Chem B3. Lab - Flame Test and Emission Spectrum
Chem B3. Lab - Flame Test and Emission Spectrum
Chem B3. Lab - Flame Test and Emission Spectrum
Introduction
If light from an incandescent bulb is passed through a prism it is separated into a rainbow of colours
ranging from red to violet. When the light produced by passing an electric current through a gas is
viewed in a similar manner, however, the result is quite different.
Each gas has its own spectrum of coloured lines. In attempting to explain why gases emit line spectra,
Neils Bohr took the concept of the atom proposed by Rutherford and developed his "solar system"
model.
You are expected to complete and turn in the BLUE sections of this lab
Purpose: To observe the line spectra of unknown elements and determine using reference emission
spectra, which elements are present in the gas discharge tubes.
Procedure:
1. Observe the incandescent light bulb through the spectroscope and sketch or take a picture of the
spectrum. Record in an observation table.
2. Point the spectroscope towards the window and sketch or take a picture of the spectrum. Record in
an observation table.
3. Observe the spectra produced by each of the two unknown gas discharge tubes and sketch or take a
picture of their spectra. Record in an observation table.
4. Compare the spectra you have drawn with the reference spectra provided to you to identify the
unknown elements.
Analysis:
Procedure:
Carry out the procedure described by your teacher. Be sure to return all wooden splints to the
appropriate container
Analysis:
Observations - Design a table to collect your data.
2. Which ion (anion or cation) is being identified using the flame test? Explain.
3. Explain how the colors in the flame tests are produced (in terms of electrons and energy states).
4. Street lights are yellow/orange in color and not white. Based on your flame test data, what
gaseous element is present in street lights?
5. Explain in your own words what a spectroscope is doing when used to view a light source.
6. Are the spectra for the sun, the incandescent light bulb and the different gases shown
continuous spectra or emission (line) spectra? Explain.
7. Why are spectral lines from the bright line spectrum referred to as "fingerprints" of the atoms?
How confident are you that your investigation produced a valid answer to the identity of the unknown
metal salt and gases? Clearly identify two limitations of the Experimental Design. Evaluate how these
might affect your result, and suggest realistic improvements that might address these limitations.