introduction to organic chemistry:...
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Introduction to Organic Chemistry:
Hydrocarbons
Chapter 12
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Chapter 12
12.1 – Organic Compounds
12.2 – Alkanes
12.3 – Alkanes with Substituents
12.4 – Properties of Alkanes
12.5 – Alkenes and Alkynes
12.6 – Cis-Trans Isomers
12.7 – Addition Reactions for Alkenes
12.8 – Aromatic Compounds
Organic Compounds
Organic chemistry is the study of carbon compounds.
An organic compound
• Always contains carbon and hydrogen atoms
• May also contain other nonmetals such as oxygen, nitrogen, phosphorus, or a halogen.
• Organic compounds are found in:
• Gasoline, medicines, shampoos, plastics, and perfumes
• Carbohydrates, fats, and proteins
Functional Groups
• Organic compounds are organized by their functional groups (groups of atoms bonded in a specific way).
• Compounds that contain the same functional groups have similar physical and chemical properties.
• The identification of functional groups allows us to classify organiccompounds according to their structure, to name compounds within each family, and to predict their chemical reactions.
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Organic vs. Inorganic
• In chemistry, molecules are classified as Organic or
Inorganic.
• Inorganic compounds are (quite expansively)
anything that is not organic.
• Organic and Inorganic compounds have different
properties.
– Organic compounds:
▪ Have low melting and boiling points.
▪ Are flammable and undergo combustion.
▪ Are not soluble in water.
– Inorganic compounds
▪ Many inorganic compounds have high
melting and boiling points.
▪ Inorganic compounds that are ionic are
usually soluble in water, and most do not
burn in air.
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Practice
Identify each characteristic as most typical of compounds that are inorganic or organic.
A. It has a high melting point.
B. It is not soluble in water.
C. It contains carbon and hydrogen atoms.
D. It has the formula MgCl2.
E. It burns easily in air.
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Representations of Carbon Compounds
• Hydrocarbons are organic compounds that consist of only carbon and
hydrogen.
– In organic molecules, every carbon atom has four bonds.
– In methane (CH4), the carbon atom forms an octet by sharing its four
valence electrons with four hydrogen atoms.
Three-dimensional and two-dimensional representations of methane: a)
space-filling model, b) ball-and-stick model, c) wedge-dash model, d)
expanded structural formula, and e) condensed structural formula
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Representations of Carbon Compounds
• In ethane (C2H6), each tetrahedral carbon forms three covalent bonds to
hydrogen and one to the other carbon.
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Alkanes
Alkanes
• are formed by a continuous chain of carbon atoms.
• are named using the IUPAC (International Union of Pure
and Applied Chemistry) system.
• have names that end in ane.
• use Greek prefixes to name carbon chains with five or
more carbon atoms.
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Study Check
In the butane molecule (C4H10), predict the shape around
each carbon atom.
C
H
H
H C
H
H
C
H
H
C
H
H
H
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Chapter 12
12.1 – Organic Compounds
12.2 – Alkanes
12.3 – Alkanes with Substituents
12.4 – Properties of Alkanes
12.5 – Alkenes and Alkynes
12.6 – Cis-Trans Isomers
12.7 – Addition Reactions for Alkenes
12.8 – Aromatic Compounds
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12.2 - AlkanesWrite the IUPAC names and draw the condensed or line-angle structural
formulas for alkanes and cycloalkanes.
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Alkanes
• More than 90% of the compounds in
the world are organic compounds.
• The larger number of carbon
compounds is possible because the
covalent bonds between carbon
atoms (C-C) is very strong, allowing
carbon atoms to form long, stable
chains.
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Alkanes
• The alkanes are a type of hydrocarbon in which the carbon atoms are
connected only by single bonds.
– Alkanes are formed by a continuous chain of carbon atoms.
– The names of alkanes and in –ane.
▪ Such names are part of the IUPAC system (International Union
of Pure and Applied Chemistry) used by chemists to name
organic chemistry.
– Alkanes made of carbon chains are named based on how many
carbons make up the chain.
– One of the most common uses of alkanes is as fuels.
▪ Methane, propane, octane, and hexane are all alkanes used
as fuels.
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Line-Angle Structural Formulas
A simplified structure of organic molecules
• is called the line-angle structural formula.
