Name: dalton’s laws and early atomic ideas
Uploaded: 2020-09-03T13:38:25.000Z
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K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.1.1

The Atomic Theory of Matter

Los antiguos griegos, como Demócrito, fueron los primeros en presentar la idea de los átomos, la unidad más pequeña e indivisible de la materia. Luego, este concepto se propuso en la teoría atómica del científico inglés John Dalton. El primer postulado de la teoría atómica de Dalton sugiere que los elementos están compuestos por diminutas partículas indivisibles llamadas átomos.Por ejemplo, el hidrógeno está hecho de dos átomos de hidrógeno enlazados, y el oxígeno está hecho de dos átomos de oxígeno enlazados. El segundo postulado afirma que los átomos de un mismo elemento son idénticos, pero difieren de los átomos de otros elementos. De este modo, todos los átomos de hidrógeno son idénticos, pero distintos a los de oxígeno.El tercer postulado enuncia que los átomos de elementos distintos pueden combinarse entre ellos en proporciones de números enteros simples para formar compuestos. Por ejemplo, dos átomos de hidrógeno y un átomo de oxígeno se combinan en una proporción de 2 a 1 para formar H2O, agua. El último postulado de la teoría de Dalton afirma que las reacciones químicas no transforman los átomos de un elemento en átomos de un elemento diferente, sino que los átomos existentes se reorganizan para formar nuevas sustancias.Durante la formación del agua, los átomos de hidrógeno y oxígeno no se crean ni se destruyen, solo se reorganizan. Dalton construyó su teoría atómica sobre dos leyes previas de las reacciones químicas:la ley de conservación de la materia y la ley de las proporciones definidas. La ley de conservación de la materia postula que la masa total antes y después de una reacción química permanece invariable.Entonces, 18 gramos de agua se descomponen en 2 gramos de hidrógeno y 16 gramos de oxígeno. La ley de las proporciones definidas postula que, independientemente de la fuente, la proporción de masa de los elementos constitutivos en un compuesto químico dado es fija. Por consiguiente, una muestra de agua pura siempre tendrá una proporción de masa de 1 a 8 entre hidrógeno y oxígeno, sin importar cuál sea la masa total del agua.Luego, Dalton propuso la ley de las proporciones múltiples basándose en su propia teoría. De acuerdo con esta ley, cuando dos elementos se combinan para formar más de un compuesto, distintas masas de uno de los elementos se combinan con una masa fija del otro elemento en una proporción de números enteros pequeños. Por tanto, una masa fija de hidrógeno de 2 gramos, se combina con distintas masas de oxígeno, 32 o 16 gramos, en una proporción de números enteros pequeños de 2 a 1 para formar dos compuestos diferentes:peróxido de hidrógeno y agua.

la teoría atómica de la materia

La primera discusión registrada de la estructura básica de la materia viene de los filósofos griegos antiguos. Leucippus y Demócrito sostuvieron que toda la materia estaba compuesta de partículas pequeñas y finitas que llamaban atomos, lo que significa “indivisible” Más tarde, Aristóteles y otros llegaron a la conclusión de que la materia consistía en varias combinaciones de los cuatro “elementos” — fuego, tierra, aire y agua — y podía ser infinitamente dividida. Curiosamente, estos filósofos pensaron en los átomos y los “elementos” como conceptos filosóficos, pero aparentemente nunca consideraron realizar experimentos para probar sus ideas. 
 
 La visión aristotélica de la composición de la materia mantuvo su influencia durante más de dos mil años hasta que el científico inglés John Dalton revolucionó la química con su hipótesis de que el comportamiento de la materia podía explicarse utilizando una teoría atómica. Muchas de las hipótesis de Dalton sobre las características microscópicas de la materia, publicadas por primera vez en 1807, siguen siendo válidas en la teoría atómica moderna. 
 
 Aquí están los postulados de la teoría atómica de Dalton:
 
 <ol>
 <li>La materia está compuesta de partículas extremadamente pequeñas llamadas átomos. Un átomo es la unidad más pequeña de un elemento que puede participar en un cambio químico.</li>
 <li>Un elemento consiste en un solo tipo de átomo, que tiene una masa que es característica del elemento y es la misma para todos los átomos de ese elemento. Una muestra macroscópica de un elemento contiene un número increíblemente grande de átomos, todos los cuales tienen propiedades químicas idénticas.</li>
 <li>Los átomos de un elemento difieren en sus propiedades de los átomos de todos los demás elementos.</li>
 <li>Un compuesto consta de átomos de dos o más elementos combinados en una pequeña relación de números enteros. En un compuesto dado, el número de átomos de cada uno de sus elementos están siempre presentes en la misma proporción</li>
 <li>Los átomos no se crean ni se destruyen durante un cambio químico, sino que se reorganizan para producir sustancias que son diferentes de las presentes antes del cambio.</li>
 </ol>
 
 Dalton utilizó tres leyes de reacciones químicas como base para su teoría: (1) la Ley de Conservación de la Masa, (2) la Ley de Proporciones Definidas, y (3) la Ley de Proporciones Múltiples. La teoría atómica de Dalton proporciona una explicación microscópica de las muchas propiedades macroscópicas de la materia. 
 
