Name: measuring light with wavelength and frequency
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 2 min 12 s
Channel: JoVE

K12 Standards

Texas Essential Knowledge and Skills

High School

Chemistry and Physics

IPC.7

IPC.7.E

The Wave Nature of Light

Das Licht der Sonne, die Mikrowellen, in denen das Essen gekocht wird, und die von Wi-Fi-Router ausgestrahlten Funkwellen sind alles Beispiele für elektromagnetische Strahlung. Elektromagnetische Strahlung ist die Übertragung der Energie, die aus der Bewegung von elektrischen geladene Teilchen entsteht. Diese Bewegung erzeugt ein senkrechtes Oszillieren elektrischer und magnetischer Felder, die sich im Raum in Form von Wellen ausbreiten.Wie alle Wellen, elektromagnetische Wellen sind durch ihre Amplitude, Wellenlänge, und Frequenz charakterisiert. Die Amplitude ist der Abstand von der Mittellinie bis zum Höhepunkt oder Tiefpunkt einer Welle. Sie bestimmt die Wellenintensität.Zum Beispiel steht die Amplitude des sichtbaren Lichts im Zusammenhang mit seiner Helligkeit;je größer die Amplitude, desto heller oder intensiver ist das Licht. Die Wellenlänge ist der Abstand zwischen identischen Punkten von benachbarte Wellen, wie z. B.aufeinanderfolgende Höhen oder Tiefen;es wird mit dem griechischen Buchstaben Lambda bezeichnet.Elektromagnetische Strahlung kann nach Wellenlänge kategorisiert werden, die von Kilometern bis zu Pikometern reichen kann. Zum Beispiel reicht der Wellenlängenbereich des sichtbaren Lichts etwa 400 bis 750 Nanometer, was violettem bzw. rotem Licht entspricht.Die Frequenz, symbolisiert durch den griechischen Buchstaben nu, ist die Anzahl der Wellenzyklen, die einen Referenzpunkt in einer Sekunde durchlaufen und wird in Hertz oder Zyklen pro Sekunde gemessen. Die Wellenlänge ist die Breite eines Zyklus. Die Geschwindigkeit einer Welle ist das Produkt ihrer Frequenz und Wellenlänge.Daher ist die Frequenz einer Welle direkt proportional zur Geschwindigkeit an dem sich die Welle ausbreitet. Sie ist jedoch umgekehrt proportional zur Wellenlänge der Welle. Daher haben die Wellen mit langen Wellenlängen, wie etwa Radiowellen, niedrige Frequenzen.Diese Wellen sind weniger energiereich als die Wellen mit hohen Frequenzen und kurzen Wellenlängen, wie zum Beispiel Gammastrahlen.

