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

Güneşten gelen ışık, yemek pişirmek için kullanılan mikrodalgalar ve wi-fi yönlendiriciler tarafından yayılan radyo dalgalarının hepsi elektromanyetik radyasyon örnekleridir. Elektromanyetik radyasyon, elektrik yüklü parçacıkların hareketinden gelen enerjinin iletilmesidir. Bu hareket, dalgalar halinde ve birbirine dik şekilde yayılan elektrik ve manyetik alan salınımları yaratır.Tüm dalgalar gibi, elektromanyetik dalgalar da genlikleri, dalga boyları ve frekansları ile karakterize edilir. Tepe genliği, orta hattan bir dalganın tepe veya çukuruna olan mesafedir. Tepe genliği dalganın yoğunluğunu belirler.Örneğin, görünür ışığın genliği parlaklığıyla ilgilidir;genlik ne kadar büyükse, ışık o kadar parlak veya daha yoğun olur. Dalgaboyu, ardışık tepeler veya çukurlar gibi bitişik dalgalar üzerindeki özdeş noktalar arasındaki mesafedir;Yunanca lambda harfi ile sembolize edilir. Elektromanyetik radyasyon, kilometreden pikometreye kadar değişebilen dalga boyuna göre kategorize edilebilir.Örneğin, görünür ışığın dalga boyu aralığı sırasıyla mor ve kırmızı ışığa karşılık gelen yaklaşık 400 ila 750 nanometredir. Yunanca harf nu ile sembolize edilen frekans, bir saniyede bir referans noktasından geçen ve hertz veya döngü saniye cinsinden ölçülen dalga döngülerinin sayısıdır. Dalgaboyu, bir döngünün genişliğidir.Bir dalganın hızı, frekansı ve dalga boyu tarafından belirlenir. Dolayısıyla, bir dalganın frekansı, dalganın hareket ettiği hız ile doğru orantılıdır. Ancak dalganın dalga boyu ile ters orantılıdır.Bu nedenle radyo dalgaları gibi uzun dalga boylu dalgaların frekansları düşüktür. Bu dalgalar, gama ışınları gibi yüksek frekanslı ve kısa dalga boylu dalgalardan daha az enerjiktir.

işığın dalga doğası

Işığın doğası, antik çağlardan beri bir araştırma konusu olmuştur. On yedinci yüzyılda Isaac Newton, mercekler ve prizmalarla deneyler yapmmış ve beyaz ışığın gökkuşağının tek tek renklerinin bir araya getirilmesinden oluştuğunu göstermeyi başarmıştır. Newton, optik bulgularını, ışığın "parçacık" doğası bağlamında, ışığın Newton hareket yasalarına göre yüksek hızlarda hareket eden son derece küçük parçacıkların akışlarından oluştuğu şeklinde açıklamıştır. 
 
 On yedinci yüzyıldaki Christiaan Huygens gibi diğerleri, yansıma ve kırılma gibi optik olayların, tüm uzaya nüfuz ettiği düşünülen "ışık saçan eter" adlı bir ortamda yüksek hızda hareket eden dalgalar ile eşit derecede iyi açıklanabileceğini göstermişlerdi. On dokuzuncu yüzyılın başlarında Thomas Young, dar, yakın aralıklı yarıklardan geçen ışığın Newton parçacıklarıyla açıklanamayan, ancak dalgalar açısından kolayca açıklanabilen girişim desenleri ürettiğini gösterdi. James Clerk Maxwell, elektromanyetik radyasyon teorisini geliştirdikten ve ışığın geniş bir elektromanyetik dalga spektrumunun görünür parçası olduğunu gösterdikten sonra, on dokuzuncu yüzyılın sonlarında, ışığın parçacık doğası tamamen gözden düştü. 
 
 On dokuzuncu yüzyılın sonunda, bilim insanları fiziksel evreni kabaca iki ayrı alan olarak görüyorlardı: Newton'un hareket yasalarına göre hareket eden parçacıklardan oluşan madde ve Maxwell denklemleri tarafından yönetilen dalgalardan oluşan elektromanyetik radyasyon. Günümüzde bu alanlara klasik mekanik ve klasik elektrodinamik (veya klasik elektromanyetizma) adı verilmektedir. Bu çerçevede açıklanamayan birkaç fiziksel fenomen olmasına rağmen, o zamanlar bilim insanları bu çerçevenin genel sağlamlığından o kadar emindiler ki, bu sapmaları nihayetinde bu çerçeve içinde bir şekilde çözülecek kafa karıştırıcı paradokslar olarak gördüler. Bu paradokslar, parçacıkları ve dalgaları, klasik görüşün yerini alan dalga-parçacık ikiliği adı verilen temel bir düzeyde yakından bağlayan çağdaş bir çerçeveye yol açtı.
 
