Download AP Chemistry Summer Assignment 2016

AP Chemistry Summer Assignment 2016
Assignment 1:
QUESTIONS TO ANSWER
Due: June 30th by 3p.m. via email to [email protected].
I will respond to your email to let you know I received it before the due date. If you don’t get an email
back from me, I didn’t get it.
Please make sure you send the assignment using an email address that YOU personally will use for the
2016-2017 school year and check regularly. I will be making an email group for our class. Having a working
email address is important in AP Chemistry as I may send updates/documents via email. A Gmail account
may be especially beneficial for file sharing.
This is the first assignment of the 1st quarter.
Please answer the following questions. Number your responses to make answering the questions easier for
both you and me. Please keep your answers brief but still say enough to fully answer the questions.
1) Have you read and do you understand the informational points from the Introduction and Commitment
document? Yes or no is fine for this question. By saying yes, you agree to have read and understood the
information.
2) Did you (and a parent) register for the Remind101 service? (Instructions are provided in the AP Course
Criteria document.)
3) Why are you taking the AP chemistry course?
4) What are you hoping to get out of the course? Are you willing to make the commitment? Are you willing
to study hard all year and for the exam?
5) What other classes are you taking this year?
6) What extracurricular activities/job are you participating in this year?
7) What topic from Regents Chemistry do you feel is your weakest area? What topic do you feel is your
strongest area?
8) What did you think about the advice former students had to offer? What did you learn by reading what
they had to say?
9) Do you have reliable Internet access daily? In most cases, a smartphone or tablet will be adequate for
viewing notes, vodcasts, etc. Please be specific.
AP Chemistry Summer Assignment 2016
Assignment 2:
MEMORIZATION AND PREPARATION OF NOTECARDS
You will need reference materials to be successful in AP chemistry. Some of the pieces of information
within these tables will need to be memorized. Not memorizing this information will put you at a huge
disadvantage compared to the 100,000+ other people who will take the AP Chemistry exam in May 2017.
Conversely, memorizing the information will help you all year and will give you an advantage over
individuals who do not know this information. If you don’t believe me that this memorization is important,
ask someone who has completed AP Chemistry. This something you have to do and is immensely important
to you getting off to a good start and having a good year!!!
Directions:
1) Download and print out the document “Reference Sheets”. This includes the same periodic table we use
in AP chemistry. Notice that the names and oxidation states of the elements are not given. There is no
excuse for making mistakes by putting the wrong symbol or oxidation state for a certain element on the AP
exam.
2) Make notecards of the following elements by placing the element symbol on one side and the name
and oxidation state(s) on the other side. For some elements (like chlorine, bromine, etc.) other oxidation
states exist; however, usually only the most common needs to be memorized/identified from the periodic
table. You should have a periodic table in front of you when trying to recite the charges, as the location of
elements often gives away the oxidation state, Example – Group 1 metals are always and only a +1. It is
strongly recommended that you review elements and charges until you have mastered them until
proceeding further in the summer assignment. An example notecard is given below:
Example Notecard:
Front
Fe
Back
Iron
+2, +3 oxidation states
Common Elements and Charges (look up the other charges on your Regents table):
H (+1, -1)
He
Li (+1)
Be
B
C (-4,+2,+4)
N (-3 to +5)
O (-2, - 1, +2)
F (-1)
Ne
Na (+1)
Mg (+2)
Al (+3)
Si
P
S
Cl (-1, +1, +3, +5, +7)
Ar
K (+1)
Ca (+2)
Sc
Ti
V
Cr
Mn
Fe (+2, +3)
Co
Ni (+2, +3)
Cu (+1, +2)
Zn (+2)
As
Se
Br (-1, +1, +5)
Kr
Sr
Ag (+1)
Cd (+2)
Sn (+2, +4)
Sb
Te
I (-1,+1,+5,+7)
Xe
Ba (+2)
W
Pt
Au (+1, +3)
Hg (+1, +2)
Pb (+2, +4)
Bi
Rn
Ra
U
Pu
AP Chemistry Summer Assignment 2016
3) Go to the following website and print a clean copy of the 2011 Physical Setting/Chemistry Reference
Table, including the periodic table. This periodic table is really nice to have because it gives all the possible
charges (oxidation states) of the elements on the periodic table. Make sure you know the charges for
common elements! The NYS Periodic table can come in handy for this! Many charges require little
memorization because the charges are given by the location of the periodic table, (Example –
Group 1 metals only form a +1 charge)
http://newyorkscienceteacher.com/sci/pages/reftables/crt.php
The way you will memorize certain charts within this reference table is by making note cards/flashcards.
