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OHT Notes are the Overhead Transparency Notes and the reading is listed by Unit (U). Units are the sections in the OHT Notes and the problems are the Study Questions that are at the end of each Unit. Textbook is the textbook for the course, "Essential Concepts of Chemistry". The reading is listed by chapter (Ch.) number and subsection and the problems are the Self-Test Exercises at the end of each chapter.

Read the introductory material in each chapter when part of that chapter is used. Read all Chemical Frontiers as the chapters are covered.

Read the Overhead Transparency Notes and textbook assignments at least twice, once before we cover it in lecture and once after as you do the homework.

Do the homework even if you can't do the homework. At the very least, write down what the problem asks and what the problem gives you to work with. Look up and write an explanation for each word whose meaning you do not understand. Write down any formulas or equations associated with the topics in the problem. When doing homework and solving problems, you must always show your work and explain how you got your answer. This helps you to see what you are doing and understand how a problem is solved, and you can use your homework to review for your tests.

When doing calculation type problems be certain that you
Write out all Formulas
Rewrite them with data (numbers and units)
Write the answer (with units)
How did you check your answer?

Week 1
  OHT Notes Textbook
  Read: Prob: Read: Problems:
I. Introduction and History Unit 1 1 Ch 1 all 3,4,5,9,13,17,20,28
A. Chemistry   2    
B. Matter   3    
C. Ancient Societies   4,5    
1. Egyptians        
2. Greeks        
3. Arabs        
D. Alchemists   6    
E. Galileo        
F. Boyle   8    
G. Scientific Method   10,11 Ch3.1 1
1. Process        
2. Hypothesis     Ch2 Intro  
3. Theory        
4. Law        
H. Lavoisier   9 p.257-258  
1. Mass vs. Weight     Ch2.9  
I. Chemistry Subdivisions   7    
II. Measurements Unit 2      
A. Qualitative & Quantitative   1    
B. Parts of a Measurement   2    
C. Accuracy   3 Ch2.4  
D. Precision        
E. Significant Figures (bathroom scale)        
F. Significant Figures Rules       1a-f,3adfgij
G. Fundamental & Derived Quantities   4    
H. Significant Figures in calculations     Ch2.6 21,22,28,29
I. Solving Word Problems   5    
J. Rounding     Ch2.6 5,7,11,13
K. Scientific Notation     Ch2.5 15d-g,17,

Week 2

III. Metric System Unit 3   Ch2.7, 2.8  
A. Distance     Ch2.8  
B. Prefixes   1 Ch2.8  
C. Mass     Ch2.9  
D. Weight     Ch2.9 117,118
E. Volume   2 Ch2.6  
F. Liquid Volume     Ch2.6  
G. Unit Factors     Ch2.8 39,41,47,51,
H. Temperature   3,4 Ch2.11 113ab,115ab
I. Heat     Ch12.2,12.3 3
J. Density/Specific Gravity   5,6,7 Ch2.10 79,81,86,90,91,101

Week 3

IV. Properties and Changes of Matter Unit 4 Percents   Ch3.6
A. Physical Properties   1    
1. State     Ch3.5  
a. Solid        
i. amorphous        
ii. crystalline        
b. liquid        
c. gas     Ch13.1  
d. plasma        
2. Type of Matter - concept     Ch4.1  
a. Pure substance     Ch3.7 6,37,38
b. Mixtures        
i. Heterogeneous     Ch3.8 5,30,42,
ii. Homogeneous        
3. Others        
B. Physical Changes        
C. Chemical Properties   2,3    
D. Chemical Changes   4 Ch3.6 7,8,47
E. Mixtures vs. Compounds and Changes       50
F. Law of Conservation of Mass     Ch3.3 49
G. Energy     Ch3.4  
1. Potential energy        
2. Kinetic energy        
3. Changes and Energy   5 Ch12.1 1ac,
a. Endothermic, endoergic, endergonic        
b. Exothermic, exoergic, exergonic        
H. Law of Conservation of Energy   7 Ch3.3 3,4
1. Energy and Matter E=MC2        
2. Einstein   6    
V. Chemical Symbology: Elements, Compounds, Formulas, and Equations Unit 5      
A. Elements     Ch3.9,3.10 9
1. Earths Crust        
2. People        
B. Symbols   1 Ch3.14 11
C. Types of Elements     Ch3.9 34
1. Metals        
2. Nonmetals        
a. Diatomic elements   2 p.150 Ch7 17
b. monatomic elements   3    
3. Semi-metals or Metalloids       Ch3 32

