Color Light Lab Results
Each element emits a unique color light. The purpose of this experiment was to observe these unique colors and calculate their energy. In order to observe this, we placed the physical elements in a 24 well plate, dipped wet q-tips into the wells to gather the element, and put it over the bunsen burner to observe the flame emitted. While observing the different flames, we saw that different elements did indeed emit unique flame colors. Colors such as red, violet, and turquoise were emitted. All of these represented the different energy emitted when the electron changes energy levels. We concluded that potassium had the highest energy emitted. Some sources of error include the q-tip affecting the flame emitted. Also, when calculating the unknown
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material #1, both orange and red flames were emitted, so we took the average of those two colors to calculate the energy, this could be considered an error.
2. INTRODUCTION
When a substance is heated in a flame, the atoms absorb energy from the flame.
This excites electrons causing them to gain energy. As the electrons gain energy they are moved into higher energy levels. Naturally, electrons want to move back to their original state. As the electrons move down from higher energy levels, a photon is emitted. A photon is a particle of light. The absorption of energy, and the energy of the energy emitted is quantized. Electrons can take one big step as it reaches its base state and release one photon. Electrons could also take many little steps as it travels to its base state, emitting a photon at each level. To determine the energy of the emitted photon we have to look at the difference in energy of the excited state and the relaxed state. This energy determines the light emitted.
In this experiment we are trying to observe this amazing phenomenon. Heating up different elements using a flame, we are able to see the change in states and the emitted photons. In the process we will try to answer questions such as: how does the amount of energy absorbed by electrons affect the color of light produced? What does the light produced tell us about the energy of the emitted photon? What has more energy, a photon that takes one big step, or photons that take many steps? Our objective is to observe the unique color of light emitted by each element, and determine the
energy.
3. Materials and Procedure
First, we collect small sample amounts of each “known” chemical in a 24-well reaction plate, making sure we knew which solid was which. Then we half-filled a beaker with distilled water, and placed the soaked in one of the beakers. Next, we lit the bunsen burner so it had the correct “blue” colored flame. Dip a soaked Q-tip into one of the wells holding copper chloride. Hold the chemical end of the Q-tip on the extreme edge of the flame of the bunsen burner. Then move it back and forth through the flame. After you have completed this, record the flame color that you observe in the results table. Last, extinguish the Q-tip in the other beaker with water. Repeat steps 1-6 for sodium chloride, potassium chloride, calcium chloride, strontium chloride, lithium chloride, barium chloride, and the 2 unknown solids.
material #1, both orange and red flames were emitted, so we took the average of those two colors to calculate the energy, this could be considered an error.
2. INTRODUCTION
When a substance is heated in a flame, the atoms absorb energy from the flame.
This excites electrons causing them to gain energy. As the electrons gain energy they are moved into higher energy levels. Naturally, electrons want to move back to their original state. As the electrons move down from higher energy levels, a photon is emitted. A photon is a particle of light. The absorption of energy, and the energy of the energy emitted is quantized. Electrons can take one big step as it reaches its base state and release one photon. Electrons could also take many little steps as it travels to its base state, emitting a photon at each level. To determine the energy of the emitted photon we have to look at the difference in energy of the excited state and the relaxed state. This energy determines the light emitted.
In this experiment we are trying to observe this amazing phenomenon. Heating up different elements using a flame, we are able to see the change in states and the emitted photons. In the process we will try to answer questions such as: how does the amount of energy absorbed by electrons affect the color of light produced? What does the light produced tell us about the energy of the emitted photon? What has more energy, a photon that takes one big step, or photons that take many steps? Our objective is to observe the unique color of light emitted by each element, and determine the
energy.
3. Materials and Procedure
First, we collect small sample amounts of each “known” chemical in a 24-well reaction plate, making sure we knew which solid was which. Then we half-filled a beaker with distilled water, and placed the soaked in one of the beakers. Next, we lit the bunsen burner so it had the correct “blue” colored flame. Dip a soaked Q-tip into one of the wells holding copper chloride. Hold the chemical end of the Q-tip on the extreme edge of the flame of the bunsen burner. Then move it back and forth through the flame. After you have completed this, record the flame color that you observe in the results table. Last, extinguish the Q-tip in the other beaker with water. Repeat steps 1-6 for sodium chloride, potassium chloride, calcium chloride, strontium chloride, lithium chloride, barium chloride, and the 2 unknown solids.