die wellen natur des lichts

Die Natur des Lichts ist seit der Antike Gegenstand wissenschaftlicher Untersuchungen. Im siebzehnten Jahrhundert führte Isaac Newton Experimente mit Linsen und Prismen durch und konnte zeigen, dass weißes Licht aus einer Kombination der einzelnen Farben des Regenbogens besteht. Newton erklärte seine optischen Befunde im Sinne einer "korpuscularen" Sichtweise des Lichts, bei der Licht aus Strömen extrem kleiner Teilchen besteht, die sich mit hoher Geschwindigkeit folgend den Newtons Gesetzen bewegen. Andere Forscher des siebzehnten Jahrhunderts, wie Christiaan Huygens, hatten gezeigt, dass optische Phänomene wie Reflexion und Brechung ebenso gut im Sinne von Licht als Wellen erklärt werden konnten, die sich mit hoher Geschwindigkeit durch ein Medium namens "Aether" ausbreiten, von dem angenommen wurde, dass es den gesamten Raum durchdringt. Anfang des neunzehnten Jahrhunderts zeigte Thomas Young, dass Licht das durch schmale, dicht beieinander liegende Spalten hindurchtritt, Interferenzmuster erzeugt, die nicht im Sinne von Newtonschen Teilchen aber leicht im Sinne von Wellen erklärt werden konnten. Später im neunzehnten Jahrhundert, nachdem James Clerk Maxwell seine Theorie der elektromagnetischen Strahlung entwickelt und gezeigt hatte, dass Licht der sichtbare Teil eines großen Spektrums elektromagnetischer Wellen ist, wurde die Annahme Licht verhalte sich als Teilchen grundlegend diskreditiert. Ende des neunzehnten Jahrhunderts betrachteten Wissenschaftler das physische Universum als in zwei unterschiedliche Bereiche getrennt: Materie, bestehend aus Teilchen, die sich nach Newtons Bewegungsgesetzen bewegen, und elektromagnetische Strahlung, bestehend aus Wellen, die durch Maxwells Gleichungen beschrieben werden können. Heute werden diese Bereiche als klassische Mechanik und klassische Elektrodynamik (oder klassischer Elektromagnetismus) bezeichnet. Obwohl es einige physikalische Phänomene gab, die innerhalb dieses Rahmens nicht erklärt werden konnten, waren die Wissenschaftler zu dieser Zeit so überzeugt von der Gesamtkohärenz dieses Rahmens, dass sie diese Abweichungen als rätselhafte Paradoxe betrachteten, die aber innerhalb dieses Rahmens gelöst werden könnten. Diese Paradoxe führten letztendlich zu einer neuen Synthese der Theorien, die Teilchen und Wellen auf fundamentaler Ebene miteinander verbindet und als Welle-Teilchen-Dualität bezeichnet wird, welche schlussendlich die klassische Ansicht abgelöst hat. Sichtbares Licht und andere Formen elektromagnetischer Strahlung spielen eine wichtige Rolle in der Chemie, da sie verwendet werden können, um die Energien von Elektronen in Atomen und Molekülen zu bestimmen. Ein Großteil unserer modernen Technologie basiert auf der Verwendung elektromagnetischer Strahlung. Zum Beispiel sind Radiowellen von Mobiltelefonen, Röntgenstrahlen, die von Zahnärzten verwendet werden, die Energie, welche in der Mikrowelle zum Kochen von Speisen verwendet wird, die Strahlungswärme von rotglühenden Objekten und das Licht des Fernsehbildschirms Formen elektromagnetischer Strahlung, die alle wellenartiges Verhalten zeigen. <h4>Wellen</h4> Eine Welle ist eine Schwingung oder periodische Bewegung, die Energie von einem Punkt im Raum zu einem anderen transportieren kann. Beispiele für Wellen gibt es überall um uns herum. Wenn zum beispiel das Ende eines Seils geschüttelt wird, wird Energie von der Hand auf das andere Ende des Seils übertragen, wenn man einen Kieselstein in einen Teich fallen lässt, bilden sich Wellen die sich entlang der Wasseroberfläche radial ausbreiten und die Luftausdehnung, die mit der Entladung eines Blitzes einhergeht erzeugt Schallwellen und somit den über mehrere Meilen hörbaren Donner. In jedem dieser Fälle wird kinetische Energie durch Materie (Seil, Wasser oder Luft) übertragen, während die Materie selbst im Wesentlichen an Ort und Stelle bleibt. Wellen müssen nicht auf die Bewegung durch Materie beschränkt sein. Wie Maxwell gezeigt hat, bestehen elektromagnetische Wellen aus einem elektrischen Feld, das im Gleichschritt mit einem senkrechten Magnetfeld schwingt, wobei beide Felder senkrecht zur Ausbreitungsrichtung verlaufen. Durch ein Vakuum bewegen sich diese Wellen mit einer konstanten Geschwindigkeit von 2,998 × 108 m/s, der Lichtgeschwindigkeit (bezeichnet mit c). Alle Wellen, einschließlich Formen elektromagnetischer Strahlung, werden durch eine Wellenlänge (bezeichnet durch λ, der griechische Kleinbuchstabe Lambda), eine Frequenz (bezeichnet durch ν, der griechische Kleinbuchstabe nu) und eine Amplitude charakterisiert. Die Wellenlänge ist der Abstand zwischen zwei aufeinanderfolgenden Spitzen oder Tiefen einer Welle (gemessen in Metern im SI-System). Elektromagnetische Wellen haben Wellenlängen, die in einem enormen Bereich liegen – es werden Wellenlängen von Kilometern (103 m) bis Pikometern (10–12 m) beobachtet. Die Frequenz ist die Anzahl der Wellenzyklen, die in einer bestimmten Zeitspanne einen bestimmten Punkt im Raum passieren (im SI-System wird dies in Sekunden gemessen). Ein Zyklus entspricht einer vollständigen Wellenlänge. Die Einheit für die Frequenz, ausgedrückt in Zyklen pro Sekunde [s−1], ist Hertz (Hz). Gängige Vielfache dieser Einheit sind Megahertz (1 MHz = 1 × 106 Hz) und Gigahertz (1 GHz = 1 × 109 Hz). Die Amplitude entspricht der Größe der Wellenverschiebung, und diese entspricht der Hälfte der Höhe zwischen den Gipfeln und Tälern. Die Amplitude hängt mit der Intensität der Welle zusammen, die bei Licht die Helligkeit und bei Schall die Lautstärke darstellt. Das Produkt aus der Wellenlänge (λ) einer Welle und ihrer Frequenz (ν), λν, ist die Geschwindigkeit der Welle. Für elektromagnetische Strahlung im Vakuum ist die Geschwindigkeit also gleich der Grundkonstante c: <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/974/974_Equations-01.png" style="height: 40px;"> Wellenlänge und Frequenz sind umgekehrt proportional: Mit zunehmender Wellenlänge nimmt die Frequenz ab. Das elektromagnetische Spektrum besteht aus allen Bereichen elektromagnetischer Strahlung.

Die Wellen Natur des Lichts

Die Natur des Lichts ist seit der Antike Gegenstand der Forschung. Isaac Newton führte im siebzehnten Jahrhundert Experimente mit Linsen und Prismen durch ...

Education

Lehre

JoVE Core

Chemistry

Chemie

Eins

Electronic Structure of Atoms

Elektronische Struktur von Atomen

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

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 imagined these waves traveling through a medium called luminiferous aether, which was thought to fill all space. In the early 1800s, Thomas Young showed that light passing through two narrow slits makes an interference pattern. That result fit the wave model much better than the particle model.

