Flame Test

3. Removed the test tube from the flame and places a piece of moistened litmus paper in the mouth of the test tube. Identified any odor that is readily apparent by wafted the fumes toward your nose. Caution: Do not sniff

3. Examine the luster of the minerals in Figure 1.2 (p. 4 lab book). Place the letter A, B, C, D, or E in

Lithium has the lowest energy of wavelength emitted. Sodium has a higher energy of wavelength emitted, and lithium has the highest. As one moves down the alkali metal family, the energy emitted increases because more shells are being added

4. The melting points of the solids were tested by placing them in crucibles and heating them using a hot plate.

Pour 50 mL of distilled water into a 100 mL beaker, and then add the unknown substance into it. Mix thoroughly to create the aqueous solution. Now fill a new cuvette with this new solution and place into the SpectroVis Plus device; after wiping the outside with a Kimwipe as usual. Be sure to take note of the absorbance when wavelength is at its maximum. Afterwards, Be sure to take all solutions containing Iron(III) and pour them into the container specified for hazardous wastes. ​

5. NaCl, sodium chloride, is a common salt and it burns in the flame test.

2. If the mineral is non-metallic, decide if it is light or dark in color.

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.

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.

Once a light beam shines through the flame, the atoms absorb some of the light. It is then detected, recorded and compared to a series of standard solutions. In the absorption spectrum, the absorbed light show up as black gaps. These distinctive gaps indicate the difference in energy levels for a particular element. If this can be compared to the concentration of its standard solution, then it can form a calibration curve.

The main objective of this experiment is to carry out qualitative analysis to identify metal cations in unknown solution 1.

Part A.1. Sodium metal is also readily oxidized by oxygen. If the product of the reaction were dissolved in water, what would be the color of the litmus for a litmus test? Explain. What is the product?

gases and smokes could have carbon dioxide, and carbon monoxide in it. Also the different colors in a firework involves chemistry too! Fireworks get their different colors from metal compounds.

To begin, a fuse is lit on a firework that eventually reaches metals inside a firework, providing heat to the metals. This heat causes the electrons of the metals in the firework to become excited, meaning that they gain energy and move up to a higher, unstable energy level. Because this higher level is unstable, the electrons soon fall back down to their initial energy level and release energy in the form of light as they do. This light is what we can see when fireworks are lit, but the color depends on the amount of energy released. Higher energy releasing metals like Copper (I) chloride and Strontium copper compounds yield blues and purples, while lower energy releasing metals like lithium carbonate, strontium carbonate, and calcium salts yield reds and oranges. Greens and yellow result when median energy releasing metals like sodium compounds and barium compound are