• shows a zigzag line in which carbon atoms are
represented as the ends of each line and as corners.
Carbon atoms
• at the end are bonded to three hydrogen atoms.
• in the middle are bonded to two hydrogen atoms.
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Condensed formula and Line-angle formula
• Pentane
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Condensed formula and Line-angle formula
• Draw the condensed structural formula and name the molecule:
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Guide to Drawing Structural Formulas for
Alkanes
Step 1: Draw the carbon chain.
Step 2: Draw the expanded structural formula by adding the
hydrogen atoms using single bonds to each of the
carbon atoms.
Step 3: Draw the condensed structural formula by combining
the H atoms with each C atom.
Step 4: Draw the line-angle structural formula as a zigzag
line in which the ends and corners represent C
atoms.
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Drawing Expanded, Condensed, and Line-
Angle Structural Formulas (1 of 3)
Draw the expanded, condensed, and line-angle structural
formula for pentane.
Step 1: Draw the carbon chain. A molecule of pentane has
five carbon atoms in a continuous chain.
Step 2: Draw the expanded structural formula by adding
the hydrogen atoms, using single bonds to each
of the carbon atoms.
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Drawing Expanded, Condensed, and Line-
Angle Structural Formulas (2 of 3)
Draw the expanded, condensed, and line-angle structural
formula for pentane.
Step 3: Draw the condensed structural formula by
combining the H atoms with each C atom.
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Drawing Expanded, Condensed, and Line-
Angle Structural Formulas (3 of 3)
Draw the expanded, condensed, and line-angle structural
formula for pentane.
Step 4: Draw the line-angle structural formula as a
zigzag line in which the ends and corners
represent C atoms.
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Conformations of Alkanes
• Single bonds can spin and rotate.
• Thus different arrangements, known as conformations, occur during
the rotation about a single bond.
• http://symmetry.otterbein.edu/gallery/index.html
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Structural Formulas: C4H10
As butane (C4H10) rotates, sometimes the
line up in front of each other, and at other times they are
opposite each other. Butane can be drawn using a variety of
two-dimensional condensed structural formulas:
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Cycloalkanes
Hydrocarbons can also form into circles or rings called:
cycloalkanes
• have two fewer hydrogen atoms than the open chain form.
• are named by using the prefix cyclo before the name of
the alkane chain with the same number of carbon atoms.
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Formulas of Cycloalkanes
Table 12.4 Formulas of Some Common Cycloalkanes
Name BLANK BLANK BLANK
Cyclopropane Cyclobutane Cyclopentane Cyclohexane
Ball-and-Stick Model BLANK BLANK BLANK
Three carbons single-bonded to each other in a triangular pattern,
with each carbon single-bonded to 2 hydrogens.
The ball and stick model shows four
carbons single-bonded to each other in a
square pattern, with each carbon single-
bonded to 2 hydrogens.
The ball and stick model shows five
carbons single-bonded to each other in
a pentagonal pattern, with each carbon
single-bonded to 2 hydrogens.
The ball and stick model shows six
carbons single-bonded to each other in
a hexagonal pattern, with each carbon
single-bonded to 2 hydrogens.
Condensed Structural Formula BLANK BLANK BLANK
The condensed structural formula shows a triangular ring of three C
H 2 molecules.
The condensed structural formula shows
a square ring of four C H 2 molecules.
The condensed structural formula
shows a pentagonal ring of five C H 2
molecules.
The condensed structural formula
shows a hexagonal ring of six C H 2
molecules.
Line-Angle Structural Formula BLANK BLANK BLANK
The line-angle structural formula is a triangle. The line-angle structural formula shows a
square.
The line-angle structural formula shows
a pentagon. The line-angle structural formula shows
a hexagon.
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Study Check
Give the IUPAC name for each of the following compounds:
A.
B.
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Study Check
Name the following alkanes:
A.
B.
C.
D.
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Chapter 12
12.1 – Organic Compounds
12.2 – Alkanes
12.3 – Alkanes with Substituents
12.4 – Properties of Alkanes
12.5 – Alkenes and Alkynes
12.6 – Cis-Trans Isomers
12.7 – Addition Reactions for Alkenes
12.8 – Aromatic Compounds
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12.3 – Alkanes and Substituents
Write the IUPAC names for alkanes with substituents and draw their
condensed and line-angle structural formulas.
