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Chemical bonds
Made by Amro
Chemical bond
Chemical bond
 What is meant by the term “chemical bond”?
 No simple, and yet complete, way to define this.
 Forces that hold groups of atoms together and make them function as a
unit.
 A bond will form if the energy of the aggregate is lower than that of the
separated atoms.
Chemical bond
 We can obtain information about the strength of a bonding interaction
by measuring Bond energy .
Bond energy: it is the energy required to break a chemical
bond
Covalent bonding
Interaatomic bonding
The Interaction of Two
Hydrogen Atoms
 When hydrogen atoms are brought close together, there are two
unfavorable potential energy terms, proton–proton repulsion and
electron– electron repulsion, and one favorable term, proton– electron
attraction.
 the hydrogen atoms will position themselves so that the system will
achieve the lowest possible energy; the system will act to minimize the
sum of the positive (repulsive) energy and the negative (attractive)
energy .
 The bond length is the distance at which the system has minimum
energy.
Covalent bonding
Covalent bonds:
H:H
2-Double covalent bonds
3-Triple covalent
bonds
• -note that the length of the
bonds changes as : from
longest to shortest:
• Mono>double>triple
• But the opposite in the
strength of bond as :
• Mono<double<triple
2- different two
non metals by
un-equal sharing
of electrons to
achieve the
stability
Covalent bonds are classified into:
1. Pure covalent
2. Nonpolar covalent
3. Polar covalent
4.Dative bond(Coordinate Bond)
Pure covalent
• Between nonmetallic elements of similar electronegativity.
• Formed by sharing electron pairs
• Difference in electronegativity between atoms = zero
• Ex: O2 , H2 , Cl2
Nonpolar covalent
• Between nonmetallic elements of slightly different
electronegativity.
• Formed by sharing electron pairs
• Difference in electronegativity between atoms more than zero till
0.4
• Ex: C-H bond in CH4
Polar covalent
more than 0.4 and less
than 1.7
• Ex: HCl
4.Dative bond(Coordinate Bond)
• In this type: the source of electrons come from an atom has a lone
pair of electrons that acts as a donor that shares its atom with
another one has vacant orbital acts as an acceptor
• It appears in the force between the water molecules like hydrogen
when surrounding the solute materials or the aqueous dissolved ions
The Pauling Electronegativity Values
• On the periodic table, electronegativity generally increases across a
period and decreases down a group.
• The range of electronegativity values is from 4.0 for fluorine (the
most electronegative) to 0.7 for cesium (the least electronegative).
Dipole Moment
• Property of a molecule whose charge distribution can be
represented by a center of positive charge and a center of
negative charge.
• Use an arrow to represent a dipole moment.
• Point to the negative charge center with the tail of the arrow
indicating the positive center of charge.
Dipole Moment
No Net Dipole Moment (Dipoles Cancel)
Ionic bonding
• when sodium and chlorine react to form sodium chloride.
• electrons are transferred from the sodium atoms to the chlorine atoms
to form Na+ and Cl-ions.
• which then aggregate to form solid sodium chloride to achieve the
lowest possible energy by behaving in this way.
Ionic Bond
• Formed Between atoms of metals and nonmetals with very
different electronegativity where the difference in
electronegativity between the metal and the nonmetal must
be more than 1.7
• Bond formed by transfer of electrons where :
1. Metal has large atomic radius so tends to lose its valence
electrons changing to +ve ion.
2. Nonmetal has small atomic radius tends to gain electrons
changing to –ve ion.
• Both to reach the structure of nearest noble gas.
• Examples; NaCl, CaCl2, K2O
Ionic Bond
The energy of interaction between a pair of ions[lattice
energy] can be calculated using Coulomb’s law in the form:
 lattice energy :The change in energy that takes place when separated
gaseous ions are packed together to form an ionic solid.
Thanks for listening
Made by Amro Farag

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Chemical bonds amro.pptx

  • 3.
  • 4. Chemical bond  What is meant by the term “chemical bond”?  No simple, and yet complete, way to define this.  Forces that hold groups of atoms together and make them function as a unit.  A bond will form if the energy of the aggregate is lower than that of the separated atoms.
  • 5. Chemical bond  We can obtain information about the strength of a bonding interaction by measuring Bond energy . Bond energy: it is the energy required to break a chemical bond
  • 6.
  • 8. The Interaction of Two Hydrogen Atoms
  • 9.  When hydrogen atoms are brought close together, there are two unfavorable potential energy terms, proton–proton repulsion and electron– electron repulsion, and one favorable term, proton– electron attraction.  the hydrogen atoms will position themselves so that the system will achieve the lowest possible energy; the system will act to minimize the sum of the positive (repulsive) energy and the negative (attractive) energy .  The bond length is the distance at which the system has minimum energy. Covalent bonding
  • 12. 3-Triple covalent bonds • -note that the length of the bonds changes as : from longest to shortest: • Mono>double>triple • But the opposite in the strength of bond as : • Mono<double<triple
  • 13.
  • 14. 2- different two non metals by un-equal sharing of electrons to achieve the stability
  • 15.
  • 16. Covalent bonds are classified into: 1. Pure covalent 2. Nonpolar covalent 3. Polar covalent 4.Dative bond(Coordinate Bond)
  • 17. Pure covalent • Between nonmetallic elements of similar electronegativity. • Formed by sharing electron pairs • Difference in electronegativity between atoms = zero • Ex: O2 , H2 , Cl2
  • 18. Nonpolar covalent • Between nonmetallic elements of slightly different electronegativity. • Formed by sharing electron pairs • Difference in electronegativity between atoms more than zero till 0.4 • Ex: C-H bond in CH4
  • 19. Polar covalent more than 0.4 and less than 1.7 • Ex: HCl
  • 20.
  • 21. 4.Dative bond(Coordinate Bond) • In this type: the source of electrons come from an atom has a lone pair of electrons that acts as a donor that shares its atom with another one has vacant orbital acts as an acceptor • It appears in the force between the water molecules like hydrogen when surrounding the solute materials or the aqueous dissolved ions
  • 22.
  • 23.
  • 25. • On the periodic table, electronegativity generally increases across a period and decreases down a group. • The range of electronegativity values is from 4.0 for fluorine (the most electronegative) to 0.7 for cesium (the least electronegative).
  • 26.
  • 27. Dipole Moment • Property of a molecule whose charge distribution can be represented by a center of positive charge and a center of negative charge. • Use an arrow to represent a dipole moment. • Point to the negative charge center with the tail of the arrow indicating the positive center of charge.
  • 29. No Net Dipole Moment (Dipoles Cancel)
  • 30.
  • 31. Ionic bonding • when sodium and chlorine react to form sodium chloride. • electrons are transferred from the sodium atoms to the chlorine atoms to form Na+ and Cl-ions. • which then aggregate to form solid sodium chloride to achieve the lowest possible energy by behaving in this way.
  • 32. Ionic Bond • Formed Between atoms of metals and nonmetals with very different electronegativity where the difference in electronegativity between the metal and the nonmetal must be more than 1.7 • Bond formed by transfer of electrons where : 1. Metal has large atomic radius so tends to lose its valence electrons changing to +ve ion. 2. Nonmetal has small atomic radius tends to gain electrons changing to –ve ion. • Both to reach the structure of nearest noble gas. • Examples; NaCl, CaCl2, K2O
  • 33. Ionic Bond The energy of interaction between a pair of ions[lattice energy] can be calculated using Coulomb’s law in the form:  lattice energy :The change in energy that takes place when separated gaseous ions are packed together to form an ionic solid.
  • 34.
  • 35.
  • 36. Thanks for listening Made by Amro Farag