Week 4

D. Compounds     Ch3.11 40
1. Molecular - covalent   10 Ch3.12,3.13  
2. Ionic/Salts - Ions        
a. Cations        
b. Anions        
E. Binary Nomenclature   4 to 9 Ch8.1,8.6 27a-f
F. Formula   11 Ch3.14 17
a. Subscript        
b. Parentheses        
G. Chemical Equations and Balancing   12,13 Ch10.1,10.2, 10.3 31,37,39
1. Reactants & Products        
2. Coefficients        
3. Balance       Balance only: Ch10 23,24

Week 5

VI. The Periodic Table and Atomic Structure Unit 6      
A. The Periodic Table     Ch6.1 6c
1. Periodic Law - arranged with respect to chemical properties        
2. Predicting formulas from a model   1,2    
3. Atomic Number     Ch4.6  
4. Features     Ch6.2 7ab,8
a. Columns        
b. Rows        
c. A & B subgroups     Ch6.2 12
i. Representative & Transition Elements        
ii. Halogens        
iii. Noble gasses        
iv. Alkali metals        
v. Alkaline metals        
B. Atomic structure     Ch4.1  
1. Daltons Atomic Theory     Ch4.2 4
2. Subatomic particles        
a. electron     Ch4.3  
b. proton     Ch4.4 16 p+ & e- only
c. # electrons = # protons     Ch4.6 57
d. neutron   3,4 Ch4.5 10,11,12
3. Rutherford Experiment     Ch4.4 5
a. Nucleus and nuclear structure of the atom        
4. Bohr atom     Ch5.1,5.2,5.3 8
5. Quantum Mechanics model     Ch5.4 22
6. Electronic Structure     Ch5.5 13
a. Principal Quantum level        
i. electrons in each different shell        
ii. valence shell        
b. Orbitals     Ch5.6  
i. spdf     Ch5.7 26,31,33,34
ii. amount of electrons per orbital        
iii. orbital shapes        
7. Electron Configuration     Ch5.8 37a,48ab
a. Filling Order        
b. Shells Overlap   5   37b,43,48c
c. Valence electron Configuration   6,7,8,9 Ch5.9 Ch7.1 53
8. Lewis Dot Structure of Atoms     Ch7.1 1
9. Atomic number     Ch4.6  
10. Mass number     Ch4.7 28,15abd
11. Isotopes     Ch4.7 17
12. Isotopic Notation   10    
End of Material for Exam I
13. Periodic Table Trends   16 Ch6.3 23
a. electron configuration     Ch6.4  
b. valence electrons     Ch6.5 45
c. atomic size   11 Ch6.6 17,18
d. Ionization Energy   15 Ch6.7 15
e. Electron Affinity   13 Ch6.8  
f. Electronegativity   12,14 Ch7.6  

Week 6 - First Exam will be given

VII. Bonding and the Formation of Compounds Unit 7   Ch7  
A. What are bonds        
B. Why bonds form        
1. stability and bonding   1,13    
2. stability of ns2np5        
3. lose electrons for octet     Ch7.1 2,5
4. gain electrons for octet   3,4,5,17   3
C. Ionic bonds   2 Ch7.4 28,29
1. Lewis Dot Structure of Ions        
2. Charge of Ions by the octet rule        
3. Lewis Dot Structure of Ionic compounds   6    
4. Formulas for Ionic Compounds or Salts   7   58 also draw Lewis dot structures

Week 7

D. Covalent bonds     Ch7.2  
1. Shared electrons        
2. Single, double, triple bonds       18
3. Lewis Dot Structure of covalent molecules   10,12   19c,20ad,22b
4. Polar Covalent Bonds   8,14,15 Ch7.6,7.6  
E. Polar/Non-polar Molecules     Ch7.8 45cd,47bcd,48ab
F. Coordinate Covalent Bonds   9,16 Ch7.3 20c,54a
G. Polyatomic Ions   11,17 Ch8.4 17abf,18af

Week 8

VIII. Nomenclature and Formulas of Compounds Unit 8      
A. Predicting Formulas of Ionic Compounds     Ch8.1,8.3 10bd
B. Oxidation Numbers and Rules   1,2 Ch8.7 29b,30ab,31c
C. Variable oxidation state elements        
D. Nomenclature        
1. Binary Compounds     Ch8.1  
a. metal and nonmetal     Ch8.3,8.7 9abce,27abdef
b. variable oxidation state metal     Ch8.3,8.7 15abcd,33cef,34cf
c. Nonmetal and nonmetal     Ch8.2,8.6 5bce,7,25,26

