Objectives:

Chapter 1:

1. Distinguish between physical and chemical properties and also between simple physical and chemical changes.
2. Differentiate between the three states of matter.
3. Distinguish between elements, compounds, and mixtures.
4. You should be able to list the basic SI and metric units and the commonly used prefixes in scientific measurements.
5. Determine the number of significant figures in a measured quantity.
6. Express the result of a calculation with the proper number of significant figures.
7. Convert temperatures among the Fahrenheit, Celsius, and Kelvin scales.
8. Perform calculations involving density.
9. You should be able to convert between units by using dimensional analysis.

Chapter 2:

1. Describe the composition of an atom in terms of protons, neutrons, and electrons.
2. Write the chemical symbol for an element, having been given its mass number and atomic number, and perform the reverse operation.
3. Describe the properties of the electron as seen in cathode rays.
4. Describe Millikan's oil-drop experiment and indicate what property of the electron he was able to measure.
5. Cite the evidence from studies of radioactivity for the existence of subatomic particles.
6. Write the symbol and charge for an atom or ion, having been given the number of protons, neutrons, and electrons, and perform the reverse operation.
7. Use the periodic table to predict the charges of monatomic ions and whether an element is a metal or a nonmetal.
8. Distinguish between empirical formulas, molecular formulas, and structural formulas.
9. Write the simplest formula for a compound, having been given the charges of the ions from which it is made.
10. Write the name of a simple inorganic compound, having been given its chemical formula, and perform the reverse operation.

Chapter 3:

1. You should be able to balance chemical equations.
2. Predict the products of the combustion reactions of hydrocarbons and simple compounds containing C, H, and O atoms.
3. Calculate the atomic weight of an element given the abundances and masses of its isotopes.
4. Calculate the molecular weight and molar mass of a substance from its chemical formula.
5. Interconvert number of moles and mass of a substance. Use Avogadro's number and molar mass to calculate the number of particles making up a substance, and vice versa.
6. Calculate the empirical formula of a compound, having been given appropriate analytical data such as elemental percentages or the quantity of CO2 and H2O produced by combustion.
7. Calculate the molecular formula, having been given the empirical formula and molecular weight.
8. Calculate the mass of a particular substance produced or used in a chemical reaction.
9. Determine the limiting reagent in a reaction.
10. Calculate the theoretical and actual yields of chemical reactions given the appropriate data.

Chapter 4:

1. Predict whether a substance is a nonelectrolyte, strong electrolyte, or weak electrolyte from its chemical behavior.
2. Predict the ions formed by electrolytes when they dissociate or ionize.
3. You should be able to identify substances as acids, bases, or salts.
4. Use solubility rules to predict whether a precipitate forms when electrolyte solutions are mixed.
5. Predict the products of metathesis reactions (including both neutralization and precipitation reactions) and write balanced chemical equations for them.
6. Identify the spectator ions and write the net ionic equations for solution reactions, starting with their molecular equations.
7. Determine whether a chemical reaction involves oxidation and reduction and assign oxidation numbers to atoms in molecules and ions.
8. Calculate molarity, solution volume, or number of moles of solute given any two of these quantities. [ n = MV ]
9. Calculate the volume of a more concentrated solution that must be diluted to obtain a given quantity of a more dilute solution. [ M1V1 = M2V2 ]
10. Calculate the volume of a solution required to react with a volume of a different solution using molarity and the stoichiometry of the reaction.
11. Calculate the amount of a substance required to react with a given volume of a solution using molarity and the stoichiometry of the reaction.
12. Calculate the concnetration or mass of solute in a sample from titration data.

Back To Top | Home | Objectives | Reading Materials | Addtional Problems | Experiments | Practice Exams | Videos

Late Update: Wednesday, January 25, 2012 2:41 PM