organic chemistry saturated & unsaturated … hydrocarbons • contain one or more double or...
TRANSCRIPT
Organic Chemistry
Saturated & Unsaturated
HydrocarbonsBIOB111
CHEMISTRY & BIOCHEMISTRY
Session 8
Key concepts: session 8From this session you are expected to develop an understanding of the following concepts:
Concept 1: Solubility of hydrocarbons in H2O
Concept 2: Creation of CFC compounds
Concept 3: Alkyl groups
Concept 4: Reactivity of saturated vs unsaturated hydrocarbons
Concept 5: Alkanes vs alkenes vs alkynes
Concept 6: Conversion between the hydrocarbon functional groups (alkane, alkene and alkyne)
Concept 7: Bromination reactions
Concept 8: Properties of benzene
Concept 9: Hydration reactions
Concept 10: Identifying primary, secondary and tertiary alcohols
These concepts are covered in the Conceptual multiple choice questions of tutorial 8
Session OverviewPart 1: Exploring saturated hydrocarbon compounds
• Saturated vs unsaturated hydrocarbon compounds
• Chemical properties of alkanes
• Alkyl groups are derived from alkanes
Part 2: Exploring unsaturated hydrocarbon compounds
• Chemical properties of alkenes
• Bromination reactions
• Chemical properties of alkynes
• Chemical properties of benzene
Part 3: The alcohol function group
• Hydrocarbon derivatives
• Chemical properties of alcohols
Part 1: Exploring saturated hydrocarbon compounds
• Saturated vs unsaturated hydrocarbon compounds
• Chemical properties of alkanes
• Alkyl groups are derived from alkanes
Hydrocarbon derivatives
Life on earth would not exist without organic compounds that contain carbon atoms
• Our genetic material (DNA) contains many carbon atoms
• Our bodies rely on the organic compounds below to function:
– Proteins are made up of amino acids
– Lipids are often made up of fatty acids (long hydrocarbons) and glycerol
– Carbohydrates are made up of one or more monosaccharide (sugar) units
Hydrocarbon compounds:
The most basic organic compounds are hydrocarbons
– Hydrocarbons contain only carbon and hydrogen atoms
– Hydrocarbons compounds are created in nature
and can be synthesised in the laboratory
Structures of Hydrocarbon compounds
Each line connecting the atoms below represents a covalent bond (2 electrons shared between the two
connected atoms)
Saturated vs unsaturated hydrocarbon compounds
HYDROCARBONS BELONG TO ONE OF THREE
FUNCTIONAL GROUPS
Type
ALKANE
CONTAIN ONLY SINGLE CARBON
TO CARBON BONDS
ALKYNEDefinition
Saturated vs unsaturated hydrocarbon compounds
ALKENE
CONTAIN ONE OR MORE DOUBLE
CARBON TO CARBON BONDS
CONTAIN ONE OR MORE
TRIPLE CARBON TO CARBON
BONDS
Example
ExampleExample
Type
Type
Definition
Definition
HYDROCARBONSType
SATURATED HYDROCARBON
CONTAIN ONLY SINGLE CARBON TO
CARBON BONDS
ORGANIC COMPOUNDS THAT CONTAIN CARBON AND HYDROGEN ATOMS
CONTAIN ONE OR MORE DOUBLE OR TRIPLE CARBON TO CARBON BOND,
ALSO CONTAIN ONE OR MORE SINGLE CARBON TO CARBON BONDS
UNSATURATED HYDROCARBON
Type
Definition
Definition
Definition
UNREACTIVE
Are
REACTIVE
Are
Due to
LARGE AMOUNT OF ENERGY NEEDED TO BREAK THE SINGLE BONDS PRESENT
Due to
DOUBLE AND TRIPLE CARBON TO CARBON BONDS CAN EASILY BE
BROKEN IN A CHEMICAL REACTION
Saturated vs unsaturated hydrocarbon compounds
Unsaturated hydrocarbons• Contain one or more double or
triple carbon to carbon bond– Are also likely to contain one or
more single carbon to carbon bonds
• Functional groups: Alkene, alkyne
Saturated hydrocarbons
• Contain only single carbon to carbon bonds
• Functional groups: Alkane
• Unreactive and stable– Due to the large amount of energy
needed to break the existing chemical
bonds
• Reactive and unstable (compared
to saturated hydrocarbons)– Due to the small amount of energy
required to break the double or triple
carbon to carbon bonds present
Saturated vs unsaturated hydrocarbon compounds
Saturated Hydrocarbons
– Saturated hydrocarbons have only single carbon to carbon bonds
Saturated vs unsaturated hydrocarbon compounds
– The carbon atoms in saturated hydrocarbons form bonds to the
maximum amount of hydrogen atoms possible
• These compounds are saturated with hydrogen atoms
– Include alkanes (straight chains) & cycloalkanes (carbon rings)
