Element Collection

Element Collection

Wednesday, March 31, 2010

Experiment: Chemical Color Changer

A video of this reaction can be seen here.

This experiment is a simple way of making a solution that changes color on its own through purple, blue, green, and yellow. I decided to try something different for this one - it doesn't end in fire! It's still pretty interesting though, and actually very easy to do with relatively common ingredients. All you need is water, sugar, sodium hydroxide (NaOH, also called lye, a cleaner), and potassium permanganate (KMnO4, a disinfectant and water treatment chemical).

Monday, March 29, 2010

Experiment: Silicon Dioxide Thermite

This old post serves as the Video Companion to  this video. This reaction was done some time before the video was shot, so some conditions here were a bit different (e.g. the ignition method).

This one was one of my favorite experiments to date. The silicon dioxide I used was common beach sand. I picked it up off the ground from Panama City Beach, ground it down to a finer powder in a mortar and pestile, and mixed it into thermite. This composition is extremely hard to ignite, so I added sulfur as well. This sets up a helper reaction between sulfur and aluminum that burns hot enough to sustain the rest of the thermite. The ratio I used was 9:12:10 SiO2:S:Al. This experiment was done when I was trying out different ignition methods, so here I used "thermite ignition mixture" from www.unitednuclear.com (my favorite science supplier), which was ignited with an M-80 fuse.

Sunday, March 28, 2010

Experiment: Black Iron Oxide Thermite

Thermite is most commonly made with red iron oxide (hematite, or common rust), but I went with black iron oxide (magnetite) because it should yield more metal per reaction. The ratio for this is 3.22:1 Fe3O4:Al by weight.

Full reaction: 8Al + 3Fe3O4 -> 9Fe + 4Al2O3

Saturday, March 27, 2010

Experiment: Manganese Dioxide Thermite

This old post serves as the Video Companion to  this video.

For this experiment, I used manganese dioxide and a much finer aluminum powder than in my other thermites, at a ratio of 2.42:1 MnO2:Al by weight (40g total). I've done this reaction before (but forgot to photograph it), and using my normal aluminum it produced a reaction similar to the iron thermite. It was a little brighter and produced more sparks. With the finer powder, things went a little differently. The small flower pot erupted in a pillar of flame about 6 feet high, with the sound of a rocket engine and heat that was felt a good 15 feet away. This is a great demonstration of the importance of particle size in thermite and most other reactions. I plan on posting a direct comparison, complete with pictures, sometime in the future.

Friday, March 26, 2010

Background: Thermite

One of the first experiments I did at my home lab, and the type I've done most often, is the thermite reaction. This is the exothermic reaction between a powdered metal oxide and a pure metal, most commonly between iron oxide and aluminum. The strength of the reaction can be determined by how far apart the two metals are in the Activity Series. For example, a copper oxide thermite should be more violent than a chromium oxide one since copper is farther from aluminum on the series than chromium (and it is, by a lot). Thermite involves a single-replacement reaction, where the more reactive aluminum replaces the other metal in its oxide, resulting in alumina (aluminum oxide) and the pure metal. The reaction is hot enough to occur in the liquid stage, so the products are generally in one solid lump after cooling. Thermite is used in some welding applications, and was used in special grenades in the military.

Wednesday, March 24, 2010

The Home Scientist: About

Welcome to The Home Scientist!

I created this blog to document and share my scientific experiments with anyone that cares to read about them. This all started with my decision to start an element collection. I'm collecting samples of every element from the periodic table that is obtainable. That leaves me with 92 elements, from Hydrogen to Uranium. Some are common around the house, some can be bought online, and others can be obtained through chemical reactions. The last is what prompted me to build my home laboratory, and the desire to document my experiments lead me to make this blog. It might have been boring in school, but I bet your chemistry class never did stuff this cool.

Also, I hope that by sharing my experiences I can get people interested in science. Sometimes the school system presents the material as too mathematical or not as fun as it can be, and kids lose interest. The fun of all science, and chemistry in particular, is in my opinion all in the experiments. Science is all about curiosity and the drive to know just how the world works, and getting kids interested early on will, if nothing else, help to open their eyes to see the wonders of the universe we live in.

With all that said, I have to put a disclaimer for anything you see on this site. Everything I do at my home, you probably shouldn't do at yours. I have years of education in laboratory safety and practices, and have worked with chemicals in three different research labs. While I'm not discouraging other people's own scientific pursuits, I have to emphasize that you exercise extreme caution and wear proper safety gear if you ever do anything like what I do.

So enjoy reading, please comment and become a follower, and again welcome to The Home Scientist!