Upload
carolina-grounds
View
224
Download
2
Embed Size (px)
Citation preview
Organic ChemistryOrganic Chemistry: - the chemistry of carbon
and carbon-based compounds- (C – C or C – H or C – R)- (can be a few to hundreds of carbons covalently
bonded to one another)
Characteristics of Organic Compounds: *Usually have strong odors and low boiling points * Most do not conduct electricity
* Most will ignite and burn * Slower rates of reactions
Smells & tastes: fruits, chocolate, fish, mint
Medications: Aspirin, Tylenol, Decongestants, Sedatives
Addictive substances: Caffeine, Nicotine, Alcohol, Narcotics
Hormones/Neurotransmitters: Adrenaline, Epinephrine
Food/Nutrients: Carbohydrates, Protein, Fat, Vitamins
Genetics: DNA, RNA
Consumer products: Plastics, Nylon, Rayon, Polyester
Organic Chemistry in everyday life:
• Animals, plants, and other forms of life consist of organic compounds.– Nucleic acids, proteins, fats, carbohydrates,
enzymes, vitamins, and hormones are all organic compounds
• Besides carbon, the most common elements in organic compounds are hydrogen, oxygen, nitrogen, sulfur, and the halogens.– All of the preceding elements are non-metals, therefore
organic compounds have covalent bonding.
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 5
Numbers and Types of Bonds for Common Elements in Organic CompoundsApplication of the octet rule indicates that these elements should
bond as shown below:
Section 14.1
Review: Octet Rule
• Rule of Eight – elements want either 8 or 0 electrons in its outermost level (except for H and He which want 2 or 0)
Each energy level can only hold a certain number of electrons.
1st level 2 electrons2nd level 8 electrons3rd level 8 electrons4th level 18 electrons
*Helium only has 2 valence electrons
Group Number Number of Valence Electrons
1 1
2 2
13 3
14 4
15 5
16 6
17 7
18 8
Periodic Table and Valence electrons
• http://phet.colorado.edu/sims/html/build-an-atom/latest/build-an-atom_en.html
Let’s Practice Bohr DiagramsEnergy Levels Diagram HW wkst
Practice Lewis Dot Structures1. Oxygen (e = _________) 2. Potassium (e = _______) 3. Bromine (e = ________)
4. Germanium (e= ______) 5. Aluminum (e = ______) 6. Phosphorus (e = ______)
Big Idea in Organic Chemistry
Structure controls Function
Each functional group has predictable reactivity
= atom or group of atoms that gives characteristic chemical properties to a class of organic compounds
Drawing Organic Structures
Butane: C4H10
C C C C
H
H
H
H
H
H
H
H
H
H
CH3 CH2 CH2 CH3
CH3CH2CH2CH3
CH3(CH2)2CH3
Shortcuts make structures easier & faster to draw
Line Structure Carbon Skeleton
• Only shows bonds• C atoms assumed at each end and
intersection of bonds• H atoms not shown• Assume 4 bonds to each C• Fulfill C’s 4 bonds by adding H’s
Lewis Structure Structural formula
Condensed Structuresmolecular formula
Carbon Atoms
Types of Organic CompoundsClassified according to functional group
Alkane
Alkene
Alkyne
Halocarbon
Alcohol
Ether
Ketone
Aldehyde
Carboxylic acid
Amine
Amino acid
AmideO
H
O
NH2
O
OH
O
H2NOH
O
OH
Cl
Br
NH2
C C
O
Hyd
roca
rbon
s (H
& C
onl
y)
Ester
Characteristics and ExamplesHydrocarbons
Alkane Alkene Alkyne
Contain C – C single bond
C = Cdouble bond
C ≡ C triple bond
Formulan is # of carbons
CnH2n+2 CnH2n CnH2n-2
Naming Prefix (# of C’s)-ane # (count from smallest direction of =) – Prefix (# C’s) - ene
# (count from smallest
direction of ≡) – Prefix (# C’s) - yne
Examples See following Slides for examples
Linear/skeletal
structure
\/ \
Organic Prefixes
• Meth- 1 carbon• Eth- 2 carbon• Prop- 3 carbon• But- 4 carbon• Pent- 5 carbon• Hex- 6 carbon
