Name: lewis structures with formal charge
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 2 min 42 s
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Formal Charges

Algunas moléculas o iones poliatómicos puede ser representados por múltiples estructuras de Lewis, pero cómo decidir cuál es la estructura dominante? Mediante el cálculo de las cargas formales de los átomos, se puede determinar la estructura de Lewis más cercana a la estructura real de la molécula. A cada átomo se le asigna una carga hipotética llamada carga formal, que sería la carga en el átomo si todos los demás átomos de la molécula tienen la misma electronegatividad.Se asume que cada electrón de enlace es igualmente compartido por los dos átomos. veamos el cloruro de hidrógeno. Para determinar la carga formal de cada átomo, primero se suma el número de electrones no enlazados a la mitad del número de electrones de enlace y luego se resta el valor obtenido del número de electrones de la valencia.Un agregado de todas las cargas formales en una molécula o ion es igual a la carga neta de la molécula o ion. Por ejemplo, el óxido nitroso se puede representar por medio de tres estructuras de Lewis:una con dos enlaces dobles, una con un enlace triple entre los átomos de nitrógeno, y una con un enlace triple entre el nitrógeno y el oxígeno;todo esto satisface al octeto. Se identifica la mejor estructura de Lewis mediante cálculos formales de las cargas.El nitrógeno tiene cinco electrones de valencia, y el oxígeno tiene seis electrones de valencia. El cálculo basado en el número de electrones no enlazados y la mitad del número de electrones de enlace da la carga formal para cada estructura. Puesto que el óxido nitroso es una molécula neutra la suma de todas las cargas formales debe ser cero.Generalmente, las cargas formales de los átomos individuales en una estructura de Lewis dominante son las más cercanas a cero. Por tanto, la tercera estructura con una carga formal superior puede ignorarse. Además, una carga formal negativa, si está presente, debe ser transportada por el átomo más electronegativo.Dado que el oxígeno es más electronegativo que el nitrógeno, la segunda estructura, con la carga formal negativa en el oxígeno, se identifica como la estructura dominante para el óxido nitroso. Las cargas formales no son las cargas reales de moléculas o átomos, sino una convención contable. La carga real de la molécula.depende de varios factores, entre ellos la diferencia en electronegatividad entre los átomos constitutivos.

cargas formales

En algunos casos, aparentemente hay más de una estructura de Lewis válida para moléculas e iones poliatómicos. El concepto de cargas formales puede ser usado para ayudar a predecir la estructura de Lewis más apropiada cuando existe más de una estructura razonable.
 
 <h4>Calcular la carga formal</h4>
 
 La carga formal de un átomo en una molécula es la carga hipotética que tendría el átomo si los electrones en los enlaces se distribuyen uniformemente entre los átomos. Alternativamente, la carga formal resulta cuando a partir del número de electrones de valencia de un átomo neutro, los electrones no enlazados se reducen primero, seguidos por la resta del número de enlaces unidos a ese átomo en la estructura de Lewis.
 
 Por lo tanto, la carga formal se calcula de la siguiente manera: 
 
 <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/1065/1065_Equations-01.png" style="height: 60px;" />
 
 Los cálculos de cargas formales se pueden verificar determinando la suma de las cargas formales para toda la estructura. La suma de las cargas formales de todos los átomos en una molécula debe ser cero; la suma de las cargas formales en un ion debe ser igual a la carga del ion. Recuerde que la carga formal calculada para un átomo no es la carga real del átomo en la molécula. La carga formal es sólo un procedimiento útil de contabilidad; no indica la presencia de cargas reales.
 
 <h4>Calculando la carga formal de las estructuras de Lewis</h4>
 
 Se siguen los siguientes pasos para asignar cargas formales a cada átomo en el ion interhalógeno ICl4−.
 
 Paso 1.Divida los pares de electrones del enlace por igual para todos los enlaces I–CL:
 
 <img alt="Figure1" src="https://www.jovecore.com/CDNSource/lessons/1065/1065image_1.svg" style="height: 120px;" />
 
 Paso 2.Asigne pares de electrones solitarios a sus átomos. Cada átomo de cloro ahora tiene siete electrones asignados, y el átomo de yodo tiene ocho.
 
 Paso 3.Reste este número del número de electrones de valencia para el átomo neutro: 
 Yodo: 7 – 8 = –1 
 Cloro: 7 – 7 = 0 
 La suma de las cargas formales de todos los átomos es igual a –1, que es idéntica a la carga del ión (–1).
 
