The syllabus lists the test dates, and the chapters which will be covered this semester.

A great deal of chemistry simplifies to the attraction of one charge for an opposite charge. We finished last semester with a discussion of bonding; molecules are held together by the attraction of one atom's elections, negative charge, to another atom's nucleus, positive charge. This semester we will start with a dicussion of intermolecular forces; molecules are attracted to other molecules by the attraction of one one charge to an opposite charge. In general, all intermolecular attractions boil down to the interaction of one dipole with another. However, all of the intermolecular interactions are not referred to as "dipole-dipole" interactions. Phase changes, metling points or boiling points for example, are are strongly influeneced by the strength of the intermolecular forces between the molecules.

We are going to look at three cubic crystal structures. These pages use Java (specifically, ChemApp a java application created by gpurvis@ix.netcom.com) and the Chemscape Chime plug-in. If you are using a Macintosh Java works best with Internet Explorer 4.5 and MRJ 2.1; Netscape's implementation of Java is very pokey (Netscape 5.0 should address this issue.) However, for both Mac and Windows Chime works best with Netscape.

From Intermolecular forces and how they relate to phase changes in pure solids, liquids, and gases we jump to the behavior of solutions. The freezing and boiling points of solutions differ from those of the sovent in a very predictable manner.

An important part of any reaction is the speed at which the reaction occurs. Rocket fuels release a great deal of energy, but the rate at which the reaction proceeds is very important. That faster the reaction the larger the thrust produced by the rocket. Industrially, the faster the product can be produced the faster it can be sold. Rates can be described using diferential rate laws or integral rate laws. The difference is that differential rate laws relate the rate at which the reactants are consumed to the concentration of the reactants, and integral rate laws relate the amount of time required to reach a certain reactant concentration from an initial state.

Svant Arrhenius derived an expression to explain reaction rates on the basis of molecular collisions. According to Arrhenius's theory only a certain number of molecules have enough energy to succesfully undergo a reaction. The Energy barrier that these molecules must overcome is refered to as the Activation Energy for the reaction.

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