• Hept- 7 carbon• Oct- 8 carbon• Non- 9 carbon• Dec- 10 carbon
Examples
NameMolecular Formula
Lewis/ Structural Formula
Condensed Structural Formula
Linear
propane C3H8 CH3CH2CH3 \/
ethane C2H6 CH3CH3 \
2-pentene C5H10 CH3CHCHCH2CH3
2-butene C4H8 CH3CHCHCH3
NameMolecular Formula
Structural Formula Condensed Structural Formula
3-heptyne C7H12 CH3CH2CCCH2CH2CH3
1-propyne
C3H5 CHCCH3
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 19
Alkanes – Energy Related Products
• Methane = primary component of natural gas• Propane & Butane = primary component of
bottled gas• Gasoline = pentane to decane• Kerosene = alkanes with n = 10 to 16• Alkanes with n > 16 diesel fuel, fuel oil,
petroleum jelly, paraffin wax, lubricating oil, and asphalt
Section 14.3
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 20
Organic Compound Nomenclature
• Due to the large number, variety, and complexity of organic compounds, a consistent method of nomenclature has been developed.
Section 14.3
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 21
IUPAC System of NomenclatureFor Alkanes
• Compound is named as a derivative of the longest continuous chain of C atoms.
• Positions & names of the substituents added– If necessary, substituents named alphabetically– More than one of same type substituent – di, tri, tetra
• The C atoms on the main chain are numbered by counting from the end of the chain nearest the substituents.– Each substituent must have a number.
Section 14.3
Names of Linear Alkanes and Alkyl Substituents
Alkane Alkyl substituents# of
C atoms
CH4
CH3CH3
CH3CH2CH3
CH3CH2CH2CH3
-CH3
-CH2CH3
-CH2CH2CH3
Methyl
Ethyl
Propyl
etc.
Methane
Ethane
Propane
Butane
Pentane
Hexane
Heptane
Octane
Nonane
Decane
Root: number of C atomsSuffix: functional group (-ane for alkanes) (-yl for alkyl groups)
1
2
3
4
5
6
7
8
9
10
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 24
An Example to Consider• The longest continuous chain of C atoms is five• Therefore this compound is a pentane derivative
with an attached methyl group– Start numbering from end nearest the substituent– The methyl group is in the #2 position
• The compound’s name is 2-methylpentane.
Section 14.3
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 25
Drawing a Structure from a NameAn Example
• Draw the structural formula for 2,3-dimethylhexane.
• Note that the end name is hexane .• Draw a continuous chain of six carbon (C)
atoms, with four bonds around each.
Section 14.3
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 26
Drawing a Structure from a NameAn Example (cont.)
• Number the C atoms from right to left.• Attach a methyl group (CH3--) to carbon
number 2 and number 3.– Add necessary H atoms.
• 2,3-dimethylhexane
Section 14.3
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 27
Drawing a Structure from a NameConfidence Exercise
• Draw the structural formula for 2,2,4-trimethylpentane.
• Note that the end name is pentane .• Draw a continuous chain of five carbon (C)
atoms, with four bonds around each.
Section 14.3
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 28
Drawing a Structure from a NameConfidence Exercise (cont.)
• Number the C atoms from right to left.• Attach two methyl groups (CH3--) to carbon
number 2 and one to number 4.
Section 14.3
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 29
Drawing a Structure from a NameConfidence Exercise (cont.)
• Add necessary H atoms.• 2,2,4-trimethylpentane
Section 14.3
C H
H
H
H
Methane CH4
H
CC C C
H H H
H
HHHH
H
Butane C4H10
Butyl -C4H9
Methyl-CH3
C H
H
H
?R
H
CC C C
H H H
H
HHHH
?
