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

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Louisiana Student Standards for Science

High School

Chemistry

Matter And Its Interactions

HS-PS1-1

Electronic Structure of Atoms

Un átomo está formado por tres partículas subatómicas: electrones, protones y neutrones. Los protones cargados positivamente y los neutrones eléctricamente neutros constituyen el núcleo atómico, donde reside toda la carga positiva y la mayor parte de la masa de un átomo.
Los electrones son los constituyentes cargados negativamente y de baja masa ubicados en el espacio vacío alrededor del núcleo. Un átomo es eléctricamente neutro cuando tiene tantos electrones como protones.
Los electrones exhiben una naturaleza dual: partícula y onda. Su ubicación en el espacio y su energía son propiedades complementarias. Por lo tanto, para un electrón con una energía bien definida, su posición es incierta.
El modelo mecánico cuántico de un átomo predice que la probabilidad de encontrar un electrón de una energía dada en una región tridimensional en el espacio se puede determinar a partir del cuadrado de la función de onda que expresa la naturaleza ondulatoria del electrón, también llamada densidad de probabilidad electrónica.
Una función que describe la ubicación espacial probable de un electrón de energía específica en un átomo se llama orbital atómico.
Cada orbital corresponde a una combinación única de tres números cuánticos. El número cuántico principal, n, agrupa los orbitales en niveles de energía o capas.
El momento angular, o número cuántico azimutal, l, agrupa los orbitales dentro de las capas en subcapas. Cada valor de l corresponde a un orbital s, p, d o f de forma variable.
Algunas formas orbitales pueden tener múltiples orientaciones posibles, cada una asociada con un número cuántico magnético, ml. El número de orientaciones para una subcapa dada es igual a dos l más uno.
El cuarto número cuántico, el número cuántico de espín, ms, está asociado con los electrones que ocupan un orbital y solo tiene dos valores posibles: 'más un medio' y 'menos un medio'. Esto asegura que no haya dos electrones en un átomo que tengan los mismos valores para los cuatro números cuánticos.
La superposición de los orbitales uno encima del otro produce una forma más o menos esférica, como una "nube" de electrones que rodea el núcleo. Esta es la razón por la que los átomos se representan generalmente como esferas.

estructura electrónica de los átomos.

Un átomo se compone de protones y neutrones, que están contenidos dentro de una densidad , llamado núcleo, con electrones presentes alrededor del núcleo. Teniendo en cuenta la dualidad onda-partícula de los electrones y la incertidumbre en la posición alrededor del núcleo, la mecánica cuántica proporciona un modelo más preciso de la estructura atómica. Describe los orbitales atómicos como las regiones alrededor del núcleo donde existen electrones con energía discreta, caracterizados por cuatro números cuánticos: n, l, m_l y m_s.

Modelo mecánico cuántico
Un átomo consta de un pequeño núcleo cargado positivamente rodeado de electrones. El núcleo contiene protones y neutrones. Los protones tienen una carga de +1 y una masa de 1,0073 uma. Los neutrones tienen carga cero y una masa de 1,0087 uma. Los electrones tienen una carga de −1 y una masa de 0,00055 uma. El número de protones en el núcleo se llama número atómico (Z) y define la identidad elemental de un átomo. La suma del número de protones y neutrones en el núcleo se llama número de masa y, expresada en uma, es aproximadamente igual a la masa del átomo. Un átomo es neutro cuando contiene igual número de electrones y protones.
Se propusieron varios modelos para describir la estructura atómica y explicar la distribución de los electrones alrededor del núcleo. La ecuación de De Broglie cuantificó que los electrones tienen propiedades tanto de partícula como de onda. Al cuantificar aún más esta dualidad onda-partícula, Heisenberg dio el principio de incertidumbre: la posición (asociada con la naturaleza de la partícula) y la velocidad o la energía (asociada con la naturaleza ondulatoria) del electrón no pueden determinarse simultáneamente con total precisión. El modelo de mecánica cuántica ofrece una imagen más precisa de la estructura atómica. Describe la posición tridimensional de un electrón con una energía específica, contenido en un átomo, de manera probabilística en términos del cuadrado de la función de onda, ψ^2. Las funciones de onda atómicas, u orbitales atómicos, describen las regiones de un átomo donde es más probable que se encuentren electrones.
Un orbital atómico se caracteriza por tres números cuánticos. El número cuántico principal, n, agrupa los orbitales en términos de ubicación del nivel de energía, o "capa". El momento angular o número cuántico azimutal, agrupa los orbitales según sus formas en "subcapas". Tiene valores enteros del 0 al n – 1 y se representa con las letras: s (l = 0), p (l = 1), d (l = 2), f (l = 3), g (l = 4) y h (l = 5). El número cuántico magnético, m_l, con valores 2l + 1 que van de –l a +l, describe la orientación del orbital en el espacio. Además, cada electrón tiene un número cuántico de espín, m_s, que puede ser igual a ±1/2. No hay dos electrones en el mismo átomo que puedan tener el mismo conjunto de valores para los cuatro números cuánticos.

Este texto está adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/6-3-development-of-quantum-theory#0"> Openstax, Chemistry 2e, Section 6</a>.

Estructura electrónica de los átomos.


Un átomo se compone de protones y neutrones, que están contenidos dentro del núcleo central denso llamado núcleo, con electrones presentes alrededor del ...

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Organic Chemistry

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Unit 1

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Covalent Bonding and Structure

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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

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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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intermolecular forces and physical properties

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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...

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Atomic Orbitals and Quantum Numbers | JoVE K12

organic chemistry

JoVE Core Química Orgánica explica los conceptos básicos de la estereoquímica, las reacciones y sus mecanismos mediante lecciones de vídeo animadas, concisas y fáciles de entender. Además, los vídeos de científicos en acción muestran la aplicación de esos conceptos en experimentos de investigación clásicos y originales, desarrollados actualmente en laboratorios de todo el mundo.

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Atomic Orbitals and Quantum Numbers

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