Name: electron regions in atomic orbitals
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 2 min 44 s
Channel: JoVE

K12 Standards

Texas Essential Knowledge and Skills

High School

Chemistry and Physics

IPC.7

IPC.7.E

Atomic Orbitals

La región más densa de la nube de electrones se describe en términos de orbitales atómicos. La forma de un orbital atómico es determinado por el número cuántico del momento angular, l. Recuerde que los valores del momento angular se basan en el número cuántco principal, n los valores posibles de l varían de cero a n menos uno.Cuando n es mayor que uno, existen múltiples subniveles. Cada valor de l corresponde a un orbital s, p, d of. El orbital de menor energía es el orbital 1-s.Este es un orbital esféricamente simétrico. La densidad de probabilidad de un orbital de 1 s revela que es más probable que el electrón se encuentre en el núcleo. Sin embargo, dadas las fuerzas electrostáticas entre los protones y electrones, esto no es probable.Es más representativo multiplicar la densidad de la probabilidad por el volumen de la capas esféricas delgadas con radios r. La probabilidad total de encontrar un electrón dentro de la capa delgada a una distancia r del núcleo es la función de distribución radial. Para el hidrógeno, la mayor probabilidad de encontrar un electrón es de 52, 9 picómetros desde el núcleo.Por tanto, la forma del orbital atómico 1-s del hidrógeno es esférica con un radio de 52, 9 picómetros. Los orbitales dos-s y tres-s también son esféricos. Son más grandes y tienen nodos.En un nodo, la probabilidad de encontrar un electrón es cero. Los niveles principales con n igual a dos o más también contienen tres orbitales p. Estos tienen forma de lóbulo con un nodo en el núcleo.Su orientación se describe por el valor de m-l. Los tres orbitales p son ortogonales entre sí. Los niveles principales de n iguales a tres o más también tienen cinco orbitales d.Los orbitales d con forma de hoja de trébol tienen cuatro lóbulos densos en electrones y dos planos nodales perpendiculares. Uno de los orbitales d es ligeramente diferente. Los orbitales f tienen más lóbulos y nodos.Estos orbitales existen para niveles principales de n igual a cuatro o más. Cuando superpone los orbitales uno encima del otro, emerge una forma aproximadamente esférica. Por eso los átomos se representan generalmente como esferas.

orbitales atómicos

Un orbital atómico representa las regiones tridimensionales en un átomo donde un electrón tiene la mayor probabilidad de residir. La función de distribución radial indica la probabilidad total de encontrar un electrón dentro de la capa delgada a una distancia r del núcleo. Los orbitales atómicos tienen formas distintas que están determinadas por l, el número cuántico del momento angular. Los orbitales a menudo se dibujan con una superficie limitante, que encierra las regiones más densas de la nube. 
 
 El número cuántico de momento angular es un entero que puede tomar los valores, l = 0, 1, 2, …, n –1. Un orbital con un número cuántico principal de 1 (n = 1) sólo puede tener un valor de l (l = 0), mientras que un número cuántico principal de 2 (n = 2) permite l = 0 y l = 1. Los orbitales con el mismo valor de l definen una subcapa.
 
 Los orbitales con l = 0 se denominan orbitales s y forman las subcapas s. El valor l = 1 corresponde a los orbitales p. Para una n dada, los orbitales p constituyen una subcapa p (es decir, 3p si n = 3). Los orbitales con l = 2 se denominan orbitales d. Los orbitales con l = 3, 4 y 5 son los orbitales f,g y h. 
 
 El orbital de menor energía es el orbital 1s. Se trata de un orbital esférico simétrico. La densidad de probabilidad (ψ2) de un orbital 1s implica que es más probable que el electrón se encuentre en el núcleo. Sin embargo, dadas las fuerzas electrostáticas entre protones y electrones, esto no representa con precisión dónde residirá el electrón. En su lugar, se utiliza la función de distribución radial, que es un gráfico de la probabilidad total de encontrar un electrón en un orbital en un radio dado r. La función de distribución radial se obtiene multiplicando la densidad de probabilidad por el volumen de subcapas esféricas delgadas con radios r. Para el orbital 1s del hidrógeno, la función de distribución radial tiene un valor cero en el núcleo, que aumenta hasta un máximo de 52,9 picómetros antes de disminuir con el aumento del radio r.
 
