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    al número entero positivo, negativo o cero que se asigna a cada elemento en un compuesto, se denomina número de oxidación.

    Santiago

    Chicos, ¿alguien sabe la respuesta?

    obtenga al número entero positivo, negativo o cero que se asigna a cada elemento en un compuesto, se denomina número de oxidación. de este sitio.

    Estado de oxidación

    Estado de oxidación

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    Enlace iónico. Un átomo dona electrones a otra especie, y al tener cargas opuestas se atraen mutuamente.

    En química, el estado de oxidación (EO) es un indicador del grado de oxidación de un átomo que forma parte de un compuesto u otra especie química (por ejemplo un ion). Formalmente, es la carga eléctrica hipotética que el átomo tendría si todos sus enlaces con elementos distintos fueran 100% iónicos.

    El EO es representado por números, los cuales pueden ser positivos, negativos o cero. En algunos casos, el estado de oxidación promedio de un elemento es una fracción, tal como +8/3 para el hierro en la magnetita (Fe3O4). El mayor EO conocido es +8 para los tetraóxidos de rutenio, xenón, osmio, iridio, hassio y algunos compuestos complejos de plutonio, mientras que el menor EO conocido es -4 para algunos elementos del grupo del carbono (elementos del grupo 14).

    Según la normativa de la IUPAC se debe escribir como superíndice del símbolo del elemento químico, indicando primero el número y seguido del signo. Por ejemplo Al3+

    La oxidación se da cuando un elemento o compuesto pierde uno o más electrones. Generalmente, cuando una sustancia se oxida (pierde electrones), otra sustancia recibe o capta dichos electrones reduciéndose. Este es el mecanismo básico que promueve las reacciones de óxido-reducción o redox.

    En un enlace covalente apolar ambos átomos comparten el par de electrones para cumplir la regla del octeto, no obstante, el de mayor electronegatividad —en este caso el carbono— los atrae más fuertemente y se recibe una carga parcial negativa (δ-); por el contrario, el otro átomo —el hidrógeno— está más alejado del par de electrones y se carga parcialmente de forma positiva (δ+). El EO busca cuantificar y explicar esta interacción: el carbono tiene un EO de -4 y cada hidrógeno +1 y al sumarlos da la carga de la molécula (0).

    Un átomo tiende a obedecer la regla del octeto para así tener una configuración electrónica igual a la de los gases nobles, los cuales son muy estables químicamente (sus átomos no forman enlaces químicos casi con nadie, ni siquiera con ellos mismos). Dicha regla sostiene que un átomo tiende a tener ocho electrones en su nivel de energía más externo. En el caso del hidrógeno este tiende a tener 2 electrones, lo cual le proporcionaría la misma configuración electrónica que la del helio.

    Cuando un átomo necesita, por ejemplo, 3 electrones para obedecer la regla del octeto, entonces dicho átomo tiende a tener un número de oxidación de 3-, cuando adquiera esos 3 electrones. Por otro lado, cuando un átomo tiene los 3 electrones que deben ser cedidos para que el átomo A cumpla la ley del octeto, entonces este átomo tiende a tener un número de oxidación de 3+, cuando ceda esos 3 electrones. En este ejemplo podemos deducir que los átomos A y B pueden unirse para formar un compuesto, y que esto depende de las interacciones entre ellos. La regla del octeto y del dueto pueden ser satisfechas compartiendo electrones (formando compuestos covalentes, por ejemplo en moléculas como el agua) o cediendo y adquiriendo electrones (formando compuestos iónicos como por ejemplo en los cristales de cloruro de sodio).

    Los elementos químicos se dividen en 3 grandes grupos, clasificados por el tipo de carga eléctrica que pueden adquirir al participar en una reacción química:

    Metales. No metales. Gases nobles.

    Existen elementos metálicos que, dependiendo de las condiciones a que sean sometidos, pueden funcionar como metales o no metales indistintamente. A estos elementos se les denomina semimetales o metaloides.