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Structural Isomers
Structural isomers
• have the same molecular formula with a different arrangement
of atoms.
• have the same number of atoms bonded in a different order.
Butane (C4H10) has two structural isomers: a straight chain and a
branched chain.
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Study Check
Draw three possible structural isomers of pentane
(C5H12).
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Solution
Draw three possible structural isomers of pentane
(C5H12).
Structural
Isomers of
C5H12
Structural Isomers of C5H12 Structural Isomers of
C5H12
Structural Isomers
of C5H12
CondensedThe first condensed structural formula is a straight chain of single-bonded molecules as follows. C H 3, C H 2, C H 2, C H 2, C H 3. The second condensed structural formula is a branched chain as follows. C H 3, C H single-bonded to C H 3 above,
C H 2, C H 3.The third condensed structural formula is a central C
single-bonded to four C H 3 molecules above, below,
rightward, and leftward.
Line-AngleThe line-angle structural formula shows a zigzag line made of 4 segments forming 3 angles. The line-angle structural formula shows a zigzag of 3 segments forming 2 angles, with
a fourth segment rising vertically from the first angle.
The line-angle structural formula shows 2 rising and falling line
segments with 2 segments rising diagonally right and left from the angle.
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Study Check
Is the pair of formulas structural isomers? Or the same molecule?
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Substituents in Alkanes
• When CH3 branches off of a carbon chain, it’s called an alkyl group
• When a halogen atom (Group 17) is attached to a carbon chain, it is
named as a halo group with the terms –fluoro, -chloro, -bromo, -iodo
based on which element it is.
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Substituents and Alkyl Groups
Table 12.5 Formulas and Names of Some Common Substituents
Formula
Name
Formula, C H 3, single bond. name, methyl.
Formula, straight chain, C H 3, C H 2, single
bond. name, ethyl.
BLANK BLANK
Formula
Name
Formula, straight chain, C H 3, C H 2, C H 2, single bond. name,
propyl.
Formula, branched chain, C H 3, C H with single bond above, C
H 3. name, isopropyl. BLANK BLANK
Formula
Name
Formula, straight chain, C H 3, C H 2, C H 2, C H 2, single bond.
name, butyl.
Formula, branched chain, C H 3, C H single-bonded to C H 3
above, C H 2, single bond. name, isobutyl.
Formula, C H 3, C H with single bond above, C H 2,
C H 3. name, secondary butyl.Formula, central C with single bond
above and three C H 3 molecules
below, rightward, and leftward.
name, tertiary butyl.
Formula
Name
Formula, F, single bond. name, fluoro. Formula, F, single bond. name, fluoro. Formula, B r, single bond. name, bromo. Formula, I, single bond. name, iodo.
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Naming Alkanes with Substituents
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Naming Alkanes with Substituents
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Naming Cycloalkanes with Substituents
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Naming Cycloalkanes with Substituents
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Naming Haloalkanes
Haloalkanes
• are alakanes with a halogen atom that replaces a hydrogen atom.
• are named by putting the substituents in alphabetical order.
• have the halo group numbered according to the carbon where it is
attached to the alkane.
Examples of
Haloalkanes
BLANK BLANK BLANK BLANK
Formulastraight chain, C H 3, C l straight chain, C H 3, C H 2, B r Branched chain, C H 3, C H single-bonded to an F above A central C single-bonded to C l above and three C H 3 molecules below, rightward, and leftward
IUPAC Chloromethane Bromoethane 2-Fluoropropane 2-Chloro-2-
methylpropane
Common Methyl chloride Ethyl bromide Isopropyl fluoride Tert-Butyl chloride
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Drawing the molecule from the name
Draw the condensed and line-angle structural formulas for
2,3-dimethylbutane.
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Drawing the molecule from the name
Draw the condensed and line-angle structural formulas for
2-bromo-3-ethyl-4-methylpentane.
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Chapter 12
12.1 – Organic Compounds
12.2 – Alkanes
12.3 – Alkanes with Substituents
12.4 – Properties of Alkanes
12.5 – Alkenes and Alkynes
12.6 – Cis-Trans Isomers
12.7 – Addition Reactions for Alkenes
12.8 – Aromatic Compounds
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12.4 – Properties of Alkanes
Identify the properties of alkanes and write a balanced chemical
equation for combustion.
