16.1 - The Nature of Covalent Bonding-Covalent bonding involves two atoms sharing electrons because there is not enough electronegativity difference to actually cause the elecrons to be transfered.
1 - Use Dot Structures to show the formation of single, double, and triple covalent bonds.

2 - Describe and give examples of: Coordinate Covalent Bonds, Resonance Structures, Octet Rule and Exceptions to Octet Rule .

16.2-Bonding Theories This model assumes that when two atoms bond their atomic orbitals overlap to produce Molecular Orbitals or orbitals that apply to the enitre molecule.

1 - Describe the molecular orbital theory of covalent bonding including orbital hybridization.

2 - Use VSEPR Theory to predict the shapes of simple covalently bonded molecules.

16.3 - Polar Bonds & Molecules The more electronegative atom in a bonded pair will sometimes not share the electrons evenly, creating a negative and a positive "pole" within the bond. If, due to the shape of the molecule, these polar bonds can be orientated in such a way that the entire molecule will have a positive and a negative "pole" and therefore be a "polar molecule". Polar molecules have different physical and chemical properties than non-polar molecules of similar size.
1 - Use electronegativity values to classify bonds Ionic, Polar Covalent or Nonpolar Covalent

2 - Name and describe the weak attractive forces that hold groups of molecules together.

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16.1 - The Nature of Covalent Bonding-Covalent bonding involves two atoms sharing electrons because there is not enough electronegativity difference to actually cause the elecrons to be transfered. 1 - Use Dot Structures to show the formation of single, double, and triple covalent bonds. 2 - Describe and give examples of: Coordinate Covalent Bonds, Resonance Structures, Octet Rule and Exceptions to Octet Rule .	single covalent bond structural formula unshared pairs of e- double covalent bonds triple covalent bond coordinate covalent bond bond dissociation energy diamagentic/paramagnetic
16.2-Bonding Theories This model assumes that when two atoms bond their atomic orbitals overlap to produce Molecular Orbitals or orbitals that apply to the enitre molecule. 1 - Describe the molecular orbital theory of covalent bonding including orbital hybridization. 2 - Use VSEPR Theory to predict the shapes of simple covalently bonded molecules.	molecular orbital bonding orbital antibonding orbital sigma bond pi bond tetrahedral angle VSPER Theory hybridization
16.3 - Polar Bonds & Molecules The more electronegative atom in a bonded pair will sometimes not share the electrons evenly, creating a negative and a positive "pole" within the bond. If, due to the shape of the molecule, these polar bonds can be orientated in such a way that the entire molecule will have a positive and a negative "pole" and therefore be a "polar molecule". Polar molecules have different physical and chemical properties than non-polar molecules of similar size. 1 - Use electronegativity values to classify bonds Ionic, Polar Covalent or Nonpolar Covalent 2 - Name and describe the weak attractive forces that hold groups of molecules together.	nonpolar covalent bond polar covalent bond ionic bond polar molecule dipole van der Waals forces dispersion forces dipole interaction hydrogen bonds network solids