Name: atomic orbitals and quantum numbers
Uploaded: 2023-04-30T18:28:31.000Z
Duration: 2 min 28 s
Channel: JoVE

K12 Standards

Louisiana Student Standards for Science

High School

Chemistry

Matter And Its Interactions

HS-PS1-1

Electronic Structure of Atoms

An atom is made of three subatomic particles &#8211; electrons, protons, and neutrons. Positively charged protons and electrically neutral neutrons constitute the atomic nucleus, where all of the positive charge and most of the mass of an atom reside.
Electrons are the negatively charged, low-mass constituents located in the empty space around the nucleus. An atom is electrically neutral when it has as many electrons as protons.
Electrons exhibit a dual nature &#8212; particle and wave. Their location in space and their energy are complementary properties. Therefore, for an electron with a well-defined energy, its position is uncertain.
The quantum mechanical model of an atom predicts that the probability of finding an electron of a given energy in a three dimensional region in space can be determined from the square of the wavefunction expressing the electron&#39;s wavelike nature, also called the electron probability density.
A function describing the probable spatial location of an electron of specific energy in an atom is called an atomic orbital.
Each orbital corresponds to a unique combination of three quantum numbers. The principal quantum number, n, groups orbitals into energy levels&#160;or shells.
The angular momentum, or azimuthal, quantum number, l, groups orbitals within shells into subshells. Each value of l corresponds to either an s, p, d, or f orbital of varying shape.
Some orbital shapes may have multiple possible orientations, each associated with a magnetic quantum number, ml. The number of orientations for a given subshell is equal to two-l plus one.
The fourth quantum number &#8212; the spin quantum number, ms &#8212; is associated with the electrons occupying an orbital and has only two possible values: &#8216;plus one-half&#8217; and &#8216;minus one-half&#8217;. This ensures that no two electrons in an atom have the same values for all four quantum numbers.
Overlaying the orbitals on top of one another produces a roughly spherical shape, like a &#8216;cloud&#8217; of electrons surrounding the nucleus. This is why atoms are generally represented as spheres.

elektronische structuur van atomen

Een atoom bestaat uit protonen en neutronen, die zich in de dichte, centrale kern bevinden, met elektronen rondom de kern. Rekening houdend met de golf-deeltjesdualiteit van elektronen en de onzekerheid in de positie rond de kern, biedt de kwantummechanica een nauwkeuriger model voor de atomaire structuur. Het beschrijft atomaire orbitalen als de gebieden rond de kern waar elektronen met discrete energie aanwezig zijn, gekarakteriseerd door vier kwantumgetallen: n, l, ml, en ms.


 Kwantummechanisch model


 Een atoom bestaat uit een kleine, positief geladen kern omgeven door elektronen. De kern bevat protonen en neutronen. Protonen hebben een lading van +1 en een massa van 1,0073 amu. Neutronen hebben geen lading en een massa van 1,0087 amu. Elektronen hebben een lading van −1 en een massa van 0,00055 amu. Het aantal protonen in de kern wordt het atoomnummer (Z) genoemd en definieert de elementaire identiteit van een atoom. De som van het aantal protonen en neutronen in de kern wordt het massagetal genoemd en, uitgedrukt in amu, is dit ongeveer gelijk aan de massa van het atoom. Een atoom is neutraal wanneer het gelijke aantallen elektronen en protonen bevat.


 Er werden verschillende modellen voorgesteld om de atomaire structuur te beschrijven en de verdeling van elektronen rondom de kern te verklaren. De Broglie-relatie kwantificeerde dat elektronen zowel eigenschappen van een deeltje als van een golf bezitten. Dit verder te kwantificeren, gaf Heisenberg het onzekerheidsprincipe: de positie (die verband houdt met de deeltjesnatuur) en de snelheid of energie (die verband houdt met de golfnatuur) van het elektron kunnen niet tegelijkertijd met volledige precisie worden bepaald. Het kwantummechanisch model biedt een nauwkeuriger beeld van de atomaire structuur. Het beschrijft de driedimensionale positie van een elektron met een specifieke energie, die in een atoom is opgesloten, op een probabilistische manier in termen van het kwadraat van de golffunctie, ψ2. Atoomgolffuncties, of atomaire orbitalen, beschrijven de gebieden in een atoom waar elektronen het meest waarschijnlijk worden aangetroffen.


 Een atomaire orbitaal wordt gekarakteriseerd door drie kwantumgetallen. Het hoofdkwantumgetal, n, groepeert orbitalen op basis van de locatie van het energieniveau, of ‘schil’. Het impulsmoment of azimutale kwantumgetal, l, groepeert de orbitalen op basis van hun vormen in ‘subschillen’. Het heeft gehele waarden van 0 tot n – 1 en wordt weergegeven door letters: s (l = 0), p (l = 1), d (l = 2), f (l = 3), g (l = 4), en h (l = 5). Het magnetische kwantumgetal, ml, met 2l + 1 waarden variërend van –l tot +l, beschrijft de oriëntatie van de orbitaal in de ruimte. Daarnaast heeft elk elektron een spinkwantumgetal, ms, dat gelijk kan zijn aan ±1/2. Geen twee elektronen in hetzelfde atoom kunnen dezelfde reeks waarden hebben voor alle vier de kwantumgetallen.


