CHEM 1111 1st EditionExam # 2 Study Guide Chapters: 4-5 Topics covered:-Precipitation reactions, ionic and net ionic equations, acid-base, redox, molarity, dilutions(C1V1=C2V2)-PV=nRT and applications, gas stoichiometry, partial pressures, kinetic molecular theorySolubility rules: Precipitation reactions involve AQUEOUS reactants to form one or more INSOLUBLE precipitate (usually one). Use the solubility rules shown above to determine if a product is soluble.The ionic equation of a precipitation reaction shows the AQUEOUS compounds as individual ions, cancel out the ions that are on each side to get the net ionic equation. This net ionic equation only includes ionsthat are actively involved in the reaction to form the solid precipitate.-Be familiar with the general properties of acids and basesBrønsted Acid: Proton donorThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.-acids with lower numbers of protons are typically strongerBrønsted Base: Proton acceptorAcid + Base reactions produce WATERRedox reactions: -Combination: x + y ? xy-Decomposition: xy ? x + y-Combustion: produces CO2 and H2O with oxygen as a reactant-Displacement: one atom replaced by anotherRules for assigning oxidation numbers: -Oxygen is -2, except in peroxides, where it's -1 (we will usually treat it as -2)-Hydrogen is +1 in compounds with nonmetals, -1 with only hydrogen + a metal-First column of periodic table (alkali metals) are +1 charge, 2nd column is +2-F is -1-See table below for more oxidation statesoxidation: the LOSS of elections (net positive charge)reduction: the GAIN of elections ( net negative charge, hence REDUCED)Molarity is given by M, which is moles of a compound/liter of solutionUse C1V1 = C2V2 to solve dilution problems, where C1 and C2 are the concentration (typically moles/liter) and V1/V2 are the volumes of solution. Dilution problems typically involve adding water to a certain amount of X molar solution. When adding water, the number of moles of the compound will remain the same, hence moles/liter * liter = moles/liter * liter ? moles = molesGas Laws:-Boyle's Law: V ??1/P (constant n and T)-Charle's Law: V ? T (constant n and P)-Avagadro's Law: V ? n (constant P and T)Combine all these to get: PV = nRT, where P=pressure(typically atm), V=volume(typically liters), n=# of moles, T=temperature in KELVIN, and R is a constant that will be given.KNOW:-1 mole of any ideal gas occupies 22.4L of space at STP-1 atm = 760mmHg = 760 torrYou can equate PV/nT = P2V2/n2T2 for changing temperature, pressure, volume, or number of molesPartial pressures: -Ppartial = Xmole_fraction*Ptotal-Mole fraction is simply the number of moles of one compound over the total number ofmoles.-ie. For example, say a reaction is determined by reactants ? 2H2 + O2 , the mole fractionson the side of the products will always be 2/3 for H2 and 1/3 for O2, as there are 2 moles of hydrogen gas per 3 moles of total products, and 1 mole of oxygen gas per 3 moles of total products. If the partial pressure is given, you can use these mole fractions to calculate partial pressures.Gas stoichiometry is the same as the stoichiometry you've been doing, but simply apply PV=nRTfor conversions. ALWAYS CONVERT TO MOLES, this will make your life easier.Kinetic molecular theory: Understand the general concepts behind this:-The sizes of the particles in a gas are negligible-Gas molecules are in constant motion, their collisions are eleastic so energy is conserved, and an ideal gas won't randomly decrease its average kinetic energy(temperature)-Gas molecules don't attract or repel eachother-The average kinetic energy is proportional to the temperature in