Download Chem Sheets to Memorize

AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
Dear AP CHEM STUDENTS,
I’m looking forward to the school year and the work we’re going to do together. This
packet is meant to refresh you on several things you already learned so that you have
them firmly in mind for the start of school I recommend that you review your Honors
Chemistry notes, and start looking at this material several weeks before school starts in
the fall. This assignment will be graded
Good luck, and have a wonderful and Productive summer!
Sincerely,
J.Boppana
Chem Sheets to Memorize
SOLUBILITY CHART
Soluble
No
NO3
CHeating
-
Exceptions
Insoluble
-2
Exceptions
Group IA, NH4+
Sr+2 Ba+2 Ca+2
---
Smoking
S
CH3COO-
---
Counter
CO3-2
Group IA, NH4+
Cellphones
Cl-
Ag+ Pb+2
Hg2+2
Productive
PO4-3
Group IA, NH4+
Bullying
Br-
''
O (ZERO)
OH-
Group IA, NH4+
Sr+2 Ba+2 Ca+2
Intimidating
I-
''
Students
SO4-2
Sr+2 Ba+2 Pb+2
Hg2+2
Acids
HF – weak
HCl – strong
HBr – strong
HI – strong
H2SO4 – strong
HNO3 – strong
HClO3 – strong
Bases
LiOH – strong
NaOH– strong
KOH – strong (all IA Metal Hydroxides)
Ca, Ba and Sr Hydroxide too
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
HClO4 – strong
All else are weak
H2CO3 → H2O + CO2
(very weak acid-breaks down!)
Special Reactions
Metal
metal + acid → salt + H2
metal oxide + H2O → metal hydroxide
metal oxide + CO2 → metal carbonate
metal chloride + O2 → metal chlorate
Oxidizers
Acid
MnO4- or MnO2→ Mn+2
CrO4-2 → Cr+3
Cr2O7-2 → Cr+3
NO3- (dil) → NO
NO3- (conc) → NO2
metallic ions → metallous ions
free halogens → halide ions
Na2O2 → NaOH
HClO4 → ClC2O4-2 → CO2
H2O2 → O2, H2O
Reducers
halide ions → free halogens
free metals → metal ions
metalous ions → metallic ions
SO3-2 → SO4-2
NO2- → NO3free halogens (dil) → hypohalite ions
free halogens (conc) → halate ions
Nonmetal
nonmetal + H2O → oxy-acid
SO3 + H2O → H2SO4
SO2 + H2O → H2SO3
N2O5 + H2O → 2 HNO3
N2O3 + H2O → 2 HNO2
P2O5 + 3H2O → 2 H3PO4
P2O3 + 3H2O → 2 H3PO3
Base
Cr2O7-2 → CrO4-2
Neutral
MnO4- → MnO2
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
Colors of Complex ions
Ion
Color
[Cr(H2O)6]+2
blue
[Cu(H2O)6]+2
blue
[Cu(H2O)6]+3
blue/violet
[Mn(H2O)6]+2
very pale pink
[Co(H2O)6]+2
pink
[Fe(H2O)6]+2
pale green
[Ni(H2O)6]+2
green
[Fe(H2O)6]+3
yellow/brown
Flame Test Colors
Ion
Flame color
Red (various shades)
Li+, Sr2+, Ca2+
Yellow/Orange
Na+
Lilac
K+
Green
Ba2+
Blue-green
Cu2+
AP Chemistry
Summer Review
Winston Churchill High School
TRANSITION METAL ION COLORS
+1
+2
+3
+4
2011-2012
+5
+6
+7
YELLOW FOR
CHROMATE
ORANGE FOR
DICHROMATE
ION
DARK GREEN
PURPLE
colorless
Sc
VIOLET
COLORLESS
VIOLET
GREEN
BLUE
Cr
BLUE
GREEN
Mn
Co
PALE
PINK
PALE
GREEN
PINK
Ni
GREEN
Ti
V
Fe
Cu
COLORLESS
Zn
BROWN
YELLOW
REDDISH
BROWN
ORANGE/
YELLOW
BLUE
Colorless
Common Precipitate colors:
WHITE
AgCl
BLUE
YELLOW
BLACK
GREEN
Many
Copper
(II) ppt’s.
AgI
Many
Sulfides
Many Fe(II)
ppt’s.
PbI2
BaSO4
PbCl2
Many
nontransition
metal
hydroxides
Many
nontransition
metal
carbonates
and sulfates
REDDISH
BROWN
Many Fe(III)
ppt’s.
