Flame Test Lab Report Results

2. When the magnesium ignited, removed it from the flame and held it over an evaporating dish or a pyrex watch glass until the metal had burned completely. Let the product fall into the evaporating dish.

One type of chemical reaction, called combustion, involves the burning of various compounds and elements. Some substances are more

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.

| After ignition of magnesium light and toxic fumes are made, and white powder (2MgO or Magnesium Oxide) is left over.

Because it is dangerous to burn magnesium, it is not possible to directly record heat change. Our lab team suggests an indirect way of determining the heat of combustion for magnesium. To accomplish this, we need to perform two separate trials. One uses a solid (powder) version of MgO, while the other uses Mg ribbon. With the results from these, we can use Hess’ Law to determine q=∆H. This provides both a safe and successful way of indirectly determining the heat of combustion for magnesium.

This light is known as the spectrum emission color of an element which can also be used to identify an element as well as determine the energy that is given off. In this lab we used this information to identify three unknown substances and determine if the energy given off was high or low. In order to conduct this lab we had to take a known substance for example Copper Chloride (CuCl) and use a splint to put the substance over a bunsen burner. We then recorded the frequency, color of the flame, and the spectrum emission line by using spectroscopes, which diffracts light.

Station one: Station one shows that when a small piece of magnesium metal is placed over the flame of the Bunsen burner, the magnesium metal ignites, giving off a bright, white light. Once the flame has extinguished itself due to the lack of fuel, the magnesium metal turned from a metallic strip to a crumbled white powder. It can be decided that station one is a combination (redox) reaction, as a new product is synthesised by the combination of two reactants. The reactants, magnesium and oxygen gas in the air bonded together to form the product of magnesium oxide.

1- Different elements give off different colors when heated because electrons go farther the nucleus, or to an upper energy level, and once they go back to their original orbit (energy level), they release colors because of the amount of energy released. This also happens because different elements are in different orbits and they hit different orbits as well.

Abstract: The purpose of this project is to measure if differing amounts of potassium perchlorate, KCIO4, mixed with shotgun powder has an effect on burn rate. The experiment was videotaped and the duration of burn time for each amount used was recorded. KClO4, amounts ranging from .2g to 2g, were added to 4g of shotgun powder. A steel pipe that is ½ inch wide and 6 inch, which is welded vertically to a steel plate base was used for confinement. Ignition occurred from the top down. The hypothesis that was accepted is that the concentration of KClO4 will accelerate the burn rate of smokeless flake powder.

Change in color once chemicals were combined (experiments b,c,d,e,f,g,h,j,l); Precipitate formation (experiments g,j,l), and formation of gas bubbles (experiment a).

The most reactive substance in this lab was the crushed liver core, it produced the most amount of heat, bubbles, and the biggest flame during the glowing splint test. The manganese dioxide and the liver core were also very reactive and they both produced a flame during the glowing splint test. Next, the potato core produced a slight reaction, but it was not as extreme as the other substances. Finally, just the hydrogen peroxide and the boiled liver core had no reaction and did not produce a flame during the glowing splint test.

4. Why does the flame color change back to orange, after the metallic solution has been turned completely into a gas

To perform the experiment, you need 2 ml of water, then contain 15 ml of 3m HCL, 6m HNO3, 6M NaOH, then 15 ml of unknown solution each one labeled on a test tube. A flame test will be conducted to determine ions. You will need a spot plate, Bunsen burner, flame-test wire, dropper bottles of 0.1 M NaCl, 0.1 M KCL, 0.1 M CaCl2. Obtain a spot plate. Place 5 to 8 drops of 0.1 M solutions of each of the following solutions into separate indentations: KCL, CaCl2, NaCl, unknown solution. To clean the flame-test wire dip the loop at the end

When white light (which is made of all the colors of the rainbow) strikes a red object, its atoms specifically absorb and re-emit red light; all the other colors of light simply cause the object to get a bit warmer. At the point when a fire works blast, it conveys smoldering protuberances that contain, in addition to other things, metal salts. These metal salts are warmed and start sparkle in fabulous hues. Metal salts that are regularly utilized as a part of fireworks presentations include: strontium carbonate (red fireworks), calcium chloride (orange fireworks), sodium nitrate (yellow fireworks), barium chloride (green fireworks) and copper chloride (blue fireworks).

Not only that, but the unique element actually glows a bright red-ish orange when it is electrified... At least, typically. Depending on the gas, chemicals, and how it is electrified, the element can also glow other colours such as red, yellow, white, and blue!