CHEMISTRY, PART 2

In this module, students gain a comprehension of the following:

• The significance of coefficients in a balanced equation, molar ratios, mole-mole calculations, mass-mass calculations and other stoichiometric calculations. 
• To solve Limiting Reactant stoichiometry problems as well as how to determine the excess reactant.
• The difference between actual, theoretical and percent yields with examples of how to calculate theoretical and percent yields.
• The concepts of solutions and solubility. The chemical structure of water, and why water is so important for life. 
• How and why water acts as a wonderful solvent and provides a medium for metabolism. 
• The various factors that affect how well a solid-liquid solute dissolves, including Particle Size, Temperature, Agitation and the Chemical Nature of the solute, particularly polarity (Like dissolves like.) 
• To interpret solubility curves and read solubility curves. 
• To identify and understand saturated, unsaturated and supersaturated solutions. 
• Colligative properties, freezing point depression and boiling point elevation. 
• The relationship between amount of solute and degree of freezing point depression-boiling point elevation.
• The general properties of acids and bases. Including the Arrhenius definitions for acids and bases. Bronsted and Lowry’s theory of acids and bases. 
• To distinguish between strong and weak acids and bases in terms of the extent of dissociation, reaction with water and electrical conductivity. 
• The pH scale and to consider the effects of acid deposition on limestone buildings and living things.To understand the nature of a strong acid and a strong base. To solve acid-base titration math problems.
• The nature of gases as related to the study of Chemistry. 
• The assumptions behind the Kinetic Molecular Theory and some general properties of gases from a molecular perspective. Avogadro’s Law, Boyle’s Law, Lussac’s Law and Charles’ law. 
• How the ideal gas equation allows one to find the pressure, volume, temperature and/or number of moles in a certain situation.
• To measure and consider the rate of a reaction. 
• The connection between concentration and reaction rate in terms of the Law of Mass Action and Rate Laws. 
• The equilibrium constant (K,) and how it can be calculated in various reversible reactions. Le Chatelier’s Principle and how it predicts changes in concentration when “stressing” reactions at equilibrium.
• Nuclear structure and stability, radioactive decay, and nuclear energy. As well as, the biological effects of radiation as well as technology related to energy, medicine, geology, and other areas.
• Organic chemistry – why the element carbon results in such a variety of compounds, how those compounds are classified, and the role of organic compounds in biology and industry.