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
Common Tests for gases
GAS
Hydrogen gas
Oxygen gas
Carbon Dioxide gas
Ammonia gas
Common tests for cations and anions
ION
Carbonate and Hydrogen carbonate
Sulfate
TEST
Squeaky pop with lighted splint
Re-lights glowing splint
Turns limewater (Calcium Hydroxide
solution) milky
Pungent odor, turns red litmus paper
blue,gives dense white fumes in
contact with conc.HCl fumes
TEST
Release CO2 gas with acids
White ppt of BaSO4 with barium ions
Chloride
White of AgCl with silver ions
Bromide
Cream ppt of AgBr with silver ions
Iodide
Yellow ppt of AgI with silver ions
Ammonium
NH3 released with hydroxide ions
HALOGENS:
Fluorine gas – pale yellow/green,
Chlorine gas – green,
Bromine liquid –orange/brown,
Iodine solid – dark purple
NO2 gas – orange/brown
Color Changes in REDOX reactions
1) MnO4-(aq) → Mn2+(aq)
(Dark Purple) →(Pale Pink)
2) Cr2O72-(aq) →Cr3+(aq)
(Orange) → (Green)
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
Acid/Base Indicator Color changes
INDICATOR
ACID
RED
RED
RED
RED
COLORLESS
Methyl orange
Methyl red
Litmus
Universal
Phenolphthalein
BASE
YELLOW
YELLOW
BLUE
BLUE/PURPLE
PINK
POLYATOMIC IONS
Group IIIB or
13
Charge -3
Group IVB or 14
Group VB or 15
Group VIB or 16
Group VIIIB or
17
Charge -2
Charge -1
NO3
nitrate
NO2-1
nitrite
O
F
-1
BO3-3
borate
one member in
the ion family
Remember:
 ions with the
greater # of
oxygens: ATE
 ions with the
fewer # of
oxygens: ITE
 adding
hydrogen in
front makes
BI and reduces
charge by 1
CO3-2
carbonate
SiO3-2
silicate
PO4-3
phosphate
PO3-3
phosphite
SO4-2
SO3-2
AsO4-3
AsO3-3
SeO4-2
selenate
SeO3-2
selenite
arsenate
arsenite
Charge -3
two members in
the ion family
sulfate
sulfite
TeO4-2
telurate
TeO3-2
telurite
Charge -2
ClO4-1
perchlorate
ClO3-1 chlorate
ClO2-1 chlorite
ClO-1
hypochlorite
BrO4-1
perbromate
BrO3-1 bromate
BrO2-1 bromite
BrO-1
hypobromite
IO4-1
periodate
IO3-1
iodate
-1
IO2
iodite
IO-1
hypoiodite
Charge -1
four members in
the ion family
AP Chemistry
Summer Review
Winston Churchill High School
Other important
acetate
hydroxide
permanganate
cyanide
hydronium
ammonium
polyatomic ions to remember:
C2H3O2-1
chromate
-1
OH
dichromate
MnO4-1
peroxide
-1
CN
oxalate
H3O+1
thiosulfate
+1
NH4
tartrate
2011-2012
CrO4-2
Cr2O7-2
O2-2
C2O4-2
S2O3-2
C2H4O6-2
bisulfite
HSO3-1
bisulfate
HSO4-1
bicarbonate
HCO3-1
biphosphite
HPO3-2
biphosphate
HPO4-2
hydrogen biphosphite
H2PO3-1
I.NOMENCLATURE: NAMING AND WRITING FORMULAS OF CHEM.COMPOUNDS
Formula
Name
1. P4O10
2. ZnAt2
3. SBr6
4. CaF2
5. P2S3
6.
carbon monoxide
7.
sodium hydride
8.
aluminum selenide
9.
xenon hexafluoride
10.
dinitrogen monoxide
11. KClO3
12. Pb(OH)2
13. Ca(MnO4)2
14. N2O4
15. Ti(HPO4)2
16.
manganese (VII) oxide
17.
francium dichromate
18.
copper (II) dihydrogen phosphate
19.
silver chromate
20.
ammonium oxalate
21. (NH4)2SO3
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
22. Ni3(PO4)2
23. Fe(IO2)3
24. NaBrO2
25. H3PO3
26.
tartaric acid
27.
hydrotellluric acid
28.
mercury (I) nitrate
29.
vanadium (V) oxide
30.
