Emission of Light & Atomic Models1

Objective At the end of this activity you should be able to:

o Explain what photons are, and be able to calculate their energies given either their

frequency or wavelength.

o Order the common kinds of radiation (UV, visible light, infrared) in the

electromagnetic spectrum according to their wavelengths or energy.

o Calculate the wavelength of electromagnetic radiation given its frequency or its

frequency given its wavelength.

o Be able to compare and contrast different models for the hydrogen atom.

o Distinguish between conceptual and physical models.

o Discuss how the emission spectrum of hydrogen gas was used to support (or refute) a

given atomic model.

o Explain how electronic transitions between quantized energy-levels are responsible for

the emission of photons of light with different energies.

o Collect emission data and apply atomic models to explain the electronic structure of

elements like hydrogen and helium.

These learning objectives are assessed in the post-lab Carmen quiz.

There is no laboratory report.

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Introduction When light from the Sun or white light is passed through a

prism it produces a “rainbow” of different colors. This has been

known for centuries, with Isaac Newton making significant

advances in the area of “Opticks” in the 1700’s by investigating

how light is reflected, refracted, dispersed, etc.

However, something very different occurs when light from a

single element is emitted and passed through a prism. In this

case only a small number of discrete lines are observed. Even

more remarkably, the pattern of these lines is a defining

characteristic of each element. What happens when light is

emitted from an element like hydrogen? As you will see in this

investigation, the answering of this question has led to profound

insights into the electronic structure of the atom and, in turn, our

modern understanding of chemistry.

The emission of photons (particles of light) from atoms is thought to occur in the following

way: First, the atom absorbs energy and an electron moves to a higher energy level, or

“excited state”. When the electron eventually returns to a lower energy state energy is

released. The specific amount of energy released corresponds to the difference between the

energy levels. When this energy difference corresponds to visible light then our eyes can

observe the photons. It is also possible the emitted photons will have energies we cannot see,

such as in the infrared or ultraviolet regions of the electromagnetic spectrum.

Atoms can absorb energy in various forms (heat, electrical, radiant) and subsequently

emit photons. Today, in this investigation, you will complete activities that involve radiant

energy (photons of light). In another laboratory experiment, later this term, you will return to

this topic and investigate the role of heat and electrical excitations. In each case the emission

of photons is similar, although different energy levels and different elements may be

investigated.

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Laboratory Instrumentation The instrument used to view line spectra is a

spectroscope. Photons emitted from the atoms in their

excited states strike the prism that separates them based

on their particular wavelength. The resulting spectrum

is superimposed on a scaled and is viewed through the

eyepiece. Note, only the visible light portion of the

spectrum is observed since the detector is the human

eye.

Scientific Models

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The following are useful expressions:

E=hν !!!!!!!Planck’s relationship for the energy of a photon where h = 6.63x10-34 J s.!

c=λν The speed of a wave is equal to the product of the wavelength x frequency,

1 nm = 1x10-9 m

The speed of light c= 3.00x108 m/s in a vacuum.

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