Light (Particle or Wave)?
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1 Sir Isaac Newton ( ) Corpuscular Theory of Light Classical Laws of Mechanics (3 Laws of Motion) Greatest and most influential scientist to ever live Einstein kept a framed picture of him Light (Particle or Wave)? James Clerk Maxwell ( ) Set of equations to describe Electricity, Magnetism and Optics. Kinetic Theory of Gases (Maxwell- Boltzmann Distribution) 3 rd Greatest Scientist of All Time "Light is never known to follow crooked passages nor to bend into the shadow" Thomas Young ( ) Double Slit Experiment Constructive and Destructive Inference Notable scientific contributions to vision, light, solid mechanics, energy, physiology, language, musical harmony, and Egyptology. Christiaan Hugens ( ) Wave Theory of Light Invented Pendulum Clock, Probability Theory
2 Planck Black Body Radiation Classical Model Fails (UV Catastrophe) Energy (Light) is quantized No reason why its quantized Einstein Photoelectric Effect Classical Model Fails (Blue and Red light should eject same number of electrons if they have the same intensity (wavelength and frequency should have no effect) Energy (Light) is quantized in order to explain why a threshold exists No reason why its quantized Rutherford Model Bohr Model De Broglie Model To Heisenberg Electrons are allowed to be anywhere Predicts continuous or rainbow like spectrum Flaw: Fails to explain Line Spectra Electrons are in quantized orbitals Predicts line spectrum Flaws (1) No reason its quantize (2) Does not work for > 1 e If light can behave like a wave and a particle than an electron can behave like a particle and a wave. Explained Quantization of Electron Orbitals therefore fixing Flaw (1). Model still fails for > 1 e Line Spectra Normal Light Rutherford Model Actual Experiment Pure Elements
3 Pauli Exclusion Principle No two electrons in an atom can have the same 4 QN s Hund s Rule Two or more orbitals with the same energy, electrons will fill each until ½ full. Electrons in partially filled orbitals have the same spin QN (spin aligned. From De Broglie Heisenberg Uncertainty Principle It is impossible to know precisely where an electron is and what path it follows. 4 Uncertainty in the position of the electron is larger than the size of the atom orbitals can t exist No model Energy Level Filling Diagrams Schrodinger Equation Statistical model using wave equations to describe the location of the electron. Does not violate Heisenberg 4 Principle Quantum Numbers result Electron Configurations To Periodic Trends Principle Quantum Number (n) 1, 2, 3 n (n = integer) Distance from the nuclei l= 0 s-orbital l= 1 p -orbital Angular Momentum Quantum Number (l) 0, 1, 2, 3 (n-1) 3D -shape of an orbital l= 2 d-orbital l= 3 f-orbital Magnetic Quantum Number (m l ) 0,1,2 l Orientation of the orbital s= 1 orbital p= 3 orbitals d= 5 orbitals f= 7 orbitals Electron Spin Quantum Number (m s ) M s = Orbitals can hold 2 electrons s = 2 electrons p = 6 electrons d= 10 electrons f= 14 electrons
4 Atomic Radius Ionic Radius Ionization Energy Energy required to remove the outermost electron from an atom. M + IE M + + e - Opposite trends as atomic radius Noble Gases are very stable (octets) Extra large amount of energy to remove an e - from a noble gas Columns: Each step down is a new orbital (bigger n) Rows: =.#. across a row.#. ~ same across a row and atom shrinks Cations are smaller: p/e ratio radius Anions are bigger: p/e raio radius From Schrodinger Equations Valence Electrons Electrons in the outermost orbital (n)of an atom. sand p electrons with highest n Responsible for the formation of ions and molecules To Lewis Structures Ionic Compounds Complete octets by gaining or losing electrons
5 Molecular Compounds Complete octets by sharing electrons From Valence Electrons Electronegativity Attractive force that an atom has for shared electrons in a covalent bond. Most EN element: $ % Least EN element: $ & Lewis Dot Structures Represents bonding between ionic and molecular compounds in terms of valence electrons and the octet rule VSEPR Theory Valence Shell Electron Pair Repulsion Theory Shape of molecules is determined by the repulsive forces between electrons. Molecules minimize this by keeping the electrons as far apart as possible.
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