Name: electromagnetic waves: uses across the spectrum
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 2 min 37 s
Channel: JoVE

K12 Standards

Pennsylvania State Academic Standards

9-12

Earth and Space Science

Earth's Systems

3.3.9-12.H

The Electromagnetic Spectrum

Das elektromagnetische Spektrum ist der Bereich der Frequenzen und entsprechender Wellenlängen der elektromagnetischen Strahlung. Wellenlänge und Frequenz sind umgekehrt proportional zueinander;je länger die Wellenlänge, desto niedriger die Frequenz. Die Energie der elektromagnetischen Strahlung ist direkt proportional zu seiner Frequenz, wie die Planck'sche Gleichung zeigt.Somit haben die energiereichsten elektromagnetischen Wellen die kürzesten Wellenlängen. Elektromagnetische Wellen werden in Radiowellen, Mikrowellen, Infrarotstrahlung, sichtbares oder ultraviolettes Licht, und Röntgen-oder Gammastrahlen, abhängig von ihren Frequenzen und Wellenlängen kategorisiert. Radiowellen, die zur Übertragung von Signalen zwischen Kommunikationssystemen verwendet werden, haben die längsten Wellenlängen, die niedrigsten Frequenzen und die geringste Energiemenge.Mikrowellen haben die nächstlängsten Wellenlängen. Ihr Einsatz reicht von Radarsystemen bis zum Erhitzen von Lebensmitteln zu Hause. Als nächstes kommt die Infrarotstrahlung, die ein wesentlicher Teil der emittierten Wärmestrahlung durch warme Gegenstände ist.Zum Beispiel, absorbiert die Erde Infrarotstrahlung als Teil der von der Sonne ausgestrahlten Strahlungsenergie und gibt auch selbst Infrarotstrahlung in den Weltraum ab. Die Wellenlängen des sichtbaren Lichts sind noch kürzer, im Bereich von 740 bis 390 Nanometern. Rotes Licht hat die längste Wellenlänge und violettes die kürzeste.Das menschliche Auge nimmt nur auf dieses kleine Wellenlängenspektrum wahr. Ultraviolette Strahlung hat noch kürzere Wellenlängen. Sonnenlicht ist die bekannteste Quelle der ultravioletten Strahlung, die so viel Energie ausstrahlt, dass sie bei übermäßiger Exposition Sonnenbrände verursacht und zu Hautkrebs führt.Röntgen-und Gammastrahlen haben die kürzesten Wellenlängen und sind die energiereichsten Formen der elektromagnetischen Strahlung. Röntgenstrahlen können viele Substanzen durchdringen, aber sie gehen nicht so leicht durch die Knochen. Das macht sie zu einem wichtigem bildgebendem Werkzeug.Gammastrahlen sind am besten bekannt als die während der Zerfallsketten bestimmter radioaktiver Elemente. Es gibt zwar keine allgemeingültige Unterscheidung zwischen Gamma und Röntgenstrahlen, Gammastrahlen haben die kürzesten Wellenlängen, die höchsten Frequenzen und höchste Energien.

