Lab report - Experiment #1: Flame Test PDF

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Experiment #1: Flame Test...

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Banawis HJC, Baluyot KJE, Bullo PVGD. Group #2 of MT 1-6 CHE 009 E#1: FLAME TEST OBJECTIVE:

solution. (Safety: in getting the HCl solution,

To observe and analyze the colors produced through flame tests of different solutions.

you MUST wear your ear loop mask to avoid the solution from smelling the somewhat sharp and irritating odor that the solution produces. In addition, in significant concentrations produces a burning and

METHODOLOGY:

choking sensation as it dissolves the tissues in your respiratory system.) After dipping it in HCl solution, place Figure 1: Materials for Flame Test Experiment

the tip of the wire loop onto flame until

In this experiment, you will need: test tubes, Bunsen burner, your test solutions, pipette and HCl. The experiment starts in setting up

red hot. Dip the wire

loop on your first test solution. You can pick whatever test solution you want first but

the Bunsen burner and of course, by getting

once you finished

all the solutions you need such as KCl,

putting it onto flame,

NaCl, LiNO3, BaCl2, Sr(NO3)2, CaCl2, BiCl3,

you must dip it again

CuSO4. For the measurements, it must be 1

in HCl solution (the

mL which is approximately, 10 drops for the

one that is not

pipette.

contaminated). But the instruction will be To start the

Figure 3. Contaminated HCl due to the dipping of wire loop

Figure 4. Flame produced by KCl solution.

different in CuSO4

entire experiment,

because you have to add 1 drop of HCl

sanitize the wire loop

before testing it. Still, you have to follow the

by dipping it in a

procedure before doing putting it to flame.

concentrated HCl

You have to dip the wire loop in HCl first Figure 2. Concentrated HCl solution

before dipping it in

laboratory burner. As a result of our

CuSO4. After that,

experiment, when we put Sodium Chloride

you can now finally put the test solution in flame. But in our experiment, we tested first the KCl

Figure 5. Flame produced by CuSO4.

(NaCl) into fire it became color orange.

which produced an orange flame, then after

Lithium Nitrate (LiNo3) became violet to red

that, we dipped it again in HCl solution to

flame, Potassium Chloride (KCl) became

sanitized the wire loop then dipped it to

yellow flame, Barium Chloride (BaCl2),

another test solution and so on and so forth.

Calcium Chloride (CaCl2) and Strontium Nitrate (Sr(NO3)2) became color red flame,

DATA AND RESULT TEST

Bismuth Chloride (BiCl) became color COLOR

orange flame and Copper Sulfate (CuSO4) became green flame.

SOLUTIONS KCl NaCl

Orange Orange

LiNO3

Violet - red

are produced from the movement of the

BaCl2

Yellow - green

electrons in the metal ions present in the

Sr(NO3)2

Red

CaCl2

Orange

an unexcited state has the structure

BiCl3

Orange

1s22s22p6.

CuSO4

Green

Another explanation, flame colors

compounds. For example, a sodium ion in

When you heat it, the electrons gain energy and can jump into any of the empty orbitals at higher levels - for example, into DISCUSSION The colors produced by chemicals when inserted into a flame can be used to identify some constituents of minerals. One procedure used was to put a small amount of the chemical on a small loop of platinum wire and place it into the open flame from a

the 7s or 6p or 4d or whatever, depending on how much energy a particular electron happens to absorb from the flame. Because the electrons are now at a higher and more energetically unstable level, they tend to fall back down to where they were before - but not necessarily all in one go.

An electron which had been excited

levels of a certain chemical. When an

from the 2p level to an orbital in the 7 level,

electron jump from one level to another and

for example, might jump back to the 2p level

jumps back, that shows the production of

in one go. That would release a certain

light.

amount of energy which would be seen as

REFERENCE:

light of a particular color. Kellner, Robert / Mermet, Jean-Michel / However, it might jump back in two (or more) stages. For example, first to the 5 level and then back to the 2 level. Each of these jumps involves a specific amount of energy being released as light energy, and each corresponds to a particular color. As a result of all these jumps, a spectrum of colored lines will be produced. The color you see will be a combination of all these individual colors. The exact sizes of the possible jumps in energy terms vary from one metal ion to another. That means that each different ion will have a different pattern of spectral lines, and so a different flame color. CONCLUSION: Doing this laboratory experiment let us observe, analyze and find out the color if the chemical produced. Each substance creates a different level of energy produced. That means that every chemical will produced a different color in the flame test. The reason behind is the different energy

Otto, Matthias / Valcarcel, Miguel / Widmer, H. Michael, Analytical Chemistry (A modern approach to analytical Science), 2004 Chemguid.co.uk Jim Clark 2005...