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Chapter 6 CHEMICAL BONDING
[object Object],[object Object],[object Object],[object Object],CHEMICAL BOND
CHEMICAL BONDING VIDEO
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],TYPES OF BONDS
COVALENT BONDS VIDEO CLIP
IONIC BOND  VIDEO CLIP
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],TYPES OF COVALENT BONDS
POLAR VS NON-POLAR COVALENT BONDS
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],MOLECULAR COMPOUNDS
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],CHARACTERISTICS OF COVALENT BONDS
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],OCTET RULE
[object Object],[object Object],ELECTRON DOT NOTATION
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],LEWIS STRUCTURES
[object Object],STRUCTURAL FORMULAS
[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],BONDS
Multiple Covalent Bonds ,[object Object],Triple Bond  – a covalent bond produced by the sharing of three pairs of electrons between two atoms. N N O O N N O O
IONIC BONDING AND IONIC COMPOUNDS ,[object Object],[object Object],[object Object]
FORMATION OF IONIC COMPOUNDS Na +  + Cl - NaCl Ca 2+  + F - CaF 2 Ca 2+  + N 3- Ca 3 N 2
CHARACTERISTICS OF IONIC BONDING ,[object Object],[object Object],[object Object]
POLYATOMIC IONS ,[object Object]
METALLIC BONDING ,[object Object],[object Object],[object Object]
[object Object],[object Object],[object Object],[object Object]
MOLECULAR GEOMETRY ,[object Object],[object Object]
VSEPR THEORY ,[object Object]
[object Object],Key:  Must consider both bonding and lone pairs in minimizing electron repulsion. Lewis Structure VSEPR Structure
•  Example:  NH 3  (both bonding and lone pairs). Lewis Structure VSEPR Structure  Molecular Shape
VSEPR APPLICATIONS The previous examples illustrate the strategy for applying VSEPR to predict molecular structure: 1.  Construct the Lewis Dot Structure 2.  Arrange the bonding and lone electron pairs   in space such that  repulsions are minimized .
Case:  Linear Structure ( AX 2 ):  angle between bonds is 180° Example:  BeF 2 180°
Case: Trigonal Planar Structure ( AX 3 ):  The angle between bonds is 120° Example:  BF 3 120°
Case:  Pyramidal ( AX 3 E ):  Bond angles are <120° structure is nonplanar due to repulsion of lone-pair.  Example:  NH 3 107° VSEPR Structure Molecular shape Lewis
Case:  Tetrahedral ( AX 4 ): the angle between bonds is ~109.5° Example:  CH 4 109.5°
Note: for ‘Tetrahedral’, the actual angle may vary slightly from 109.5°, due to size differences between bonding and lone pair electron densities bonding pair: more elongated, less repulsive lone pair: puffier, more repulsive
Example of  distorted tetrahedron: water ( AX 2 E 2 ): the angle is reduced to 104.5° by repulsion of the lone pairs “ bent” VSEPR structure Molecular shape
Case:  Trigonal Bipyramidal ( AX 5 ):  non-equivalent  bond positions: three in-plane (equatorial, 120°), and two at 90° to plane (axial) Example, PCl 5 90° 120°
Octahedral ( AX 6 ):  all angles are 90° Example SF 6 90° Lewis VSEPR
INTERMOLECULAR FORCES ,[object Object],[object Object],[object Object],H - Cl
[object Object],[object Object],[object Object],[object Object],[object Object]

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Chemical Bonding

  • 2.
  • 4.
  • 6. IONIC BOND VIDEO CLIP
  • 7.
  • 8. POLAR VS NON-POLAR COVALENT BONDS
  • 9.
  • 10.
  • 11.
  • 12.
  • 13.
  • 14.
  • 15.
  • 16.
  • 17.
  • 18. FORMATION OF IONIC COMPOUNDS Na + + Cl - NaCl Ca 2+ + F - CaF 2 Ca 2+ + N 3- Ca 3 N 2
  • 19.
  • 20.
  • 21.
  • 22.
  • 23.
  • 24.
  • 25.
  • 26. • Example: NH 3 (both bonding and lone pairs). Lewis Structure VSEPR Structure Molecular Shape
  • 27. VSEPR APPLICATIONS The previous examples illustrate the strategy for applying VSEPR to predict molecular structure: 1. Construct the Lewis Dot Structure 2. Arrange the bonding and lone electron pairs in space such that repulsions are minimized .
  • 28. Case: Linear Structure ( AX 2 ): angle between bonds is 180° Example: BeF 2 180°
  • 29. Case: Trigonal Planar Structure ( AX 3 ): The angle between bonds is 120° Example: BF 3 120°
  • 30. Case: Pyramidal ( AX 3 E ): Bond angles are <120° structure is nonplanar due to repulsion of lone-pair. Example: NH 3 107° VSEPR Structure Molecular shape Lewis
  • 31. Case: Tetrahedral ( AX 4 ): the angle between bonds is ~109.5° Example: CH 4 109.5°
  • 32. Note: for ‘Tetrahedral’, the actual angle may vary slightly from 109.5°, due to size differences between bonding and lone pair electron densities bonding pair: more elongated, less repulsive lone pair: puffier, more repulsive
  • 33. Example of distorted tetrahedron: water ( AX 2 E 2 ): the angle is reduced to 104.5° by repulsion of the lone pairs “ bent” VSEPR structure Molecular shape
  • 34. Case: Trigonal Bipyramidal ( AX 5 ): non-equivalent bond positions: three in-plane (equatorial, 120°), and two at 90° to plane (axial) Example, PCl 5 90° 120°
  • 35. Octahedral ( AX 6 ): all angles are 90° Example SF 6 90° Lewis VSEPR
  • 36.
  • 37.