Week Four Lecture Notes
Week Four Lecture Notes Chem 105
Popular in Fundamental Chemistry
Popular in Chemistry
This 3 page Class Notes was uploaded by Marisa Loken on Monday October 19, 2015. The Class Notes belongs to Chem 105 at University of Wisconsin - Stevens Point taught by Dr. Riha in Fall 2015. Since its upload, it has received 16 views. For similar materials see Fundamental Chemistry in Chemistry at University of Wisconsin - Stevens Point.
Reviews for Week Four Lecture Notes
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: 10/19/15
Week Four Notes September 21September 25 Radiant energy is quantinized l line spectra Rydberg Equation 1X RH 1nquot2 1nquot22 RH109677610quot7 Nenergy state of an orbit quantum number N1 lowest energy level ground state N is greater than or equal to 2 an electron in a high energy level excited state N 3 to N 7 absorbs energy absorbance39sabsorption N 7 to N 3 emits energy emission electron releases from Concepts of Bohr model that still apply E only exist in discrete energy levels 0 Described by quantum numbers Electron transitions involve absorptionemission of energy matteralso has waves Debrogne wavelength Wavelength hmv o Mmass kg 0 Vveocity Tried to pass xrays and electrons through aluminum foil Matter has wavelike particle like properties Hersenbergs uncertainty principle Wavelike function Orbitals have speci c energy and shapes which are described by quantum numbers Nprincipe quantum number 0 Energy of orbital valves of positive integers 1 2 3 0 Larger n higher energy farther from nucleus Languar momentum quantum number 0 Describes shape of the orbital values of 0n1 o Valuesofl0123 Mmagnetic quantum number 0 Describes orientation of orbital can have values 2L1 Electron shell All orbitals with the same n values SubsheH All orbitals with same n values Wednesday Quantum numbers Nenergy of orbital values 1 2 3 Lshape of orbital values 0n1 M values L to L including zero Pauli exclusion principle No two electrons in an atom can have the same set of quantum numbrs Ms magnetic spin quantum number 0 12 spin up 12 spin down S orbital o Spherical shape 0 Electron near center of atom as n increases the probability of nding an electron increases as you get further from the nucleus Apply to all orbitals P orbitals Have a dumbbell shape D orbitals cover leaf like shape F orbitals Complex in shape Seven orientations all orbitals with same value n have the same energy Electron repulsions Increase energy 0 More electrons put in an orbital higher the energy of that orbital o Orbital energy increases with increasing n and l in a many electron atom all orientations of an orbital subshell have the same energy Ddegenerate Electron lling and electron con guration Only put two electrons into one orbital o Aufbau principle 0 ll electrons from lowest energy occupy low energy orbitals rst 0 spread electrons over all orientations of degenerate orbitals F day Aufbau principle electrons must occupy the lowest energy orbital available Hund39s rule spread out the electrons in degenerate orbitals before adding 2 electrons to the same orbital Condensed electron con gurations and orbital diagrams use preceding noble gas determine how many electrons remain to be distributed electrons in element of interest distribute remaining electron starting with next shell that follows the noble gas 0 do not participate in reactions valence electrons louter most electrons that remain o participate in reaction
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'