Dichloromethane, CH2Cl2, is an important laboratory solvent.
(a) The molecule may be represented by a central carbon atom bonded to two hydrogen atoms and two chlorine atoms in a tetrahedral arrangement. All valence electrons are located in single σ bonds or as lone pairs on chlorine.
Answer the following questions about its bonding and charge distribution.
(a) Draw a complete Lewis structure for CH2Cl2, showing all lone-pair electrons.
(b) For each of the four C–X single bonds (X = H or Cl), indicate the direction of the bond dipole by adding the appropriate δ+ and δ− symbols directly on the Lewis structure. Justify your choices by referencing qualitative periodic trends in electronegativity.
(c) Identify the single atom in the molecule that carries the largest magnitude partial negative charge. Explain your reasoning.
(d) Considering both the orientations and magnitudes of the bond dipoles you assigned in part (b), predict the direction of the overall molecular dipole moment. Clearly describe that direction with respect to the geometry you drew.