    Los elementos metálicos (los cuales tienden a ceder electrones) cuando forman compuestos tienen normalmente estados de oxidación positivos. Los elementos no metálicos y semimetálicos, en cambio, pueden tener estados de oxidación positivos y negativos, dependiendo del compuesto que estén constituyendo.

    Índice

    1 Ejemplos

    2 Reglas de los estados de oxidación

    3 Véase también 4 Referencias 5 Enlaces externos

    Ejemplos[editar]

    Cloruro de sodio

    2Na0 + Cl02 → 2Na1+ + 2Cl1-

    Los gases de un solo tipo de elemento, en este caso el cloro, están presentes en forma diatómica.

    El sodio (Na) se combina con el cloro (Cl), produciendo cloruro de sodio. El número de oxidación de ambos elementos sin combinar es 0 (cero), ya que están equilibrados eléctricamente. El número de oxidación del sodio combinado es 1+, ya que cede un electrón. El número de oxidación del cloro combinado es 1-, ya que acepta el electrón cedido por el sodio.

    Óxido de aluminio

    Al0 + O02 → Al3+ + 2O2−

    El oxígeno (O) está presente en forma diatómica (gas).

    El aluminio (Al) se combina con el oxígeno (O), produciendo óxido de aluminio (Al2O3). El número de oxidación de ambos elementos sin combinar es 0 (cero), ya que están equilibrados eléctricamente. El número de oxidación del aluminio combinado es 3+, ya que cede tres electrones. El número de oxidación del oxígeno combinado es 2−, ya que acepta hasta 2 electrones.

    Los electrones cedidos y aceptados por los distintos elementos crean un problema con las cargas eléctricas. Por ejemplo, el aluminio cede tres electrones y el oxígeno solo acepta dos, por lo que sobra uno. De esto se concluye que en la reacción no interviene un solo átomo de oxígeno, por lo que se procede a balancear la ecuación, para que coincidan todos los electrones transferidos con las capacidades de cada elemento aceptor.

    fuente : es.wikipedia.org

    Imprimir Test: Construcción fórmulas químicas (1º

    Imprimir Recursos educativos (Test): Construcción fórmulas químicas (1º - Bachillerato - formulas quimicas) - Actividad de evaluación diagnóstica

    Construcción fórmulas químicas

    Autor:

    Javier Cruz Guardado

    1. La fórmula H2O expresa que la molécula de agua está constituida por dos átomos de hidrógeno y uno de oxígeno.

    Falso Verdadero

    2. En América, la construcción de una fórmula química se escribe primero la parte negativa y enseguida la positiva.

    Falso Verdadero

    3. En una fórmula química la suma de cargas negativas y positivas siempre es mayor de cero.

    Falso Verdadero

    4. Los subíndices expresan el número de átomos de los elementos presentes en una molécula o unidad fórmula.

    Falso Verdadero

    5. El símbolo Cl - indica que el átomo de cloro ha tenido una reducción o pérdida de electrones.

    Falso Verdadero

    6. Al número entero positivo, negativo o cero que se asigna a cada elemento en un compuesto, se denomina número de oxidación.

    Falso Verdadero

    7. En una fórmula química, los coeficientes indican el número de moléculas o unidades fórmula; así como también el número de moles presentes de la sustancia.

    Falso Verdadero

    8. En la fórmula 3 NH4Cl el coeficiente es el 4.

    Falso Verdadero

    9. El número de oxidación de un elemento combinado con otro, es cero.

    Falso Verdadero

    10. Una fórmula química sólo expresa la composición cualitativa de una sustancia.

    Falso Verdadero

    fuente : es.educaplay.com

    Al numero entero, positivo ,negativo o cero,que se asigna a un elemneto presente en una formula

    Encuentra una respuesta a tu pregunta Al numero entero, positivo ,negativo o cero,que se asigna a un elemneto presente en una formula quimica se le domina

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    Al numero entero, positivo ,negativo o cero,que se asigna a un elemneto presente en una formula - Brainly.lat

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    fuente : brainly.lat

    ¿Quieres ver la respuesta o más?
    Santiago 17 day ago
    4

    Chicos, ¿alguien sabe la respuesta?

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