Everyone is required to do flashcards and will serve as part of the grade for the summer assignment. You
will want to hang onto these flashcards all school year so they may reviewed throughout the year and leading
up to Unit Tests and the AP chemistry exam. The tables, which need to be put on note cards and
memorized, are as follows:
Table E: Name on one side, formula and charge on the other side.
Table F: Ions on one side, soluble or not with exceptions on the other side.
The “Big Six” Strong Acids: Name on one side for each, formula on the other side for each (6 separate
notecards)
Sulfuric Acid – H2SO4; Nitric Acid – HNO3; Hydrochloric Acid – HCl; Hydrobromic Acid – HBr;
Hydroiodic Acid – HI; Perchloric Acid – HClO4
Common Weak acids: Name on one side, formula on the other side (4 separate notecards) – Acetic Acid
(Ethanoic Acid) – CH3COOH or C2H4O2 Hydrofluoric Acid – HF, Carbonic Acid – H2CO3 Phosphoric
Acid – H3PO4
Strong Bases: Name on one side for each, formula on the other side for each (8 separate notecards) Group
1 bases are all strong bases and are covered by solubility rules, NaOH, KOH, LiOH, RbOH, and CsOH,
Calcium Hydroxide – Ca(OH)2 Strontium Hydroxide – Sr(OH)2 Barium Hydroxide – Ba(OH)2
Weak bases: (Name on one side, formula on the other side) – Ammonia – NH3 (not to be confused with
the ammonium ion NH4+)
Diatomic Elements: (I would put these on your periodic table as well) Br2 I2 N2 Cl2 H2 O2 F2
Never throw out any of the note cards you make all year. You will need them to study for the AP chemistry
exam. It might be worth it to invest in a note card box to keep them handy.
It is strongly recommended that you work hard on the memorization component before moving on
to the rest of the summer assignment and you need to certainly have mastered the memorization
component before attempting the “practice test”.
AP Chemistry Summer Assignment 2016
Assignment #3:
SIGNIFICANT FIGURES
Go to the following websites and review sig figs. These websites are so fantastic that they will have you
learning sig figs in 5 minutes or less!
http://www.chem.sc.edu/faculty/morgan/resources/sigfigs/index.html
http://science.widener.edu/svb/tutorial/sigfigurescsn7.html
On the AP Chemistry exam, significant figures matter and we will not have time to cover them through
the year; however, you will be graded upon using sig figs all year long. It is something you must learn and
get comfortable with now and learn to do the remaining problems with significant figures in mind.
Solve the following problems by determining the number of significant figures. For the calculations, you
need to find the answer using a calculator and then report the answer to the correct number of significant
figures. I would suggest writing down what the calculator gives you first and then coming up with
the right answer according to the significant figures rules.
Please complete the following the following problems on notebook paper.
