SG for EXAM 2
SG for EXAM 2 CHM 11500 - 004
Popular in General Chemistry
Popular in Chemistry
This 4 page Study Guide was uploaded by Karmen Young on Friday October 16, 2015. The Study Guide belongs to CHM 11500 - 004 at Purdue University taught by Scott Alexander McLuckey in Fall 2015. Since its upload, it has received 72 views. For similar materials see General Chemistry in Chemistry at Purdue University.
Reviews for SG for EXAM 2
Report this Material
What is Karma?
Karma is the currency of StudySoup.
You can buy or earn more Karma at anytime and redeem it for class notes, study guides, flashcards, and more!
Date Created: 10/16/15
CHM 115 Study Guide for EXAM 2 October 19th 2015 Lecture 8 The Atom and Spectroscopy Atom Force Microscopy atoms can be picked up and relocated Atom a dense nucleus containing p n with e surrounding in an electron cloud Thomason plum pudding model Rutherford s Exp Alpha particles shot at gold foil de ected by nucleus Disproved A Electrons behave as particles and waves Atoms don t collapse due to energy E KE PE Travels in waves with a wavelength lambda and frequency Travel in a vacuum at the speed of light c 30010quot8 ms c frequency wavelength inversely proportional The intensitybrightness is related to its amplitude Electromagnetic Spectrum Gamma ray Xray Ultraviolet VisibleVIB GYOR Infrared Microwave Radio waves IN ORDER OF INCREASING WAVELENGTH AND DECREASING FREQUENCY Refraction is the change in a wave s speed when entering a different medium Diffraction is the bend of a wave around an edge of an object amp A wavelike Blackbody Radiation and the photoelectric effect show the energy properties Light exists as photons whose energy is directly proportional to frequency Quantam Theory an atom has only certain energy quantites and can change its energy only by absorbing or emitting a photon whose energy equals the change in atom s energy Ephoton hv hcwavelength change in Eatom Bohr s Model had many deficiencies orbiting electrons would lose energy and spiral into the nucleus allocation of values of n were used arbitrarily and it would work with only Hydrogen Lambda hmv Schrodinger s Wave Mechanical Model of the H atom electrons are treated as a matter wave and is described mathematically by a wave equation Lecture 9 The Atom and Spectroscopy Each allowed electron energy is described by a wave function with values of particular quantam numbers 6 7p The wave function has a radial and an angular component The greater the electron energy the further out the electron tends to be SEE SLIDES WITH THE ORBITAL SHAPES Order 182 2s2 2p6 3s2 3p6 4s2 3d 4p6 5s2 4d 5p6 6s2 4f 5d 6p6 7s2 5f 6d Orbitals overlap to form bonds which determines the shape of the final product molecule Lecture 10 The Atom and Spectroscopy Spectroscopy white light shines through a prism and the colors in the spectrum separate no absorbance If the solution is insert color it means that the color went through and the others were absorbed Absorbance log IoI ebc where e is the molar absorptivity b is the width and c is the concentration Lecture 11 Trends in Chemical Reactivity Recap of Lecture 9 Know how to build an atom Ex 33 electrons using 1s2 2s2 2p6 3s2 3p6 4s2 3d 4p3 Paramagnetic unpaired electron Diamagnetic all electrons are paired so no magnetic field Electron Shielding core electrons shield valence electrons from nucleus Valence electrons feel effective nuclear charge ZEFF Z shielding The attraction for electrons is specified by the ZEFFradius Electrons drift toward atom with higher ZEFFradius Lecture 12 Trends in Chemical Reactivity Atoms interact with each other through their skins Ionic bonding Between nonmetal and metal ionic solid Covalent bonding Between 2 nonmetals separate molecules Metallic bonding Between metals electron pooling metal ion in electron sea Atomic radius increases as you move down the periodic table and decreases as you go across Electron affinity the loveattractiveness for electrons Lecture 13 Trends in Chemical Reactivity Metals weaker hold over valence electros form cations Nonmetals stronger hold over valence electrons form anions share electrons With metalloidsnonmetals The more valence electrons the stronger the bonding and the higher the melting point Oxide Behaviors Metal oxide amp water forms OH39 basic Nonmetal oxide and water for H30 acidic Some metals and metalloids form amphoteric oxides act as bases or acids in water Hess s LaW the enthalpy change of an overall process is equal to the sum of the enthalpy change of the individual steps Lecture 14 Trends in Chemical Reactivity Endothermic absorbs energy Exothermic releases energy Unit kJmol Electrostatic energy equation GIVEN Covalent bonding sharing of valence electrons both atoms are electron hungry Forming a bond releases energy and Breaking a bond requires energy To Study Lectures 814 Readings 71 72 74 82 131 134 135 83 84 27 28 91 92 93 96 65 62 64 94 Homework Assignments 814 Labs 2 and 3 Recitation Worksheets Learning Objectives Exam 2 Practice Problems Reminders You have a helpful information sheet given to you at the exam Look and see What material you do not need to remember because you are given it Arrive around 730 PM on Monday October 19 2015
Are you sure you want to buy this material for
You're already Subscribed!
Looks like you've already subscribed to StudySoup, you won't need to purchase another subscription to get this material. To access this material simply click 'View Full Document'