CH 115 1st Edition Lecture 5Unit 1: Atoms, Isotopes, and IonsOutline of Last Lecture I. Photoelectric Effecta. Definition and InsightII. Line Emission Spectruma. Definition and Insightb. Second Energy EquationOutline of Current Lecture III. Wave Particle DualityVI. Heisenberg Uncertainty Principle VII. Quantum Numbersa. Electron Shells and Subshells b. Principal, Subsidiary and Magnetic Quantum NumbersCurrent LectureWave Particle DualityWave-Particle Duality– Having the same properties as a wave and a particle. Originally presented by Louis de Broglie.- Wave-particle duality is exhibited by electrons, light and even mangos. - Electrons go through diffraction and can interact with each other as waves, but they also act as electric charges and have particle-like mass.- Light is seen as a wave because itcan diffract, reflect, refract, andinterfere like all other waves.- At certain times, however, scientistscouldn’t explain some of thestrange behaviors of light.- That was, until Einstein proposedthe photoelectric effect (electronsare “knocked” off of metal whenlight is shined on it), which explained the odd behaviors of light and greatly supported wave-particle duality. These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.- When light hits a metal, electrons are released through the energy of photons (particles of light). This proved that wave and particle characteristics could overlap.- The behavior of larger objects are dominated by their particle nature, so if electrons exhibit wave-particle duality then all matter would exhibit it as well (including mangos ).- Louis de Broglie showed that both light andmatter exhibited properties of waves andparticles. He developed this formula to calculate the wavelength associated with particles and their momentum (momentum=mv-mass times velocity; “h” represents Planck’s constant.):Heisenberg Uncertainty PrincipleIt’s impossible to know the exact position and exact momentum of an objectsimultaneouslyThe reason for this is simple: basically when you try to find one (whether position or momentum), you alter the other (again, position or momentum): If you wanted to know the position of a particle, you would need to use high frequency light. However, you wouldn’t be able to find the momentum, because the light altered it. If you wanted to know the momentum of a particle, you would need to uselow frequency light. Unfortunately, you wouldn’t be able to locate the position at that exact time, since the particle would have moved. Even with extensive experimentation, it has been proven impossible to know the location and momentum of a particle, simultaneously.Quantum NumbersThere are 4 kinds of quantum numbers: Principal quantum number: n = 1, 2, 3, 4, ...o Determines relative energy & orbital size Subsidiary quantum number: l = 0, 1, 2, …, (n‐1)o Determines orbital shape (& some energy) Magnetic quantum number: ml = (-l, …, 0, …, l)o Determines orientation Spin quantum number: ms = +½ or ‐½o Determines spin- The principal quantum number defines a “shell.”- The principal and subsidiaryquantum numbers define a “subshell.”- The principal, subsidiary and magneticquantum numbers define an “orbital.”- All four quantum numbers (n, l, ml, ms) define a specific electron.- The principal quantum number corresponds to the energy level (n=1 is the first energy level or “ground state”).- These energy levels are the same as the periods (rows) of the periodic table (i.e. Hydrogen is in the n=1