Sommerfeld corrections to Bohr model.pdf
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Sommerfeld extended the Bohr model of the atom by introducing elliptical electron orbits and an azimuthal quantum number. This accounted for variations in the electron's velocity around the elliptical orbit and introduced a relativistic correction term to the electron's energy. Sommerfeld's model explained the fine structure splitting of spectral lines as arising from small differences in the energy levels of elliptical orbits due to the azimuthal quantum number.
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This document provides an overview of atomic physics, including:
1. Models of the atom including Rutherford and Bohr models, and explanations of atomic energy levels and quantum numbers.
2. Quantum physics concepts including Planck's quantum theory, Einstein's theories of light and the photoelectric effect, and de Broglie's hypothesis of matter waves.
3. Lasers including production of laser light, properties, types, and applications.
4. Nuclear physics including structure of the nucleus, radioactive decay, nuclear stability, fission and fusion processes, and applications of nuclear technology.
Bhor's Atomic model
1. Electromagnetic radiation travels as waves through space at the speed of light and includes radio waves, microwaves, infrared, visible light, ultraviolet, X-rays and gamma rays.
2. Wavelength is the distance between peaks of a wave and frequency is the number of waves passing a point per second.
3. The Bohr model describes atoms with electrons orbiting the nucleus in discrete energy levels, absorbing or emitting energy when changing orbits.
electronic configuration
The document discusses electronic configurations of atoms. It explains that the electron configuration represents the arrangement of electrons in an atom's orbital shells and subshells in its ground state, and can also represent ionized atoms. Many physical and chemical properties correlate to unique electron configurations, especially the valence electrons in the outermost shell. Electrons fill orbitals according to increasing energy levels and subshells in a set order. Orbital diagrams, spdf notation, and noble gas notation are used to represent electron configurations.
Chapter4electronsinatoms 111110092817-phpapp02
This document provides a summary of key concepts about electrons in atoms, including:
1) It discusses the evolution of atomic models from Rutherford to Bohr, focusing on explaining the arrangement of electrons. The quantum mechanical model describes electron probability clouds rather than fixed orbits.
2) It covers atomic orbitals and how electrons fill different orbitals based on their principal and angular momentum quantum numbers. Higher principal quantum numbers correspond to higher energy levels further from the nucleus.
3) The document emphasizes that electrons fill orbitals based on the Aufbau principle to achieve the lowest possible energy configuration. Understanding electron configurations is essential to describing elements and their properties.
Quantum theory and the atom
The highest energy level in Bohr's model of the atom is the one that is farthest from the nucleus. According to Bohr's model, electrons can only exist at certain discrete energy levels or orbits around the nucleus, with the lowest energy level being closest to the nucleus. When an electron gains energy, it moves to a higher energy level in an "excited state". It then releases energy as a photon when it falls back to its lower "ground state". Later, the quantum mechanical model improved on Bohr's model by treating electrons as waves rather than definite orbits, better explaining experimental observations.
Ch06 outline
The document discusses the electronic structure of atoms. It introduces quantum numbers like the principal quantum number n, angular momentum quantum number l, and magnetic quantum number ml, which describe the allowed electron orbitals in an atom. The Pauli exclusion principle states that no two electrons can have the same set of quantum numbers. Electron configurations show how electrons are arranged among the orbitals in an atom based on filling orbitals in order of increasing energy.
AP Chemistry Chapter 6 Outline
The document discusses the electronic structure of atoms. It introduces quantum numbers like the principal quantum number n, angular momentum quantum number l, and magnetic quantum number ml, which describe the allowed orbitals for electrons. Orbitals include s, p, and d orbitals with different shapes. The Pauli exclusion principle states that no two electrons can have the same set of quantum numbers. Electron configurations show how electrons are arranged in orbitals based on increasing energy.
Tang 02 wave quantum mechanic model
This document provides information on wave quantum mechanics and electron configurations. It discusses:
- Erwin Schrodinger's contributions to developing quantum mechanics and proposing the wave-like nature of electrons.
- How electrons occupy distinct energy levels and orbitals around the nucleus, rather than defined circular orbits. Electrons have wave-like properties.
- The shapes of s, p, d and f orbitals and how electrons fill these orbitals according to various principles like Aufbau and Hund's rule.
- Exceptions to the Aufbau principle seen in some elements.
- How to represent electron configurations using both energy level diagrams and shorthand notation.
Tang 02 wave quantum mechanic model
This document provides information on wave quantum mechanics and electron configurations. It discusses:
- Erwin Schrodinger's contributions to developing quantum mechanics and proposing the wave-like nature of electrons.
- How electrons occupy distinct energy levels and orbitals around the nucleus, with specific shapes defined by Schrodinger's wave equation.
- Rules for building up electron configurations, including Hund's rule and the Aufbau principle for filling orbitals in order of increasing energy.
- Exceptions to the Aufbau principle seen in some transition metals where half or fully filled subshells are more stable.
- How electron configurations are written using shorthand notation based on noble gas cores.
