las sustancias con este tipo de enlace se disuelven fácilmente en agua y conducen la corriente eléctrica

obtenga las sustancias con este tipo de enlace se disuelven fácilmente en agua y conducen la corriente eléctrica de este sitio.

Enlaces (covalente, iónico y metálico).

Hipervínculos a los contenidos de 3ºESO

Enlaces (covalente, iónico y metálico)

Enlace químico

Regla del octeto y Estructura de Lewis

Tipos de enlace Enlace iónico Enlace covalente:

Consideraciones básicas

Sustancias moleculares

Sólidos covalentes Enlace metálico

Análisis del tipo de enlace más probable:

Según el tipo de átomos que forman la sustancia

Según las propiedades

Fórmulas químicas

Enlace iónico.

Consideraciones básicas

¿Qué es el enlace iónico?

Es el enlace que se da entre elementos de electronegatividades muy diferentes. Se produce una cesión de electrones del elemento menos electronegativo al mas electronegativo y se forman los respectivos iones positivos (los que pierden electrones) y negativos (los átomos que ganan los electrones).

Este tipo de enlace suele darse entre elementos que están a un extremo y otro de la tabla periódica. O sea, el enlace se produce entre elementos muy electronegativos (no metales) y elementos poco electronegativos (metales).

¿Qué mantiene la unión?

La fuerza de atracción entre las cargas positivas y las cargas negativas que se forman; es decir, la fuerza de atracción entre los cationes y los aniones.

¿Se forman moléculas?

No, se forman redes cristalinas (ordenadas). Por tanto, los iones que se forman con este enlace no forman moléculas aisladas sino que se agrupan de forma ordenada en redes en las que el número de cargas positivas es igual al de cargas negativas, compuesto es neutro.

La fórmula que habitualmente se da es una fórmula empírica.

Propiedades

Temperaturas de fusión y ebullición muy elevadas. Sólidos a temperatura ambiente. La red cristalina es muy estable por lo que resulta muy difícil romperla.

Son duros (resistentes al rayado).

No conducen la electricidad en estado sólido, los iones en la red cristalina están en posiciones fijas, no quedan partículas libres que puedan conducir la corriente eléctrica.

Son solubles en agua por lo general, los iones quedan libres al disolverse y puede conducir la electricidad en dicha situación.

Al fundirse también se liberan de sus posiciones fijas los iones, pudiendo conducir la electricidad.

Enlace covalente.    Consideraciones básicas

¿Qué es el enlace covalente?

Es el enlace que se da entre elementos de electronegatividades altas y muy parecidas, en estos casos ninguno de los átomos tiene más posibilidades que el otro de perder o ganar los electrones. La forma de cumplir la regla de octeto es mediante la compartición de electrones entre dos átomos. Cada par de electrones que se comparten es un enlace.

Este tipo de enlace se produce entre elementos muy electronegativos (no metales).

Los electrones que se comparten se encuentran localizados entre los átomos que los comparten.

¿Qué mantiene la unión?

La fuerza de atracción entre las cargas positivas de los núcleos y las cargas negativas de los electrones que se comparten.

¿Se forman moléculas?

Tenemos moléculas como tales en el caso de las sustancias moleculares. Si los átomos que se unen con enlace covalente forman 'sólidos covalentes' o 'redes covalentes', no tendremos moléculas como tales entidades que se puedan aislar.

Sustancias moleculares

Están constituidas de moléculas; es decir, agrupaciones de un número concreto de átomos que se encuentran unidos dos a dos mediante enlace covalente. Se representa mediante la fórmula molecular.

Son las únicas sustancias que podemos considerar que tienen moléculas como tales entes que se pueden aislar.

Propiedades.

Son las habituales de los enlaces covalentes:

Temperaturas de fusión bajas. A temperatura ambiente se encuentran en estado gaseoso, líquido (volátil) o sólido de bajo punto de fusión.

La temperaturas de ebullición son igualmente bajas.

No conducen la electricidad en ningún estado físico dado que los electrones del enlace están fuertemente localizados y atraídos por los dos núcleos de los átomos que los comparten.

Son muy malos conductores del calor.

La mayoría son poco solubles en agua. Cuando se disuelven en agua no se forman iones dado que el enlace covalente no los forma, por tanto, si se disuelven tampoco conducen la electricidad.

Sólidos covalentes o redes covalentes

En los sólidos covalentes no se forman moléculas. Los enlaces covalentes permiten asociaciones de grandes e indeterminadadas cantidades de átomos iguales o diferentes cuando esto ocurre no se puede hablar de moléculas, sino de redes cristales covalentes. La fórmula de las redes covalentes es al igual que la de las sustancias iónicas, una fórmula empírica.

