Notes for 10/26 and 10/28
Notes for 10/26 and 10/28 CH 101
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This 6 page Class Notes was uploaded by Rani Vance on Friday October 30, 2015. The Class Notes belongs to CH 101 at University of Alabama - Tuscaloosa taught by a professor in Fall 2015. Since its upload, it has received 18 views. For similar materials see General Chemistry in Chemistry at University of Alabama - Tuscaloosa.
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Date Created: 10/30/15
Chem 101 Notes for 1026 and 1028 sz hypridization atom With 3 electron groups around it trigonal planar system 120 degree bond angles at ie BH3 Types of bonds sigma bond result When the interacting atomic orbitals point along the axis connecting the two bonding nuclei ss and pp hybrid to hybrid pi bond results when the bonding atomic orbitals are parallel to each other and perpendicular to the axis connecting the two bonding nuclei pp When p orbitals are perpendicular to bond axis sigma is stronger than pi Types of bonds hybrid orbitals overlap to form a sigma bond unhybridized p orbitals overlap to form a pi bond overlap between 1028 Chapter 7 Molecular Orbital Theory Draw lewis structure 02 9 is it diamagnetic or paramagnetic diamagnetic has no unpaired electrons para sticks to magnet How does Molecular Orbital Theory work in MO theory linear combinations of atomic orbitals are used to construct molecular orbitals basically we add and subtract orbitals from each other Bonding vs Antibonding Molecular Orbitals when wave functions combine constructively the resulting orbital is lower in energy bonding orbitals sigma and pi electrons in bonding orbitals are primarily between the nuclei when added together the energy drops when wave functions combine destructively energy goes up antibonding orbitals sigma or pi nodes between nucleus Bond order bond order 12 bonding electrons antibonding electrons bond order considers valence electrons higher bond order stronger shorter bonds if bond order less than or equal to 0 molecule is unstable substance will be paramagnetic Rules for M0 diagrams molecular orbitals are a linear combination of atomic orbitals AO s total MO s of AO s when two AO s combine to form 2 MO s 1 MO is lower in energy the bonding MO and the other is higher in energy antibonding MO When assigning the electrons of a molecule to MO s we fill the lowest MO s first with a max of 2 spinpaired electrons per orbital
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