Honors Chemistry
Note Packet
Organic Chemistry Unit
I. Terms and Definitions
Organic chemistry = branch of chemistry studying the compounds made primarily of carbon
 Inorganic compounds are those containing at least one metal ion;
 also known as “Salts” because they create electrolytes in solution
Biochemistry = a study of the compounds and reactions occurring in living organisms
General properties of Organic compounds versus Inorganic compounds
Organic Compounds
Covalent bonds
Based on Carbon
Weak IMF’s
Low boiling and melting points
High vapor pressures
Nonpolar or weakly polar molecules
Slow to react
Nonelectrolytes
Inorganic Compounds
Ionic bonds
Involve metals or ions
Strong IMF’s in solutions
Very high boiling and melting points
Ionic molecules
Low vapor pressures
Electrolytes
Fast reaction rates
II. Hydrocarbons…
Hydrocarbons = compounds composed of only hydrogen and carbon
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Derived from fossil fuels or life-based compounds
Different homologous series are referred to as the parrifins, olefins, aromatics, to name a few.
Also See Reference Table Q
II. B. Representations of Hydrocarbons
1) Molecular formulas
Tells the types of atoms present and their ratios; remember: not usually the lowest ratio!
Ex. C2H6, C2H6O, C8H18
2) Structural formulas
Shows how the atoms are bonded together
C2 H6
C2 H 6 O
C8H18
3) Condensed structural formulas
Show how the atoms are bonded together without showing all the bonds
CH3CH3
CH3CH2OH
H3CCH2CH2CH2CH2CH2CH2CH3 or it can be condensed further: H3C-(CH2)6—CH3
4) Lewis structures
These are the structural formulas. Lewis structures can also be drawn to represent the various
bond angles that actually exist within the 3D structure.
CH3CH2OH
CH3CH3
C8H18
C. Bond Types
How many valence electrons does carbon have? How many bonds can it form?____________
Carbon can form its 4 bonds in several ways.
-Forming single bonds with 4 separate elements, sharing _________ electrons with each atom
-Forming a double bond with another carbon to share __________ electrons with that atom
-Forming a triple bond with another carbon to share _______ electrons between carbon atoms
Single bond is formed when 2 atoms share 2 electrons to form a bond.
Longest bond
Weakest bond
Most flexible bond
Double bonds occur when 2 atoms 4 electrons to form a bond.
Shorter bond than single
Not very flexible
More unstable than a single bond
Triple bonds occur when atoms share 6 electrons between atoms.
Very short bond length
Very rigid, no flexibility
Most susceptible to attack!
D. Homologous Series = group of related compounds where members differ via a pattern
TABLE Q!
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General formula is used to calculate the ratios of Carbons and Hydrogens given one the
values.
The alkenes and alkynes all contain only one multiple bond!
Saturated = all single bonds
Unsaturated = one [or more] double/triple bond
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All these only contain Hydrogen and Carbon, and make Hydrocarbons!
II. Naming
Structure of the Names
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Hydrocarbons are names using a prefix and suffix system.
Prefix = Number of carbons
Suffix = Bond type present
Rules for Naming Hydrocarbons
1. Determine the longest continuous carbon chain. This is the prefix of the main
name.
2. Identify the bond types as all single, or as having a double/triple bond present.
3. Identify any groups or smaller carbon chains branching off the longest chain.
4. Number the carbons in the longest chain to provide the smallest numbers
possible for the groups. [go left to right or right to left only!]
5. Name all groups, if attached. Group names use the number of carbons as a
prefix, with a “-yl” suffix.
6. List the number of the carbon in the longest chain that has each group attached.
7. Write the number and the group names first. Alphabetize if necessary!
8. Write the prefix of the longest carbon chain.
9. Write the suffix of the bond type found in the longest chain.
Ex.
Isomers
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Isomers = a group of compounds having the same molecular formula, but different
structural formulas, AND different names and properties
Can only occur with carbon chains having 4 or more carbons!
Number of isomers increase with the number of carbons within the chain.
Ex. Find 4 different structural formulas and different names for the isomers of C6H14.
B. Cyclic Compounds
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Hydrocarbons that form a ring structure are called “Cyclic” compounds
They have the same general formula as the alkenes.
If all single bonded, then the prefix “cyclo-“ is used before the hydrocarbon name.
Aromatics = compounds containing the benzene ring
Benzene = cyclic six carbon compound with alternating double bonds. Instead of drawing
as resonance structures, benzene takes on its own structure
IV. Functional Groups
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Hydrocarbons may bond with other elements to form new organic compounds
These new compounds have unique characteristics and properties, often very different from the
original hydrocarbon in the main chain.
The particular arrangement of the atoms, as well as the atoms themselves, determine the functional
group.
For a complete list of the groups studied in this course, see TABLE R of your Reference Tables.
Follow the format below to record basic information and examples of each group. Extra examples
for structure and naming are listed on the reference tables also.
Group Name=_______________________ Contains (atoms and configurations):
Name changes:______________________________________________________
Examples:
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Repeat this pattern for all 10 functional groups discussed in class.
Most of these functional groups are found on Table R of your reference tables.
Use these examples and the examples in your reference tables to name and write structural
formulas on the given worksheets.
All naming methods used in this course are based on the naming system
formulated by International Union of Pure and Applied Chemists, or
“IUPAC”.
Other naming systems exist and may be explored further using online
resources.
V. Organic Reactions
The following list of organic reactions are a basic introduction of how certain organic compounds react.
Remember that these are much slower than reactions involving inorganic compounds.
A. Addition
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Adding two atoms to an unsaturated compound.
When adding only hydrogen atoms, the process is called “Hydrogenation”!
Example:
B. Substitution
 This reaction replaces a hydrogen already present in a saturated compound with
another atom.
 Usually involves a halogen element and produces an acid!
Example:
C.
Combustion
Burning hydrocarbons in oxygen
Two types:
1. Complete Combustion = Produces ONLY CO2 and H2O!!
Example:
2. Incomplete Combustion = May produce carbon, CO, and other products as
well as CO2 and H2O
Example:
D. Fermentation
Process of breaking down sugars to form an alcohol and carbon dioxide
Uses enzymes as a catalyst!
Example:
E. Saponification
Process of creating a soap and glycerol using a fatty acid and a base
Example:
F. Esterification
Forming an ester from an organic acid plus an alcohol
Hint: The alcohol becomes the “group” and the acid becomes the “-oate” or
the ‘ester’ portion of the name
Example:
G. Polymerization
Formation of a “poly-“mer using “mono-“mers! Creates a compound by joining single units
into a substance with many repeating units.
Two types:
1] Addition polymerization = simply adds all monomers into a single compound!
Only one product created!
Example:
2] Condensation polymerization = adds monomers by removing an OH- from one
side and an H- from the other side of a monomer to create water and the polymer as
products.
Example: