AP CHEMISTRY SUMMER ASSIGNMENT
Mr. Vu’s email: [email protected]
1. Join Edmodo at Edmodo.com using the Code: tjdosx for AP Chemistry 2012-2013. Here,
you will get news and information on the class. Join the online text to start your summer
work. Information on how to do that is in the post.
2. Purchase your own copy of any AP Chemistry Review Book (Princeton, Barons, etc..) I
suggest you look at each book to see if it is not too simple and to brief. Some books are
too long in the explanation and others are too short.
3. Buy a few color highlighters.
4. Read and highlight material that applies to you in the introductory chapters to learn
what the exam will be on and how it will be administered.
5. Take the diagnostic test, if they have one to see what you know.
6. Take a look at the AP and other websites, check my school website and Google AP
chemistry. List the three most useful in the front cover of your book.
7. Sign up for online textbook
NO LATE ASSIGNMENTS WILL BE ACCEPTED!!!
AP CHEMISTRY FIRST WEEK TEST
AP Chemistry is a difficult course. It is not all about memorization; however, having these items
memorized is essential for success in learning the concepts covered in the course. Make
flashcards, (I suggest a site called studyblue.com) have your friends and family quiz you, take
the lists with you on vacation, or do whatever it takes to get this information firmly planted in
your head. Do not wait until the night before school begins.
The first day test will cover six areas of memorization:
1. Rules for Naming Compounds
2. Determining Oxidation Numbers
3. The Solubility Rules
4. Rules for Naming Acids
5. Significant Figures/Sig Figs
6. Variable Valences for Transition Metals
7. Polyatomic Ions (including name, symbol and charge)
Rules for Naming Compounds
When naming compounds, remember the following rules:
Binary Ionic Compounds (Type I)
1. The cation (positively charged ion; Na+, Al3+) is always named first and the anion
(negatively charged ion; Cl-, O2-) second.
2. A monatomic (meaning one-atom) cation takes its name from the name of the element.
For example, Na+ is called sodium in the names of compounds containing this ion.
3. A monatomic anion is named by taking the root of the element name and adding -ide.
Thus, the Cl- ion is called chloride, the S2- ion is called sulfide, and the O2- ion is called
oxide.
Some common monatomic cations and anions are shown below
Cation
Name
Cation
H+
Hydrogen Li+
Na+
Sodium
Cs+
Cesium
Mg2+
Magnesium Ca2+
Ba2+
Barium
Zn2+
Zinc
Name
Anion
Name
Anion
Name
Lithium
H-
Hydride F-
Fluoride
K+
Potassium
Cl-
Chloride Br-
Bromide
Be2+
Beryllium
I-
Iodide
O2-
Calcium
S2-
Sulfide
Se2- Selenide
Al3+
Aluminum
N3-
Nitride
P3-
Ag+
Silver
As3-
Arsenide C4-
Oxide
Phosphide
Carbide
Binary Ionic Compounds (Type II)
1. The cation of a transition metal is always named first (like any cation) and the anion
second.
2. A monatomic (meaning one-atom) cation takes its name from the name of the element.
For example, Cu+ is called Copper(I) and Cu2+ is called Copper(II) in the names of
compounds containing these ions. The number in parentheses is the charge of the cation.
3. All transition metal cations, except Zn2+, Cd2+, and Ag+ (which always have the charges
shown here), must show the oxidation number (charge) in parantheses following the
English spelling of the element, such as Iron(III), Copper(I), or Vanadium(V), whenever a
compound containing these ions, which have multiple charges, is named.
4. For the cations in Groups IIIA-VIA (including, Sn, Pb, Ga, Bi, etc.) also have multiple
charges, even though they are not transition metals. For all the metals in these groups
(except Al, which, of course, always has a +3 charge), include a paranthesis after the
name, and show its positive charge as a Roman numeral (Pb2+ is Lead(II) in names)
Binary Covalent Compounds (Type III)
Compounds containing only non-metal elements are named using Type III binary compound rules.
These compounds are always neutral (not ions which have charges), and consist of only two
elements (see acid naming below for compounds containing only non-metal elements, but with
more than two elements. The prototypical compound is CO2, which is called carbon dioxide.
1. The first element shown in the compound is named as the element (e.g., for CO2, first
element is "carbon")
2. The second element shown in the compound is named according to the anion name, ending
in -ide (e.g., for CO2, the second element is named "oxide")
3. The second element always carries a prefix indicating the number of times it is present in
the compound (e.g., for CO2, the second element (oxide) is present twice, so it has the
"di" prefix)
4. The amount of the first element is only shown, if it is present more than once. It is
assumed to be present only once, hence just the name of the element. However, if it is
present more than once, you must then specify the number of times it is duplicated (di,
tri, tetra, etc.)
The following prefixes are used to specify the number of times an element is present in binary
covalent compounds:
prefixes (1-5)
1 — mono
2 — di
3 — tri
4 — tetra
5 — penta
prefixes (6-10)
6 — hexa
7 — hepta
8 — octa
9 — nona
10 — deca
Examples using prefixes
CCl4 — carbon tetrachloride
P2O5 — diphosphorus pentoxide
N2O — ninitrogen monoxide
ICl3 — iodine trichloride
Please note that ionic compounds (Type I & II binary compound names) never use prefixes to
specify how many times an element is present. Prefixes are only used for covalent compounds
formed from non-metal elements.