Chapter 4 electrons in atoms
This chapter discusses the evolution of atomic models and the arrangement of electrons in atoms. It covers difficult concepts such as electrons occupying specific energy levels and orbitals. Students are advised to do all assigned homework and bring their textbook to class to fully understand these abstract ideas. Key models discussed include the Rutherford model, the planetary model, Bohr's model linking electrons and photon emission, and the modern quantum mechanical model based on probability.
Fine structure constant.pdf
It is also renowned as the Sommerfeld constant. So, its name signifies that it is a constant quantity introduced by the German physicist Arnold Sommerfeld in 1916 to determine the size of fine-structure splitting of the hydrogen spectrum.
In fact, Sommerfeld extended the Bohr atomic model to explain the fine structures of the hydrogen spectrum by introducing the relativistic variation of electron mass with velocity in the elliptical electron orbits. To account for the amount of splitting of spectral lines, he entailed a term that he named fine structure constant. In Sommerfeld's analysis, it was the ratio of the electron's velocity in the ground state of the relativistic Bohr atom to the speed of the light in the vacuum. And he used the Greek letter α (alpha) to symbolize it.
For more information on this concept, kindly visit our blog post at;
https://jayamchemistrylearners.blogspot.com/2022/04/bohr-sommerfeld-model-chemistrylearners.html
Adv chem chapt 7
This document discusses the development of atomic structure models from the early 20th century to the present. It describes experiments that showed light and matter have both wave-like and particle-like properties. This led to the development of quantum mechanics and quantum numbers to describe electron orbitals. The Bohr model of the hydrogen atom was an early success but did not apply to other atoms. Modern quantum mechanics uses probability distributions and accounts for electron spin and the Pauli exclusion principle.
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de-Broglie equation.pdf
If everyone is thinking alike, we cannot solve the hurdles of a problem. It seems true if we observe these hypotheses' hierarchy once. Italian physicist Francesco Maria Grimaldi discovered the wave phenomenon of light in 1665. But the uncertainty about light's nature was finally solved by Einstein's explanation of the photoelectric effect. Similarly, Neil Bohr succeeded in describing the structure of an atom with quantized electron orbits. But his stipulation of allowed stationary orbits was only a supposition until the discovery of the de-Broglie equation.
Louis de-Broglie, a French physicist, presumed that moving microscopic and macroscopic objects are waves. He introduced a word called 'matter wave' to describe the waves of material objects in motion. As a result, matter exhibits a dual character of both particle and wave. Moreover, he derived an empirical formula to measure the wavelength of matter waves in 1923 called the de-Broglie equation.
Wien displacement law graph.pdf
It is a graphical explanation of a blackbody's emissive power and radiation wavelength at various temperatures. We know blackbody emissions are temperature specific. And a blackbody graph is an overall variation of a blackbody's emissive power as a function of wavelength measured at different temperatures. But the Wien displacement law graph focuses on spectral intensities of blackbody emissions as a function of wavelength at a peak wavelength state λmax at a specific temperature T.
MCQs of blackbody & its radiation .pdf
It is an e-book of MCQs & answers on blackbody. It is in PowerPoint format with 40 questions and detailed answer explanation that makes you clear every single point of blackbody and its radiation. The e-book has 54 beautifully designed slides. The contents of the e-book are below.
Multiple choice questions and answers - 20 no.s
True or false questions-10 no.s
Reasoning questions - 10 no.s
To disclose all the contents of the e-book, visit this link.
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Fatafat check list of blackbody.pdf
A blackbody is an imaginary object that absorbs all incident light without reflecting any, invented by German physicist Gustav Kirchhoff in 1860 to help understand thermal radiation. Examples of materials that approximate a blackbody include lamp black, graphite, and platinum black. The energy distribution of electromagnetic radiation emitted by a blackbody, known as blackbody radiation, depends only on the body's temperature according to Planck's law.
Wien displacement law .pdf
It discusses Wien displacement law. To go through the numerical problems of the Wien displacement law topic, visit our e-book at;
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The blackbody is a hollow enclosure with a pinhole to emit its radiations. The secure covering of the blackbody prevents the absorbed light from escaping.
A blackbody is a solid closed unreal body that is inexistent. But lamp black, platinum black, and graphite-coated surfaces are non-ideal black bodies for laboratory purposes. An object with above 0.95 emissivities is an approximate blackbody. Besides, the hotter bodies emitting electromagnetic radiation under thermal equilibrium conditions are also considered partial black bodies.
Blackbody mind map.pdf
An ideal black body is an imaginary concept developed by Gustav Kirchhoff that perfectly absorbs all electromagnetic radiation that falls on it and reflects none. It plays a significant role in quantum mechanics by being a perfect emitter and absorber of thermal radiation, releasing electromagnetic radiation when heated that follows specific laws like Planck's quantum law, Wien's displacement law, and Stefan-Boltzmann law. Real blackbodies have opaque, closed surfaces that absorb radiation based on factors like temperature, emissivity, and surface area, and their radiation is used in applications like thermal imaging, optical sensors, and burglar alarms.