das elektromagnetische spektrum

Das elektromagnetische Spektrum besteht aus allen Arten elektromagnetischer Strahlung, geordnet nach ihrer Frequenz und Wellenlänge. Jeder der verschiedenen Farben des sichtbaren Lichts können bestimmte Frequenzen und Wellenlängen zugeordnet werden, wobei das sichtbares Licht nur einen kleinen Teil des elektromagnetischen Spektrums ausmacht. Da die Technologien, die innerhalb verschiedener Bereiche des elektromagnetischen Spektrums arbeiten, teils sehr unterschiedlich sind, werden aus Gründen der Anschaulichkeit und sowie historisch bedingt meist unterschiedliche Einheiten für verschiedene Bereiche des Spektrums verwendet. Beispielsweise werden Radiowellen üblicherweise als Frequenzen angegeben (in der Einheit MHz), während der sichtbare Bereich meist in Wellenlängen angegeben wird (in der Einheit nm oder Angström).  <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/975/975Image_1.png" style="width: 700px;"> Abbildung 1: Teile des elektromagnetischen Spektrums werden in der Reihenfolge zunehmender Frequenz und abnehmender Wellenlänge dargestellt. Die Arten elektromagnetischer Wellen sind Radiowellen, Mikrowellen, infrarote, sichtbare, ultraviolette, Röntgen- und Gammastrahlen. Radiowellen haben die längsten Wellenlängen, die niedrigsten Frequenzen und übertragen die geringste Energiemenge. Sie werden in der Mobilfunktechnik, bei Radio- und Fernsehübertragungen, in der Flugsicherung usw. eingesetzt. Mikrowellen haben im Vergleich zu Radiowellen kürzere Wellenlängen. Sie werden beispielsweise von Wasser aufgenommen und können zum Erhitzen und Kochen von Speisen verwendet werden.  Bei höher Frequenz liegt die Infrarotstrahlung, die von warmen Objekten abgegeben wird. Beispielsweise absorbiert die Erde Strahlungsenergie der Sonne und sendet wiederum Infrarotstrahlung aus. Ein Teil der Infrarotstrahlung wird von der Atmosphäre absorbiert und wieder Richtung Erde abgegeben, so wird durch den Treibhauseffekt die Durchschnittstemperatur der Erde aufrechterhalten. Nachtsichtbrillen erfassen die Infrarotstrahlung, die unser Körper aussendet. Sichtbares Licht ist nur ein winziger Teil der elektromagnetischen Strahlung im Bereich von 740 bis 390 nm.  Das menschliche Auge kann nur diesen kleinen Wellenlängenbereich sehen. Sichtbares Licht besteht hauptsächlich aus sieben Farbkomponenten, darunter Rot, Orange, Gelb, Grün, Blau, Indigo und Violett.  Ultraviolette Strahlung hat Wellenlängen zwischen 400 und 10 nm. Sonnenlicht ist die bekannteste Quelle von UV-Strahlung. Sie enthält außreichend Energie, um bei übermäßiger Exposition zu einem Sonnenbrand zu führen. Röntgenstrahlen können viele Substanzen durchdringen und sind daher ein wichtiges Instrument in verschiedenen bildgebenden Verfahren. Zahnärzte nutzen Röntgenstrahlen zu Diagnosezwecken während das Flughafenpersonal sie nutzt, um beispielsweise den Inhalt eines Koffers sichtbar zu machen. Gammastrahlen haben kleinere Wellenlängen, hohe Frequenzen und hohe Energien. Gammastrahlen werden durch Kernreaktionen und natürlich vorkommende radioaktive Elemente freigesetzt. Röntgen- und Gammastrahlen sind die energiereichsten Formen elektromagnetischer Strahlung. Ihre hohen Energien können Atome und Moleküle ionisieren. Die ionisierende Strahlung kann biologische Moleküle dauerhaft verändern oder schädigen. Sie werden zur Zerstörung von Krebszellen eingesetzt.     Dieser Text wurde angepasst von <a href="https://openstax.org/books/chemistry-2e/pages/6-1-electromagnetic-energy">Openstax, Chemistry 2e, Section 6.1: Electromagnetic Energy.</a>

Das elektromagnetische Spektrum

Das elektromagnetische Spektrum setzt sich aus allen Arten elektromagnetischer Strahlung zusammen, die nach ihrer Frequenz und Wellenlänge angeordnet sind. Jedes der ...

Education

Lehre

JoVE Core

Chemistry

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Electronic Structure of Atoms

Elektronische Struktur von Atomen

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

electromagnetic waves: uses across the spectrum

The electromagnetic spectrum includes all electromagnetic radiation arranged by frequency and wavelength. Visible light is only a small part of it, and each color of visible light has its own frequency and wavelength. Different parts of the spectrum also use different units. Radio waves are usually measured in MHz, while the visible range is often measured in nm or angstroms.

The spectrum is organized from radio waves to gamma rays as frequency increases and wavelength decreases. Radio waves have the longest wavelengths, the lowest frequencies, and the least energy. They are used in cell phones, radio and television broadcasts, and air-traffic control. Microwaves have shorter wavelengths than radio waves and are absorbed by water, which is why they can heat and cook food.

Infrared radiation is next and is emitted by warm objects. The Earth absorbs energy from the Sun and gives off infrared radiation. Some of this radiation is absorbed and re-emitted by the atmosphere, which helps keep Earth’s average temperature stable through the greenhouse effect. Night vision goggles also detect the infrared radiation that our bodies emit.

Visible light spans only about 740 to 390 nm, so the human eye can see just a narrow band of electromagnetic radiation. This band includes red, orange, yellow, green, blue, indigo, and violet. Ultraviolet radiation has wavelengths from about 400 to 10 nm. Sunlight is the most familiar source of UV radiation, and too much exposure can cause sunburn.

X-rays can pass through many materials, so they are useful for imaging. Dentists use x-rays for diagnosis, and airport security uses them to view what is inside a suitcase. Gamma rays have even smaller wavelengths, higher frequencies, and higher energies. They come from nuclear reactions and naturally occurring radioactive elements. X-rays and gamma rays are the most energetic forms of electromagnetic radiation, and their ionizing radiation can damage biological molecules. Because of that, they can be used to destroy cancer cells.

