CrackOChem_OChem Basics II - pt 2

This video picks up right where the Organic Chemistry Basics Part I video leaves off. We will finish learning the fundamentals of organic chemistry to give you a solid foundation for the rest of the course. Here we talk about VSEPR Theory and the 2 Main Bonding Theories (molecular orbital theory and orbital hybridization theory). Enjoy!

Watch the entire video for free at...

www.crackochem.com---
Let CrackOChem be your personal Organic Chemistry video tutor.
Each video lesson provides an easy, yet comprehensive approach made from the student perspective. We assume you have no prior knowledge in the field, and will guide you every step of the way.

-------------------------------------------------------------------------------
About The Tutor

Garrett is a Harvard graduate. While earning his doctorate from the Harvard School Of Dental Medicine, he was hired by the university to propose and develop educational videos to complement the curriculum. During this time he worked with instructors at the medical and dental school to produce video tutorials in the areas of neurobiology, cardiology, pharmacology, radiology and pre-clinical dental laboratory.

However, Garrett's love for tutoring and helping students be able to understand complex subjects in a simple manner began with organic chemistry. He was initially told by his family, friends and instructors that organic chemistry would be the worst class he would ever take in college. Fortunately, with a lot of sweat, a few tears, and plenty of dry erase markers, Garrett was able to "crack the code" behind organic chemistry. In the process, he discovered a technique to teach ochem in a logical, straight forward manner, and the "CrackOChem" project was born. He spent the next several years developing this technique and passing it on to others through university organic chemistry tutorials, a study club, and organic polymer research. He was later hired by the University of California, Irvine for a full time position teaching advanced tutorials in chemistry and biology, and was also responsible for the hiring, training, and managing of university tutors.

Garrett is currently in orthodontic residency, but continues to actively help students through tutoring and future editions of organic chemistry video tutorials.

Category:

Education

Tags:

• organic
• chemistry
• basics
• covalent
• bonding
• vsepr
• theory
• valence
• shell
• electron
• pair
• repulsion
• basic
• shapes
• bond
• angles
• tetrahedral
• sigma
• bonds
• lone
• pairs
• trigonal
• planar
• linear
• molecular
• orbital
• atomic
• lewis
• diagram
• hybridization
• hybridized
• orbitals
• sp
• sp2
• sp3

[CrackOChem]

To everyone: as a general note, always pay attention to what types of things your profs want you to know. If they want you to know details about things like exact bond angles (ex. 107 vs. 109.5 degrees), then definitely know those for the test. I'm not at all saying that those things aren't important. They are. A lot of times though, we just have to pick and choose where to spend our time studying. It's great to memorize everything if you can, but prioritize if necessary as well. =)

[Assassin1801]

NH3 is a trigonal pyramid not bipyramidal. Bipyramidal is formed when you have two lone pairs of electrons. Also, the bond angle for octahedrals such as CH4 is 109.5 degrees not 109 degrees. I like your teaching style though.

[CrackOChem]

@Assassin1801 (1)

Hi Assassin, thanks for the comments.

Yes you're indeed correct, the bond angles for CH4 are technically 109.5 degrees. 109 was written here because it's easier to see/remember, & unless your professor is super ticky tack, 109 is usually close enough. It's more about the general idea that bonds/electrons want to be as far apart from each other as possible.

[CrackOChem]

@Assassin1801 (2)

When you have 4 single bonds/lone pairs, the bond angles will be ~109. When you have 3 single bonds/lone pairs, the bond angles will be ~120. When you have 2 single bonds/lone pairs, the bond angles will be ~180. Whether it is slightly more or slightly less by a few degrees does not usually play a huge role in how these compounds react.

[CrackOChem]

@Assassin1801 (3)

As you mentioned, lone pair & bond repulsion are not exactly equal, but they behave similarly when looking at bond angles. Lone pairs do have a slightly greater repulsion effect which is why you see a compound like NH3 (which has 3 bonds + 1 lone pair) having bond angles slightly less than 109 degrees (approx 107 degrees instead). But the big picture is that it is a compound with a combination of 4 single bonds/lone pairs, so it has bond angles of ~109.

Happy studying!

[Assassin1801]

Sorry, trigonal bipyramidal is formed when you have 5 pairs of electrons.

[Assassin1801]

You dont treat lone pair repulsion as equal to bond pair repulsion. Lone pair pushes the bond further down.

[Almaasak]

i love u