A quick and simlple study guide that contains all rudimenary concepts studied in introductory classes to Organic chemsitry. Includes 9 concepts, images and examples.
Organic Chemistry Fulls Study Guide
Eyenain Misgar
Table of contents
1.Introduction a.Carbon
b.Valence electrons
c.Octet rule
2.Drawings a.Bonds
b.Condensed formula
c.Conventional drawings
d.Line angle formula
3.Molecular Orbitals, Hybridization, Geometry a.Subshells
b.Atomic oribitals
c.Hybridization
d.Sigma and pi bonds
e.Geometry
f.Bond angles
4.Lewis Structures, Formal Charge, Resonance structure a.Lewis structure
b.Atoms formal charge
c.Resonance
d.Major resonance vs. Minor resonance
5.Basic Names (Alkanes) a.Nomenclature
b.Alkanes naming
6.Functional Groups a.Introduction to functional groups
b.Basics of each functional group
7.Acid Base Chemistry a.Arrhenius Acid and Base
b.Brownstead- Lowry Acid and Base
c.Lewis Acid and Base
d.pKa and pKb
e.Acid-Base Reactions f.Effects on acididtu
g.Effects on Bacisty
8.Isomers a.Constitutional Isomers
b.Congrontational Isomers
c.Diastereomers
d.Geometric Isomers
e.Contfrontational Isomers analysis
f.Newman Projections
g.Cychohexane Chair Conformation Organic Chemistry Fulls Study Guide
Eyenain Misgar
9.Chirality and Enantiomers a.Chiral vs. Achiral
b.R and S Nomenclature of Enetiomers
c.Properties of Enantiomers
d.Racemic Mixtures
e.Meso Compound
10.Organic Reactions a.Reaction Format b.Degree of Substitution in Alkanes
c.Degree of Substitutuion in Alkenes
d.Reaction of Intermediates: Radical, Carbocation, Carbanion
Introduction-
Organic Chemistry also known as “Orgo” is the study of the molecular structure and reactions relative to living matter, and is referred to the study of compounds containing carbon. Carbon is a particularly central element to life because all living creatures contain carbon. Understanding health, medicine, pharmachology and industry all come down to the study of carbon and its keyholder place in organic chemistry. -Carbon
Atomic Number: 6 Electron configuration: 1s²2s²2p²
-Valence electrons
Definition: The number of electrons found in the outermost shell in the atom.
●These atoms participate in bonding
●Lone pair electrons are a subset of valence electrons that do not participate in bonding
●1s²2s²2p²
○Electrons in the second shell (2s²2p²) Represent carbon's valence electrons
○(2+2=4) So, carbon has 4 valence electrons
-Octet rule
Definition: The sum of all bonded and non-bonded electrons ina given atom in the 2nd row of the periodic table, which is always less than or equal to 8. ●Exceptions to the Octet Rule:
○Hydrogen and Lithium = 1 Valence Electron
○Beryllium = 2 Valence Electrons
○Elements in period 3 can occupy more than 8 valence electrons (e.g. Phosphorus and Sulfur)
Ex:If carbon has four electrons it may accommodate four more electrons by gaining four more bonds. These bonds include single or more than one like double or triple, etc. Each bond takes 2 electrons.
Drawings-
e.Bonds
-Bonds are represented by lines. One line is a single bond, two is a double and three is a triple bond. Organic Chemistry Fulls Study Guide
Eyenain Misgar
-Bonds can be in different planes, and to denote this there are different shapes to show the direction. A straight line represents a bond within the same plane of the drawing. A triangle shows the bond coming out of the paper pointing to your direction. A triangle drawn in vertical lines in a barcode manner is a bond pointing away from you. f.Condensed formula
g.Conventional drawings
h.Line angle formula
General Rule #1:
-When a line is drawn, the atom at each end is a Carbon by default, unless specified as otherwise
-Even if there is no indication, the proper number of hydrogen atoms are attached to any compound
-Ex:
General Rule#2:
-At each bend within the line is a new carbon atom at the joint.
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