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

전자기 스펙트럼은 전자기 복사의 진동수와 해당 파장의 전체 범위를 배열한 것입니다. 파장과 진동수는 서로 반비례합니다. 즉 파장이 길수록 진동수는 낮아집니다.

플랑크의 방정식에서 보여주는 바와 같이 전자파 복사의 에너지는 진동수에 정비례합니다. 따라서 전자파의 에너지가 클수록 파장은 짧아집니다. 전자파는 진동수와 파장에 따라 전파, 마이크로파, 적외선, 가시광선, 자외선, X선 또는 감마선으로 분류됩니다.

통신 시스템 간 신호 전송에 사용되는 전파는 파장이 가장 길고, 진동수가 가장 낮으며, 에너지가 가장 적습니다. 마이크로파는 다음으로 긴 파장을 가지고 있습니다. 사용 범위는 레이더 시스템에서부터 집에서 음식을 가열하는 것까지 다양합니다.

다음은 온도를 가진 물체가 방출하는 열 복사의 중요한 부분이기도 한 적외선입니다. 예를 들어 지구는 태양에서 방출하는 복사 에너지의 일부로 적외선을 흡수하며 또한 우주로 적외선을 방출합니다. 가시광선의 파장은 740에서 390나노미터로 더 짧습니다.

적색 빛은 파장이 가장 길고 보라색은 가장 짧습니다. 인간의 눈은 이 좁은 파장 범위에 대해서만 반응합니다. 자외선은 파장이 더 짧습니다.

태양 빛은 자외선 복사의 가장 잘 알려진 원천으로 과도하게 노출되면 화상을 입고 피부암으로 이어질 만큼 충분한 에너지를 가지고 있습니다. 엑스선과 감마선은 파장이 가장 짧으며 전자기 복사에서 가장 큰 에너지를 가진 형태입니다. 엑스선은 많은 물질을 통과할 수 있지만 뼈는 쉽게 통과하지 못합니다.

이로부터 엑스선은 중요한 이미징 도구가 됩니다. 감마선은 특정 방사성 원소의 붕괴 사슬에서 방출되는 것으로 가장 잘 알려져 있습니다. 감마선과 엑스선 사이에는 보편적인 구분이 없지만 감마선은 일반적으로 가장 짧은 파장 가장 높은 주파수 및 가장 높은 에너지를 갖는 것으로 간주됩니다.

전자기 스펙트럼

전자기 스펙트럼은 주파수와 파장에 따라 배열된 모든 유형의 전자기 방사선으로 구성됩니다. 가시광선의 다양한 색상은 각각 특정 주파수와 파장과 연관되어 있으며 가시광선은 전자기 스펙트럼의 작은 부분만을 차지한다는 것을 알 수 있습니다. 전자기 스펙트럼의 다양한 부분에서 작동하도록 개발된 기술이 다르기 때문에 편의성과 역사적 유산으로 인해 일반적으로 스펙트럼의 다른 부분에 대해 서로 다른 단위가 사용됩니다. 예를 들어, 전파는 일반적으로 주파수(일반적으로 MHz 단위)로 지정되는 반면, 가시 영역은 일반적으로 파장(일반적으로 nm 또는 옹스트롬 단위)으로 지정됩니다.

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/975/975Image_1.png" style="width: 700px;" />

Figure 1: 전자기 스펙트럼의 일부는 주파수가 증가하고 파장이 감소하는 순서로 표시됩니다.

전자기파의 종류에는 전파, 마이크로파, 자외선, 가시광선, 적외선, X선, 감마선이 있습니다.

전파는 가장 긴 파장, 가장 낮은 주파수를 가지며 가장 적은 양의 에너지를 전달합니다. 이는 휴대폰 기술, 라디오 및 TV 방송, 항공 교통 관제 등에 사용됩니다.

마이크로파는 전파에 비해 파장이 짧습니다. 물에 흡수되어 음식을 가열하고 요리하는 데 사용됩니다.

다음은 따뜻한 물체에서 방출되는 적외선입니다. 예를 들어, 지구는 태양으로부터 복사 에너지를 흡수하고 적외선을 방출합니다. 적외선 복사 중 일부는 온실 효과를 통해 지구의 평균 온도를 유지하기 위해 대기에 의해 흡수되고 재방출됩니다. 야간 투시경은 우리 몸에서 방출되는 적외선을 감지합니다.

가시광선은 740~390nm 범위의 전자기 방사선 중 아주 작은 부분에 불과합니다. 인간의 눈은 이 작은 범위의 파장만 볼 수 있습니다. 가시광선은 주로 빨간색, 주황색, 노란색, 녹색, 파란색, 남색, 보라색 등 7가지 색상 구성 요소로 구성됩니다.

자외선은 400~10nm 범위의 파장을 가지고 있습니다. 햇빛은 가장 친숙한 UV 방사선원입니다. 과도한 노출로 인해 일광화상을 일으킬 만큼 충분한 에너지를 전달합니다.

X선은 많은 물질을 통과할 수 있으므로 중요한 영상 도구로 사용됩니다. 치과 의사는 진단 목적으로 엑스레이를 사용하고 공항 보안 검색대에서는 엑스레이를 사용하여 여행 가방에 있는 구성 요소를 시각화합니다.

감마선은 더 작은 파장, 높은 주파수 및 에너지를 가지고 있습니다. 감마선은 핵반응과 자연적으로 발생하는 방사성 원소에 의해 방출됩니다.

X선과 감마선은 전자기 방사선의 가장 강력한 형태입니다. X선과 가마선의 높은 에너지는 원자와 분자를 이온화할 수 있습니다. 이온화 방사선은 생물학적 분자에 영구적인 변화나 손상을 일으킬 수 있습니다. X선과 감마선은 암세포를 파괴하는 데 사용됩니다.

이 문서는 에서 발췌되었습니다 <a href="https://openstax.org/books/chemistry-2e/pages/6-1-electromagnetic-energy">Openstax, Chemistry 2e, Section 6.1: Electromagnetic Energy.</a>

전자기 스펙트럼은 주파수와 파장에 따라 배열된 모든 유형의 전자기 복사로 구성됩니다. 각각의 ...

Education

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Electronic Structure of Atoms

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KEY TERMS AND CONCEPTS

주요 용어 및 개념

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

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Weather and Climate

3.3.9-12.E

Physical Science

Waves and Electromagnetic Radiation

3.2.9-12.X

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

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Alabama Course of Study Science

Matter and Its Interactions

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Earth's Place in the Universe

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Next Generation Science Standards

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SC.912.P.8

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SC.912.P.10.19

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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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Water exists in any one of the three classical states: solid (ice), liquid (water), and gas (steam or water vapor). The state of water depends on i) the ...

The Water Cycle

The Earth&rsquo;s hydrosphere includes all of the areas where the storage and movement of water occurs. Since water is the basis of all living processes, ...

Cohesion

Cohesion is the attraction between molecules of the same type, such as water molecules. Water molecules have an overall neutral charge but are polar ...

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 ...

Chemistry of the Cell

The cell is chemically composed of water, organic molecules and inorganic ions.
Water
The polarity of the water molecule and its resulting hydrogen ...

Water: A Bronsted-Lowry Acid and Base

The reaction between a Br&#248;nsted-Lowry acid and water is called acid ionization. For example, when hydrogen fluoride dissolves in water and ionizes, ...

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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