obtenga es distribución más estable de los electrones en los diferentes niveles subniveles y orbitales de este sitio.
Configuración Electrónica
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Configuración Electrónica
Configuración Electrónica
Configuración electrónica
La configuración electrónica del átomo de un elemento corresponde a la ubicación de los electrones en los orbitales de los diferentes niveles de energía. Aunque el modelo de Scrödinger es exacto sólo para el átomo de hidrógeno, para otros átomos es aplicable el mismo modelo mediante aproximaciones muy buenas.La manera de mostrar cómo se distribuyen los electrones en un átomo, es a través de la configuración electrónica. El orden en el que se van llenando los niveles de energía es: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p. El esquema de llenado de los orbitales atómicos, lo podemos tener utilizando la regla de la diagonal, para ello debes seguir atentamente la flecha del esquema comenzando en 1s; siguiendo la flecha podrás ir completando los orbitales con los electrones en forma correcta.
Escribiendo configuraciones electrónicasPara escribir la configuración electrónica de un átomo es necesario:Saber el número de electrones que el átomo tiene; basta conocer el número atómico (Z) del átomo en la tabla periódica. Recuerda que el número de electrones en un átomo neutro es igual al número atómico (Z = p+).Ubicar los electrones en cada uno de los niveles de energía, comenzando desde el nivel más cercano al núcleo (n = 1).Respetar la capacidad máxima de cada subnivel (s = 2e-, p = 6e-, d = 10e- y f = 14e-). Ejemplo:Los orbitales se llenan en orden creciente de energía, con no más de dos electrones por orbital, según el principio de construcción de Aufbau.Litio (Z = 3). Este elemento tiene 3 electrones. Empezaremos llenando el orbital de menor energía con dos electrones que tendrán distinto spin (ms). El electrón restante ocupará el orbital 2s, que es el siguiente con menor energía:
La flecha indica el valor del cuarto número cuántico, el de spin: para +1/2: y para –1/2, respectivamente.
También podemos describir la distribución de electrones en el átomo de litio como:
Los electrones que tienen números de espín opuestos cancelan los efectos magnéticos y se dice que son electrones apareados. Un ejemplo son los dos electrones que ocupan el orbital 1s en el átomo de Litio. De manera similar decimos que el electrón que ocupa el orbital 2s orbital está desapareado.
En la tabla a continuación vemos como se distribuyen los electrones de los átomos en orden creciente a su número atomico (Z):
En el helio se completa el primer nivel (n=1), lo que hace que la configuración del He sea muy estable.Para el Boro el quinto electrón se sitúa en un orbital 2p y al tener los tres orbitales 2p la misma energía no importa cuál de ellos ocupa.
En el carbono el sexto electrón podría ocupar el mimo orbital que el quinto u otro distinto. La respuesta nos la da:
la regla de Hund: la distribución más estable de los electrones en los subniveles es aquella que tenga el mayor número de espínes paralelos.
Los electrones se repelen entre sí y al ocupar distintos orbitales pueden situarse más lejos uno del otro. Así el carbono en su estado de mínima energía tiene dos electrones desapareados, y el nitrógeno tiene 3.
El neón completa el nivel dos y al igual que el helio tiene una configuración estable.Las configuraciones electrónicas pueden también escribirse de manera abreviada haciendo referencia al último nivel completo. Para ello, debemos ocupar la configuración de los gases nobles, ya que ellos tienen todos su orbitales completos con electrones (s2p6), como por ejemplo en el caso del helio (s2) y neon (s2p6) como se muestra en la tabla anterior.
Así la configuración del sodio Na, la podemos escribir como [Ne]3s1 También podemos escribir la configuración del litio como [He]2s1 A los electrones que pertenecen a un nivel incompleto se les denomina electrones de valencia.El gas noble Argón representa el final del período iniciado por el sodio para n=3
1s 2s 2p 3s 3p En el siguiente elemento, el potasio con 19 electrones, deberíamos empezar a llenar los orbitales 3d. Sin embargo el comportamiento químico del potasio es similar al de litio y el sodio, ambos con un electrón de valencia desapareado en un orbital s, por lo que al potasio le correspondería la configuración [Ar] 4s1. Por lo tanto, el orbital 4s tendrá que tener menor energía que los orbitales 3d (el apantallamiento de los electrones en los orbitales 3d es mayor que el de los electrones en los orbitales 4s).
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Distribución electrónica
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Distribución electrónica
Concepto: Representación esquemática de los átomos de los elementos químicos de acuerdo con la concepción actual del átomo.
Distribución electrónica: Es la distribución de los electrones de un átomo en los diferentes estados energéticos determinados por los orbitales en dicho átomo. Así, mediante la configuración electrónica se representan los diferentes estados de los electrones presentes en el átomo.
