Quantum Physics

• Wave-Particle Duality


  A property where particles, such as electrons or photons, can exhibit both wave-like and particle-like behavior.
• Wave-like behavior


  Exhibits diffraction, interference, and superposition.
• Particle-like behavior


  Exhibits definite position, definite momentum, and discrete packets.
• Double-Slit Experiment


  An experiment where electrons passing through two slits create an interference pattern, showing wave-like behavior, but behave like particles when observed individually.
• Work Function


  The minimum energy required to remove an electron from a solid or metal and convert it into a free electron.
• measured in

  Electronvolts (eV).
• used in

  Electron spectroscopy to study the electronic properties of materials.
• Fluorescent Lamp


  A type of electric lighting that uses an electric current to excite a gas, which produces light.
• Phosphor Coating


  Converts ultraviolet light into visible light.
• Phosphor Coating


  A thin layer of phosphor material that covers the inside of the glass tube in a fluorescent lamp.
• UV Light


  Produced by the excited gas inside the tube in a fluorescent lamp.
• Phosphor Emits


  Energy as visible light, releasing it in a specific color.
• Phosphor Absorbs


  UV light and converts it into visible light.
• Line Spectra Absorption


  A technique used to study the interaction between light and matter, showing the absorption of specific wavelengths of light by a gas or chemical sample.
• Monochromatic Light


  Light with a single wavelength.
• Gas Sample


  Used to study electronic transitions within atoms or molecules.
• Line Spectra


  A plot of the intensity of the light as a function of its wavelength, showing distinct lines corresponding to the absorption of specific wavelengths.
• Absorption Spectrum


  A plot of the intensity of the transmitted light versus its wavelength, used to identify the presence of specific elements or molecules.
• Line Spectra Emission


  A technique used to study the interaction between light and matter, showing the emission of specific wavelengths of light by a gas or chemical sample.
• Excitation Energy


  Added to a gas or chemical sample to cause energy release as light.
• Gas Sample


  Used to study energy levels and transitions within atoms or molecules.
• Emission Spectrum


  A plot of the intensity of the light as a function of its wavelength, showing distinct lines corresponding to the emission of specific wavelengths.
• Line Spectra


  A plot of the intensity of the light as a function of its wavelength, used to identify the presence of specific elements or molecules.
• Ground State


  The lowest energy state of an atom, where the electrons are in their most stable configuration.
• Excited States


  Higher energy states of an atom, where the electrons are in a higher orbital or have gained energy.
• Energy Levels


  Discrete values of energy that an atom can have, corresponding to the different electron configurations.
• Transitions


  Changes between energy levels, such as when an electron moves from a higher energy level to a lower energy level.
• Discrete Energy Levels


  Energies that an electron can occupy are limited to specific values, with no values in between.
• Atom-Specific Energy Levels


  Different atoms have unique energy levels due to the arrangement of their electrons.
• Absorption of Energy


  When an atom absorbs energy, an electron moves from a lower energy level to a higher energy level.
• Emission of Energy


  When an atom emits energy, an electron moves from a higher energy level to a lower energy level.
• Collisions


  When atoms collide, energy can be transferred between them, causing transitions between energy levels.
• Radiation


  Exposure to electromagnetic radiation, such as light or radiation, can also cause transitions between energy levels.
• Energy Interactions


  Various energy interactions can cause transitions between energy levels, including absorption and emission of energy.
• Stopping Potential


  The minimum negative voltage required to prevent the emission of electrons from a metal.
• Electron Emission


  When a metal is bombarded with photons or other particles, it can emit electrons.
• De Broglie Hypothesis


  In 1924, Louis de Broglie proposed that particles, such as electrons, can exhibit wave-like behavior.
• Wave-Particle Duality


  De Broglie's hypothesis states that particles can exhibit both wave-like and particle-like behavior.
• Wavelength


  De Broglie relation: wavelength (λ) is inversely proportional to the momentum (p) of a particle: λ = h/p, where h is Planck's constant.
• Vacuum Photocell


  A device that uses the photoelectric effect to convert light into electrical energy.