Dear Future AP Chemistry Student,

We are excited to see that you have signed up for AP Chemistry next year! It is a challenging course that will improve your analytical and problem solving skills. Most students who take the class leave with an enhanced enthusiasm for science, and many go on to major in chemistry or chemical engineering in college.

To improve your readiness for the course, you are expected to complete a summer assignment on the first four chapters of our textbook. This involves memorizing a list of common ions, writing names and formulas confidently, using significant figures and solving stoichiometry problems systematically. This is material that was covered during your Honors Chemistry course. Students should complete the summer assignment in small segments throughout the summer, rather than all at once soon before school begins. On the first day of school the packets will be collected and graded for correctness.

We have included a packet of the material containing the practice problems you are expected to solve. It is expected that you come to class next fall with the majority of this material already mastered, needing only light review and clarification. Please see either of us if you wish to check out a textbook now.

Contents of the Review Packet:

  • List of common ions to memorize
  • A sample quiz on names and formulas
  • Review of first 4 chapter
  • Sample questions of Unit One Test

Please do not hesitate to stop by the AP Chemistry room, B217, if you have any questions or need any additional materials to help in your preparation. Enjoy your summer!

Sincerely,

Ap- Chemistry Teachers

Mr. Hall and Ms. Balimtas

AP-CHEM Handout 1 REVIEW TOPICS FROM HONORS CHEMISTRY

Here are some of the most important concepts from HONORS CHEMISTRY for which you need to have a good understanding.

Naming: molecular compounds, ionic compounds, acids

Stoichiometry and limiting reactant problems

Electrolytes, Solubility, Net Ionic Equations

Be able to identify whether a compound is a strong, weak or nonelectrolyte

Be able to determine whether a compound is soluble in water or not (refer to Solubility Chart)

Write molecular, total ionic, and net ionic equations for exchange (precipitation and acid-base), and simple oxidation-reduction reactions

Molarity calculations, including dilution and stoichiometry

Electron Configurations and Orbital Diagrams of Atoms and Ions



MATH REVIEW

SOLVING FOR x

You need to get x all by itself in the numerator and everything else on the other side of the equation. Read the following examples:

(1)multiply both sides by 4:

divide both sides by 3:

(2)multiply both sides by x:

divide both sides by 8:

(3)divide both sides by 4:

take the square root of both sides:

(4)divide both sides by 2:

raise both sides to the 1/3 power

NOTE: On your calculator you should have a yx or xy button to do this. Find it and learn how to use it.

(5)square and cube terms:

gather terms:

divide both sides by 108:

raise both sides to the 1/5 power:

(6)subtract 3 from both sides:

raise both sides to the 1/3 power:

(7)multiply left side out:

gather terms on the left side:

This is a quadratic equation. It has the form ax2 + bx + c = 0. Your calculator may have the solutions for this already programmed in, so you can use that. If not, you can calculate the solutions (there are two) from the quadratic formula:

In this case, a = 1, b = 4 and c = 13, so x = 6 or 2. You would need to decide which choice is better based on the problem.

(8)multiply both sides by (0.010  x):

gather terms on the left side:

use the quadratic formula:a = 1, b = 3.0104 and c = 3.0106

solve for x:x = 0.016 or 0.019

LOGARITHMS

common or base 10 logarithm:loginverse:if x = log(y) then y = 10x

natural logarithm:lninverse:if x = ln(y) then y = ex

Find these buttons on your calculator and learn how to use them.

Significant Figure Rule for Logarithms:

log(3.0103) = 2.52108.39 = 4.1109

   

2 total SF 2 decimal places 2 decimal places 2 total SF

Other Rules to Memorize:log(1) = 0 100 = 1ln(1) = 0 e0 = 1

log(xy) = log(x) + log(y)ln(xy) = ln(x) + ln(y)