tetraphosphorous decaoxide
II. Significant Figures
1. Give the number of sig figs in each of the following numbers
a. 123 b. 0.078 c. 89007 d. 12,000 e. 1,000,000,000.0
f. 0.009 g. 23,000. h. 34,000 i. 34.89 j. 101
2. Do the following calculations giving the answer in the appropriate number of sig figs.
a. 1.23 + 75 b. 1.89 - .20 c. 45.6 x 8.2 d. 234/0.298
e. 0.887 + 0.3 f. 2340 - 100 g. 12.45 x 3 h. 25,600/ 3.0
3. Do the following calculations giving the answer in the appropriate number of sig figs
a. 45.0 x 9.0 + 89.22/ 75 b. (2.88 + .5) x ( 23,000 - 0.11)
c. 0.8897 x 2.15 + 0.002/.1 d. (8 + 9)/(34.0 – 20.)
III. Reactions
Please write net ionic balanced reactions (with states of matter included) for the following
questions on a separate piece of paper. You’ll have reactions that are classified as
precipitation, acid-base, or redox (reduction-oxidation…like, synthesis, decomposition, and
single displacement/replacement).

Any ion has an aqueous state of matter.

For acid-base reactions, strong acids (HCl, HBr, HI, H2SO4, HClO4, and HNO3) and
strong bases (metal ions in groups 1 and 2 paired with hydroxide (OH-) completely
dissociate. Weak acids and bases do not.

For precipitation (and some redox) reactions, use the solubility rules below to
determine which salts are soluble (aqueous) or insoluble (solid). Only aqueous
solutions can dissociate…solids, liquids, and gases cannot.
1. Salts containing Group I elements are soluble (Li+, Na+, K+, Cs+, Rb+). Exceptions to
this rule are rare. Salts containing the ammonium ion (NH4+) are also soluble.
2. Salts containing nitrate ion (NO3-) and acetate ion (C2H3O2) are generally soluble.
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
3. Salts containing Cl -, Br -, F-, and I - are generally soluble. Important exceptions to
this rule are halide salts of Ag+, Pb2+, and (Hg2)2+. Thus, AgCl, PbBr2, and Hg2Cl2 are
all insoluble.
4. Most silver salts are insoluble. AgNO3 and AgC2H3O2 are common soluble salts of
silver; virtually anything else is insoluble.
5. Most sulfate salts are soluble. Important exceptions to this rule include BaSO4,
PbSO4, Ag2SO4 and SrSO4 .
6. Most hydroxide salts are only slightly soluble. Hydroxide salts of Group I elements
are soluble. Hydroxide salts of Group II elements (Ca, Sr, and Ba) are slightly
soluble. Hydroxide salts of transition metals and Al3+ are insoluble. Thus, Fe(OH)3,
Al(OH)3, and Co(OH)2 are not soluble.
7. Most sulfides of transition metals are highly insoluble. Thus, CdS, FeS, ZnS, and
Ag2S are all insoluble. Arsenic, antimony, bismuth, and lead sulfides are also
insoluble.
8. Most chromates, phosphates, bicarbonates, and carbonates are frequently insoluble
except those with alkali metals and ammonium.
Acid-Base Example: Hydrochloric acid is added to a solution of zinc hydroxide.
*First, write a molecular equation.
HCl + Zn(OH)2  ZnCl2 + H2O
*Next, you need to see what dissociates and what does not. Hydrochloric acid is a strong
acid, so it will completely dissociate into its ions while zinc hydroxide is a weak base, so it
will not dissociate. Zinc chloride is a soluble salt according to the solubility rules above, so it
will also dissociate into its ions.
*Wait to balance the reaction until the end.
H+ + Cl- + Zn(OH)2  Zn+2 + Cl- + H2O
*Last, you need to see what can be cancelled out. Species that are identical on both sides of
the reaction, called spectator ions, can be cancelled out. Cl- is present on both sides of the
reaction and therefore can be cancelled out…giving you your net ionic reaction that you’ll
now balance and put back on states of matter.
2 H+ (aq) + Zn(OH)2 (aq)  Zn+2 (aq) + 2 H2O (l )
Redox Example: Silver metal reacts with a solution of sodium nitrate.
Ag + NaNO3  Na + AgNO3
*Ag is a solid. NaNO3 is a soluble salt according to the solubility rules above, so it will
dissociate into its ions. Na is a solid. AgNO3 is also a soluble salt and will dissociate.
Ag + Na+ + NO3-  Na + Ag++ NO3-
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
*NO3- is a spectator ion.
