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    si el numero de neutrones cambia pero se conserva el numero de protones se

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    Núcleo atómico

    Núcleo atómico

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    Para otros usos de este término, véase Núcleo.

    Representación aproximada del átomo de Helio: en el núcleo los protones están representados en rojo y los neutrones en azul. En la realidad el núcleo también es simétricamente esférico.

    El núcleo atómico es la parte central de un átomo, tiene carga positiva, y concentra más del 99,9 % de la masa total del átomo.

    Está formado por protones y neutrones (denominados nucleones) que se mantienen unidos por medio de la interacción nuclear fuerte,y detallada la cual permite que el núcleo sea estable, a pesar de que los protones se repelen entre sí (como los polos iguales de dos imanes). La cantidad de protones en el núcleo (número atómico), determina el elemento químico al que pertenece. Los núcleos atómicos no necesariamente tienen el mismo número de neutrones, ya que átomos de un mismo elemento pueden tener masas diferentes, es decir son isótopos del elemento.

    La existencia del núcleo atómico fue deducida del experimento de Rutherford, donde se bombardeó una lámina fina de oro con partículas alfa, que son núcleos atómicos de helio emitidos por rocas radiactivas. La mayoría de esas partículas traspasaban la lámina, pero algunas rebotaban, lo cual demostró la existencia de un minúsculo núcleo atómico.

    Índice

    1 Historia

    2 Descripción del núcleo

    2.1 Forma y tamaño del núcleo

    2.2 Estabilidad del núcleo

    3 Modelos de estructura del núcleo atómico

    3.1 Modelo de la gota líquida

    3.2 Modelo de capas 4 Véase también 5 Referencias 6 Bibliografía

    Historia[editar]

    El descubrimiento de los electrones fue la primera indicación de la estructura interna de los átomos. A comienzos del siglo xx el modelo aceptado del átomo era el de J.J Thomson, 'pudín de pasas', modelo en el cual el átomo era una gran bola de carga positiva con los pequeños electrones cargados negativamente incrustado dentro de la misma. Por aquel entonces, los físicos habían descubierto también tres tipos de radiaciones procedentes de los átomos: alfa, beta y radiación gamma. Los experimentos de 1911 realizados por Lise Meitner y Otto Hahn, y por James Chadwick en 1914 mostraron que el espectro de decaimiento beta es continuo y no discreto. Es decir, los electrones son expulsados del átomo con una gama de energías, en vez de las cantidades discretas de energía que se observa en rayos gamma y decaimiento alfa. Esto parecía indicar que la energía no se conservaba en estos decaimientos. Posteriormente se descubrió que la energía sí se conserva, con el descubrimiento de los neutrinos.

    En 1906 Ernest Rutherford publicó "El retraso de la esfera alfa del radio cuando atraviesa la materia", en Philosophical Magazine (12, p. 134-46). Hans Geiger amplió este trabajo en una comunicación a la Royal Society (Proc. Roy. Soc. 17 de julio de 1908) con experimentos y Rutherford se había hecho pasar aire a través de las partículas α, papel de aluminio y papel de aluminio dorado. Geiger y Marsden publicaron trabajos adicionales en 1909 (Proc. Roy. Soc. A82 p. 495-500) y ampliaron aún más el trabajo en la publicación de 1910 por Geiger (Proc. Roy. Soc. 1 de febrero de 1910). En 1911-2 Rutherford explicó ante la Royal Society los experimentos y propuso la nueva teoría del núcleo atómico. Por lo que se considera que Rutherford demostró en 1911 la existencia del núcleo atómico.1​