Conversion Factors

METRIC UNITS THAT USE THE PREFIXES
Base Units / Derived Units
length / meter / m / pressure / pascal / Pa
mass / gram / g / pressure / bar / bar
time / second / s / energy / joule / J
amount of substance / mole / mol / energy / calorie / cal
volume / liter / L
METRIC PREFIXES
“U” stands for any unit listed above
Symbol / Definition
L
A
R
G
E / mega, M / 1 MU = 1106 U or 1,000,000 U
kilo, k / 1 kU = 1103 U or 1000 U
S
M
A
L
L / deci, d / 1 U = 10 dU or 1101 dU
centi, c / 1 U = 100 cU or 1102 cU
milli, m / 1 U = 1000 mU or 1103 mU
micro,  / 1 U = 1,000,000 U or 1106U
nano, n / 1 U = 1,000,000,000 nU or 1109 nU
pico, p / 1 U = 1,000,000,000,000 pU or 11012 pU
CONSTANTS
NAME / SYMBOL / VALUE
Avogadro’s number / NA / 6.0221023 /mol*
Gas constant / R / 0.08206 atm-L/mol-K*
Speed of light / c / 3.00108 m/s*
Standard temp. & pressure (gas) / STP / 273.15 K and 1 atm
CONVERSION FACTORS
METRIC / ENGLISH / ENGLISH  METRIC
LENGTH / 1 cm = 1108 Å / 12 in. = 1 ft.
3 ft. = 1 yd.
5280 ft. = 1 mi. / 1 in. = 2.54 cm
1 mile = 1.609 km*

MASS / WEIGHT

/ 1000 kg = 1 metric ton / 2000 lb. = 1 ton
16 oz. = 1 lb. / 1 lb. = 453.6 g*
VOLUME / 1 L = 1 dm3
1 mL = 1 cm3
1000 L = 1 m3 / 3 tsp. = 1 Tbsp.
16 Tbsp. = 1 cup
2 cups = 1 pint
2 pints = 1 quart
4 quarts = 1 gal.
8 fluid oz. = 1 cup / 1 qt. = 0.9464 L*
or 1.057 qt.* = 1 L
TEMPERATURE / K = °C + 273.15 / °F = (1.8)(°C) + 32
°C = (°F  32) / 1.8
Note: 1.8 = 9/5
ENERGY / 1 cal = 4.184 J
PRESSURE / 1 atm= 760 mm Hg
= 760 torr
= 101.325 kPa*
= 1.01325 bar* / 1 atm= 14.7 psi*
= 29.92 in. Hg*

NOTE:The ounces that measure mass are completely different from and unrelated to the fluid ounces that measure volume.

PROPERTIES OF WATER
NAME / VALUE
Density of liquid / 1.00 g/mL*
Specific heat of liquid / 4.184 J/gC
Freezing/Melting point / 0.00 C
Boiling point / 100.00 C

List of Common Ions to Know

The following ions must be memorized.

