CHEM 1364 Introduction: Matter and Measurement (Chapter 1) Textbook references to Brown, LeMay, Bursten, Murphy, and Woodward 12 th Edition Classification of matter Given sufficient information be able to distinguish between pure substances and 1.1 HW #2 8/24 mixtures (1.2) 1.2 Be able to distinguish between elements and compounds (1.2) HW #2 8/24 1.3 Be able to distinguish between homogeneous and heterogeneous mixtures (1.2) 5 HW #2 8/24 Physical and chemical changes and properties 2.1 Identify properties as being either physical or chemical properties (1.3) 3 HW #2 8/24 2.2 Identify changes as being either physical or chemical changes (1.3) HW #2 8/24 Introduction to measurement SI system, unit conversion, dimensional analysis 3.1 State the base units in the SI system (1.4) HW #3 8/25 3.2 Identify units and the measurement type to which they correspond (1.4) HW #3 8/25 3.3 Interconvert metric units (1.4) HW #3 8/25 3.4 Given a formula for temperature conversion, be able to convert between Celsius, Kelvin, and Fahrenheit (1.4) HW #3 8/25 3.5 Use the definition of density to find missing information (1.4) 2 HW #4 8/29 3.6 Distinguish between measured and exact numbers (1.5) 2 HW #4 8/29 3.7 Identify and operate with significant figures in given measured quantities (1.5) All experiments that require measurement HW #4 8/29 3.8 Use dimensional analysis to convert from one set of units to another (1.6) HW #5 8/30 3.9 Use dimensional analysis to convert one derived quantity (density, volume, etc.) to another set of units (1.6) HW #5 8/30
CHEM 1364 Atoms, Molecules, and Ions (Chapter 2) Textbook references to Brown, LeMay, Bursten, Murphy, and Woodward 12 th Edition Atomic theory of matter and subatomic particles 4.1 Identify key results of historical experiments that led to the discovery of subatomic particles (2.1 2.2) HW #6 8/31 4.2 Identify the three primary subatomic particles with which chemists deal including the charge and relative masses of these particles (2.3) HW #6 8/31 4.3 Describe the current view of the atom in terms of subatomic particles (2.3) HW #6 8/31 4.4 Define and use the terms atomic number, atomic weight, mass number, and isotope (2.3) HW #7 9/1 4.5 Given sufficient information state the number of protons, electrons, and neutrons in a species (2.3) HW #7 9/1 4.6 Determine the atomic weight of an element given its isotopic abundances (2.4) HW #7 9/1 An introduction to the periodic table 5.1 Identify periods and groups on the periodic table (2.5) HW #7 9/1 Formation of molecular and ionic compounds 6.1 Distinguish between pairings of elements likely to form molecular compounds and those likely to form ionic compounds (2.6-2.7) HW #8 9/6 6.2 Identify the seven elements that exist in nature in the diatomic state (2.6) HW #8 9/6 6.3 Define the terms molecular compound, molecule, molecular formula, and empirical formula (2.6) HW #8 9/6 6.4 Predict the ion most likely formed from an element s position on the periodic chart (2.7) HW #8 9/6 6.5 Write formulas for the ionic compound formed between metals and nonmetals (2.7) HW #8 9/6 6.6 Name both molecular and ionic compounds including the Stock system (2.8) HW #9 9/7 6.7 Name aqueous inorganic acids (2.8) HW #9 9/7
CHEM 1364 Stoichiometry: Calculations with Chemical Equations and Formulas (Chapter 3) - Textbook references to Brown, LeMay, Bursten, Murphy, and Woodward 12 th Edition Chemical equations 7.1 Identify reactants and products in a chemical equation (3.1) HW #10 9/8 7.2 Balance a given chemical equation (3.1) HW #10 9/8 Some simple patterns of reactivity 8.1 Identify reactions as being combination, decomposition, or combustion (3.2) HW #10 9/8 Formula weights 9.1 Given a substance by name or formula, calculate its formula weight (3.3) HW #11 9/12 Determine the elemental percentages in a compound from its chemical formula 9.2 (3.3) Avogadro s number and the mole Given sufficient starting information, determine other information about a 10.1 sample size i.e., number of grams, moles, atoms, molecules, etc (3.4) Empirical formulas from analyses Given a mass or percent composition of a chemical compound, determine its 11.1 empirical formula and, if sufficient information is provided, its molecular formula (3.5) 11.2 Determine the chemical formula of a compound from the results of a combustion analysis (3.5) Quantitative information from balanced equations 12.1 Using information about one reactant, determine the quantities, in various units, of reactants consumed and products formed in a chemical reaction (3.6) Limiting reactants 13.1 Given starting quantities of multiple reactants, determine the amounts of reactants consumed and products formed (limiting reactant problem) (3.7) 13.2 Determine the percent yield of products in a reaction given sufficient information (3.7) HW #11 9/12 HW #12 9/13 6 HW #13 9/14 HW #13 9/14 HW #14 9/19 HW #15 9/20 7 HW #15 9/20