 Görünür ışık ve elektromanyetik radyasyonun diğer biçimleri, atomlar ve moleküller içindeki elektronların enerjilerini çıkarmak için kullanılabildikleri için kimyada önemli rol oynarlar. Örneğin, bir cep telefonundan gelen radyo dalgaları, diş hekimleri tarafından kullanılan X-ışınları, mikrodalgada yemek pişirmek için kullanılan enerji, kırmızı sıcak nesnelerden yayılan ısı ve televizyon ekranınızdan gelen ışık, tümü dalga benzeri davranış sergileyen elektromanyetik radyasyon biçimleridir.
 
 <h4>Dalgalar</h4>
 
 Dalga, enerjiyi uzayda bir noktadan diğerine taşıyabilen bir salınım veya periyodik harekettir. Yaygın dalga örnekleri her yerdedir. Bir ipin ucunu sallamak, elinizden ipin diğer ucuna enerji aktarır, bir gölete bir çakıl taşı düşürmek, dalgaların su yüzeyi boyunca dalgalanmasına neden olur ve bir yıldırım çarpmasına eşlik eden havanın genişlemesi, birkaç kilometre boyunca dışarıya doğru hareket edebilen ses dalgaları (gök gürültüsü) üretir. Bu durumların her birinde, madde esasen yerinde kalırken kinetik enerji madde (halat, su veya hava) yoluyla aktarılır. 
 
 Maddede dolaşmak için dalgaların sınırlandırılmasına gerek yoktur. Maxwell'in gösterdiği gibi, elektromanyetik dalgalar, her ikisi de hareket yönüne dik olan dikey bir manyetik alan ile adım adım salınan bir elektrik alanından oluşur. Bu dalgalar boşlukta, ışık hızı olan (c ile gösterilir) 2,998 × 108 m/sn sabit hızda hareket edebilir.
 
 Elektromanyetik radyasyon formları da dahil olmak üzere tüm dalgalar, bir dalga boyu (λ, küçük Yunan harfi lambda ile gösterilir), bir frekans (ν, küçük Yunan harfi nu ile gösterilir) ve bir genlik ile karakterize edilir. 
 
 Dalgaboyu, bir dalgadaki iki ardışık tepe veya çukur arasındaki mesafedir (SI sisteminde metre cinsinden ölçülür). Elektromanyetik dalgalar, kilometre (103 m) ila pikometre (10−12 m) arasındaki muazzam dalga boyuna sahip dalga boylarıdır. Frekans, uzayda belirli bir noktadan belirli bir sürede geçen dalga döngülerinin sayısıdır (SI sisteminde bu, saniye cinsinden ölçülür). Bir döngü, bir tam dalga boyuna karşılık gelir. Saniyedeki döngü [sn−1] olarak ifade edilen frekans birimi hertz'tir (Hz). Bu birimin ortak katları megahertz (1 MHz = 1 × 106 Hz) ve gigahertz'dir (1 GHz = 1 × 109 Hz). 
 
 Genlik, dalganın yer değiştirmesinin büyüklüğüne karşılık gelir ve bu, tepeler ve çukurlar arasındaki yüksekliğin yarısına karşılık gelir. Genlik, ışık için parlaklık ve ses için ses yüksekliği olan dalganın yoğunluğu ile ilgilidir. Bir dalganın dalga boyu (λ) ve frekansının (ν) çarpımı λν, dalganın hızıdır. Bu nedenle, vakumdaki elektromanyetik radyasyon için hız, temel sabite eşittir, c:
 
 <img alt=""Eq1"" src=""https://www.jovecore.com/CDNSource/lessons/974/974_Equations-01.png"" style=""height: 40px;"" />
 
 Dalgaboyu ve frekans ters orantılıdır: Dalga boyu arttıkça frekans azalır. Elektromanyetik spektrum, her tür elektromanyetik radyasyonun aralığıdır. 
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/6-1-electromagnetic-energy"">Openstax, Chemistry 2e, Section 6.1: Electromagnetic Energy.</a>

Işığın Dalga Doğası

Işığın doğası antik çağlardan beri bir araştırma konusu olmuştur. On yedinci yüzyılda, Isaac Newton lensler ve prizmalarla deneyler yaptı ...

Education

JoVE Core

Chemistry

Kimya

Electronic Structure of Atoms

Atomların Elektronik Yapısı

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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 Kimya, özlü ve kolay anlaşılır animasyon video derslerini kullanarak genel kimya kavramlarına hayat veriyor. Ek olarak, bilim insanı uygulama videolarımız ile klasik ve orijinal araştırma deneylerini dünya çapında günümüz laboratuvarlarında görselleştiriyoruz.

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

The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

Subatomic Particles

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Elements: Chemical Symbols and Isotopes

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Ions and Ionic Charges

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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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Covalent Bonding and Lewis Structures

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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

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

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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 ...

Alkali Metals

Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the ...

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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