#atomicmodel

[tutoroot]

What is the Comparison of Atomic Models? 

The evolution of atomic theory reflects humanity’s relentless pursuit of knowledge, from the speculative ideas of ancient philosophers to the precise quantum mechanical models of today. For students looking to master these concepts and excel in their studies, platforms like Tutoroot provide personalised guidance, interactive learning resources, and expert tutoring tailored to individual needs. With Tutoroot’s support, exploring the fascinating world of atomic models becomes an engaging and enriching experience. 

[tadashiscience]

Master Electron Configurations Fast! #shorts | Tadashi Science

https://www.youtube.com/watch?v=S7Mmi3rwCcY Master Electron Configurations Fast! #shorts #chemistry #electronconfigurations #periodictable #atomicstructure #electrons #scienceeducation #learnchemistry #studenttips #atomicmodel #studyguide Watch the full video here: https://www.youtube.com/watch?v=Vdf9GPNwz4c 🔗 Stay Connected With Me. 🔔 Looking to ace science concepts fast? Hit that subscribe for quick, concise lessons and clear explanations that make complex topics easy to grasp! https://www.youtube.com/@tadashiscience/?sub_confirmation=1 📩 For Business Inquiries: tadashiscience@gmail.com ============================= 🎬 Recommended Playlists 👉 Chemistry Midterm https://www.youtube.com/playlist?list=PL-_8ZguMqTyMn7QWwyDJqSZJWrrJ8WocA 👉 S24 Final Exam https://www.youtube.com/playlist?list=PL-_8ZguMqTyM-UuTpU5wDGhQS-m8Y2UAk 🎬 WATCH MY OTHER VIDEOS: 👉 Atomic Structure Made Easy: Protons, Neutrons & Electrons Explained Simply | Tadashi Science https://www.youtube.com/watch?v=jYa-gLEmYxM 👉 How To Calculate Force Using Newton’s 2nd Law Of Motion: Physics Made Easy | Tadashi Science https://www.youtube.com/watch?v=nR1kMuT03Wg 👉 Chemistry Basics: Understanding The Difference Between Atoms & Molecules | Tadashi Science https://www.youtube.com/watch?v=1PRAeq4_Gsk 👉 How To Calculate Kinetic Energy: Simple Formula & Easy Examples | Tadashi Science https://www.youtube.com/watch?v=aFZPWL8RqYw 👉 Physics Made Easy: Calculate Gravitational Potential Energy With The mgh Formula | Tadashi Science https://www.youtube.com/watch?v=YPeCawUjB4c ============================= ✅ About Tadashi Science. Need help making science simple to understand? Tadashi Science is here to make science SIMPLE! I produce short, easy-to-understand videos that cut out the fluff and get straight to the point. Science is easy, and I aim to present information in a simple and easy-to-understand manner. The videos get straight to the point and make learning easy and simple! On this channel, I break down challenging topics in various science subjects, including physics and chemistry, into simple lessons. Whether you're struggling with the laws of motion, chemical reactions, or any other scientific principles, my videos are designed to help you grasp the essentials quickly and efficiently. For Collaboration and Business inquiries, please use the contact information below: 📩 Email: tadashiscience@gmail.com 🔔 Want to master science quickly? Subscribe now for quick & short lessons and simple explanations that turn complex science topics into easy wins! https://www.youtube.com/@tadashiscience/?sub_confirmation=1 ================================= ADD HASHTAGS ⚠️ Disclaimer: I do not accept any liability for any loss or damage incurred from you acting or not acting as a result of watching any of my publications. You acknowledge that you use the information I provide at your own risk. Do your research. Copyright Notice: This video and my YouTube channel contain dialogue, music, and images that are the property of Tadashi Science. You are authorized to share the video link and channel and embed this video in your website or others as long as a link back to my YouTube channel is provided. © Tadashi Science via Tadashi Science https://www.youtube.com/channel/UCXrKyd6XS4oyhjKppE4ZZvw October 04, 2024 at 05:00PM

[sciencehook]

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[vidhyakshethra]

NCERT 12th Class : Atoms - II - Bohr's Atomic Model of Hydrogen Atom

[oylays]

