SYLLABUS FOR CHEMISTRY I
Science Skills and Attitudes, Applications, and Contexts of Chemistry
Observation. Exploratory activities. Identification of variables. Development of problem statements. Types of investigation designs. Hypotheses. Independent (manipulated) and responding (dependent) variables. Quantification of variables. Experimental control. Analysis. Collection and organization of data. Qualitative and quantitative data. Interpretation of experimental data using mathematics and statistics. Conclusions. Analysis of conclusions. Identification, function, care, and use of scientific equipment. Accurate measuring. Safety precautions and procedures.
Beneficial and detrimental effects of discoveries made by chemists. Advantages and disadvantages of traditional and alternate energy resources such as, fossil fuels, nuclear energy, solar energy and energy efficiency/conservation projects. Chemistry of air pollution for phenomena such as, acid rain, ozone depletion, and global warming. Diversity of experimental results interpretation. Reproducibility of experimental results. Research and career opportunities in chemistry. Contributions of physical science researchers from various ethnic and cultural backgrounds. Importance of continuous development and sharing of scientific information.
Atomic Theory and The Periodic Table
Electron configurations/orbital diagrams for elements or monoatomic ions. Rutherford's, J. J. Thompson's, Bohr's and Planck's experiments and their implications for the structure of the atom. Relationship among the period table and: atomic size, ionic size, ionization energy, electron affinity, metallic character, electronegativity. Prediction of type of bonding between two elements based on the location of those elements on the periodic chart. Types of bonds (ionic, covalent, metallic) and intermolecular forces (Van der Waal and hydrogen). Properties of a substance based on its bond type. Electron dot (Lewis) diagrams for ions or molecules.
Chemical Reactions and Calculations
Nomenclature and formula for inorganic or organic
compounds. Balance specific reactions as composition, decomposition,
replacement, ionic, or acid/base. Balance chemical equations. Law of
conservation of matter. Moles in terms of volume, mass, or number of particles.
Stoichiometric problems using mass/mass and volume/volume relationships.
Calculation of empirical and molecular formulas based on percent composition and
vice versa. Distinction between strength and concentration of acids and bases.
pH. Conductivity. Arrhenius and Bronsted/Lowery definitions of acids and bases.
Classification of compounds in chemical reactions. Estimation of pH from
concentration data. Concentration of an acid or base from titration data.
Definition of oxidation, reduction, oxidizing agent, reducing agent, oxidation
number, and half reaction. Applications of this definitions to selected reactions
Factors Affecting Chemical Reactions
Effects of temperature, concentration and surface area on the rate of reaction. Plotting potential energy diagrams of catalyzed and uncatalyzed chemical reactions. Calculation of activation energy and heat of reaction. Classification of reactions as exothermic and endothermic based upon enthalpies of formation. Conditions in a chemical reaction that lead to increased entropy.
Physical Changes
Application of the primary assumptions of the kinetic molecular theory to the behavior and properties of gases, liquids, and solids. Qualitative description and quantitative application of the relationships among pressure, temperature, volume, and the number of moles of gases. (Boyle's Law, Charles' Law, Dalton's Law, Avogadro's Law, and Ideal Gas Law). Relationship between entropy and changes in the state of matter. Analysis of a solution process in terms of intermolecular forces and entropy.
Solution of specific heat problems. Plotting temperature versus time graph for a phase change. Enthalpy problems based laboratory investigations (heat of combustion, heat of formation, heat of solution. heat of vaporization, heat of fusion). Solubility in terms of the effect of temperature, pressure, and solvent selection. Concentration of solutions expressed in molarity and molality. Freezing point depression and boiling point elevation.
Nuclear Reactions
Balance of nuclear transmutation equations. Half-life of various nuclear wastes. Solutions for their storage.