CHEM 1364 Aqueous Reactions and Solution Stoichiometry (Chapte 4) Textbook references to Brown, LeMay, Bursten, Murphy, and Woodward 12 th Edition General properties of aqueous solutions 14.1 Define the terms electrolyte, nonelectrolyte, strong electrolyte, and weak electrolyte (4.1) HW #16 9/21 Identifying the nature of an electrolyte 15.1 Be able to identify (without a chart) whether a particular ionic compound is soluble or insoluble in water (4.2) 8 HW #16 9/21 15.2 Be able to identify (without a chart) whether a particular acid is a strong or weak acid (4.3) 8 HW #17 9/22 15.3 Be able to identify (without a chart) whether a particular base is a strong or weak base (4.3) 8 HW #17 9/22 15.4 Using your knowledge from the three items immediately above, classify a given substance as to whether it is an acid, base, or salt; soluble in water or insoluble in water; strong or weak/non electrolyte (4.3) 8 HW #17 9/22 Completing and balancing chemical equations 16.1 Given the reactants in a metathesis (exchange, double displacement are synonyms) complete and balance the equation (4.2) HW #18 9/26 16.2 Given the reactants in a neutralization reaction (a specific type of metathesis reaction) complete and balance the equation (4.3) HW #18 9/26 16.3 Assign oxidation numbers to atoms in both neutral compounds and ions (4.4) 9 HW #19 9/27 16.4 Identify the reducing agent and oxidizing agent in an oxidation-reduction reaction (4.4) 9 HW #19 9/27 16.5 Complete and balance single displacement chemical equations (4.4) 9 HW #19 9/27 16.6 Predict whether or not a redox reaction will occur given the activity series (4.4) HW #19 9/27 16.7 Write the molecular equation, total ionic equation, and net ionic equation for any given chemical reaction (4.2-4.4) 8 HW #20 9/28 Expressing concentrations of solutions quantitatively 17.1 Define molarity for a solution (4.5) HW #21 9/29 17.2 Interconvert molarity, moles solute, grams solute, and volume of solution (4.5) HW #21 9/29 17.3 Determine missing information in a dilution type of problem (4.5) HW #21 9/29 Solution stoichiometry and chemical analysis 18.1 Define titration (4.6) 10 HW #22 10/3 18.2 Work stoichiometry problems (including limiting reactant) when one or more reactants are initially in solution (4.6) 10 HW #22 10/3
CHEM 1364 Thermochemistry (Chapter 5) Textbook references to Brown, LeMay, Bursten, Murphy, and Woodward 12 th Edition The nature of energy 19.1 Recognize energy as the capacity to do work or transfer heat (5.1) HW #22 10/4 19.2 Distinguish between kinetic and potential energy (5.1) HW #22 10/4 19.3 Identify commonly used units of energy (5.1) HW #22 10/4 19.4 Define the terms system, surrounding, isolated system, open system, and closed system (5.1) HW #22 10/4 The First Law of Thermodynamics and its applications 20.1 State the First Law of Thermodynamics in terms of heat and work (5.2) HW #23 10/5 20.2 Calculate internal energy changes, heat, and work given sufficient information (5.2) HW #23 10/5 20.3 Define the terms endothermic and exothermic (5.2) HW #23 10/5 20.4 Define the term state function and give examples (5.2) HW #23 10/5 Enthalpy 21.1 Define enthalpy in terms of internal energy (5.3) HW #24 10/6 21.2 State the reason enthalpy is our most commonly used thermodynamic function (5.3) HW #24 10/6 Calorimetry 22.1 Define the terms heat capacity and specific heat capacity (5.5) 11, 12 HW #24 10/6 22.2 Use the definitions of heat capacity and specific heat capacity to find missing numerical information (5.5) 11, 12 HW #24 10/6 22.3 Find missing information in a calorimetry experiment given sufficient data (5.5) 11, 12 HW #24 10/6 Hess Law and its applications 23.1 State Hess s Law (5.6) HW #25 10/10 23.2 23.3 23.4 Given a sufficient set of data apply Hess s Law to find missing numerical information (5.6) Write the formation reaction for defining the enthalpy of formation of a substance (5.7) Use given enthalpies of formation to determine missing thermochemical information about a reaction (5.7) HW #25 10/10 HW #26 10/11 HW #26 10/11
