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Chapter 19: Lattice Energy
Chapter 19: Lattice Energy
■■ explain and use the term lattice energy
■■ explain and use the terms ionisation energy, enthalpy change of atomisation and electron aff inity
■■ construct Born–Haber cycles
■■ use Born–Haber cycles to calculate lattice energies
■■ explain, in qualitative terms, the effect of ionic charge and ionic radius on the numerical magnitude of a lattice energy
■■ interpret and explain qualitatively the trend in the thermal stability of the nitrates and carbonates of Group 2 elements in terms of the charge density of the cation and the polarisability of the large anion
■■ apply Hess’s law to construct energy cycles to determine enthalpy changes of solution and enthalpy changes of hydration
■■ interpret and explain qualitatively the variation in solubility of Group 2 sulfates in terms of the relative values of the enthalpy change of hydration and the corresponding lattice energy
Born-Haber
Born-Haber
Entropy
Entropy
Chapter 20: Electrochemistry
Chapter 20: Electrochemistry
Learning outcomes
you should be able to:
■■ describe electrolytic cells and the redox reactions occurring at the anode and cathode during electrolysis
■■ state the relationship, F = Le, between the Faraday constant, the Avogadro constant and the charge on the electron
■■ predict the identity of the substance liberated during electrolysis from:
– the state of electrolyte (molten or aqueous)
– the position of the ions (in the electrolyte) in the redox series (electrode potential)
– the concentration of the ions in the electrolyte
■■ calculate:
– the quantity of charge passed during electrolysis
– the mass and/or volume of substance liberated during electrolysis, including those in the electrolysis of H2SO4(aq) and Na2SO4(aq)
■■ describe the determination of a value of the Avogadro constant by an electrolytic method
■■ define the terms:
– standard electrode (redox) potential
– standard cell potential
■■ describe the standard hydrogen electrode
■■ describe methods used to measure the standard electrode potentials of:
– metals or non-metals in contact with their ions in
aqueous solution
– ions of the same element in different oxidation states
■■ calculate a standard cell potential by combining two standard electrode potentials
■■ use standard cell potential to:
– deduce and explain the direction of electron flow in a simple cell
– predict the feasibility of a reaction
■■ construct redox equations using the relevant half-equations
■■ describe and deduce from electrode potential values the relative reactivity of the Group 17 elements as oxidising agents
■■ predict qualitatively how the value of an electrode potential varies with the concentration of the aqueous ion
■■ use the Nernst equation to predict quantitatively how the value of an electrode potential varies with the concentration of the aqueous ion
■■ state the possible advantages of developing other types of cell, e.g. the H2/O2 fuel cell, and improved batteries (as in electric vehicles) in terms of smaller size, lower mass and higher voltage.
Electrode Potential
Electrode Potential
Eelectro-Chemical Series
Eelectro-Chemical Series
Chapter 21: Further aspects of equilibria
Chapter 21: Further aspects of equilibria
Learning outcomes
You should be able to:
■ explain the terms pH, pKa and Kw and use them in calculations
■ calculate [H+(aq)] and pH values for strong and weak acids and strong bases
■ explain the choice of suitable indicators for acid–base titrations, given appropriate data
■ describe the changes in pH during acid–base titrations and explain these changes in terms of the strengths of the acids and bases
■ explain how buffer solutions control pH
■ describe and explain the uses of buffer solutions, including the role of HCO3– in controlling pH in the blood
■ calculate the pH of buffer solutions, given appropriate data
■ show understanding of and use the concept of solubility product, Ksp
■ calculate Ksp from concentrations and vice versa
■ show understanding of the common ion effect
■ state what is meant by the term partition coefficient
■ calculate and use a partition coefficient for a system in which the solute is in the same molecular state in the two solvents.
Chapter 22 Ionic Equilibria.pdfAcids, Bases and pH
Acids, Bases and pH
Kw and Bases
Kw and Bases
Chapter 22: Reaction Kinetics
Chapter 22: Reaction Kinetics
Learning outcomes
you should be able to:
■ explain and use the terms:
– rate equation
– order of reaction
– rate constant
– half-life of a reaction
– rate-determining step
■ construct and use rate equations of the form rate = k[A]m[B]n (limited to simple cases of single-step reactions and of multi-step processes with a rate-determining step for which m and n are 0, 1 or 2) including:
– deducing the order of a reaction by the initial rates method
– justifying, for zero- and first-order reactions, the order of reaction from concentration–time graphs
– verifying that a suggested reaction mechanism is consistent with the observed kinetics
– predicting the order that would result from a given reaction mechanism (and vice versa)
– calculating an initial rate using concentration data (not including integrated forms of the rate equation)
■ show understanding that the half-life of a first-order reaction is independent of concentration
■ use the half-life of a first-order reaction in calculations
■ calculate a rate constant using the initial rates or half- life method
■ for a multi-step reaction:
– suggest a reaction mechanism that is consistent with the rate equation and the equation for the overall reaction
– predict the order that would result from a given reaction mechanism (and vice versa)
■ devise a suitable experimental technique for studying the rate of a reaction, from given information
■ outline the different modes of action of homogeneous and heterogeneous catalysts, including:
– the Haber process
– the catalytic removal of oxides of nitrogen in the exhaust gases from car engines
– the catalytic role of atmospheric oxides of nitrogen in the oxidation of atmospheric sulfur dioxide
– the catalytic role of Fe3+ in the I–/S2O32– reaction.
Chapter 23 Reaction Kinetics.pdfKinetic
Kinetic
Rate Equation
Rate Equation
Chapter 24 Group IV.pdfChapter 25 Transition Elements.pdfChapter 26 Benzene and Its Compounds.pdfcie-a2-chemistry-9701-znotes.pdfcie-a2-chemistry-9701-practical-znotes.pdfGoogle Sites
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