1. Polar Vs. Non Polar Molecule Practice

2. Quick Review of Bonding
Ionic Bond (∆EN>1.8) – occurs when there is a complete transfer of electrons between the elements or compounds involved.
Polar Covalent Bonding (∆EN ) – Molecules with an unequal sharing of electrons resulting in a positive dipole at one end and a negative dipole at the other. Every polar covalent bond has a bond dipole (δ+ and δ-)
Nonpolar Covalent Bonding (∆EN<0.4) – Molecules with an equal sharing of electrons resulting in no localized charges. C-C bonds and C-H bonds are always non-polar.
not all molecules with polar bonds are polar molecules: equal bond dipoles acting in opposite directions in three-dimensional space counteract each other

4. Shape of Molecules
Molecules with single-bonded carbon atoms are not flat; their tetrahedral shape can be represented with wedges (forward) or dashes (receding)
The best spatial arrangement of the bonding pairs of electrons in the valence orbital is one in which the repulsions are minimized (VSEPR Theory)

5. Practice Symmetrical Non- Polar Non-Symmetrical Polar Non-Symmetrical

6. Practice
Symmetrical
Non- Polar
Non-Symmetrical Polar

7. Non Polar

8. NonPolar

9. Polar

10. Non Polar

11. Polar

12. Polar

13. Polar

14. Non Polar

15. Polar