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

Un atome est composé de trois particules subatomiques : les électrons, les protons et les neutrons. Les protons chargés positivement et les neutrons électriquement neutres constituent le noyau atomique, où résident toute la charge positive et la majeure partie de la masse d’un atome.
Les électrons sont les constituants de faible masse chargés négativement situés dans l’espace vide autour du noyau. Un atome est électriquement neutre lorsqu’il a autant d’électrons que de protons.
Les électrons présentent une double nature : particule et onde. Leur localisation dans l’espace et leur énergie sont des propriétés complémentaires. Par conséquent, pour un électron avec une énergie bien définie, sa position est incertaine.
Le modèle de mécanique quantique d'un atome prédit que la probabilité de trouver un électron d'une énergie donnée dans une région tridimensionnelle de l'espace peut être déterminée à partir du carré de la fonction d'onde exprimant la nature ondulatoire de l'électron, également appelée densité de probabilité d'électron.
Une fonction décrivant l’emplacement spatial probable d’un électron d’énergie spécifique dans un atome est appelée orbitale atomique.
Chaque orbitale correspond à une combinaison unique de trois nombres quantiques. Le nombre quantique principal, n, regroupe les orbitales en niveaux d’énergie ou couches.
Le moment angulaire, ou azimutal, nombre quantique, l, regroupe les orbitales à l’intérieur des couches en sous-couches. Chaque valeur de l correspond à une orbitale s, p, d ou f de forme variable.
Certaines formes orbitales peuvent avoir plusieurs orientations possibles, chacune associée à un nombre quantique magnétique, ml. Le nombre d’orientations pour une sous-couche donnée est égal à deux-l plus un.
Le quatrième nombre quantique — le nombre quantique de spin, ms — est associé aux électrons occupant une orbitale et n’a que deux valeurs possibles : « plus un demi » et « moins un demi ». Cela garantit qu’il n’y a pas deux électrons dans un atome qui ont les mêmes valeurs pour les quatre nombres quantiques.
La superposition des orbitales les unes sur les autres produit une forme à peu près sphérique, comme un « nuage » d’électrons entourant le noyau. C’est pourquoi les atomes sont généralement représentés sous forme de sphères.

structure électronique des atomes

Un atome est constitué de protons et de neutrons, contenus à l'intérieur du noyau dense et central appelé noyau, avec des électrons présents autour du noyau. En tenant compte de la dualité onde-particule des électrons et de l'incertitude de leur position autour du noyau, la mécanique quantique fournit un modèle plus précis pour la structure atomique. Elle décrit les orbitales atomiques comme les régions autour du noyau où les électrons d'énergie discrète existent, caractérisées par quatre nombres quantiques : n, l, ml, et ms.

<h4>Modèle mécanique quantique</h4>

Un atome se compose d'un petit noyau chargé positivement entouré d'électrons. Le noyau contient des protons et des neutrons. Les protons ont une charge de +1 et une masse de 1,0073 u. Les neutrons ont une charge nulle et une masse de 1,0087 u. Les électrons ont une charge de -1 et une masse de 0,00055 u. Le nombre de protons dans le noyau est appelé numéro atomique (Z) et définit l'identité élémentaire d'un atome. La somme des nombres de protons et de neutrons dans le noyau est appelée numéro de masse et, exprimée en u, est approximativement égale à la masse de l'atome. Un atome est neutre lorsqu'il contient un nombre égal d'électrons et de protons.

Divers modèles ont été proposés pour décrire la structure atomique en expliquant la distribution des électrons autour du noyau. La relation de de Broglie a quantifié que les électrons ont des propriétés à la fois de particule et d'onde. En quantifiant cette dualité onde-particule plus loin, Heisenberg a donné le principe d'incertitude : la position (associée à la nature de particule) et la vitesse ou l'énergie (associée à la nature d'onde) de l'électron ne peuvent être déterminées simultanément avec une précision totale. Le modèle mécanique quantique donne une image plus précise de la structure atomique. Il décrit la position tridimensionnelle d'un électron avec une énergie spécifique, contenue dans un atome, de manière probabiliste en termes du carré de la fonction d'onde, ψ2. Les fonctions d'onde atomiques, ou orbitales atomiques, décrivent les régions dans un atome où les électrons sont les plus susceptibles d'être trouvés.

