Flame Test Lab Report Kieran Sidebotham Period 3 10/4/17 1. Purpose: The purpose of the flame test lab was to further study the process of electron excitation. We tested the different reactions of each chemical compound that we used with the flame. The purpose was to see the electron excitation of each reaction and the color that it emitted. Also, to see the color of each reaction determining the amount of energy released using our color scale. 2. Materials: -Bunsen burner -Pre soaked popsicle sticks Chemical compounds: -Lithium Chloride -Potassium chloride -Sodium nitrate -Copper Sulfate -Copper Nitrate -Strontium chloride -Assigned Unknown (D for us) 3. Safety/Lab Partners: Safety: Lab aprons goggles Partners: -Anna Wilde, Malia Halafuka, Caleb 4. Procedure: …show more content…
What did you observe when the popsicle sticks were placed into the bunsen burner flame? Depending on the compound on the popsicle stick, the reactions emitted lights of all different colors which shows the amount of energy released on the color scale. 2. Each compound use consists of a metal component and a nonmetal component. In other words, in lithium chloride, the lithium component was the metal and chloride component was the nonmetal. Which of the two components do you think determined the color emitted by the popsicle stick? How does your data support your answer? I think the metal component produced the color emitted. For example copper nitrate, and copper sulfate produced the same color as each other. 3. Write a four step process of electron excitation. -Electron absorbs energy produced from another electron -The excited electron moves to a higher energy level -That electron gets pulled toward the nucleus of the atom -The electron then jumps down an energy level and emits a light of energy 4. Why would an electron in an excited state want to return to a lower energy
The experiment is to observe a variety of chemical reactions and to identify patterns in
For the test tube with the ratio of Acetylene to air is 1:3, a flame traveled down a test tube even slower, there was a slight popping noise and black residue . For the test tube with the ratio of Acetylene to air is 1:7, a flame traveled quickly down a test tube, popping noise and less black residue. Refer to table 1 for the specific lab results.
Procedure: In this experiment, various chemicals were mixed together, to determine a reaction. Using two drops from chemical 1 and two drops of chemical two, unless otherwise stated, then recording the type of physical reaction or color changes that occurred.
chloride solutions, which resulted in a variety of colored flames. The color with which each cation
A chemical reaction is when substances (reactants) change into other substances (products). The five general types of chemical reactions are synthesis (also known as direct combination), decomposition, single replacement (also known as single displacement), double replacement (also known as double displacement), and combustion. In this lab, the five general types of chemical reactions were conducted and observations were taken before, during, and after the reaction. Then the reactants and observations were used to determine the products to form a balanced chemical equation. The purpose of this lab was to learn and answer the question: How can observations be used to determine the identity of substances produced in a chemical reaction?
In a combustion reaction, a compound or element reacts with oxygen, releasing a large amount of energy in the form of light and heat.
Prior to conducting this lab, it was known that flame colors are produced from the electronic transitions in the metallic ions present in the salt compounds. When heated, the electrons absorb energy, jumping from ground states of lower energy to higher-energy, excited states. The electrons must return to their lower energy levels as energy is emitted in specific amounts in the form of light. Each energy emission correlates to a certain color, and since the transitions of metallic ions vary from each other, each ion produces a unique pattern of spectral lines, therefore creating an equally unique flame color.
In this experiment you will observe some physical and some chemical changes. You will observe that energy must be used to start some chemical reactions, and that it is produced in others.
We repeated this for a total of 6 known substances and 3 unknown substances. We also made a table for each element showing the color of the flame that we saw,
The luminous yellow flame is smoky because no air is entering the burner and hydrocarbon is converted into carbon dioxide
Every 4th of July, many people go out at night and spend hours watching firework shows. Most of us are content to simply enjoy the pretty colors and sparks, without questioning the chemistry behind the spectacle, but have you ever really thought about how fireworks produce such vibrant colors? The colors emitted when a firework explodes come from an aerial shell inside the firework that contains explosive chemicals and metallic salts. These colors appear to us because of luminescence. Luminescence occurs as a result of the valence electrons in the metal salt atoms moving and changing positions. The explosion of fireworks is not a miracle; it’s simply chemistry at work.
For example, silver nitrate formed a white precipitate when it was tested with ammonium chloride. In contrast, unknown 3 did not formed any precipitate with ammonium chloride. Ammonium chloride change the color of unknown 3 to a light green while the solution of silver nitrate and ammonium chloride was cloudy white solution. Likewise, the metal in unknown 3 could have been Calcium neither. Data and observation shows that calcium nitrate whether formed a white precipitate or did not react at all while unknown 3 formed an orange precipitate. Therefore, silver and calcium are not the two metal present in unknown
Introduction: The theory behind this experiment is the heat of a reaction (∆E) plus the work (W) done by a reaction is equal to
The aim of this experiment was to test the heat of combustion over a period of time, and the energy required to combust alcohols with different carbon chain levels. It was hypothesised that the higher the carbon chain of the alcohol present, the faster the heat of combustion will occur. Meaning more energy will be released for a higher carbon chain. After calculating the results from the experiment it was found that the hypothesis was partially supported. The reasoning for this is as the alcohol that posses a higher carbon chain, generally increased there reaction rates. However there were a few exceptions to this rule.
Purpose: This lab taught procedures for determining heat of capacity of a calorimeter and measuring enthalpy of change for three reactions. It also enforced methods of analyzing data obtained through experimentation and calculating enthalpy. These procedures are used in the branch of thermodynamics known as thermochemistry which is the study of energy changes that accompany chemical reactions. Concepts from this lab can be used to determine the potential energy of a chemical reaction. Much of the energy people depend on comes from chemical reactions. For example, energy can be obtained by burning fuel, metabolizing of food or discharging a batter.