Propiedades

Algunas son similares a las de las sustancias moleculares

No conducen el calor ni la electricidad.

Son insolubles en agua.

A diferencia de las sustancias moleculares:

Presentan temperaturas de fusión y ebullición muy elevadas. Son sólidos a temperatura ambiente.

Son muy duros (resistencia a ser rayado).

Enlace metálico.

Consideraciones básicas

¿Qué es el enlace metálico?

Es el enlace que se da entre elementos de electronegatividades bajas y muy parecidas, en estos casos ninguno de los átomos tiene más posibilidades que el otro de perder o ganar los electrones. La forma de cumplir la regla de octeto es mediante la compartición de electrones entre muchos átomos. Se crea una nube de electrones que es compartida por todos los núcleos de los átomos que ceden electrones al conjunto..

fuente : www.educamix.com

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Compuesto iónico

Compuesto iónico

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Estructura de un cristal de cloruro de sodio, un típico ejemplo de un compuesto iónico. Las esferas púrpuras son cationes de sodio, y las esferas verdes son aniones de cloruro.

Un compuesto iónico es un compuesto químico formado por dos sustancias con una diferencia significativa en sus electronegatividades.1​Se forma preferentemente cuando metales de los grupos I A y II A se unen con los no metales de los grupos VI A y VII A.2​

Los compuestos iónicos tienen las propiedades siguientes:3​

A temperatura ambiente (25 °C) son sólidos cristalinos, duros y frágiles.

Poseen altos puntos de fusión.

En estado anhidro no conducen la corriente eléctrica, pero cuando se calientan al estado de fusión (si no se descomponen), sí la conducen.

Muchos compuestos iónicos se disuelven en disolventes muy polares (como el agua) y, cuando lo hacen, la solución es eléctricamente conductora.

Los compuestos covalentes, a diferencia de los iónicos, a temperatura ambiente pueden ser sólidos, líquidos o gases. Generalmente, debido a la naturaleza de enlace, los compuestos covalentes tienen propiedades diferentes a los compuestos iónicos, siempre y cuando no se disocien o ionicen en H2O como es el caso de los ácidos fuertes.

Cristales de cloruro de sodio.

Ejemplo[editar]

Un ejemplo de un compuesto iónico es NaCl (sal de mesa) o GaCl3 (cloruro de galio). Cuando se forma un compuesto iónico, el elemento que tiene mayor electronegatividad (en este caso Cl) tratará de quitarle electrones al otro con menor electronegatividad (Na) y se convertirán en anión (Cl-) y catión (Na+), respectivamente. Los electrones quedan "prestados" en la última órbita del Cl y al mismo tiempo en la del Na, haciendo que el Cl complete su octeto (8 electrones, en su última capa), cumpliendo con la regla del octeto o estructura de Lewis.

Cuando se combinan átomos de elementos metálicos (de bajo potencial de ionización, por lo que es fácil arrancarles electrones) con átomos de elementos no metálicos (de alta afinidad electrónica, por lo que ganan electrones con facilidad) el camino que suelen seguir estos átomos para completar su última capa es que el átomo del metal pierde electrones y el del no metal los gane.

Otros ejemplos: KCl (cloruro de potasio), CaCl2 (cloruro de calcio).

Formas[editar]

Las sustancias iónicas forman redes cristalinas en estado sólido4​debido a la forma en la que se acomodan las moléculas del compuesto. Esto provoca que sean sólidos frágiles (no se pueden deformar, sólo fracturar). Para su representación se utiliza la fórmula mínima.

En disoluciones acuosas, los compuestos iónicos se separan en cationes y aniones (ver electrolito)5​ ocurre una disociación electrolítica, donde el agua se convierte en conductora de electricidad debido al flujo de iones en presencia de un campo eléctrico.

Referencias[editar]

↑ Atkins, Peter; Jones, Loretta (2006). . Ed. Médica Panamericana. ISBN 9789500600804. Consultado el 2 de febrero de 2018.

↑ pág. 245 en Google libros

↑ Picazo, Susana María López (2009). . Cultivalibros. ISBN 9788499231099. Consultado el 2 de febrero de 2018.

↑ Irles, Sergio Menargues; David, Fernando Latre; Siurana, Amparo Gómez (2009-04). . Universidad de Alicante. ISBN 9788479089986. Consultado el 2 de febrero de 2018.

↑ Brown, Theodore L.; Jr, H. Eugene LeMay; Bursten, Bruce E.; Burdge, Julia R. (2004). . Pearson Educación. ISBN 9789702604686. Consultado el 2 de febrero de 2018.

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Proyectos WikimediaDatos: Q2366155Diccionarios y enciclopediasBritannica: url

Datos: Q2366155

Categorías: Estructura químicaIones

fuente : es.wikipedia.org