- An introduction to bonding
Содержание
- 2. INTRODUCTION This Powerpoint show is one of several produced to help students understand selected topics at
- 3. CONTENTS Introduction Chemical and physical bonding Ionic bonding Covalent bonding Simple molecules Van der Waals’ forces
- 4. STRUCTURE AND BONDING The physical properties of a substance depend on its structure and type of
- 5. STRUCTURE AND BONDING The physical properties of a substance depend on its structure and type of
- 6. IONIC BONDING
- 7. THE IONIC BOND Ionic bonds tend to be formed between elements whose atoms need to “lose”
- 8. THE IONIC BOND Ionic bonds tend to be formed between elements whose atoms need to “lose”
- 9. THE IONIC BOND Ionic bonds tend to be formed between elements whose atoms need to “lose”
- 10. ELECTRON TRANSFER Mg ——> Mg2+ + 2e¯ and 2Cl + 2e¯ ——> 2 Cl¯ Mg Cl
- 11. Positive ions also known as cations; they are smaller than the original atom. formed when electrons
- 12. Negative ions known as anions are larger than the original atom due to electron repulsion in
- 13. IONIC BONDING Animations
- 14. SODIUM CHLORIDE Cl SODIUM ATOM 2,8,1 Na CHLORINE ATOM 2,8,7
- 15. SODIUM CHLORIDE Cl SODIUM ION 2,8 Na CHLORIDE ION 2,8,8 both species now have ‘full’ outer
- 16. SODIUM CHLORIDE Cl SODIUM ION 2,8 Na CHLORIDE ION 2,8,8 Na Na+ + e¯ 2,8,1 2,8
- 17. MAGNESIUM CHLORIDE Cl MAGNESIUM ATOM 2,8,2 Mg CHLORINE ATOMS 2,8,7 Cl
- 18. MAGNESIUM CHLORIDE Cl MAGNESIUM ION 2,8 Mg CHLORIDE IONS 2,8,8 Cl 2+
- 19. GIANT IONIC CRYSTAL LATTICE Cl- Chloride ion Na+ Sodium ion Oppositely charged ions held in a
- 20. GIANT IONIC CRYSTAL LATTICE Each Na+ is surrounded by 6 Cl¯ (co-ordination number = 6) and
- 21. GIANT IONIC CRYSTAL LATTICE Each Na+ is surrounded by 6 Cl¯ (co-ordination number = 6) and
- 22. Physical properties of ionic compounds Melting point very high A large amount of energy must be
- 23. IONIC BONDING BRITTLE IONIC LATTICES IF YOU MOVE A LAYER OF IONS, YOU GET IONS OF
- 24. IONIC COMPOUNDS - ELECTRICAL PROPERTIES SOLID IONIC COMPOUNDS DO NOT CONDUCT ELECTRICITY IONS ARE HELD STRONGLY
- 25. COVALENT BONDING
- 26. Definition consists of a shared pair of electrons with one electron being supplied by each atom
- 27. Definition consists of a shared pair of electrons with one electron being supplied by each atom
- 28. • atoms share electrons to get the nearest noble gas electronic configuration • some don’t achieve
- 29. Orbital theory Covalent bonds are formed when orbitals, each containing one electron, overlap. This forms a
- 30. HYDROGEN Another hydrogen atom also needs one electron to complete its outer shell Hydrogen atom needs
- 31. HYDROGEN CHLORIDE Cl Hydrogen atom also needs one electron to complete its outer shell Chlorine atom
- 32. METHANE C Each hydrogen atom needs 1 electron to complete its outer shell A carbon atom
- 33. AMMONIA N Each hydrogen atom needs one electron to complete its outer shell Nitrogen atom needs
- 34. WATER O Each hydrogen atom needs one electron to complete its outer shell Oxygen atom needs
- 35. HYDROGEN H H H H H H H H both atoms need one electron to complete
- 36. METHANE C H H H H C H H H H H C H H H
- 37. AMMONIA N H H H N H H H H N H H each atom needs
- 38. WATER O H H O H H each atom needs one electron to complete its outer
