MYP Chemistry Covalent Bonding and Compounds International College Spain Covalent Bonds Covalent bonding is the bonding that occurs between non-metal atoms A covalent bond is formed when.
Download ReportTranscript MYP Chemistry Covalent Bonding and Compounds International College Spain Covalent Bonds Covalent bonding is the bonding that occurs between non-metal atoms A covalent bond is formed when.
Slide 1
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 2
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 3
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 4
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 5
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 6
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 7
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 8
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 9
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 10
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 11
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 12
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 13
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 2
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 3
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 4
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 5
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 6
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 7
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 8
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 9
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 10
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 11
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 12
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp
Slide 13
MYP Chemistry
Covalent Bonding and
Compounds
International College Spain
Covalent Bonds
Covalent bonding is the bonding that
occurs between non-metal atoms
A covalent bond is formed when a pair of
electrons is shared between two atoms
A covalent bond is usually represented by a
single line
A lone pair is any electrons not shared in a
covalent bond
Valence electrons
These are the electrons in the outer
energy shell of the atom
Full electrons shells are stable electron
arrangements
Atoms share electrons to attain full outer
shells
The hydrogen molecule
Each hydrogen atom has only one outer
(valence) electron
H
H
The hydrogen molecule
The outer energy shell can overlap to
make it appear as if there were two
electrons in each shell
H
H
The hydrogen molecule
Now there are two electrons (with negative
charges) in between the two (positive)
nuclei of the hydrogen atoms. This holds
the nuclei, together forming a covalent
bond
H
H
Covalent structure
Covalent substances are usually simple
molecules such as oxygen and hydrogen
gas O2 and H2
O
O
An oxygen molecule
Covalent structures
Soft structures (only weak forces holding
the molecules together)
Low melting and boiling points - they are
often gases or liquids at RT, e.g. O2, N2
Non-conductors (no charged particles)
Insoluble in water
Soluble in other covalent liquids (e.g.
petrol, tetrachloromethane)
Giant covalent structures
If the covalent bonds keep linking atoms
together in a never ending way this gives
rise to giant covalent molecules
Examples include the element carbon and
silicon and the compounds silicon dioxide
Such structures have billions of very
strong bonds and high melting and boiling
points.
Graphite
Diamond
Silicon dioxide
Covalent summary
Shared electron pairs
Full outer shells
Molecules
Non-conductors (exception graphite)
Two types – simple and giant
Simple covalent substances v. low mp
Giant covalent substances v. high mp