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- Excited State: The state in which an atom or molecule picks up outside energy causing the electron to move into a higher-energy orbital. Questions: 1. Why is it important to test the flame color of the methanol without any compounds dissolved in it?...
- List the colors observed in this lab from shortest wavelength to longest wavelength. What is the relationship between energy, frequency, and wavelength? The relationship between energy and frequency is that when the frequency of a wave increased the...
- The sun is related because the electrons are constantly being heated, going to excited state, dropping down to ground state, and then letting out the absorbed energy into light. Can you think of a way in which to use the flame test? Please describe below. You can use the flame test to create fireworks. You can use the different compounds to make different colors and this would create a firework show. This taught us how the light is emitted, how each compound reacts differently, and the observations we made. The purpose of this lab was to allow us to observe compounds and how they react to an energy in different ways.
- This happens because every metal has a different bright line spectra. Table 2 shows that you can identify a metal in a compound by using a flame test. The metal in the compound was identified by the light orange color seen during the flame test. Table 1 proves my hypothesis to be correct. Conclusion- The purpose of this lab was to see what colors are characteristic of particular metallic ions in a flame test and use their characteristic color to identify other elements. Another purpose was to understand how fireworks work. This experiment can help to identify elements in space to help scientists know whether a planet has oxygen or not. It can also help one determine what metal to use in fireworks to portray a certain color. The experiment was conducted by burning a salt and recording the color of the flame.
- This experiment showed that every metal emits a different color and this proves the hypothesis to be correct, that every metal emits a different color when put into a flame. This experiment also shows that a metal can be identified by looking at the color of the flame and matching it to previous data results. This also proves my hypothesis to be correct. Table 1 and Table 2 prove both of my hypotheses to be correct. More experiments can be done with machines to find the exact wavelengths of light for every element. If the exact wavelengths can be found, it would be easier to identify elements with a flame test. Possible sources of error in this experiment were that the nichrome wire may not have been fully cleaned off every time, the color might have looked different because of other light sources, and there could have been particles in the bottom of the Bunsen burner.
- Acknowledgments: The author of this paper thanks Union Springs High School for use of their facilities to conduct this experiment with. Cite this page.
- Flame Test Lab: Introduction to the Flame Test Lab: The Flame Test lab was an in-class lab where we tested chemicals in the flames to see the wide range of colors in the color spectrum. The secondary purpose of the lab was to identify unknown compounds that we would test and then guess as to what they were. The Flame Test lab was done in several parts.
- The first one that I will focus on is the Pre Lab questions: Pre Lab questions: This is a replication of the article used in the pre lab: Introduction By placing atoms of a metal into a flame, electrons can be induced to absorb energy and jump to an excited energy state, a quantum jump. They then return to their ground state by emitting a photon of light the law of conservation of energy indicates that the photon emitted will contain the same amount of energy as that absorbed in the quantum jump. The amount of energy in the photon determines its color; red for the lowest energy of visible light, increasing energy through the rainbow of orange, yellow, green, blue, indigo, and finally violet for the highest energy of visible light. Photons outside the visible spectrum may also be emitted, but we cannot see them.
- The arrangement of electrons in an atom determines the sizes of the quantum jumps, and thus the energy and colors of the collection of photons emitted, known as emission spectrum. In this way the emission spectrum serves as a "fingerprint" of the element to which the atoms belong. We can view the emission spectrum of colors all at once with the naked eye. It will appear to be one color, which we will carefully describe. A flame test is a procedure used to test quantitatively for the presence of certain metals in a chemical compounds. When the compound to be studied is excited by heating it in a flame, the metal ions will begin to emit light. Based on the emission spectrum of the element, the compound will turn the flame a characteristic color.
- This technique of using certain chemical compounds to color flames is widely used in pyrotechnics to produce the range of colors seen in a fireworks display. In this lab, we will record the flame test color of several metals by making solutions of salts, or ionic compounds, of those metals then igniting them with a match. We will observe the separate colors of the emission spectra, as the solution burns. If time permits, we will also compare the flame tests of crystals of a compound with that of a solution of the same compound. Background: The electrons in an atom occupy different energy levels, as you know.
