APPLICATIONS OF ORGANIC
CHEMISTRY
UNIT 14 ASSIGNMENT B
C: Understand the reactions and properties of aromatic compounds.
BENZENE
Benzene's chemical formula is C6H6. It's a kind of Cyclic hydrocarbon, meaning
that each of its Carbon atoms is arranged in a six-membered ring and only has
one Hydrogen atom connected to it. In benzene, there are two different
resonance configurations.
It's an aromatic petrochemical and a natural component of crude oil. The liquid
is colourless, highly toxic, and carcinogenic, with an odour similar to gasoline.
It is found in the environment and formed as a result of volcanic eruptions and
forest fires. It's also made in coal and oil-based industries. [1]
Benzene melts at 5.5 degrees Celsius and boils at 80.1 degrees Celsius.
Benzene is insoluble in water but soluble in organic solvents. It has a pleasant
aroma. Benzene undergoes a substitution reaction that replaces one or more
hydrogen atoms with another atom or radical, some industries use it to make
other chemicals that are used to make plastics, resins, nylon, and synthetic
fibres.
Hybridisation
It is believed that benzene underwent sp2 type hybridization. Benzene is made
up of six carbon and six hydrogen atoms, with the centre atom frequently being
hybridised. [7]
the chemical make-up of benzene. This chemical molecule is made up of a
number of hydrogen and carbon atoms. But in order to produce benzene, the
carbon atoms will need to make bonds with two other carbon atoms and one
hydrogen atom. Additionally, there aren't enough unpaired electrons in the
carbon atom to form the bonds. At this time, its electrical configuration will be
1s2, 2s2, 2px1, and 2py1. The open 2pz orbital is then filled by one pair of 2s2
electrons.
,Benzene is made up of six carbon atoms grouped in a cyclic configuration, each
of which is connected to a hydrogen atom. In benzene, there are 6 sigma bonds
between carbon atoms, which alternate with 3 pi bonds. In bonding electron
pairs, each carbon atom possesses four electrons. Three of them are involved in
sigma bonds, while one is involved in a pi bond.
A ring of delocalized pi electrons can be discovered in benzene, because it
spreads the charge of the electrons over a larger area, this ring of delocalisation
is relatively powerful and stable. Disrupting delocalization takes a lot of energy.
As a result, benzene is resistant to reactions that require the breaking of the ring,
such as addition reactions. It does, however, participate in substitution reactions.
These are electrophilic replacements. [2]
The carbon atoms of the benzene ring are arranged in a trigonal planar
arrangement. In contrast to the hybrid orbitals, which are grouped in a plane at a
120° angle, the p orbitals are organised at right angles to them.
Delocalization of electrons
It is a regular hexagon since all the connections are the same. The delocalization
of the electrons prevents alternating double and single bonds from existing.
There is no other way for the p orbitals to overlap sideways and create the
delocalised pi system, thus it must be planar.
Delocalization can be used to explain this, the more evenly dispersed or
delocalized the electrons are, the more stable the molecule is considered to be.
The improved stability of benzene is usually referred to as "delocalisation
energy".
Benzene is approximately 150 kJ mol-1 more stable than it would be without
the delocalized electrons. Additional atoms would need to be added to a
, benzene ring, requiring the use of some of the delocalized electrons. The
system's stability would decline and the delocalization would be disturbed.
Although benzene still has the Kekulé structure, we prefer the structure on the
right for the vast majority of our needs.
The hexagon displays a ring of six carbon atoms with one hydrogen atom
connected to each one.
The circle depicts the delocalization of the electrons. Circle must be included; it
is essential. If you don't get it, you'll draw cyclohexane rather than benzene.
Kekulé Structure
This is the kekulé structure of benzene.
The chemistry of the Kekulé structure is problematic because of the three
double bonds; there is the assumption that benzene would react similarly to
ethene. Ethene goes through addition reactions in which one of the two bonds
connecting the carbon atoms breaks and the electrons are used to bond with
other atoms. Benzene almost never does this. Instead, substitution reactions
occur in which one of the hydrogen atoms is replaced by something new.
The shape of the Kekulé structure is problematic. Benzene is a planar molecule
(all of its atoms are in one plane), and the Kekulé structure would be the same.