 Existen ciertas distancias desde el núcleo en las que la densidad de probabilidad de encontrar un electrón localizado en un orbital determinado es cero. En otras palabras, el valor de la función de onda ψ es cero a esta distancia para este orbital. Este valor de r se denomina nodo radial. El número de nodos radiales en un orbital es n – l – 1. Para los orbitales 2s, donde n = 1, hay un nodo radial, mientras que los orbitales 3s tienen dos nodos radiales. 
 
 Cada nivel principal con n = 2 o más contiene tres orbitales p. Los tres orbitales p tienen dos lóbulos con un nodo localizado en el núcleo . La orientación de los orbitales p en el espacio se describe por el valor de ml. Los tres orbitales p son perpendiculares entre sí (ortogonales). Los orbitales p más altos (3p, 4p, 5p y superiores) tienen formas similares pero son de mayor tamaño con nodos radiales adicionales.
 
 Los niveles principales con n = 3 o más contienen cinco orbitales d. Cuatro de estos orbitales consisten en una forma de trébol, con cuatro lóbulos electrón-densos. Hay dos planos nodales perpendiculares que se entrecruzan en el núcleo. En estos planos nodales, la densidad de electrones es cero. Uno de los orbitales d es ligeramente diferente en forma y tiene dos lóbulos orientados en el eje z con un anillo en forma de dona en el plano xy. Los niveles principales con n = 4 y superiores contienen siete orbitales f, que tienen formas complejas. Estos orbitales tienen más nodos y lóbulos que los orbitales d.
 
 <img alt="Figure1" src="https://www.jovecore.com/CDNSource/lessons/983/983Image 1.png" style="width: 700px;" />
 
 Figura 1: Orbitales representativos s, p, d y f .
 
 Estas diferentes formas de los orbitales atómicos representan las regiones tridimensionales dentro de las cuales es probable que se encuentre el electrón. Todos los orbitales juntos conforman una forma más o menos esférica, razón por la cual los átomos generalmente se representan como esferas.
 
 Este texto ha sido adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/6-3-development-of-quantum-theory">Openstax, Química 2e, Sección 6.3: Desarrollo de la Teoría Cuántica.</a>

Orbitales Atómicos

Un orbital atómico representa las regiones tridimensionales de un átomo donde un electrón tiene la mayor probabilidad de residir. La distribución radial ...

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Electronic Structure of Atoms

Estructura electrónica de los átomos

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

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 = 0 orbitals are s orbitals, and they make up s subshells. The l = 1 orbitals are p orbitals, which form a p subshell such as 3p when n = 3. The l = 2 orbitals are d orbitals. The l = 3, 4, and 5 orbitals are called f, g, and h orbitals.

The lowest-energy orbital is the 1s orbital. It is spherically symmetric. The probability density, ψ², suggests that an electron is most likely found at the nucleus. But this does not fully match electron behavior. The radial distribution function gives the total probability of finding an electron at a distance r from the nucleus. It is found by multiplying the probability density by the volume of thin spherical shells.

For the 1s orbital of hydrogen, the radial distribution function is zero at the nucleus. It rises to a maximum at 52.9 picometers and then decreases as r increases. Some distances from the nucleus have zero probability density for a given orbital. These points are called radial nodes. The number of radial nodes is n - l - 1. A 2s orbital has one radial node, and a 3s orbital has two.

Each principal level with n = 2 or more contains three p orbitals. Each p orbital has two lobes and a node at the nucleus. Their orientation in space is described by m_l. The three p orbitals are mutually perpendicular. Higher p orbitals, such as 3p, 4p, and 5p, have the same general shape but are larger and contain additional radial nodes.

Principal levels with n = 3 or more contain five d orbitals. Four of them have a cloverleaf shape with four electron-dense lobes. They also have two perpendicular nodal planes that meet at the nucleus. The fifth d orbital has two lobes along the z-axis and a donut-shaped ring in the xy plane.

Principal levels with n = 4 and greater contain seven f orbitals. These orbitals have complex shapes with more nodes and lobes than d orbitals. Together, s, p, d, and f orbitals help explain why atoms are often drawn as spheres, even though the electron regions inside them have distinct shapes.

Electron Regions in Atomic Orbitals

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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 =...

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key terms and concepts

Explore electron regions in atomic orbitals, including s, p, d, and f shapes, radial nodes, and the radial distribution function for high school chemistry.

Electron Regions in Atomic Orbitals | JoVE K12

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Electron Regions in Atomic Orbitals

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