CHM 203 Unit 2 Study Guide PDF

CHM 203 Unit 2 Review Grams, Moles and Particles (OpenStax Atoms First Ch 6.1 and 7.1, McMurry General Chemistry Ch 6.2-6.3)  Avogadro’s Number and the Mole o Convert moles to number of particles, atoms, ions, molecules o Covert particles, atoms, ions, molecules to moles  M...

CHM 203 Unit 2 Review Grams, Moles and Particles (OpenStax Atoms First Ch 6.1 and 7.1, McMurry General Chemistry Ch 6.2-6.3)  Avogadro’s Number and the Mole o Convert moles to number of particles, atoms, ions, molecules o Covert particles, atoms, ions, molecules to moles  Molar Mass o Calculating molar mass o Convert grams to moles o Convert moles to grams Chemical Reactions (OpenStax Atoms First Ch 6.2 and 7.2-7.3, McMurry General Chemistry Ch 6.3 and 6.6)  Balancing Chemical Reactions o Determine if a reaction is balanced or unbalanced o Assigning coefficients to balance chemical equations  Reaction Types o Assigning the 5 Basic Types  Combination (A + B  AB) Two or more elements or compounds bond to form one product  Decomposition (AB  A + B) Single reactant splits into two or more products  Single Replacement (A + BC  AC + B) An uncombined element takes the place of an element in a compound  Double Replacement (AB + CD  AD + CB) The positive ions in the reacting compounds switch places ∆ 𝑌𝑌  Combustion 𝐶𝐶𝑋𝑋 𝐻𝐻𝑌𝑌 + 𝑍𝑍𝑂𝑂2 (𝑔𝑔) → 𝑋𝑋𝐶𝐶𝐶𝐶2 (𝑔𝑔) + 2 𝐻𝐻2 𝑂𝑂(𝑔𝑔)  Carbon-containing compound that is the fuel burns in oxygen from air to produce carbon dioxide, water, and energy in the form of heat or a flame  Empirical Formulas o Calculations using  From percent composition  From combustion  Convert from empirical formula to molecular formula  Mass Percent composition o From mass o From molar mass Chemical Reaction Stoichiometry (OpenStax Atoms First Ch 6.2, 7.2-7.3, McMurry General Chemistry Ch 6.3, 6.6)  Stoichiometry Calculations o Convert between moles of one reactant to another o Convert between moles of one reactant to a product o Convert between mass of one reactant to another o Convert between mass of one reactant to a product  Limiting Reagent – the reactant that is completely used up; present in limiting amount o Be able to identify the limiting reagent o Convert mass of each reactant to moles or mass of a single product  Lesser value is the limiting reagent  Theoretical Yield – maximum amount of product possibly formed, in grams, if the starting materials were pure and the reaction went to completion  Percent Yield-the percentage of the theoretical yield that was formed; the amount of product actually formed in a reaction divided by the amount theoretically possible and multiplied by 100%. Actual yield Percent Yield = x 100% Theoretical yield Solutions (OpenStax Atoms First Ch 6.3-6.4, McMurry General Chemistry Ch 6.8-6.10 and 7.4-7.5)  Other Reactions o Precipitation Reactions  Electrolytes – Strong, Weak, Nonelectrolytes  Be Able to Identify which substances (generally speaking, molecular compouds, ionic salts, strong acids or bases, weak acids or bases) belong to the different types of electrolytes  Solubility – Unsaturated, Saturated, Supersaturated Salts – Soluble, Slightly soluble, Insoluble Solubility Tables & Physical States o If given a reaction identify the chemical states o Go from written equation (in words) to chemical reaction with states  Acid-Base Neutralization Reaction o H + nonmetal nomenclature o Strong acid: HCl, HBr, HI, HClO4, HNO3, H2SO4 o Strong base: LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 o Be able to write the products of a neutralization reaction between any strong acid and any strong base  Concentrations o Molarity  Calculating molarity  Using molarity as a conversion factor o Mass/Volume Percent  Calculating mass/volume percent o Dilution [M1V1 = M2V2] o Titration  Determining how much of an acid/base needed to neutralize an acid/base Things that are provided for the exam:  Periodic Table (a blank version of the one you were given in class)  Solubility Rules  Avogadro’s Number  Common Transition Metal Charges  Common Conversion (g to mL, mg to g, etc)  Formulas for Percent Yield, Molarity, Percent Concentration, Dilutions New Things You Need to Memorize: These will not be provided on the exam. Strong Acids Strong Bases Hydrochloric Sodium HCl NaOH Acid Hydroxide Hydrobromic Lithium HBr LiOH Acid Hydroxide Potassium HI Hydroiodic Acid KOH Hydroxide Calcium HNO3 Nitric Acid Ca(OH)2 Hydroxide Barium H2SO4 Sulfuric Acid Ba(OH)2 Hydroxide Strontium HClO4 Perchloric Acid Sr(OH)2 Hydroxide Other Information You Should have Already Memorized From Unit 1: Polyatomic Ions Formula Names Formula Name NO3- nitrate SO42- sulfate PO43- phosphate CO32- carbonate ClO3- chlorate CH3COO- acetate BrO3- bromate CN- cyanide OH- hydroxide H3O+ hydronium NH4+ ammonium O22- peroxide