- 39. OXYGEN O each atom needs two electrons to complete its outer shell each oxygen shares 2
- 40. Bonding Atoms are joined together within the molecule by covalent bonds. Electrical Don’t conduct electricity as
- 41. Although the bonding within molecules is strong, that between molecules is weak. Molecules and monatomic noble
- 42. Although the bonding within molecules is strong, that between molecules is weak. Molecules and monatomic noble
- 43. Although the bonding within molecules is strong, between molecules it is weak. Molecules and monatomic gases
- 44. ‘The ability of an atom to attract the electron pair in a covalent bond to itself’
- 45. ‘The ability of an atom to attract the electron pair in a covalent bond to itself’
- 46. Occurrence occurs between molecules containing polar bonds acts in addition to the basic van der Waals’
- 47. Occurrence not all molecules containing polar bonds are polar overall if bond dipoles ‘cancel each other’
- 48. Evidence place a liquid in a burette allow it to run out place a charged rod
- 49. BOILING POINTS OF HYDRIDES Mr °C CH4 16 -161 SiH4 32 -117 GeH4 77 -90 SnH4
- 50. BOILING POINTS OF HYDRIDES The boiling points of the hydrides increase with molecular mass. CH4 has
- 51. BOILING POINTS OF HYDRIDES NH3 has a higher boiling point than expected for its molecular mass.
- 52. BOILING POINTS OF HYDRIDES H2O has a very much higher boiling point for its molecular mass.
- 53. BOILING POINTS OF HYDRIDES HF has a higher boiling point than expected for its molecular mass.
- 54. BOILING POINTS OF HYDRIDES GROUP IV GROUP V GROUP VI GROUP VII H2O HF NH3 The
- 55. BOILING POINTS OF HYDRIDES GROUP IV GROUP V GROUP VI GROUP VII
- 56. an extension of dipole-dipole interaction gives rise to even higher boiling points bonds between H and
- 57. HYDROGEN BONDING - ICE each water molecule is hydrogen-bonded to 4 others in a tetrahedral formation
- 58. HYDROGEN BONDING - ICE hydrogen bonding
- 59. HYDROGEN BONDING - HF Hydrogen fluoride has a much higher boiling point than one would expect
- 60. A dative covalent bond differs from covalent bond only in its formation Both electrons of the
- 61. Boron trifluoride-ammonia NH3BF3 Boron has an incomplete shell in BF3 and can accept a share of
- 62. MOLECULAR SOLIDS
- 63. IODINE At room temperature and pressure, iodine is a greyish solid. However it doesn’t need to
- 64. COVALENT NETWORKS GIANT MOLECULES MACROMOLECULES They all mean the same!
- 65. DIAMOND, GRAPHITE and SILICA Many atoms joined together in a regular array by a large number
- 66. GIANT (MACRO) MOLECULES DIAMOND MELTING POINT VERY HIGH many covalent bonds must be broken to separate
- 67. GIANT (MACRO) MOLECULES GRAPHITE MELTING POINT VERY HIGH many covalent bonds must be broken to separate
- 68. GIANT (MACRO) MOLECULES DIAMOND GRAPHITE
- 69. GIANT (MACRO) MOLECULES SILICA MELTING POINT VERY HIGH many covalent bonds must be broken to separate
- 70. METALLIC BONDING
- 71. METALLIC BONDING Involves a lattice of positive ions surrounded by delocalised electrons Metal atoms achieve stability
- 72. METALLIC BONDING Involves a lattice of positive ions surrounded by delocalised electrons Metal atoms achieve stability
- 73. METALLIC BONDING Involves a lattice of positive ions surrounded by delocalised electrons Metal atoms achieve stability
