The document discusses different types of chemical bonding including metallic bonding, ionic bonding, and covalent bonding. Metallic bonding is described as involving delocalized electrons in a "sea of electrons" that provides properties like luster, malleability, and ductility. Ionic bonding involves the transfer of electrons and results in orderly crystal lattices and very strong bonds, forming hard but brittle solids. Covalent bonding involves the sharing of valence electrons and can be polar or nonpolar. Intermolecular forces like dipole-dipole interactions and London dispersion are also discussed.

1. Chemical Bonding
Mrs. Kuzara
Chemistry 2009-2009

2. Chemical Bonding
Types of Bonding

3. Chemical Bonding
Metallic Bonding & Properties
empty d-orbitals high luster
 
delocalized electrons malleability
 
‘sea of electrons’ ductility
 
attraction between

atoms & sea of electrons

4. Chemical Bonding
Ionic vs. Covalent

5. Chemical Bonding
Ionic vs. Covalent

6. Chemical Bonding
Ionic vs. Covalent

7. Chemical Bonding
Ionic Bonding
transfer of electrons

orderly crystal lattice

very strong bond

hard but brittle solids

conduct electricity in

molten or dissolved
state
formula unit


8. Chemical Bonding
Covalent Bonding
sharing of valence electrons

molecular formula

polar covalent & nonpolar covalent


9. Chemical Bonding
Intermolecular Forces
Molecular Polarity & Dipole-dipole

 the attraction between polar molecules
depends on electronegativities

polar molecules have a positive pole and

a negative pole

10. Chemical Bonding
Intermolecular Forces
Molecular Polarity & Dipole-dipole

 Molecular polarity depends on bond
orientation

11. Chemical Bonding
Nonpolar Covalent

12. Chemical Bonding
Intermolecular Forces
London Dispersion

 weakest!
 occurs between all atoms & molecules
 …even noble gases!

13. Chemical Bonding
Polar Covalent

14. Chemical Bonding
Hydrogen Bonding
very strong dipole-

dipole force
HF, H2O, NH3

large eN- difference

very high boiling

points