Chemistry 107
Spring 1999

1.1 (1/20) Introduction
Reading: Chapter 1
Keywords: chemistry
Learning objectives:

Although we do not explicitly discuss Chapter 1, there are a couple of things in there which are essential to your being able to work problems in this course.  Just to be clear, I will list a couple of objectives for these.

Objectives

• Express numbers in scientific notation and carry out simple arithmetic operations
• Convert units on various quantities using appropriate conversion factors

1.2 (1/22) Matter: Atoms & Molecules
Reading: Chapter 2
Keywords: atom, molecule
Learning objectives:

Be able to...

• paraphrase the atomic theory of matter.
• calculate the molar mass of a substance from its chemical formula.
• convert between mass and number of molecules

2.1 (1/25) Composition & Representations of Molecules
Reading: Sections 3.1, 3.2, 3.4-3.6
Keywords: formula, mole
Learning objectives:

Be able to...

• calculate the mass % composition of a substance from its chemical formula.
• explain the definition of a mole in your own words.
• interconvert between mass, number of molecules, and number of moles.
• determine a chemical formula from elemental analysis data (i.e., from % composition).

2.2 (1/27) Introduction to Chemical Reactions
Reading: Sections 4.1, 4.2
Keywords: Reaction, equation, conservation laws
Learning objectives:

Be able to...

• recognize some common types of chemical reactions (decomposition, combustion, etc.).
• explain balancing a chemical equation as an application of the law of conservation of mass.
• list at least 3 quantities which must be conserved in chemical reactions.
• write balanced chemical equations for simple reactions, given either an unbalanced equation or a verbal description (i.e., nitrogen and hydrogen gases react under appropriate conditions to form gaseous ammonia (NH₃)).
• interpret chemical equations in terms of both moles and molecules.

2.3 (1/29) Reaction Stoichiometry
Reading: Sections 4.2 - 4.4
Keywords: Stoichiometry, conservation laws
Learning objectives:

Be able to...

• calculate the amount of product expected to be formed in a chemical reaction, given the amounts of reactants used.  ("Amount" might refer to either mass or number of moles.)
• calculate the amount(s) of reactants which need to be used in a chemical reaction in order to produce a specified amount of product.  ("Amount" might refer to either mass or number of moles.)
• identify a limiting reagent and calculate the amount of product formed from a non-stoichiometric mixture of reactants.

3.1 (2/1) Ions & Solutions
Reading: Sections 2.4, 3.3, 3.7
Keywords: Ions, solutions, concentration
Learning objectives:

Be able to...

• define the concentration of a solution, and calculate the molarity of solutions from various data.
• calculate the molarity of solutions prepared by dilution, or calculate the quantities needed to carry out a dilution to prepare a solution of a specified concentration.
• distinguish between electrolytes and non-electrolytes, and explain how their solutions differ.
• describe the species expected to be present (ions, molecules, etc.) in various simple solutions.
• recognize some ionic compounds from their formulas.

3.2 (2/3) Reactions in Solution, Acids & Bases
Reading: Sections 4.5, 4.6
Keywords: Acid, base, stoichiometry
Learning objectives:

Be able to...

• write both molecular and ionic equations for solution reactions.
• define acid and base.
• identify some common acids and bases.
• distinguish between strong and weak acids or bases, and describe the species expected to be present in their solutions.
• write equations for acid-base reactions.
• calculate solution concentrations from titration data.

3.3 (2/5) Solution Stoichiometry
Reading: Sections 4.5, 4.6
Keywords: Solution stoichiometry
Learning objectives:

Be able to...

• perform stoichiometric calculations involving reactions in solutions, including precipitation reactions.

Be able to...

• describe experiments that lead to the gas laws as empirical observations.

4.2 (2/10) Exam #1 (Morning broadcast will be a review.)
Reading: None
Keywords: Exam
Learning objectives:

Be able to...

• Demonstrate your mastery of the material from Chapters 1 - 5.

4.3 (2/12) The Ideal Gas Law & the Kinetic Theory of Gases
Reading: Sections 5.1 - 5.4
Keywords: Ideal gas, gas law
Learning objectives:

Be able to...