- 74. METALLIC BOND STRENGTH Depends on the number of outer electrons donated to the cloud and the
- 75. METALLIC BOND STRENGTH Depends on the number of outer electrons donated to the cloud and the
- 76. METALLIC BOND STRENGTH Depends on the number of outer electrons donated to the cloud and the
- 77. METALLIC PROPERTIES MOBILE ELECTRON CLOUD ALLOWS THE CONDUCTION OF ELECTRICITY For a substance to conduct electricity
- 78. MALLEABLE CAN BE HAMMERED INTO SHEETS DUCTILE CAN BE DRAWN INTO RODS AND WIRES As the
- 79. HIGH MELTING POINTS Melting point is a measure of how easy it is to separate individual
- 80. HIGH MELTING POINTS Melting point is a measure of how easy it is to separate individual
- 81. REVISION CHECK What should you be able to do? Recall the different types of physical and
- 82. You need to go over the relevant topic(s) again Click on the button to return to
- 83. WELL DONE! Try some past paper questions
- 85. Скачать презентацию
INTRODUCTION
This Powerpoint show is one of several produced to help students
INTRODUCTION
This Powerpoint show is one of several produced to help students
CONTENTS
Introduction
Chemical and physical bonding
Ionic bonding
Covalent bonding
CONTENTS
Introduction
Chemical and physical bonding
Ionic bonding
Covalent bonding
STRUCTURE AND BONDING
The physical properties of a substance depend on its
STRUCTURE AND BONDING
The physical properties of a substance depend on its
STRUCTURE AND BONDING
The physical properties of a substance depend on its
STRUCTURE AND BONDING
The physical properties of a substance depend on its
IONIC
BONDING
IONIC
BONDING
THE IONIC BOND
Ionic bonds tend to be formed between elements whose
THE IONIC BOND
Ionic bonds tend to be formed between elements whose
THE IONIC BOND
Ionic bonds tend to be formed between elements whose
THE IONIC BOND
Ionic bonds tend to be formed between elements whose
THE IONIC BOND
Ionic bonds tend to be formed between elements whose
THE IONIC BOND
Ionic bonds tend to be formed between elements whose
ELECTRON
TRANSFER
Mg ——> Mg2+ + 2e¯ and 2Cl + 2e¯ ——> 2
ELECTRON
TRANSFER
Mg ——> Mg2+ + 2e¯ and 2Cl + 2e¯ ——> 2
Positive ions
also known as cations; they are smaller than the
Positive ions
also known as cations; they are smaller than the
Negative ions
known as anions
are larger than the original atom
Negative ions
known as anions
are larger than the original atom
IONIC BONDING
Animations
IONIC BONDING
Animations
SODIUM CHLORIDE
Cl
SODIUM ATOM
2,8,1
Na
CHLORINE ATOM
2,8,7
SODIUM CHLORIDE
Cl
SODIUM ATOM
2,8,1
Na
CHLORINE ATOM
2,8,7
SODIUM CHLORIDE
Cl
SODIUM ION
2,8
Na
CHLORIDE ION
2,8,8
both species now have ‘full’ outer shells; ie
SODIUM CHLORIDE
Cl
SODIUM ION
2,8
Na
CHLORIDE ION
2,8,8
both species now have ‘full’ outer shells; ie
SODIUM CHLORIDE
Cl
SODIUM ION
2,8
Na
CHLORIDE ION
2,8,8
Na Na+ + e¯
2,8,1 2,8
ELECTRON TRANSFERRED
Cl +
SODIUM CHLORIDE
Cl
SODIUM ION
2,8
Na
CHLORIDE ION
2,8,8
Na Na+ + e¯
2,8,1 2,8
ELECTRON TRANSFERRED
Cl +
MAGNESIUM CHLORIDE
Cl
MAGNESIUM ATOM
2,8,2
Mg
CHLORINE ATOMS
2,8,7
Cl
MAGNESIUM CHLORIDE
Cl
MAGNESIUM ATOM
2,8,2
Mg
CHLORINE ATOMS
2,8,7
Cl
MAGNESIUM CHLORIDE
Cl
MAGNESIUM ION
2,8
Mg
CHLORIDE IONS
2,8,8
Cl
2+
MAGNESIUM CHLORIDE
Cl
MAGNESIUM ION
2,8
Mg
CHLORIDE IONS
2,8,8
Cl
2+