    Por esas mismas fechas (1909) Ernest Rutherford realizó un experimento en el que Hans Geiger y Ernest Marsden, bajo su supervisión dispararon partículas alfa (núcleos de helio) en una delgada lámina de oro. El modelo atómico de Thomson predecía que la de las partículas alfa debían salir de la lámina con pequeñas desviaciones de sus trayectorias. Sin embargo, descubrió que algunas partículas se dispersan a grandes ángulos, e incluso completamente hacia atrás en algunos casos. Este descubrimiento en 1911, llevó al modelo atómico de Rutherford, en que el átomo está constituido por protones y electrones. Así, el átomo del nitrógeno-14 estaría constituido por 14 protones y 7 electrones.1​

    El modelo de Rutherford funcionó bastante bien durante muchos años. Se pensaba que la repulsión de las cargas positivas entre protones era solventada por los electrones (con carga negativa) interpuestos ordenadamente en medio, por lo que el electrón era considerado como un "cemento nuclear".1​ Esto fue hasta que los estudios llevados a cabo por Franco Rasetti, en el Institute of Technology de California en 1929. En 1925 se sabía que los protones y electrones tiene un espín de 1 / 2, y en el modelo de Rutherford nitrógeno - 14 los 14 protones y seis de los electrones deberían cancelar sus contribuciones al espín total, estimándose un espín total de 1 / 2. Rasetti descubierto, sin embargo, que el nitrógeno - 14 tiene un espín total unidad.2​

    En 1930 Wolfgang Pauli no pudo asistir a una reunión en Tubinga, y en su lugar envió una carta famoso con la clásica introducción "Queridos Señoras y señores radiactivos ". En su carta Pauli sugirió que tal vez existía una tercera partícula en el núcleo, que la bautizó con el nombre de "neutrones". Sugirió que era más ligero que un electrón y sin carga eléctrica, y que no interactuaba fácilmente con la materia (y por eso todavía no se le había detectado). Esta hipótesis permitía resolver tanto el problema de la conservación de la energía en la desintegración beta y el espín de nitrógeno - 14, la primera porque los neutrones llevaban la energía no detectada y el segundo porque un electrón extra se acoplaba con el electrón sobrante en el núcleo de nitrógeno - 14 para proporcionar un espín de 1. Enrico Fermi redenominó en 1931 los neutrones de Pauli como neutrinos (en italiano pequeño neutral) y unos treinta años después se demostró finalmente que un neutrinos realmente se emiten en el decaimiento beta.

    fuente : es.wikipedia.org

    Conceptos de número atómico, número de masa, masa atómica e isótopos

    materia, estructura atómica, Tabla perdiódica, enlace quíimico, nomenclatura química inorgánica, reacciones químicas inorgánicas

    Scroll Inicio Química Estructura atómica Contenidos

    Conceptos de número atómico, número de masa, masa atómica e isótopos

    Conceptos de número atómico, número de masa, masa atómica e isótopos

    Antes de iniciar revisarás el concepto de elemento.

    Un elemento es una sustancia pura que no puede descomponerse en sustancias más sencillas por métodos químicos ordinarios; algunos ejemplos de elementos son: oro, hierro, hidrógeno y helio.

    Número atómico y número de masa

    El átomo en conjunto es neutro ya que cada protón en el núcleo está en equilibrio con un electrón en los orbitales. Todos los átomos de un elemento determinado tienen el mismo número de protones en el núcleo y de electrones en los orbitales.

    DFIE - IPN (2015). Átomo 2 [Imagen de elaboración propia]

    Un elemento se define como una sustancia compuesta por átomos que poseen la misma carga nuclear. La carga nuclear es distinta para cada uno de los elementos, ello da lugar a lo que se ha denominado como número atómico.

    El número atómico es el número de protones que se hallan en el núcleo de un átomo y es igual al número de electrones. Este número sirvió para ordenar los elementos en la tabla periódica y se representa con la letra Z. Por encontrarse tanto los protones como los neutrones en el núcleo se les llama nucleones.

