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CHE 105 Exam 2 Study Guide

by: Christina Binkowski

CHE 105 Exam 2 Study Guide CHE 105

Marketplace > University of Kentucky > Chemistry > CHE 105 > CHE 105 Exam 2 Study Guide
Christina Binkowski

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About this Document

This study guide for Exam 2 includes Charts to Memorize, Mathematical Methods, and Equations.
Gen College Chemistry I
Dr. Soult
Study Guide
Chemistry, General Chemistry, genchem
50 ?




Popular in Gen College Chemistry I

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This 4 page Study Guide was uploaded by Christina Binkowski on Sunday October 9, 2016. The Study Guide belongs to CHE 105 at University of Kentucky taught by Dr. Soult in Spring 2016. Since its upload, it has received 77 views. For similar materials see Gen College Chemistry I in Chemistry at University of Kentucky.


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Date Created: 10/09/16
I. Ions/Rules to Memorize A. Polyatomic Ions (Table 3.5) Name Formula Name Formula − − Acetate C 2 O3 2 Hypochlorite ClO 2− − Carbonate CO 3 Chlorite ClO 2 − − Hydrogen HCO 3 Chlorate ClO 3 Carbonate − − Hydroxide OH Perchlorate ClO 4 − − Nitrate NO 2 Permanganate MnO 4 − 2− Nitrate NO 3 Sulfite SO 3 2− − Chromate CrO 4 Hydrogen Sulfite HSO 3 2− 2− Dichromate Cr 2 7 Sulfate SO 4 Phosphate 3− Hydrogen sulfate HSO − PO 4 4 Hydrogen HPO 2− Cyanide CN − 4 phosphate − 2− Dihydrogen H 2O 4 Peroxide O 2 phosphate Ammonium NH +4 B. Solubility Rules (Table 4.1) Generally Soluble Compounds Compounds Exceptions Li +, Na +, K +, NH + None (always soluble) 4 NO − , C H O − None (always soluble) 3 2 3 2 − − − + 2+ 2+ Cl , Br , I Ag , Hg 2 , Pb 2− + 2+ 2+ 2+ 2+ SO 4 Ag , Ca , Sr , Ba , Pb Generally Insoluble Compounds Compounds Exceptions − + + + + 2+ OH Li , Na , K , NH 4 , [ Ca , Sr2 +, Ba 2+(slightly soluble)] − + + + + 2+ 2+ S 2 Li , Na , K , NH 4 , [Ca , Sr , 2+ Ba (slightly soluble)] CO 2−, PO 3− Li +, Na +, K +, NH + 3 4 4 ​Another Way to Memorize Soluble Exceptions Chlorates Acetates Sulfates Ca, Sr, Ba, Hg, Ag, Pb Halogens Hg, Ag, Pb Nitrates, NH +4 Group 1A C. Rules for Assigning Oxidation Numbers (ON) 1. In free elements, the ON of each atom is 0 2. For monoatomic ions, the ON is the same as the charge of the ion 3. The ON of oxygen is -2 a) Exception: peroxides (like H O 2 w2ich are -1 4. The ON of hydrogen is +1 a) Exception: when bonded to metals in binary compounds = -1 5. The ON of fluorine and other halide anions is -1 6. In neutral molecules, the sum of ONs has to be 0 a) In polyatomic ions, ON= net charge of ion 7. ON’s do not have to be integers (in this class they will be) II. Mathematical Methods A. Composition of Compounds (3.9) B. Balancing Chemical Equations (3.10) 1. Write the correct formula(s) for reactants on left and products on right 2. Change coefficients to make # of atoms of each element the same on each side of the equation 3. Start by balancing elements that appear in only one reactant or one product 4. Balance elements that appear in 2 or more reactants/products a) Use fractions to balance odd # elements b) Multiply to get rid of fractions C. Tools for Unit Conversion (4.2) Conversions between: Use: Grams and moles Molar mass Moles and actual # (molecules, Avogadro’s # atoms) Grams and milliliters Density Grams and kilograms (for example) Prefix meaning Molecule and atoms in molecule Subscripts Moles of A and moles of B Coefficients of balanced equation D. Amounts of Reactants and Products (4.2) E. Solution Stoichiometry (4.4) F. Precipitation Equations (4.5) 1. Write balanced molecular equations 2. Write the ionic equation showing strong electrolytes dissociated into cations and anions 3. Cancel spectator ions on both sides 4. Check that charges and number of atoms are balanced III. Equations A. Percent Composition in Compounds (3.9) 1. % Composition = n×molar mass of eleme× 100% molar mass of compound 2. n = subscript of element in formula B. Percent Yield (4.3) actual yield 1. % Y ield = theoretical yield00% C. Solution Concentration (4.4) moles of solute 1. M = volume of solvent (L) 2. M= Molarity D. Dilutions (4.4) 1. M V1 1 = M V2 2


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