Where R = any other C atom or arrangement of C atoms
R
First Ten Hydrocarbons: PropertiesName
Methane
Ethane
Propane
Butane
Pentane
Hexane
Heptane
Octane
Nonane
Decane
1
2
3
4
5
6
7
8
9
10
CH4
C2H6
C3H8
C4H10
C5H12
C6H14
C7H16
C8H18
C9H20
C10H22
Number ofCarbon Atoms
Molecular Formula
Melting Point, oC
# of Isomers
Boiling Point, oC
-182.5
-183.2
-187.7
-138.3
-129.7
- 95.3
- 90.6
- 56.8
- 53.6
- 29.7
-161.5
-88.6
-42.1
-0.5
36.1
68.7
98.4
125.7
150.8
174.0
1
1
1
2
3
5
9
18
35
75
Properties of Alkanes
CompoundMethaneEthanePropaneButanePentane
MW1630445872
Boiling point (°C)-164-88.6-42.1-0.5
+36.0
Linear Alkanes:1 - 4 C atoms: gas at room temp
5 - 15 C atoms: liquid at room temp>15 C atoms: solid at room temp
Larger molecular weight → Stronger London dispersion forcesNonpolar → only London Dispersion Forces IMF
Formula
CH4
C2H6
C3H8
C4H10
C5H12
Naming Branched Alkanes (IUPAC)
1. Root name: name of longest continuous C chain (parent chain)• 2 equally long? Choose the one with more branches
2. Number C atoms in chain, starting at end with first branch3. Identify substituents, give each a number (C it is connected to)
• Two or more identical substituents: use prefixes (di-, tri-, tetra-, etc.)
4. List substituents alphabetically before root name• Do not alphabetize prefixes
5. Punctuation: commas separate numbers from each otherhyphens separate numbers from namesno space between last substituent & root name
4-ethyl-3,5-dimethyloctane1
2
3
658
74
4-ethyl
3-methyl and 5-methyl = 3,5-dimethyl
Octane
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 35
Alkenes are very Reactive and are termed “unsaturated hydrocarbons”
• Alkenes will characteristically react with hydrogen to form the corresponding alkane.
Section 14.3
Copyright © Houghton Mifflin Company. All rights reserved. 14 | 36
Alkynes are Unsaturated Hydrocarbons
• Due to the triple carbon bond, each alkyne molecule can react with two molecules of hydrogen.
Section 14.3
Hydrocarbon Derivatives
Derivatives = molecules that contain C and H, as as hydrocarbons, but also contain other elements
• derivatives depend on their functional groups which are atoms or group of atoms that give the derivative its characteristic chemical behavior
Derivatives
Alkane
Alkene
Alkyne
Halocarbon
Alcohol
Ether
Ketone
Aldehyde
Carboxylic acid
Amine
Amino acid
AmideO
H
O
NH2
O
OH
O
H2NOH
O
OH
Cl
Br
NH2
C C
O
Esters
Halocarbon Definition One or more of hydrogen atoms replaced with a member of
halogen family
General Formula R – XR symbolizes the hydrocarbon portionX symbolizes the halogen atomX can be F, Cl, Br, or I
Naming (IUPAC)
1. Name hydrocarbon portion2. Add prefix to indicate halogen, add -o3. # of halogen placement
Properties Primarily non polarLow boiling pointsInsoluble in waterSoluble in hydrocarbon solvent
Structure
Examples CFC’s –chlorofluorocarbons Methanol (aerosol cans, refrigerate gases) PesticidesDry cleaning chemicals
AlcoholsDefinition One or more of hydrogen atoms replaced with a member of
hydroxyl group (-OH)
General Formula R – OHR symbolizes the hydrocarbon portionOH – hydroxyl group
Naming (IUPAC)
Suffix –ol added to hydrocarbon root
Properties *Similar to water (OH)*Up to 4 C are soluble in water*Higher boiling points *Can be –diol (2 –OH) or –triol (3 -OH)
Structure
Examples
Methanol Ethanol – grain alcohol
Butanol
Definition Oxygen atom that is bonded to two carbon atoms
General Formula R – O – R’R and R’ → hydrocarbon chains-O- → functional group
Naming (IUPAC)