Models of Atomic Structure In 1902 #English #scientist Joseph John Thomson created the first atomic model. He presented the #atom as #homogeneous matter with a positive charge. This matter fills the whole volume of the atom and contains tiny insertions of negative particles, like raisins in a pudding. In the history of science this model is still referred to as the “plum pudding model” or “raisin pudding.” Later the negative particles were named #electrons (from the Greek word for “amber”) and the positive ones got the name of #protons (from the Greek for the "first, basic"). The unfairly neglected creator of the second #atomicmodel was Hantaro Nagaoka, a pioneer in the field of #nuclear #physics in #Japan. According to Nagaoka, the structure of an #atom resembles the #planet #Saturn, in that it has a massive positively charged #nucleus with #electrons #revolving around it on one plane. #oylasciencemagazine #youthscience #youth #nz #auckland #oyla #oylascience #science #education #school #magazine For full information, subscribe to our magazine. https://www.oyla-science.com

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[babyawacs]

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#materialfatigue #condititons #of #applied @dino @doescience @sciam @science @nature @mathematics

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[pruebasypracticas]

Historia de los atomos.

Origen de la imagen

https://www.compoundchem.com/2016/10/13/atomicmodels/

Toda la materia está compuesta de átomos. Esto es algo que ahora tomamos como un hecho, y una de las cosas que aprende al comienzo de las clases de química de la escuela secundaria o secundaria. A pesar de esto, nuestras ideas sobre qué es un átomo son sorprendentemente recientes: hace tan solo cien años, los científicos aún debatían cómo era exactamente un átomo. Este gráfico analiza los modelos clave propuestos para el átomo y cómo cambiaron con el tiempo.

 Aunque nuestro gráfico comienza en el siglo XIX, la idea de los átomos existía mucho antes. De hecho, tenemos que regresar a la antigua Grecia para encontrar su génesis. La palabra "átomo" en realidad proviene del griego antiguo y se traduce aproximadamente como "indivisible". La teoría del griego antiguo se ha acreditado a varios eruditos diferentes, pero a menudo se atribuye a Demócrito (460-370 a. C.) y su mentor Leucipo. Aunque sus ideas sobre los átomos eran rudimentarias en comparación con nuestros conceptos actuales, esbozaron la idea de que todo está hecho de átomos, esferas invisibles e indivisibles de materia de tipo y número infinitos.

 Estos estudiosos imaginaron que los átomos varían en forma dependiendo del tipo de átomo. Imaginaban que los átomos de hierro tenían ganchos que los unían, explicando por qué el hierro era sólido a temperatura ambiente. Los átomos de agua eran suaves y resbaladizos, lo que explicaba por qué el agua era un líquido a temperatura ambiente y podía verterse. Aunque ahora sabemos que este no es el caso, sus ideas sentaron las bases para futuros modelos atómicos. 

 Sin embargo, fue una larga espera antes de que se construyeran estos cimientos. No fue hasta 1803 que el químico inglés John Dalton comenzó a desarrollar una definición más científica del átomo. Se basó en las ideas de los antiguos griegos al describir los átomos como esferas pequeñas y duras que son indivisibles, y que los átomos de un elemento dado son idénticos entre sí. El último punto es uno que sigue siendo cierto, con la notable excepción de los isótopos de diferentes elementos, que difieren en su número de neutrones. Sin embargo, dado que el neutrón no se descubriría hasta 1932, probablemente podamos perdonar a Dalton este descuido. También se le ocurrieron teorías sobre cómo los átomos se combinan para formar compuestos, y también se le ocurrió el primer conjunto de símbolos químicos para los elementos conocidos.

 El bosquejo de Dalton de la teoría atómica fue un comienzo, pero todavía no nos dijo mucho sobre la naturaleza de los átomos en sí. Lo que siguió fue otra pausa más corta en la que nuestro conocimiento de los átomos no progresó tanto. Hubo algunos intentos de definir cómo se verían los átomos, como la sugerencia de Lord Kelvin de que podrían tener una estructura similar a un vórtice, pero no fue sino hasta después del cambio del siglo XX que el progreso en dilucidar la estructura atómica realmente comenzó a recoger. 

 El primer avance se produjo a finales de 1800 cuando el físico inglés Joseph John (JJ) Thomson descubrió que el átomo no era tan indivisible como se afirmaba anteriormente. Realizó experimentos utilizando rayos catódicos producidos en un tubo de descarga, y descubrió que los rayos eran atraídos por placas de metal cargadas positivamente pero repelidas por las de carga negativa. De esto dedujo que los rayos deben estar cargados negativamente.

 Al medir la carga de las partículas en los rayos, pudo deducir que eran dos mil veces más livianas que el hidrógeno, y al cambiar el metal del que estaba hecho el cátodo pudo notar que estas partículas estaban presentes en muchos tipos de átomos. Había descubierto el electrón (aunque se refirió a él como un "corpúsculo"), y demostró que los átomos no eran indivisibles, sino que tenían partes constituyentes más pequeñas. Este descubrimiento le haría ganar un Premio Nobel en 1906. 

 En 1904, presentó su modelo del átomo basado en sus hallazgos. Apodado "El modelo de pudín de ciruela" (aunque no por el propio Thomson), preveía el átomo como una esfera de carga positiva, con electrones punteados como ciruelas en un budín. Los científicos habían comenzado a mirar dentro de las entrañas del átomo, pero el modelo de Thomson no se quedaría por mucho tiempo, y fue uno de sus estudiantes el que proporcionó la evidencia para enviarlo a la historia. 

 Ernest Rutherford era un físico de Nueva Zelanda que estudió en la Universidad de Cambridge con Thomson. Fue su trabajo posterior en la Universidad de Manchester lo que proporcionaría más información sobre el interior de un átomo. Este trabajo se produjo después de que ya había recibido un Premio Nobel en 1908 por sus investigaciones sobre la química de las sustancias radiactivas. Rutherford ideó un experimento para sondear la estructura atómica que implicaba disparar partículas alfa cargadas positivamente en una lámina delgada de lámina de oro. Las partículas alfa eran tan pequeñas que podían pasar a través de la lámina de oro, y de acuerdo con el modelo de Thomson que mostraba la carga positiva difundida sobre todo el átomo, debería hacerlo con poca o ninguna desviación. Al llevar a cabo este experimento, esperaba poder confirmar el modelo de Thomson, pero terminó haciendo exactamente lo contrario.

 Consultar entrada original en 

https://www.compoundchem.com/2016/10/13/atomicmodels/

[tutoroot]

What is the Comparison of Atomic Models? 

An atom is the smallest unit of matter that retains the properties of an element. It is composed of subatomic particles: protons, neutrons, and electrons. These particles interact to form the building blocks of all matter, from the simplest hydrogen atom to complex molecules. 

Early Ideas of Atomism (Greek Philosophers) 

Democritus (460–370 BCE) theorized that the universe comprises two entities: indivisible atoms and void (space). He believed atoms varied in shape, size, and motion, giving rise to the diverse materials we observe. However, due to the lack of scientific methods during his time, these ideas remained speculative. 

Dalton’s Atomic Theory 

Centuries later, in the early 19th century, John Dalton revitalized atomic theory with his scientific approach. His work marked the beginning of modern chemistry. 

Key Postulates 

Indivisibility: Atoms are indivisible and indestructible. 

Identical Elements: Atoms of the same element are identical in mass and properties. 

Compound Formation: Atoms combine in simple whole-number ratios to form compounds. 

Chemical Reactions: Chemical reactions involve the rearrangement of atoms, but the atoms themselves remain unchanged. 

Limitations of Dalton’s Theory 

Dalton’s theory had several limitations: 

It could not explain the existence of isotopes (atoms of the same element with different masses). 

The idea of indivisible atoms was later disproven by the discovery of subatomic particles. 

Discovery of Subatomic Particles 

The late 19th and early 20th centuries saw groundbreaking discoveries that unveiled the internal structure of atoms. 

Electron: J.J. Thomson’s Cathode Ray Experiment 

J.J. Thomson’s cathode ray tube experiment demonstrated the existence of negatively charged particles called electrons. He observed that cathode rays were deflected by electric and magnetic fields, proving they were composed of charged particles. This discovery challenged Dalton’s notion of indivisible atoms. 