Electromagnetic Waves: Uses Across the Spectrum

electromagnetic-waves-uses-across-the-spectrum

the wave nature of light

Measuring Light with Wavelength and Frequency

Light can be described as an electromagnetic wave, and its behavior helps explain many patterns seen in science. For centuries, scientists have tried to understand light. Newton used lenses and prisms to show that white light is made of the colors of the rainbow mixed together. He explained light as tiny particles moving at high speed. Other scientists, including Christiaan Huygens, showed that reflection and refraction could also be explained by treating light as a wave. At the time, people...

the electromagnetic spectrum

The electromagnetic spectrum includes all electromagnetic radiation arranged by frequency and wavelength. Visible light is only a small part of it, and each color of visible light has its own frequency and wavelength. Different parts of the spectrum also use different units. Radio waves are usually measured in MHz, while the visible range is often measured in nm or angstroms. The spectrum is organized from radio waves to gamma rays as frequency increases and wavelength decreases. Radio waves...

interference and diffraction

Wave Patterns from Light and Slits

Light can form wave patterns through interference and diffraction. When two electromagnetic waves meet with their peaks and troughs lined up, they combine into a larger wave. This is constructive interference, and the waves are in phase. When a peak of one wave meets a trough of the other, the waves reduce each other. This is destructive interference, and the result has a much lower amplitude. Diffraction is another wave behavior. When light passes through a slit that is about the same size as...

photoelectric effect

Why Light Ejects Electrons from Metals

Light can eject electrons from a metal surface when it has the right frequency. This process is called the photoelectric effect. Each metal has its own threshold frequency, which is the minimum light frequency needed to free electrons. Light below the threshold frequency cannot cause emission, even if it is very bright. When the light frequency is above the threshold, electrons are ejected. In that case, the number of electrons released is directly proportional to the intensity, or brightness,...

the bohr model

Bohr’s Quantized Atomic Orbits

Bohr’s quantized atomic orbits explain why hydrogen atoms can stay stable. Early in the twentieth century, Ernest Rutherford and his colleagues described atoms as tiny dense nuclei with lighter electrons moving around them. This picture was called the planetary model because it compared the atom to a miniature solar system, with electrons orbiting the nucleus like planets around the sun. The simplest atom is hydrogen. It has one proton in the nucleus and one electron moving around it. In the...

emission spectra

Line Spectra from Heated Gases

Line spectra are produced when heated gases give off light at specific wavelengths. In contrast, hot solids, liquids, or condensed gases radiate excess energy as a continuous spectrum. That spectrum contains an unbroken range of wavelengths. A gas at low partial pressure can produce a line spectrum when it is excited by an electric current or heated. Fluorescent light bulbs and neon signs work in this way. Each element has its own characteristic set of lines, and molecules can also produce...

the de broglie wavelength

Electron Waves and Standing Orbits

Electron waves and standing orbits explain how tiny particles can behave like waves. Large objects in the macroscopic world, like a billiard ball on a table, follow classical physics. A ball keeps moving in a straight line unless it hits another ball or a force such as friction acts on it. It also has a well-defined position, velocity, and momentum, where momentum is mass times velocity. Waves behave differently from macroscopic particles. When waves interact, they can form interference...

the uncertainty principle

Electron Position and Momentum Limits

Heisenberg’s uncertainty principle sets a limit on how precisely we can know an electron’s position and momentum at the same time. Momentum is the motion of a particle, and the two measurements affect each other. If the momentum is known more accurately, the position becomes less certain, and the reverse is also true. Heisenberg described this limit with an equation that uses Planck’s constant. The equation shows the smallest possible uncertainty for position and momentum together. It explains...

the quantum-mechanical model of an atom

Electron Orbitals in Quantum Mechanics

Quantum mechanics explains how electrons behave in atoms using waves and probability. Erwin Schrödinger built on de Broglie’s idea that an electron in hydrogen could act like a circular standing wave instead of moving in fixed circular paths. He then derived the Schrödinger equation, which became a major step in modern atomic theory. When Schrödinger applied his equation to hydrogen-like atoms, it matched Bohr’s energy expression and the Rydberg formula for hydrogen spectra. He described...

quantum numbers

Electron Orbitals and Spin

Electron orbitals are described by quantum numbers that show where an electron is most likely to be found around the nucleus. These numbers come from the quantum mechanical model, which is based on solutions of the Schrödinger equation. They also help explain why electron energy comes in set values instead of changing smoothly. The principal quantum number, n, labels the energy level. It can be 1, 2, 3, and so on, and higher n values usually mean higher electron energy. This number also tells...

atomic orbitals

Electron Regions in Atomic Orbitals

Electron regions in atomic orbitals show where an electron is most likely to be found in an atom. These three-dimensional regions are often drawn as boundary surfaces around the densest part of the cloud. The shape of an orbital depends on the angular momentum quantum number, l. This value can range from 0 to n - 1, where n is the principal quantum number. For n = 1, only l = 0 is allowed. For n = 2, both l = 0 and l = 1 are allowed. Orbitals with the same value of l form a subshell. The l =...