Blackbody Vs. graybody.pdf
It explains the difference between a blackbody and a gray body following Kirchhoff's law of thermal radiation.
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https://kameswariservices201831.myinstamojo.com/product/3439450/planck-quantum-theory-postulates
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It is a PowerPoint presentation of Kirchhoff's law of thermal radiation. And it gives a brief idea of Kirchhoff's law, its applications, and examples. Moreover, it explains the terms absorptivity, emissive power, thermal equilibrium, and emissivity.
Kirchhoff's law.pdf
It discusses Kirchhoff's law and its examples. It explains blackbody emissions in thermal equilibrium conditions.
We are sorry to inform you about a small error in Kirchhoff's formula section of the above infographic. Kirchhoff's formula states that the absorptivity and emissivity of the body are equal in thermal equilibrium conditions. 'a' is the absorbing power of the body at a wavelength λ. And 'e' is the emissivity of the body at the same wavelength. So, we will write aλ=e but not aλ=eλ. We request you read it correctly while going through the PDF.
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Planck's constant.pdf
It describes the definition of Planck's constant. Planck constant helps compute the discrete energy changes of a body by relating to the frequency of the photon. Planck constant explains the proportionality relationship between the photon's energy and the frequency.
For more information on this topic, kindly visit our blog article at;
https://jayamchemistrylearners.blogspot.com/2022/08/plancks-constant-chemistry-learners.html
Numerical problems of Planck's quantum theory.pdf
It is a PowerPoint presentation on numerical problems of Planck quantum theory topic.
It includes 12 numerical problems with solved answers. Besides, this PowerPoint presentation has a mind map to remember all formulas of Planck quantum law.
MCQ on Planck constant.pdf
This document contains 10 multiple choice questions about Planck's constant. It provides explanations for why Planck's constant was introduced, its value in different units, and that it explains both the quantum and particle nature of light. The questions cover topics like the relationship between photon energy and frequency, experimental methods used to determine Planck's constant, and why LED lights are used in these calculations. Additional resources on Planck's constant and quantum theory are provided at the end.
Detailed light theories.pdf
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Theories of light.pdf
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The document contains 10 multiple choice questions about the hydrogen spectrum. It discusses that the essential condition to observe the hydrogen spectrum is high temperature and low pressure. The hydrogen spectrum appears as distinct lines, with the prominent line being red with a wavelength of 656 nm. It is an example of a line spectrum and can be recorded using a spectroscope. Robert Bunsen and Gustav Kirchhoff discovered the hydrogen spectrum and spectroscope, while Isaac Newton first discovered the word "spectrum".
Rydberg equation.pdf
The Rydberg formula helps to determine the wavenumber or wavelengths of hydrogen spectral lines obtained in the hydrogen spectrum. Previously, Johann Jakob Balmer discovered an empirical formula to determine the wavelengths of hydrogen spectral lines obtained in the visible region of the hydrogen spectrum. As we all know, the hydrogen spectrum is not limited to the visible zone only. It occupies the ultraviolet and infrared parts of the electromagnetic spectrum also. Hence, the scientists' quests to determine the spectral positions of various spectral lines of the hydrogen spectrum finally came to an end with the Rydberg formula.
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- 1. Sommerfeld described that a portion of electron energy is associated with its orbital motion. To enumerate the orbital angular momentum, he introduced a new quantum number named azimuthal quantum number. The letter 'k' denotes it. And its value varies from 1 to n, where n is a principal quantum number. Sommerfeld corrections to Bohr atomic model E l l i p t i c a l e l e c t r o n o r b i t s In Sommerfeld extension, the path of the electron's rotation is an ellipse with a major and a minor axes of 2a & 2b lengths. Out of the two foci on the major axis, the nucleus locates in only one of them. I n t r o d u c t i o n o f a z i m u t h a l q u a n t u m n u m b e r The considerable variation in the electron’s velocity on the elliptical orbit added a new relativistic correction term to the total energy of the electron. Now, the modified Sommerfeld’s energy equation is below. E n e r g y c o r r e c t i o n t e r m R e l a t i v i s t i c e l e c t r o n m o t i o n In the Sommerfeld model, the electron travels at nearly the speed of the light. Hence, its motion is relativistic. Moreover, the velocity of the electron moving in the elliptical orbit is different at the various parts of the ellipse. And it causes a relativistic variation in the electron’s mass. It changed the path of the electron from a simple ellipse to a more complicated rosette structure. E x p l a n a t i o n f o r f i n e s t r u c t u r e s If you observe the energy equation, you can understand that the electron's energy not only depends on the principal quantum number but also on the azimuthal quantum number. This correction brought a variation in the energy of the elliptical orbits. The electron transitions to energy levels that have a slight difference in energies will show spectral line splitting. The splitting of the spectral lines into two or more components with a mild variation in their wavelengths is known as fine structures. Even though Bohr successfully explained the structure of an atom with circular stationary orbits, it could not explain the fine structures of spectral lines. In 1916, Sommerfeld extended the Bohr model to explain spectral line splitting. Blog:https://jayamchemistrylearners.blogspot.com/