Different Flame Levels Lab

2. Used a test tube clamp to held the test tube and gently heated the tube in a laboratory burner flame for about 30 seconds.

Explain why this was important. If a splint is left in the flame for so long, it will begin to burn. The burning wood will produce a yellow flame and it will cause the results of the test to be inaccurate. For each of the solutions that you tested, it was a metal ion that gave it the flame colour.

2- It is impossible to identify all element with the naked eye because they don’t release enough energy, therefore the color is not as visible. Besides, not all elements give a light that it is in the visible part of the spectrum, so we need to use a prism.

4.Measure 35mL of warm water and add them into each of the 4 test tubes at about roughly the same time. It is essential that the water is warm. Do not seal the test tube.

Add 15 drops of 6 M NaOH to each. Then place a strip of moistened red litmus paper across the top of each test tube and set the test tubes in a beaker of warm water. Do not let the litmus paper touch the NaOH. The NH3(g) given off will turn the red litmus paper blue. The color of the unknown did not occur and the color of the NH4Cl changed to a blue color. Then place 2 ml of 0.1 M FeCl3 in one test tube and 2 ml of your unknown in another test tube. Add 5 drops of 6 M HNO3 to each test tube. Add 2-3 drops of 0.1 M KSCN to each test tube. A deep red color indicates that Fe3+ is present. A faint pink color is not positive test from iron. The color of unknown B was not present while the color of 0.1 M FeCl3 was red. Therefore, neither NH4+ Fe3+ was present in unknown

Procedure 1. Obtain 7 test tubes and stoppers from the instructor. Label each vial L1, L2, L3, D1, D2, D3 and N1. 2. Cut 7 cotton balls in half and place each wad in the bottom of each vial by using the wooden stick to push it down.

The size of the beaker was recorded in the observation table, while the flame duration time was recorded in the column labeled Trial 1, beside the size of the beaker. 8) Steps 3 to 6 was repeated with the same beaker. The duration time was recorded in the same row as the previous time, but in the column named Trial 2. 9) Steps 3 to 7 was repeated with the rest of the three different sized beakers. 10) Steps 3 to 8 was repeated with the 2 unknown

Next inserting a rubber stopper wit tubing connector into each of the test tubes and into each of the test tubes using a piece of parafilm around the stopper and tubing to fully seal the test tubes. Obtain a 1mL pipette and dip the free end into a tube of colored water and tap the pipette until the water reaches the first marking of the pipette (0.1mL). Then, connect the pipette to the tubing on the rubber stopper, double checking that all tubing connections are secure. After connecting the pipette and tubing together place the pipette horizontally on the ring stand, keeping the pipette leveled. Let it sit for five minutes to equilibrate, this will be used as a zero starting point.

Practiced holding the empty test tube with gloves and sliding the test tube into the Erlenmeyer flask, and sealed the flask with the stopper. 3. Took 5mL of sodium hydroxide in the

1 ml of water should be added to the first test tube and make a note. In the second test tube, 1 ml of methyl alcohol should be added. In the third test tube, 1 ml of hexane must be added. Lastly, the fourth test tube will be a control.

6. Add warm tap water to each test tube, filling each test tube 4/5 of the way to the top. 7. Cover the opening of each test tube with a balloon to catch any gas that is formed. Using the balloon to seal the end of the tests tube, hold a finger over the end of each test tube and shake it vigorously to thoroughly mix the contents.

Close the test tube and shake for a moment then leave the test tube back into the water bath. Wait for the data collection to finish. 8. Afterward, dispose of the solution as your instructor has announced. 9.

Numerous metals and different substances radiate splendid shades of obvious light when they are warmed. The colors originate from electrons moving between energy levels. The energy gaps between their electron shells relate with the energy of the colour they give off. so the energy of every colour of light matches the energy gaps between electron shells in different atoms. Electrons are orchestrated into energy levels.

Measure and fill the graduated cylinder with 10 ml of HCl, and transfer to the test tube labeled A. Repeat step 2 for test tube labeled B and C. Add 3 drops of universal indicator to each of the test tube A, B and C. Add as many drops of Milk of Magnesia as you need to test tube A, swirling around between drops, until the color is neutral by comparing it to the control test tube of water. Make sure to stop at the

Flame Test Purpose: The premise of the lab experiment was to observe the color of visible light emitted from several compounds and find what the unknown substance is by comparing its reaction to others. The emission of light, more so, occurs when an electron releases absorbed energy from its excited state and reverts back to a position of lower energy, a ground state. Procedure: In order to achieve the results for the experiment, a Q-tip was used to place near the Bunsen burner.