The issue is that the lengths of C-C single and double bonds differ. Kekule's
structure did not explain benzene's low reactivity. According to the Kekule
CHEMISTRY
UNIT 14 ASSIGNMENT B
C: Understand the reactions and properties of aromatic compounds.
BENZENE
Benzene's chemical formula is C6H6. It's a kind of Cyclic hydrocarbon, meaning
that each of its Carbon atoms is arranged in a six-membered ring and only has
one Hydrogen atom connected to it. In benzene, there are two different
resonance configurations.
It's an aromatic petrochemical and a natural component of crude oil. The liquid
is colourless, highly toxic, and carcinogenic, with an odour similar to gasoline.
It is found in the environment and formed as a result of volcanic eruptions and
forest fires. It's also made in coal and oil-based industries. [1]
Benzene melts at 5.5 degrees Celsius and boils at 80.1 degrees Celsius.
Benzene is insoluble in water but soluble in organic solvents. It has a pleasant
aroma. Benzene undergoes a substitution reaction that replaces one or more
hydrogen atoms with another atom or radical, some industries use it to make
other chemicals that are used to make plastics, resins, nylon, and synthetic
fibres.
Hybridisation
It is believed that benzene underwent sp2 type hybridization. Benzene is made
up of six carbon and six hydrogen atoms, with the centre atom frequently being
hybridised. [7]
the chemical make-up of benzene. This chemical molecule is made up of a
number of hydrogen and carbon atoms. But in order to produce benzene, the
carbon atoms will need to make bonds with two other carbon atoms and one
hydrogen atom. Additionally, there aren't enough unpaired electrons in the
carbon atom to form the bonds. At this time, its electrical configuration will be
1s2, 2s2, 2px1, and 2py1. The open 2pz orbital is then filled by one pair of 2s2
electrons.
,Benzene is made up of six carbon atoms grouped in a cyclic configuration, each
of which is connected to a hydrogen atom. In benzene, there are 6 sigma bonds
between carbon atoms, which alternate with 3 pi bonds. In bonding electron
pairs, each carbon atom possesses four electrons. Three of them are involved in
sigma bonds, while one is involved in a pi bond.
A ring of delocalized pi electrons can be discovered in benzene, because it
spreads the charge of the electrons over a larger area, this ring of delocalisation
is relatively powerful and stable. Disrupting delocalization takes a lot of energy.
As a result, benzene is resistant to reactions that require the breaking of the ring,
such as addition reactions. It does, however, participate in substitution reactions.
These are electrophilic replacements. [2]
The carbon atoms of the benzene ring are arranged in a trigonal planar
arrangement. In contrast to the hybrid orbitals, which are grouped in a plane at a
120° angle, the p orbitals are organised at right angles to them.
Delocalization of electrons
It is a regular hexagon since all the connections are the same. The delocalization
of the electrons prevents alternating double and single bonds from existing.
There is no other way for the p orbitals to overlap sideways and create the
delocalised pi system, thus it must be planar.
Delocalization can be used to explain this, the more evenly dispersed or
delocalized the electrons are, the more stable the molecule is considered to be.
The improved stability of benzene is usually referred to as "delocalisation
energy".
Benzene is approximately 150 kJ mol-1 more stable than it would be without
the delocalized electrons. Additional atoms would need to be added to a
, benzene ring, requiring the use of some of the delocalized electrons. The
system's stability would decline and the delocalization would be disturbed.
Although benzene still has the Kekulé structure, we prefer the structure on the
right for the vast majority of our needs.
The hexagon displays a ring of six carbon atoms with one hydrogen atom
connected to each one.
The circle depicts the delocalization of the electrons. Circle must be included; it
is essential. If you don't get it, you'll draw cyclohexane rather than benzene.
Kekulé Structure
This is the kekulé structure of benzene.
The chemistry of the Kekulé structure is problematic because of the three
double bonds; there is the assumption that benzene would react similarly to
ethene. Ethene goes through addition reactions in which one of the two bonds
connecting the carbon atoms breaks and the electrons are used to bond with
other atoms. Benzene almost never does this. Instead, substitution reactions
occur in which one of the hydrogen atoms is replaced by something new.
The shape of the Kekulé structure is problematic. Benzene is a planar molecule
(all of its atoms are in one plane), and the Kekulé structure would be the same.
The issue is that the lengths of C-C single and double bonds differ. Kekule's
structure did not explain benzene's low reactivity. According to the Kekule
