This new chemistry course is completely different from the previous one I wrote, Exploring Creation with Chemistry, 2nd Edition. It covers the standard college-prep chemistry topics in a different order, but more importantly, it emphasizes aspects of those topics in a way that makes them more relevant to this decade. For example, when discussing Dalton’s Atomic Theory, I point out that he used his theory to predict something about the masses of two elements that can react to form completely different compounds. That prediction was later confirmed, and we now call it “The Law of Multiple Proportions.” I point out that a theory can’t be considered scientific unless it can make such predictions. I then discuss this in the context of creation science. I talk about how the scientific theory of creation has been used to make many successful predictions, including the fact that there is very little “junk DNA” in the human genome.
The most important difference between the courses, however, is the experimental component. When I wrote the older course, I had the students perform the best experiments they could with reasonably-priced equipment. Since that book was written, however, the cost of certain chemistry equipment, such as precise mass scales, has gone down significantly. As a result, what is available at a reasonable price today is quite different from what was available back when the old course was written. Because of this, the experiments are significantly better in this new course.
For example, there are certain chemicals that tend to incorporate water into their solid phase. We call them hydrates. Consider the picture below:
You might think these are two different compounds, but they are not. Both jars contain cobalt (II) chloride. The reason they look different is because the solid on the left has no water in it. As a result, we call it the anhydrous form of cobalt (II) chloride. The solid on the right has water in it, so we call it the hydrated form of cobalt (II) chloride. Both solids perform exactly the same chemistry. The only difference between them is the presence of water.
Now don’t make the mistake of thinking that the water is chemically bonded to the cobalt (II) chloride. It is not. If you heat the hydrated form of cobalt (II) chloride, the water will simply evaporate, producing the anhydrous form. In other words, if you heat the purple solid, it will slowly turn blue as the water evaporates from it.
In my new chemistry course, students do this experiment with copper (II) sulfate. The kit that comes with the course contains the hydrated form, which is blue. The students measure the mass of a sample of this hydrated copper (II) sulfate, and then they heat it. As time goes on, the blue hydrated form turns into a white powder, which is the anhydrous form of copper (II) sulfate. Once the sample is completely white, they measure the mass again and see that it has decreased. Why? Because water has evaporated from the sample. The students use that change in mass to actually calculate how many molecules of water are incorporated into the solid for each ion in the sample! They then add water to the white powder and watch it change back into the blue solid with which they started the experiment.
Students can do an experiment like this at home (or at a small, private school) because inexpensive digital mass scales that have a precision of 0.1 grams have been produced. One of those scales is in the $70 kit that comes with the course, and as a result, students can do some really incredible experiments. In addition to the one I just discussed, for example, they can determine the amount of sodium bicarbonate in an Alka-Seltzer tablet (or any other effervescent tablet).
There are other really great experiments in the course as well. For example, students look through a feather at a light bulb that is a couple of meters away from them. When they do that, they see multiple images of the light bulb, and each image has a rainbow attached to it. This is because the light waves interfere with one another as they pass through the thin slits between the barbules of the feather. In addition, students use steel wool to see that even metals can burn, and they do an experiment which demonstrates that a catalyst is not used up when it changes the rate of a reaction. There are a total of 46 experiments in the year-long course, which gives the students significantly more laboratory experience than most students would get in a public school.
I will close with comments made by two of the people who reviewed the course. The first comes from a scientist who did peer review prior to publication. After finishing his review, Dr. Richard S. Pottorf (who is on the faculty of Anderson University) says:
Discovering Design with Chemistry is a great read for the new chemistry student. Dr. Wile’s descriptions of chemical principles are very easy to understand and are backed up with experiments that aid the high school chemistry student in grasping these chemical principles. Additionally, Dr. Wile exhibits excitement that should capture the student’s attention.
A refreshing theme is Dr. Wile’s use of chemistry to illustrate the design that exists in God’s Creation. The short descriptions of several of our great scientists and how their faith has affected their work is a wonderful addition to this subject.
I wholeheartedly recommend this book for the student who desires a college-preparatory high school chemistry course.
The second comes from one of my former university students, Nancy Dalton (no relation to the Dalton discussed above). She was able to achieve a perfect score in the chemistry course I taught last fall. Because of her outstanding work, I asked her to review all of the problems in the course while it was being written, looking for any errors I made. She found several, and they were corrected before the book went to press. After she was done, she was kind enough to write:
Having been taught by Dr. Wile as a professor at the university level, I can still experience his voice and his excitement for the subject of chemistry throughout his writing. His easy, personal writing style made me feel at ease as I ventured through the text. Most of all, his faith is weaved throughout the chemistry content in challenging and authentic ways. I can tell his chief desire is to share with his students the glory of our Creator through studying world around us.