Define the difference between a polar and non-polar covalent bond. How do you determine if a molecule is polar or non-polar?  Explain how a lone pair affects the bond angles of a substance

please draw a lewis structure, determine the # of electron groups around the central atom, and determine the geometry of the molecule. (please state both the name of the geometry and draw the molecular shape) molecule lewis structure electron pair geometry around the central atom(s) molecular shape around the central atom(s) CO2       H2S       H2O2       NF3       SO2Cl2       NO2       C2H2       C2H4       C2H6

Following is a molecule with polar bonds whose shape was obtained using the VSEPR theory. Specify the molecular shape of this molecule, and whether the molecule is polar or nonpolar. (Hint: In terms of polarity, see whether the dipoles in the molecule cancel or not. A molecule containing polar bonds can be nanpolar if the dipoles cancel each other. You can imagine the dipoles as ropes pulling on the central atom–If the pulls cancel each other, that is, the central atom cannot move, then the molecule is nonpolar. If on the other hand the opposite is true, then the molecule is polar.) O trigonal pyramidal shape, nonpolar O trigonal planar shape, nonpolar O tetrahedral shape, polar O trigonal pyramidal shape, polar O trigonal planar shape, polar

The compound XeCl2F2 can exist in two different forms.  One form is polar and the other form is non-polar.  Draw a valid Lewis structure of XeCl2F2.  Then, draw two 3-dimensional representations of this molecule (including all lone pairs); one that shows the polar form with a correct dipole arrow and the other that shows the non-polar form of the molecule.