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Properties of Alkanes
Many types of alkanes are the components
of fuels that power our cars and oil that
heats our home.
The solid alkanes that make up waxy
coatings on fruits and vegetables help
retain moisture, inhibit mold, and enhance
appearance.
The different uses of alkane compounds
result from their physical properties,
including their solubility and density.
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Uses of Alkanes (1 of 2)
Alkanes with one to four carbons are gases at room
temperature and are widely used as heating fuels.
methane, ethane, propane, butane
Butane has four carbons:
Alkanes with five to eight carbons are highly volatile liquids
at room temperature, which makes them useful as fuels.
pentane, hexane, heptane, octane
Octane has eight carbons:
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Uses of Alkanes (2 of 2)
Alkanes with 9−17 carbons are liquids with higher boiling
points and are found in motor oils, mineral oil, kerosene,
diesel, and jet fuels.
Decane has 10 carbons:
• Alkanes with 18 or more carbon atoms, known as
paraffins, are waxy solids at room temperature.
• Petroleum jelly, or Vaseline, is a semisolid mixture of
hydrocarbons with more than 25 carbon atoms.
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Melting and Boiling Points (1 of 4)
Alkanes
• have the lowest melting and boiling points of organic
compounds.
• contain only the nonpolar bonds of
• exhibit only weak dispersion forces in the solid and liquid states.
Longer-chain alkanes have more dispersion forces.
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Melting and Boiling Points (2 of 4)
Branched alkanes
• have lower boiling points than the straight-chain isomers.
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Melting and Boiling Points (2 of 4)
Branched alkanes
• have lower boiling points than the straight-chain isomers.
• tend to be more compact, reducing the points of contact
between the molecules.
• do not have linear shapes and cannot line up close to each
other.
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Melting and Boiling Points (3 of 4)
Cycloalkanes
• have higher boiling points than the straight-chain alkanes
with the same number of carbon atoms.
• have limited rotation of carbon bonds; they maintain their
rigid structure and can be stacked closely together, which
gives them many points of contact and attractions to each
other.
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Melting and Boiling Points (4 of 4)
We can compare the boiling points of straight-chain alkanes,
branched-chain alkanes, and cycloalkanes.Table 12.6 Comparison of Boiling Points of Alkanes and Cycloalkanes with Five Carbons
Formula Name Boiling Point (°C)
Straight-Chain Alkane BLANK BLANKStraight chain alkanes. condensed structural formula, C H 3, C H 2, C H 2, C H 2, C H 3
Pentane 36
Branched-Chain Alkanes BLANK BLANKBranched chain alkanes. condensed structural formula, C H 3, C H single-bonded to C H 3, C H 2, C H 3
2-Methylbutane 28
Central C single-bonded to four C H 3 molecules
Dimethylpropane 10
Cycloalkane BLANK BLANKline-angle structural formula, a pentagonal ring
Cyclopentane 49
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Combustion of Alkanes (1 of 3)
The carbon–carbon single bonds in alkanes are difficult to
break, which makes them the least reactive family of organic
compounds.
However, alkanes burn readily in oxygen to produce carbon
dioxide, water, and energy.
Alkane O2 CO2 H2O + energyg g g g
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Combustion of Alkanes (3 of 3)
Methane is the natural gas we use to cook our food and
heat our homes. The equation for the combustion of
methane (CH4) is written as follows:
4 2 2 2CH 2O CO 2H O + energyg g g g
Propane is the gas used in portable heaters and gas
barbecues. The equation for the combustion of propane
(C3H8) is written as follows:
4 2 2 2CH 5O 3CO 4H O + energyg g g g
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Solubility and Density of Alkanes
Alkanes are
• nonpolar.
• insoluble in water.
• less dense than water.
• flammable in air.
• found in crude oil.
If there is an oil spill in the ocean, the alkanes in the crude oil
do not mix with the water but float on top, forming a thin
layer on the surface.
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Chapter 12
12.1 – Organic Compounds
12.2 – Alkanes
12.3 – Alkanes with Substituents
12.4 – Properties of Alkanes
12.5 – Alkenes and Alkynes
12.6 – Cis-Trans Isomers
12.7 – Addition Reactions for Alkenes
12.8 – Aromatic Compounds