Sumario
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1 Distribución electrónica
1.1 Por niveles electrónicos
1.1.1 Particularidades de los electrones de los últimos niveles y la tabla periódica
1.2 Por la notación nlx
1.2.1 Reglas para el llenado de los orbitales:
2 Ambas distribuciones
3 La distribución electrónica y su relación con la tabla periódica
4 Propiedades derivadas de la estructura electrónica
5 Referencias 6 Fuentes
7 Enlace relacionado
Distribución electrónica
Como resultado de los grandes esfuerzos realizados por muchos científicos, en la actualidad, la ciencia dispone de múltiples informaciones, comprobadas en la práctica, acerca de las leyes de distribución de los electrones en los átomos, partiendo del modelo de Bohr en la que señalaba la existencia de un núcleo formado por protones y neutrones, donde está concentrada la masa y la carga positiva del átomo. El electrón gira en órbitas circulares alrededor del núcleo, pero con algunas restricciones, como que solamente lo podía hacer en ciertas órbitas, cuya energía se encuentra cuantizada.
Por niveles electrónicos
Asumiendo el modelo de Bohr, los electrones se distribuyen en los átomos formando capas alrededor del núcleo que reciben el nombre de capas electrónicas o también niveles energéticos. Todos ellos forman la envoltura electrónica que rodea al núcleo. Mientras mayor número de capas electrónicas posea un átomo, mayor será la distancia que separa al núcleo de los electrones más externo.
Cada una de las capas electrónicas posee distinto contenido o nivel de energía y se encuentran a diferentes distancias del núcleo, de forma tal que la capa electrónica de menor nivel de energía será la más próxima al núcleo y las de mayores niveles energéticos se encontrarán más alejadas de éste. A medida que los electrones se encuentren en una capa electrónica alejada del núcleo con gran contenido energético estarán más débilmente unidos a éste. .
Los diferentes niveles energéticos toman valores enteros a partir de 1; por lo que el valor del primero, o sea, para el que corresponde a la capa más próxima al núcleo es 1, el que corresponde a la segunda capa es 2, etcétera. Estos niveles se representan también, a veces, por las letras K,L,M,N,O,P y Q.
Distribución electrónica por niveles de energía
Aunque de acuerdo con la concepción actual del átomo no es posible representarlo gráficamente, desde un punto de vista pedagógico es conveniente tener una representación visual, que, aunque no corresponda exactamente a la realidad, tampoco la contradiga, en la que se utilizan esquemas como el mostrado a continuación:
El núcleo se puede representar con un pequeño círculo donde se señalan tanto protones como indica su número atómico, y tantos neutrones como indica la diferencia entre el índice de masa y el número atómico. La envoltura se puede representar por arcos de circunferencia con centro en el núcleo. Cada arco corresponde a un nivel de energía y en el se coloca un número que indica los electrones que existen en ese nivel.
Se ha podido determinar el número máximo de electrones que pueden agruparse en los distintos niveles de energía y tenemos:
Primer nivel de energía n=1: 2 . 12 = 2 electrones
Segundo nivel de energía n=2: 2 . 22 = 8 electrones
Tercer nivel de energía n=3: 2 . 33 = 18 electrones
Al analizar bien lo anterior, se observa que cada nivel puede contener un número máximo de electrones igual a 2n2, donde n puede ser 1,2,3, etc., según el nivel energético. Aunque esto no quiere decir que siempre tendrán ese número máximo de electrones. Así, se tendrá que: .
El máximo número de electrones en la penúltima capa es 18 Si la penúltima capa no está completa, el máximo número de electrones en la capa más externa es 2
Particularidades de los electrones de los últimos niveles y la tabla periódica
Puesto que la capa K solo puede alojar dos electrones quedará completa en el gas inerte Helio. Después de este, se va llenando la capa L, con un electrón en el Litio hasta ocho en el Neón, cuya situación es análoga a la del Helio. Con dos en la capa K y ocho en la L quedan ambas capas totalmente ocupadas, mientras que las exteriores a ellas continúan vacías por completo.
El Neón es también un gas inerte, lo que significa que tras un período o ciclo de ocho átomos reaparece la propiedad de la inercia química. En los ocho átomos siguientes, los electrones se adicionan a la tercera capa, M, aumentando gradualmente su número desde el Sodio hasta ocho en el Argón. Cabria suponer que este elemento, número 18 no debería ser un gas inerte, ya que de acuerdo al diagrama de los niveles energéticos la capa M puede admitir hasta diez electrones más, esto es, 18; pero la observación nos dice que el Argón es un gas inerte, y que por tanto, la tercera capa debe considerarse completa cuando contenga ocho electrones.
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fuente : brainly.lat
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