- When all of the electrons are at the lowest possible energy level they are said to be in the ground state. Electrons do not always stay in the ground state. Sometimes they can be promoted to a higher-energy electron shell. This can happen in two ways. First, the electron can absorb a photon of just the right amount of energy to move it from one quantum shell to another. Second, when atoms are heated their electrons can gain energy from the heat. This promotes them to the higher-energy shell. When an electron is in a higher-energy shell it is said to be in an excited state.
Flame Test – Flame Test Lab Report Answers – Lab Report Sample
Electrons in excited states do not usually stay in them for very long. When electrons lose their energy they do so by emitting a photon of light. Photons are particles with energy but no mass. The photons emitted precisely match the quantum energy difference between the excited state and the ground state. For different elements the spacing between the ground state and the higher energy levels is different. This gives rise to a way to uniquely identify elements based on their spectrum. A spectrum is the scientific name for a rainbow: light broken into the different wavelengths that make it up. Pre lab Questions: Submit your answers to these questions on a separate sheet of paper if more room is needed before you begin the lab.- What color of light is the lowest in energy? Red has the lowest amount of visible light energy. What color of light is the highest in energy? Violet has the highest amount of visible light energy. What color of light has the highest frequency? Violet has the highest frequency because the amount of energy is directly proportional to the frequency. What color of light has the lowest frequency? Red has the lowest frequency because it is directly proportional to the energy amount.
- How are electrons "excited"? When atoms are heated their electrons gain energy from the heat. What does it mean when the electrons are "excited"? It means that they are in a higher energy state. If you test 2 solutions and find that they both produce a red flame, how can you determine for sure whether they contain the same metal? Different elements have different spacing between their ground state and higher energy state.
- This gives a way to identify elements by their spectrum. In your own words, write a short explanation of how an electron absorbs energy and re-emits it as light and why different elements have different spectra. Electrons absorb energy and become excited and re-emit it by shooting a photon out to lose their energy. Flame Test Lab Purpose Observe the characteristic colors produced by certain metallic ions when vaporized in a flame. Identify unknown metallic ions by means of its flame test. Materials 5 watch glasses, clean and dried 1 glass dropper 1 thin glass stir rod this glass stir rod is very delicate, please handle gently!
- Free statement of participation on completion of these courses. Create your free OpenLearn profile Anyone can learn for free on OpenLearn, but signing-up will give you access to your personal learning profile and record of achievements that you earn while you study. Course content Course content What is a metal? Start this free course now. Just create an account and sign in. Enrol and complete the course for a free statement of participation or digital badge if available. Free course What is a metal? You will be using solid samples of different metal salts. The metal chlorides you will be analysing are those of copper, lithium, potassium and strontium.
- This practical activity will take 45 minutes. You will perform the experiment in the virtual OpenScience Laboratory the OU online laboratory for practical science. What you need to do: 1. Turn on the gas, pick up the lighter and light the Bunsen burner, which should give a low yellow flame. Rotate the barrel of the burner so the air hole is open and the flame is blue. One end of the nichrome wire is embedded in a cork for safe handling, and the other end has a small loop.
- Clean the loop of wire by dipping it into the small beaker containing a solution of hydrochloric acid. Place the loop into the side of the blue flame, as shown in Figure If the wire is clean it should make no difference to the colour of the flame. If the colour of the flame does change there is an impurity on the wire. Dip it again in the acid and return it to the side of the flame. Dip the loop of the wire into the acid and then use it to pick up a few grains of a metal salt. Place the loop in the side of the flame and note down the colour of the flame in your copy of Table 2. Use the hand spectroscope provided to separate the constituent colours present in the light and look at the emission line spectrum of the flames. Note down the description of spectra in your copy of Table 2. The hand spectroscope is a simple piece of equipment that houses a prism system in order to provide spectra from visible light Figure Repeat this procedure and observe the flame colour given by the other metal salts.
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