 La ley de conservación de la masa fue descubierta por el químico francés Antoine Lavoisier. Establece que los átomos no son creados ni destruidos durante un cambio químico; la masa total de la materia presente cuando la materia cambia de un tipo a otro permanece constante.
 
 Dalton también conocía los experimentos del químico francés Joseph Proust, quien demostró que todas las muestras de un compuesto puro contienen los mismos elementos en la misma proporción en masa. Esta declaración es conocida como la ley de proporciones definidas o la ley de composición constante. La sugerencia de que el número de átomos de los elementos en un compuesto dado siempre existe en la misma proporción es consistente con estas observaciones. 
 
 Dalton también utilizó datos de Proust, así como resultados de sus propios experimentos, para formular otra ley interesante. La ley de proporciones múltiples establece que cuando dos elementos reaccionan para formar más de un compuesto, una masa fija de un elemento reaccionará con las masas de los otros elementos en una proporción de números pequeños y enteros.
 
 La teoría de Dalton proporcionó un marco que más tarde se expandió para demostrar que el átomo está compuesto de partículas subatómicas y que los átomos del mismo elemento pueden diferir en masa, conocidos como isótopos.
 
 Este texto es adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/2-1-early-ideas-in-atomic-theory">Openstax, Química 2e, Sección 2,1: Primeras Ideas en Teoría Atómica.</a>

La Teoría Atómica de la Materia

La primera discusión registrada de la estructura básica de la materia proviene de los antiguos filósofos griegos. Leucipo y Demócrito argumentaron que toda la materia...

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dalton’s laws and early atomic ideas

Dalton’s atomic theory explains matter with atoms, elements, and compounds. It also shows how chemical changes follow simple laws. This idea gave chemistry a microscopic model for what can be seen in the lab.

The earliest recorded ideas about matter came from ancient Greek philosophers. Leucippus and Democritus said all matter was made of tiny, finite particles called atomos, meaning “indivisible.” Aristotle and others later argued that matter was made from four elements: fire, earth, air, and water. They also believed matter could be divided forever, and these ideas were treated as philosophy rather than experiments.

That view lasted for more than two thousand years. Then English scientist John Dalton changed chemistry with an atomic theory of matter. He first published it in 1807. Many of his ideas still fit modern atomic theory.

Dalton’s postulates describe matter at the atomic level. Matter is made of extremely small particles called atoms. An atom is the smallest unit of an element that can take part in a chemical change. An element contains only one type of atom, and atoms of the same element have the same characteristic mass and chemical properties. Atoms of different elements have different properties. A compound is made of atoms of two or more elements joined in a small, whole-number ratio, and the ratio stays the same in a given compound. During a chemical change, atoms are not created or destroyed. They are rearranged into new substances.

Dalton built his theory using three key laws of chemistry. The law of conservation of mass says mass stays constant during a chemical change, a result linked to Antoine Lavoisier. The law of definite proportions, also called the law of constant composition, says every pure sample of a compound contains the same elements in the same mass ratio, as shown by Joseph Proust. Dalton also used the law of multiple proportions, which says that when two elements form more than one compound, fixed masses of one element combine with the other in small whole-number ratios.

Dalton’s atomic theory gives a microscopic explanation for macroscopic matter. It also helped later scientists show that atoms contain subatomic particles. Later work also showed that atoms of the same element can differ in mass, which are called isotopes.

Dalton’s Laws and Early Atomic Ideas

the atomic theory of matter

Dalton’s atomic theory explains matter with atoms, elements, and compounds. It also shows how chemical changes follow simple laws. This idea gave chemistry a microscopic model for what can be seen in the lab. The earliest recorded ideas about matter came from ancient Greek philosophers. Leucippus and Democritus said all matter was made of tiny, finite particles called atomos, meaning “indivisible.” Aristotle and others later argued that matter was made from four elements: fire, earth, air, and...

subatomic particles

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key terms and concepts

Explore Dalton’s atomic theory, the laws of conservation of mass, definite proportions, and multiple proportions, plus the early ideas that shaped modern chemistry.

Dalton’s Laws and Early Atomic Ideas | JoVE K12

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Matter And Its Interactions

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Dalton’s Laws and Early Atomic Ideas

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