Ag (s) + Na+ (aq)  Na (s) + Ag+ (aq)
Precipitation Example: Barium acetate is mixed with potassium sulfate.
Ba(C2H3O2)2 + K2SO4  BaSO4 + KC2H3O2
*According to the solubility rules, barium sulfate is the only insoluble salt. So, everything
else will dissociate.
Ba+2 + C2H3O2- + K+ + SO4-2  BaSO4 + K+ + C2H3O2*The potassium ions and acetate ions can be cancelled out.
Ba+2 (aq) + SO4-2 (aq)  BaSO4 (s)
***Here are your questions. Please do these on a separate piece of paper.
1. Solid sodium bicarbonate is mixed with copper (II) nitrate.
2. Magnesium oxide is heated.
3. Acetic acid is added to a solution of ammonia.
4. Iron (III) chloride is mixed with silver sulfite.
5. A solid piece of aluminum is put into a solution of nickel (II) chloride.
6. A solution of lithium chloride is added to a solution of lead (IV) nitrite.
7. Sulfuric acid is added to a solution of aluminum hydroxide.
8. Cadmium nitrate is added to sodium sulfide.
9. Chromium (III) sulfate is added to ammonium carbonate.
10. Methane combusts in air.
In each of the equations below, the reactants are written correctly. You must write the
correct products and then balance the equation. It might be useful to identify the type of
chemical reaction before writing the products.
1. CaCO3 
2. Al + O2 
3. Fe + CuSO4 
4. C6H12 + O2 
5. Zn + H2SO4 
6. Cl2 + MgI2 
7. NaOH 
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
8. Fe + HCl 
9. NaOH + H3PO4 
10. (NH4)2SO4 + Ca(OH)2 
11. AgNO3 + K2SO4 
12. Mg(OH)2 + H3PO4 
13. Na + H2O 
14. KClO3 
15. Al2(SO4)3 + Ca3(PO4)2 
16. SO2 + H2O 
17. (NH4)3PO4 + Ba(OH)2 
18. Ca(OH)2 + HNO3 
19. C3H8 + O2 
20. Li + S 
IV.Electron Structure and Periodicity
*Please do all questions on a separate piece of paper.
*You will need to know about valence electrons, electron shells, orbital notation, electron
configuration, atomic radius, ionization energy, and electronegativity to do these questions.
1. Draw the orbital notation for nickel.
2. How many unpaired electrons are in arsenic?
3. Write the electron configuration for palladium.
4. How many valence electrons are in mercury?
5. Write the electron configuration for uranium.
6. Write the noble gas electron configuration for lead.
7. Which is more electronegative, sulfur or chlorine, and why?
8. Which has a larger atomic radius, potassium or bromine, and why?
9. Which has the smaller ionization energy, nitrogen or phosphorus, and why?
10. Write the noble gas electron configuration for copper.
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
Short Answer question from previous AP EXAM
11. Use the principles of atomic structure and/or chemical bonding to explain each of the
following. In each part, your answer must include references to both substances.
a. The atomic radius of Li is larger than that of Be.
b. The second ionization energy of K is greater than the second ionization energy
of Ca.
c. The carbon-to-carbon bond energy in C2H4 is greater than it is in C2H6.
d. The boiling point of Cl2 is lower than the boiling point of Br2.
Atomic Structure Sample problems:
12. Give the symbols for the isotopes of Carbon, nitrogen and uranium and Determine
the number of protons, electrons and neutrons in each isotope.
13. Given the data below determine the average atomic mass
Isotope %
a. Sb-121 57.25%
Sb-123 42.75%
Abundance Isotopic Mass
120.9038 amu
122.0041 amu
b. Ag-107 51.82%
Ag-109 48.18%
106.90509 amu
108.9047 amu
Mole Concept Sample Problems
14. Convert each of the following to moles.
a. 12.64 g NaOH
b. 3.00 x 1024 atoms Au
c. 40.0 L of Ne gas
d. 800. g CaBr2
e. 3.011 x 1022 molecules H2O
f. 6.78 L of Ar gas
15. Do the following
a. Given 0.250 moles of krypton determine
(i) the mass (ii) the number of atoms (iii) the volume at STP
b. Given 0.750 moles of oxygen determine
V. Bonding
*Please do all questions on a separate piece of paper.
*You will need to know about Lewis structures, covalent bonding, shape names, and bond
angles to do these questions.
*For the following questions, draw the Lewis Structure, name the shape, and state the bond
angle.
