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by: Moses O'Conner


Moses O'Conner
GPA 3.87

Libby Puckett

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About this Document

Libby Puckett
Class Notes
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This 2 page Class Notes was uploaded by Moses O'Conner on Friday October 2, 2015. The Class Notes belongs to CHE 1101 at Appalachian State University taught by Libby Puckett in Fall. Since its upload, it has received 6 views. For similar materials see /class/217699/che-1101-appalachian-state-university in Chemistry at Appalachian State University.




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Date Created: 10/02/15
Test 2 Study Guide Chapter 6 Quantum mechanics 4 quantum numbers symbols names descriptions possible values n 1 m1 ms Orbital energy level comparisons H vs many electron systems Representation of orbitals shapes descriptions number of orbitals 7 s p d f Pauli Exclusion Principle amp its ramifications Electron spin electrons per orbital Electron con gurations s p d f 7 know how to write complete and condensed electron con gurations understand why exceptions happen How do the con gurations relate to the periodic table s amp p 7 main block elements d 7 transition metals f 7 rare earth lanthanides amp actinides Understand how certain energy levels ll rst amp why Hund s rule 7 maximize electrons with the same electron spin lowest energy Write orbital diagrams to determine pairedunpaired electrons Core electrons and valence electrons De nitions orbitals electron shell subshell nodes electron density probability density w I412 wave functions degenerate orbitals all things bold in your chapters Chapter 7 Development of the periodic table gt periodicity Effective nuclear charge Trend increases across a row due to increase in Z slightly increases down a group because Z increases but core electrons are less able to shield Zeff Z 7 S know what each variable means Shielding effect Explain why Zeff is estimated but not exactly correct Atomic radii bonding vs nonbonding radius Trend decreases across a row because Z63 increases increases going down a column due to increase in n Ionic radii Cations are smaller than their parent atom why Anions are larger than their parent atom why Trend decreases biphasically across a row or decreases across an isoelectronic series increases down a column due to increase in n Ionization energy 7 lose electrons energy amount The greater the IE the more dif cult it is to remove an electron IlltIzlt13 Trend Increase a row due to increasing Zeff39 decrease down a column because n increases As n increases distance from the nucleus increases Electron con gurations of ions 7 remove electrons from largest n rst for cations add electrons to lowest n rst for anions Electron Af nities 7 gain electrons energy amount The more negative the number the greater the electron affinity Introductory Chemistry I Test 1 Study Guide Chapter 1 Basic definitions 7 matter elements atoms 39 39 pure 39 mixtures Three states of matter and their characteristics solids liquids gases Law of Constant Composition Mixtures 7heterogeneous vs homogeneous solutions Physical properties vs chemical properties Intensive vs extensive properties Physical changes vs chemical changes Separation of mixtures 7filtering distillation physical separation The Scienti c Method Units of measurement 7 metric system SI base units metric pre xes and conversions mass temperature 3 scales 7 K C F and conversions between each derived SI units volume density Uncertainty in measurement 7 precision and accuracy signi cant gures scienti c notation signi cant gures in calculations Dimensional analysis 7 conversion factors Know metric conversions and basic conversions Beware of cubic conversions 7 cube number and unit I will put uncommon conversion factors on the test Chapter 2 Dalton s postulates and corresponding laws Law of Constant Composition Law of Conservation of Mass Law of Multiple Proportions Cathode rays and cathode ray tubes 9 presence of subatomic particles Key players Thomson CRT 7 chargemass of an electron Millikan oil drop experiment 7mass and charge of an electron Radioactivity Becquerel Curies Rutherford 7 orparticles 2 Bparticles l39 and yrays Plum pudding model Thomson Rutherford experiment 9 discovery of a nucleus in the center of an atom Protons neutrons electrons electronic charge atomic mass unit angstroms isotopes nuclides atomic number mass number atomic weight average atomic masses know how to calculate Periodic table 7 periodic trends groups columns common group names periods rows metals metalloids nonmetals know location of each atomic number atomic symbol atomic weight protons neutrons and electrons in each element bases on atomic number and weight Molecules Molecular compounds 7 usually only nonmetals


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