GIANT IONIC CRYSTAL LATTICE
Cl-
Chloride ion
Na+
Sodium ion
Oppositely charged ions held in a
GIANT IONIC CRYSTAL LATTICE
Cl-
Chloride ion
Na+
Sodium ion
Oppositely charged ions held in a
GIANT IONIC CRYSTAL LATTICE
Each Na+ is surrounded by 6 Cl¯ (co-ordination
GIANT IONIC CRYSTAL LATTICE
Each Na+ is surrounded by 6 Cl¯ (co-ordination
GIANT IONIC CRYSTAL LATTICE
Each Na+ is surrounded by 6 Cl¯ (co-ordination
GIANT IONIC CRYSTAL LATTICE
Each Na+ is surrounded by 6 Cl¯ (co-ordination
Physical properties of ionic compounds
Melting point
very high A large amount of energy
Physical properties of ionic compounds
Melting point
very high A large amount of energy
IONIC BONDING
BRITTLE IONIC LATTICES
IF YOU MOVE A LAYER OF IONS, YOU
IONIC BONDING
BRITTLE IONIC LATTICES
IF YOU MOVE A LAYER OF IONS, YOU
IONIC COMPOUNDS - ELECTRICAL PROPERTIES
SOLID IONIC COMPOUNDS DO NOT CONDUCT ELECTRICITY
IONS
IONIC COMPOUNDS - ELECTRICAL PROPERTIES
SOLID IONIC COMPOUNDS DO NOT CONDUCT ELECTRICITY
IONS
COVALENT
BONDING
COVALENT
BONDING
Definition consists of a shared pair of electrons with one electron being
supplied
Definition consists of a shared pair of electrons with one electron being
supplied
Definition consists of a shared pair of electrons with one electron being
supplied
Definition consists of a shared pair of electrons with one electron being
supplied
• atoms share electrons to get the nearest noble gas electronic
• atoms share electrons to get the nearest noble gas electronic
Orbital theory
Covalent bonds are formed when orbitals, each containing one electron,
Orbital theory
Covalent bonds are formed when orbitals, each containing one electron,
HYDROGEN
Another hydrogen atom also needs one electron to complete its outer
HYDROGEN
Another hydrogen atom also needs one electron to complete its outer
HYDROGEN CHLORIDE
Cl
Hydrogen atom also needs one electron to complete its outer
HYDROGEN CHLORIDE
Cl
Hydrogen atom also needs one electron to complete its outer
METHANE
C
Each hydrogen atom needs 1 electron to complete its outer shell
METHANE
C
Each hydrogen atom needs 1 electron to complete its outer shell
AMMONIA
N
Each hydrogen atom needs one electron to complete its outer shell
AMMONIA
N
Each hydrogen atom needs one electron to complete its outer shell
WATER
O
Each hydrogen atom needs one electron to complete its outer shell
WATER
O
Each hydrogen atom needs one electron to complete its outer shell
HYDROGEN
H
H H
H
H
H
H H
both atoms need one electron to complete their outer
HYDROGEN
H
H H
H
H
H
H H
both atoms need one electron to complete their outer
METHANE
C
H
H
H
H
C
H
H
H
H
H C H
H
H
each atom needs one electron to complete its outer
METHANE
C
H
H
H
H
C
H
H
H
H
H C H
H
H
each atom needs one electron to complete its outer
AMMONIA
N
H
H
H
N
H
H
H
H N H
H
each atom needs one electron to complete its outer
AMMONIA
N
H
H
H
N
H
H
H
H N H
H
each atom needs one electron to complete its outer
WATER
O
H
H
O
H
H
each atom needs one electron to complete its outer shell
atom
WATER
O
H
H
O
H
H
each atom needs one electron to complete its outer shell
atom
OXYGEN
O
each atom needs two electrons to complete its outer shell
each
OXYGEN
O
each atom needs two electrons to complete its outer shell
each
Bonding Atoms are joined together within the molecule by covalent bonds.
