finalexamreview - CHEM 1100 Final Exam Review Hey everyone...

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CHEM 1100 Final Exam Review Hey everyone, here is a study guide I made up based on JUST the class notes of the semester. It is broken up by exam and by chapter. I don’t know how much it will help you, but I just wanted to give you a condensed and more focused version of the topics covered. Definitely make sure you go over your tests and quizzes as well as your own notes. Also go to www.wmich.edu/asc click on schedules and scroll down to CHEM 1100 to get practice problems not in the book for each chapter if you have not already done so. There are answers for all these questions as well as outlines you can fill out if you have time. It’s been such a pleasure getting to know you guys this semester and I hope I helped some of you to a small degree. Thank you for your kindness and good luck on the exam as well as everything to come in your bright futures! -Jody Exam One Material I. Chapter One (1.1—1.3) A. Changes 1. Chemical Changes-substance(s) undergoes reaction to become a new substance(s) 2. Physical Changes-change of state (solid, liquid, gas) B. Properties 1. Intensive—independent of amount of material present (color, temp, freezing point, density, malleability, etc.) 2. Extensive—dependent of amount of material present (mass, volume, surface area) C. Periodic Table 1. Atomic Number 2. Atomic Mass D. Mixtures 1. Heterogeneous-variable composition, can separate out different parts of the mixture (bucket of wood, sand, and rocks) 2. Homogeneous-fixed composition, properties uniform throughout (air, beer, salt water, soda pot, bronze, brass, etc.) II. Chapter Two—atoms, elements, and ions A. Law of Definite Proportions—molecules of a given kind are always made of a certain proportion in a compound. Each compound is made up of a certain number of each kind of atom and these atoms are in certain specific proportions based on how many of each there are. B. Law of Multiple Proportions—when you have two different compounds with the same elements and you hold one constant, the other(s) must be in whole number rations to the one held constant C. Periodic Table 1. Rows = periods (period number = shell number) 2. Columns = Groups/families D. Nomenclature of Compounds 1. Binary Compounds: metal first, nonmetal second; IDE ending; eg NaCl is sodium chloride 2. Molecular Compounds 3. Cations 4. Anions 5. KNOW THE PINK SHEET!!! 6. when making an acid, ate ending changes to –ic acid and ite ending changes to –ous acid E. Formulas 1. Molecular 2. Empirical—simplest whole-number ratio of the elements in a compound; sometimes is the molecular formula 3. Ionic—know what ions a compound breaks up into III. Chapter Six A. Wave nature of light 1. Wavelength 2. Frequency—number of complete waves per second; units are inverse seconds 3. Speed of light = Frequency x Wavelength. Units of speed are meters per second 4. Energy = Planks constant x Frequency = planks constant x (speed of light / wavelength). Units for energy are Juoles
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5. Jumping shells: (1/wavelength) = Ridburg’s constant x [ (1/square of final shell number) – (1/square of
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This note was uploaded on 04/18/2008 for the course CHEM 1100 taught by Professor Dr.guzinski during the Spring '08 term at Western Michigan.

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finalexamreview - CHEM 1100 Final Exam Review Hey everyone...

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