Indicate which of the following molecules would NOT have a net dipole: water, carbon monoxide, carbon tetrachloride, boron trifluoride and nitrogen tribromide. b) Explain your answer in part a c) Indicate the direction of the dipole for the molecules from part a that have a dipole and how you know?

A. Write the number of valence electrons below each formula. No points if valence electrons are incorrect.B. Draw the Lewis structure. No additional points if Lewis structure is incorrect.C. Determine the molecular polarity. Write “P” for polar and “NP” for nonpolar. D. Determine the dominant attractive force. Write “L” for London force, “D-D” for dipole-dipole interaction and “H-B” for hydrogen bond. E. Predict the H2O solubility of each compound. Write “H” if it is high. Write “L” if it is low. Compound Lewis Structure Polar or Nonpolar DominantAF H2OSolubility H2S         NH3         C2H6         OF2         C3H6O

How man hydrogens are in the molecule below 04 10 12

Answer the following about drawing the attractive force between a water molecule (H2O) and an ammonium ion (NH4*). The water molecule is and the ammonium ion is a. diatomic b. linear c. tetrahedral d. bent e. pyramidal