Unsaturated Hydrocarbons– Unsaturated hydrocarbons have one or more double or triple
carbon to carbon bond(s)• Will also contain single carbon to carbon bonds
Saturated vs unsaturated hydrocarbon compounds
– The carbon atoms in unsaturated hydrocarbons form bonds to less than the maximum amount of hydrogen atoms possible
• These compounds are not saturated with hydrogen atoms (unsaturated)– Due to the presence of double or triple carbon to carbon bonds
– Include Alkenes (straight chains) & Cycloalkenes (carbon rings)
Number of Carbon Atoms Prefix Alkane Alkene Alkyne
1 Meth- Methane - -
2 Eth- Ethane Ethene Ethyne
3 Prop- Propane Propene Propyne
4 But- Butane Butene Butyne
5 Pent- Pentane Pentene Pentyne
6 Hex- Hexane Hexene Hexyne
7 Hept- Heptane Heptene Heptyne
8 Oct- Octane Octene Octyne
9 Non- Nonane Nonene Nonyne
10 Dec- Decane Decene Decyne
Saturated vs unsaturated hydrocarbon compounds
Chemical properties of alkanesPropane is an alkane:
Used as a fuel for cars
(LPG gas)
Functional Group: Alkane
Distinguishing characteristic: Alkane compounds contain only single
carbon to carbon bonds
Naming convention: Alkane compounds have –ane at the end of their
name e.g. propane
Example compound:
Propane
HYDROCARBONS BELONG TO ONE OF THREE
FUNCTIONAL GROUPS
Type
ALKANE
CONTAIN ONLY SINGLE CARBON
TO CARBON BONDS
ALKYNEDefinition
Chemical properties of alkanes
ALKENE
CONTAIN ONE OR MORE DOUBLE
CARBON TO CARBON BONDS
CONTAIN ONE OR MORE
TRIPLE CARBON TO CARBON
BONDS
Example
ExampleExample
Type
Type
Definition
Definition
Chemical properties of alkanes
Alkanes are non-polar compounds
– Alkanes contain only carbon and hydrogen atoms which are connected via non-polar covalent bonds (equal electron sharing)
H2O is a polar compound
– H2O contains polar covalent bonds where the shared electrons are more attracted to the oxygen atom than the hydrogen atoms
• Compounds must be polar to dissolve in H2O
Chemical properties of alkanes
Will an alkane compound (such as propane) dissolve in H2O?
– Non-polar alkanes do not dissolve in polar H2O
– Alkanes are insoluble in H2O
– The non-polar alkane will only dissolve in non-polar solvents such as chloroform
Propane
Chemical properties of alkanesCombustion– Combustion reactions are exothermic
reactions that release heat
– Alkanes burn in the presence of oxygenproducing CO2, H2O and heat via combustion reactions
– Example: combustion of methane
CH4 + 2O2 → CO2 + 2H2O + Energy
https://www.freeimages.com/photo/fire-camp-1174281
– All combustion reactions are redox
reactions where one reactant is oxidised
and one is reduced
• Oxygen is always reduced
in redox reactions
Chemical properties of alkanes
Halogenation
– Halogenation reactions involve an alkane reacting with
a halogen molecule such as Cl2 or F2
– The end result of a halogenation reaction:
• Substitution of one of the alkane’s hydrogen atoms with a halogen
atom, producing a halogenated alkane
Stoker 2014, p368-70
Methane Halogen molecule
Halogenated alkane
C Cl
H
H
H
H Cl C
H
H
H
Cl H Cl+ +Methane
Halogen molecule
Halogenated alkane
• During a halogenation reaction the alkane’s hydrogen atom is replaced by
a single halogen atom, producing a halogenated alkane
• The lost hydrogen atom forms a compound with the other halogen atom (from the
halogen molecule), in this case creating the strong acid HCl
• Additional hydrogen atoms can be substituted in the halogenated alkane by performing
additional halogenation reactions
Large energy input
Halogenation
C Cl
H
H
H
H Cl+MethaneReactant
Halogen moleculeReactant
Halogenated alkane
HCl product
Animation of a halogenation reaction
Chemical properties of alkanes
Energy input Energy
input
Chemical properties of alkanes
Chlorofluorocarbons (CFCs)– Synthetic organic compounds that were developed to be used as refrigerants
• Refrigerants can be used to heat a pump that powers refrigeration
– The 2 most commonly used CFCs were Freon-11 and Freon-12
• CFCs destroyed a significant amount of the ozone layer in the stratosphere until banned
Stoker 2014, p373
How many halogenation reactions would it take to
convert methane (CH4) into a halogenated alkane
that contains three fluorine atoms?