1) Determine the number of significant digits in each of the following:
a) 6.571 g
c) 54.52 cm
b) 30.07 g
d) 0.006700 g
2) Add, and round properly:
a) 16.5 + 8 + 4.37
b) 13.25 + 10.00 + 9.6
e) 2500 m
f) 0.0230 cm
c) 0.0853 + 0.0547 + 0.0370 + 0.00387
3) Subtract, and round properly:
a) 350.0 – 200
b) 13.57 - 6.3
c) 27.68 - 14.3694
4) Multiply, and round properly:
a) 2.6 x 3.78
b) 6.54 x 0.37
c) 0.0036 x 0.02
5) Divide, and round properly:
a) 35 / 0.62
b) 0.58 / 2.1
c) 39 / 24.2
6) Express the following in scientific notation: (The spaces are just to help you count the zeros)
a) 0.000 03
c) 0.000 007
e) 0.002
b) 55 000 000
d) 8 000 000
f) 65 000
7) The density of the element gold in a coin is to be calculated from the following data:
Mass of coin = 13.512 g
Volume of coin and water = 25.1 ml Volume of water alone = 24.4 ml
The density of the metal in the coin equals 13.512 g / (25.1 ml – 24.4 ml)
The answer to the correct number of significant figures is:
(a) 19.303 g/ml (b) 19.3 g/ml (c) 19.30 g/ml (d) 19 g/ml
8) Which of the following has four significant figures? (a) 0.0005 (b) 0.0050
(c) 0.0500 (d) 0.5000 (e) all of
these
AP Chemistry Summer Assignment 2016
Assignment #4:
USING DIMENSIONAL ANALYSIS (FACTOR LABEL METHOD)
Dimensional analysis is a way of problem solving that we will use to solve many (50% or more) of the
problems this year. You must learn/review this process before the course begins or you will be lost for the
remainder of this assignment and you will not understand much of problem solving techniques in AP
Chemistry. Please do not try your own method of problem solving. The graders on free response questions
will be looking for you to show your work using dimensional analysis (if you aren’t using one of the
provided equations from the reference sheet). This is the way problems must be done in AP chemistry, so
please do not try your own methods. The website below has a more detailed tutorial on dimensional
analysis.
http://www.mhhe.com/physsci/chemistry/chang7/esp/folder_structure/ch/m4/s1/index.htm
Solve the following problems by using dimensional analysis and show your work on all problems. Be sure to
give the correct number of significant figures. Helpful Hint: Conversion factors do not impact the number
of significant figures on the answers EVER. The prefixes for the metric conversion problems can be found
at: http://physics.nist.gov/cuu/Units/prefixes.html or on table C in the Regents Reference Table. For the
non-metric problems I am assuming you can determine the number of seconds in one minute. Do not move
the decimal; this is for 6th graders. Other handy conversion factors are given below.
Common conversion factors
1 m = 1000 mm
1 m = 100 cm
1 km = 1000 m
1 m = 109 nm
1 L = 100 cL
1 kL = 1000 L
1 m = 1012 pm (picometers)
1 yard = 3 feet
1 inch = 2.54 cm
1 gallon = 3.78 L
1 mile = 1.609 km
1 gallon = 128 oz
1 pound = 16 oz
1 mile = 1609 m
Please complete the following on notebook paper. Label your units clearly!
1) How many millimeters is 13 meters?
2) There are 3.78 Liters in one gallon. How many mL is this?
3) The average human hair is 0.000062 m thick. How many nanometers is this?
4) The average laptop is now only 1.80 inches think. How many centimeters is this?
5) The average cell is in only 30.0 nm thick. How many cm is this?
6) My gas tank only holds 12 gallons. How many mL is this?
7) There are 0.500 mL in every drop of water. How many kL is this?
8) Challenge Question: The average life expectancy is the U.S. for females is 78.2 years. How many
milliseconds is this? (Yes, it is going to be a big number.)
Assignment #5:
MOLE CONVERSIONS USING DIMENSIONAL ANALYSIS
Converting between mass and moles is an absolute must for anyone studying chemistry. These problems are
meant to serve as a review of molar weights (molar mass, gram formula mass), using sig figs and converting
readily between mass, moles and molecules. Solve the following and show all work USING
DIMENSIONAL ANALYSIS on notebook paper. Please clearly label everything. Make sure you solve the
problems to the correct number of significant figures. Remember that molar weights (an exact
conversion factor) have no impact on significant figures. Use your AP periodic table to find the molar
weights needed. The following website has some helpful hints and shows the proper way of labeling
calculations. https://chemfiesta.org/2015/02/06/mole-calculations-3/
AP Chemistry Summer Assignment 2016
1) How many moles does 80.0 grams of H2O represent?
2) What is the mass (in grams) of 5.4 moles of Ba(CN)2?
3) How many atoms does 2.0 moles of He represent?
4) Convert 3.01 x 1023 molecules of C2H6 to moles.
5) How many grams of CaCl2 does 2.41 x 1024 molecules represent?
Assignment #6:
BALANCING EQUATIONS
If you can’t balance an equation you can’t do many problems in chemistry; or, if you can’t balance correctly
you will get the problem wrong automatically. A tutorial on balancing can be found at the site below. This
site also has some nice problems at the bottom where you can check if you are doing them correctly.
https://chemfiesta.org/2016/03/30/equations/
Balance the following equations below. Remember, change coefficients only, and use the lowest possible
whole number coefficients to balance the reaction.
