Principles of Chemistry I
Principles of Chemistry I CHEM 1307
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This 4 page Class Notes was uploaded by Kara Dibbert on Thursday October 22, 2015. The Class Notes belongs to CHEM 1307 at Texas Tech University taught by Tamara Hanna in Fall. Since its upload, it has received 26 views. For similar materials see /class/226511/chem-1307-texas-tech-university in Chemistry at Texas Tech University.
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Date Created: 10/22/15
Chemistry 1307 Exam 3 Review Chapter 8 Covalent bond vs Ionic bond Valence vs Core electrons Lewis Dot Structures 0 octet bonding pair lone pair 0 count valence electrons determine central atom single bonds to each terminal atom octet around terminal atoms extra electrons go on central atom Octet Rule 0 exceptions expanded octet less than an octet Isoelectronic 0 definition Formal Charge 0 FC group number lone pair electrons 12 bonding electrons o be able to assign a formal charge to all atoms in a compound Resonance 0 definition 0 be able to draw or predict the number of resonance structures for a compound Coordinate Covalent Bond 0 definition Free Radical 0 definition VSEPR Theory shape 0 electron pair and molecular geometry for 2 3 4 5 and 6 terminal groups 0 electron pair geometry includes lone pairs 0 molecular geometry places lone pairs in the correct position but does not include them in the shape Bond Angles 0 know approximate values 0 what changes the value of a bond angle Bond Polarity o polar covalent bond polar bond Electronegativity 0 definition periodic trend 0 be able to predict the polarity of a bond Dipole Moment 0 be able to predict if a molecule is polar or nonpolar Bond Order 0 definition 0 BO umber of shared electron pairs number of Xy bonds Bond Length 0 definition periodic trend Bond Dissociation Enthalpy o BDE 2 AH broken 2 AH formed 0 be able to calculate provided values Be able to compare bond length and bond strength for a set of elements Chapter 9 Valence Bond Theory 0 why is this theory useful 0 rules Sigma bond 0 characteristics Hybridization 0 definition be able to assign to a central atom Multiple Bonds double and triple bonds 0 unhybridized p orbitals 0 characteristics of a pi bond Be able to describe the bonding in a molecule Molecular Orbital Theory 0 why is this theory useful 0 principles and how they apply BondingAntibonding 0 definition energy ordering Bond Order 0 B0 12 bonding electrons antibonding electrons 0 can be fractional MO Diagrams o be able to fill in the electrons in an M0 diagram o look if the question asks for valence electrons only or valence and core electrons o be able to predict magnetism Use MO diagrams to predict bond length and bond strength due to bond order Chapter 11 Pressure conversions Boyle s Law 39 P1V1 P2V2 Charles s Law h amp T1 T2 General Gas Law P1V1 P2V2 T1 T2 Avogadro s Hypothesis Ideal Gas Law o PV nRT o know definition of ST P Use Ideal Gas Law to solve for densitymolar mass E d gMMzP V RT Gas Laws and Stoichiometry Partial Pressure and Mole Fraction 39 PA XAPtotal 0 XA ra ntotal o know definitions o there are multiple ways to ask these questions so practice on OWL Kinetic Theory of Gases Root Mean Square Speed 0 remember to change molar mass to kgmol 0 use R 83145 Jmol K where 1J 1 kngsz 3RT x u2 MM Diffusion and Effusion o be able to calculate molar mass or rate of effusion rate of effusion of gas A MMB time of effusion of gas B rate of effusion of gas B MMA time of effusion of gas A Nonideal Gases o what does van der Waals equation do 0 how are real gases different from ideal gases
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