1. SeCl2
2. NO3-1
3. OF2
4. BF3
5. SO4-2
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
6. NH4+
7. CO2
8. CH3NH2
9. HCOOH
10. HCN
VI.Stoichiometry
*Please do all questions on a separate piece of paper.
*You will need to be able to write molecular chemical reactions and do mole conversions to
do these questions.
1. 30.5 g of sodium metal reacts with a solution of excess lithium bromide. How many
grams of lithium metal are produced?
2. How many molecules are in 100. L of potassium hydroxide solution at STP?
3. Propane, C3H8, undergoes combustion. How many grams of propane are needed to
produce 45.9 g of water?
4. How many moles are in 3.02 x 1026 molecules of water?
5. Find the empirical and molecular formulas for a compound containing 11.66 g iron
and 5.01 g oxygen if the molar mass of the compound is 320 g/mol.
6. A solution of 3.50 g of sodium phosphate is mixed with a solution containing 6.40 g
of barium nitrate. How many grams of barium phosphate can be formed?
7. Find the empirical and molecular formulas for a compound containing 5.28 g of tin
and 3.37 g of fluorine if the molar mass of the compound is 584.1 g/mol.
8. Octane, C8H18, undergoes combustion. How many grams of oxygen are needed to
burn 10.0 g of octane?
9. Sodium azide, NaN3, decomposes into its elements. How many grams of sodium
azide are required to form 34.8 g of nitrogen gas?
10. Ammonia reacts with oxygen gas to form nitrogen monoxide and water. How many
grams of nitrogen monoxide are formed when 1.50 g of ammonia react with 2.75 g of
oxygen gas?
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
Short Answer Problems from Previous AP EXAMS
2. The reaction between silver ion and solid zinc is represented by the following
equation:
2Ag+ (aq) + Zn (s)  Zn+2 (aq) + 2Ag (s)
A 1.50 g sample of Zn is combined with 250 mL of 0.110 M AgNO3 at 25°C.
a. Identify the limiting reagent. Show calculations to support your answer.
b. On the basis of the limiting reactant that you identified in part (i),
determine the value of [Zn+2] after the reaction is complete.
3. Consider the hydrocarbon pentane, C5H12 (molar mass 72.15 g).
a. Write the balanced equation for the combustion of pentane to yield carbon
dioxide and water.
b. What volume of dry carbon dioxide, measured at 25°C and 785 mmHg,
will result from the complete combustion of 2.50 g pentane?
4) Find the mass percent of nitrogen in each of the following compounds:
a. NO
b. NO2
c. N2O4
d. N2O
5) Benzene contains only carbon and hydrogen and has a molar mass of 78.1 g/mol.
Analysis shows the compound to be 7.74% H by mass. Find the empirical and
molecular formulas of benzene.
6) Calcium carbonate decomposes upon heating, producing calcium oxide and carbon
dioxide gas.
a. Write a balanced chemical equation for this reaction.
b. How many grams of calcium oxide will be produced after 12.25 g of calcium
carbonate is completely decomposed?
c. What volume of carbon dioxide gas is produced from this amount of calcium
carbonate, at STP?
AP Chemistry
Summer Review
Winston Churchill High School
2011-2012
7) Hydrogen gas and bromine gas react to form hydrogen bromide gas.
a. Write a balanced chemical equation for this reaction.
b. 3.2 g of hydrogen gas and 9.5 g of bromine gas react. Which is the limiting
reagent?
c. How many grams of hydrogen bromide gas can be produced using the amounts in
(b)?
d. How many grams of the excess reactant is left unreacted?
e. What volume of HBr, measured at STP, is produced in (b)?
8) When ammonia gas, oxygen gas and methane gas (CH4) are combined, the products
are hydrogen cyanide gas and water.
a. Write a balanced chemical equation for this reaction.
b. Calculate the mass of each product produced when 225 g of oxygen gas is reacted
with an excess of the other two reactants.
c. If the actual yield of the experiment in (b) is 105 g of HCN, calculate the percent
yield.
9) When solutions of potassium iodide and lead (II) nitrate are combined, the products
are potassium nitrate and lead (II) iodide.
a. Write a balanced equation for this reaction, including (aq) and (s).
b. Calculate the mass of precipitate produced when 50.0mL of 0.45M potassium
iodide solution and 75mL of 0.55M lead (II) nitrate solution are mixed.
c. Calculate the volume of 0.50M potassium iodide required to react completely with
50.0mL of 0.50M lead (II) nitrate.