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CSU - CHEM 111 - Class Notes - Chem 111 - Week 04 Notes

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CSU - CHEM 111 - Class Notes - Chem 111 - Week 04 Notes

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background image Chem 111 ­ CSU Week 04 Notes StudySoup ­ Avery  Chapter 3: Atomic Structure (cont.)  Highlight ​: Topics talked about extensively in lecture  ​Highlight​: Helpful examples    3.4: The Hydrogen Spectrum and the Bohr Model (cont.)  ● Energy Level Diagram:  ​shows the transition of electrons between energy levels  ● Atomic Emission (on an energy level diagram):  ​arrows point down when an  electron emits energy; higher to lower energy level  ○ Represented by a negative change in energy  ○ When an electron emits energy, visible light energy is also released  ■ Color is based on wavelength and frequency of the electron  emissions  ● Atomic Absorption (on an energy level diagram):  ​arrows point up when an  electron absorbs energy from a photon; lower to higher energy level  ○ Represented by a positive change in energy  ● ΔE = n f ­n i  / n ○ E = energy  ○ n = final state of the electron  ○ n i  = initial state of the electron  ● Bohr Model:  ​a model of an atom that depicts electrons traveling in circular orbits  around the nucleus  ○ Strengths:  ■ Accurate prediction of energy needed to ionize an atom  ● Ionization:  ​to remove an electron from an atom  ■ Allowed scientists to begin using quantum theory to explain matter  at an atomic level  ○ Limitations:   ■ Movement of electrons is not as defined as the Bohr Model depicts  ■ Does not account for electron spectra of multielectron atoms 
background image Chem 111 ­ CSU Week 04 Notes StudySoup ­ Avery  ● Electrons move more like waves rather than like a ball (as depicted in many  diagrams)  ○   3.8: The Periodic Table and Filling Orbitals  ● Aufbau Principle:  ​building electron configurations of atoms by adding one  electron at a time as atomic number increases across rows of the periodic table  ● Effective Nuclear Charge (Z eff ):  ​the attraction toward the nucleus experienced  by an electron in an atom   ● Electron Configuration:  ​the distribution of electrons of an atom among the  orbitals of an atom or ion  ○ Ex: Li = 1s 2 2s ● Orbital Diagrams:  ​depiction of arrangement of electrons in an atom or ion using  boxes to represent orbitals  ○ Up/down arrows to indicate e ­  with positive or negative spin  ○ See Carbon example below  ● Hund’s Rule:  every orbital in a subshell is singly occupied with one electron  before any one orbital is doubly occupied  Ex: Carbon    ● Condensed Electron Configuration:  ​matches the electron configuration of a  noble gas plus extra electrons   ○ Ex: Carbon = [He]2s 2 2p ● Orbital Energies in Multielectron Atoms: 

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School: Colorado State University
Department: Chemistry
Course: General Chemistry I
Professor: Ruth Tucker
Term: Summer 2016
Tags: Chem, Chemistry, general, Colorado, state, and University
Name: Chem 111 - Week 04 Notes
Description: These notes go over what was covered in week 04 of Chem 111: the Bohr Model, electron configurations, and atomic/molecular orbitals. They are a combination of book notes and lecture notes, with important information highlighted in yellow and helpful examples highlighted in green.
Uploaded: 09/21/2016
3 Pages 11 Views 8 Unlocks
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