The Color Spectrum Lab Step 1: Make an observation

The Color Spectrum Lab
Step 1: Make an observation
Ions within the ionosphere react with ultraviolet radiation produce the aurora effect.
Step 2: Ask Questions
1. What characteristic colors will be produced by various metallic ions?
2. What test will we use to determine the metal ions?
Step 3: Create a Hypothesis
If energy in the form of a flame is used to test metallic ions, then________________________________
Step 4: Conduct an Experiment
1. What safety precautions should we take?
2. What will our independent variable be?
3. What will our dependent variable be?
4. How will we clean the spatula to avoid contamination?
7 small test tubes filled (and label) with the following solutions:
o 15ml Sodium chloride
o 15ml Potassium chloride
o 15ml Lithium chloride
o 15ml Calcium chloride
o 15ml Strontium chloride
o 15ml Copper (II) chloride
o 15ml Barium chloride
1 small beaker filled with 30mL of acid
Expo marker- to label test tubes
Bunsen Burner
Rubber tubing
Safety goggles
Gather and check all materials and lab equipment.
Place 7 test tubes in holder and on your lab bench away from flame.
Dip spatula into one of the solutions, completely immersing the tip.
Hot spatula over flame and observe the color change.
Turn down the lights if needed. Record data.
a. All flames will start out blue in color or invisible but will change to the colors
characteristic of the metal salts.
b. The copper chloride will begin to burn after a few minutes. Be sure thoroughly
extinguish this fire with water.
Dip the spatula into the acidic solution.
Repeat steps 3-6 for the remaining 6 solutions.
Clean up lab station, turn off burner and see Mrs. Dawson for discard instructions.
Have lab station checked by TA or Mrs. DAwson
Step 5: Record Data
Chloride Solution
Sodium chloride
Potassium chloride
Lithium chloride
Color of Flame
Calcium chloride
Strontium chloride
Copper (II) chloride
Barium chloride
Step 6: Conclusion:
1. How does this experiment relate to Earth Science?
2. When an element or compound is placed in a burning solution, the atoms absorb energy and
promote electrons to “excited” energy levels, which are different from their normal ground
state. Explain how this creates colored light.
3. What is the name of this spectrum of specific wavelengths produced by exciting an element?
4. Why is the spectrum different for every element?