- 2 types of bonding: Sigma(o-) and Pi(~)(I know these aren't the actual signs but i do not know how to make them on a computer so I will just use these)
- Sigma is ALWAYS the first bond
- Pi will be the second bond or any after that
- Single bond: 1 o-
- Double bond: 1 o-, 1 ~
- Triple bond: 1 o-, 2~
IN HYBRIDIZATION YOU ONLY PAY ATTENTION TO THE SIGMA BONDS AND LONE PAIRS(LP)!!!!!!!!!!
- Example: Methane, CH4
(Hydrogen does not form hybrids)
Because HB is o- bonds plus LPs, to hybrid Carbon, first find out the number of o- bonds, ~ bonds and LPs. (You may have to draw the Lewis structure for this). In C there are 4 o- bonds and no LPs. Therefore the HB=4=sp^3.
- If HB results in an sp orbital, then the molecular geometry is 180 degrees(linear)
- If HB results in an sp^2 orbital, then the molecular geometry is 120 degrees(trigonal-planar)
- If HB results in an sp^3 orbital, then the molecular geometry is 109.5 degrees(tetrahedral)
Intermolecular Forces (IMF)
- The forces of attraction between molecules are known as intermolecular forces
- The boiling point of a liquid is a good measure of the IMF but its molecules: the higher the boiling point, the stronger the forces between the molecules
- IMF varies in strength but are generally weaker between atoms within molecules, ions in ionic compounds, or metal atoms in solid metals
- Boiling points for ionic compoundsand metals to be much higher than those for molecular substances: forces between molecules are weaker than those between metal atoms or ions
- The strongest IMF is between polar molecules
- Because of their uneven charge distribution, polar molecules have dipoles. A dipole is created by equal but opposite charges that are separated by a short distance
- The direction of a dipole is from the dipole's positive pole to it's negative pole
TEST IS THURSDAY! MAKE SURE YOU STUDY! READ THE CHAPTER
HOMEWORK: PAGE 211-212, #'s 50-60. IT IS HOMEWORK 6
(If you couldn't tell, I decided to go Memphis colors for the game tonight because Memphis is the best team in the nation. Hope you can read the gray good enough. I don't think it should be a problem. GO TIGERS!!!!)
PS Ben Smith
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i got it donnie and im lovin the colors. GO TIGERSSSSSSSSSSS!!!!!!!!!!!!!!!!!!!!!!! but anywho, here is a website on dipoles:
ReplyDeletehttp://dwb4.unl.edu/Chem/CHEM869E/CHEM869ELinks/www.uis.edu/7Etrammell/organic/introduction/polarity.htm
This site shows a few descriptions on hybridization and bonding.
ReplyDeletehttp://chemistry.boisestate.edu/people/richardbanks/inorganic/bonding%20and%20hybridization/bonding_hybridization.htm
Ben's PS is for what..?
ReplyDeleteAnd, yes GOOOOO TIGERS!
but, here's a site on intermolecular molecules.
http://www.mindbites.com/lesson/4971-chemistry-intermolecular-forces
site talks about dipoles
ReplyDeletehttp://www.chemistrydaily.com/chemistry/Dipole
Here is site about intermolecular forces:
ReplyDeletehttp://chemed.chem.purdue.edu/genchem/topicreview/bp/intermol/intermol.html
GO ILLINOIS!!!
ReplyDeleteThis site talks about intermolecular forces
http://www.chem.ufl.edu/~itl/2045/lectures/lec_g.html
I SEE THE BUNNY!! GO TIGERS
ReplyDeletehttp://chemed.chem.purdue.edu/genchem/topicreview/bp/intermol/intermol.html
Good site on intermolecular forces
http://www.mikeblaber.org/oldwine/chm1045/notes/Geometry/Hybrid/Geom05.htm
ReplyDeleteTalks about The Hybridization of orbitals
site about interactions between dipoles
ReplyDeletehttp://www.newton.dep.anl.gov/askasci/gen01/gen01606.htm
This website explains intermolecular forces.
ReplyDeletehttp://www.ausetute.com.au/intermof.html
Dipoles: http://world.std.com/~mmcirvin/bluesky/molecule.html
ReplyDeletehttp://www.chem.purdue.edu/gchelp/liquids/dipdip.html
ReplyDeleteDipole forces
this is a great presentation about intermolecular forces such as dipole forces, also including london forces which we will learn about tomorrow:
ReplyDeletehttp://www.wisc-online.com/objects/index_tj.asp?objID=GCH6804
Go Bucks! who happen to be ranked ahead memphis in both basketball and football. Here is a website about the majority of Chapter Six from non other than tOSU. you have to scroll down a tad to get to the Chemical Bonding part
ReplyDeletehttp://mansfield.osu.edu/~sabedon/campbl02.htm
everyone beats memphis in football but i predict c-usa champs again this year. here is a website on dipoles
ReplyDeletewww.orbitfr.com/Products/Components/
Scheuner no one care cares about ohio state
ReplyDeleteGood website on intermolecualr forces
http://library.thinkquest.org/C006669/data/Chem/bonding/inter.html
GO TIGERS
Wow donnie that is an awesome bunny. i didnt even know it was one until ben said it was, any way this site talks about Hybridization of atomic orbitals and VSPER theory http://www.science.uwaterloo.ca/~cchieh/cact/c120/hybrid.html
ReplyDeleteThis comment has been removed by the author.
ReplyDeletehttp://answers.yahoo.com/question/index?qid=20080401224300AAAkwRW
ReplyDeletetalks about identifying dipoles mucho helpful
dont worry Donnie i knew it was a bunny
this site talks about hybridization http://pages.towson.edu/ladon/carbon.html
ReplyDeletek
ReplyDelete