the pauli exclusion principle

Electron Spin and Orbital Pairing

Electron spin and orbital pairing explain why only two electrons can fit in one atomic orbital. Electron configuration describes how electrons are arranged in an atom’s orbitals. It is written with three parts: the principal quantum number, n, the orbital type, or subshell, and a superscript that shows how many electrons are in that subshell. For example, 2p4 means four electrons in a p subshell with n = 2, and 3d8 means eight electrons in a d subshell with n = 3. The three quantum numbers...

the energies of atomic orbitals

Shielding and Orbital Penetration

Shielding and orbital penetration help explain why electrons in an atom have different energies. Electrons are attracted to the positive nucleus, but they also repel one another in atoms with more than one electron. The strength of these forces depends on the charge and the distance between the particles. Opposite charges attract, like charges repel, and the force gets weaker as the particles move farther apart. An electron that stays closer to the nucleus is held more tightly. That means...

the aufbau principle and hund's rule

Electron Filling Order in Atomic Orbitals

Electron filling order in atomic orbitals follows the aufbau principle and Hund's rule. To write an electron configuration, we build atoms in order of atomic number. Starting with hydrogen and moving across the periods of the periodic table, one proton is added to the nucleus and one electron is placed into the correct subshell. This process describes the ground-state electron configurations of the elements. The aufbau principle comes from the German word aufbau, which means "to build up." It...

electron configuration of multielectron atoms

electron-configuration-of-multielectron-atoms

Valence Electrons and Noble Gas Shorthand

Valence electrons and noble gas shorthand help show how electrons are arranged in multielectron atoms. Sodium, the alkali metal with atomic number 11, has one more electron than neon. That extra electron goes into the lowest-energy subshell available, the 3s orbital, so sodium has the configuration 1s2 2s2 2p6 3s1. Electrons in the outermost shell, where n is highest, are called valence electrons. Electrons in the inner shells are called core electrons. Because core electrons often match a...

key terms and concepts

Explore the electromagnetic spectrum from radio waves to gamma rays, including visible light, infrared, UV, X-rays, and their real-world uses.

Electromagnetic Waves: Uses Across the Spectrum | JoVE K12

chemistry

JoVE Core Chemie erweckt allgemeine Konzepte der Chemie durch kompakte und leicht verständliche animierte Videolektionen zum Leben. Außerdem zeigen wir in den Videos Wissenschaftler in Aktion bei klassischen und neuartigen Forschungsexperimenten, wie sie heutzutage in Laboren weltweit durchgeführt wurden.

Weather and Climate

3.3.9-12.E

Physical Science

Waves and Electromagnetic Radiation

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Louisiana Student Standards for Science

High School

Earth Science

Earth’s Systems

HS-ESS2-4

Tennessee Academic Standards

Physics

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Waves and Their Applications in Technologies for Information Transfer

PHYS.PS4.7

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HS+C.P1U1.2

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New Jersey Student Learning Standards for Science

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Alabama Course of Study Science

Matter and Its Interactions

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Earth's Place in the Universe

9-12.ESS.1.2

9-12.ESS.1.2.a

Next Generation Science Standards

Florida Department of Education

SC.912.E.5

SC.912.E.5.8

SC.912.P.8

SC.912.P.8.3

SC.912.P.10

SC.912.P.10.19

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South Carolina College and Career Ready Science Standards

C-PS4-4

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New York State Science Learning Standards

HS. Chemical Reactions

HS-PS1-7.

HS. Waves and Electromagnetic Radiation

HS-PS4-3.

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Students who demonstrate understanding can develop a model based on evidence of Earth's interior to describe the cycling of matter by thermal convection.  Clarification Statement: Emphasis is on both a one-dimensional model of Earth, with radial layers determined by density, and a three-dimensional model, which is controlled by mantle convection and the resulting plate tectonics.  Examples of evidence include maps of Earth's three-dimensional structure obtained from seismic waves, records of the rate of change of Earth's magnetic field (as constraints on convection in the outer core), and identification of the composition of Earth's layers from high-pressure laboratory experiments.  Assessment Boundary:

3.3.9-12.I

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Students who demonstrate understanding can plan and conduct an investigation of the properties of water and its effects on Earth materials and surface processes. [cite: 44] Clarification Statement: Emphasis is on mechanical and chemical investigations with water and a variety of solid materials to provide the evidence for connections between the hydrologic cycle and system interactions commonly known as the rock cycle. [cite: 45] Examples of mechanical investigations include stream transportation and deposition using a stream table, erosion using variations in soil moisture content, or frost wedging by the expansion of water as it freezes. [cite: 46] Examples of chemical investigations include chemical weathering and recrystallization (by testing the solubility of different materials) or melt generation (by examining how water lowers the melting temperature of most solids). [cite: 47] Assessment Boundary:

3.3.9-12.K

Electromagnetic Waves: Uses Across the Spectrum

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