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.Ītoms can absorb energy in various forms (heat, electrical, radiant) and subsequently emit photons. When this energy difference corresponds to visible light then our eyes can observe color. The specific amount of energy released corresponds to the difference between the energy levels. 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.
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 lines represent the photon of energy that is emitted from the atom. Each has its own discreet lines at particular wavelengths. Here are the atomic spectra of mercury and strontium as examples. In this case only a small number of discrete lines are observed.Įven more remarkably, the pattern of these lines is a defining characteristic of each element. However, something very different occurs when a photon of light from a single element is emitted and passed through a prism. 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. When light from the Sun or white light is passed through a prism it produces a "rainbow" of different colors. To complete the lab, go to the PhET model at. This lab derives from material covered in Unit 4, Lessons 17 through 19.
You will use a snapshot you took of the experimental spectrum wavelength for this comparison. You will examine the different models of hydrogen atom, consider the emission spectrum generated and compare it to the YOUR experimental emission spectra above. You will test Dalton's Billiard Ball model, Classical Solar System Model, Bohr's Model of Hydrogen and Schrodinger's Model. You will then look at spectra predicted by different models of the atom. You must run this at least 5 minutes and take a snapshot of your experimental results. This experiment generates a simulated light spectrum of hydrogen. CHEM1315 Lab 8: Atomic Spectrum CHEM 1315Ĭalculate energy and understand atomic models
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