Determine whether each molecule in Exercise 36 is polar or nonpolar.
Problem 50EDetermine whether each molecule in Exercise 36 is polar or nonpolar.REFERENCE:Determine the electron geometry, molecular geometry, and idealized bond angles foreach molecule. In which cases do you expect deviations from the idealized bond anglea.b.c.d. Step by step solutionStep 1 of 4(a)Draw a Lewis structure for the molecule by counting the total valence electrons in the compoundas shown below: Total valence electrons =(number of valence for P )+3(number of valence for F)Arrange the various atoms in space by distributing the electrons in bond pair and in lone pairsand determine the molecular geometry as shown below.The Lewis structure has three bonding groups and one lone pair about the central atomphosphorus. Therefore, the molecular geometry is Trigonal pyramidal.The electronegativity of Phosphorus and Fluorine is 2.1 and 4, respectively. Now, show the bondvectors in the direction of more electronegative element as shown below:Therefore, the bonds are polar\nShow the net dipole moment in the molecule as shown below.Since, the three dipole moment vectors sum to generate a net dipole moment hence, themolecule is polar in nature.____________________________________________________________________________