American Chemical Society Cumulative Exam (Chemistry and Measurement)

Chemistry and Measurement  Understand the process of using scientific experiments and describing the law of conservation of matter  Compare and contrast physical and chemical properties of matter  Be able to calculate density, mass, and volume of a substance  Display the knowledge on determining the appropriate significant figures and correct use of scientific Atoms, Molecules, and Ions  Understand the names and symbols of common elements  Demonstrate the ability of writing the nuclide symbols  Display an understanding of the mass, charge, and location of the electrons, protons, and neutrons  Be able to calculate the atomic weight, fractional abundance, and isotopic weights  Demonstrate an understanding of periodic table and how the elements are arranged (metals, non-metals, metalloids)  Understand the ionic and molecular formulas, common polyatomic ions and nomenclature of organic  Be able to write and balance chemical equations Chemical Reactions  Recognize the importance of mole concept in calculating moles, mass, formula weight and their inter- conversions  Calculation of percent composition from given formula, empirical formula, and mass of an element in a given mass of compound  Be able to calculate the limiting reagent and relate the quantities in a chemical equation  Understand the basic concepts of acid-base reactions  Determine the molecular, complete and net ionic equations and be able to predict whether precipitation occurs  Write equations for neutralization and those involving gas formation  Classify electrolytes, acids and bases as weak or strong  Be able to assign oxidation numbers and balance redox reactions  Work with solution in determining molarity, dilutions and volumetric analysis The Gaseous State  Be able to convert units of pressure  Understand the empirical gas laws and its application.  Deriving empirical gas laws from the ideal gas law.  Apply the ideal gas law.  Relate gas density and molecular weight.  Solve stoichiometry problems involving gases.  Calculate partial pressures and mole fractions.  Calculate the amount of gas collected over water.  Calculate the rms speed of gas molecules.  Calculate the ratio of effusion rates of gases.  Using the van der Waals equation. Thermochemistry  Calculate the heat of reaction from the stoichiometry.  Relate heat and specific heat.  Calculate heat of reaction from stoichiometry  Calculate ∆H from calorimetric data.  Calculate the enthalpy of reaction from standard enthalpies of formation.  Able to apply Hess’s law Quantum Theory of the Atom  Relate wavelength and frequency of light.  Calculate the energy of a photon.  Determine the wavelength, frequency, or the energy level difference of a hydrogen atom transition.  Determine and apply the rules for quantum numbers and orbital shapes Electron Configurations and Periodicity  Apply the Pauli exclusion principle.  Determine the configuration of an atom using the Aufbau principle.  Determine the configuration of an atom using the period and group numbers.  Apply the Hund’s rule.  Applying periodic trends and predict behavior elements Ionic and Covalent Bonding  Use Lewis symbols to represent ionic bond formation.  Write electron configurations of ions.  Using periodic trends to obtain relative ionic radii.  Use electronegativities to obtain relative bond polarity.  Write Lewis formulas.  Write resonance structures.  Use formal charges to determine the best Lewis formula.  Relate bond order and bond length.  Estimate ∆H from bond energies. Molecular Geometry and Chemical Bonding Theory  Predict molecular geometries.  Relate dipole moment and molecular geometry.  Apply valence bond theory.  Describe molecular orbital configurations.  Relate dipole moment and molecular geometry  Apply valence bond theory in terms of hybrid and unhybridized atomic orbitals  Describe molecular orbital configurations and apply molecular orbital theory to determine magnetic behavior and bond order/stability States of Matter; Liquids and Solids • Calculate heat for a phase change of a given mass of substance. Calculate vapor pressures and heats of vaporization. • Identify intermolecular forces. Determine relative vapor pressure on the basis of intermolecular attraction. • Identify types of solids. Determine the relative melting points based on types of solids. • Determine the number of atoms per unit cell. Calculate atomic mass from unit-cell and density. Solutions  Apply Henry’s law.  Calculate solution concentration in molarity and molality.  Convert concentration units.  Calculate vapor-pressure lowering.  Calculate the boiling-point elevation and freezing-point depression.  Calculate the molecular weights  Calculate the osmotic pressure.  