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This 2 page Class Notes was uploaded by Kara Nichols on Tuesday May 31, 2016. The Class Notes belongs to CHM 111 at Calhoun Community College taught by Mona Chaudhary in Spring 2016. Since its upload, it has received 27 views.
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Date Created: 05/31/16
College Chemistry 1 – Mona Chaudhary 5/25/2016 Important Words or Important People Important Concepts Definitions Lesson 4 Electron Configuration Types o Bohr – electrons are fixed in concentric, circular orbits at a specified distance from the nucleus o Quantum Mechanical – electrons are defined to regions with in energy levels outside the nucleus Electron Configuration o Describes the arrangement of electrons o Methods: Shorthand Notation Orbital Energy Diagram They both give the same information o Components: Principal energy level (1-7) S = electron Orbital holding e (s,p,f,d) Subscript on orbital letter = #e - P present o Orbital Notes S can have 1-2 electrons D P can have 1-6 D can have 1-10 F F can have 1-14 Shorthand Notation o Level, orbital, e- o The periodic table gives all 3 components Level = period 1-7 Orbital = Groups I & II = S III – VIII = P Transition Metals = D # e = number of electrons in outer shell (+/- for ions) o EXAMPLE H = 1s 1 He = 1s 2 Orbital Energy Diagrams o Graphic representation of shorthand notation Written from bottom to top Orbitals are represented by dashed line(s) s orbital = 1 dash p orbital = 3 dashes d orbital = 5 dashes f orbital = 7 dashes (we do not show) Aufbau Principle – fill the lowest energy level first Hund’s Rule – Fill in orbitals unpaired first Give each orbital an electron first, then go back and double up Draw arrows in the opposite direction because electrons are magnetic and opposite ends attract Octet configurations are extremely stable because the valence (outermost) orbital is filled with electrons. o Duet configurations are also extremely stable Examples: 1 1H= 1s 1s 32Ge = 1s , 2s , 2p , 3s , 3p , 4s , 3d , 4p 2 4p 3d 4s 3p 3s 2p 2s 1s
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