Reacciones Químicas: Clasificación y Ejemplos

Reacciones Químicas: Clasificación y Ejemplos

Las reacciones químicas forman parte de nuestro día a día a pesar de que algunas no podamos percibirlas o entenderlas. Ejemplo de ellas tenemos la fermentación, la combustión y la corrosión u oxidación de metales. Otras de gran importancia son las que ocurren en el organismo de todos los seres vivos, con la finalidad de proveer al cuerpo de energía para luego almacenarla y consumirla. Este tipo de reacciones son indispensables para la vida. Ahora bien, ¿qué es una reacción química? ¿Cómo se llevan a cabo?

Una reacción química es un proceso termodinámico en el cual dos o más sustancias denominadas reactantes (elementos o compuestos) se combinan y se transforman de manera tal que ocurre un cambio en sus estructuras moleculares y enlaces para luego formar otras sustancias llamadas productos.

Este fenómeno también es conocido como cambio químico ya que a diferencia de las mezclas, no solo ocurre una combinación entre varias sustancias y un cambio físico, sino que también acontece un cambio interno y estructural de cada una de ellas.

Cuando sucede una reacción química está generalmente viene acompañada de ciertas características que nos permitirá clasificar o identificar, como por ejemplo, cambio de olor, variación de la temperatura, variación de color, formación de un precipitado o desprendimiento de gases, entre otros.

De igual manera, para que se lleve a cabo ciertas reacciones, en algunos casos, se necesita de intermediarios para que estas ocurran, por ejemplo la temperatura y el uso de catalizadores.

Las reacciones químicas las representamos haciendo uso de ecuaciones químicas.

A + B → C + D   ; donde:

A+ B: Reactantes o reactivos

C+ D: Productos

: Produce

Según el tipo de energía que es intercambiada en una reacción química, estas se pueden clasificar: reacciones exotérmicas, endotérmicas, exoluminosas y endoluminosas.
Reacciones Exotérmicas

Son aquellas donde ocurre desprendimiento de energía en forma de calor.

Exotérmica

En el diagrama de energía se puede observar como el nivel de energía de los reactantes es mayor que el de los productos, por lo cual se puede deducir que una vez que se suministre energía para dar inicio a la reacción, está se desarrollará liberando energía.

A + C → C+ D + calor

Energía reaccionante >  Energía resultante

En la vida diaria se puede encontrar ejemplos de este tipo de reacción química. Cuando encendemos un cerillo ocurre desprendimiento de energía en forma de calor, en este caso reacción el fósforo con el oxígeno para formar óxido de fósforo, como se ilustra en la siguiente ecuación química:

P4 + 5O2 → 2P2O5

El fósforo rojo empleado para la fabricación de cerillos no se halla en la cabeza de del mismo, sino que está ubicado en la superficie áspera de la caja, combinada con una sustancia abrasiva como el vidrio en polvo. Al ser sometido el fósforo a la pared de la caja, una mínima cantidad de fósforo rojo de la superficie se transforma en fósforo blanco, el cual se enciende.

Otros ejemplos de reacciones exotérmicas tenemos:

2 H2 + O2 → 2 H2O + calor (reacción de combustión)

C + O2 → CO2 + calor (reacción de combustión)

4 Fe + 3 O2 → 2 Fe2O3 + calor (reacción de oxidación)

HCl + NaOH → NaCl + H2O + calor (reacción de neutralización)

 

Reacciones Endotérmicas

Son aquellas reacciones donde se necesita de calor para que se lleve a cabo, es decir ocurre una absorción de energía durante todo el proceso.

Endotérmica

En el diagrama de energía se puede observar como el nivel de energía de los reactantes es menor que el de los productos, por lo cual se puede deducir que una vez que se suministre energía durante toda la reacción, la energía de activación será mayor que el calor liberado en la misma.

X + Y + calor → Z + W

Energía reaccionante < Energía resultante

Un ejemplo común de reacción endotérmica es la que se lleva a cabo para producir sulfuro de hierro (II). Para obtener el FeS se requiere suministrar calor durante toda la reacción.

