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CSU - CHEM 111 - Chem 111 Study Guide 1 - Study Guide

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CSU - CHEM 111 - Chem 111 Study Guide 1 - Study Guide

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background image 3.2­3.7
Electronic Structure and Periodic Properties of Elements
1. Relate the photons absorbed and emitted by atoms to positive and negative energy  transitions 2.Explain the location and movement of electrons in an atom 3.Give examples that demonstrate that the absorption and emission of light is quantized 4.Relate the energies and wavelengths of photons absorbed and emitted by atoms to electron 
transitions between atomic energy levels
Ground state to excited stage and back down 5.Relate atomic emission spectra to transitions in energy level diagrams using the Bohr model 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 Released energy corresponding to what wavelengths 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 2­D images 11.Compare the relative sizes and energies of orbitals in different subshells within an atom 12.Use the Aufbau principle to write electron configurations of atoms and monatomic ions of  elements that are not exceptions to the rule 13.Use the Aufbau principle and Hund’s rule to draw orbital diagrams of atoms and monatomic 
ions of elements
14.Differentiate between core and valence electrons 15.Identify periods, groups, rows, columns, and families in the periodic table 16.Identify alkali metals, alkaline earth metals, halogens and noble gases by name based on  location in periodic table 17.Use the general location of metals, nonmetals, and metalloids on the periodic table to predict
the general characteristics of atoms
background image 18.Use electron configurations to determine the number of valence electrons in neutral atoms of
the main group elements
19.Use the concept of effective nuclear charge to explain differences in the energies of the  same atomic orbital in different atoms 20.Relate the atomic radius of the elements to their positions in the periodic table 21.Rank the relative sizes of atoms and monatomic ions in an isoelectronic series 22.Explain the relative sizes of atoms and monatomic ions using the concept of effective nuclear
23.Relate the ionization energies of the elements to their positions in the periodic table 24.Relate subsequent ionization energy data (first, second, third...) of neutral atoms to their  position on the periodic table. 25.Relate the electron affinities of the elements to their positions in the periodic table 26.Explain exceptions to trends in ionization energies using the energies of empty, full and half­
filled subshells in electron configurations
27.Use electron configurations to predict the charge of monatomic ions of the main group  elements 28.Determine the formulas for ionic compounds 29.Know the trends in the periodic table 4.1­4.2
Chemical Bonding:  Ionic and Molecular Compounds 
29.Describe ways in which covalent and ionic bonds are alike and ways in which they are  different  30.Classify compounds as ionic or molecular 31.Recall the general periodic trend for electronegativity  32.Differentiate ionic, polar covalent and non­polar covalent bonds 33.Predict the relative polarity of covalent bonds based on trends in the electronegativities of the
bonded elements 
34.Distinguish electronegativity from electron affinity 

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School: Colorado State University
Department: Chemistry
Course: General Chemistry I
Professor: Ruth Tucker
Term: Summer 2016
Name: Chem 111 Study Guide 1
Description: - 3.2-3.7 and 4.1-4.2 - Bohr model - Spectrum - Ground state and energy levels - Energy of an electron - Energy of transitions - Quantum theory - Subshells - Orbitals - Aufbau principle - Electron conf
Uploaded: 02/26/2018
3 Pages 39 Views 31 Unlocks
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