Unit+7+-+Covalent+Bonding

= __COVALENT BONDING__ = media type="custom" key="9696940" -Two non-metals bonded together. -Share electrons

LEWIS STRUCTURES: drawn for molecules and poly atomic ions [|How To Draw A Lewis Structure]

OCTET RULE: Atoms are surrounded by electrons in an octet. They would like to attain a noble gas structure. Bond types: -Single bond: 2 shared electrons -Double bond: 4 shared electrons -Triple bond: 6 shared electrons

RESONANCE FORMS: -Draw the Lewis Structure. -To write resonance structure change the position of the multiple bond. Do NOT change skeleton structure.



Formal Charge: The charge an atom would have if the valence electrons were distributed evenly Most likely structure is the one with the formal charge closest to ZERO. **Cf = x - ( y + z/2 )** x - Valence electrons y- number of lone pair electrons ( count dots) z- number of bonded elcetrons

MOLECULAR GEOMETRY: (VSEPR) The shape f molecule describing the relative positions of the atoms.



POLARITY: Polar or Non Polar Polar: share electrons unevenly Non Polar: share electrons evenly. Symmetrical

HYBRIDIZATION: Formation of Hybrid orbitals 1. S orbital + P orbital --> 2 sp hybrid orbitals 2. S orbital + 2 P orbital --> sp^2 hybrid orbitals 3. S orbital + 3 P orbital --> sp^3 hybrid orbitals

-Unshared pairs can be hybridized. -Only one electron pair in a multiple bond is hybridized.

SIGMA and PI BONDS: Sigma: The first electron pair in a bond. - Single bonds are always sigma. - In multiple bonds there is only one sigma bond.

Pi: All other bonds that are not sigma bonds. - Found in compounds with multiple bonds.

Citations: bond picture: http://kimia.cikgupaatz.com/wp-content/uploads/2010/08/covalent_bonding.gif Video: http://www.schooltube.com/video/7870b1153b034ec08d7a/Comparing-Ionic-and-Covalent-Bonds