Week 9

2. Ternary compounds   3,4 Ch8.5,8.8 21dea,22cd
3. Acids, Bases and Neutralization Reactions     Ch8.9 39abc,40bd,41bde
a. Binary acid        
b. Ternary acids   5    
c. Base   6   36cd
b. Neutralization Reactions   7,8 p242,243  
d. Binary & Ternary Salts   9,10,11    
E. Determining Formulas from Names   12    

Week 10

IX. Calculations Involving Formulas, Elements, and Compounds Unit 9   Ch3.15
Ch9 all
A. moles     Ch9.1 2
B. Avogadros number and calculations mol-atom   1    
C. atomic weight and calculations g-mol       3,7ab,9,13ac
D. grams to moles to atoms or molecules   2,3   15
E. Formula weight and calculations     Ch3.16 Ch9.3 Ch3 5bcde
Ch9 29,33,37, 39,41,43
F. percent composition   4,5 Ch9.5  
G. empirical formula and molecular formula   6,7 Ch9.2,9.3  
End of Material for Exam II

Week 11 - Second exam will be given.

X. Equations for Chemical reactions Unit 10   Ch10  
A. completing and balancing   1 Ch10.1,10.2, 10.3 1a,2e,3a,32,39,41
B. other symbols   2    
C. Types of Chemical Equation       5
D. Synthesis     Ch10.4 11abc,13de
1. two elements - burning or combustion        
2. nonmetal oxide & water   3    
3. metal oxide and water        
E. Decomposition     Ch10.4 11fh,13ab,14a
1. binary compound        
2. ternary acid 4
3. base   5    
F. Single displacement     Ch10.4 13f,14g
1. activity series     Ch10.5 20ac
2. oxidation and reduction     Ch10.6 22ab,23ac
G. Double displacement reactions     Ch10.4 11p,19eg,20e
1. neutralization reactions        
2. precipitation reactions        
H. Energy and chemical reactions   9 Ch12.1,12.2, 12.9  
1. combustion   6,7    
2. exothermic        
3. endothermic        
4. photosynthesis   8    

Week 12

XI. Calculations from chemical equations Unit 11      
A. what coefficients mean   1,2 Ch11.1  
B. mole - mole calculations   3,4,5,6 Ch11.2  
C. mass - mole - mole - mass calculations   7   3,17,19,

Week 13

XII. Water and Changes of State Unit 12   Ch13.1,14.1 3,4,5
A. Abundance of H2O     Ch14.7  
B. Boiling point   1 Ch14.2,14.3 9,14,15,18,25acd,
1. Heat of vaporization       87
C. Melting point/freezing point   2 Ch14.4  
1. Heat of fusion        
D. Changes of state       31
1. energy   3,4,5   83
2. effects (heating and cooling)        
E. Sublimation        
F. Heating and cooling curve   6 Ch14.5  
G. Water compared to other Hydrogen compounds     Ch14.7  
1. Why H2O is so different than H2S, H2Se   7    
2. H-bonding       63,66,95
H. Other related concepts   12    
Think about deleting this        
1. Formation of water        
2. Decomposition of water        
3. Reaction with oxides   8   70ab
4. Hydrates   9,10 Ch14.7 74,77a,78b,82a
5. H2O2        
6. O3   11    
i. pollution        
ii. ozone layer        
iii. destruction of the ozone layer        

Week 14

XIII. Properties of solutions Unit 13   Ch15  
A. solutions     Ch15.1 1,3,5
1. Solute        
2. solvent        
3. types     Ch15.2 11,14
4. terms        
B. factors that affect solubility   1,2,3    
C. factors that affect rate of dissolving   4,5,6    
D. why solutions are important        
E. concentration units        
1. weight percent   7 Ch15.3 15
2. PPM   8,9    
3. Molarity     Ch15.4 45,
4. Dilution calculations     Ch15.6 81,83,85
F. Colligative Properties     Ch15.9 101,102,121
a. Freezing point and boiling point        
b. Diffusion and Osmosis   10 Ch15.11 111,112,114
End of Material for Exam III

Week 15 - Third exam will be given

Complete Unit XIII

Week 16 - Final Exam

Attendance is required.
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