CCL 1110 1st EditionExam # 1 Study Guide Lectures: 1 - 7Lecture 1 (January 23)Chapter 1- Matter & Measurement•C = K- 273.15•F = 1.8C +32Lecture 2 (January 28) •Molecular Mass- sum of the atomic masses of each atom in a molecule•Formula Mass- sum of the atomic masses of each atom in a formula unitAtomic mass = (% abundance)(mass) + (% abundance)(mass)… etc•Rows = periods; Columns = groups•Molecular compound- composed of molecules that contain more than one type of atom (usually contain nonmetals and/or metalloids)•Ions- atom gains or loses an electron -Cation: + ion when electrons are lost -Anion: - ion when electrons are gains•Ionic compound- a compound that contains a metal and a nonmetal; contains a positive and negative ion•Hydrates- compounds whose crystals contain discrete H2O molecules•-ate has one more oxygen than -ite•Acids- yield H+ ions in water (Arrhenius Theory) -Binary Acid: contain 2 elements (aq in water)-“ate” to “ic”; “ite” to “ous”Lecture 3 (January 30)•Stoichiometry- quantitative study of the reactants/products of a chemical reaction•Chemical reaction- symbolic representation of a balanced chemical reactionHow to balance:-write all components with states of matter-start with most complex formula~Balance elements that occur in only one other species~Continue until all balanced-Convert coefficients to smallest integer ratioCH3NH2 + O2 —> CO2 H2O + N24CH3NH2 + 9O2 —> 4CO2 + 10H2O + 2N2•Combination reaction- occur when 2 or more substances (the reactants) react to form one product•Decomposition Reaction- one substance breaking down into 2 or more substances•Compustion Reaction- generally rapid reactions that produce a flame and often involve hydrocarbons reacting with oxygen in the airMass % of Element A = Mass of atoms of A/ Mass of all the atoms x 100•Mole- amount of substance that contains many entities-Avagadro’s Number: 6.022x10^23 molecules per mole•Molar mass (in amu) and molar mass (in grams) are the sameGrams —> Moles —> Formula UnitsLecture 4 (February 2)Finding empirical formula from molecular:-Divide each # by smallest subscript value-Multiply each result by same integer if necessary•Empirical formula- smallest integer ratioEmpirical formula C4H5N2O & molar mass 194. What is Molecular formula?4(12.01g C) + 5(1.008g H) + 2(14.01g N) + 16 g O = 97 g empirical molar mass194 g (molecular molar mass)/ 97 g (empirical molar mass) = about 2= C8H5N4O2Lecture 5 (February 4)•Theoretical yield- maximum possible yield of a product, predicted by the balanced equation & reactant limitationsPercent yield = actual yield/ theoretical yield x 100Lecture 6 (February 6)•Electrolyte- ions in solution•Ionic compounds- made of a metal and a nonmetal•Molecular (covalent) compound- made of 2 nonmetals•Dissociation- process of separating the individual ions by salvationAcids:-100% dissociation = strong acid- 1-2% dissociation = weak acidWhen 2 aq solutions mix, either a reaction occurs A + B —> C + D, or a reaction doesn’t happen X +Y —> X + Y•Precipitation reaction- a reaction that yields an insoluble solid product•Double displacement- Ax + By —> Ay + Bx•Spectator ions- ions that do not participate in the reaction-in a net ionic equation, omit spectator ionsLecture 7 (February 9)•Arrhenius Theory:-Acids yield H+ ions in water-Bases yield OH- ions in water•Strong acids and bases are strong electrolytes•Weak acids and bases are weak electrolytes•Neutralization reaction- reaction of an acid & baseAcid + Base —> Salt + Water- Salt: ionic compound not containing H+, OH-, or O*Net ionic equation left with water is a reaction b/w strong acids &basesStrontium Hydroxide w/ Nitric AcidSr(OH)2 (aq) + 2HNO3 (aq) —> Sr(NO3)2 (aq) + 2 H2O (l)Total: Sr^2- + 2OH^- +2H^+ +2NO3 —> Sr^2+ +2NO3^- + 2H2 +2ONet: OH^- (aq) + H^+ (aq) —> H2O (l)Aluminum Hydroxide with Hydrochloric AcidAl(OH)3 (s) + 3HCl (aq) —> AlCl3 (aq) + 3H2O (l)Net: Al(OH)3 (s) + 3 H^+ (aq) —> Al^3+ (aq) + 3 H2O (l)•Sometimes the molecular compound formed after neutralization is a gas with low solubilityex. 2HCL (aq) + Na2S (aq) —> H2S (g) + 2 NaCl (aq)•Sometimes the compound formed is originally unstable & breaks down further to yield a gasex. HCl (aq) + NaHCO3 (aq) —> H2CO3 (aq) + NaCl (aq)—> HCl (aq) + NaHCO3 (aq) —> CO2 (g) + H2O (l) + NaCl (aq)•Bronsted-Lowry Theory-Acid: proton donor-Base: proton acceptor•Solution- homogenous mixture of 2 or more substances •Concentration- amount of salute dissolved in a given quantity of solutionMolarity- # of moles of solute in one liter of solutionM = moles of solute/ liters of solutionDilution: (moles)(volume) =