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Chem 211 Midterm 1 Study Guide

by: Teresa Notetaker

Chem 211 Midterm 1 Study Guide Chem 211 003

Marketplace > George Mason University > Chemistry > Chem 211 003 > Chem 211 Midterm 1 Study Guide
Teresa Notetaker

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This study guide covers essential information that you will need to know for the upcoming midterm exam. It is separated into questions from chapters 1, 2, and 3 from the textbook; chapter 4 will no...
General Chemistry
Dr. Pritha G. Roy
Study Guide
Chemistry, General Chemistry
50 ?




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This 6 page Study Guide was uploaded by Teresa Notetaker on Tuesday September 27, 2016. The Study Guide belongs to Chem 211 003 at George Mason University taught by Dr. Pritha G. Roy in Fall 2016. Since its upload, it has received 16 views. For similar materials see General Chemistry in Chemistry at George Mason University.


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Date Created: 09/27/16
CHEMISTRY MIDTERM #1 STUDY GUIDE CHAPTER 1: MEASUREMENTS, UNITS, PRECISION, PROBLEM SOLVING 1. Which is not a state of matter? a. Gas b. Liquid c. Plasma d. Dark Matter 2. What is the equation for Density? 3. What is the correct number of Signifigant Figures for the numbers below? a. 1.030 mL b. 5300 L c. 5300. L d. 0.00000000350 m 4. Define Precision 5. Define Accuracy 6. What is the difference between Systematic Error and Random Error? 7. Lead is heated to a temperature of 1056 °C. What is it’s temperature in Kelvin and Farenheit? ____________ °F _____________ °K 8. Number the order of the Systematic Approach to solving Chemistry Problems Plan Prepare Visual Summary of Steps Check State Problem Clarify Known and Unknown Solution Comment Follow up Problem Suggest steps from Known to Unknown 9. What is the equation used to get the degrees Celsius from degrees Fahrenheit? CHAPTER 2: COMPONENTS OF MATTER (ATOMS, MOLECULES, AND IONS) 1. What is an Element? What is a Molecule? 2. What is a Compound? What is a Mixture? 3. What are the different parts that make up an atom, and what are their charges? 4. Define the Law of Definite/Constant Composition 5. Define the Law of Multiple Properties 6. What is an Isotope? What is Natural Abundance? What is Fractional Abundance? 7. What are Ionic Bonds? What are Covalent Bonds? 8. What is an Ion? What is a Cation? What is an Anion? What is an Ionic Compound? 9. What are Hydrocarbons? 10.Balance the chemical equation: ____C 8 18+ ____ O 2  ____CO 2 ____ H2O 2 CHAPTER 3: STOICHIOMETRY & CHEMICAL EQUATIONS 1. What is a mol? What is Avogadro’s Number? 2. What is Molar Mass? 3. What is the Molar Mass of O ? 2 4. What is the Molar Mass of SO ? 2 5. How many molecules of water (H O) ar2 there in 250 kg of water? How many atoms of Hydrogen? 6. How many Sulfur atoms are there in 25 g of Al S ? 2 3 7. What is the mass percentage of each of the elements in CH COOH? 3 8. What is the mass percent of each element in NH4NO ? 3 9. What is the Empirical Formula of C2H ? 4 10.What is Molecular Formula? 11.What is the Empirical and Molecular formulas of a molecule if it’s molecular weight is 146 amu and its mass percentages are 48.1% C, 2.7% H. and 48.2% Cl? 3 12.Balance the equation: ___C H 8 18+ ___O 2___CO + _2_ H O 2 13.What is a limiting reactant? If you need to find the Practice Midterm on Blackboard, here is how you find it:  Open up the class on Blackboard  Click on Course Content  Click on the folder labelled “Class Slides”  Open the “Midterm Reviews” folder  Click on the second link, labelled “Practice Midterms 1” 4 CHEMISTRY MIDTERM 1 ANSWERS CHAPTER 1 1. D 2. D ensity = mass / volume 3. a) 4 b) 2 c) 4 d) 3 4. H ow close measurements in a series are to each other 5. H ow close each measurement is to the actual value 6. S ystematic error is when all results are consistently above or below the actual value. Random Error produces values that are both higher and lower than the actual value at random . 7. 1 932.8 °F 1329.15 °K 8. S tate Problem Plan Clarify Known and Unknown Suggest steps from Known to Unknown Prepare visual Summary of Steps Solution Check Comment Follow up Problem 9. T emperature °C = (Temperature °F – 32) (5)/ 9 CHAPTER 2 1. Element: Simplest type of substance with unique physical and chemical properties. Consists ONLY of one type of atom. Molecule: Consists of two or more atoms that are chemically bonded together. It acts as an independent unit. 2. Compound: A substance composed of two or more elements that are chemically combined. Mixture: Two or more elements/compounds that are physically intermingled, not chemically combined. 3. Electron: A negatively charged particle that is found surrounding the nucleus, in what is termed an “electron cloud.” Proton: Positively charged particle, found in the nucleus. Neutron: A particle that has no charge. It is found in the nucleus. 4. Law of Definite/ Constant Composition: No matter what the source of a compound, its elements occur in the same proportion by mass; atoms combine in whole number ratios, therefore proportion by mass is always the same. 5. Law of Multiple Properties: Mass proportions must be proportional 6. Isotope: Atoms whose nuclei have the same atomic number, but a different number of neutrons and thus a different mass number. Natural Abundance: The naturally occurring percentage of the isotopes of a particular abundance. Adding all the numbers should lead to getting 1. Fractional Abundance: The fraction of the total number of atoms composed of a particular isotope. Adding all the fractions for a certain element should get to 1. 7. Ionic Bonds: A bond where electrons are transferred to create the bond. Covalent Bonds: A bond where electrons are shared to create the bond. 8. Ion: Charged particles composed of an atom with excess/deficient numbers of electrons. Cation: Positively charged ions (Missing one or more electrons) Anion: Negatively charged ions (Has one or more extra electrons) Ionic Compound: A neutral compound formed by combining Cation(s) with Anion(s); formula in terms of smallest whole number of ions. 9. Hydrocarbons: Substances containing only Carbon and Hydrogen 10.2 C H + 25 O  16 CO + 18 H2O 8 18 2 2 CHAPTER 3 1. A mol: The amount of a substance that contains the same number of entities as the number of atoms in 12 grams of Carbon - 12 23 Avogadro’s number: 6.022 x 10 entities 2. Molar Mass: Mass per mol of its entities 3. 32.00 g / mol 4. 64.00 g / mol 5. 8.36 x 1027molecules 1.67 x 1028atoms 23 6. 3.006 x 10 atoms 7. C—40% H—6.72% O—52.8% 8. Mass % N = 35% Mass % H = 5% Mass % O = 60% 9. CH 2 10. Molecular Formula is the actual number of atoms of each element in a molecule of a particular compound. 11. Empirical Formula: C3H2Cl Molecular Formula: C6H4Cl2 12. 2 C8H18+ 25 O 2 16 CO +218 H O 2 13. Limiting reactant: The reactant that is completely used up in a reaction. 2


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