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CHM 115 Exam 2 study guide

by: Zack Bales

CHM 115 Exam 2 study guide CHM 11500 - 002

Marketplace > Purdue University > Chemistry > CHM 11500 - 002 > CHM 115 Exam 2 study guide
Zack Bales

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About this Document

Exam 2 study guide
General Chemistry
Chittaranjan Das,Suzanne C Doucette
Study Guide
Chemistry, 115, Purdue, Exam 2, Study Guide
50 ?




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This 2 page Study Guide was uploaded by Zack Bales on Thursday March 3, 2016. The Study Guide belongs to CHM 11500 - 002 at Purdue University taught by Chittaranjan Das,Suzanne C Doucette in Fall 2015. Since its upload, it has received 101 views. For similar materials see General Chemistry in Chemistry at Purdue University.


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Date Created: 03/03/16
CHM 115 Exam 2  Quantum Numbers o n – (1-7) o ℓ - (n-1) down to zero o m - (-ℓ to ℓ ) o m -s+1/2  NRG Orbitals o Filling orbitals  Add-electrons to lowest NRG first  2 e per orbital with opposite spins  Fill each with one e before filling with 2  Types of electrons o Outer – highest n o Valence – involved in bonds o Core – lower n levels  Composition of Solutions o Ions are stabilized by solution o Non electrolytes retain structure when dissolved o Gases become less soluable as temp increases o Solids become more soluble as temp increases o Solute + solvent  solution  Spectroscopy o Molecules absorb light at different energies o Absorbance = εℓc  Atomic Radii o Distance between atoms o Ionization Energy  Energy needed to remove electron o Electron Affinity  Change in energy accompanying additional electrons  Larger EA = more energy  Metallic o Main group – ionic oxides, basic o Main group nonmetals – covalent oxides, acidic o Amphoteric oxides – acid or base o Oxidation loses electron, reduction gain electrons  Bonds o Cations are smaller than parent atoms o Anions are larger than parent atoms o Magnetic Properties  Spinning electrons generate magnetic field  Paramagnetic: one or more d orbital with unpaired electron, weak  Diamagnetic: only one paired electron set not attracted by magnetic field o Chemical bond  Ionic – metal + nonmetal  Covalent – nonmetal + nonmetal  Metallic – metal + metal  Atoms are unpaired in ionic and metallic  Enthalpy of Rxn ΔH o ΔH = sum ofΔHf products – sum of ΔHf reactants o ΔHoverall = ΔH1 + ΔH2 + ΔH3 + … o Lattice Energy  -ΔHlat = - ΔH final - (ΔH1 + ΔH2 + …) o ΔHrxn = sum Bonds formed – sum bonds broken


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