|CHM112 Home Page||Reference Materials||Homework Assignments||Lectures||Exams & Quizzes||Grades||Study Aids||URI Home Page|
The following is a list of topics used in CHM 112 that you learned about in CHM 101. You must be able to understand all of these ideas thoroughly and without using a lot of thinking to recall them. Oftentimes the trouble a student has in CHM 112 is rooted in his/her lack of a complete comprehension of CHM 101 material!
While anything covered in CHM 101 may be used in CHM 112, the following list gives some of the ideas used most often.
All page references are to General Chemistry, 4th edition, by J. W. Hill, R. H. Petrucci, T. W. McCreary, and S. S. Perry.
You must know the names and charges of all of the ions in table 2.4. The single most common repeated error in CHM 112 is not keeping track of ionic charges.
Balancing simple reactions must be second nature. This includes writing out the states of matter (g, l, s, aq) for all components in a chemical reaction - chemical reactions that do not include the states of matter are incomplete.
The stoichiometric coefficients in a balanced chemical reaction provide a great deal of useful information about that reaction.
Nearly all of the quantitative problems in CHM 112 use molarity as the concentration unit. Students must be comfortable using molarity units, know how to find molarity of solutions, and be able to find the molarity of solutions that are diluted.
PV = nRT in all its glory.
Enthalpy is one of the important driving forces in chemical reactions.
The distribution of electrons is arguably the single most important concept of the study of chemistry. Lewis dot structures provide one simple method of determining where electrons are located in a molecule.
The combination of electron distribution and electronegativity allows chemists to predict, qualitatively, the regions of positive and negative charge in a molecule or ion. Clues about chemical reactivity are always found in charge distribution.