• perform simple gas calculations.
• state the postulates of the kinetic theory of gases.
• describe how the postulates of kinetic theory account for the gas laws (qualitatively).
• identify conditions under which gases might behave non-ideally.

Be able to...

• describe the Maxwell-Boltzmann distribution of speeds, and the effect of temperature and molar mass on molecular speed
• perform stoichiometric calculations for reactions involving gases as reactants or products.

5.2 (2/17) Light: The Wave Particle Duality
Reading: Sections 6.1 & 6.2
Keywords: Waves, interference, photons, photoelectric effect
Learning objectives:

Be able to...

• describe waves in terms of frequency, wavelength, and amplitude.
• interconvert between frequency, wavelength, and amplitude for light.
• describe interference as a wave property.
• relate properties of light such as color and brightness to wave characteristics (i.e., l, n, etc.).
• discribe the photoelctric effect by stating what sort of experiment is involved and what results are seen.
• explain how the results of the photoelectric effect experiment are consistent with a photon model of light.
• use the Planck equation to calculate the energy of a photon from wavelength or frequency

5.3 (2/19) Spectra and Energy Levels
Reading: Section 6.3
Keywords: Absorption, emission, quantized
Learning objectives:

Be able to...

• describe in your own words what is seen when atoms absorb or emit light.
• use conservation of energy ideas to explain how the observation of atomic spectra implies that atoms have quantized energies.
• draw an energy level diagram for a simple atom.
• use an energy level diagram to predict the wavelengths or frequencies of light an atom will absorb or emit, or use the observed wavelengths or frequencies to determine the allowed energy levels.

6.1 (2/22) Atoms, Electrons & Energy Levels
Reading: Sections 6.2, 6.3, Box 7-2
Keywords: Energy level, ionization energy, photoelectron
Learning objectives:

Be able to...

• define ionization energy.
• appreciate that the idea of energy levels has its origins in measurable experimental data.
• describe what happens in photoelectric spectroscopy, and explain how the results show that electrons in atoms have only certain allowed energies.
• given a photoelectron spectrum, determine what element the data correspond to.

6.2 (2/24) Electrons, Quantum Numbers, and Orbitals
Reading: Sections 6.5, 7.1
Keywords: Wave, orbital, delocalized, quantum number
Learning objectives:

Be able to...

• paraphrase the uncertainty principle.
• recognize how quantum numbers arise as a consequence of the wave model.
• define the term "orbital."
• state the meanings of the quantum numbers n, l, ml, and ms, and list the allowed values for each quantum number.
• identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.
• list the number of orbitals of each type (1s, 3p, etc.) in an atom.

6.3 (2/26) Atomic Orbitals: Size, Shape, & Energy
Reading: Sections 7.1 - 7.5
Keywords: Orbital, electron configuration
Learning objectives:

Be able to...

• sketch the shapes of s and p type orbitals, and recognize orbitals by their shapes.
• rank various orbitals in terms of size and energy.
• describe the role of screening in determining orbital size and energy.
• use the Pauli exclusion principle and Hund's rule to write electron configurations for atoms and ions of representative elements.
• explain the connection between valence electron configurations and the periodic table.

7.1 (3/1) Electron Configuration & Periodic Properties
Reading: Sections 7.4 - 7. 8
Keywords: Electron configuration, valence electrons, periodic table
Learning objectives:

Be able to...

• define the following properties of atoms: atomic radius, ionization energy, electron affinity.
• state how the above properties vary with position in the periodic table.
• explain the periodic variation of atomic properties in terms of orbitals and shielding.
• list several physical properties which distinguish metals and non-metals.
• explain, in terms of electron configurations, why metals tend to form cations while non-metals tend to form anions.

7.2 (3/3) Chemical Bonding & Lewis Structures
Reading: Sections 8.1 - 8.3
Keywords: Electronegativity, covalent bonding, Lewis structure
Learning objectives:

Be able to...

• define electronegativity, and state how electronegativity varies with position in the periodic table.
• identify/predict polar, non-polar, and ionic bonds by comparing electronegativities.
• write Lewis electron structures for simple molecules or ions.