Alkyl groups are derived from alkanes
Alkyl Groups
– Once an alkane loses one of its hydrogen atoms
it becomes an alkyl group
Alkane: methane Alkyl group: methyl
Alkane loses a hydrogen atom
• Naming: replace the -ane with -yl at the end of the name
– Methane becomes methyl
Alkyl groups are derived from alkanesAlkyl Groups
– Once an alkane loses one of its hydrogen atoms it becomes an alkyl group
– Alkyl groups can attach to an atom or compound
by forming a covalent bond
Alkyl group: methyl
R represents an attachment point to another atom or
compound
Methyl Group
Methyl group branching off a 5 carbon chain
Alkyl groups: derived from alkanes
Ethyl Group
Ethyl group branching off a 5
carbon chain
After methane loses a hydrogen = methyl group R—CH3
After ethane loses a hydrogen = ethyl group R—CH2—CH3
After propane loses a hydrogen = propyl group R—CH2—CH2—CH3
Identify the name and position of the alkyl group in
the compound below
Attempt Socrative questions: 1 to 3
Google Socrative and go to the student login
Room name:
City name followed by 1 or 2 (e.g. PERTH1)
1 for 1st session of the week and 2 for 2nd session of the week
Part 1: Exploring saturated hydrocarbon compounds
• Saturated vs unsaturated hydrocarbon compounds
– Saturated hydrocarbons contain only single carbon to carbon bonds and
contain the maximum number of hydrogen atoms attached to the carbon
atoms
– Alkanes and cycloalkane are saturated hydrocarbons
– Unsaturated hydrocarbons contain one or more double or triple carbon to
carbon bonds, as well as other single carbon to carbon bonds
– Unsaturated hydrocarbons contain less than the maximum number of
hydrogen atoms attached to the carbon atoms, due to the presence of double
or triple carbon to carbon bonds
– Alkenes and cycloalkenes are unsaturated hydrocarbons
Part 1: Exploring saturated hydrocarbon compounds
• Chemical properties of alkanes
– Alkanes are non-polar compounds that do not dissolve in H2O (insoluble in
H2O)
– Alkanes burn in oxygen in combustion reactions (type of redox reaction)
– Alkanes can react with halogen molecules (e.g. Cl2) to replace one hydrogen
at a time with a halogen atom via a halogenation reaction
• Alkyl groups are derived from alkanes
– Once an alkane loses one of its hydrogen atoms it becomes an alkyl group
– Alkyl groups can attach to an atom or compound by forming a covalent bond
– Methane becomes a methyl group by losing a hydrogen atom
Part 2: Exploring unsaturated hydrocarbon compounds
• Chemical properties of alkenes
• Bromination reactions
• Chemical properties of alkynes
• Chemical properties of benzene
Chemical properties of alkenes
Functional Group: Alkene
Distinguishing characteristic: Alkene compounds contain one or more
double carbon to carbon bond(s), and will also likely contain some single
carbon to carbon bonds
Naming convention: Alkene compounds have -ene at the end of their
name e.g. propene
Example compound:
Propene
HYDROCARBONS BELONG TO ONE OF THREE
FUNCTIONAL GROUPS
Type
ALKANE
CONTAIN ONLY SINGLE CARBON
TO CARBON BONDS
ALKYNEDefinition
Chemical properties of alkenes
ALKENE
CONTAIN ONE OR MORE DOUBLE
CARBON TO CARBON BONDS
CONTAIN ONE OR MORE
TRIPLE CARBON TO CARBON
BONDS
Example
ExampleExample
Type
Type
Definition
Definition
Stereoisomers are a group of two compounds that are very similar:
• The group of compounds has the same number of each type of atom present and the same
chemical bonding pattern
• Each of the two stereoisomer compounds are arranged differently in space
– The two different variations of the stereoisomer compounds
have different chemical properties
– Example:
• cis stereoisomer = both large CH3 groups are on the same side of the carbon to carbon double bond
• Trans stereoisomer = The large CH3 groups are on different sides of the carbon to carbon double bond