James Clerk Maxwell later developed electromagnetic theory and showed that visible light is part of a much larger spectrum of electromagnetic waves. By the end of the nineteenth century, many scientists accepted a split view of the physical world. Matter was described as particles, while electromagnetic radiation was described as waves. These ideas are now called classical mechanics and classical electrodynamics, or classical electromagnetism.

Some experimental results did not fit that classical picture. Scientists first saw them as strange puzzles that might still be solved within the old framework. Those puzzles eventually led to wave-particle duality, a modern idea that links waves and particles at a basic level. This idea replaced the older view.

Electromagnetic radiation matters in chemistry because it can help reveal the energies of electrons in atoms and molecules. It also powers many technologies. Radio waves from a mobile phone, X-rays used by dentists, microwave energy used to cook food, radiant heat from red-hot objects, and the light from a television screen are all forms of electromagnetic radiation. Each of these shows wavelike behavior.

A wave is an oscillation, or repeating motion, that carries energy from one place to another. Rope waves, ripples on water after a pebble falls in, and sound waves from thunder are common examples. In these cases, energy moves through the rope, water, or air while the material itself stays mostly in place. Waves do not have to travel through matter, because electromagnetic waves can move through empty space.

Maxwell showed that electromagnetic waves contain an electric field and a magnetic field that oscillate together. These fields are perpendicular to each other and to the direction the wave travels. In a vacuum, electromagnetic waves move at 2.998 × 10^8 m/s, which is the speed of light, c. Like all waves, they are described by wavelength, frequency, and amplitude.

Wavelength is the distance between two peaks or two troughs. Frequency is the number of wave cycles that pass a point in a given time. Amplitude is the size of the wave’s displacement, which is half the height between a peak and a trough. Amplitude is related to intensity, so for light it affects brightness, and for sound it affects loudness. Wavelength and frequency are linked by the equation λν = speed, so in a vacuum c = λν. As wavelength increases, frequency decreases. Electromagnetic waves span a huge range, from kilometers to picometers, and the full set is called the electromagnetic spectrum.

Measuring Light with Wavelength and Frequency

measuring-light-with-wavelength-and-frequency

the wave nature of light

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

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...

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 light as an electromagnetic wave, including wavelength, frequency, amplitude, the speed of light, and examples from the electromagnetic spectrum.

Measuring Light with Wavelength and Frequency | 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.

Pennsylvania State Academic Standards

9-12

Earth and Space Science

Earth's Systems

3.3.9-12.H

Space Systems

3.3.9-12.B

Weather and Climate

3.3.9-12.E

Physical Science

Waves and Electromagnetic Radiation

3.2.9-12.X

Louisiana Student Standards for Science

Earth Science

Earth’s Place In The Universe

HS-ESS1-1

HS-ESS1-2

Earth’s Systems

HS-ESS2-4

Energy

HS-PS3-3

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Physics

Waves

Light phenomena

Tennessee Academic Standards

waves-and-their-applications-in-technologies-for-information-transfer

Waves and Their Applications in Technologies for Information Transfer

PHYS.PS4.7

CHEM1.PS4.1

Virginia  Standards of Learning

HIgh School

ES.2

ES.2.a

Arizona Science Standards

HS+C.P1

HS+C.P1U1.2

CHEM.6

CHEM.6.C

Alabama Course of Study Science

Matter and Its Interactions

9-12.C.1.1.c

Earth's Place in the Universe

9-12.ESS.1.2

9-12.ESS.1.2.a

9-12.ESS.1.2.b

Next Generation Science Standards

HS-PS4-1

HS-PS4-3

Earth’s Place in the Universe

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.12

SC.912.P.12.7

PHYS.9

PHYS.9.A

PHYS.9.C

PHYS.9.D

south-carolina-college-and-career-ready-science-standards

South Carolina College and Career Ready Science Standards

C-PS4-4

P-PS3-3

P-PS4-1

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Chemical Reactions

HS-PS1-7.

HS. Waves and Electromagnetic Radiation

HS-PS4-3.

The Atomic Theory of Matter

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Molar Mass

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Periodic Classification of the Elements

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Types of Chemical Bonds

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Ionic Bonding and Electron Transfer

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The Born-Haber Cycle

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Trends in Lattice Energy: Ion Size and Charge

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Covalent Bonding and Lewis Structures

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Electronegativity

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Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

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lewis-structures-of-molecular-compounds-and-polyatomic-ions

Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

Bond Energies and Bond Lengths

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Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Dr&#xFC;de called the ...

Model basic atomic structure and relate an element's atomic structure to its bonding, reactivity, and placement on the Periodic Table.

IPC.7.A

physical-and-chemical-properties-of-matter

Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Use patterns within the Periodic Table to predict the relative physical and chemical properties of elements.

IPC.7.B

Science concepts. The student knows that relationships exist between the structure and properties of matter. The student is expected to:

Measuring Light with Wavelength and Frequency

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