Chemistry 100 - Review Sheet for Exam #3

Chapter 6: Energy States of matter Solid Liquid Gas Energy Potential energy Kinetic energy Heat Temperature Celsius (oC) Fahrenheit (oF) oF = 1.8oC + 32 Kelvin scale (K=oC+273) Absolute zero calorie (cal) Joule (J) 1 cal = 4.18 J Specific heat (S.H.) q = SH x m x DT Change of state Melting point (solid to liquid) Freezing point (liquid to solid) Heat of fusion (energy to form solid) Sublimation (solid to gas) Boiling point Vaporization (liquid to gas) Condensation (gas to liquid) Heat of vaporization Heating (cooling) curve Heat of reaction Exothermic (release of energy) Endothermic (gain of energy) Equilibrium Chemical changes

Chapter 6 (continued) Chemical reactions Combination Decomposition Replacement Double replacement Single replacement Combustion Reactants Products Reaction coefficients Balancing a Chemical Equation Oxidation-reduction reactions Oxidation - loss of electrons Reduction - gain of electrons Rate of reactions catalysts energy of activation Chemical equilibrium  Chapter 8: Solutions Hydrogen bond Surface tension Solute Solvent Solution Electrolyte Ionic solution Strong electrolyte Weak electrolyte Non-electrolyte Unsaturated solution Saturated solution Supersaturated solution Solubility rules Predicting reactions: Solid formed Gas formed Water formed Percent concentration Osmotic pressure Dialysis Molarity (M=mol/L) M x V = mol McVc=MdVd

Compound naming review Valence electrons Electron dot structures Ions (Octet rule) Cations (+) - Na+, Al3+, Fe3+ Anions (-) - O2-, Cl-, NO3- Ionic compounds Naming ionic compounds Type I Binary (Ionic) NaCl: sodium chloride MgCl2: magnesium chloride Type II Binary (Ionic) FeO: iron(II) oxide Cu2S: copper(I) sulfide Naming binary covalent compounds Type III (CO2: carbon dioxide) Ion names -ide — element as ion (S2-, O2-, Cl-) -ate — anion of acid (sulfate, nitrate, phosphate) -ous acid contains one less "O" than -ic acid -ite — anion of an -ous acid (sulfite, nitrite, etc.)