cis = same trans = different
Chemical properties of alkenes
The stereoisomer
pair to the right are alkenes
• Unsaturated hydrocarbons (such as alkenes and alkynes)
are more reactive than saturated hydrocarbons (such as alkanes)
Chemical properties of alkenes
Each line represents a single covalent bond that requires significant input
energy to break
– Alkanes contain only single carbon to carbon bonds, which require
significant input energy to break
• Difficult to replace hydrogen atoms attached to carbons with other
atoms (e.g. halogens Cl, F)
– Alkanes stable and unreactive
• Unsaturated hydrocarbons (such as alkenes and alkynes) are more
reactive than saturated hydrocarbons (such as alkanes)
– Alkenes and alkynes have double and triple carbon to carbon bonds, respectively
Chemical properties of alkenes
Multiple carbon to carbon bonds which can be broken with a
small amount of input energy
– A double or triple carbon to carbon bond can be broken with a smaller amount of input energy than single carbon to carbon bond
– Once a double or triple carbon to carbon bond has been broken:• Other atoms can bond to the carbon atoms that were previously part
of the multiple carbon to carbon bond– Carbon must have 4 covalent bonds at all times to be stable
Chemical properties of alkenes
C C CH
H
HH
H
H
Cl Cl+Energy input
Energy input
Once the double carbon to carbon bond is broken the two chlorine atoms are incorporated into the compound, which allows each carbon atom to have 4 covalent bonds
Animation of the reactivity of an alkene
Addition Reaction Reactants Products
HYDROGENATION Alkene + H2 Alkane
HALOGENATION Alkene + Cl2 or Br2 Halogenated alkane
HYDRATION Alkene + H2O Alcohol
• Alkenes can take part in addition reactions:
– Once a double or triple carbon to carbon bond has been broken:• Other atoms can bond to the carbon atoms that were previously part
of the multiple carbon to carbon bond– Carbon must have 4 covalent bonds at all times to be stable
• Breaking a multiple carbon to carbon bond creates new positions where carbon atoms can form covalent bonds to other atoms
Chemical properties of alkenes
Addition of a H2 molecule into an alkene:
• Replaces the double carbon to carbon bond with two new covalent bonds between
the carbon atoms and the added hydrogen atoms
– End result: the alkene is converted to an alkane
• The carbon atoms that form the new bonds with the added hydrogen atoms
were previously part of the double carbon to carbon bond
Chemical properties of alkenes
Propene (alkene) Hydrogenmolecule
Propane (alkane)
Hydrogenation reaction
Chemical properties of alkenes
C C CH
H
HH
H
H
H H+Energy input
Energy input
Once the double carbon to carbon bond is broken the two hydrogen atoms are incorporated into the compound, which allows each carbon atom to have 4 covalent bonds
Animation of a hydrogenation reaction where an alkene is converted into an alkane
Hydration reaction
Chemical properties of alkenes
Propene (alkene) watermolecule
Propanol (alcohol)
Alcohol functional group
Addition of a H2O molecule into an alkene:
• Replaces the double carbon to carbon bond with two new covalent bonds between
one carbon atom and H, a second carbon atoms and an OH group
– End result: the alkene is converted to an alcohol (contains the alcohol functional group)
• The carbon atoms that form the new bonds with the H and OH
were previously part of the double carbon to carbon bond
Chemical properties of alkenes
C C CH
H
HH
H
H
OH H+Energy input
Energy input
Once the double carbon to carbon bond is broken the OH group and a hydrogen atom are incorporated into the compound, which allows each carbon atom to have 4 covalent bonds
Animation of a hydration reaction where an alkene is converted into an alcohol
H2O
Alcohol functional group
Halogenation reaction
Chemical properties of alkenes
