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Rainbow Fire

Difficulty
Time Required Average (6-10 days)
Prerequisites None
Material Availability Requires specific chemicals; see Materials for more details. For your convenience, a kit is available for purchase at the Science Buddies Store.
Cost Average ($50 - $100)
Safety Adult supervision required. This science fair project involves creating small controlled fires. Make sure you follow all the safety guidelines in the Experimental Procedure.

Abstract

Astronomers can figure out what distant stars are made of (in other words, their atomic composition) by measuring what type of light is emitted by the star. In this science project, you can do something similar by observing the color of flames when various chemicals are burned.

Objective

To investigate the colors produced when different chemicals are burned.

Credits

Andrew Olson, Ph.D., Science Buddies
Justin Spahn, Science Buddies
Sandra Slutz, Ph.D., Science Buddies
Teisha Rowland, Ph.D., Science Buddies

Sources

This science project is based on an entry to the 2007 San Mateo County (California) science fair (author names not published).

Cite This Page

MLA Style

Science Buddies Staff. "Rainbow Fire" Science Buddies. Science Buddies, 25 June 2014. Web. 29 July 2014 <http://www.sciencebuddies.org/science-fair-projects/project_ideas/Phys_p058.shtml>

APA Style

Science Buddies Staff. (2014, June 25). Rainbow Fire. Retrieved July 29, 2014 from http://www.sciencebuddies.org/science-fair-projects/project_ideas/Phys_p058.shtml

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Last edit date: 2014-06-25

Introduction

All matter is made of atoms. Atoms have a nucleus, which consists of protons and neutrons, and is surrounded by electrons. The nucleus is concentrated in a very small space, about 10-15 m. An entire atom is on the order of 10-10 m, so the electrons are relatively far from the nucleus, and, strangely enough, atoms are mostly empty space.

Physicists have found that the electrons traveling around the atomic nucleus can have only certain amounts of energy, called energy levels. In other words, the energy levels of atomic electrons are quantized. If electrons gain energy, they can move from one energy level up to a higher level, but these different energy levels are not continuous—they come in discrete steps. (Watch the animation in Figure 1, below, to see an electron gain energy and move up to a higher energy level.) This fundamental discovery is known as quantum mechanics. Quantum mechanics describes how an atom's electrons interact with electrons of other atoms and with photons.

Animated model of an atomic electron changing energy levels.
Figure 1. In this animation, the red circle represents an atom's nucleus and the blue circle is an electron orbiting around the atom. The black rings are different energy levels the electron can be at. When the electron gains energy (represented by the red arrow going towards the electron), the electron moves to a higher energy level. When the electron loses energy (represented by the red arrow moving away from the electron), the electron moves to a lower energy level. (Animation credits: Kurzon)

Atomic electrons at higher energy levels can also lose energy, dropping down to a lower energy level. (You can also see this in the animation in Figure 1, above.) Again, the electron moves from one allowed energy state to another. The lost energy can be carried away in the form of heat (vibrational energy) or in the form of light—when the electron reverts to a lower energy state, a photon of light is produced. The photon produced will have an energy equal to the difference between the electron's initial high energy state and the later lower-energy state. For visible light, we perceive these differences in photon energy as differences in the color of the light. Because different types of atoms have different gaps between their energy levels, they make light of different colors when their electrons lose energy.

Not only can astronomers use this knowledge to figure out the atomic composition of distant stars, but it can also be used to create fireworks shows. Have you ever watched a fireworks show and wondered how all the different colors — amazing reds, yellows, oranges, blues, purples, greens, and more — are made? The color, or colors, that a firework makes depends on what chemicals are in the firework. These chemicals are various metal compounds that burn when the firework goes off, and burning the compounds is what makes the colors, like the ones shown in Figure 2, below.

Fireworks Show  Lake of Annecy festival 2005
Figure 2. The beautiful colors of fireworks, like the ones shown here, are the result of atomic electrons emitting energy as light. (Image credits: Semnoz)

In this science project, you will use a procedure that is similar to flame photometry or a flame test to observe the color of light produced when various metal compounds are burned. You will need an adult to help you with this experiment, and you will have to perform the experiment extremely carefully so that the flames stay small and under control. What colors will different chemical compounds produce?