Proton: Goldstein’s Experiment 

Eugen Goldstein, using a modified cathode ray tube, discovered positively charged particles, later named protons. These particles had a much greater mass than electrons and were crucial in balancing atomic charge. 

Neutron: James Chadwick’s Discovery 

In 1932, James Chadwick discovered neutrons, uncharged particles located in the atomic nucleus. Neutrons explained the mass differences between isotopes and further refined the atomic model. 

Thomson’s Plum Pudding Model 

Following his discovery of electrons, J.J. Thomson proposed the “plum pudding” model in 1904. 

Description of the Model 

Thomson envisioned the atom as a spherical cloud of positive charge with negatively charged electrons embedded within it, resembling raisins in a pudding. 

Limitations of the Plum Pudding Model 

While the model explained atomic neutrality, it failed to account for the arrangement of subatomic particles or the existence of a dense nucleus. 

Rutherford’s Nuclear Model 

Ernest Rutherford’s gold foil experiment in 1911 revolutionized atomic theory. 

Gold Foil Experiment 

Rutherford bombarded a thin gold foil with alpha particles and observed their scattering pattern. Most particles passed through, but some were deflected at large angles. 

Observations and Conclusions 

Atoms consist of a dense, positively charged nucleus. 

Electrons orbit the nucleus, with most of the atom being in space. 

Drawbacks of Rutherford’s Model 

Rutherford’s model could not explain the stability of atoms, as orbiting electrons should lose energy and spiral into the nucleus. 

Bohr’s Model of the Atom 

Niels Bohr refined Rutherford’s model by introducing quantum concepts. 

Postulates of Bohr’s Theory 

Electrons orbit the nucleus in fixed energy levels or shells. 

Electrons can transition between energy levels by absorbing or emitting energy. 

Explanation of Hydrogen Spectrum 

Bohr’s model explained the discrete spectral lines of hydrogen, corresponding to electron transitions between energy levels. 

Successes and Limitations 

While Bohr’s model successfully described hydrogen, it could not account for more complex atoms or the behaviour of electrons as waves. 

Quantum Mechanical Model 

The quantum mechanical model, developed in the 20th century, provided a more comprehensive understanding of atomic structure. 

Introduction to Wave-Particle Duality 

Electrons exhibit both particle-like and wave-like behaviour, as demonstrated by experiments such as the double-slit experiment. 

Schrodinger’s Equation (Basic Understanding) 

Erwin Schrödinger developed a mathematical equation to describe the behaviour of electrons in terms of probability rather than fixed orbits. 

Concept of Orbitals 

Orbitals are regions around the nucleus where electrons are most likely to be found. These are categorized into s, p, d, and f shapes, representing different energy levels and sublevels. 

Comparison of Atomic Models 

Key Differences Between Thomson, Rutherford, and Bohr Models 

Feature 

Thomson Model 

Rutherford Model 

Bohr Model 

Nucleus 

Absent 

Present 

Present 

Electron Arrangement 

Embedded in a sphere 

Orbiting the nucleus 

Fixed energy levels 

Stability Explanation 

None 

Incomplete 

Quantum transitions 

The evolution of atomic theory reflects humanity’s relentless pursuit of knowledge, from the speculative ideas of ancient philosophers to the precise quantum mechanical models of today. Each advancement has not only deepened our understanding of matter but also driven technological innovation, shaping the modern world. 

For more simplified explanations like the one above, visit the physics blogs on the Tutoroot website. Elevate your learning with Tutoroot’s personalised Physics online tuition. Begin your journey with a FREE DEMO session and discover the advantages of one on one personalised tuitions. 

For students looking to master these concepts and excel in their studies, platforms like Tutoroot provide personalised guidance, interactive learning resources, and expert tutoring tailored to individual needs. With Tutoroot’s support, exploring the fascinating world of atomic models becomes an engaging and enriching experience. 

[tracyctr-blog]

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[vidhyakshethra]

NCERT 12th Class : Atoms - III - Bohr's Atomic Model of Hydrogen Atom Contd

[babyawacs]

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