Unit test!

Will update this with more information when I receive my score, but so far I thought it was fairly easy and hope that this trend will continue into further units.

Update: I did really well on this test! Probably my best test this year. Overall this unit wasn't too difficult and I hope to continue this trend in the future.

Chemical Bonding Unit Start!

This unit seems to be a continuation of the last unit. The good news is that last unit was relatively easy. I got a pretty good grade on the last unit too! So far, it seems to be easy, hopefully that will not change as we proceed into the future. We learned about finding valence and making Lewis dot diagrams. We also learned about how to measure bond length. This link will help with bond length: Bond length! 

Chemical Bonding: Molecular Shapes!

New pictures! This one is of my dog, Fisher.

Molecular shapes can be hard to comprehend, mainly because there are so many! However, of the 8+ shapes the molecules can come in, there are only 6 that you have to really remember.

1.) Tetrahedral

http://people.uwplatt.edu/~sundin/images/vspr4.gif

This molecule is non-polar with 4 bonds. It is 3D and has depth.

2.) Trigonal Pyramidal

https://upload.wikimedia.org/wikipedia/commons/e/e9/Pyramidal-3D-balls.png

 This molecule is polar and has 3 bonds with a lone pair on top.

3.) Trigonal Planar

http://users.stlcc.edu/gkrishnan/vspr3.gif

This molecule structure is like trigonal pyramidal, except that the lone pair on top is missing. This makes the molecule "2D". This molecule is non-polar.

4.) Linear

http://www.ochempal.org/wp-content/images/D/dipolemoment9.png

This molecule is also "2D" but it is locked in a straight line. This molecule is non-polar. Usually there will be on lone pairs on the central atom.

5.) Bent

http://i.stack.imgur.com/xC0NU.jpg

This molecule is polar, and usually has a pair of lone electrons on top of it. It has only two bonds.

6.) Octahedral

http://chemwiki.ucdavis.edu/@api/deki/files/860/=copper(II)_fluoride.jpg?revision=1

This molecule is non-polar and has 6 bonds. It is three dimensional, and has depth.

More help on this topic can be found here: http://intro.chem.okstate.edu/1314f00/lecture/chapter10/vsepr.html