curved arrows to show the electron pair movement among resonance structures. c) Compare the pKa’s of nitromethane and methane: which is the stronger acid?d) Explain why nitromethane is able to act as an acid.4. a) Write the full electronic configurations for carbon, oxygen, chlorine, and hydrogen. b) Then identify the number of valence electrons each has.5. 2Na(s) + Cl2(g) 2NaCl a) What is the physical state of NaCl at room temperature?b) The physical state is dictated by the type of bond present in NaCl. What type of bond is present in NaCl? c) What type of bond is present in Cl2? How do you know this?d) Use your knowledge of intermolecular forces to explain why NaCl is soluble in water.e) Use your knowledge of intermolecular forces to explain why NaCl is insoluble in hexane, C6H14. 6. For CO2, SO2, H2O, and XeF2: a) Draw the Lewis structure b) Give the hybridization on the central atom c) Give the bond angle d) Show the dipole moments, overall dipole moment, and identify the molecule as polar or nonpolar. e) Name the intermolecular forces present in each.