1. Review for the Final Exam: A Study Guide Review: 1-6 Chapter 1:Chemistry : The Study of Change Chapter 2:Atoms, Molecules, and Ions Chapter 3:Mass Relationships in Chemical Reactions Chapter 4:Reactions in Aqueous Solutions Chapter 5:Gases Chapter 6:Thermochemistry

2. Review for the Final Exam: A Study Guide (Cont.) Review: 7-11 Chapter 7:Quantum Theory and the Electronic Structure of Atoms Atoms Chapter 8:Periodic Relationships Among the Elements Chapter 9:Chemical Bonding I: Basic Concepts Chapter 10:Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Hybridization of Atomic Orbitals Chapter 11:Intermolecular Forces and Liquids and Solids

3. Chapter 1: The Study of Change Chapter 1  Definition and examples of: matter, states of matter, mixtures (homogeneous and heterogeneous), pure substances, elements, and compounds  Law of constant composition/definite proportion  Names and symbols of common elements  Chemical and physical properties  Chemical and physical changes  Units of measurements (metric, SI, and British systems)  Dimensional analysis and conversion factors in problem solving  Density = Mass / Volume  Temperature relationships and related problems: 0 C = 5/9( 0 F - 32), K = 0 C + 273  Rules for determination of significant figures in a measured quantity Electrolytes (classification and example)

4. Chapter 2: Atoms, Molecules, & Ions Chapter 2  Law of conservation of mass  Atomic mass unit  Modern view of atomic structure (electrons, protons and neutrons)  Nuclear symbol for an atom  Atomic number, mass number, and isotopes  Molecules and ions  Cations, anions, monoatomic and polyatomic ions  Periodic table (periods, groups, metals, nonmetals, transition metals, and metalloids)  Molecular, empirical and structural formula  Chemical bonding: ionic bonds (metal and nonmetal), covalent bonds (among nonmetals)  Naming ionic compounds, ionic charges: Group 1A: +1, 2A: +2, 3A: +3, 5A: -3, 6A: -2, 7A: -1  Naming binary covalent compounds (CO 2, N 2 O 4, etc.)

5. Chapter 3: Mass Relationships in Chemical Reactions Chapter 3  Balancing chemical equations  Determination of average atomic mass (atomic weight) with isotopic distribution  Calculation of % composition and formula weight  The mole and related problems (Avogadro’s number = 6.022 x 10 23 )  Determination of empirical formula and molecular formula  Calculations based on the stoichiometry of chemical equations including limiting reactants, theoretical yields and % yields

6. Chapter 4: Reactions in Aqueous Solutions Chapter 4  Electrolytes (classification and example)  Acids, bases, and salts (definition, classifications and examples)  Double displacement and metathesis reactions (definitions and examples)  Solubility tables and net ionic equations  Oxidation and reduction ("redox") reactions  Single displacement reactions and the activity series  Oxidation numbers  Solution concentration: Molarity = moles of solute per liter of solution; M = moles/L  Dilution (V 1 M 1 = V 2 M 2 )  Titrations and related problems

7. Chapter 5: Gases Chapter 5  Kinetic-Molecular Theory  Atmospheric pressure, units of pressure (atm, mm Hg or torr)  Gas laws: Boyle ’ s law, Charles ’ s law, Avogadro ’ s law, Ideal- Gas equation,  Definition of STP conditions  At STP, one mole of any ideal gas occupies 22.41 L  Gas densities and molar mass, Dalton ’ s law of partial pressure,  Kinetic-Molecular Theory, Graham ’ s law of effusion..  Deviations from ideal behavior

8. Chapter 6: Thermochemistry Chapter 6  Energy, kinetic and potential  Units, joules and calories, 1 cal = 4.184 J  First law of Thermodynamics  Internal energy (E),  E = q + w  State functions  Enthalpy (H),  H = q p at constant pressure, exothermic processes (negative  H value) and endothermic processes (positive  H value)  Hess’s law and related problems  Specific heat and heat capacity  H = q = specific heat x grams of substance x  T  Heat = heat capacity x  T  Calorimetry, problems dealing with coffee-cup and bomb calorimeter  Calculating enthalpies of reactions using enthalpies of formation (  H f o )

9. Chapter 7: Quatum Theory and Electronic Structure of Atoms Chapter 7  Electromagnetic radiation  c = wavelength x frequency (c = ln)  Relationship between the energy of radiation and its frequency or wavelength  Planck’s quantum theory, E = hn  Photoelectric effect and the photon  Bohr’s model of the hydrogen atom  Principal quantum number n, E n = -R H (1/ n 2 ), n = 1, 2, 3,.

10. Chapter 7: Quatum Theory and Electronic Structure of Atoms (Cont.) Chapter 7  Electronic transitions,  E = R H (1/n i 2 - 1/n f 2 )  Wave functions and electron density  Quantum mechanical description of orbitals, their shapes and energies  Shells and subshells  Four quantum numbers (n, l, m l, m s )  Pauli exclusion principle and Hund’s rule  Electron configuration and orbital ("box") diagram for different elements

11. Chapter 8: Periodic Relationships Among the Elements Chapter 8  Atomic sizes, ionization energies and electron affinities  The periodic table, groups and periods  Physical and chemical properties of metals, nonmetals, and metalloids  Review of groups 1A, 2A, 6A, 7A, 8A, and hydrogen

12. Chapter 9: Chemical Bonding I: Basic Concepts Chapter 9  Chemical bonding and the octet rule  Ionic bonding, lattice energy, ionic sizes (cations, anions, and isoelectronic ions)  Covalent bonding, Lewis dot structures, formal charges, and resonance  Exception to octet rule, less than an octet (e.g., BF 3 ), "expanded octet" (e.g., PF 5, SF 6 )  Bond dissociation energy and related problems  Electronegativity  Polar and nonpolar covalent bonds

13. Chapter 10: Chemical Bonding II: Molecular Geometry & Hybridization of Atomic Orbiatls Chapter 10  Molecular shape, bond angle and bond length  The VSEPR model  Electron domain (or "pair") geometry (Table: 9.1)  Molecular geometry (distortion due to nonbonding pairs, tables: 9.2 & 9.3)  Polarity in molecules  Valence-bond theory, sigma and pi bonds  Hybrid orbitals (sp, sp 2, sp 3, sp 3 d, sp 3 d 2 )  Molecular orbital (MO) description of covalent bonding

14. Chapter 11: Intermolecular Forces & Liquids & Solids Chapter 11  Characteristic properties of the three states of matter  Intermolecular forces: ion-dipole forces, dipole-dipole forces, London dispersion forces, and hydrogen bonding  Phase changes and dynamic equilibrium  Heating curves and related calculations  Phase diagrams  Structures of solids: Unit cells (primitive cubic, body- centered cubic, face-centered cubic)  Calculating the density of a solid from the type of unit cell and the unit cell dimensions.