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CSU - CHEM 111 - chem 2 test study guide - Study Guide

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CSU - CHEM 111 - chem 2 test study guide - Study Guide

School: Colorado State University
Department: Chemistry
Course: General Chemistry I
Professor: Ruth Tucker
Term: Summer 2016
Tags: Chemistry
Name: chem 2 test study guide
Description: this study guide cover all the listed "things to know" for exam 2
Uploaded: 02/25/2018
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background image Test 2 study guide   1 .Relate the photons absorbed and emitted by atoms to positive and negative energy 
transitions 
● Energy is negative when light is being emitted because the change in energy from  a higher energy level to a lower level decreases.   ● Energy is positive when it is being absorbed because energy increases as the  electron’s energy increases as it transition from a lower level to a higher level.  2. Explain the location and movement of electrons in an atom  ● Electrons travel in orbitals around the nucleus. Electrons are attracted to protons  and repelled by other electrons. In metals the outermost electrons ​ (valence  electrons) ​ are basically free and can easily move from atom to atom.   3.Give examples that demonstrate that the absorption and emission of light is quantized  ● The bohr model increasing or decreasing by whole number  
● Quantized=whole numbers 
● wavelengths = exact numbers 
4. Relate the energies and wavelengths of photons absorbed and emitted by atoms to 
electron transitions between atomic energy levels 
● The energies and wavelengths of photons absorbed and emitted the atom increase  energy levels when light is absorbed and atoms decrease energy levels when it is 
emitted.  
5.Relate atomic emission spectra to transitions in energy level diagrams using the Bohr 
model 
● When light is emitted energy levels decrease because energy is being released.   6.Calculate the energy, wavelength and frequency of a specific Electronic transition in a 
hydrogen atom 
●   7.Relate transitions in energy level diagrams to regions of the electromagnetic spectrum 
background image ● Energy levels on the electromagnetic spectrum( frequency) are related because the  higher the frequency the smaller the wavelength or in other words the higher the 
energy level the smaller your wavelength will be.  
8.Predict a qualitative line spectrum given a simple energy level diagram  ●   9.Use the Bohr equation to explain the quantitative nature of energy level diagrams, 
including that the energy levels are negative 
●   10. Identify s, p, and d orbitals from 2-D images  ●   11. Compare the relative sizes and energies of orbitals in different subshells within an 
atom 
● As the subshells increase in energy level the size directly increases as well   12. Use the Aufbau principle to write electron configurations of atoms and monatomic 
ions Of Elements that are not exceptions to the rule 
● The orbitals will fill from the lowest energy level before it fills the higher energy  levels. For example 1s fills before 2s.   13. Use the Aufbau principle and Hund’s rule to draw orbital diagrams of atoms and 
monatomic ions of elements 
● Hunds rule- all subshells fill with one electron before a second will join  14.Differentiate between core and valence electrons  ● Core electrons fill the innermost and lowest energy shells while the valence  electrons fill the outermost and highest energy level. The placement and position 
differentiate core and valence electrons. 
     

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School: Colorado State University
Department: Chemistry
Course: General Chemistry I
Professor: Ruth Tucker
Term: Summer 2016
Tags: Chemistry
Name: chem 2 test study guide
Description: this study guide cover all the listed "things to know" for exam 2
Uploaded: 02/25/2018
6 Pages 33 Views 26 Unlocks
  • Better Grades Guarantee
  • 24/7 Homework help
  • Notes, Study Guides, Flashcards + More!
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