Propene (alkene) Halogenmolecule
Halogenated alkane
Addition of a halogen molecule (e.g. Cl2) into an alkene:
• Replaces the double carbon to carbon bond with two new covalent bonds between
the carbon atoms and the added halogen atoms
– End result: the alkene is converted to a halogenated alkane
• The carbon atoms that form the new bonds with the added halogen atoms were previously part of the double carbon to carbon bond
• Each halogenation reaction with an alkene adds two halogen atoms at a time
Chemical properties of alkenes
C C CH
H
HH
H
H
Cl Cl+Energy input
Energy input
Once the double carbon to carbon bond is broken the two chlorine atoms are incorporated into the compound, which allows each carbon atom to have 4 covalent bonds
Animation of a halogenation reaction where an alkene is converted into a halogenated alkane
• Bromine is a halogen (Br2) that can readily be added into an alkene via a halogenation reaction
• A large amount of input energy is needed to add bromine atoms into an alkane
one at a time via a halogenation reaction, so the reaction occurs less often
Propene (alkene) Halogenmolecule
Halogenated alkane
Propane (alkane) Halogenmolecule
Halogenated alkane
Large energy input
Reactive
Less reactive
Bromination reactions
• A Bromination test is used to determine whether a solution contains a dissolved alkane or alkene
– When in solution, bromine is red
– When bromine is incorporated into a compound
the solution becomes colourless
Stoker 2014, p399
The red colour shows that bromine is in the solution
Once all of the bromine is incorporated into a compound,
the solution is colourless
Bromination reactions
What will happen when bromine is added to an alkane solution?
– When bromine (Br2) is added to an alkane solution,
the red color of bromine persists• Br2 is not incorporated into the alkane compound
• No chemical reaction occurs due to large amount of energy needed to begin the reaction
The red bromine is not incorporated into the alkane
compound
The red colour remains as bromine has not been incorporated into a
compound Stoker 2014, p399
Bromination reactions
What will happen when bromine is added to an alkene solution?
– When bromine (Br2) is added to an alkene or alkyne solution, the red color of bromine disappears quickly
• Br2 is readily incorporated into the alkene compound, which becomes a halogenated alkane via a halogenation reaction
Bromine is readily incorporated into
the alkene compound
Once all of the bromine is incorporated into a compound,
the solutions is colourless Stoker 2014, p399
Chemical properties of alkynes
Functional Group: Alkyne
Distinguishing characteristic: Alkyne compounds contain one or more
triple carbon to carbon bond(s), and will also likely contain some single
carbon to carbon bonds
Naming convention: Alkyne compounds have –yne at the end of their
name e.g. propyne
Example compound:
Propyne
HYDROCARBONS WHICH CONTAIN ONLY
CARBON AND HYDROGEN ATOMS BELONG TO
ONE OF THREE FUNCTIONAL GROUPS
Type
ALKANE
CONTAIN ONLY SINGLE CARBON
TO CARBON BONDS
ALKYNEDefinition
Chemical properties of alkynes
ALKENE
CONTAIN ONE OR MORE DOUBLE
CARBON TO CARBON BONDS
CONTAIN ONE OR MORE
TRIPLE CARBON TO CARBON
BONDS
Example
ExampleExample
Type
Type
Definition
Definition
Chemical properties of alkynes
• Alkynes can participate in many of the same chemical reactions as alkenes:
– Hydrogenation • Adding two hydrogen atoms
– Hydration• Adding H2O, which creates an alcohol group
– Halogenation reactions• Adding two halogen atoms
• Alkynes behave similarly to alkenes in chemical reactions
– Both have multiple carbon to carbon bonds which can be broken with a small energy input
Chemical properties of alkynes
Which addition reaction could be used to convert
and alkyne into an alkane? – How many of these addition reactions would be required?
