Click on the link. You'll see a periodic table with a spectrum above it. Locate the white icons labelled "Absorption" and "Emission." Click on the "Emission " icon; it is on the right. If it is active, its center should be dark. Next, click on the symbols of the elements you worked with in the experiment and observe the spectrum for each element. Check your lab notes to remember the colors you saw when you did the flame tests. Once you have had a chance to explore the site a bit (Who can resist?) answer the following questions:
a. Which element in the experiment has fewest intense red lines in its spectrum?Now click on the icon to view this element's absorption spectrum. You should see a color continuum with black lines at certain positions.
b. Which element in the experiment has the most broad lines in its spectrum?
c. Which element in the experiment has the fewest lines in its spectrum?
d. At what positions do the black lines appear, relative to the emission spectrum?Helium, the second lightest element, was discovered because people saw its absorption lines in the spectrum of sunlight. Its name comes from Helios, the Greek sun god.
e. Given that the elements emit light in narrow frequency bands, rather than a color continuum, which of the following statements must be true?
Click on the symbol for helium and observe its emission spectrum. If you place the cursor on a line and right click (with a Macintosh, just hold down the mouse or button) you'll see the wavelength of that line in Angstroms (1 Angstrom = 0.1 nm = 1x10-10 m).
Find the most intense (broadest) band of each color in the table, and give its wavelength in Angstroms.õ x.øi5valign="top">Blue
Red Yellow Green
Give the frequency of the red band: sec-1 Give the energy of the blue band: J