Une orbitale atomique est caractérisée par trois nombres quantiques. Le nombre quantique principal, n, regroupe les orbitales en termes de niveau d'énergie, ou « couche ». Le nombre quantique de moment angulaire ou azimutal, l, regroupe les orbitales en fonction de leur forme dans des « sous-couches ». Il a des valeurs entières de 0 à n - 1 et est représenté par des lettres : s (l = 0), p (l = 1), d (l = 2), f (l = 3), g (l = 4), et h (l = 5). Le nombre quantique magnétique, ml, avec 2l + 1 valeurs allant de -l à +l, décrit l'orientation de l'orbitale dans l'espace. De plus, chaque électron a un nombre quantique de spin, ms, qui peut être égal à ±1/2. Deux électrons d’un même atome ne peuvent avoir le même ensemble de valeurs pour les quatre nombres quantiques.

Ce texte est adapté de<a href="https://openstax.org/books/chemistry-2e/pages/6-3-development-of-quantum-theory#0"> Openstax, Chemistry 2e, Section 6</a>

Structure électronique des atomes


Un atome comprend des protons et des neutrons, qui sont contenus à l’intérieur du noyau central dense appelé noyau, avec des électrons présents autour du ...

Education

Enseignement

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Organic Chemistry

Chimie organique

Unit 1

Unité 1

Covalent Bonding and Structure

Liaison covalente et structure

KEY TERMS AND CONCEPTS

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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...

electron configurations

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chemical bonds

Chemical Bonds: Types and Strength

Chemical bonds help atoms reach a full valence shell like the nearest noble gas. The main bond types are ionic, covalent, and metallic. Bond energy and bond length also help explain how strong a bond is. An ionic bond forms from electrostatic attraction between cations and anions. In many cases, one atom transfers electrons to another atom, and the ions form from that transfer. Ionic bonds have no defined direction because the attraction spreads evenly through three-dimensional space. A...

polar covalent bonds

Electronegativity in Polar Covalent Bonds

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lewis structures and formal charges

Lewis Structures, Bonds, and Formal Charge

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vsepr theory

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molecular geometry and dipole moments

Predicting Shape and Molecular Polarity

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resonance and hybrid structures

Resonance in Nitrite and Carbonate Ions

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Covalent Bond Overlap and Orbital Hybridization

Covalent bonds form when orbitals on two atoms overlap and their single electrons pair up. The bond is stronger when the overlap is greater. Maximum overlap happens when the orbitals meet along a direct line between the two nuclei. A sigma bond, or σ bond, is the kind of covalent bond found in a single bond in a Lewis structure. In a σ bond, electron density is concentrated along the internuclear axis. A pi bond, or π bond, forms when two p orbitals overlap side by side. In a π bond, the...

mo theory and covalent bonding

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Molecular orbital theory explains how electrons are arranged in molecules. It treats electron regions in a molecule much like atomic orbitals in an atom. A molecular orbital is the region of space where a valence electron is most likely to be found. Molecular orbitals form through the linear combination of atomic orbitals, or LCAO. When atomic wave functions combine in phase, they create regions with high electron density. When they combine out of phase, they create nodes, or regions with no...

intermolecular forces and physical properties

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solubility

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Solution formation depends on how solutes and solvents interact. A solution is a homogeneous mixture made of a solvent, which is the larger part, and a solute, which is the smaller part. The physical state of a solution is usually the same as the solvent. Concentration is often described as dilute for a low amount of solute or concentrated for a high amount of solute. When a solute dissolves, its particles are surrounded by solvent species. This process is called solvation. If water is the...

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

Advanced Functional Groups in Organic Chemistry

Advanced functional groups are atom clusters in organic molecules that give those molecules specific chemical properties. They are sometimes shown as "R" in formulas. By changing the atoms attached to a carbon skeleton, a functional group can make a compound behave differently in physical and chemical reactions. This topic covers several major classes of organic compounds with advanced functional groups. Aromatic hydrocarbons include benzene. Phenol is another example and is also called...

key terms and concepts

Learn how atomic orbitals, shells, subshells, and the four quantum numbers describe electron arrangement in atoms through the quantum mechanical model.

Atomic Orbitals and Quantum Numbers | JoVE K12

organic chemistry

JoVE Core Chimie Organique explique les concepts de base de la stéréochimie, des réactions et des mécanismes à l'aide de leçons vidéo animées concises et faciles à comprendre. De plus, les vidéos de scientifiques à l'action présentent l'application de ces concepts grâce à des expériences de recherche classiques et originales réalisées dans des laboratoires modernes.

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Motion And Stability: Forces And Interactions

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Matter and Its Interactions

Florida Department of Education

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South Carolina College and Career Ready Science Standards

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Atomic Orbitals and Quantum Numbers

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