• Two hydrogenation reactions are required to
convert an alkyne into an alkane
– Each hydrogenation reaction adds two hydrogen atoms to the compound
Propene (alkene) Propane (alkane)Propyne (alkyne)
Hydrogenation Hydrogenation
+ 2 hydrogen atoms
+ 2 hydrogen atoms
Chemical properties of alkynes
C C CH
HH H H H+
Energy input
Energy input
Once the triple carbon to carbon bond is broken, two hydrogen atoms are incorporated into the compound, which allows each carbon atom to have 4 covalent bondsThe alkyne has been converted into an alkene
Animation of the two hydrogenation reactions required to convert an alkyne into an alkane
Energy input
H HEnergy input+
Once the double carbon to carbon bond is broken, two hydrogen atoms are incorporated into the compound, which allows each carbon atom to have 4 covalent bondsThe alkene has been converted into an alkane
Are saturated or unsaturated hydrocarbons
more reactive?
What types of chemical reactions do the
reactive hydrocarbons participate in?
What allows the reactive hydrocarbons
to participate in these reactions?
How is an alkyne converted to alkane?
Does the alkyne compound become more or less stable
through the conversion to an alkane? Why?
Key concept: bonding arrangements of hydrocarbons
Attempt Socrative questions: 4 to 8
Google Socrative and go to the student login
Room name:
City name followed by 1 or 2 (e.g. PERTH1)
1 for 1st session of the week and 2 for 2nd session of the week
Chemical properties of benzene
• Aromatic hydrocarbons contain the benzene ring
• Benzene is a unique compound due to the behaviour of its carbon to carbon bonds
Representations of benzene:
Aromatic compound:Benzene is toxic to
liver cells (can cause liver cell death)
Chemical properties of benzene
• When benzene was discovered scientists were puzzled – Benezene had multiple double carbon to carbon bonds but was stable
• Benzene behaved more like an alkane than an alkene or alkyne
• Benzene continually switches between two forms where the positions of the double and single carbon to carbon bonds alternate– The two forms of benzene are called resonance structures
Resonance structure 1 Resonance structure 2
Chemical properties of benzene
Animation of the benzene ring switching between it’s resonance structures
Chemical properties of benzeneIn the benzene ring:– Every carbon atom is attached to two other carbon atoms
by at least one carbon to carbon bond
– 3 extra carbon to carbon bonds in the benzene ring are formed by 6 electrons (2 electrons for each bond)
• The extra bonds alternate their positions (see the resonance structures below)
Chemical properties of benzeneIn the benzene ring:
• The 6 electrons within the three extra carbon to carbon bonds are equally shared between all 6 carbons in the ring, as the extra bonds continually change position
– The extra carbon to carbon bonds changing position makes it difficult to break them via addition reactions, which makes benzene very stable
– Benzene is much more stable than other unsaturated hydrocarbons, which have static multiple carbon to carbon bonds like alkenes and alkynes
How is benzene different to other hydrocarbons
such as alkanes, alkenes and alkynes?
What are resonance structures of benzene and
how do they explain the stability of benzene?
Would it be easier to break a double carbon to carbon bond
within an alkene or in benzene? Justify your answer.