7.3 (3/5) Chemical Bonding and Orbital Overlap
Reading: Section 8.1
Keywords: bonding, orbital overlap, geometry
Learning objectives:

Be able to...

• write Lewis electron structures for simple molecules or ions.
• describe chemical bonding in simple molecules using a model based on the overlap of atomic orbitals.
• recognize some of the limitations of this simple model.

Be able to...

• appreciate that molecular geometries can be measured experimentally.
• state how hybridization reconciles observed molecular shapes with the orbital overlap model.
• predict the geometry of a molecule from its Lewis structure.
• rationalize common molecular geometries in terms of orbital overlap and hybridization.

8.2 (3/10) Exam #2 (Morning broadcast will be a review.)
Reading: None
Keywords: Exam
Learning objectives:

Be able to...

• Demonstrate your mastery of the material covered since the last exam .

8.3 (3/12) Molecular Geometries, Multiple Bonds
Reading: Sections 8.4, 8.6, 9.1
Keywords:
Learning objectives:

Be able to...

• use models (real and/or software) to help visualize the common molecular shapes.
• use the basic shapes we've examined to determine the geometry of larger molecules.
• explain the formation of multiple bonds in terms of overlap of a combination of hybridized and unhybridized atomic orbitals.
• identify sigma and pi bonds in a molecule, and explain the difference between them.

Be able to...

• state some shortcomings of the (localized) orbital overlap model.
• describe similarities and differences between the localized and delocalized orbital models for bonding.
• draw molecular orbital energy level diagrams for simple diatomic molecules.
• use MO energy levels to predict bond orders and magnetic properties of simple diatomic molecules.
• recognize that the MO approach can be generalized to larger molecules. (But you are not expected to be able to construct energy level diagrams for these larger molecules.)

9.2 (3/24) Bonding in Solids: Metals & Insulators
Reading: Section 9.6
Keywords: band diagram, band gap, conductor, insulator
Learning objectives:

Be able to...

• describe the generalization of the MO theory to describe bonding in solids.
• draw band diagrams for metals, insulators
• explain how the electrical properties of metals & insulators are related to their chemical bonding.

9.3 (3/26) Bonding in Solids: Semiconductors
Reading: Section 9.6
Keywords: band diagram, band gap, semiconductor
Learning objectives:

Be able to...

• draw band diagrams for semiconductors (including n- and p-type devices).
• identify a material as metal, insulator, or semiconductor from its band diagram.
• explain how the electrical properties of metals, insulators, and semiconductors are related to their chemical bonding.

10.1 (3/29) Chemical Energetics
Reading: Sections 9.2, 12.1, 12.2
Keywords: Bond energy, [delta]E, thermodynamics
Learning objectives:

Be able to...

• use tabulated bond energies to obtain approximate values of [delta]E for chemical reactions.
• define exothermic and endothermic in your own words.
• explain (in your own words) the significance of kinetic and thermodynamic factors in controlling chemical reactions.

10.2 (3/31) Thermodynamics: First Law & Calorimetry
Reading: Sections 12.1 - 12.3
Keywords: heat, work, first law
Learning objectives:

Be able to...

• define work and heat using the standard sign conventions explained in your book.
• define state functions, and explain their importance.
• state the first law of thermodynamics in word and in equation forms.
• use experimental data to obtain values for [delta]E for a chemical reaction.

11.1 (4/5) Calorimetry & Enthalpy
Reading: Sections 12.3 & 12.4
Keywords: Calorimetry & enthalpy
Learning objectives:

Be able to...

• use experimental data to obtain values for [delta]E and [delta]H for chemical reactions.
• Define [delta]H_f.
• Write formation reactions for compounds.

11.2 (4/7) Enthalpy & Hess's Law
Reading: Sections 12.3 & 12.4
Keywords: Enthalpy, Hess's Law
Learning objectives:

Be able to...

• explain Hess's Law in your own words.
• Calculate the amount of energy liberated or consumed in chemical reactions from tabulated data.
• Obtain thermodynamic data (i.e., [delta]H_f ) from lab measurements.

