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Study Guide for Exam 2

by: Alexa Johnson

Study Guide for Exam 2 CHEM 111

Marketplace > Colorado State University > CHEM 111 > Study Guide for Exam 2
Alexa Johnson
GPA 4.0
General Chemistry I (GT-SC2)
Claire M Filloux

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About this Document

This is a very easy to follow overview of the material that will be covered on Exam 2!
General Chemistry I (GT-SC2)
Claire M Filloux
Study Guide
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This 2 page Study Guide was uploaded by Alexa Johnson on Friday October 2, 2015. The Study Guide belongs to CHEM 111 at Colorado State University taught by Claire M Filloux in Fall 2015. Since its upload, it has received 49 views.

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Date Created: 10/02/15
CHEM 111 Study Guide for Exam 2 The exam is not cumulative Information taught at the beginning of the course prior to Exam 1 may be integrated into questions but the material covered will be from after the test For those of you with a textbook the material covered on Exam 2 will come from section 3742 Atomic orbitals an orbital is a region of space where an electron can be foundelectron density are 3D shapes representing the electron density and distribution within an atom s orbitaI electron density greatest at the nucleus holds 2 electrons p orbitaI direction xy and z in 3 different ways they can occupy space holds 6 electrons Contain node or area of orbital with no electron density perpendicular planes d orbitaI 5 orientations 4 that are similar and 1 donut shaped holds 10 electrons f orbitaI 7 orbital orientations holds 14 electrons Use the aufbau principle to place electrons in electron con guration distribution of electrons among the orbitals of an atom or ion diagram from lowest energy to the highest When drawing the diagram use Hund39s ruIe ll empty rooms before making them pair up You can write electron con gurations long or condensed if condensed use closest noble gas with lower atomic number in brackets then continue con guration Remember the number of electrons in each orbitalblock and how you read from left to right like a book Ix Bi itk lid lilmk 1 Blank If Hlmk Be sure you have correct number of electrons when writing con gurations just add them together Recall that ions will have one less for and one more for There are trends in the periodic table concerning atomic radii and ionization energy atomic radii decrease from bottom left Fr to top right He and ionization energy increases in same pattern lonization energy is the amount of energy needed to remove 1 mole of electrons from 1 mole of atoms or ions in gas phase The size of an anion will be much larger than the parent element while a cation will be much smaller Eectron af nity values show that the more negative the value the more energy is released when 1 mole of atoms combines with 1 mole of electrons to form 1 mole of anions with a 1 charge the greater the release of energy re ects more attraction between atoms and free electrons Three main types of bonds were discussed lonic metals and nonmentals transferred electrons Covalent nonmetals andor metalloids shared electrons Metallic metals pooled together electrons To name binary ionic compounds Keep rst name of cation and replace ending of second with ide To name oxoanions Names ending in ate or ite and may have a per or hydro pre x To name binary molecular compounds Keep the rst name and replace second word ending with ide Use pre xes based on how many of each atom there are Hill I39ll39l her Prefix l inonua 2 db 3 i 4 tuna S penta hcxna 7 hcpt E b 939 noun 1n dcca


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