<p>Chemistry 111: Exam 2 Topics</p><p>+ + Chapter 12 o H3O , NH4 2- -  Molecular Geometry o HPO4 , HCO3 , … o How many VSEPR pairs (electron  Some common names: NH3, H2O domains are there?)  Oxyacids – HNO3 = nitric acid (-ate- o What is the VSEPR shape? ic, …) o What is the angle? o What is the molecular shape (when Chapter 7 there are lone pairs)  Calculate molecular weight o What is the angle when there are  Understand moles. lone pairs?  Determine % composition  Bond Polarity (applied to next item)  Determine empirical formula from %  Molecular Polarity composition o Sum up the bond dipoles to  (for above 2, use my table method!) decide if a molecule is polar. o Good examples: CH4, CH2F2, Chapter 8 CO2, H2S, CH3F  Balance chemical equations  Write chemical equations from Chapter 6 descriptions.  Names of Cations for elements (metals)  Get mole ratios from balanced equations  Names of Anions for element  Know reactions from in class (nonmetals)  Names of covalent compounds from Chapter 9 formula  Mass calculations  Formulas of covalent compounds from (massmolesmolesmass) name.  You will have the map on the exam  Names of Ionic compounds  cover sheet! Formula of ionic compounds.  Find % yield  Transition metal ions:  Use % yield as a conversion factor o formula from Stock system name for  Find limiting reagents any element o ion from stock system name for any Chapter 4 element  Understand kinetic theory – explain o know charges of selected elements pressure/temp/volume based on (see class notes) molecular collisions o Common names (ferric ion = Fe3+,  Understand how to read a barometer ferrous = Fe2+)  Understand how to read a manometer o Understand Hg2+ = mercury(II) ion,  Be able to convert pressure units 2+ Hg2 = mercury(I) ion  Remember to use Kelvin!  Polyatomic Ions  Understand what’s held constant in o Oxyanions Boyle’s Law, Charles’ Law - - o CN , CH3COO , …  Use combined gas law (P1V1/T1=P2V2/T2 is given).</p>