Ammonium, NH4+

Hydronium, H3O+

Mercury(I), Hg22+

Mercury(II), Hg2+

Zinc, Zn2+

Silver, Ag+

Nitrite, NO2-

Nitrate, NO3-

Acetate, C2H3O2-

Carbonate, CO32-

Bicarbonate, HCO3-

Sulfite, SO32-

Sulfate, SO42-

Phosphite, PO33-

Phosphate, PO43-

Hypochlorite, ClO-

Chlorite, ClO2-

Chlorate, ClO3-

Perchlorate, ClO4-

Hydroxide, OH-

Chromate, CrO42-

Dichromate, Cr2O72-

Cyanide, CN-

Fluoride, F-

Chloride, Cl-

Bromide, Br-

Iodide, I-

Thiosulfate, S2O32-

Permanganate, MnO4-

IONS TABLE

ANIONS
1 / 2 / 3
-ide / H1 / hydride / O2 / oxide / N3 / nitride
F1 / fluoride / S2 / sulfide
Cl1 / chloride / Se2 / selenide
Br1 / bromide / Te2 / telluride
I1 / iodide / O22 / peroxide
CN1 / cyanide
OH1 / hydroxide
-ite / ClO1 / hypochlorite / SO32 / sulfite
ClO21 / chlorite
BrO1 / hypobromite
BrO21 / bromite
IO1 / hypoiodite
IO21 / iodite
HSO31 / hydrogen sulfite (bisulfite)
NO21 / nitrite
-ate / ClO31 / chlorate / CO32 / carbonate / PO43 / phosphate
ClO41 / perchlorate / CrO42 / chromate
BrO31 / bromate / Cr2O72 / dichromate
BrO41 / perbromate / HPO42 / monohydrogen phosphate
IO31 / iodate / C2O42 / oxalate
IO41 / periodate / SO42 / sulfate
HCO31 / hydrogen carbonate (bicarbonate) / S2O32 / thiosulfate
HSO41 / hydrogen sulfate (bisulfate)
H2PO41 / dihydrogen phosphate
C2H3O21 / acetate
NO31 / nitrate
MnO41 / permanganate
CATIONS
1+ / 2+ / 3+ / 4+
Monatomic
Without
Roman
Numeral / H1+ / hydrogen / Be2+ / beryllium / Al3+ / aluminum
Li1+ / lithium / Mg2+ / magnesium / Ga3+ / gallium
Na1+ / sodium / Ca2+ / calcium / In3+ / indium
K1+ / potassium / Sr2+ / strontium / Al3+ / aluminum
Rb1+ / rubidium / Ba2+ / barium
Cs1+ / cesium / Zn2+ / zinc
Au1+ / gold(I)
Ag1+ / silver / Cd2+ / cadmium
Monatomic
With
Roman
numeral / Cu1+ / copper(I) / Co2+ / cobalt(II) / Bi3+ / bismuth(III) / Pb4+ / lead(IV)
Tl1+ / thallium(I) / Cr2+ / chromium(II) / Co3+ / cobalt(III) / Sn4+ / tin(IV)
Cu2+ / copper(II) / Cr3+ / chromium(III)
Fe2+ / iron(II) / Au3+ / gold(III)
Mn2+ / manganese(II) / Fe3+ / iron(III)
Hg2+ / mercury(II) / Mn3+ / manganese(III)
Ni2+ / nickel(II) / Tl3+ / thallium(III)
Pb2+ / lead(II)
Sn2+ / tin(II)
Polyatomic / NH41+ / ammonium / Hg22+ / mercury(I)

MONATOMIC IONS YOU MUST KNOW

1 / 2 / 3 / 4 / 5 / 6 / 7 / 8 / 9 / 10 / 11 / 12 / 13 / 14 / 15 / 16 / 17 / 18
H1+ / H1
Li1+ / Be2+ / N3 / O2 / F1
Na1+ / Mg2+ / Al3+ / S2 / Cl1
K1+ / Ca2+ / Cr3+ / Mn2+ / Fe2+
Fe3+ / Co3+ / Ni2+ / Cu1+
Cu2+ / Zn2+ / Ga3+ / Se2 / Br1
Rb1+ / Sr2+ / Ag1+ / Cd2+ / In3+ / Sn2+ / Te2 / I1
Cs1+ / Ba2+ / Hg22+
Hg2+ / Tl1+
Tl3+ / Pb2+ / Bi3+

NOTE: Hg2+2 is not really a monatomic ion; it is included here only for comparison.

SOLUBILITY RULES FOR IONIC COMPOUNDS IN WATER

Rule / Applies to / Statement / Exceptions
1 / Li1+,, Na1+, K1+, NH41+ / Group IA and ammonium compounds are soluble. / none
2 / C2H3O21 and NO31 / Acetates and nitrates are soluble. / none
3 / Cl1, Br1, I1 / Most chlorides, bromides, and iodides are soluble. / AgCl, Hg2Cl2, PbCl2
AgBr, HgBr2, Hg2Br2, PbBr2
AgI, HgI2, Hg2I2, PbI2
4 / SO42 / Most sulfates are soluble. / CaSO4, SrSO4, BaSO4, Ag2SO4, Hg2SO4, PbSO4
5 / CO32 / Most carbonates are insoluble. / Group IA carbonates, (NH4)2CO3
6 / PO43 / Most phosphates are insoluble. / Group IA phosphates, (NH4)3PO4
7 / S2 / Most sulfides are insoluble. / Group IA sulfides, (NH4)2S
8 / OH1 / Most hydroxides are insoluble. / Group IA hydroxides, Ca(OH)2, Sr(OH)2, Ba(OH)2

Source: “Essentials of General Chemistry”, Ebbing, Gammon and Ragsdale, 2nd ed., page 99.