Organics Lectures

Organics Lectures - Organic ChemistryAn Introduction I am...

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Organic Chemistry—An Introduction I am not the best person to be giving a lecture on organic chemistry—the world is filled with two kinds of people, the ones who despise organic, and the ones who love it. During the year I took organic in college, I was also plastering the words from sad songs all over my dorm room walls—looking back I realize there was a cause and effect relationship between organic and typing up those songs. Honestly, I always thought the lunch each Tuesday afternoon before my organic lab felt pretty much like a person going before a firing squad, only it happened over and over and over for an entire year. With that off my chest, here is a nice lecture that surveys the important foundational concepts for the vocabulary that describes organic chemistry. Mostly you will get a feel for the fact that organic is a lot of nomenclature and a lot of systematic rules. For those who likes languages and lists, and for those who can close their eyes and imagine a three-dimensional world of molecular structures, organic is quite easy. For those, like me, who would rather reduce the subject to a couple of simple mathematical formulas, it is quite difficult. I mean, what kind of science course doesn’t need a calculator. But enough rant. Things you already know about organic just because you took my course. As much as I don’t like organic, the physical basis for pretty much everything you would learn in organic is developed in freshman chemistry—some things you need to remember throughout your organic course are: Bonding theory like VSEPR, VB and MO that allow you to draw the structures, even in three dimensions. Your friend, Δ EN, which allows you to assign local and molecular polarities of the electron clouds and armed with where δ + and δ - assignments across an organic compound, let you intelligently discuss physical properties and chemical reactivities with the best of them. After all, you have worked a huge number of organic chemistry problems throughout the year. For example: Tell me everything you know about the compound CH 3 CH 2 OH (ethanol): To start, you are actually capable of drawing this 3-dimensional image of ethanol yourself using simple bonding ideas. The large grey balls are the carbon, the small grey balls are the hydrogen and the red ball is oxygen.
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So what can you already say about this molecule from being a student in general chemistry? Plenty. All the atoms achieve a Nobel gas structure, either 1s 2 for H or 2s 2 2p 6 for the C and O. The C and O have four electron rich regions which means they have tetrahedral electronic geometry, are approximately 109.5 o bond angles, and have sp 3 hydridization. The carbons have four bonding regions and are either tetrahedral or distorted tetrahedral
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Organics Lectures - Organic ChemistryAn Introduction I am...

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