1) ____ Na +____ I2 ____ NaI
2) ____ KClO3 ____ KCl + ____ O2
3) ____ C3H8 + ____ O2 ____ CO2 + ____ H2O
4) ___ H3PO4 + ____ KOH  ____ K3PO4 + ____ H2O
5) ____Na + ____ NaNO3  ____Na2O + ____ N2
Write and balance the following chemical equations. Check your formulae carefully!
6) Nitrogen plus hydrogen produce ammonia. (Remember diatomic elements!)
7) Sodium oxide combines with water to form sodium hydroxide.
8) Sodium sulfate reacts with calcium nitrate to produce sodium nitrate and calcium sulfate.
9) Zinc reacts with iron (III) chloride yielding zinc chloride plus iron.
10) Octane is burned in oxygen gas and produces carbon dioxide and water.
Assignment #7:
STOICHIOMETRY
Balance all reactions, show all work using dimensional analysis with units, and have the correct number of
sig figs in your answer. Conversion factors (Molar weights as well as coefficients from the balanced
equation) have no impact on the number of significant figures, as they are exact amounts. Please use your
AP periodic table to find the molar weights needed. Please label all calculations properly or credit will not be
granted! The website below has some basic help with stoichiometry problems and links to two excellent
video tutorials: https://chemfiesta.org/2015/09/18/reactions-and-stoichiometry/
1) LiOH + HBr  LiBr + H2O
If you start with 10.00 grams of lithium hydroxide, how many moles of lithium bromide will be produced?
2) C2H4 + O2  CO2 + H2O
If you start with 45.5 moles of ethene (C2H4) how many grams of carbon dioxide will be produced?
3) Mg+ NaF  MgF2 + Na
If you start with 5.50 grams of magnesium, how many grams of magnesium fluoride will be produced?
4) HCl + Na2SO4  NaCl + H2SO4
If you start with 20.555 moles of hydrochloric acid, how many moles of sulfuric acid will be produced?
AP Chemistry Summer Assignment 2016
5) Given the reaction S + O2  SO2
(a) How many grams of sulfur must be burned to give 100.0 g of SO2? (b) How many grams of oxygen will
be required for the reaction in part (a)?
Assignment #8:
LIMITING AND EXCESS REAGENT
Determine the limiting and excess reactant. Be sure to balance the equation or give the equation when not
given. Be sure to use units, the correct number of sig figs, and dimensional analysis to solve the problems.
These two sites have very helpful information to help with limiting reagent problems:
http://www.chemcollective.org/stoich/limiting-reagents.php
http://www.chem.tamu.edu/class/majors/tutorialnotefiles/limiting.htm
1) _____ Cu(s) + _____ AgNO3 (aq)  _____ Cu(NO3)2 (aq) + _____ Ag(s)
If 2.5 moles of copper and 5.5 moles of silver nitrate are available to react, what is the limiting reactant?
What is the excess reactant?
2) _____ CaO(s) + _____ H2O(l)  _____ Ca(OH)2(aq)
How many grams of calcium hydroxide will be formed in this reaction when 4.44 g of calcium oxide and
7.77 g of water are available to react? Also identify the limiting and excess reactants.
3) Magnesium undergoes a single replacement reaction with hydrochloric acid. (a) Write the balanced
equation for this reaction. (b) How many grams of hydrogen gas will be produced from the reaction of 3.00
g of magnesium with 4.00 g of hydrochloric acid? (c) Identify the limiting and excess reactants. (d)
Determine the amount of excess reagent left over.
4) Sulfur reacts with oxygen to produce sulfur trioxide gas. (a) Write the balanced equation for this reaction.
(b) If 6.3 g of sulfur reacts with 10.0 g of oxygen, what is the limiting reactant? (c) How many grams of
sulfur trioxide will be produced?
Assignment 9:
NOMENCLATURE PRACTICE
If given the formula, write the name. If given the name, write the formula.
