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Four scenarios involving absorption of light and electron jumps are shown. This graph is almost identical to the diagram of the hydrogen atom on the left side of the infographic, but does not show the nucleus of the atom. The energy levels are represented by straight horizontal lines instead of concentric circles. As in the atom diagram, the electron is represented as a small circle. Light is represented as a wavy colored arrow. The change in energy level is shown with a dashed, straight gray arrow.

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The spectrum is graphed as a line. The overall shape of the line resembles a bell curve cut off on the left and right sides. The curve begins on the far left with a brightness of about 0.83, increases to a peak of 1 at about 500 nanometers, and then decreases gradually to a low of about 0.7 on the right side of the graph.

This four-part infographic titled “Absorption of Light by Hydrogen” illustrates the relationship between the wavelength of light absorbed by an electron in a hydrogen atom, the change in energy level of the electron, a picture of the absorption lines in the hydrogen spectrum, and the graph of hydrogen’s absorption spectrum. The graphic includes:

At the bottom, directly below the picture of the spectrum is a graph of the same spectrum. The vertical y-axis is labeled “Brightness.” The horizontal x-axis is labeled “Wavelength (nanometers)” and ranges from about 375 nanometers at the origin on the far left, to about 775 nanometers on the far right. The axis is labeled in even increments of 100 nanometers, starting at 400 nanometers.

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Four scenarios involving absorption of light and electron jumps are shown. In all four cases, the electron is represented as a small circle. Light is represented as a wavy colored arrow. The change in energy level is shown with a dashed, straight white arrow. In all four scenarios, the small circle is positioned on energy level 2 to indicate the electron’s starting energy level.

A diagram of a hydrogen atom shows the relationship between the color of light absorbed by an electron and its change in energy level.

SI (Système International) units are used throughout this tutorial. Many international organizations, including the CIE (Commission Internationale de l'Eclairage), have exclusively adopted this system of units. The terminology used follows that of the CIE International Lighting Vocabulary. See for instance the e-ILV, electronic version off the International Lighting Vocabulary, on the website of the CIE.

Absorptionspectra

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At the center is a solid circle representing hydrogen’s nucleus. Six concentric circles representing electron energy levels (or orbitals) surround the nucleus. The circles are labeled “level 1” through “level 6” with level 1 closest to the nucleus, and level 6 farthest. The distance between adjacent energy levels decreases with distance from the nucleus.

The Gigahertz Optik GmbH is silver supportive member of the CIE and active in many technical committees (TC's). All our products follow the guidelines of international standards and technical reports.

Visiblelightwavelength

Superimposed on the curve are absorption features: four steep valleys of relatively low brightness. From left to right, the valleys appear at wavelengths of 410 nanometers, 434 nanometers, 486 nanometers, and 656 nanometers. The depths of the valleys increase from left to right.

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The three graphics on the right side of the infographic are aligned to show the relationship between the color of light absorbed and the electron jumps, the absorption lines in the picture of the spectrum, and the absorption valleys on the graph.

Directly below this graph is an illustration of a hydrogen absorption spectrum. The spectrum is a rectangle with rainbow coloring: purple on the left to red on the right. The rainbow pattern is not continuous and includes four black lines of varying width.

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However, optical radiant energy does not only encompass visible “light”, but also radiation that is invisible to the human eye. The term optical is used because this radiation follows the laws of geometrical optics.

This tutorial is an introduction to the radiometric, photometric, colorimetric, reflection and transmission principles as well as quantities, symbols, units and the basic nature of light and color. Sections covering a sampling of current applications, detectors, electronics and calibration are included. A list of reference sources is provided for future study.

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The relationship between a hydrogen atom and its absorption spectrum. (Left) A simple model of a hydrogen atom showing four of the many possible “jumps” the electron could make when it absorbs light. (Right) The relationship between the electron jumps and the specific wavelengths of light that the atom absorbs. An electron jumps from one energy level to another only when it absorbs a very specific wavelength of light (i.e., when it absorbs a photon with a specific energy). The shorter the wavelength, the higher the energy, and the greater the jump. Wavelengths that are absorbed appear as black lines in the spectrum. This illustration shows a set of jumps that correspond to absorption of visible wavelengths (the Balmer Series).

Light, which is the visible part of the electromagnetic radiation spectrum, is the medium through which human beings receive the major part of environmental information. Evolution has optimized the human eye into a highly sophisticated sensor for electromagnetic radiation. Joint performance between the human eye and the visual cortex, which makes up a large part of the human brain, outshines even the latest technical and scientific developments in image processing and pattern recognition. As a matter of fact, most of the information flow from external stimuli to our brain is transferred visually. Photometry deals with the measurement of this visible light energy.

1. The act of physically illuminating or the condition of being filled with light: light, lighting. 2. Electromagnetic radiation that makes vision possible:.

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