CHEM 1364 Electronic Structure of Atoms (Chapter 6) Textbook references to Brown, LeMay, Bursten, Murphy, and Woodward 12 th Edition The wave nature of light 24.1 Interconvert wavelength, speed, frequency, and energy for electromagnetic radiation (6.1) HW #27 10/12 24.2 Correlate wavelength, frequency, and energy with regions of the electromagnetic spectrum(6.1) HW #27 10/12 Further understanding of the nature of light 25.1 Describe the contributions of the black-body effect and the photoelectric effect toward our current understanding of the nature of light (6.2) HW #27 10/12 Describe line spectra in terms of the Bohr model of the atom 26.1 Qualitatively describe the Bohr model of the atom (6.3) HW #28 10/17 26.2 Use the Rydberg equation (or its equivalent) to determine missing information (6.3) HW #28 10/17 26.3 State the limitations of the Bohr model (6.3) HW #28 10/17 The wave nature of matter 27.1 State the contribution of debroglie to a description of matter as both wave and particulate (6.4) HW #29 10/18 27.2 State the Heisenberg Uncertainty Principle and its contribution to our understanding of the atom (6.4) HW #29 10/18 Applying quantum mechanics to atoms 28.1 State the four quantum numbers and their interrelationships (6.5) HW #29 10/18 28.2 Correlate the quantum numbers with the designations s, p, d, and f (6.5) HW #29 10/18 28.3 Correlate the shapes and sizes of orbitals with the corresponding quantum numbers (6.6) HW #30 10/19 28.4 Apply the Pauli Exclusion Principle to the writing of electron configurations (6.7) HW #30 10/19 28.5 Apply Hund s Rule to the writing of electron configurations (6.8) HW #30 10/19 28.6 Write orbital diagrams for any given element or ion (6.8) HW #30 10/19 28.7 Write condensed electron configurations for any given element or ion (6.8) HW #31 10/24 28.8 Identify the number of valence electrons for any given species (6.8) HW #31 10/24 28.9 Use the periodic table to write electron configurations (6.9) HW #31 10/24 28.10 In a few cases, be able to explain why the electron configuration of an element differs from that normally expected examples Cu and Cr (6.9) HW #31 10/24
CHEM 1364 Periodic Properties of the Elements (Chapter 7) Textbook references to Brown, LeMay, Bursten, Murphy, and Woodward 12 th Edition Development of the periodic table 29.1 Describe contributions of Mendeleev, Meyer, and Moseley to the development of the periodic table (7.1) 13 HW #32 10/25 Effective nuclear charge 30.1 Define effective nuclear charge (7.2) HW #32 10/25 30.2 Discuss qualitatively the effective nuclear charges in a series of atoms/ions (7.2) HW #32 10/25 30.3 Describe trends in effective nuclear charge (7.2) HW #32 10/25 Sizes of atoms and ions 31.1 Given a set of atoms and ions, arrange in order of decreasing or increasing radius (7.3) HW #33 10/26 31.2 Explain the cause of trends in atomic and ionic radii (7.3) HW #33 10/26 31.3 Identify species that are isoelectronic (7.3) HW #33 10/26 Ionization energy 32.1 Define ionization energy (7.4) HW #33 10/26 32.2 Explain the cause for observed trends in ionization energy (7.4) HW #33 10/26 32.3 Explain general cause for key deviations from trends in ionization energy (7.4) HW #33 10/26 32.4 Given a set of atoms and/or ions, arrange in order of decreasing or increasing ionization energy (7.4) HW #33 10/26 Electron affinities 33.1 Define electron affinity (7.5) HW #34 10/27 33.2 Explain the cause for observed trends in electron affinity (7.5) HW #34 10/27 33.3 Explain general cause for key deviations from trends in ionization energy (7.5) HW #34 10/27 Given a set of atoms and/or ions, arrange in order of decreasing or increasing 33.4 HW #34 10/27 electron affinity (7.5) Electronegativity Given a set of atoms, arrange in order of increasing or decreasing 34.1 HW #34 10/27 electronegativity (8.4) Metals, nonmetals, and metalloids 35.1 Identify acidic or basic nature of oxides based on their composition (7.6) HW #35 10/31 Group trends for active metals 36.1 Distinguish between alkali and alkaline earth metals (7.7) HW #35 10/31 Group trends for selected nonmetals 37.1 Distinguish between chalcogens, halogens, and noble gases (7.8) HW #35 10/31
