the following. Show all work, use correct sig figs and units in final
answer.
Molarity = moles of solute / liter of solution
a. What is the molarity of a solution in which 58 g of NaCl are dissolved in 1.0 L of
solution?
b. What is the molarity of a solution in which 10.0 g of AgNO3 is dissolved in 500. mL of
solution?
M1V1 = M2V2 ( volume needs to be in L)
c. How much concentrated 18 M sulfuric acid is needed to prepare 250 mL of a 6.0 M
solution?
d. To what volume should 25 mL of 15M nitric acid be diluted to prepare a 3.0 M solution?
Education is the most powerful weapon which you can use to
change the world. Nelson Mandela
11. Oxidation Numbers: Determine the oxidation number for each element in the
following.
a. H2O i. SO-2
b. CO2 j. F2
c. H2SO4 k. Zn
d. NaOH l. NH+
e. HF
f. H2O2
g. MgCO3
h. LiNO3
12. Oxidation Reduction Reactions: For each reaction, determine what is being oxidized
and what is being reduced ( remember: OIL, RIG )
a. 2Li + CaCl2 Ca + 2LiCl
b. 2Mg + O2 2 MgO
c. HNO3 + H3PO3 NO + H3PO4
d. 4Al + 3O2 2Al2O3
13. Net-Ionic Equations: Write the balanced complete, total ionic, and net ionic equation
for the following. Some will actions will require you to predict the products first. (use
the Solubility Rules below)
a. AgNO3 (aq) + KCl (aq) AgCl (s) + KNO3 (aq)
b. manganese(II) chloride (aq) + ammonium carbonate (aq)
manganese(II) carbonate (s) + ammonium chloride (aq)
c. K3PO4 (aq) + Al(NO3)3 (aq)
d. cobalt(III) bromide + potassium sulfide
Solubility Rules: (These DO NOT have to be memorized, you only have to know the BIG
THREE)
1. All salts of Group IA, and ammonium are soluble.
2. All salts of nitrates, chlorates and acetates are soluble.
3. All salts of halides are soluble except those of silver(I), copper(I), lead(II), and
mercury(I).
4. All salts of sulfate are soluble except for barium sulfate, lead(II) sulfate, and strontium
sulfate.
5. All salts of carbonate, phosphate and sulfite are insoluble, except for those of group IA
and ammonium.
6. All oxides and hydroxides are insoluble except for those of group IA, calcium,
strontium and barium.
7. All salts of sulfides and insoluble except for those of Group IA and IIA elements and
of ammonium.
BIG THREE:
1.) All nitrates (NO3-) are soluble!!!!!
2.) All Group I Metals and Ammonium (NH4+) are soluble!!!!!
3.) All Halogens are soluble except when combined with Pb, Ag, Hg!!!!
14. Thermochemistry: Give the thermodynamically favorable conditions (spontaneous) for each:
a.) Enthalpy (ΔH) Ex: negative exothermic_
b.) Entropy (ΔS) ____________ _ _________________
c.) Free Energy (ΔG) ____________ _ _________________
d.) Label each of the Potential Energy Graphs with the following: Endothermic or Exothermic, ΔH, reactants, products, transition state (aka: activated complex), activation energy)
15. Equilibrium: Indicate if the following reactions are going to favor products (shift to the
right) or reactants (shift to the left).
(c)
(d)
How would increasing the temperature affect each reaction below? Answer the following as
favors products or favors reactants.