Terms and Concepts

  • Atoms
  • Protons
  • Neutrons
  • Electrons
  • Photons
  • Flame photometry
  • Flame test
  • Metals
  • Fireworks
  • Spectral lines

Questions

  • How are the colors produced by a chemical when it burns related to the atomic structure of the chemical?
  • What is flame spectrometry and how is it used by physicists and chemists?
  • How does this science project relate to what astronomers do when they are trying to identify the atomic makeup of a star?
  • In the chemicals used in this science project which elements in the compounds are metals?

Bibliography

Here are some good references to get you started with your background research on spectral lines and flame tests:

Materials and Equipment Product Kit Available

These specialty items can be purchased from the Science Buddies Store:

  • Rainbow Fire kit (1). Includes:
    • Solid fuel tablets (2). These are sometimes alternatively called fire starters or fire starting tinder.
    • Disposable gloves (2 pairs), for handling chemicals
    • Chemical safety goggles
    • Chemicals; 12 grams (g) each of:
      • Copper sulfate
      • Strontium chloride
      • Boric acid
      • Sodium chloride

You will also need to gather these items:

  • White glue (1 small bottle), such as Elmer's
  • Bamboo skewers (12)
  • Masking tape
  • Pen or marker
  • Aluminum foil
  • Matches
  • Hard nonflammable outdoor surface like a sidewalk, driveway, or brick/concrete patio
  • Container of water
  • Heat resistant bowl (1); a soup or cereal bowl would work well
  • Lab notebook
  • Optional: video camera or digital camera and tripod
  • Optional: flashlight

Order Product Supplies

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Project Kit: $59.95

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Experimental Procedure

Safety Note: This experiment requires adult supervision. Do not breathe in dust from the chemicals and wear gloves when handling them to prevent contact with skin. Also avoid breathing combustion fumes from this experiment.

The results will be most clear in the dark. We suggest performing this science experiment outside in the evening on a nonflammable surface like brick, concrete, cement, or other driveway surface. Make sure that there are no flammable materials nearby. Be prepared for an emergency with a container of water. A fire extinguisher would also be a fine alternative.

Preparing the Chemical Skewers

  1. Do your background research so that you are knowledgeable about the terms, concepts, and questions, in the Background section.
  2. Have an adult present when you do the experiment, and follow all of the safety precautions, above.
  3. Several hours before sunset (a day or more is also fine), prepare the bamboo skewers. You will be making 3 skewers per chemical.
  4. Put a piece of masking tape around the blunt end of each skewer (a total of 12 skewers) like a flag as seen in Figure 3, below. With a pen, write the name of a chemical on each skewer's masking tape label.
    1. In the end you should have 3 skewers labeled for each chemical.
science kit chemical covered skewer for flame test Physics science project
Figure 3. A completed skewer is shown here. Notice the masking tape label at the blunt end, and the copper sulfate coating approximately 1 inch of the tip.
  1. Apply a thin layer of glue to the last 2 to 3 centimeters (cm) of the tip of a skewer as shown in Figure 4, below.
    1. Just a little bit of glue is enough.
    2. You can squeeze the glue directly from the glue bottle onto the skewer.
creating chemical covered skewer for flame test Physics science project
Figure 4. Cover approximately 2 to 3 cm of the tip of each skewer with a small amount of glue. Make sure the glue is on all sides of the skewer.
  1. While wearing the chemical goggles and disposable gloves, dip the glue-coated tip end of the skewer in the jar of chemical. Twist the skewer back and forth a bit to coat the skewer with the chemical.
    1. Make sure the name of the chemical on the skewer label is a match for the chemical you are using.
    2. If you are not using the Science Buddies kit you may need to put your chemicals into vials or small ziplock bags to do this step. The Science Buddies Kit chemical jars are just the right size to coat the skewer in.
  2. Repeat steps 5 and 6 until you have made 3 skewers for each of the chemicals.
  3. Let the skewers dry for at least two hours before performing the flame tests.

