Draw a Lewis Structure for each of the following.
Identify any that would have resonance structures and draw all
possible structures.
Determine the formal charge on all the atoms in each of the
molecules.
Determine the molecular geometry (giving the appropriate name)
using VSEPR theory.
Determine if the molecule is polar or nonpolar.
Give the hybridization of the central atom.
CF2Cl2
SO42-
CN-
IF5
BeF2
SeF6
H3O+
O2
CO32-
PF3
Complete the Lewis structures of SO2 and
SO3. Be sure to draw only the resonance form with the
lowest formal charges (zero) on all atoms. Do not add the formal
charges to the structures. Then predict the solubility of the
structures.
Resonance structures are Lewis structures drawn for a molecule
when more than one Lewis structure is needed to explain the
molecular structure. Resonance results in extended
__________?
of some electrons among more than two nuclei of the molecule.
This results in lowering of kinetic and potential energies that
imparts added stability to the molecule.
Note. In covalent bond formation the bonding electrons are
delocalized between only two atoms. Resonance is taking the
delocalization of electrons between nuclei to the next...
3) for one resonance structure of a nitrate(NO3-)
provide the:
a) Lewis structure
b) formal charge on each atom
c)name of the electro pair(electron domain)
geometry
d) hybridization of the central atom
e)name of the molecular geometry (shape)
. a) Draw the Lewis structure of SO3 2- . b)- Identify the
electronic and molecular geometries of the molecule, and the
hybridization of the central atom. c) Is this molecule polar?
Justify your answer by drawing the VSEPR molecular geometry and
labeling the molecular dipole moment.
Draw the lewis dot structure and all resonance structures for
the dithiorcarbonate molecule (S2CO -2).
Which lewis structure is the best for this structure?(formal
charge)
The best Lewis structure of N2H2 showsa) a nitrogen-nitrogen triple bondb) a nitrogen-nitrogen single bondc) each nitrogen with one nonbonding electron paird) each nitrogen with two nonbonding electron pairs