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HOMEWORK SCHEDULE

See Table Below
Back to the Chemistry Home Page 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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