I. Binary Ionic Compounds
1. CaH2
4. aluminum oxide
2. Na2O
5. calcium fluoride
3. K3N
6. sodium phosphide
II. Binary Ionic Compounds with Transition Metals
1. Cu2O
2. Mn2O3
3. FeS
4. Pb3N4
5. cobalt (II) bromide
6. manganese (II) oxide
7. tin (II) phosphide
8. iron (III) hydride
III. Ternary Ionic Compounds – Polyatomic Ions
1. Ca(NO2)2
2. Fe(OH)3
3. Mn(NO3)3
4. Pb(CN)4
5. Au2SO4
6. magnesium hydroxide
7. aluminum nitrate
8. iron (III) nitrite
9. ammonium nitrite
10. cobalt (II) chlorate
AP Chemistry Summer Assignment 2016
IV. Binary Molecular Compounds
1. PCl5
2. NO
3. P2O3
Assignment #10:
4. iodine heptafluoride
5. dichlorine monoxide
6. dibromine trioxide
PRACTICING SOLUBILITY RULES AND NET IONIC EQUATIONS
Solubility is an important concept in AP Chemistry. You are expected to know the solubility rules from
memory and use them correctly. You can use TABLE F from the NYS reference table to get you started but
you need to be able to do them from memory when you come back to school and take the summer
assignment test.
Here is help with solubility rules and net ionic equations:http://chemistry.bd.psu.edu/jircitano/soluble.html
A. Write a balanced equation to show the dissociation of each of the following ionic compounds in water.
How many moles of ions are formed when 1 mole of the solid is dissociated?
1. Na2S
Example: Na2S (s) 2Na+ (aq) + S2- (aq) 2 moles of sodium ions and 1 mole of sulfur ions
2. Ca(NO3)2
Example: Ca(NO3)2 (s)  Ca2+(aq) + 2NO3-(aq) 1 mole of calcium ions and 2 moles of nitrate ions
BE SURE NOT TO SPLIT APART THE POLYATOMIC ION!!!
3. MgSO4
4. K3PO4
5. (NH4)2CO3
B. Predict whether each of the following compounds is soluble or insoluble in water.
1. Magnesium phosphate
6. Na2SO4
2. Silver nitrate
7. Li2CO3
3. Barium carbonate
8. NH4Br
4. Calcium chloride
9. Ni(NO3)2
5. Aluminum sulfide
10. PbSO4
C. Consider the following pair of aqueous solutions being mixed. On the basis of the solubility rules,
(a) write the complete molecular equation (M), (b) complete ionic equation (CI), and (c) net ionic equation
for each (NI). Please label each type of equation for each problem. You can use the letters M, CI, and NI to
shorten the work. A reaction occurs in all cases. Please put state symbols (s, aq) on each form (M, CI, NI) of
the equation. Be sure to avoid the common mistakes of not ionizing compounds correctly.
1. Sodium sulfide and manganese (II) chloride
2. Lead (II) nitrate and ammonium carbonate
3. Sodium sulfate and silver nitrate
Assignment #11:
ELECTRON CONFIGURATION
The following site provides some help on electron configuration:
http://www.ausetute.com.au/econfig.html
Write a ground state electron configuration for each neutral atom. Ground state means that all of the lowest
possible energy levels (up to the proper number of electrons for the element) are filled.
1. Na
2. Pb
3. Sr
4. U
5. N
AP Chemistry Summer Assignment 2016
Write a ground state electron configuration for these ions. Remember that ions have a change in the total
number of electrons (positive have lost electrons and negative have gained).
Example: N-3 is 1s22s22p6. It
has three extra electrons.
6. O-2
7. Cl+7
8. Mn+4
9. B+3
Assignments 12-14: TEXTBOOK WORK
Read the following chapters:
Chapter 1—Chemical Foundations
Complete these questions:
p. 31-36 # 6, 8, 15, 36, 66, 71, 74, 82, 84, 94
Chapter 2—Atoms, Molecules, and Ions
Complete these questions:
p. 69-75 #4, 20, 26, 28, 56
Chapter 3—Stoichiometry
Complete these questions:
p. 117-128 # 22, 38, 39, 47, 49, 51, 53, 66, 68, 76, 90, 108, 112, 114, 168
Complete your work very neatly. This is an essential practice for all work this year. Show ALL work for all
calculations. All work must contain your name and be ready to be submitted on the first day of school.