Rules for Determining Oxidation Number
Oxidation Number: A number assigned to an atom in a molecular compound or molecular ion
that indicates the general distribution of electrons among the bonded atoms.
1. The oxidation number of any uncombined element is zero, O.
2. The oxidation number of a monatomic ion equal the charge on the ion.
3. The more electronegative element in a binary compound is assigned the number equal to
the charge it would have if it were an ion.
4. The oxidation number of fluorine in a compound is always –1.
5. Oxygen has an oxidation number of –2 unless it is combined with F, when it is +2, or it is
in a peroxide, when it is –1.
6. The oxidation state of hydrogen in most of its compounds is+1 unless it combined with a
metal, in which case it is –1.
7. In compounds, the elements of groups 1 and 2 as well as aluminum have oxidation number
of +1, +2, and +3, respectively
8. The sum of the oxidation numbers of all atoms in a neutral compound is zero, O.
9. The sum of the oxidation number of all atoms in a polyatomic ion equals the charge of the
ion.
Solubility Rules
1. All compounds containing alkali metal cations and the ammonium ion are soluble.
2. All compounds containing nitrates (NO3-), Chlorate (ClO4-), chlorite (ClO3-), and acetate
(C2H3O2 -) anions are soluble.
3. All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+, or Hg2+.
4. All sulfates, SO4-2, are soluble except those containing Hg2+, Pb2+, Sr2+, Ca2+, or Ba2+.
5. All hydroxides (OH-) are insoluble except compounds of the alkali metals, Ca2+, Sr2+, and
Ba2+.
6. All compounds containing phosphate (PO43-), sulfide (S2-), carbonate (CO32-), and sulfite
(SO32-) ions are insoluble except those that also contain alkali metals or ammonium
(NH4+).
Rules for Naming an Acid
1. When the name of the anion ends in –ide, the acid name begins with the prefix hydro-,
the stem of the anion has the suffix –ic and it is followed by the word acid.
-ide becomes hydro _____ic Acid
Cl- is the Chloride ion so HCl = hydrochloric acid
2. When the anion name ends in –ite, the acid name is the stem of the anion with the suffix
–ous, followed by the word acid.
-ite becomes ______ous Acid
-
ClO2 is the Chlorite ion so HClO2. = Chlorous acid.
3. When the anion name ends in –ate, the acid name is the stem of the anion with the suffix
–ic, followed by the word acid.
-ate becomes ______ic Acid
-
ClO3 is the Chlorate ion so HClO3 = Chloric acid.
Rules for Significant Figures/ Sig Figs
1. All non-zero digits are significant.
2. Zeros between other significant figures are significant.
3. Zeros to the right of a decimal point and to the right of a number are significant.
4. A zero standing alone to the left of a decimal point is not significant.
5. Zeros to the right of the decimal and to the left of a number are not significant.
6. Zeros to the right of the last number but left of the decimal point may or may not be
significant. This information is known only to the person that made the measurement.
Use scientific notation when in doubt. The use of a bar over the last significant zero is
acceptable as well as using the decimal point to indicate that all digits to its left are
significant.
7. In multiplication and division, the result may have no more significant figures than the
factor with the fewest number of significant figures.
8. When adding and subtracting numbers that come from measurements, arrange the
numbers in columnar form. The final answer can contain only as many decimal places as
found in the measurement with the fewest number of decimal places.
9. When calculating the number of significant figures allowed in an answer, the following
categories are NOT considered:
a. numbers representing a numerical count
Example: 25 students, each carrying 2.693 54 kg of sugar
25 x 2.693 54 kg = 67.338 5 kg
b.
numbers that are part of a mathematical formula
example: volume of a sphere = 4/3 π r3
3
4/3 π 2.11111 = 39.4114 cm
3
for sphere with radius 2.11111 cm
(using 3.141 6 for π)
c. conversions
1 km = 1000 m
the 1 is considered to have several significant figures
Naming Compounds Practice
Show Formulas for the Following Compounds. Do this on another sheet of paper.
hydrogen bromide (g)
ammonia (g)
CO2 (g)
dinitrogen pentoxide
P2O3
HF
H 2S
HCl(aq)
CO(g)
NO (g)
SF6 (g)
sulfur trioxide (g)
tetraphosphorus decoxide
disulfur dichloride
boron trifluoride
carbon tetrachloride
iodine monochloride
sulfur trioxide
hydrogen sulfide (g)
carbon tetrachloride
hydrosulfuric acid
H2Se (aq)
CS2
NO2
PCl5
sulfur dioxide
CO2 (s)
HF (g)
NO2 (g)
hydrochloric acid
carbon disulfide
Oxidation Numbers
1. Give the oxidation numbers of all the elements in the following molecules and ions:
a. SO, SO2, SO3, SO32-, SO42b. ClO2, ClO-, ClO2-, ClO3-, ClO4c. N2O, NO, NO2, N2O4, N2O5, NO2-, NO32. Determine the oxidation number of the sulfur atom:
a) H2S b) S c) H2SO4
d) S2- e) HS-
f) SO2
g) SO3
3. Indicate the oxidation number of phosphorus in each of the following compounds:
a. HPO3 _____ d. H3PO4 _____
b. H3PO2 _____ e. H4P2O7 _____
c. H3PO3 _____ f. H5P3O10 _____
4. Give oxidation numbers for the underlined atoms in these molecules and ions:
a) Cs2O
f) ClF3
k) MoO42b) PtCl62g) H3AsO3
l) MnO4c) CaI2
h) SbF6m) PtCl42d) SnF2
i) TiO2
n) O2
e) Al2O3
j) P4
o) O3
Significant Figures Practice
How many significant figures are in each of the following numbers?