Deze tekst is aangepast van<a href="https://openstax.org/books/chemistry-2e/pages/6-3-development-of-quantum-theory#0"> Openstax, Chemistry 2e, Section 6</a>.

Elektronische structuur van atomen


An atom comprises protons and neutrons, which are contained inside the dense, central&#160;core called the nucleus, with electrons present around the ...

Education

JoVE Core

Organic Chemistry

Organische chemie

Unit 1

Onderdeel 1

Covalent Bonding and Structure

Covalente binding en structuur

KEY TERMS AND CONCEPTS

BELANGRIJKE TERMEN EN CONCEPTEN

atomic orbitals and quantum numbers

Atomic orbitals and quantum numbers describe how electrons are arranged around the nucleus. An atom has a small, positively charged nucleus with electrons surrounding it. The nucleus contains protons and neutrons, and the quantum mechanical model gives a better picture of this structure than older models.

Protons carry a +1 charge and have a mass of 1.0073 amu. Neutrons have no charge and have a mass of 1.0087 amu. Electrons carry a −1 charge and have a mass of 0.00055 amu. The number of protons is the atomic number, Z, and it defines the element. The total number of protons and neutrons is the mass number, and it is approximately equal to the atom’s mass in amu. An atom is neutral when it has equal numbers of protons and electrons.

The quantum model grew from ideas about electron behavior. The de Broglie relation showed that electrons act like both particles and waves. Heisenberg’s uncertainty principle added that an electron’s position and its velocity or energy cannot both be known with full precision at the same time. Because of this, electron location is described in a probabilistic way using the square of the wavefunction, ψ².

Atomic wavefunctions, or atomic orbitals, show the regions where electrons are most likely to be found. Orbitals are described by four quantum numbers. The principal quantum number, n, gives the energy level or shell. The angular momentum, or azimuthal, quantum number, l, describes orbital shape and forms subshells. Its values run from 0 to n − 1, and the labels are s, p, d, f, g, and h for l = 0 through 5.

The magnetic quantum number, ml, describes how an orbital is oriented in space. It has 2l + 1 possible values, ranging from −l to +l. The spin quantum number, ms, can be +1/2 or −1/2. No two electrons in the same atom can have the same set of values for all four quantum numbers.

Atomic Orbitals and Quantum Numbers

what is organic chemistry?

Carbon Compounds in Everyday Life

Organic chemistry focuses on carbon compounds called organic compounds. These compounds may come from living things or be made by chemists. Carbon is the main element in them, and it bonds with other carbon atoms as well as hydrogen, oxygen, nitrogen, and sulfur. Carbon can form up to four strong bonds. That ability lets carbon atoms build chains and rings of many sizes, shapes, and levels of complexity. Not every carbon-containing substance is classified as organic. Carbonates, cyanides, and...

electronic structure of atoms

Atomic orbitals and quantum numbers describe how electrons are arranged around the nucleus. An atom has a small, positively charged nucleus with electrons surrounding it. The nucleus contains protons and neutrons, and the quantum mechanical model gives a better picture of this structure than older models. Protons carry a +1 charge and have a mass of 1.0073 amu. Neutrons have no charge and have a mass of 1.0087 amu. Electrons carry a −1 charge and have a mass of 0.00055 amu. The number of...

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chemical bonds

Chemical Bonds: Types and Strength

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Electronegativity in Polar Covalent Bonds

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lewis structures and formal charges

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Resonance in Nitrite and Carbonate Ions

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Covalent Bond Overlap and Orbital Hybridization

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mo theory and covalent bonding

Bond Order and Molecular Orbitals

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intermolecular forces and physical properties

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introduction to functional groups

Functional Groups and Organic Molecules

Functional groups are groups of atoms with specific chemical properties that appear within organic molecules. They are sometimes shown as "R." These groups sit along the carbon backbone of macromolecules, which can form chains or rings of carbon atoms. Functional groups help functionalize a compound. That means they can give the molecule different physical and chemical properties. In organic chemistry, this change in group structure can strongly affect how a compound behaves. Common...

overview of advanced functional groups

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Atomic Orbitals and Quantum Numbers | JoVE K12

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Virginia  Standards of Learning

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Physical Science

Matter and Its Interactions

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SC.912.P.8

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South Carolina College and Career Ready Science Standards

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Physics

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Chemical Bonds


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HS-PS1-4

Atomic Orbitals and Quantum Numbers

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