Name: line spectra from heated gases
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 2 min 39 s
Channel: JoVE

K12 Standards

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NC K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.1.4

Emission Spectra

Когда атом поглощает энергию, электроны возбуждаются и переходят на более высокий энергетический уровень. Когда электроны релаксируют либо до состояния с более низкой энергией, либо до основного состояния, избыточная энергия выделяется в виде фотона. Длина волны поглощенного и испускаемого света зависит от разницы между высоким и низким уровнями энергии.Излучаемый свет с высокой энергией является результатом релаксации электронов с более высокого энергетического уровня, а излучаемый свет с низкой энергией возникает в результате релаксации электронов с более низкого энергетического уровня. Спектр излучения это мера испускаемого излучения в диапазоне длин волн. В случае чистых элементарных частиц поведение излучения проявляется в виде линий с определенной длиной волны, а не в виде широкого спектра.Это спектр излучения водорода. Набор спектральных линий в области видимого света известен как серия Бальмера. Это происходит, когда электроны переходят с энергетического уровня выше n 3 обратно на n 2.Спектр видимого света выглядит как спектральные линии с длиной волны 410, 434, 486 и 656 нанометров, которые соответствуют переходам энергетических уровней с n 3, 4, 5 и 6 соответственно на n 2. За пределами видимого диапазона могут быть измерены дополнительные спектральные линии, например серия Лаймана в УФ-области и серия Пашена в инфракрасной области. Длины волн спектральных линий для водорода можно предсказать с помощью математического выражения, где RH постоянная Ридберга, n1 главное квантовое число нижнего энергетического уровня, а n2 главное квантовое число для более высокого энергетического уровня.Для серии Бальмера n1 2. Поскольку разные атомы имеют разные уровни энергии, спектральные линии излучения варьируются от элемента к элементу и используются для идентификации веществ. Спектр, обратный спектру излучения, это спектр поглощения.Если посмотреть на водород, то линии в его спектре поглощения расположены на тех же длинах волн, что и его спектр излучения, однако они темные. Это длины световых волн, которые поглощаются атомом водорода, когда он подвергается воздействию непрерывного спектра белого света.

Спектры излучения

Когда твердые вещества, жидкости или конденсированные газы достаточно нагреваются, они излучают часть избыточной энергии в виде света. Фотоны, производимые таким образом, обладают рядом энергий, и, таким образом, создают непрерывный спектр, в котором присутствует неразорвана серия длин волн. 
 
 В отличие от непрерывных спектров, свет может также иметь дискретные или линейные спектры с очень узкими линейными значениями, которые чередуются по спектральным областям. При возбуждении газа при низком частичном давлении с использованием электрического тока или нагревании он будет генерировать линейные спектры. Таким образом работают флуоресцентные лампы и неоновые знаки. Каждый элемент отображает свой собственный набор линий, как и молекулы, хотя их спектры, как правило, намного сложнее. 
 
 Каждая линия излучения состоит из одной длины волны света, что означает, что свет, излучаемый газом, состоит из набора дискретных энергий. Например, когда электрический разряд проходит через трубку, содержащую газообразный водород при низком давлении, молекулы H2 разбиваются на отдельные атомы H, и наблюдается синих-розовый цвет. Прохождение света через призму создает линейный спектр, указывающий на то, что этот свет состоит из фотонов четырех видимых длин волн. 
 
 Происхождение дискретных спектров в атомах и молекулах было чрезвычайно озадачено ученым в конце девятнадцатого века. Согласно классической электромагнитной теории, следует наблюдать только непрерывные спектры. Другие дискретные линии для атома водорода были обнаружены в УФ- и ИК-областях. Йоханнес Ридберг обобщала работу Балмера и разработала эмпирическую формулу, которая предсказывала все линии выбросов водорода, а не только те, которые ограничены видимым диапазоном, где n1 и n2 являются целыми числами n1 < n2 
 
 <img alt=""Eq1"" src=""https://www.jove.com/files/core/CDNSource/lessons/977/977_Equations-01.png"" style=""height: 40px;"" />
 
 Даже в конце девятнадцатого века спектроскопия была очень точной наукой, и поэтому длины волн водорода измерялись c очень высокой аккуратностью, что подразумевало, что константу Ридберга можно было определить очень точно. Такая простая формула, как формула Ридберга, могла бы в то время учитывать такие точные измерения, казалась поразительной, но именно окончательное объяснение спектров излучения Нильсом Бором в 1913 году убедило ученых отказаться от классической физики и стимулировало развитие современной квантовой механики. 
 
 Этот текст адаптирован из <a href=""https://openstax.org/books/chemistry-atoms-first-2e/pages/3-1-electromagnetic-energy"">Openstax, Химия 2е изд., раздел 3.1: Электромагнитная энергия</a>.

Когда твердые тела, жидкости или конденсированные газы нагреваются достаточно, они излучают часть избыточной энергии в виде света. Фотоны, полученные таким образом, обладают ...

Education

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Chemistry

Химия

Один

Electronic Structure of Atoms

Электронное строение атомов

KEY TERMS AND CONCEPTS

ОСНОВНЫЕ ТЕРМИНЫ И ПОНЯТИЯ

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 line spectra, although their patterns are usually more complex.

Each emission line is a single wavelength of light. That means the light from a gas is made of discrete energies rather than a smooth spread of values. A good example is hydrogen gas in an electric discharge tube. The H2 molecules break apart into separate H atoms, and the gas gives off a blue-pink color.

When that light is passed through a prism, it separates into a line spectrum. For hydrogen, this shows four visible wavelengths. Scientists also found other hydrogen lines in the ultraviolet and infrared regions. In the late nineteenth century, these discrete spectra were hard to explain because classical electromagnetic theory predicted only continuous spectra.

Johannes Rydberg extended Balmer's work and wrote an empirical formula that predicted all of hydrogen's emission lines, not just the visible ones. The wavelengths of hydrogen were measured with high accuracy, so the Rydberg constant could also be determined very precisely. Later, Niels Bohr explained emission spectra in 1913. His explanation helped push scientists away from classical physics and toward modern quantum mechanics.

Line Spectra from Heated Gases

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

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 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

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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 how heated gases produce line spectra, why hydrogen shows discrete wavelengths, and how Rydberg and Bohr helped explain emission lines.

Line Spectra from Heated Gases | JoVE K12

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Classifying Matter by State

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Phase Transitions: Sublimation and Deposition

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Heating and Cooling Curves

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Physical and Chemical Properties of Matter

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Physical Properties of Matter

A physical property is ...

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Molecular Comparison of Gases, Liquids, and Solids

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Intermolecular vs Intramolecular Forces

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Intermolecular Forces

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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

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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 ...

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Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

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Following the work of Ernest Rutherford and his colleagues in the early twentieth century, the picture of atoms consisting of tiny dense nuclei surrounded ...

Use models to interpret the data presented in Bohr diagrams and electron dot diagrams for neutral atoms of elements 1 through 18.

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Line Spectra from Heated Gases

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