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Flame Color Change Lab Results

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Analysis: The ion that causes the color change in flames is because of the cation in a chemical formula. The reason why the cation is the cause of the color change is because when I observed the flame color created by the different salts, there some a couple of similarities and differences that I found in each chemical formula. Two formulas that I were drawn to first were potassium chloride and sodium chloride. They both have the same anions however they have different cations and this is the first clue that I found to try to find out which ion causes the flame color change. The next clue that I found that the anion wasn’t the ion causing the color change was also the chemical formulas. Sodium sulfate and sodium chloride both have similar cations however they have different anions but they produce the same color. …show more content…

Based on the data collected in my data table, I can give an educated guess and say that the cation of this unknown salt is strontium. During the flame test, I observed strontium chloride and strontium nitrate to produce the same color and that color was described as red. This unknown salt was stimulated and it showed similar characteristics as the strontium. The light that is produced by an atom can be simply explained because of an atom being stimulated. When an electron is stimulated the electron gains energy and can jump orbitals in the atoms and this is when the electron emits the light. The electron however cannot emit this light/energy forever so the electron moves back to it’s most basic orbital that it can sustain forever. This is why the salt isn’t always emitting the light whenever we see it. Once this electrons aren’t being stimulated, the salt will lose the color of the cation because of the loss of

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Chemical compounds that are available to determine are CaCO3, CaCl2, Ca(NO3)2, mgCl2, MgSO4, KCl, HCl, HC2H3O2, KNO3, K2SO4, NaC2H3O2, Na2CO3, NaCl, Na2SO4, HNO3, H2SO4, HNO3, H2SO4, NH4Cl, (NH4)2SO4, K2CO3, 0.1 M AgNO3, 0.2 M BaCl, Mg(s), NaOH, and KOH. To start this experiment, start with the flame test by gathering a Bunsen burner and a Nichrome wire. Connect the Bunsen burner with a rubber tube to a laboratory gas. To prepare solutions for the flame test, weigh out 0.205 gram of Unknown Compound using an analytical balance and mixed it into a 140 mL beaker filled with 20 mL ionized water. Ensure that solid is completely dissolved using a stirring rod.

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The wavelength of light emitted by sodium light sources is made up of yellow wavelengths from 589.0 - 589.6nm so no colour version is possible. These lights may not be ideal at night time this is because, the human eye cannot function fully in the photopic state, and its colour sensitivity shifts to the scotopic night vision conditions. This phenomenon is known as the Purkinje shift. Herein lies a deficiency of our measure of light because it is based on the normal daylight sensitivity curve of the eye.

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Some compounds have very distinctive colors when burned, such as Potassium, which is a white/purple, and sodium, which is a deep red hue. The first step for a flame test is to gather the needed materials. These include beakers, distilled water, the unknown substance, a Bunsen burner, matches, a nichrome wire, tubing to connect the gas line to the Bunsen burner, goggles, and known compounds to compare with. The first step is to make aqueous solutions of all the substances to be tested. This is done by adding .5

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These color changes indicate a chemical change, which show that a reaction had occurred. In the first step when o-vanillin and p-toludine, imine was formed. The color change from green to orange suggests that imine appears as orange colored. In the second step, the addition of sodium borohydride reduced the imine into another derivative, which was yellowish lime color. The solution turned clear when acids and anhydrides was added, which indicated the precipitate were dissolved.

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It was found that the reaction was limited to taking place to only the mouth of the test tube, as it is the only place where a mostly yellow and orange flame burned, which was opening downwards. The part of the flame that is furthest from the mouth glowed blue. During the reaction, very little sound was produced to the extent that one can only hear it in a quiet room. In addition, very large amounts of black soot was produced continuously throughout the entire reaction, which congregated towards the mouth of the test tube so that the amount of soot decreased as the distance between it and the mouth of the test tube

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Part A When sodium was added to water, the sodium melted to form a ball that moved around on the surface of water rapidly and hydrogen gas was produced. Because of the amount of heat liberated during this exothermic reaction, the hydrogen gas ignited the sodium with an orange flame while floating on the water. Also, when potassium was put onto the water, the observation was similar to how sodium reacted towards water. The metal was also set on fire, with sparks and a lilac flame. But, in the case of speed of tarnishing between the two elements, potassium was faster than sodium.

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THis was found through a combination of the tests, in whic the ammonia and sulfuric parts of the compound reacted to the different variables. In the flame test, it reacted with an orange flame, with little difference from the uninterrupted flame created by the bunsen burner normally. This meant that it was unlikely for the final compound to have either sodium or potassium, due to their reactions including yellow and purple flames. These results were confirmed when after the KOH Test, the unknown salt also reacted with a similar smell, and the Ba(NO3)2 test in which the salt also reacted closely to Ammonium sulfate. These variables together meant that the final, unknown, compound was a combination of ammonium cation and sulfate anion, or Ammonium

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The wax melted first, followed by the salt, and lastly the sugar. The salt not only burned before the sugar, but developed a brown color throughout most of the substance at a faster pace. In the water solubility test, the salt dissolved in the water, as soon as it was properly mixed and the sugar dissolved in the water as well, but was stirred for a longer period of time until it was completely dissolved. The wax did not dissolve in the water, however bits of the substance broke off from the main piece. With this information, the final results included: wax as a nonpolar covalent compound, since the substance melted first and was not soluble in water; salt as a polar covalent compound, since the substance was soluble in water and the second to melt; and sugar as an ionic compound because the substance melted last and was soluble in

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