EM Spectrum, de Broglie, PE Notes
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The document discusses key concepts in the development of quantum theory including: 1) De Broglie hypothesized that particles like electrons exhibit wave-like properties and can have an associated wavelength. 2) Schrodinger used de Broglie's idea to develop the first quantum theory based on wave equations to describe electrons rather than classical orbits. 3) Heisenberg formulated the uncertainty principle - that the exact position and momentum of a particle cannot be known simultaneously. 4) Experiments on the photoelectric effect showed photons eject electrons from metals immediately, contradicting classical wave theory but supporting a particle-like nature for photons.
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- The principle of complementarity states that matter and light cannot be fully described as either purely waves or particles, as the two models complement each other and neither is complete. Observing one property precludes observation of the other.
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This document discusses the structure of the atom. It begins by describing Bohr's model of the atom and its limitations. It then introduces shells and subshells, as well as quantum numbers and the shapes of atomic orbitals. Rules for filling electrons into orbitals, such as the Aufbau principle and Pauli exclusion principle, are also covered. The document discusses atomic spectra, photoelectric effect, and the dual wave-particle nature of light and matter. It provides an overview of concepts like de Broglie wavelength, Heisenberg uncertainty principle, and atomic electron configuration.
Strawberry model2new
The document discusses several topics related to atomic structure and quantum mechanics. It begins by discussing quantization and how the work of Planck, Einstein, and others led to the concept of photons and quantized energy levels in atoms. It then discusses the photoelectric effect demonstrated by Einstein that helped establish the particle nature of light. Finally, it discusses population inversion in lasers and how certain materials like argon can be excited to a state that allows for stimulated emission of coherent light.
Quantum physics
Quantum Physics is already a very interesting subject, and so even though the presentation has all the required information to get yourself a hold on the subject, I would highly recommend everyone to do some extensive research. Well actually, there is no need for anyone to point out on the research part, you will automatically find yourselves filling the search history with some deep quantum-ish.
Astonishing Astronomy 101 - Chapter 4
This document provides an overview of spectroscopy and how it can be used to determine the composition of astronomical objects. It discusses how light interacts with matter on an atomic level, causing absorption and emission spectra that act as "elemental barcodes." The spectra are caused by electrons transitioning between quantized energy levels in atoms and emitting or absorbing photons of specific wavelengths. Measuring the absorption lines in a star's spectrum allows astronomers to identify the elements present in a star's atmosphere and determine its chemical composition, such as the fact that hydrogen and helium make up over 97% of the Sun's mass.
Particle Properties of Waves
This document discusses the development of quantum mechanics. It summarizes that classical physics could not explain certain experimental observations, leading to quantum theory. Key events were Planck's blackbody radiation law, Einstein's explanation of the photoelectric effect using light quanta (photons), and Compton's discovery that photons transfer momentum to electrons. The photoelectric effect showed that light behaves as particles (photons), while the de Broglie hypothesis and Davisson-Germer experiment showed that electrons can behave as waves. This established the wave-particle duality of both light and matter.
Ch.7 Modern Physics - 1.ppt
Quantum theory describes the behavior of matter and energy at the microscopic scale. Some key ideas are:
- Light and matter can behave as both particles and waves (wave-particle duality).
- Planck's constant relates the energy of a system to its frequency or wavelength.
- Einstein's photon model explained the photoelectric effect.
- The Heisenberg uncertainty principle limits the precision with which certain pairs of physical properties can be known.
- Schrödinger's equation describes how quantum systems evolve over time.
Matter wave, atomic spectrum and Bohr model.pptx
introduction to matter wave, atomic spectrum and Bohr model
Diploma sem 2 applied science physics-unit 5-chap-2 photoelectric effect
This document summarizes the photoelectric effect and its laws and characteristics. It describes how the photoelectric effect was discovered and involves the emission of electrons from metal surfaces when light shines on it. The key laws are that photoelectric current is proportional to light intensity, there is a threshold frequency below which no emission occurs, and kinetic energy depends on frequency not intensity. Characteristics explained include how intensity affects current but not energy, and how increasing frequency increases energy. Einstein's model using photons is described along with the photoelectric equation. Applications of photocells are provided.
Chapter 3 photoelectric effect
The document discusses the photoelectric effect and provides details on several key topics:
1. It outlines 5 main subtopics to be covered in the chapter, including how the intensity and frequency of light affects photoelectrons and the quantitative equations involved.
2. It describes the photoelectric effect as the emission of electrons from a metal surface when light shines on it. Experimental results showed inconsistencies with the wave theory of light.