 <h4>Uso de las cargas formales para predecir la estructura molecular</h4>
 
 La disposición de los átomos en una molécula o ión se llama su estructura molecular. En muchos casos, seguir los pasos para escribir las estructuras de Lewis puede conducir a más de una estructura molecular posible — múltiples enlaces diferentes y colocaciones de pares de electrones solitarios o diferentes arreglos de átomos, por ejemplo. Unas pocas pautas que implican la carga formal pueden ser útiles para decidir cuál de las posibles estructuras es más probable para una molécula o ión particular:
 
 <ol>
 <li>Una estructura molecular en la que todas las cargas formales son cero es preferible a una en la que algunas cargas formales no son cero.</li>
 <li>Si la estructura de Lewis debe tener cargas formales distintas de cero, es preferible la disposición con las cargas formales más pequeñas distintas de cero.</li>
 <li>Las estructuras de Lewis son preferibles cuando las cargas formales adyacentes son cero o del signo opuesto.</li>
 <li>Al elegir entre varias estructuras de Lewis con distribuciones similares de cargas formales, es preferible la estructura con cargas formales negativas en los átomos más electronegativos.</li>
 </ol>
 
 Para ver cómo se aplican estas directrices, considere algunas estructuras posibles para el dióxido de carbono, CO2. Se sabe que el átomo menos electronegativo ocupa típicamente la posición central, pero las cargas formales ayudan a entender por qué ocurre esto. Se pueden trazar tres posibilidades para la estructura: Carbono en el centro con dos enlaces dobles, carbono en el centro con un enlace sencillo y uno triple, y oxígeno en el centro con enlaces dobles. 
 
 <img alt="Figure2" src="https://www.jovecore.com/CDNSource/lessons/1065/1065image_2.svg" style="height: 80px;" />
 
 Al comparar las tres cargas formales, la estructura de la izquierda puede ser identificada como preferible porque sólo tiene cargas formales de cero.
 
 Como otro ejemplo, el ion tiocianato, un ion formado por un átomo de carbono, un átomo de nitrógeno y un átomo de azufre, podría tener tres estructuras moleculares diferentes: NCSndash;, CNS–, o CSN–. Las cargas formales presentes en cada una de estas estructuras moleculares pueden ayudar a escoger la disposición más probable de los átomos. Las posibles estructuras de Lewis y las cargas formales para cada una de las tres estructuras posibles para el ion tiocianato son: Carbono en el centro con enlaces dobles, nitrógeno en el centro con enlaces dobles, y azufre en el centro con enlaces dobles. 
 
 <img alt="Figure3" src="https://www.jovecore.com/CDNSource/lessons/1065/1065Image_3.svg" style="height: 95px;" />
 
 Tenga en cuenta que la suma de las cargas formales en cada caso es igual a la carga del ion (–1). Sin embargo, se prefiere la primera disposición de átomos con carbono en el centro porque tiene el menor número de átomos con cargas formales distintas de cero. Además, coloca el átomo menos electronegativo en el centro y la carga negativa en el elemento más electronegativo.
 
 Este texto es adaptado de<a href="https://openstax.org/books/chemistry-2e/pages/7-4-formal-charges-and-resonance">Openstax, Química 2e, Capítulo 7.4 Cargas Formales y Resonancia.</a>

Cargas Formales

En algunos casos, aparentemente hay más de una estructura de Lewis válida para moléculas e iones poliatómicos. El concepto de cargos formales se puede utilizar para ...

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lewis structures with formal charge

Lewis structures can sometimes show more than one reasonable arrangement for a molecule or polyatomic ion. Formal charge helps chemists choose the best Lewis structure when that happens. It is a useful way to compare possible structures in chemistry.

Formal charge is the hypothetical charge an atom would have if bonding electrons were shared evenly between the atoms. It can also be found by starting with the valence electrons of the neutral atom, subtracting the nonbonding electrons, and then subtracting the number of bonds on that atom in the Lewis structure. This is a bookkeeping tool, not the actual charge on the atom.

The formal charge of a full structure should also be checked as a whole. For a neutral molecule, the sum of all formal charges must be zero. For an ion, the sum of all formal charges should match the ion’s overall charge.

A common example is the interhalogen ion ICl4−. To assign formal charges, the bonding electron pairs are divided equally among the I–Cl bonds. Then lone pairs are assigned to their atoms. In this structure, each chlorine has seven electrons assigned to it, and iodine has eight. That gives iodine a formal charge of −1 and each chlorine a formal charge of 0, which adds up to the −1 charge of the ion.

Formal charge also helps predict molecular structure when several Lewis structures are possible. A structure with all formal charges equal to zero is preferred over one with nonzero charges. If nonzero charges are needed, the best choice has the smallest charges possible. Structures are also preferred when adjacent formal charges are zero or opposite in sign. When several choices are still possible, the negative charge should be on the more electronegative atom.

Carbon dioxide shows why these rules matter. One possible structure has carbon in the center with two double bonds. Other possibilities place carbon between a single and a triple bond, or place oxygen in the center with double bonds. The structure with carbon in the center and two double bonds is preferred because all of its formal charges are zero.

The thiocyanate ion, NCS−, gives another clear example. It can be written with carbon, nitrogen, or sulfur in the center. The formal charges in each possible Lewis structure help identify the most likely arrangement of atoms. The carbon-centered structure is preferred because it has the fewest atoms with nonzero formal charges. It also places the least electronegative atom in the center and the negative charge on the more electronegative element.

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Lewis Structures with Formal Charge

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