Electrical Don’t conduct
Bonding Atoms are joined together within the molecule by covalent bonds.
Electrical Don’t conduct
Although the bonding within molecules is strong, that between molecules is
Although the bonding within molecules is strong, that between molecules is
Although the bonding within molecules is strong, that between molecules is
Although the bonding within molecules is strong, that between molecules is
Although the bonding within molecules is strong, between molecules it is
Although the bonding within molecules is strong, between molecules it is
‘The ability of an atom to attract the electron pair in
‘The ability of an atom to attract the electron pair in
‘The ability of an atom to attract the electron pair in
‘The ability of an atom to attract the electron pair in
Occurrence occurs between molecules containing polar bonds
acts in addition to the basic
Occurrence occurs between molecules containing polar bonds
acts in addition to the basic
Occurrence not all molecules containing polar bonds are polar overall
if bond dipoles
Occurrence not all molecules containing polar bonds are polar overall
if bond dipoles
Evidence place a liquid in a burette
allow it to run out
place a
Evidence place a liquid in a burette
allow it to run out
place a
BOILING POINTS OF HYDRIDES
Mr °C
CH4 16 -161
SiH4 32 -117
GeH4 77 -90
SnH4 123 -50
NH3 17 -33
PH3 34 -90
AsH3 78 -55
SbH3 125 -17
Mr °C
H2O 18 +100
H2S 34 -61
H2Se 81 -40
H2Te 130 -2
HF 20 +20
HCl 36.5 -85
HBr 81 -69
HI 128 -35
GROUP IV
GROUP V
GROUP VI
GROUP VII
The values of
BOILING POINTS OF HYDRIDES
Mr °C
CH4 16 -161
SiH4 32 -117
GeH4 77 -90
SnH4 123 -50
NH3 17 -33
PH3 34 -90
AsH3 78 -55
SbH3 125 -17
Mr °C
H2O 18 +100
H2S 34 -61
H2Se 81 -40
H2Te 130 -2
HF 20 +20
HCl 36.5 -85
HBr 81 -69
HI 128 -35
GROUP IV
GROUP V
GROUP VI
GROUP VII
The values of
BOILING POINTS OF HYDRIDES
The boiling points of the hydrides increase with
BOILING POINTS OF HYDRIDES
The boiling points of the hydrides increase with
BOILING POINTS OF HYDRIDES
NH3 has a higher boiling point than expected
BOILING POINTS OF HYDRIDES
NH3 has a higher boiling point than expected
BOILING POINTS OF HYDRIDES
H2O has a very much higher boiling point
BOILING POINTS OF HYDRIDES
H2O has a very much higher boiling point
BOILING POINTS OF HYDRIDES
HF has a higher boiling point than expected
BOILING POINTS OF HYDRIDES
HF has a higher boiling point than expected
BOILING POINTS OF HYDRIDES
GROUP IV
GROUP V
GROUP VI
GROUP VII
H2O
HF
NH3
The higher than expected
BOILING POINTS OF HYDRIDES
GROUP IV
GROUP V
GROUP VI
GROUP VII
H2O
HF
NH3
The higher than expected
BOILING POINTS OF HYDRIDES
GROUP IV
GROUP V
GROUP VI
GROUP VII
BOILING POINTS OF HYDRIDES
GROUP IV
GROUP V
GROUP VI
GROUP VII
an extension of dipole-dipole interaction
gives rise to even higher
an extension of dipole-dipole interaction
gives rise to even higher
HYDROGEN BONDING - ICE
each water molecule is hydrogen-bonded to 4
others in
HYDROGEN BONDING - ICE
each water molecule is hydrogen-bonded to 4
others in
HYDROGEN BONDING - ICE
hydrogen bonding
HYDROGEN BONDING - ICE
hydrogen bonding
HYDROGEN BONDING - HF
Hydrogen fluoride has a much higher boiling point
HYDROGEN BONDING - HF
Hydrogen fluoride has a much higher boiling point
A dative covalent bond differs from covalent bond only in its
A dative covalent bond differs from covalent bond only in its
Boron trifluoride-ammonia NH3BF3
Boron has an incomplete shell in BF3 and can
Boron trifluoride-ammonia NH3BF3
Boron has an incomplete shell in BF3 and can
MOLECULAR
SOLIDS
MOLECULAR
SOLIDS
IODINE
At room temperature and pressure, iodine is a greyish solid. However
IODINE
At room temperature and pressure, iodine is a greyish solid. However
COVALENT NETWORKS
GIANT MOLECULES
MACROMOLECULES
They all mean the same!