1) 5.40 ____
2) 1.2 x 103 ____
3) 2,370.0 ____
4) 210 ____
5) 0.00120 ____
6) 9.6x 10-6 ____
7) 801.5 ____
8) 0.0102 ____
9) 101.0100 ____
A. Complete the multiplication or division problem and provide the final answer with the
correct number of significant figures
Problem
Calculator Answer
Answer Rounded to the
correct number of significant
figures
1) 2.698 x 33.20 x 1.5611
2) 8.032 / 0.591
3) (3.2 x 103) (4.21 x 102)
4) (2.5000 x 106) (3.92 x 10-3)
5) 3 x 154
6) 3.00 x 154
7) 1.65 x 102 / (2.3456 x 103)
8) 32.21000 x 3.540000
9) 5.5 x 105 / 3.3 x 103
10) 2.5 x 2.34 x 3.6543
B. Complete the addition or subtraction problem and provide the final answer with the
correct number of significant figures.
Problem
Calculator Answer
Answer Rounded to the correct
number of places past the decimal
11. 7.623 + 85.0 + 9.815
12. 230.72 + 0.00861
13. 10.96-5.5
14. 10.96-5.555
15. 9.0731 +0.00078
16. 23.6 – 16.1218
17. 21.5- 2.5 + 5.5555
18. 32.21000 +3.540000
19. 5.5 - 3.325
20. 2.5 + 2.34 + 3.6543
C. Complete the indicated operation and provide the final answer with the correct number
of significant figures and proper units.
Problem
Calculator
How many sig figs Rounded answer
Answer
or places past the with units
decimal?
21. 0.00598 mm + 0.004 mm
22. 79.6 mL + 0.0168 mL
23. 27 L – 0.0838 L
24. 420 cm – 19.11 cm
25. 6.77 kg x 0.9 kg
26. 16.2 mL x 23.79 mL
27. 596,000 mg ÷ 0.0023 mg
28. 56.200 g ÷ 260.5 g
29. 23 L + 1.59 L – 3.01 L
30. 21.4 km x 0.569 km ÷ 0.9 Km
Solubility Table Practice
Directions: Put an “S” next to the soluble compounds and an “I” next to insoluble compounds.
Treat a slightly soluble compound as insoluble and use an “I”. Write “MS” next to those
marginally soluble compounds that may go either way. Make a statement justifying why the
compound is “S”, “I” or “MS”.
Example:
Ca(OH)2:
1. Mg(SO4):
2. HCl:
3. NaBr:
4. (NH4)2S:
5. Ba(OH)2:
6. Na(NO)3:
7. Ag(SO4):
8. K(C2H 3O2):
9. Li 2(SO4):
10. Sr(SO4):
11. AgCl:
MS - only IA and IIA metal hydroxides are soluble (with exception of Be
and Mg metal hydroxide which are insoluble).
12. Ca(ClO3) 2:
13. PbI2:
14. KBr:
15. Ni(NO3)2:
16. Be(OH) 2:
17. Rb3(PO4):
18. Ca(CO3):
19. Na2S:
20. HNO3:
Naming Acids Practice
Write the formula for each of the acids listed below:
1. Nitric acid
2. Chloric acid
3. Acetic acid
4. Hydrobromic acid
5. Sulfurous acid
6. Chlorous acid
7. Hydrochloric acid
8. Phosphoric acid
9. Nitrous acid
10. Hydrofluoric acid
11. Perchloric acid
12. Hydroiodic acid
13. Phosphorous acid
14. Carbonic acid
15. Sulfuric acid
Name each of the following acids:
16. HClO4
17. H3PO4
18. HCl (aq)
19. H2SO4
20. HNO2
21. HI (aq)
22. HC2H3O2
23. HF
(aq)
24. H3PO3
25. HClO3
26. H2CO3
27. H2SO3
28. HClO2
29. HNO3
30. HBr
(aq)
Important Scientists (Use studyblue.com to help study)
Scientists
Democritus
Antoine Lavoisier
John Proust
John Dalton
Dmitri Mendeleev
JJ Thomson
Ernst Rutherford
Marie Curie
Max Planck
Henry Moseley
Niels Bohr
Important experiments
Discoveries/Contributions
de Broglie
Heisenberg and Schrodinger
James Chadwick
Glenn Seaborg