Chemistry Objectives Unit VI- Ch. 17 I. Compare and contrast endothermic and exothermic reactions and explain them in terms of energy required to break old bonds and energy released in forming new bonds. II. Define enthalpy and explain what is meant by an enthalpy change. III. Interpret a potential energy diagram for a reaction and be able to recognize the energy changes it shows. IV. Calculate the standard enthalpy change for a reaction or use the standard enthalpy change to calculate heat released or absorbed by a given amount of reactants.
Chemistry Objectives Unit VI – Ch. 17 V. Use the equation Q = m Δt C to solve calorimetry problems and determine standard enthalpy. VI. Calculate the Energy for changes of state given the heat of fusion or heat of vaporization of a given substance. VII. Differentiate between heat and temperature. Explain them in terms of potential and kinetic energy of molecules.
Chemistry I Objectives Unit VI Ch. 18 I. Define the rate of a chemical reaction. II. Identify the intermediate products of a reaction mechanism. III. Describe a rate law for a chemical reaction. IV. Explain chemical reactions in terms of collision theory. V. Use energy changes to explain endothermic and exothermic reactions. VI. Define activation energy and the activated complex and explain how they affect reaction rates. Know the five factors that affect reaction rate and explain each in terms of collision theory
Chemistry I Objectives Unit VI - Chapter 18 VII. Describe reversible reactions and explain how they work. IX. Define chemical equilibrium and explain how it is achieved in terms of rates of forward and reverse reactions and concentrations of products and reactants. X. Write the mass action expression used to calculate the equilibrium constant for a given reaction. XI. Use the equilibrium constant (Keq) to analyze the extent of the reaction. XII. Calculate the reaction quotient (Q) for a given reaction and use it to determine if the reaction is at equilibrium. If the reaction is not at equilibrium use the reaction quotient and equilibrium constant to determine the direction (forward or reverse) the reaction will proceed to reach equilibrium. XIII. Explain Le Chatelier’s principle and use it to predict the effect of changes in concentrations of reactants or products, pressure, or temperature on the position of the equilibrium. XIV. Relate the Haber process to Le Chatelier’s principle and be able to apply it to other reactions at equilibrium in order to maximize a given product.
Chemistry I Objectives Unit VI – Ch.19 I. Compare and contrast the Bronsted-Lowry and Arrhenius definitions of acids and bases. II. Use the proton donor / acceptor concept to identify conjugate acid-base pairs. III. Identify the common physical and chemical properties of acids and bases and know how indicators are used to identify them. IV. Write the expression for the acid / base dissociation constant and use data to calculate the dissociation constant. V. Explain how the dissociation constant can be used to compare the relative strengths of acids and bases. VI. Describe a salt hydrolysis reaction and identify the result as acidic basic or neutral. VII. Know the types of acids and bases be able to name them using correct nomenclature.
Chemistry I Objectives Unit VI - Chapter 19 VIII. Identify the ion concentrations in pure water Kw= 1X10-14 = [H3O+] [OH-] = (1x10-7) (1x10-7) IX. Describe the pH and pOH scales and be able to calculate [H+] and [OH-] from pH or pOH. Be able to calculate pH and pOH from [H+] or [OH-] pH=-log[H3O+] pOH=-log[OH-] [H3O+]=antilog - pH [OH-]=antilog –pOH [H3O+] [OH-]=1X10-14 pH +pOH=14 X. How is pH measured? XI. What is a buffer and how do buffers work? XII. Describe an acid base titration and how an appropriate indicator is selected. XIII. Calculate the concentration of an unknown acid or base from its volume and the volume of acid or base with known concentration required to complete neutralization in a titration reaction. NA ·VA=NB ·VB XIV. Explain how indicators work. Hin ↔In- + H+