Atomic Emission Spectra Questions

Name: _________________________________ Section Number: _________

Watch the Video: https://www.youtube.com/watch?v=BgNzEERlBf4

Fill in the tables with 4 significant figures and answer the following questions and make sure you show your work for ALL calculations.

Table 1. Silicon Metal

Wavelength (nm)

Frequency (Hz)

Energy (J)

Light color or Radiation

100

   

300

   

(max) _______

   

Calculations:

Table 2. Different Metals

Metal

Max. Wavelength (nm)

Frequency (Hz)

Energy (J)

Germanium

   

Tin

   

Lead

   

Calculations:

What do your results for silicon, germanium, tin, and lead indicate? The energy you calculated for the maximum wavelength represents the minimum energy required to eject an electron. Is there any trend? Consider the position of these elements in the periodic table and what ejecting an electron from an atom represents?

Table 3. Hydrogen emission

Line Number:

Wavelength (nm)

Frequency (Hz)

Energy (J)

Line #1 (Left)

410

  

Line #2

434

  

Line #3

487

  

Line #4 (Right)

656

  

Calculations:

The four lines you see in the visible region for the atomic emission spectrum of hydrogen are the so called Balmer series. They are due to electron transitions from atomic energy n=6 to n=2, n=5 to n=2, n=4 to n=2, and n=3 to n=2.

Table 4. Balmer Series for hydrogen

Transition

Energy Difference (J)

Wavelength (nm)

Color

n=3 to n=2

   

n=4 to n=2

   

n=5 to n=2

   

n=6 to n=2

   

Calculations:

What is the difference between the emission spectra of the molecules and those of the elements you observed in the video? Why do you think the emission spectra of the elements and molecules are so different?

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