Determine the colligative properties of ionic solutions. Rates of Reaction  Relate the different ways of expressing reaction rates  Calculate the average reaction rate  Determine the order of reaction from the rate law  Determine the rate law from initial rates  Use the concentration-time equation for first-order reactions  Relate the half-life of a reaction to the rate constant  Use the Arrhenius equation  Write the overall chemical equation from a mechanism  Determine the molecularity of an elementary reaction  Write the rate equation for an elementary reaction  Determine the rate law from a mechanism Chemical Equilibrium  Apply stoichiometry to equilibrium  Write equilibrium constant expression  Calculate equilibrium constant  Use reaction quotient  Calculate equilibrium concentration  Solve equilibrium problems and equations  Apply “change-reaction-condition” principle  Understand and apply the Le Chatelier’ principle Acids and Bases and their Equilibria  Identify acid and base species  Identify Lewis acid and base species  Decide whether reactants or products are favored in an acidbase reactions  Calculate the concentration of H and OH in solutions of strong acid or base  Calculate the pH from the hydrogen-ion concentration, and vice versa  Determine K (or K) from the solution pH  Calculate the concentration of a species in a weak acid solution using Ka  Calculate the concentration of a species in a weak base solution using Kb  Predict whether a salt solution is acidic, basic, or neutral  Obtain Ka from Kb or Kb from Ka  Calculate concentrations of species in a salt solution  Calculate the common-ion effect on acid ionization  Calculate the pH of a buffer from given volumes of solution  Calculate the pH of a solution of a strong acid and a strong base  Calculate the pH at the equivalence point in the titration of a weak acid with a strong base Solubility and Complex-Ion Equilibria  Understand the solubility product constant as the equilibrium constant for the solubility  Equilibrium of a slightly soluble ionic compound  Familiarize with writing expressions for the solubility product  Comprehend the influence of a common ion on solubility  Describe the qualitative effect of a pH change on solubility  Comprehend the process of complexation and the meaning of the formation constant K  Calculate Ksp from solubility or solubility from Ksp  Predict if/when precipitation will occur when two solutions are mixed given the volumes, molarities, and Ksp values  Predict whether a precipitate will form in the presence of a complex ion given K and K  Calculate solubility of a slightly soluble ionic compound in a solution of the complex ion Thermodynamics and Equilibrium  Comprehend relationship between free energy change for a reaction and the reaction quotient for a reaction  Comprehend relationship between standard state free energy change and equilibrium constant  Understand and apply the entropy and second law of thermodynamics  Understand the change of free energy with temperature Electrochemistry  Comprehend half-reactions  Demonstrate proficiency in balancing oxidation-reduction equations  Understand a voltaic cell: cathode, anode, salt bridge, cell emf, notation  Relate chemical reactions to cell voltage  Calculate standard cell voltages from table of standard electrode potentials  Comprehend relation between standard cell emf, equilibrium constant, and standard free energy change  Predict direction of electron flow (spontaneity) given cell voltage  Calculate cell emf from standard state cell emf and ion concentrations using the Nernst equation  Calculate ion concentrations from cell emf and reference electrode emf  Understand an electrolytic cell: cathode, anode, driving emf  Comprehend factors that govern what anodic and cathodic products are formed of an electrolytic cell  Understand common everyday examples of voltaic and electrolytic cells: fuel cells, Li ion, lead-acid, cathodic protection of pipes, production of hydrogen and oxygen from water  Contrast and compare voltaic and electrolytic cells Nuclear Chemistry  Familiarity writing and interpreting nuclear equations for radioactive decay processes  Determine the product or reactant from a nuclear equation given all but 1 nuclide  Predict relative stabilities of nuclides  Predict most likely type of decay for a given radioactive isotope  Familiarity with notation for a nuclear bombardment reaction  Comprehend the meaning of the decay constant and the impact of radioactive decay on the change in the amount of material present over a given period of time  Calculate the decay constant given the activity of a radioactive isotope  Relate the decay constant, half-life, and activity  Calculate the fraction of nuclei remaining after a given time from the half-life of a radioactive isotope Chemistry of Main-Group and Transition Elements and Coordination Compounds  Understand the general observations about main-group elements  Familiarize with key physical and chemical properties of the main-group elements  Familiarize with the chemistry of non-metals in each family and nobble gases  Understand the periodic trends in the transition metal elements  Be able to name according to IUPAC and determine the structure of complexes  Comprehend the relative magnitude of crystal field splitting induced by major components of the spectrochemical series  Apply crystal field theory to describe bonding in coordination compounds (high-spin and/or low spin) as well as magnetic properties (paramagnetic vs. diamagnetic) Organic Chemistry  Know nomenclature for alkanes, alkenes, alkynes, aromatic hydrocarbons, and functional groups  Comprehend the organic molecules containing oxygen  Comprehend the organic molecules containing nitrogen Polymer Materials  Know the synthesis of organic polymers  Comprehend the properties of electrical conducting polymers  Understand proteins and nucleic acids as forms of biological polymers