    DFIE - IPN (2015).. Átomo 2 [Imagen de elaboración propia]

    A la suma de neutrones más protones del núcleo se le nombra número de masa y se representa con la letra A; este valor es siempre un número entero, por ejemplo, en el flúor hay 9 p+ y 10 n0, por lo tanto, el número de masa A será 9 + 10 = 19: A = 19, el número de masa del flúor es 19. Si el número de masa A es igual al número de protones más neutrones y el número atómico Z es igual al número de protones, entonces la diferencia de A – Z debe ser igual al número de neutrones que tiene el núcleo.

    El uranio tiene número de masa (A) = 238 y su número atómico (Z) es 92, por lo que el número de neutrones en su núcleo será A – Z = n0, es decir, n0 = 238 – 92 = 146, por lo que en el núcleo hay 146 neutrones.

    Isótopos

    Los isótopos son átomos que tienen el mismo número de protones (igual número atómico) pero distinto número de neutrones, por lo tanto, diferente número de masa, además ocupan el mismo lugar en la tabla periódica de los elementos.

    Video que explica qué es un átomo y de dónde viene.

    JOLULIPA: Reason&Science (2014) Los Atomos (sic). [Archivo de video]. Recuperado de https://youtu.be/19NOlgO7wC0

    Revisa el siguiente enlace en donde podrás observar la tabla periódica de los elementos.

    Enciclopedia Libre Universal en Español (2011). Tabla periódica de los elementos. Recuperado de http://enciclopedia.us.es/index.php/Tabla_peri%F3dica_de_los_elementos

    Los átomos del mismo elemento pueden tener diferente número de neutrones; las diferentes versiones posibles de cada elemento son llamadas isótopos. Por ejemplo, el isótopo más común del hidrógeno no tiene ningún neutrón; también hay un isótopo del hidrógeno llamado deuterio, con un neutrón, y otro nombrado tritio, con dos neutrones.

    DFIE - IPN (2015). Átomos [Imagen de elaboración propia]

    La mayoría de los elementos no existen como un isótopo sencillo sino que son una mezcla de isótopos; por esta razón las masas atómicas son realmente las masas atómicas promedio. Los isótopos ocupan el mismo lugar en la clasificación periódica y pertenecen, por tanto, al mismo elemento.

    Los isótopos que tienen menos neutrones son más ligeros y se llaman isótopos ligeros, los que tienen más neutrones pesan más y se llaman isótopos pesados. Para distinguir los isótopos entre sí se escribe el símbolo del elemento y como exponente el número de masa, por ejemplo: hierro-57, uranio-238 y helio-3. En los casos anteriores: 57Fe, 238U y 3He.

    El Ca (calcio) tiene varios isótopos, si se quiere encontrar el número de neutrones de alguno de ellos debes saber su número de masa y el número atómico de cada isótopo, por ejemplo:

    En la siguiente tabla se dan ejemplos de isótopos del calcio, así como de su vida media (tiempo que tarda en desaparecer la radiación) y el porcentaje de cada uno en la naturaleza.

    La unidad de masa atómica (u.m.a), se define exactamente como 1/12 de la masa de un átomo de carbono que tiene una masa de 12 u.m.a.

    Pero, ¿por qué las masas atómicas de los elementos no son un número entero?

    Esto se debe a que los elementos tienen isótopos y para determinar la masa atómica de un elemento se toman en cuenta los isótopos del elemento y el porcentaje de cada uno de ellos para obtener la masa promedio del elemento, por lo tanto, las masas atómicas no son exactas, por ejemplo:

    Entonces, para encontrar la masa atómica del cloro se toma en cuenta el número de masa y el porcentaje de cada uno de los isótopos.

    Hasta este momento identificaste lo que es el número de masa, comprendiste que existen los isótopos de los elementos y porqué la masa atómica no es siempre un número entero, todo esto te ayudará para entender el próximo tema.

    Dirección de Formación e Innovación Educativa

    Créditos

    fuente : www.aev.dfie.ipn.mx

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    fuente : brainly.lat

    ¿Quieres ver la respuesta o más?
    Santiago 12 day ago
    4

    Chicos, ¿alguien sabe la respuesta?

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