1. Suffix –oxy added to smaller chain bonded to central oxygen atom, remainder is named as before2. Or use similar name: add suffix –yl to each hydrocarbon and add ether
Properties Oxygen creates slightly polar regionSome smaller molecules are soluble in waterNo H bonds so lower boiling points than alcohol but higher than hydrocarbons
Structure
Examples
Ethe
rs
Definition -oxygen atom bonded to single carbon atom by a double bond -called a carbonyl group (C=O) Aldeyde has carbonyl group attached to end of hydrocarbon chain
General Formula R – CHO
Naming (IUPAC)
Add suffix –al to the root name
Properties More polar than hydrocarbonsHigher melting and boiling points than hydrocarbonsLower melting and boiling points than alcohol
Structure
Examples -Methanol (HCOH) = formaldehyde – used to make polymers and used to be used for biological preservation – found to be carcinogenic-Used as flavorings in food and candy and as fragrances in inhalants and perfumes-Vanilla flavor in ice cream and cinnamon in hot chocolate
Alde
hyde
s
Keto
nes
Definition Ketone has a carbonyl group on the interior of a hydrocarbon
General Formula R-COR’
Naming (IUPAC)
Add suffix –one to the root nameName must include which C it is attached to b/c always on interior C when a Ketone
Properties More polar than hydrocarbonsHigher melting and boiling points than hydrocarbonsLower melting and boiling points than alcohol
Structure
Examples -Propanone (CH3COCH3) = acetone - volatile liquid and vapor is flammable-Cortisone= hormonal response to fight or flight, treatment of severe allergic reactions; too much bad b/c breaks down connective tissue, increases production of stomach acid and decreasing protective mucus membranes resulting in gastric ulcer
Definition Characterized by presence of a carboxyl group
General Formula R – COOH
Naming (IUPAC)
Prefix + -anoic acid
Properties -carboxyl end is very polar making it soluble in water-higher boiling points than hydrocarbons
Structure
Examples
(see also book pg 852)
-Fatty acids -Formic acids (simplest form HCOOH) – from ants-Acetic acid – (CH3COOH) – responsible for sour taste of vinegar-lactic acid – responsible for sour cow’s milkCa
rbox
ylic
Aci
ds
Definition Similar to carboxylic acid, but has hydrocarbon group in place of H atom of carboxy group
General Formula
R-COOR’
Naming (IUPAC)
-named for the alcohol and acid from which they are produced-alcohol name (suffix changed to –yl) + acid name (suffix changed to –oate)
Example : ethanol + propanoic acid = ethyl propanoate
OR-alcohol name (-yl) + acid (-ate) = propyl alcohol + formic acid = propyl formate
Properties -polar but do not form H bonds with each other-boiling points are lower than BP of similar alcohols or acids -distinctive odors based on alcohol and acid reaction (typically fruity odors)
Structure
Examples
(see also book pg 856)
Este
r
Definition Contains an amino group (-NH2) attached to hydrocarbon chain
General Formula R-NH2 2◦ = R-NHR’ 3◦ = R-NR’R”
Naming (IUPAC)
-add suffix –amine to root name of hydrocarbon
Properties -amino group is polar -higher boiling points than HC but lower than alcohols-weak bases
Structure
Examples -amino groups found in DNA, vitamins, anesthetic drug-basis of nicotine, cocaine, amphetamines-unpleasant odors = cadaverine produced by bacteria on decaying organisms – can cause food poisoning-found in suntan lotion
Amin
es
Definition Amino group attached to carbon of carboxyl group
General Formula R-CONH2
Naming (IUPAC)
-add suffix –amide to root of hydrocarbon
Properties
Structure
Examples
Amid
es
nylon and urea, which exist in chains, and caffeine, which exists in a ring