Conducting the Flame Tests

  1. The flame test should be conducted outside, in the dark (or at twilight), on a hard nonflammable surface. Adult supervision is needed.
  2. Find a hard nonflammable surface outside for the flame test. A driveway, sidewalk, or brick/concrete/cement patio are all examples of a good testing surface.
  3. Bring the dried chemical skewers (make sure they have dried for at least two hours first) and all other materials outside. You may find it easiest to use a flashlight or other outdoor light while you are getting set up. When you are done setting up and ready to test the skewers make sure to turn off the light(s).
  4. Place a solid fuel tablet on a square of aluminum foil on your nonflammable surface as shown in Figure 5, below.
science kit flame test with chemicals
Physics science project
Figure 5. Outside on a nonflammable surface is the ideal place to conduct your flame test. For easy cleanup make sure to but your solid fuel tablet on a square of aluminum foil.
  1. As a safety precaution make sure to have a container of water with you. A fire extinguisher would be a fine alternative. If you are using a video camera, start recording.
  2. Have an adult use a match to light the solid fuel tablet. You may find that laying the lighted match on the foil next to the tablet is the easiest way to get the tablet to start burning. Note the color of the flame in your lab notebook. If you are using a digital camera to document your experiment, take a picture of the burning tablet.
  3. Once the solid fuel tablet is burning, carefully take a skewer and hold the chemical coated end in the flame. Be sure not to breathe the fumes or smoke from the burning skewer. Observe the flame color and record it in your lab notebook. Take a photo if you are using a digital camera for documentation.
    1. Tip: You may be able to see the color in the tablet's flame, or by holding the skewer away from the candle (once the chemical has caught on fire) and looking at the flame on the chemical-coated end of the skewer.
    2. The skewer may also catch fire after a few moments. Simply remove it from the flame and blow it out like a birthday candle. You can also extinguish the skewer in the container of water.
  4. Repeat step 7 for all 12 skewers (3 per chemical). Record all your observations in your lab notebook.
  5. When you are done either wait for the solid fuel tablet to burn itself out or extinguish it by carefully putting a heat resistant bowl over the tablet, as shown in Figure 6, for a few minutes.
science kit flame test cleanup
Physics science project
Figure 6. The solid fuel table will burn itself out in under 20 minutes. If you do not want to wait, you can extinguish it by covering it with a heat resistant bowl for 1 minute. This will deprive the fire of oxygen thus causing the flame to go out.
  1. When you are sure everything has been extinguished, you can dispose of the aluminum foil, used chemical coated skewers, and spent fuel tablet in the garbage.
  2. What colors were produced as each chemical burned?
  3. Sodium chloride (table salt) and strontium chloride both have chloride, but have a different metal (sodium vs. strontium). Are the flame colors produced by these two compounds similar or different? What does this tell you about the source of the color?

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Variations

  • You could try this science project using other metal compounds known to produce certain flame colors when burned. Check out the resources in the Bibliography section in the Background for some ideas on how to do this. Be sure to always look into and follow all proper safety precautions when handling and burning different chemicals. What colors do other metal compounds make when burned?

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Ask an Expert

The Ask an Expert Forum is intended to be a place where students can go to find answers to science questions that they have been unable to find using other resources. If you have specific questions about your science fair project or science fair, our team of volunteer scientists can help. Our Experts won't do the work for you, but they will make suggestions, offer guidance, and help you troubleshoot.

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Contact Us

If you have purchased a kit for this project from Science Buddies, we are pleased to answer your questions.

In your email, please follow these instructions:
  1. What is your Science Buddies kit order number?
  2. Please describe how you need help as thoroughly as possible:

    Examples

    Good Question I'm trying to do Experimental Procedure step #5, "Scrape the insulation from the wire. . ." How do I know when I've scraped enough?
    Good Question I'm at Experimental Procedure step #7, "Move the magnet back and forth . . ." and the LED is not lighting up.
    Bad Question I don't understand the instructions. Help!
    Good Question I am purchasing my materials. Can I substitute a 1N34 diode for the 1N25 diode called for in the material list?
    Bad Question Can I use a different part?

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