COVALENT NETWORKS
GIANT MOLECULES
MACROMOLECULES
They all mean the same!
DIAMOND, GRAPHITE and SILICA
Many atoms joined together in a regular array
by
DIAMOND, GRAPHITE and SILICA
Many atoms joined together in a regular array
by
GIANT (MACRO) MOLECULES
DIAMOND
MELTING POINT VERY HIGH
many covalent bonds must be broken to
GIANT (MACRO) MOLECULES
DIAMOND
MELTING POINT VERY HIGH
many covalent bonds must be broken to
GIANT (MACRO) MOLECULES
GRAPHITE
MELTING POINT VERY HIGH
many covalent bonds must be broken to
GIANT (MACRO) MOLECULES
GRAPHITE
MELTING POINT VERY HIGH
many covalent bonds must be broken to
GIANT (MACRO) MOLECULES
DIAMOND
GRAPHITE
GIANT (MACRO) MOLECULES
DIAMOND
GRAPHITE
GIANT (MACRO) MOLECULES
SILICA
MELTING POINT VERY HIGH
many covalent bonds must be broken to
GIANT (MACRO) MOLECULES
SILICA
MELTING POINT VERY HIGH
many covalent bonds must be broken to
METALLIC
BONDING
METALLIC
BONDING
METALLIC BONDING
Involves a lattice of positive ions surrounded by delocalised electrons
Metal
METALLIC BONDING
Involves a lattice of positive ions surrounded by delocalised electrons
Metal
METALLIC BONDING
Involves a lattice of positive ions surrounded by delocalised electrons
Metal
METALLIC BONDING
Involves a lattice of positive ions surrounded by delocalised electrons
Metal
METALLIC BONDING
Involves a lattice of positive ions surrounded by delocalised electrons
Metal
METALLIC BONDING
Involves a lattice of positive ions surrounded by delocalised electrons
Metal
METALLIC BOND STRENGTH
Depends on the number of outer electrons donated
to the
METALLIC BOND STRENGTH
Depends on the number of outer electrons donated
to the
METALLIC BOND STRENGTH
Depends on the number of outer electrons donated
to the
METALLIC BOND STRENGTH
Depends on the number of outer electrons donated
to the
METALLIC BOND STRENGTH
Depends on the number of outer electrons donated
to the
METALLIC BOND STRENGTH
Depends on the number of outer electrons donated
to the
METALLIC PROPERTIES
MOBILE ELECTRON CLOUD ALLOWS THE CONDUCTION OF ELECTRICITY
For a substance
METALLIC PROPERTIES
MOBILE ELECTRON CLOUD ALLOWS THE CONDUCTION OF ELECTRICITY
For a substance
MALLEABLE CAN BE HAMMERED INTO SHEETS
DUCTILE CAN BE DRAWN INTO RODS AND
MALLEABLE CAN BE HAMMERED INTO SHEETS
DUCTILE CAN BE DRAWN INTO RODS AND
HIGH MELTING POINTS
Melting point is a measure of how easy it
HIGH MELTING POINTS
Melting point is a measure of how easy it
HIGH MELTING POINTS
Melting point is a measure of how easy it
HIGH MELTING POINTS
Melting point is a measure of how easy it
REVISION CHECK
What should you be able to do?
Recall the different types
REVISION CHECK
What should you be able to do?
Recall the different types
You need to go over the relevant topic(s) again
Click on the
You need to go over the relevant topic(s) again
Click on the
WELL DONE!
Try some past paper questions
WELL DONE!
Try some past paper questions
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