G
Key concept: hydrocarbon functional groups
Attempt Socrative questions: 9 and 10
Google Socrative and go to the student login
Room name:
City name followed by 1 or 2 (e.g. PERTH1)
1 for 1st session of the week and 2 for 2nd session of the week
Part 2: Exploring unsaturated hydrocarbon compounds
• Chemical properties of alkenes– Alkenes contain a double carbon to carbon bond, which makes the alkene compound
more reactive than an alkane compound
– The double carbon to carbon bond in an alkene can be broken with a small energy input
– Once a double carbon to carbon bond has been broken, other atoms can bond to the carbon atoms (that were previously part of the multiple carbon to carbon bond) to ensure that each carbon forms 4 covalent bonds
– Hydrogenation reactions involve breaking the double bond within an alkene compound and replacing the double bond with two new bonds to two hydrogen atoms
• Hydrogenation reactions convert alkenes into alkanes
– Hydration reactions involve breaking the double bond within an alkene compound and replacing the double bond with two new bonds to one hydrogen atom and one OH group
• Hydration reactions convert alkenes into alcohols
– Halogenation reactions involve breaking the double bond within an alkene compound and replacing the double bond with two new bonds to two halogen atoms (e.g. chlorine or fluorine)
• Halogenation reactions convert alkenes into halogenated alkanes
Part 2: Exploring unsaturated hydrocarbon compounds
• Bromination reactions
– Bromine readily reacts with an alkene solution to be incorporated into a new compound, so the red bromine solution becomes colourless as the bromine is taken up into the compound
– Bromine does not react readily with an alkane solution, so the red bromine solution remains red
• Chemical properties of alkynes
– Alkynes behave similarly to alkenes in chemical reactions
– Both alkynes and alkenes have multiple carbon to carbon bonds which can be broken with a small amount of input energy
– Alkynes can participate in hydrogenation, hydration and halogenation reactions (just like alkenes) to replace multiple carbon to carbon bonds with new bonds to other atoms
Part 2: Exploring unsaturated hydrocarbon compounds
• Chemical properties of benzene
– Benzene continually switches between two forms, called resonance
structures, where the positions of the double and single carbon to carbon
bonds alternate
– Within benzene, the 6 electrons in the three extra carbon to carbon bonds are
equally shared by all 6 carbons in the ring, as the bonds continually change
position
– The movement of the double carbon to carbon bonds within benzene makes it
difficult to break the bonds via addition reactions, which makes benzene very
stable
Part 3: The alcohol function group
• Hydrocarbon derivatives
• Chemical properties of alcohols
Hydrocarbon derivatives
Hydrocarbon derivatives are:
• Hydrocarbon compounds that contain atoms such as oxygen, nitrogen, fluorine or chlorine as well as carbon and hydrogen atoms
– The location within the hydrocarbon derivative that has atoms other than just carbon and hydrogen is where the functional group is located
Ethanol: present in alcoholic beverages
Alcohol
What are functional groups?– A functional group is a group of atoms within a compound that provides chemical reactivity
• The functional group is usually the part of the compound that is involved in chemical reactions
• All compounds with a particular functional group will behave similarly in chemical reactions
– To find a functional group within a compound,
look for atoms other than just carbon and hydrogen atoms
Alcohol
Hydrocarbon derivatives
Ethanol: present in alcoholic beverages
Chemical properties of alcohols
Functional Group: Alcohol
Functional group formula:
Naming convention: Alcohol compounds have –ol at the end of the name
e.g. ethanol
Example compound:
Propanol
R OHThe alcohol functional group is also
known as the hydroxyl group
The alcohol functional group is located at the
end of a compound (or a branch point), as it
contains one R-group
Alcohol
Functional group
PRIMARY (1°) ALCOHOL
THE CARBON BONDED TO THE ALCOHOL
FUNCTIONAL GROUP IS BONDED TO ONE
OTHER CARBON ATOM
Definition SECONDARY (2°) ALCOHOL
THE CARBON BONDED TO THE ALCOHOL
FUNCTIONAL GROUP IS BONDED TO TWO
OTHER CARBON ATOMS
THE CARBON BONDED TO THE ALCOHOL
FUNCTIONAL GROUP IS BONDED TO THREE
OTHER CARBON ATOMS
Type
TypeType
Definition
Example
Example
TERTIARY (3°) ALCOHOL
Example
Definition
Chemical properties of alcohols
How to work out whether an alcohol is 1°, 2° or 3°:
The compound has two carbons attached to the carbon bonded
to the alcohol functional group = secondary alcohol
– Step 1: Identify the carbon that is directly bonded to the alcohol functional group
– Step 2: Count the number of carbon atoms attached to the carbon identified in step 1
– Step 3: The number of attached carbons identified in step 2
specifies whether it is a primary, secondary or tertiary alcohol
• 1 attached carbon = 1° Alcohol
• 2 attached carbon = 2° Alcohol
• 3 attached carbon = 3° Alcohol
Classify the following compounds
as either a 1°, 2° or 3° alcohols:
1.
2.
3.
4.