3. Einstein's photon theory predicted the kinetic energy of ejected electrons would increase linearly with frequency, in agreement with experiments, resolving discrepancies with the wave theory.
Chapter 3 photoelectric effect
The document summarizes key concepts about the photoelectric effect from the chapter on photoelectricity. It discusses 5 main topics to be learned: how intensity and frequency of light affect photoelectrons, photoelectric current graphs, quantitative equations for work function and threshold frequency, the photon theory of light, and why wave theory fails to explain the photoelectric effect. It provides definitions and examples of photoelectric terms and experiments. The document contrasts predictions of wave and photon theories, and shows photon theory agrees with experimental results that kinetic energy increases linearly with frequency.
Wave mechanics
The document discusses wave-particle duality and Louis de Broglie's hypothesis that all matter has both wave-like and particle-like properties. It summarizes key experiments that supported this idea, including Davisson and Germer's 1927 experiment in which electron beams were diffracted by crystal lattices, demonstrating their wave-like behavior. The document also explains how de Broglie's hypothesis resolved issues with early atomic models by introducing the concept of electron standing waves within atoms.
Unit 6 Presentation.ppt
Light was originally thought to behave as waves, but evidence showed it also behaves as particles. Max Planck's work established that light transfers energy in discrete packets called quanta. Albert Einstein later proposed that light consists of small particles called photons that exhibit wave-like properties. The photoelectric effect provided further evidence that light behaves as both waves and particles. Electrons also exhibit dual wave-particle properties, with wavelengths determined by the de Broglie equation. Heisenberg's uncertainty principle states the exact position and momentum of an electron cannot be known simultaneously. Quantum theory describes electrons as existing in distinct energy levels around an atom's nucleus.
Cmcchapter05 100613132827-phpapp02
The document discusses electrons in atoms and is divided into three sections. Section 5.1 covers light and quantized energy, explaining that light has both wave and particle properties and matter emits and absorbs energy in quanta. Section 5.2 discusses quantum theory and the atom, comparing Bohr's model to the quantum mechanical model which assumes electrons have wave properties. Section 5.3 is about electron configuration, explaining that the arrangement of electrons in an atom follows rules such as the aufbau principle and can be represented with orbital diagrams and electron configuration notation.
Basic Quantum Theory
Basic Quantum Theory:
Particle properties of waves
Blackbody radiation
Photoelectric effect
Compton effect
Wave properties of particles
Davisson–Germer experiment
Double slit experiment with particles
Thank you
Preeti Choudhary
Chaudharypreeti1997@gmail.com
https://www.linkedin.com/in/preeti-choudhary-266414182/
https://t.me/physiwaves
https://t.me/barcphysics
https://t.me/phyiscswaves
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EM Spectrum, de Broglie, PE Notes
- 4. de Broglie • Pictured the electron in its circular orbit as a particle wave • Can produce "standing waves" under resonant conditions • Developed the idea that a particle with mass, m, and a velocity, v, has a wavelength associated with it => de Broglie Wavelength
- 5. de Broglie
- 6. de Broglie
- 7. de Broglie
- 8. Schrödinger • Used de Broglie wavelength to create a quantum theory based on waves • Did not keep the "orbits" • The wave/particle model cannot determine the location and momentum of an electron at the same time • The quantum model predicts the probability that an e- is at a specific location
- 9. Heisenberg Uncertainty Principle • Can only determine the location or the momentum (velocity) of the particle - not both at the same time!
- 11. Photons and Photoelectric Effect
- 12. Photoelectric Effect • Metal is illuminated by electromagnetic radiation • Energy that is absorbed near the surface can free electrons, causing e's to fly off • Released electrons are called photoelectrons
- 13. Wave theory predicts the following: • Significant time delay between the illumination and ejection - build up of KE to free e-'s • Increasing the intensity of light = cause electrons to leave with greater KE • Photoelectrons would be released regardless of frequency of light, as long as the intensity was great enough.... But these are FALSE!
- 14. Photoelectric Effect Findings • Photons were ejected immediately • Increasing the intensity did not change the KE although more e-'s were ejected, KE does not increase. • If the frequency fell below a threshold (specific for each metal), no photoelectrons would be ejected, regardless of intensity! • If the frequency increases above the threshold, KE increases linearly
- 16. PE Effect - Math • Threshold Frequency • Work Function - the minimum amount of energy required on a metal surface to eject an electron • How are these two related?
- 17. PE Effect - Math