S8(s) + 8Fe(s) → 8FeS(s)

Otros ejemplos de reacciones endotérmicas tenemos:

Descomposición química del agua: 2H2O + energía → 2 H2 + O2    (ΔH = +285 KJ/mol de agua) (Reacción de electrólisis)

Producción de ozono: 3O2 + energía (luz ultravioleta) → 2O3

Descomposición del carbonato de calcio: CaCO3 (s) → CO2 (s)+ CaCO (s)


Reacciones Exoluminosas

Son aquellas donde ocurre desprendimiento de energía en forma luminosa. Por ejemplo la reacción entre el sodio y el agua, la combustión del magnesio, magnesio más agua, entre otras.

Al mezclar glicerina y permanganato potásico, la mezcla comienzan hasta alcanzar temperaturas muy altas. Incluso llegan a producir una bonita llama púrpura.

Reacciones Endoluminosas

Son aquellas que requirieren de energía luminosa para poder llevarse a cabo. Por ejemplo la reacción de la fotosíntesis.

Reacciones Endoeléctricas

Son aquellas que requieren de energía eléctrica para que se puedan llevar a cabo. Por ejemplo: la electrólisis del agua, que permite la obtención de forma pura, de los elementos que la componen (hidrógeno y oxígeno).

La electrólisis del agua permite que se obtenga los elementos químicos que la componen de forma pura o sea el hidrógeno(H2) a través del cátodo y el oxígeno(O2) a través del ánodo, ambos en estado gaseoso.
Reacciones Endoeléctricas

Son aquellas reacciones químicas donde el sistema transfiere energía eléctrica al exterior. Por ejemplo: La reacción de las baterías comerciales.

 

Desde un punto de vista estructural, las reacciones químicas se pueden clasificar en: reacciones de combinación, descomposición y desplazamiento.

 Reacciones de Combinación

En este tipo de reacción química dos sustancias simples o compuestas, es decir dos elementos o dos compuestos se combinan para originar una sustancia más compleja.

La expresión general de este tipo de reacciones es la siguiente:

A + B → C

La reacción entre el potasio y el oxígeno es un ejemplo de la combinación de dos sustancias simples:

4K + O2 → 2K2O (óxido de potasio)

Reacción entre el yodo más aluminio
Reacción entre el yodo y aluminio para generar yoduro de aluminio.

Un ejemplo de la combinación de dos sustancias compuestas tenemos la reacción entre el óxido de magnesio más agua:

MgO + H2O  → Mg(OH)2 (hidróxido de magnesio)


Reacciones de Descomposición

En este tipo de reacción química, una sustancia compuesta reacciona para dar origen a dos o más sustancias menos complejas.

La expresión general es la siguiente:

AB → A + B; o también: ABC → AB + C

Por ejemplo, la descomposición del óxido de aluminio en aluminio y oxígeno:

2Al2O3 → 4Al + 3O2

Es una descomposición de peróxido de hidrógeno en la que se ha utilizado ioduro potásico

Reacciones de Doble Descomposición

En este caso dos sustancias compuestas reaccionan para dar origen a otras dos nuevas sustancias compuestas.

La expresión general es la siguiente:

AB + CD → CB + AD

Por ejemplo, la reacción entre el nitrato de plata y el cloruro de potasio para originar nitrato de potasio y cloruro de plata.

AgNO3 + KCl → KNO3 + AgCl


Reacciones de Desplazamiento o Sustitución

En este tipo de reacción química una sustancia simple químicamente más activa reemplaza a otra dejándola libre y generando un nuevo compuesto.

La expresión general es la siguiente:

AB + C → CB + A

Por ejemplo, la reacción entre el ácido clorhídrico con el zinc para generar cloruro de zinc e hidrógeno.

2HCl + Zn → ZnCl2 + H2

Reacción química entre el cesio y agua
Reacción química del cesio + agua: 2Cs + 2 H2O —> 2CsOH + H2

 

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