Chemical properties of alcoholsCombustion– Combustion reactions are exothermic reactions that
release heat
– Alcohols burn in the presence of oxygen producing CO2, H2O and heat via combustion reactions
– Example: combustion of ethanol
C2H6O + 3O2 → 2CO2 + 3H2O + Energy
– All combustion reactions are redox reactions where one reactant is oxidised and one is reduced
• Oxygen is always reduced in redox reactions
https://www.freeimages.com/photo/hell-of-a-drink-1218762
Chemical properties of alcohols
Alcohol compound Alkene compound + H2O
Dehydration (removal of H2O)
Hydration (addition of H2O)
Hydration reaction
Chemical properties of alkenes
Propene (alkene) watermolecule
Propanol (alcohol)
Alcohol functional group
Addition of a H2O molecule into an alkene:
• Replaces the double carbon to carbon bond with two new covalent bonds between
the carbon atoms and a H and an OH
– End result: the alkene is converted to an alcohol (contains the alcohol functional group)
• The carbon atoms that form the new bonds with the H and OH
were previously part of the double carbon to carbon bond
Chemical properties of alkenes
C C CH
H
HH
H
H
OH H+Energy input
Energy input
Once the double carbon to carbon bond is broken the OH group and a hydrogen atom are incorporated into the compound, which allows each carbon atom to have 4 covalent bonds
Animation of a hydration reaction where an alkene is converted into an alcohol
H2O
Alcohol functional group
Dehydration reaction:
Chemical properties of alcohols
Propene (alkene)Propanol (alcohol)
Alcohol functional group
watermolecule
Removal of a H2O molecule from an alcohol:• The bonds to the OH and H within the compound are broken, allowing an extra
carbon to carbon bond to form, which creates a double carbon to carbon bond
– End result: the alcohol is converted into an alkene
• The carbon atoms that lost the bonds to H and OH are the carbon atoms that form the double carbon to carbon bond
• The OH and H that are released from the compound come together to form a H2O molecule
Chemical properties of alcohols
C C CH
H
HH
H
H
OH H
+
Once the bonds connecting OH and H to the carbon atoms break, the OH and H come together to form H2O and the carbon atoms form an additional carbon to carbon bond, which allows each carbon atom to have 4 covalent bonds
Animation of a dehydration reaction where an alcohol is converted into an alkene
H2O
Alcohol functional group
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Part 3: The alcohol function group• Hydrocarbon derivatives
– Hydrocarbon derivatives are compounds that contain atoms such as oxygen,
nitrogen, fluorine or chlorine as well as carbon and hydrogen atoms
• Chemical properties of alcohols– The alcohol functional group is located at the end of a compound (or a branch point), as it contains
one R-group
– The number of carbons attached to the carbon that is bonded to the alcohol group specifies whether the alcohol is primary, secondary or tertiary:
• 1 attached carbon = 1° Alcohol
• 2 attached carbon = 2° Alcohol
• 3 attached carbon = 3° Alcohol
– Alcohols burn in oxygen via combustion reactions (a type of redox reaction)
– Hydration reactions involve breaking the double bond within an alkene compound and replacing the double bond with new bonds to one hydrogen atom and one OH group
• Hydration reactions convert alkenes into alcohols
– Dehydration reactions involve the removal of a H2O molecule from an alcohol, where the bonds to the OH and H that make up H2O are replaced by a extra carbon to carbon bond (creates a double carbon to carbon double bond in the compound)
• Dehydration reactions convert alcohols into alkenes
Readings & Resources• Stoker, HS 2014, General, Organic and Biological Chemistry, 7th edn,
Brooks/Cole, Cengage Learning, Belmont, CA.
• Stoker, HS 2004, General, Organic and Biological Chemistry, 3rd edn, Houghton Mifflin, Boston, MA.
• Timberlake, KC 2014, General, organic, and biological chemistry: structures of life, 4th edn, Pearson, Boston, MA.
• Alberts, B, Johnson, A, Lewis, J, Raff, M, Roberts, K & Walter P 2008, Molecular biology of the cell, 5th edn, Garland Science, New York.
• Berg, JM, Tymoczko, JL & Stryer, L 2012, Biochemistry, 7th edn, W.H. Freeman, New York.
• Dominiczak, MH 2007, Flesh and bones of metabolism, Elsevier Mosby, Edinburgh.
• Tortora, GJ & Derrickson, B 2014, Principles of Anatomy and Physiology, 14th edn, John Wiley & Sons, Hoboken, NJ.
• Tortora, GJ & Grabowski, SR 2003, Principles of Anatomy and Physiology, 10th edn, John Wiley & Sons, New York, NY.