11.3 (4/9) Entropy & The Second Law
Reading: Sections 13.1 - 13.3
Keywords: Entropy, Spontaneity, Second Law
Learning objectives:

Be able to...

• explain entropy in your own words in terms of atomic and molecular order.
• deduce the sign of [delta]S for many chemical reactions by examining the physical state of the reactants and products.
• state the Second Law of Thermodynamics, in words and equations, and use it to predict spontaneity.
• state the Third Law of Thermodynamics.
• use tabulated data to calculate the entropy change for a chemical reaction.

Be able to...

• state the Third Law of Thermodynamics.
• use tabulated data to calculate the entropy change for a chemical reaction.
• use tabulated data to predict the spontaneity of a chemical reaction.
• derive the relationship between the free energy change of a system and the entropy change of the universe.
• use tabulated data to calculate the free energy change for a chemical reaction.
• explain the role of temperature in determining whether a reaction is spontaneous.
• use tabulated data to determine the temperature range for which a reaction will be spontaneous.

12.2 (4/14) Exam #3 (Morning broadcast will be a review.)
Reading: None
Keywords: Exam
Learning objectives:

Be able to...

• demonstrate your mastery of the material covered since the last exam .

12.3 (4/16) Introduction to Chemical Kinetics
Reading: Sections 14.1 - 14.3
Keywords: Rate, order of reaction
Learning objectives:

Be able to...

• define the rate of a chemical reaction, and express the rate in terms of the various reactants or products.
• use experimental data to determine rate laws for reactions by the method of initial rates. (Note that this method is NOT discussed in your text!)

Be able to...

• use experimental data to determine rate laws for reactions using graphical methods.
• distinguish between elementary reactions and multi-step reactions.
• find the rate law predicted for a particular reaction mechanism.

13.2 (4/21) Rate Laws & Mechanisms
Reading: Sections 14.4 & 14.5
Keywords: mechanism, rate determining step
Learning objectives:

Be able to...

• distinguish between elementary reactions and multi-step reactions.
• find the rate law predicted for a particular reaction mechanism.

13.3 (4/23) Kinetics & Equilibrium: Reversible Reactions
Reading: Sections 14.5, 15.1
Keywords: reversible reaction, equilibrium
Learning objectives:

Be able to...

• derive rate laws for mechanisms involving reversible steps in equilibrium.
• realize that equilibrium is dynamic, and that at equilibrium, the forward and backward reaction rates are equal. Be able to state these ideas in your own words.
• define the equilibrium constant for a reversible reaction.
• calculate equilibrium constants from experimental data.

14.1 (4/26) Chemical Equilibrium & LeChatlier's Principle
Reading: Sections 15.4 & 15.6
Keywords: Equilibrium, LeChatlier's Principle
Learning objectives:

Be able to...

• calculate equilibrium composition from initial data and equilibrium constant.
• explain the response of an equilibrium system to applied stresses: LeChatlier's Principle.
• calculate new equilibrium composition of a system after an applied stress.

14.2 (4/28) Chemical Equilibrium & LeChatlier's Principle
Reading: Sections 15.4 & 15.6
Keywords: Equilibrium, LeChatlier's Principle
Learning objectives:

Be able to...

• calculate equilibrium composition from initial data and equilibrium constant.
• explain the response of an equilibrium system to applied stresses: LeChatlier's Principle.
• calculate new equilibrium composition of a system after an applied stress.

14.3 (4/30) Temperature, Reaction Rates, Molecular Collisions, & Catalysis
Reading: Section 14.6, 14.7
Keywords: Arrhenius Equation, activation energy, catalyst
Learning objectives:

Be able to...

• explain (in your own words) the significance of the terms in the Arrhenius equation based on collision theory.
• calculate the activation energy for a reaction from experimental data.
• explain the role of a catalyst in the design of practical chemical reactions.

Be able to...

• list topics and concepts to be addressed in the final exam.
• get help with any problems or concepts which are giving you trouble.

15.2 (5/4) NO CLASS BROADCAST!