CHEM 1364 Basic Concepts of Chemical Bonding (Chapter 8) Textbook references to Brown, LeMay, Bursten, Murphy, and Woodward Chemical bonds, Lewis symbols, and the octet rule 38.1 Draw Lewis symbols for monatomic atoms and ions (8.1) HW #36 11/1 38.2 Identify ions formed based on the octet rule (8.1) HW #36 11/1 Ionic bonding 39.1 Identify pairs of atoms likely to form primarily ionic bonds (8.2) HW #36 11/1 39.2 Draw Lewis structures representing the transfer of electrons occurring during the formation of ionic bonds (8.2) HW #36 11/1 Covalent bonding 40.1 Identify pairs of atoms likely to form primarily covalent bonds (8.3) HW #37 11/2 40.2 Draw Lewis structures depicting the combination of pairs of species that form single, double, and triple bonds (8.3) HW #37 11/2 40.3 Estimate the polarity of a chemical bond based on the electronegativity and/or position on the periodic chart of atoms involved (8.4) HW #37 11/2 Draw and use Lewis structures 41.1 Draw the Lewis structure for a given molecule or polyatomic ion (8.5) 14 HW #38 11/4 41.2 Determine from the Lewis structure the formal charge of all atoms involved in a 14 HW #39 11/7 molecule or polyatomic ion (8.5) 41.3 Identify situations which offer the possibility of resonance (8.6) 14 HW #39 11/7 41.4 Draw resonance structures in situations where resonance is possible (8.6) 14 HW #39 11/7 41.5 Identify and draw structures for situations which are exceptions to the octet rule (8.7) 14 HW #39 11/7
CHEM 1364 Molecular Geometry and Bonding Theories (Chapter 9) Brown, LeMay, Bursten, Murphy, and Woodward 12 th Edition VSEPR model and conclusions from Lewis strusture 42.1 State the valence shell electron pair repulsion theory (9.2) 14 HW #40 11/8 42.2 From a Lewis structure you have drawn, determine the number of bonding domains and nonbonding domains in molecules and ions (9.2) 42.3 From a Lewis structure you have drawn, determine the electron domain geometry of molecules and ions through octahedral (9.2) 42.4 From a Lewis structure you have drawn, determine the molecular geometry of molecules and ions through octahedral (9.2) 42.5 From a Lewis structure you have drawn, approximate bond angles within a molecule or ion 42.6 From a Lewis structure you have drawn, determine the whether a molecule or ion is polar or nonpolar (9.3) 42.7 From a Lewis structure you have drawn, determine the hybridization about any atom in the a molecule or ion (9.5) 42.8 From a Lewis structure you have drawn, determine the number of σ and π bonds in a given molecule or ion (9.6) Molecular orbital theory 43.1 Given a molecular orbital energy level diagram for a simple diatomic species, determine the bond order of the species (9.7) 43.2 Given a molecular orbital energy level diagram for a simple diatomic species, determine the diamagnetic or paramagnetic nature of the species (9.7) 14 HW #40 11/8 14 HW #40 11/8 14 HW #40 11/8 14 HW #41 11/9 14 HW #41 11/9 14 HW #42 11/15 HW #42 11/15 HW #43 11/16 HW #43 11/16
CHEM 1364 Gases (Chapter 10) Brown, LeMay, Bursten, Murphy, and Woodward 12 th Edition Physical characteristics of gases 44.1 State in general the physical properties of gases (10.1) HW #44 11/17 Working with gas laws 45.1 Define pressure (10.2) HW #44 11/17 45.2 Work with information from various pressure measuring devices (10.2) HW #44 11/17 45.3 Convert between different pressure units (10.2) HW #44 11/17 45.4 Work with Boyle s Law (10.3) HW #45 11/21 45.5 Work with Charles s Law (10.3) HW #45 11/21 45.6 Work with Avogadro s Law (10.3) HW #46 11/22 45.7 Work with the combined gas law (10.4) HW #46 11/22 45.8 Work with ideal-gas equation (10.4) 15 HW #47 11/28 Other applications of the ideal gas equation 46.1 Determine density from ideal-gas equation (10.5) 15 HW #48 11/29 46.2 Use gas volumes in stoichiometric problems (10.5) HW #48 11/29 46.3 Define partial pressure (10.6) HW #49 11/30 46.4 Given a mixture of gases and sufficient information, determine the partial pressure of each gas (10.6) HW #49 11/30 Kinetic-molecular theory 47.1 Give and work with the five statements of the kinetic-molecular theory (10.7) HW #50 12/1 47.2 Given sufficient information, determine the relative rates of effusion and diffusion of gases (10.8) HW #50 12/1