AP Chemistry Summer Preparation

AP Chemistry Summer Preparation

Course Description______

• AP Chemistry is designed so that it is equivalent to a first year college chemistry course.
• The topics learned in Chemistry Pre-AP will be elaborated upon and many new topics will be discussed in great detail:

▫Matter & Measurement

▫Stoichiometry

▫Chemical Reactions (single & double replacement, redox, synthesis, decomposition, etc.)

▫Acids & Bases

▫Atomic Structure & Periodic Trends

▫Covalent & Ionic Bonding

▫Thermochemistry & Spontaneity

▫Solutions

▫Solids & Liquids

▫Equilibrium

▫Kinetics

▫Electrochemistry

▫Nuclear Chemistry

▫Organic Chemistry

• Grades will be distributed so that they will mirror a college level course. As a result, most of the overall average in the course will be dependant on tests and quizzes.
• There will be quiz after every chapter and unit test after every 2-3 chapters.

Summer Preparation______

• You are expected to enter AP Chemistry with specific material learned in Chemistry Pre-AP.
• There will be a 100-point Test on the FRIDAY OF THE FIRST WEEK OF SCHOOLassessing your knowledge of BASIC material you should have learned in Chemistry Pre-AP and in this packet.
• There are reaction prediction practice problems on the class website under future AP Chemistry students.
• The following you NEED TO KNOW

▫Naming Ionic Compounds

▫Naming Covalent Compounds

▫Naming Acids

▫Common Polyatomic

▫Common Transition Metal Ions and their variable oxidation states

▫Solubility Rules

▫ Reaction Rules

▫Reaction Prediction (being able to predict the products and write a balanced NET IONIC chemical equation for a given set of reactants).

The documents included in this packet are a shortened version of materials you should have received in honors. Original documents maybe downloaded from my website under the Chemistry Pre-AP link!!!

Variable Oxidation States for Transition Metals______

Name / Symbol / Charge / Stock Name
Chromium / Cr / +2
+3 / Chromium (II)
Chromium (III)
Manganese / Mn / +2
+3 / Manganese (II)
Manganese (III)
Iron / Fe / +2
+3 / Iron (II)
Iron (III)
Cobalt / Co / +2
+3 / Cobalt (II)
Cobalt (III)
Copper / Cu / +1
+2 / Copper (I)
Copper (II)
Lead / Pb / +2
+4 / Lead (II)
Lead (IV)
Mercury / Hg / +1
+2 / Mercury (I)
Mercury (II)
Tin / Sn / +2
+4 / Tin (II)
Tin (IV)
Gold / Au / +1
+3 / Gold (I)
Gold (III)
Silver / Ag / +1
+2(rarely) / Silver
Silver (II)
Bismuth / Bi / +3
+5 / Bismuth (III)
Bismuth (V)
Antimony / Sb / +3
+5 / Antimony (III)
Antimony (V)
Cadmium / Cd / +2 / Cadmium
Zinc / Zn / +2 / Zinc

Polyatmic Ions______

Remember, hypo- prefix used when 1 less Oxygen than the -ite and per- prefix is used when there is 1 more oxygen than the -ate. You are responsible for being able to name an ion that it is not on this list by applying recognizing patterns among the ions.

Name / Symbol / Charge
Ammonium
Hydronium
Mercury I (Dimercury) / NH4
H3O
Hg2 / +1
+1
+2
Acetate
Benzoate / C2H3O2
C7H5O2 / -1
-1
Bromate
Perchlorate / BrO3
ClO4 / -1
-1
Chlorate / ClO3 / -1
Chlorite
Hypochlorite / ClO2
ClO / -1
-1
Cyanide
Cyanate
Cyanide / CN
OCN
CN / -1
-1
-1
Dihydrogen phosphate / H2PO4 / -1
Hypochlorite / ClO / -1
Hydrogencarbonate(bicarbonate) / HCO3 / -1
Hydrogen sulfate (bisulfate) / HSO4 / -1
Hydrogen sulfite (bisulfite) / HSO3 / -1
Hydroxide / OH / -1
Iodate / IO3 / -1
Nitrate / NO3 / -1
Nitrite / NO2 / -1
Perchlorate / ClO4 / -1
Permanganate
Manganate / MnO4
MnO4 / -1
-2
Thiocyanate / SCN / -1
Carbonate / CO3 / -2
Chromate / CrO4 / -2
Dichromate / Cr2O7 / -2
Oxalate
Peroxide / C2O4
O2 / -2
-2
Selenate / SeO4 / -2
Silicate / SiO3 / -2
Sulfate / SO4 / -2
Sulfite
Thiosulfate / SO3
S2O3 / -2
-2
Phosphate / PO4 / -3
Phosphite / PO3 / -3

Solubility Rules______

1. All compounds containing alkali metal cations and the ammonium ions are soluble – no exceptions.
2. All compounds containing nitrate, chlorate, perchlorate, acetate, and bicarbonate anions are soluble – no exceptions.
3. All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+, or Hg2+.
4. All sulfates are soluble except those containing Hg2+, Pb2+, Sr2+, Ca2+, or Ba2+.
5. All hydroxides are insoluble except compounds of the alkali metals, Ca2+, Sr2+,and Ba2+.
6. All compounds containing phosphate, sulfide (alkaline metals of sulfides are soluble), carbonate, and sulfite ions are insoluble except those that also contain alkali metals or NH4+.

Reaction Rules ______

I. Synthesis

A. Two elements produce a compound

B. Metal oxide + water produce a base (metallic hydroxide)

C. Nonmetal oxide + water produce an oxyacid

D. Metal oxide + nonmetal oxide produce a salt (ionic solid)

II. Decomposition

A. Reverse of above combination reactions

B. Metallic chlorates produce metallic chlorides + O2

C. Metallic carbonates produce metallic oxides + CO2

D. Compound electrolyzed produce foundational elements (may involve solute or water)

E. H2O2 produces H2O + O2

III. Single Replacement (Redox)

A. Metal replaces metal ion in compound if metal is more active (use activity series)

B. Metal replaces H in acids if metal is more active than H

C. Halogen replaces a halogen in compound if halogen more active

D. Very active metal replaces H in H2O; forms metallic hydroxide & H2

IV. Double Replacement:

Two aqueous ionic compounds react if one product is a precipitate, gas, or molecule (such as water). Be able to write net ionic equations.

V. Combustion

Oxygen (also termed as air in a problem) + compound (usually a hydrocarbon) produce oxides (usually carbon dioxide) of elements in compound and water.

*Remember there are always exceptions to rules in chemistry so practice reaction prediction problems. There are practice reaction prediction problems on the class website under FUTURE AP STUDENTS. Click on Chem Pre-AP equation notes (in word and power point form) for extra practice. Practicing will help you in preparation for the 1st test.

Please visit the class website for more info:

(There is also a link to my website from the Nova High School website)